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Fall 2012 First Quarter Chemistry Progress Assessment Study Guide ( not complete )General Knowledge
Multiple Choice: Select the option that best answers the question or task.
1) Which of the following is NOT a major component of the scientific method?
a) observing b) generalizing c) measuring d) testing e) theorizing
2) Which of the following is an example of quantitative information?
a) volume b) color c) texture d) shape e) smell
3) Which of the following is an example of qualitative information?
a) density b) taste c) length d) weight e) area
4) The main difference between mass and weight is a factor known as:
a) quantity b) inertia c) gravity d) conservation e) composition
5) Among the following, which are examples of matter?
a) elements b) chemicals c) pure substances d) atoms e) all of the above
6) Which of the following are the two major types of energy?
a) kinetic and chemical b) potential and solar c) kinetic and potential
d) potential and mechanical e) solar and mechanical
7) Which of the following is NOT an example of potential energy?
a) water behind a dam b) water flowing over a dam c) a boulder at the top of a hill
d) a stretched rubber band e) a stick of dynamite
8) Which of the following is NOT an example of kinetic energy?
a) a baseball in flight b) a water balloon c) a hurricane d) a burning candle
9) Which of the following is a state of matter?
a) solid b) liquid c) gas d) all of the above
10) Which of the following is NOT a physical property?
a) melting point b) height c) flammability d) volume e) color
11) Which of the following is NOT a chemical property?
a) density b) flammability c) toxicity d) reactivity e) oxidation state
12) Which of the following is an intensive physical property?
a) mass b) volume c) density d) length e) area
13) Which of the following is an extensive physical property?
a) color b) melting point c) ductility d) crystal structure e) weight
*** continued ***
14) Which one of the following is an intensive property that is qualitative in nature?
a) density b) color c) mass d) length e) volume
15) Which one of the following is an intensive property that is quantitative in nature?
a) area b) melting point c) ductility d) crystal structure e) malleability
16) Which of the following is an example of a chemical change?
a) decomposition b) cooking c) rusting d) oxidation e) all of the above
17) Which of the following is an example of a physical change?
a) grinding a sugar cube into powder b) melting c) boiling d) freezing e) all of the above
18) When ice melts, the water undergoes which of the following?
a) a chemical change b) a physical change c) both
19) The chopping of wood into smaller pieces can be classified as which of the following?
a) a chemical change b) a physical change c) both
20) The burning of paper can be classified as which of the following?
a) a chemical change b) a physical change c) both
21) When salt is dissolved in water, the salt undergoes which of the following?
a) a chemical change b) a physical change c) both
22) The boiling of water until it evaporates is an example of which of the following?
a) a chemical change b) a physical change c) both
23) Which of the following is NOT an observable change that would indicate that a chemical reaction has
occurred?
a) The evolution of heat and light. b) The production of a gas.
c) The formation of a precipitate. d) The freezing of a solid.
24) Which of the following is NOT an example of an exothermic process?
a) combustion of fuels b) condensation of a vapor to a liquid c) explosion of a firecracker
d) the melting of ice e) the formation of snow flakes
25) Which of the following is NOT an example of an endothermic process?
a) the making of ice cream b) the melting of ice cream c) the eating of ice cream
26) In photosynthesis, the transfer of energy from sunlight to the plant’s cells is an example of which of the
following processes?
a) endothermic b) exothermic c) both a & b d) neither a nor b
*** continued ***
27) The transferring of energy during both a 100 megaton nuclear bomb explosion and a drop of water freezing
is an example of which of the following processes?
a) endothermic b) exothermic c) both a & b d) neither a nor b
28) Which of the following processes describes what happens to the energy (heat) in the air that surrounds solid
water (ice) as the water turns into a liquid?
a) endothermic b) exothermic c) both a & b d) neither a nor b
29) Each sample of matter can be classified into which of the following types?
a) a pure substance b) a mixture c) both a & b d) either a or b
30) Referring to samples of matter, which of the following is NOT an example of a mixture?
a) gasoline b) air c) sugar d) Dr. Pepper e) grapefruit juice
31) Referring to samples of matter, which of the following is NOT an example of a pure substance?
a) milk b) distilled water c) salt d) oxygen e) silver
32) Which of the following is an example of a heterogeneous mixture?
a) vegetable soup b) milk c) chocolate chip cookies d) all of the above
33) Which of the following is an example of a homogeneous mixture?
a) air b) sea water c) Mountain Dew d) chocolate syrup e) all of the above
34) The two categories for classifying samples of homogeneous matter are homogeneous mixture and which of
the following?
a) pure substances b) pure solutions c) pure phases d) pure precipates
35) Which of the following is an example of an element?
a) salt b) water c) copper d) NaCl e) H2O
36) Which of the following is an example of a compound?
a) gold b) silver c) copper d) calcium e) salt
For the following questions, #37 & #38, refer to the chemical equation as diagramed in the box (fig 1) below.
fig 1:
37) In reference to the above chemical reaction, which substance or substances are the reactants?
a) 2H b) O c) H2O d) both a & b e) both b & c
38) In reference to the above chemical reaction, which substance or substances are the products?
a) 2H b) O c) H2O d) both a & b e) both b & c
*** continued ***
2H + O → H2O
For the following questions 46 – 51, refer to the periodic table.
39) Which of the following sets is a representation of a periodic table group?
a) [ Li, Be, B, C, N, O, F, Ne ] b) [ F, Cl, Br, I, At ]
40) Which of the following sets is a representation of a periodic table period?
a) [ Na, Mg, Al, Si, P, S, Cl, Ar ] b) [ B, Al, Ga, In, Tl ]
41) Which of the following sets is a representation of periodic table metals?
a) [ Mg, Co, Ga, In, Os, Ba, Ra ] b) [ B, Si, Ge, As, Se, Sb, Te ] c) [ C, N, P, S, Cl, Br, I ]
42) Which of the following sets is a representation of periodic table non-metals?
a) [ Mg, Co, Ga, In, Os, Ba, Ra ] b) [ B, Si, Ge, As, Se, Sb, Te ] c) [ C, N, P, S, Cl, Br, I ]
43) Which of the following sets is a representation of periodic table metalloids?
a) [ Mg, Co, Ga, In, Os, Ba, Ra ] b) [ B, Si, Ge, As, Se, Sb, Te ] c) [ C, N, P, S, Cl, Br, I ]
44) Which of the following is NOT a physical property of the element copper?
a) metallic luster b) ductile c) malleable d) translucent
True or False: Read the statement, decide if the statement is true or false, then bubble A for true or B for false.45) T / F : The Periodic Table arranges the elements according to their properties.
46) T / F : In the Periodic Table, elements with similar properties are found in the same period (row).
47) T / F : The ultimate goal of scientific investigations is to explain and predict natural phenomena.
48) T / F : Pharmaceutical Chemistry is the study of substances found within the atomic nucleus.
49) T / F : In the scientific method, testing and experimenting are basically the same thing.
50) T / F : In the scientific method, a hypothesis and a theory are basically the same thing.
