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Fall Final Exam Review

Scientific Method

1- Which of the following is the most important thing with regard to protecting your eyes while in a science laboratory?a. Never look directly into a light source.b. If you get a chemical in your eyes, immediately

go to an eyewash station and flush your eyes and eyelids for 15 minutes.

c. Always wear safety goggles while performing laboratory work, including cleanup

d. Do not wear contact lenses while in the lab.

Scientific Method (Continue)

1- The observation that the sun sets in the west would be considered.a. a scientific law. c. a scientific

modelb. a scientific theory d. an inference

(conclusion)2- A series of orderly steps used to solve problems is

a. the experimental process. c. the scientific theory.

b. A procedure. d. the scientific method.

Scientific Method (Continue)1- Which question cannot be answered by

experimentation?a. Does penicillin kill Salmonella bacteria?b. Is rabies caused by a virus?c. Did a comet kill the dinosaurs?d. Can radiation cause cancer?

2- Before beginning an experiment, you should always ______.a. mix all the solutions together c. weigh all

substancesb. read all instructions d. answer pre-lab

questions

Scientific Method (Continue)Scientists wished to determine if a new type of antibiotic, called Antibiotic F, was effective against a particular type of bacteria that causes pneumonia. To test the antibiotic, the scientists enlisted 100volunteers, who were all suffering from pneumonia. The scientists gave 50 of the volunteers Antibiotic F for 10 days. The remaining 50 volunteers were given a sugar pill (called a placebo) that looked like the antibiotic. A volunteer was considered to be cured when their temperature remained normal (37oC) for three days.

Scientific Method (Continue)1- What problem was being investigated by the scientists?

a. Is pneumonia caused by bacteria?b. Is Antibiotic F effective against pneumonia causing bacteria?c. How many people can be cured of pneumonia?d. How many days does it take to cure pneumonia?

2- What was the experimental group?a. The bacteria.b. The volunteers that received the antibiotic.c. The volunteers that received the placebo.d. The sugar pill.

3- Was there an experimental control (group)?a. Nob. Yes, the bacteria.c. Yes, the volunteers that received the antibiotic.d. Yes, the volunteers that received the placebo (sugar pill).


1- What type of observation is “The water temperature is 25oC”?a. Subjective b. Qualitative c. Quantitative d. Vector

2- Scientist test a hypothesis by a. formulating questions. c. designing models.b. performing experiments. d. drawing conclusions.

3- The metric unit for volume of a fluid isa. liters b. meters b. c. grams d. cubic centimeters (cm3)

Scientific Method (Continue)1- The figures to the right represents a graduatedcylinder before and after an objectwas placed in it. What is the volumeof the object?

a. 14 cm3

b. 15 mlc. 20 mld. 24 cm3


25 Graph #1 – The relationship between time and and the temperature of a sodium

20 bicarbonate solution. Temperature

15

10

5

0 2 4 6 8 10 12

Time

1- In a graph, the independent variable isa. Temperatureb. Timec. Sodium bicarbonated. Decreasing (going down)

2- An appropriate interpretation of the data in the graph is

a. As time decreases, the temperature decreases and then remains the same.b. As time increases, the temperature goes down.c. As the temperature goes down, the time increases.d. As time increases, the temperature goes down and then remains the same.

Density (Continue)2- A block of maple wood

with a volume of 405 cubic centimeters and a density of 0.67 g/cm3 is sawed in half. The density of the two smaller blocks is now —

A one-fourth the original density

B one-half the original density

C two times the original density

D the same as the original density

Density1- The density of a 10.0 gram liquid that has a volume of 5 ml is ________.

a. 20 g/ml c. 5 g/mlb. 2 g/ml d. 0.5 g/ml

2- Methanol has the density of 0.79g/ml. How much would be the mass of 589ml of methanol?

mass = density x volume = 0.79 g/ml x 589 ml = 465.31g3- Copper has the density of 8.90 g/ml. What would be the volume of 746g

sample of copper? volume = mass/density= 465.31g/(8.90g/ml)=52.28ml4- Calculate the density of a solid, knowing that the mass is 123.4g and the

volume is 14.3ml.Density= mass/volume = 123.4g/14.3ml = 8.63g/ml 5- the tendency of a less dense object to float in a more dense liquid is

calleda. viscosityb. densityc. sublimationd. buoyancy

Density (Continue)

1- Swimmers find that they can float more easily in the ocean than in a freshwater pond. The most likely reason for this phenomenon is that the —

