2010Fall_HonorsReview

PreAP ChemistryFall Semester Exam Review

Name: ____________________________

Teacher:________________________

Period: _______

Date: ____________________

SHAPE \* MERGEFORMAT U = Unfamiliar (I can apply this target to a new situation.)

F = Familiar (I can apply this target to a present or prior situation.)

O = Objective Target (I can identify the target in a situation.)

Matter UnitTARGET U F O Questions I

HaveSP1 Plan and carry

out experiments using the scientific methods (2E).

SP2 Write or select a hypothesis that can be tested or supported in a lab situation (2B).

SP3 Select and use appropriate laboratory equipment to measure and collect observations accurately and precisely

SP7 Express, manipulate, and calculate chemical qualities using (2G):dimensional analysisscientific notation

SP6 Use observational

data to do the following Organize data in a table or graphMake predictions (inferences) and predict trends from a graphAnalyze data to make connections or relationships between concepts

SP10 Determine the best disposal method of everyday products (examples: metals, paper, organics (food), plastics, etc) (1C).

SP9 Gather, analyze, and report valid conclusions from data (2F, 2H, & 2I).

SP8 Apply rules for significant figures in: (2G)

M1 Differentiate among the three physical states of matter. (4C)

M2 Distinguish between types of substances

M3 Classify mixtures and apply terms to everyday examples (4D):

M4 Identify a sample as an aqueous solution

M5 Understand and apply: (8C)

M6 Apply several techniques to separate a mixture of 3 or more substances (4D).

M7 Understand how significant figures are determined by the calibration of lab equipment (2G).

Chapter 1: Introduction to Chemistry: Scientific Methods & ResearchLab Safety Rules and Procedures pp.16 Table 2-1

See HYPERLINK "http://www.chemistryclasses.com/Lab/lab_safety.htm" http://www.chemistryclasses.com/Lab/lab_safety.htm

Finding and Interpreting MSDS information to address first aid, clean up of spills, handling, storage, etc.See any MSDS source sheet (e.g.) Flinn MSDS Collection at

HYPERLINK "http://www.flinnsci.com/homepage/sindex.html" http://www.flinnsci.com/homepage/sindex.html

1. What is found on an MSDS? True or Falsea. safety data and precautions _______________________b. poison control telephone number _______________________c. physical data: color, odor, melting and boiling pts., etc. _______________________d. first aid _______________________e. manufacturer and telephone number _______________________f. hazards and reactivity _______________________g. expiration date _______________________

2. List the following in order of precision, beginning with the most precise (Remember precision is reproducibility)

graduated cylinder, Erlenmeyer flask, volumetric flask, beaker, graduated pipet, volumetric pipet

________________________________________________________________________3. Read the meniscus:

Explain how to set up an appropriate graph based on a data table of info.7. Explain how to determine which set of information goes on the X axis vs Y axis

____________________________________________________________________to determine an appropriate scale…do you always have to start at 0?

____________________________________________________________________Discuss the implications of not recording measurements correctly in a lab setting. Chapter 2: Data AnalysisSI Units of Measurement- Base SI Units, pg.26 Table2-1, and Derived Units pp.25-30Scientific Notation pp.31-33; pp.889-892 Math HandbookMetric Conversions pp.34-35; pp.900-902 Math HandbookAccuracy and Precision of Measurement pp.36-37Percent Error Calculations pp.37-38Significant Figures Determination pp. 38-42; pp.893-896 Math Handbook8. Give the number of significant figures in the following measurements:

_____a. 1505 kg _____ d. 1500 cal _____ g. 137 m _____ j. 8.6 x 103 g _____b. 3.85 x 10 –3 dm _____ e. 0.0037 mm _____ h. 4006 cm

_____c. 17.30 cm3 _____ f. 250.00 mL _____ i. 0.78 J9. Perform the following operations and give the answers in standard exponential form with the correct number of significant figures.

a. 37.2mL + 18.0mL + 380mL = ___________________________________b. 0.57cm x 0.86cm x 17.1cm = ___________________________________c. (8.13 x 104) divided by (3.8 x 102) = ___________________________________d. (1.04 x 10-5) x (4.33 x 10-3) = ___________________________________e. 71.3kg + 0.08kg = ___________________________________