51) T / F : A pure substance can be either a homogeneous sample of matter or a heterogeneous sample of matter.
52) T / F : Every sample of a given pure substance can have different physical and chemical properties.
53) T / F : Every sample of a given pure substance has exactly the same chemical composition.
54) T / F : A pure substance cannot be separated into other substances without changing its identity.
55) T / F : A pure substance is an element and never a compound.
56) T / F : A solution in which water is the solvent is referred to as an aqueous solution.
57) T / F : The volume of an object is the amount it weighs.
58) T / F : In the Periodic Table, elements within a period have many similar properties.
59) T / F : The noble gases do not fit into other classes within the Periodic Table because of their non- reactive natures.
60) T / F : The micro-electronics revolution, which has resulted in PCs, smart-phones, digital cameras, and hundreds of other gadgets that are changing global communication, business, economies, and politics, is based upon semi-conducting elements.
*** continued ***
Diagram:
Use the three diagrams below to answer the next three questions.
61) Which diagram shows the boulder when its kinetic energy is at its greatest?
a) Diagram A b) Diagram B c) Diagram C
62) Which diagram shows the boulder when its potential energy is at its least?
a) Diagram A b) Diagram B c) Diagram C
63) Which diagram shows the boulder when its potential energy is at its greatest?
a) Diagram A b) Diagram B c) Diagram C
Multiple Choice – Terms: Select the term that best fits the given definition.
64) Numerical information.a) Quantitative Information b) Qualitative Information
65) Non-numerical information.a) Quantitative Information b) Qualitative Information
66) A broad generalization that explains a body of known facts or phenomena.a) Theory b) Law c) Hypothesis
67) A generalization that describes a wide variety of behaviors in nature.a) Theory b) Law c) Hypothesis
68) A testable statement.a) Theory b) Law c) Hypothesis
69) The study of the composition and structure of materials and the changes they undergo.a) Chemistry b) Biology c) Physics d) Botany e) Zoology
70) A logical approach to the solution of problems that lend themselves to investigations by observing, generalizing, theorizing, and testing.
a) Scientific Method b) Scientific Calculations c) Scientific Calculator d) Science Stuff
71) The study of the properties and transformations of matter in terms of fundamental physical properties.a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry
*** continued ***
72) The study of substances containing carbon and hydrogen.
A CB
a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry
73) The study of all substances and processes that occur in living things.a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry
74) The study of all substances not classified as organic chemicals.a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry
75) Resistance to change in motion.a) Inertia b) Weight c) Mass d) Matter e) Energy
76) A measure of the earth’s gravitational attraction for matter.
a) Inertia b) Weight c) Mass d) Matter e) Energy
77) A measure of the quantity of matter.
a) Inertia b) Weight c) Mass d) Matter e) Energy
78) Anything that has mass and occupies space.
a) Inertia b) Weight c) Mass d) Matter e) Energy
Lab book Investigations section:
Inv # 1
Term match-up: Match the term with its definition.
79) ______ Interaction
80) ______ Observation
81) ______ Conductivity
82) ______ Chemical Name
83) ______ Chemical Formula
84) ______ Classification System
85) ______ Clarity
86) ______ Color
87) ______ Solution
88) ______ Slovent
89) ______ Solute
90) ______ Soluble
91) ______ Insoluble
92) ______ Dissolve
93) ______ Quantitative Information
94) ______ Qualitative Information
Term match-up ( continued ): Match the term with its definition.
95) ______ Interpret
96) ______ Criteria
97) ______ Characteristics
98) ______ Homogenous
99) ______ Heterogeneous
100) _______ Analyze
101) _______ Suspension
102) _______ Mixture
103) _______ Distributed
104) _______ Particles
105) _______ Derive
106) _______ Colloidal
107) _______ Disperse
108) If sugar dissolves in water to form a solution, then why would a certain amount of sugar stop
dissolving in a certain amount of water? ____________________________________________________
_____________________________________________________________________________________
Multiple Choice:
109) If the mass of a solute is 10 g and its volume is 2 ml, what is its density ?
a) 0.05 g/ml b) 0.5 g/ml c) 5.0 g/ml d) 50 g/ml e) 500 g/ml
110) If the density of a solution is 20 g/ml and its volume is 5.0 ml, what is its mass ?
a) .100 g b) 1.00 g c) 10.0 g d) 100 g e) 0.01 g
111) If the density of a solvent is 6 g/ml and its mass is 120 g, what is its volume ?
a) .002 ml b) .02 ml c) .20 ml d) 2.0 ml e) 20 ml
112) The ability for an aqueous solution to transfer electrons between positive and negative poles is called:
a) conductivity b) ion exchangeability c) electron flowability d) all of the above
Inv # 2
Term match-up: Match the term with its definition.
113) _______ Substance
114) _______ Evaporation
115) _______ System
116) _______ Percentage
117) _______ Calculate
118) _______ Value
119) _______ Conclusion
120) _______ Procedure
121) _______ Record
122) _______ Physical Change
123) _______ Chemical Change
124) _______ Reversible
125) _______ Irreversible
126) _______ Complex
127) _______ Informative
128) _______ Uniformly
129) _______ Fermentation
130) _______ Effervescent
131) _______
132) Give three ( 3 ) examples of numbers that have digits in two decimal places.
________________ __________________ ________________
133) The investigation manual uses the word “test” often during experiments. Is this a correct usage of the
word test? (circle one) yes no
134) Where else in the world of science is the term “test” used? _______________________________
_______________________________________________________________________________
Inv # 3
Term match-up: Match the term with its definition.
135) _____ Property ( as used in science, not real estate )
136) _____ Sample
137) _____ Appropriate
138) _____ Alcohol
139) _____ Graduated ( as it applies to glassware )
140) _____ Collect
141) _____ Transfer
142) _____ Density
143) _____ Relationship
144) _____ Average
145) _____ Apparatus
146) _____ Compare
147) _____ Determine
148) _____ Evidence
149) _____ Experiment
150) _____ Appearance
151) _____ Cylindrical
152) _____ Assume
153) _____ Absorb
154) _____ Displacement
155) _____ Scientific Hypothesis
156) _____ Scientific Theory
157) _____ Scientific Law
Supplemental General Knowledge
What is Chemistry?Match-up:For each numbered term, enter the letter corresponding to the definition that best matches the term.____ 1- Chemistry A- Numerical information.____ 2- Scientific Method B- A broad generalization that explains a body of known facts or
phenomena.____ 3- Quantitative Information C- The study of the composition and structure of materials and the
changes they undergo.____ 4- Qualitative Information D- Non-numerical information.____ 5- Hypothesis E- A generalization that describes a wide variety of behaviors in nature.____ 6- Law F- A testable statement.____ 7- Theory G- A logical approach to the solution of problems that lend
themselves to investigations by observing, generalizing, theorizing, and testing.
____ 8– Organic Chemistry H- The study of the properties and transformations of matter in terms of fundamental physical properties.