A viscosity of pond water is greater than that of ocean water

B density of ocean water is higher than that of pond water

C temperature of pond water is lower than that of ocean water

D mass of ocean water is greater than that of pond water

Density (Continue)

1- The resistance of a fluid to flow is referred to as a. Pressure b. energyc. Viscosity d. shape

Viscosity

Heating Curve of water

Bonding 1. What kind of chemical bond is formed when electrons are

transferred from one atom to another?a. Covalent b. ionicc. metalllic d. transition

2. In the formula Fe2O3, what is the oxidation number for iron?a. 3+ b. 4+/- c.3- d. 2+

3. A group of atoms that acts as one charged atom is a ______.a. Molecule c. positive ionb. negative ion d. polyatomic ion

4. The formula for Calcium Carbonate is ________ . a. CCa4 b. C2CO3 c. CaCO3 d. Ca3OH

Bonding (Continue)1- The name for Ca(OH)2 is ________.

a. calcium hydroxide c. hydroxide calcium

b. calcium oxygen hydrogen d. calcium dihydroxide

2- The name for CCl4 is ________.a. carbon tetrachloride c. carbon chlorideb. carbon chlorine d. chlorine carbon

3- What type of bond does the chemical compound KCl contain?a. ionic c. both ionic and covalentb. covalent d. polar

Bonding (Continue)

1- Water is a polar molecule because it ______.a. shares electronsb. shares electrons

unequally c. transfers electronsd. transfers electrons

unequally

Periodic table

Periodic Table (Continue)1-The element Magnesium is classified as a

a. Nobel gas b. Transition metal c. Alkaline-Earth metal d. Halogen

2- What do elements H, Na, and Li all have in common?a. They have one valence electron. c. They belong in same

period.b. They commonly form covalent bonds. d. They take electrons

during bonding.3- Elements in groups 3 – 12 on the periodic table are called ______.

a. metalloids c. nonmetalsb. transition metals d. ions

4- Hydrogen is grouped with the alkali metals because it ______.a. is a metal c. is a gasb. has one valence electron d. does not easily form

compounds

Periodic Table (Continue)

1- Atoms of the same element with different numbers of neutrons are called ______.a. groups c. clustersb. Isotopes d. ions

2- Antimony (Sb) is a ______.a. metal c. metalloidb. nonmetal d. transition meta

Periodic Table (Continue)

1- Substances that conduct electric current under certain conditions are most likely ______.

a. metals b. metalloidsb. c. nonmetals d. noble gases

2-What is the oxidation number for Silicon?a. 3+ b. 4+/- c. 3- d. 2+

3- Where are metals found on the periodic table?a. left side c. along the staircaseb. right side d. at the bottom

4- Horizontal rows on the periodic table are called ______.a. groups c. clustersb. families d. periods

5- What kind of chemical bond occurs when atoms share electrons?

a. covalent b. metallic c. ionic d. mixed

Periodic Table (Continue)1- Which element has 35 protons?

a. chlorine c. argonb. bromine d. iodine

2- A certain atom has 92 protons, 92 electrons and 146 neutrons. Its mass number is ______.a. 184 c. 238b. 146 d. 54

4- How many electrons are needed in the outermost energy level of

most atoms to be chemically stable?a. 2 b. 6 c. 8 d. 10

5- Group 17 on the periodic table is known as the ______.a. alkaline earth metals c. halogensb. alkali metals d. noble gases

Periodic Table (Continue)1. Which of the following is NOT a property of nonmetals?

a. can be solids, liquids or gases c. dullb. conduct electricity d. brittle

2. The nucleus of an atom contains the ______.a. protons only c. protons and neutronsb. neutrons only d. protons and electrons

3. The chemical symbol for Potassium is ______.a. P b. K c. Po d. Pt

4. Which of the following is NOT a characteristic of metals?a. are shiny c. brittleb. are malleable d. conduct electricity

Chemical Reactions

1- What type of reaction is 2KCl 2K + Cl2?a. synthesis c. single replacementb. decomposition d. double replacement

2- What type of reaction is 3NaOH + FeCl3 NaCl + Fe(OH)3?

a. Synthesis c. single replacementb. Decomposition d. double replacement3- What type of reaction is 2KCl 2K + Cl2?a. Synthesis c. single replacementb. Decomposition d. double replacement

Rock Cycle

Rock Cycle (Continue)

rock cycle

Rock Cycle (Continue)

Chemical Reactions (Continue)

Chemical Reactions (Continue)1- A chemical reaction in which energy is released is ______.

a. exothermic c. flammableb. endothermic d. decomposing

2- Each substance on the left side of the arrow in a chemical equation is a ______.a. reactant b. catalyst c. product d. inhibitor

3- Coefficients (the numbers in front of) the chemical formulas in a chemical equation show

a. the number of atoms of each element.b. the number of molecules.c. the number of reactants.d. the number of products.