Significant Figures and Conversions: Use dimensional analysis (conversion factors) where appropriate. Give answers with the correct number of significant figures.10. 12.52m + 349.0m + 8.24m = ?m __________ 15. 1.36m + 10.17m = __________11. 74.626m – 28.34m = ?m ___________ 16. 13m = ?km __________12. 8.3m X 1.22m = ___________ 17. 62.46mm = ?m __________13. 7.55m X .34m = ___________ 18. 13.565mm + 16m + 13.472cm = ?m ________14. 8432g / 12.5L = ___________ 19. 22.4kg = ?mg __________Know the SI base units – p 26; Table 2-1Be able to make conversions with various metric units, including conversions involving squaring.20. If a room is 6 meters by 10 meters, what would the area of the room be in cm2?

p51: 80, 93 (d,e,f); p53: 1-3

Density Calculations / Interpreting Density Graphs pp.27-2921. A rock has a mass of 127g and displaces 32.1 mL of water. What is the density of the rock?

22. A 1.00L sample of carbon tetrachloride weighs 1.58kg. What is the density in g/cm3?

23. Set up a graph that would appropriately display density… which information would go on which axis? How would you determine the density from the graph?

p52: 87 using Table 2-7

If you needed to determine the density of an irregularly shaped object (like in the density lab), outline a brief procedure to determine it. See HYPERLINK "http://www.middleschoolscience.com/irregularvolume.htm" http://www.middleschoolscience.com/irregularvolume.htm24. Why does oil float on water? Give numerical evidence and explain.

Correct Set Up, Reading and Interpretation of Graphs pp.43-45

25. Complete the crossword using Chapter 2 vocabulary. 1

2 3

4

5

6

7

8

Properties & Changes Unit

TARGET U F O Questions I Have

SP1 Plan and carry out experiments using the scientific methods

SP3 Select and use appropriate laboratory equipment to measure and collect observations accurately and precisely (2F).

SP5 Distinguish between quantitative and qualitative observations

SP6 Use data to do the following (2H):

SP8 Apply rules for significant figures in: (2G)

SP9 Gather, analyze, and report valid conclusions from data

SP10 Determine the best disposal method of everyday products (examples: metals, paper,

organics (food), plastics, etc) (1C).

SP15 Investigate connections between chemistry and careers

PC1 Distinguish between physical and chemical properties and apply to examples. (4A)

PC2 Distinguish between extensive and intensive physical properties. (4B)

PC3 Know SI base units of time, length & mass. (CRS II. F1)

PC4 Apply metric prefixes (kilo, deci, centi, milli) with the following units (CRS II. F1):

PC5 Determine density of an unknown substance (regular & irregular solids) (4A, 2F, 2G, 2I).

PC6 Apply the following derived units to calculations: (2G, 4A)

PC7 Identify when a physical or chemical change has occurred

PC8 Apply the law of conservation of mass to

laboratory observations. (8D)

27. Car batteries give off a potentially explosive mixture of gases. What kind of change is taking place in the battery? ___________________________________________________________________28. Identify the technique you would use to separate each mixture.

a. two liquid substances with different boiling points b. sand from water

29. If you have a substance that goes through a type of change that involves a color change, how can you determine if it was a chemical or physical change?

30. Fill in the chart describing the differences between solid, liquid, & gas as they go through phase changes

SOLID LIQUID GASFluidity

Compressibility

Relative speed & movement of particlesSpace between particles

Effects of container on Volume

Law of Conservation of Mass p63When 400.0g of wood are burned, 30.0g of ash remain. What happened to the missing 370.0g of matter?

States of Matter: Comparing Solids, Liquids, and Gases pp.58-60Pure Substances, Elements, Mixtures, and Compounds pp.66-71

32. Draw how you would represent an element, a compound, and a mixture of all.

33. Which is an example of a compound? salt air nickel34. Which is an example of an element? salt brass aluminum35. Match each term in column A with its example in column B.

Column A Column B

_____ alloy a. gold_____ element b. methane_____ gas c. steam_____ vapor d. sterling silver (silver and copper)Periodic Table Elements, Element Symbols pp.72-73p82: 43, 46, 48, 49

Atomic Structure & Electrons Unit


SP9. Gather, analyze, and report valid conclusions from data

SP12. Understand how a theory develops from scientific hypotheses and experimental data. Know that a theory can evolve/change with new evidence. (2B,C,D)

SP15. Investigate connections between chemistry and careers (3E).