____ 9- Inorganic Chemistry I- The study of substances containing carbon and hydrogen.____ 10- Physical Chemistry J- The study of all substances and processes that occur in living
things.____ 11- Biochemistry K- The Identification of materials and the qualitative and
quantitative determination of the composition of materials.____ 12- Analytical Chemistry L- The study of all substances not classified as organic chemicals.____ 13- Chemical M- A substance produced by or used in a chemical process.
Scientific Method:Put the following scientific method categories listed in the right column in their typical proper order as
explained and diagramed in your textbook. (Reminder: “Categories” are groupings of the individual scientific method steps that scientists take within a particular category grouping. Do not confuse categories with steps. For example: Testing is a category meaning to test or “confirm” or “challenge” a theory or hypothesis; and experiment is a step within the observing category.)14 ______ a- Theorizing15 ______ b- Generalizing16 ______ c- Testing (note: “Testing” is not “Experimentation” )17 ______ d- Observing
Short Answer:18, 19: What are the two categories of natural sciences? ___________________ _______________________
20: Into which of the above two categories of natural science does chemistry fall? ________________________
21, 22: Give two examples of a chemical: _______________________ ___________________________
23, 24: Name the two laws mentioned in the reading that are studied in chemistry: ____________ , _____________
25: What type of microscope mentioned in the reading can magnify a specimen 100 million times? ______________
True or False:26: T / F -- The ultimate goal of scientific investigations is to explain and predict natural phenomena.
27: T / F -- Pharmaceutical Chemistry is the study of substances found within the atomic nucleus.
Matter and EnergyMatch-up: _____ 1 – Mass A- Resistance to change in motion._____ 2 – Matter B- A measure of the earth’s gravitational attraction for matter.
_____ 3 – Energy C- A measure of the quantity of matter.
_____ 4 – Weight D- Anything that has mass and occupies space.
_____ 5 – Solid State E- A proven theory stating that matter cannot be either created nor destroyed in ordinary chemical or physical changes.
_____ 6 – Inertia F- The ability to cause change or the ability to do work.
_____ 7 – Kinetic Energy G- The energy of an object in motion.
_____ 8 – Potential Energy H- The energy that an object has because of its position or composition.
_____ 9 – Law of Conservation of Matter I – A proven theory stating that energy can be converted from one form to another, but it cannot be created nor destroyed in ordinary chemical or physical changes.
_____ 10 – Law of Conservation of Energy J- The state of any matter that has a definite shape and volume.
_____ 11 – Liquid State K-The state of any matter that has a definite volume but an indefinite shape.
_____ 12 – Physical Property L- The state of any matter that has neither a definite shape nor a definite volume.
_____ 13 – Properties M- Characteristics that enable us to distinguish one kind of matter from another.
_____ 14 – Intensive Physical Properties N –A type of property that can be observed or measured without altering the identity of a material.
_____ 15 – Extensive Physical Properties O –A type of physical property determined from the amount of matter present and includes mass, length, and volume.
_____ 16 – Gaseous State P – A type of physical property determined not from the amount of matter present and includes melting point, boiling point, density, ductility, malleability, color, crystalline shape, and refractive index.
_____ 17 – Changes of State Q – Any change in a property of matter that does not result in a change of identity.
_____ 18 – Physical Change R – The physical changes between gaseous, liquid, or solid forms.
_____ 19 – Chemical Property S – A type of property in reference to the ability of a substance to undergo a change that alters its identity.
_____ 20 – Exothermic T – Any change in which one or more substances are converted into different substances with different characteristic properties.
_____ 21 – Chemical Change (chemical reaction) U – The substances that undergo a chemical reaction.
_____ 22 – Precipitate V – The new substances produced by a chemical reaction.
_____ 23 – Products W – A solid that separates from a solution.
_____ 24 – Endothermic X – A process that releases heat.
_____ 25 – Reactants Y – A process that absorbs heat.
Short Answer:
26: What is the difference between weight and mass?
__________________________________________________________________________________________
27: What is the difference between kinetic energy and potential energy?
__________________________________________________________________________________________
28: What is the difference between extensive physical properties and intensive physical properties of matter?
__________________________________________________________________________________________
29: What is the difference between physical properties and chemical properties of matter?
___________________________________________________________________________________________
30: What is the difference between physical changes and chemical changes?
___________________________________________________________________________________________
31: What is the difference between exothermic processes and endothermic processes?
___________________________________________________________________________________________
Classification of MatterMatch-up:
____ 1- Law of Definite Composition A- A combination of two or more kinds of matter each of which retains its own composition and properties.
____ 2- Solutions B- A type of mixture in which the composition and properties are not uniform; they differ from point to point in the mixture.
____ 3- Phase C- Where portions of matter have both the same chemical and physical properties.
____ 4- Pure Substance D- A type of mixture in which the composition and properties are uniform throughout the mixture.
____ 5- Homogeneous E- Another way to describe homogeneous mixtures.
____ 6- Chemical Compound F- A homogeneous sample of matter that has the same composition and properties, whatever its sourcs.
____ 7- Heterogenous G- A substance that cannot be separated into other substances by any ordinary chemical change.
____ 8– Element H- A pure substance that can be decomposed into two or more simple substances by an ordinary chemical change.
____ 9- Mixture I – A law that states: A chemical compound contains the same elements
in exactly the same proportions by mass regardless of the size of the sample or source of the compound.
Short Answer:
Give two examples of a homogeneous mixture.
10)______________________________________________________________________________
11)______________________________________________________________________________
Give two examples of a heterogeneous mixture.
12)______________________________________________________________________________
13)______________________________________________________________________________
The Chemical ElementsMatch-up:
____ 1- Groups or Families A- The vertical columns of elements in the Periodic Table are referred to as these.
____ 2- Non-metal B- The name for the horizontal rows of elements in the Periodic Table.
____ 3- Periods C- An element that is a good conductor of heat and electricity.
____ 4- Metalloid D- An element that is a poor conductor of heat and electricity.
____ 5- Metal E- An Element that has some properties characteristic of metals and others characteristic of nonmetals.
Short Answer:6: Cuprum is the older name for which element? ______________________
7: Aurum is the older name for which element? _______________________
8: Ferrum is the older name for which element? _______________________
9: Natrium is the older name for which element? ______________________
10: The elements in Group 18 are known as ____________ ____________
11: In reference to the Periodic Table, what are the groups? ____________________________________________
12: In reference to the Periodic Table, what are the periods? ____________________________________________
The three general classes of elements are: 18: _______________ 19: ________________ 20: ________________.
21: A _________________ is somewhat like a metal, but not entirely.
22: All metals except for __________________ are solids under ordinary conditions.
True or False:
23) T / F : In the Periodic Table, elements within a period have many similar properties.
24) T / F : The noble gases do not fit into other classes within the Periodic Table because of their non-reactive natures.
25) T / F : The micro-electronics revolution, which has resulted in PCs, smart-phones, digital cameras, and hundreds of other gadgets that are changing global communication, business, economies, and politics, is based upon semi-conducting elements.