4- Subscripts represent a. the number of atoms of each element.b. the number of molecules.c. the number of reactants.d. the number of products


1- Which of the following shows a correctly balanced chemical equation for the following reaction?

a. 2 Mg + O2 MgO c. Mg + 2 O2 MgOb. 2 Mg + O2 2 MgO d. 2 Mg + 2 O2 2 MgO2- When one element displaces another element

in a compound, this reaction is a ______.a. synthesis c. single replacementb. decomposition d. double replacement


1- According to the law of conservation of mass, how much zinc was present in the zinc carbonate?

A 40 gB 88 gC 104 gD 256 g

Properties of Matter1- The image that represents a solid is _____ .

a. A b. Bc. C d. None of the above.

2- The phase that possesses the greatest amount of energy would be ______.

a. A b. Bc. C d. None of the above

3- Most matter ______ when heated.a. condenses b. expands c. contracts d. solidifies

Properties of Matter (Continue)1- As a sample of matter is cooled, its particles ______.

a. move more slowly c. do not changeb. move more quickly d. stop moving

2- The change of state in which a gas changes into a liquid is ______.a. melting b. sublimationc. freezing d. condensation

3- Vaporization refers to the phase change froma. liquid to gas. c. solid to liquid.b. gas to liquid. d. liquid to solid.

4- All matter is made up of tiny particles that are in constant motion is known as ______.

a. law of conservation of mass c. kinetic theory of matter

b. law of conservation of energy d. archimedes’ principle

Properties of Matter (Continue)

1- Which of the following is not a physical property of matter?

a. mass b. colorc. density d. flammability

2- Ice (solid water) floats becausea. it is more dense than water.b. it is less dense than water.c. it is the same density as water. d. it has fewer total particles than water.

Properties of Matter (Continue)

E D

B C A

Heat Energy

1- What portion of the diagram represents a solid? a. A b. B c. C d. D e. E

2- What line segment represents vaporization? a. A b. B c. C d. D e. E

3- If heat energy were being removed from the substance in the diagram, Line Section “B” would represent a. a solid. b. condensationc. melting. d. freezing.

Properties of Matter (Continue)1. What happens to the temperature of a

substance while it is undergoing a phase change?a. it increases c. it stays the same until

the change is complete

b. it decreases d. nothing 2. The particles in a solid move ______ than

particles in a gas (at the same temperature).a. more quickly c. the sameb. more slowly d. depends on the substance

Properties of Matter (Continue)1. Which of the following is a CHEMICAL property?

a. Color c. densityb. melting point d. ability to rust

2. Which of the following is a PHYSICAL change?a. rusting b. evaporatingb. c. burning d. corroding

3. Which of the following is a homogeneous mixture?a. water. c. isopropyl (rubbing) alcohol.b. italian salad dressing. d. grape kool-aid4. Which one of the following represents a correctly balanced

equation for the following equation? KI + Br2 KBr + I2

a. 2 KI + 2 Br2 2 KBr + I2 c. 2 KI + Br2 2 KBr + I2

b. 2 KI + Br2 2 KBr + 2 I2 d. 3 KI + Br2 3 KBr + I2

Properties of Matter (Continue)1. The change of state in which a liquid changes into a solid is

______.a. Evaporation c. meltingb. Freezing d. sublimation

2. The color of ink is a ______.

a. chemical property c. chemical changeb. physical property d. physical change

3. Smoke is an example of a ______.a. colloid b. suspensionc. solution d. molecule

4. Temperature is a measure of a. how hot or cold something is. c. degrees Celsiusb. particle motion. d. cubic centimeters (cm3)

Properties of Matter (Continue)1. Which of these is NOT homogeneous?

a. a compound c. a solutionb. an element d. a suspension

2. the law of the conservation of mass states that mass cannot be a. Burned b. changed in form

c. created or destroyed d. heated or cooled 3. during a chemical or physical change, energy may be

a.created c. destroyed b. greatly increased in strength d.converted into another

form

4. all changes of the state of matter requirea. Water b. vibrationc. Energy d. sublimation