Units of MeasurementMatch-up:
____ 1- Meter A- A physical quantity of a defined size.____ 2- Fundamental Unit B- Objects or natural phenomena of constant value, easy to preserve
and reproduce, and practical in size that are used to define units for measuring.
____ 3- Kilogram C- The abbreviation for the International System of Units.____ 4- Conversion Factor D- A unit that is defined by a physical standard of measurement.____ 5- Second E- The SI standard unit for length.____ 6- Factor-label F- The SI standard unit for mass.____ 7- Derived Unit G- The SI standard unit for time.____ 8- Density H- A problem solving method based upon treating units in calculations
as if they are algebraic factors. ____ 9- Volume I- A ratio derived from the equality between two different units and can
be used to convert from one unit to the other.____ 10-Standards of Measurements J- A unit that can be obtained from combinations of fundamental units.____ 11- SI K- The amount of space occupied by an object.____ 12-Unit of Measurement L- A ratio of the mass of an object or substance to it’s volume.
Short Answer: What are the fundamental SI units for the following:
13) length: _____________ 14) mass: ________________ 15) time: ________________
16) temperature: __________________ 17) amount of substance: _________________
18: The system that uses units of inches, ounces, and pounds is known as the __________________ system.
19: The measurement system used by most scientists and countries of the world is the ________
Fill-the-chart:20 - 41
Prefix Symbol Exponential Factor Meaningtera 1,000,000,000,000giga Gmega 1,000,000
k 103
hecto 100deca dadeci 1/10 (0.1)centi 10-2
milli 1 / 1,000 (0.001)micro µ 1 / 1,000,000 (0.000001)nano 10-9
pico
Conversions: 42) 43) Express 24 meters in: centimeters; __________________ kilometers; _________________ 44) 45) Express 5.6 kilograms in: grams; __________________ milligrams; _____________
Calculations: Calculate the following:
46) 2 kg x 6 kg = ________
47) 2 m x 6 m = ________
48) 4 quarters ÷ 1 dollar = ________ (don’t forget to convert)
49) 75 dollars x 4 quarters = ________ ___________ (don’t forget to cancel units) 1 dollar
50) 40 cm x 2 cm = _________ (don’t forget to reduce)8 square
51) The density for a substance that has a mass of 600 grams and a volume of 20 cm3
52) The mass for a 40 mL solution sample that has a density of 2 grams per mL
53) The volume of a substance that weighs 10 grams and has a density of 2 grams per cm3
54) What volume of water, in liters, would be required to fill a tank 30 cm long, 20 cm wide, and 10 cm deep?
True or False:
55) T / F : Fundamental Units are also known as “Base Units”.
56) T / F : One liter is equal to one cubic decimeter.
57) T / F : 1 cg = 10 mg
58) T / F : 1 g = 100 cg
59) T / F : The volume of most kinds of matter changes with temperature.
60) T / F : To “calibrate” a measuring device means to adjust its scale reading to agree with a measurement standard.
Circle the answer: 61) What is more dense, cork or lead ?
62) What is more dense, a gas or a liquid ?
63) The area of a circle would be expressed in units that are: squared cubed other
64) The volume of a liquid would be expressed in units that are: squared cubed other
Heat and TemperatureMatch-up: ____ 1- Celsius A- A measure of the average kinetic energy of the particles in a sample of
matter.____ 2- Calorie B- The sum total of the kinetic energies of the particles in a sample of matter.____ 3- Heat Capacity C- A unit of temperature developed by some Swedish astronomer guy.____ 4- Joule D- The unit of temperature developed by an English Lord and is the
fundamental SI unit for temperature.____ 5- Specific Heat E- The degree scale for temperature used by the United States.____ 6- Kelvin F- An older unit originally defined as the quantity of heat required to raise the
temperature of 1 g of water from 14.5 degrees C to 15.5 degrees C.____ 7- Temperature G- The amount of heat energy needed to raise the temperature of a given
sample of matter by one Celsius degree. ____ 8- Heat (heat energy) I- The amount of heat energy required to raise the temperature of 1g of a
substance by one Celsius Degree.____ 9- Fahrenheit J – The SI unit for heat energy and all forms of energy.
10) Give the names of the two temperature scales that are commonly used in chemistry._______________________________________________________________________________________
11) How much heat would be absorbed by 75 g of iron, which has a specific heat index of 0.444, when heated from 22 degrees C to 28 degrees C?
_______________________________________________________________________________________
Conversions:12) Convert 30 degrees C to K. ___________________________________________________________
13) Convert -20 degrees C to K ___________________________________________________________
14) Convert 200 K to degrees C __________________________________________________________
15) Convert 110 calories to J _____________________________________________________________
16) Convert 22 kJ to calories _____________________________________________________________
17) Convert 275 calories to joules ________________________________________________________
18) Convert 355 calories to kilojoules _____________________________________________________
19) Convert 55 calories to joules _________________________________________________________
20) Convert 650 joules to calories _________________________________________________________
Calculations: Calculate the following:
A 4.0 g sample of glass was heated from 0oC to 41oC and was found to have absorbed 32 J of heat.
21) What is the specific heat of this type of glass?
_____________________________________________________________________________
22) How much heat did the same glass sample gain when it was heated from 41oC to 70o
___________________________________________________________________________________________________________________
23) Determine the specific heat of a material if a 12 g sample absorbed 48 J as it was heated from 20oC to 40oC.
______________________________________________________________________________
True or False:
25) T / F : Normal boiling and freezing points are those at 1 atm.
26) T / F : The direction of heat flow is determined by the temperature differences between two masses.
27) T / F : If the final temperature is lower than the initial temperature, then delta t is negative.
Chart: Complete the following chart:
Kelvin Celsius Fahrenheight
373.15 Boiling point of water
0o Freezing point of water
-320.44 Boiling point of nitrogen
-273.15 Lowest possible temp.
6,000 The sun’s surface temp.
100 Current temp outside
Using Scientific MeasurementsMatch-up:
____ 1- Significant Figures A- Refers to the closeness of a measurement to the true or accepted value of the quantity measured.
____ 2- Precision B- Refers to the agreement among the numerical values of a set of measurements of the same quantity made in the same way.
____ 3- Scientific Notation C- The numerical values in a measurement that consist of all the digits that are known with certainty plus one final digit, which is uncertain or estimated.
____ 4- Accuracy D- Numbers that are written in the form M x 10n.
Multiple Choice:5) The true volume of a liquid sample is 8.4125 mL. A student measures the volume of this sample three times
and records readings of 8.42 mL, 8.41 mL, and 8.40 mL. The student’s readings are: (circle one)a. Accurate b. Precise c. both d. neither
6) The true volume of a liquid sample is 8.4125 mL. A student measures the volume of this sample three times and records readings of 8.92 mL, 8.93 mL, and 8.94 mL. The student’s readings are: (circle one)
a. Accurate b. Precise c. both d. neither
7) The true volume of a liquid sample is 8.4125 mL. A student measures the volume of this sample three times and records readings of 8.92 mL, 8.41 mL, and 9.34 mL. The student’s readings are: (circle one)
a. Accurate b. Precise c. both d. neither
Conversions:8) In scientific notation Avogardo’s number is 6.022 x 1023. Write this number in non-scientific notation.
_________________________________________________________________________________
9) The mass of an electron is 0.0000000000000000000000000000009109 kg. Write this number in scientific notation: ___________________________________________________________
Diagram: Refer to the following three scales (A, B, C) for questions # 10 - 12
Scale A:
_______|___________|____________|____________|____________|___________|_________10 20 30 40 50 60
Scale B:
_|_____|______|______|______|______|______|_____|_____|______|______|______|______|___10 11 12 13 14 15
Scale C:
__|_____|______|______|______|______|______|______|______|______|______|______|______|____10.4 10.5 10.6 10.7 10.8 10.9
10) Which scale will have readings up to three ( 3 ) significant figures? A B C
11) Which scale will have readings up to two ( 2 ) significant figures? A B C
12) Which scale will have readings up to one ( 1 ) significant figures? A B C
True or False:
13) T / F : A set of measurements can be both accurate and precise.
14) T / F : A set of measurements can be precise without being accurate.
15) T / F : A set of measurements can be accurate without being precise.
16) T / F : A single measurement amongst a set of measurements can be accurate without the set being accurate.
17) T / F : A single measurement amongst a set of measurements can be accurate without the set being
precise.
18) T / F : A single measurement amongst a set of measurements can be precise without the set being precise.
19) T / F : A single measurement amongst a set of measurements can be precise without the set being
accurate.
20) T / F : Exact conversion factors have no uncertainty numbers.
21) T / F : Exact numbers can be considered to have an unlimited number of sig figs.
Rounding Off:
Round the following numbers to three (3) significant figures.
22) 42.68 g = _________________
23) 17.32 m = ________________
24) 2.7851 cm = _______________
25) 4.635 kg = ________________
26) 78.65 mL = _______________
Round off each of the following measurements to the indicated number of significant figures.
27) 35.27 g -- 3 sig figs: ___________________
28) 0.414 kL -- 2 sig figs: __________________
29) 87.257 dm -- 3 sig figs: ________________
30) 1.35K -- 2 sig figs: ____________________
31) 6250 cm -- 2 sig figs: __________________
32) 6.42 g -- 2 sig figs: ____________________
33) 7.535 mL -- 3 sig figs: _________________
34) 4.681 cm -- 2 sig figs: _________________
35) 56.45 kg -- 3 sig figs: _________________
Chart: Complete the following chart:
Measurement Examples Number of Sig Figs
36 438 g
37 26.42 m
38 1.7 cm
39 0.653 L
40 506 dm
41 10,050 mL
42 900.43 kg
43 4830 km
44 60 g
45 4830.0 L
46 60.0 K
47 0.06 g
48 0.0047 L
49 0.005o C
50 0.8 g
51 8.0 g
52 16.40 dm
53 35.000 L
54 1.60 sec
55 605.03 g
56 0.00603 mL
57 450 m
58 300.0 dm
59 0.8030 L
60 20.00 cm
61 0.000070 kg
62 350.0 K
Calculations: Calculate the following and express your answers with the correct number of sig figs:
63) 213.67 m + 98 m = _____________________________________
64) 6.43 L + 2.015 L = ____________________________________
65) 6.821 g + 2.0 g = _____________________________________
66) 107.38 km – 65 km = _____________________________________
67) 12.0 cm x 4.3 cm = ______________________________________
68) 2.50 g ÷ 0.04 cm3 = _____________________________________
69) 26.50 dm x 0.062 dm = ___________________________________
70) 1.30 mL ÷ 0.02 mL = _____________________________________
71) 2.30 cm x 10 cm x 6.01 cm = _______________________________
72) (6.3 x 104) + (2.1 x 105) = __________________________________
73) (23.5 x 105) – (2.35 x 106) = ________________________________
74) (6.85 x 107) ÷ (2.0 x 103) = _________________________________
75) (9.9 x 105) ÷ (3.0 x 1010) = _________________________________
76) (6.81 x 1010) ÷ (1.2 x 10-2) = ________________________________
77) (4.3 x 108) x (2.51 x 10-4) = _________________________________
78) (3 x 107) + (5 x 106) = _____________________________________
79) (4.6 x 105) + (3.2 x 105) = __________________________________
80) (5.7 x 106) x (2.8 x 109) = __________________________________
81) (7.7 x 10-12) ÷ (2.5 x 105) = __________________________________
82) 430.62 m + 6.1 m + 10.5300 m = _____________________________
83) 804.00 g ÷ 20 cm3 = ______________________________________
84) 68 – 3.1 x 103 = __________________________________________
85) 55.5 x 10-2 + .445 = _______________________________________
Chart: Complete the following chart:
Number Scientific Notation
86 4,325,045.2
87 0.00000361
88 85,000,000
89 0.0009
90 74,000
91 0.000005
92 30,000,000,000
93 864,000
94 0.000602
95 4700
96 2.31 x 10-7
97 5.3 x 104
98 7 x 10-5
99 4.2 x 10-6
100 45,000
101 0.0000027
102 301 x 1011
Solving Quantitative ProblemsMatch-up: ____ 1- Variable A- A quantity that can change in value.____ 2- inversely proportional B- A relationship between two variables in which dividing one by the other
gives a constant value.____ 3- directly proportional C- A relationship between two variables in which their product has a constant
value.
Short Answer:4) List and explain the four steps in problem solving.
1-__________________________________________________________________________________
2-__________________________________________________________________________________
3-__________________________________________________________________________________
4-__________________________________________________________________________________
Calculations:
5) Calculate the number of seconds in exactly one week. Answer here:_____________
6) What is the volume of a 12 g piece of gold? (d = 19.3 g/cm3 ) Answer here: _____________
7) An object travels at a speed of 7500 cm / s. How far will it travel in a day? Answer here: ____________
What type of relationship is illustrated between the variables A and B in each of the following?
8) As A increases, B decreases, and A x B = 35 ____________________________
9) As A increases, B increases, and A / B = ½ . _____________________________
The AtomMatch-up: ____ 1- Law of Multiple Proportions A- A law used in science that states: Matter can neither be created nor
destroyed.____ 2- Law of Conservation of Mass B- A law used in science that states: If two or more different
compounds are composed of the same two elements, the masses of the second element combined with a certain mass of the first element can be expressed as ratios of small whole numbers.
____ 3- Law of Definite Composition C- A law used in science that states: Energy can neither be created nor destroyed.
____ 4- Law of Conservation of Energy D- A law used in science that states: Every chemical compound has a definite composition by mass.
Short Answer:7 -11) List the five essential points of Dalton’s atomic theory:
1-__________________________________________________________________________________
2-__________________________________________________________________________________
3-__________________________________________________________________________________
4-__________________________________________________________________________________
5-__________________________________________________________________________________
True or False:12) T / F : The word “atom” comes from an Epytian word meaning dividable.