Properties of Matter (Continue)1- you burn a log of wood and only a small pile of ashes is left, what has

happened?a. a large amount of mass has been lostb. a small amount of mass has been turned into a large amount of heat

energyc. the total amount of wood and oxygen is the same as the amount of ash

and gasesd. the total amount of energy is less than before 2- knowing the chemical properties of a substance will tell you how the

substancea. Looks c. can be broken down into atomsb. Smell d. reacts with other substances3- which of the following is an example of physical changea. dissolving salt in water c. cooking an eggb. burning wood into charcoal d. rusting iron 4- ice floats in water because it isa. more dense than water c. colder than waterb. less dense than water d. warmer than water

Properties of Matter (Continue)1- which of the following is not an example of a physical

property?a. freezing point c. reactivityb. boiling point d. density 2- which of the following is an example of chemical change?a. ice melting c. pounding gold into a coinb. paint fading d. a puddle of water evaporating 3- digesting food is an example ofa. physical change c. chemical changeb. change of state d. physical change 4- grinding quartz crystals down to produce sand is an

example of aa. change in state c. chemical reactionb. chemical change d. physical change

Properties of Matter (Continue)1- The smallest unit of a substance that behaves like a

substance is a. an element c. a moleculeb. an atom d. a compound2- The kinetic theory states that the higher the temperature,

the faster thea. the particles that make up the substance moveb. bonds between atoms breakc. molecules of gas rush together d. the lighter particles within a substance clump together3- you put on gram of salt in one liter of water and stir the

resulting liquid is an example ofa. pure substance c. a

homogeneousb. a heterogeneous mixture d. immiscible

Acids & Bases1- Coffee has a pH of about 5. Coffee is a ______.

a. strong acid c. strong baseb. weak acid d. weak base

2- Lye has a pH of 13.8. Lye is a ______. a. strong acid b. strong basec. weak acid d. weak base

3- Red litmus paper turns blue in a ______.a. acid b. basec. either acid or base d. neither acids nor bases

4- The terms dilute and concentrated refer to the ______ of a solution.a. acidity c. pHb. concentration d. strength

5- A substance that produces OH- ions in solutions is a ______.a. acid c. saltb. base d. water

Acids & Bases (Continue)

1- A substance that produces H+ ions in a solution is a ______.a. acid b. salt c. base d. soap

2- OH- represents _____.a. the hydroxide ion c. oxygen hydrideb. hydrochloric acid d. sodium hydroxide

3- Blue litmus paper turns red in a ______.a. acid c. either acid or baseb. base d. neither acids nor bases

4- A reaction between an acid and a base that produces salt and water is a ______ reaction.a. Synthesis c. neutralizationb. Decomposition d. combustion

Solutions1- The terms dilute and concentrated refer to the ______ of a

solution.a. acidity c. pH

b.concentration d. strength2- When a gas is dissolved in a liquid, the gas dissolves faster if the

liquid is ______.a. heated c. under low pressureb. cooled d. none of the above

3- Increasing the surface area of a solid ______.a. slows the rate of dissolving. c. has no effect on the rate

of dissolving.b. speeds up the rate of dissolving d. increases the amount that

can be dissolved.4. The concentration of a solution that contains a small amount of

solute in a solvent can be described as ______.a. saturated c. concentratedb. polar d. dilute

Solutions (Continue)1- A solution with a bitter taste and

slippery feel is most likely a ______.a. acid c. saltb. base d.

water 2- A solution that contains all the

solute is can normally hold at a given temperature is ______.

a. saturated c. supersaturated

b. Unsaturated d. dilute 3- Sugar dissolved in water is an

example of a ______.a. homogeneous mixtureb. suspensionc. heterogeneous mixtured. d. colloid

Solutions (Continue)1- Which of the following will NOT

speed up the dissolving of a solid solute in water?

a. stirring the solutionb. heating the solutionc. crushing the solute d. increasing pressure 2- A solution that contains less solute

than it can hold at a given temperature is ______

a. saturated c. supersaturated

b. unsaturated d. dilute 3- In a solution, the substance that is

being dissolved is the ______.a. solute c.

liquidb. solvent d. solid

Solutions (Continue)1- How much potassium nitrate is

present in a saturated solution at 30oC?a. 35 grams b. 45 grams

c. 65 grams d. 95 grams 2- At what temperature will 20 grams

of potassium chlorate (KClO3) produce a saturated solution?

a. 30 degrees b. 44 degrees

c. 53 degrees d. 80 degrees

3- Will 80 grams of sodium nitrate (NaNO3) dissolve completely in 100 grams of water at 10oC?

a. Yes b. Noc. Maybe d. Not enough information