13) T / F : Dalton developed his Atomic Theory mainly from his observations of gases in the atmosphere.
14) T / F : Mass is always conserved in chemical reactions.
15) T / F : In all chemical reactions, a portion of energy used by the reaction is destroyed.
16) T / F : Chemical reactions are simply the combination, separation, or rearrangement of atoms.
17) T / F : Scientists often use more than one method to gather data.
Fill-in-the-blanks:18: ________________________ was the name of the Greek dude that lived around 400 BC who came up with the
name “Atom” for tiny particles that can’t be divided any further.
19: ________________________ , another Greed dude who lived about 50 years later than the Greek dude in number xx above did not believe in atoms, but rather that all matter was ____________________________ .
20: Over 2,000 years later than the Greek dudes above, an English dude named _____________ ______________ , who was a school teacher, developed a theory that in five basic statements summarizes the Atomic Model.
Chart: Complete the following chart:
Quiz # Compound Name Compound Symbol
21 Carbon Monoxide
22 CO2
23 Di-hydrogen Monoxide
24 NaCl
25 C6H12O6
26 Sulphuric Acid
27 Hydrochloric Acid
28 Nitric Acid
29 CaCO3
30 Hydrogen Peroxide
31 Ethanol
The Structure of the AtomMatch-up: ____ 1- Atom A- The short-range proton-neutron, proton-proton, and neutron-neutron forces that
hold the nuclear particles within an atom together.____ 2- Atomic Structure B- The identity and arrangement of smaller particles within atoms.____ 3- Electron C- A negatively charged sub-atomic particle.____ 4- Nucleus D- The positively charged dense center portion of the atom that contains nearly all of
it’s mass but takes up only an insignificant fraction of it’s volume.____ 5- Proton E- A subatomic particle that has a positive charge equal in magnitude to the negative
charge of an electron and is present in atomic nuclei.____ 6- Neutron F- Atoms of the same element that have different masses.____ 7- Nuclear Forces G- The smallest unit of an element that can exist alone or in combination with other
elements.____ 8- Isotopes H- An electrically neutral, sub-atomic particle found in atomic nuclei.
True or False:9) T / F : Hydrogen and its isotopes have different nuclei.
10) T / F : Every element has exactly the same number of protons as electrons.
11) T / F : Every element has isotopes.
12) T / F : The only difference between isotopes of the same element is the number of electrons.
13) T / F : Nuclear forces are responsible for the delicate balance held within an atom.
Fill-in-the-blanks:14: The discovery of _________________ was made in 1897 by an English physicist dude named Sir Joseph John
Thompson who built and used cathode-ray tubes to identify these sub-atomic ______________. Although cathode-ray tubes were useful in figuring-out the structure of the ___________, their real usefulness came about 50 years later when they were used to make the first _________ sets in America which resulted in the end of the radio entertainment era. Further refinement of the cathode-ray tube, which energizes different types of ________ to make different colors, resulted in a type of sign that used to light-up the __________ strip but are now a rare sign to see.
15: An American physicist dude named Robert Millikan figured out the mass of an __________________ in 1909.
16: In 1909 a dude from New Zealand named Ernest Rutherford discovered that the atom has a _________________ and that it gives off a ___________________ charge.
17: In 1986, the ______________ Prize in science achievement was shared by Ernst Ruska, Gerd Binning, and Heinrich Rohrer for their work on ________________________.
Diagram:18) In the space below, make a model sketch of the Boron atom showing and labeling all sub-atomic particles and
their proper locations. (12 points)
Weighing and Counting AtomsMatch-up:
____ 1- Atomic Number A- The number of particles in exactly one mole of a pure substance.
____ 2- Mass Number B- The amount of a substance that contains the same number of particles as the number of atoms in exactly 12 grams of carbon-12.
____ 3- Nuclide C- The relative atomic mass of atoms of a nuclide.
____ 4- Atomic Mass Unit D- The weighted average of the atomic masses of the naturally occurring isotopes of an element.
____ 5- Atomic Mass E- A general term for any isotope of any element.
____ 6- Average Atomic Mass F- Symbolized by the letter u, and is exactly 1/12th the mass of a carbon-12 atom, or 1.66 x 10-24 grams.
____ 7- Nuclide Atomic Mass G- The mass of an atom that is expressed in atomic mass units.
____ 8- Mole H- The total number of protons and neutrons in the nucleus of an isotope.
____ 9- Avogadro’s Number I- The abbreviation for the Mole.
____ 10- Molar Mass J- The number of protons in the nucleus of each atom of that element.
____ 11- mol K- The mass in grams of one mol of an element.
Calculations:
12 – 15) Determine the number of protons, electrons, and neutrons in each of the following isotopes.
12) sodium-23 | 13) calcium-40P = _________ | P = _________
|E = _________ | E = _________
|N = ________ | N = ________
---------------------------------------------------------------------------------------------------------------------------------14) 64
29 Cu | 15) 10847 Ag
P = _________ | P = _________ |
E = _________ | E = _________ |
N = ________ | N = ________---------------------------------------------------------------------------------------------------------------------------
16 – 18) Determine and write both the nuclear symbol and the hyphen notation for each of the following described neutral isotopes using the given information.
16) Mass number = 28, Atomic number = 14
17) 26 Protons and 30 Neutrons
18) 56 Electrons and 82 Neutrons
Calculations continued:
19) To three decimal places, what is the relative atomic mass of Potassium ? ____________________________
20) To three decimal places, what is the molar mass of Calcium ? ______________________________
21) What is the mass in grams of 2.00 mol N ? _______________________________
22) What is the mass in grams of 3.01 x 1023 atoms of Cl ? _________________________
23) How many moles are in 12.15 g Mg ? ______________________________
24) How many moles are in 1.50 x 1023 atoms of F ? ____________________________
25) How many atoms are contained in 2.50 mol Zn ? ____________________________
26) How many atoms are contained in 1.50 g C ? _____________________________
True or False:
27) T / F : The term atomic weight is sometimes used synonymously with the term atomic mass.
28) T / F : The term nuclide atomic mass is sometimes used synonymously with the term relative atomic
mass.
29) T / F : The isotopes protium, deuterium, and tritium are isotopes of helium.
30) T / F : Most isotopes are identified only by their mass numbers and have no individual names.
31) T / F : Avogadro was smart Spaniard who got his bachelor’s degree at the age of 16.
32) T / F : Most elements occur naturally on Earth as isotopes.
33) T / F : The super script placed before an element’s symbol is that element’s mass number.
34) T / F : The subscript placed before an element’s symbol is that element’s atomic number.
Chemistry Investigation # 5 Pre-read Quiz / 54
1. Define “Composition”: ______________________________________________________________
2. Define “Compound”: _______________________________________________________________
3. Define “Formula”: ________________________________________________________________
4. Define “Exploration”: ______________________________________________________________
5. Define “Residue”: _________________________________________________________________
6. Define “Integer”: __________________________________________________________________
7. Define “System”; _________________________________________________________________
8. Explain what an “evaporating dish” is: _______________________________________________
9. Explain what a “crucible” is: ________________________________________________________
10. Explain the difference between an “evaporating dish” and a “crucible” is: _____________________
11. A student weighs a crucible and a crucible lid three times ( 3 trials ) and obtains the following data:
trial # 1: 5.02 grams trial # 2: 4.96 grams trial # 3: 5.00 grams
What is the average weight of the crucible w/ lid? ______________________
A student puts a strip of magnesium metal ribbon in a crucible and covers the crucible with a lid then weighs the
system three times and obtains the following weights:
trial # 1: 7.02 grams trial # 2: 6.96 grams trial #3: 7.00 grams
12. What is the average weight of the system? ______________________
13. What is the calculated weight of the magnesium? ______________________
14. Explain what it means to heat a system gently. ________________________________________
_______________________________________________________________________________
15. Explain what it means to heat a system strongly. _____________________________________
______________________________________________________________________________
16. Explain what a mathematical operation is: ____________________________________________
______________________________________________________________________________
17. List the four ( 4 ) basic operations of mathematics:
_____________________________________
_____________________________________
_____________________________________
_____________________________________
18. Give the symbol for magnesium: ______________
19. Give the name for Mg: ______________________
20. Give the symbol for copper: __________________
21. Give the symbol for sulphur: _________________
22. Give the symbol for oxygen: _________________
23. Give the formula for the compound: sulfate ____________________
24. Give the formula for the compound: copper (II) sulfate ____________________________________
25. Explain what “hydrated” means: _______________________________________________________
26. Explain what it means to make a “prediction”: ____________________________________________
__________________________________________________________________________________
27. Explain what “Expansion of an Idea” means: _____________________________________________
__________________________________________________________________________________
Chemistry Investigation # 4 Pre-read Quiz
28. Define “Pure Substance”: ______________________________________________________________
29. Define “Heating”: ________________________________________________________
30. Define “Cooling”: _______________________________________________________
31. Define “ Physical Change”: _________________________________________________________
32. Define “Chemical Change”: _________________________________________________________
33. Define “System”; _________________________________________________________________
34. Define “ Evidence” : ______________________________________________________________
35. How many phases ( or states ) of matter are there? _______________ and what are their names? :
______________________ _______________________ _____________________
36. Are phase changes physical or chemical in nature? ( circle one )
37. What is a coordinate axis? ( hint: think graph ) _____________________________________________
Chemistry Investigation # 2 Pre-read Quiz
38. Define “Evaporation”: ______________________________________________________________
_______________________________________________________________
Round the following weights to two ( 2 ) decimal places: ( don’t forget to include the units )
39. 05.8556 g ______________
40. 11. 45678 g ______________
41. 3.9876 g ______________
42. 1.94587 g ______________
43. Define “Physical Property”: ________________________________________________________
44. Define “Chemical Property”: _______________________________________________________
45. Define “ Physical Change”: _________________________________________________________
46. Define “Chemical Change”: _________________________________________________________
47. Define “system”; _________________________________________________________________
48. Give the chemical formula for ordinary table salt: _______________
49. Give the chemical formula for the element Calcium: _____________
Chemical Names and Formulas
Terms:
Define the following terms:
Chemical name:
Chemical formula:
Chemical compound:
ion:
monatomic ion:
binary compound:
Nomenclature:
polyatomic ion:
oxyanion:
oxyacid:
salt:
Oxidation Numbers
Match-up:
____ 1- Oxidation number A- Numbers that are assigned to the atoms in molecules, icluding molecular ions, to show the general distribution of electrons among the bonded atoms. ____ 2- Oxidation state B- Also called oxidation state.
True or False:3) T / F : An uncombined element has an oxidation number of zero.4) T / F : A monatomic ion has an oxidation number equal to its charge.5) T / F : Flourine has an oxidation number of -1 in all compounds.6) T / F : Oxygen has an oxidation number of -2 in almost all compounds.7) T / F : Hydrogen has an oxidation number of -1 in all compounds except those with metals, in
which it has an oxidation number of +1.8) T / F : The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion.9) T / F : The algebraic difference of the oxidations number of all atoms in a polyatomic ion is equal to zero.10) T / F : The algebraic sum of the oxidation numbers of all atoms in a neutral compound is equal to the charge of the ion.
Fill-in-the-blank: Select the word or phrase that best completes each sentence.
11. Oxidation numbers are also called oxidation ________________ .
a. States b. Levels c. Charges d. Elements e. Atoms
12. The algebraic ________ of the oxidation numbers of all atoms in a neutral compound is ______ .
b. Sum , Zero b. Difference , Neutral c. Difference , Zero
13. The algebraic ________ of the oxidation numbers of all atoms in a ____________ ion is equal to the
charge of the ion.
c. Total , Monatomic b. sum , diatomic c. sum , polyatomic
14. An uncombined element has an oxidation number of ________.
d. three b. two c. one d. zero
15. A _____________ ion has an oxidation number equal to its charge.
e. polyatomic b. monatomic c. catatomic d. diatomic
Using Chemical Formulas
Multiple Choice: Select the term that best fits the given definition.
2. The sum of the atomic masses of all the atoms represented in formula of any compound or polyatomic
ion.
a. formula weight b. formula mass c. atomic mass d. atomic weight
3. The percent by mass of each element in a compound.
a. mass composition b. mass percent c. percent composition
Calculations: For each of the following tasks, select the correct answer.
4. Calculate the formula mass for H2SO4.
a. 9.807 u b. .9807 u c. 98.07 u d. 980.7 u e. .09807 u
5. Calculate the formula mass for Ca(NO3)2.
a. 16.409 u b. 1.6409 u c. 1640.9 u d. .16409 u e. 164.09 u
6. Calculate the molar mass for NaNO3.
a. 8.49947 g b. 84.9947 g c. 849.947 g d. .849947 g
7. Calculate the molar mass for Ba(OH)2.
a. .17134 g b. 1.7134 g c. 17.134 g d. 171.34 g
8. Calculate the number of moles contained in 11.0 grams of CO2.
a. .0250 mol b. 0.250 mol c. 02.50 mol d. 025.0 mol
9. Calculate the number of moles contained in 6.60 grams of (NH4)2SO4.
a. .00500 mol b. 0.0500 mol c. 00.500 mol d. 005.00 mol
10. Calculate the number of moles contained in 4.5 kg Ca(OH)2.
a. 0.61 mol b. 6.10 mol c. 61.0 mol d. 610 mol
11. Calculate the percent composition of lead in PbCl2.
a. .7451 % b. 7.451 % c. 74.51 % d. 745.1 %
12. Calculate the percent composition of barium in Ba(NO3)2.
a. .52548 % b. 5.2548 % c. 52.548 % d. 525.48 %
13. How many grams of oxygen would be contained in 175 grams of the compound Magnesium hydroxide
which is 54.87 % oxygen by mass ?
a. .960 g b. 9.60 g c. 96.0 g d. 960 g
Determining Chemical Formulas
Match-Up: For each of the following terms on the left, select from the right its definition.
1) _____ simplest formula A – The form of a formula that consists of the symbols for the elements combined, with subscripts showing the smallest whole-number
ratio of the atoms.2) _____ empirical formula B – Another way to say “Empirical Formula”.
Calculations: Evaluate each of the following word problems.
3) A compound is found to contain 36.48% sodium, 25.41% sulfur, and 38.02% oxygen. Find it’s simplest
formula.
4) Find the simplest formula of a compound found to contain 53.70% iron and 46.30% sulfur.
5) Analysis of a compound indicates that it contains 1.04 g K, 0.70 g Cr, and 0.82 g O. Find it’s simplest
formula.
6) If 4.04 g N combine with 11.46 g O to produce a compound with a formula mass of 108.0 u, what is the
molecular formula of this compound?
7) The formula mass of a compound is 92 u. Analysis of a sample of the compound indicates that it contains
0.606 g N and 1.390 g O. Find it’s molecular formula.
History of the Periodic Table
Match-up:
____ 1- Ionic Radius A- One half the distance between the nuclei of identical atoms joined in a molecule.
____ 2- Atomic Radius B- Any process that results in the formation of an ion.____ 3- Ionization Energy C- The energy required to remove one electron from an atom of an
element.____ 4- Electronegativity D- One half the diameter of an ion in an ionic compound.____ 5- Anion E- An ion with a positive charge.____ 6- Cation F- An ion with a negative charge.____ 7- Valence Electron G- The electrons available to be lost, gained, or shared in the formation
of chemical compounds.____ 8- Ionization H- A measure of the ability of an atom in a chemical compound to
attract electrons.
True or False:9) T / F : Atomic radii decrease from right to left across a period in the Periodic Table.
10) T / F : Atomic radii increase from down to up across a group in the Periodic Table.
11) T / F : Period trends are patterns that exist in the Periodic Table groups.
12) T / F : Group trends are patterns that exist in the Periodic Table periods.
13) T / F : Metals are more electronegative than non-metals.
Short Answer:
15. State the general period and group trends among main-group elements with respect to each of the following:
a. Atomic radii ____________________________________________________________________
b. First ionization energy ____________________________________________________________
c. Electron affinity _________________________________________________________________
d. Ionic radii ______________________________________________________________________
e. Electronegativity ________________________________________________________________
16. Among the main-group elements, what is the relationship between group number and the number of valence
electrons among group members? __________________________________________________________
_________________________________________________________________________________________
17. ( part A ) In general, how do the periodic properties of the d-block elements compare with those of the main-
group elements? _________________________________________________________________________
__________________________________________________________________________________________
( part B ) Explain your reasoning for the comparisons you made in part A above: ______________________
__________________________________________________________________________________________
__________________________________________________________________________________________
Rules for determining significant figures involving zeros_____________Rule________________________________________________Examples_____# of sig fig_____________________________________________________________________________________________1. All nonzero digits are significant. 438 g 3
26.42 m 4 1.7 cm 2
0.653 L 3
2. All zeros between two nonzero digits are significant. 506 dm 3 10,050 mL 4
900.43 kg 5
3. Zeros to the right of a nonzero digit, but to the left of an understood 4,830 km 3 decimal point, are not significant. If such zeros are known to have been 60 g 1 measured, however, they are significant and should be specified as such 4,830. L 4 by inserting a decimal point to the right of the zero. 60. K 2
4. In decimals less than one, zeros to the right of a decimal point that are 0.06 g 1 to the left of the first non-zero digit are never significant. They are simply 0.0047 L 2 placeholders. 0.005o 1 5. In decimals less than 1, the zero to the left of the decimal is never significant. 0.8 g 1 It is there to make sure the decimal point is not overlooked. 6. All zeros to the right of a decimal point and to the right of a nonzero digit 8.0 dm 2 are significant. 16.40 g 4
35.000 L 5 1.60 sec 3
Rules for Rounding Off Numbers
If the digit immediately to the right of the last Then the last significant Example (rounding for 3significant digit you want to retain is: digit should: significant figures):
1) Greater than 5 be increased by 1 42.68 g → 42.7 g
2) Less than 5 stay the same 17.32 m → 17.3 m
3) 5, followed by nonzero digit(s) be increased by 1 2.7851 cm → 2.79 cm
4) 5, not followed by nonzero digit(s), andpreceded by an odd digit be increased by 1 4.635 kg → 4.64 kg
(since 3 is odd)5) 5, not followed by nonzero digit(s), and
the preceding significant digit is even stay the same 78.65 mL → 78.6 mL (since 6 is even)
In addition or subtraction, the arithmetic result should be rounded off so that the final digit is in the same place as the leftmost uncertain digit.
In multiplication and division, the arithmetic product or quotient should be rounded off to the same number of significant figures as in the measurement with the fewest significant figures.
T(K) = t(Co) + 273.15 t(Co) = 5/9 x [t(Fo) – 32] one calorie = 4.184 J
specific heat = heat lost or gained / mass (g) x change in temperature (Co)
SI prefixes
Prefix Symbol 1000m 10n Decimal Short scale Long scale Scientific notation Since[n 1]
yotta Y 10008 10 24 1000000000000000000000000Septillion Quadrillion 1E24 1991zetta Z 10007 10 21 1000000000000000000000Sextillion Trilliard 1E21 1991exa E 10006 10 18 1000000000000000000Quintillion Trillion 1E18 1975peta P 10005 10 15 1000000000000000Quadrillion Billiard 1E15 1975tera T 10004 10 12 1000000000000Trillion Billion 1E12 1960giga G 10003 10 9 1000000000Billion Milliard 1E9 1960mega M 10002 10 6 1000000 Million 1E6 1960kilo k 10001 10 3 1000 Thousand 1E3 1795hecto h 10002/3 10 2 100 Hundred 1E2 1795deca da 10001/3 10 1 10 Ten 1E1 1795
10000 10 0 1 One – –deci d 1000−1/3 10 −1 0.1 Tenth 1E-1 1795centi c 1000−2/3 10 −2 0.01 Hundredth 1E-2 1795milli m 1000−1 10 −3 0.001 Thousandth 1E-3 1795micro μ 1000−2 10 −6 0.000001 Millionth 1E-6 1960nano n 1000−3 10 −9 0.000000001 Billionth Milliardth 1E-9 1960pico p 1000−4 10 −12 0.000000000001 Trillionth Billionth 1E-12 1960femto f 1000−5 10 −15 0.000000000000001 Quadrillionth Billiardth 1E-15 1964atto a 1000−6 10 −18 0.000000000000000001 Quintillionth Trillionth 1E-18 1964zepto z 1000−7 10 −21 0.000000000000000000001 Sextillionth Trilliardth 1E-21 1991yocto y 1000−8 10 −24 0.000000000000000000000001 Septillionth Quadrillionth 1E-24 1991
1. ̂ The metric system was introduced in 1795 with six prefixes. The other dates relate to recognition by a resolution of the CGPM.