SP11. Know the definition of science and understand its limitations such as changes over time and how society uses science (2A).

A1 Understand the experimental design and conclusions of the following scientists in the development of the atomic model/structure (2A, 3F, & 6A).

A2 Distinguish between the subatomic particles in terms of: (6A)

A3 Calculate the number of electrons, protons, and neutrons in an atom or ion (6D).

A4 Write the isotopic notation for an atom or ion (6D).

A5 Recognize isotopes and explain why atomic masses are not whole numbers (6D).

A6 Calculate average atomic mass from data. (6D; 2G, 2I).

A7 Explain the electromagnetic spectrum in terms of the relationships between energy, wavelength, and frequency.

A8 Calculate relationships between wavelength, frequency, energy & speed of light using (6C):

A9 Using the Bohr model of the atom, identify the valence electrons and core electrons for a specific element. (6A)

A10 Explain how the bright line emission spectra led to the development of the quantum mechanical model. (6B,E)

A11 Understand the EM spectrum and rank the visible light spectrum in order of increasing energy (ROYGBIV).

A12 Explain how a quantum of energy is related to the energy changes (both KE & PE) of valence electrons in matter. (6A; 11A)

A13 Understand the significance of orbital shapes (s, p, d, f) in the quantum mechanical model. (6E)

A14 Write electron configurations for atoms and ions using the following methods: (6E)

A15 Contrast the Bohr and quantum mechanical

models of the atom. (6A, 2B, 2C)

A16 Draw electron-dot (Lewis) structures representing an atom’s valence electrons. (6E)

A17 Illustrate how an element could become isoelectronic with another element. (6E)

Chapters 4 & 25: Structure of the Atom and Nuclear ChemistryReview yellow boxes on p 88,8936. Theorist Prior

Understanding of the Atom

Basics of Experiment

Results of Experiment

What they got credit for finding

New Model of the Atom

DemocritusJohn Dalton

J.J.Thomson

Ernest RutherfordNeilsBohrBecquerelJames ChadwickCharacteristics and Properties of Subatomic Particles —including location, charge and relative mass pp.92-9737. How do atoms, ions and isotopes differ from each other?

38. The element copper is found to contain the naturally occurring isotopes: copper-63 and copper-65. The relative abundances are 69.1% and 30.9%, respectively. Calculate the average atomic mass of copper.

39. Based on the periodic table's average atomic mass for uranium, which isotope must be more abundant uranium-234, uranium-238 or uranium-239?

40. Which statement is consistent with the results of Rutherford's gold foil experiment?a. All atoms have a positive charge.b. Atoms are mostly empty space.c. The nucleus of an atom contains protons and electrons.

41. How many protons are found in an atom of each of the following?

a. boron _____ c. neon _____b. sulfur _____ d. lithium _____

Atomic Number, Atomic Mass, Isotopes, Isotope stability (6A, 6B) pp.98-104p836: 44

Radioactivity / Types of Radiation pp.105-107; pp.806-809p112: 49, 50

42. Complete the table for the following elements:Element Number of

protonsNumber of electrons

Number of neutrons

Atomic number

Mass Number

Charge of atom or ion

25 30 0Na 10 12

35 45 -139 89 0

Arsenic 33 75 0Ac 227 0

43. Complete the tableSymbol for each Location Relative Mass Charge Changing the amt

makes a(n)ProtonNeutronElectron

Ground state and ion electron configurations pp. 135-140Aufbau Principle, Pauli Exclusion Principle, Hund’s Ruleorbital diagramsProblems Associated with Nuclear Waste Disposal pp.824-826Applications and Effects of Nuclear Reactions pp.827-831List several ways that radiation can be used in a positive way.

Periodicity Unit


SP6. Use observational data to do the following (2H):

Organize data in a table or

graph Make predictions (inferences) and predict trends from a graphAnalyze data to make connections or relationships between concepts

SP9. Gather, analyze, and report valid conclusions from data

SP12. Understand how a theory develops from scientific hypotheses and experimental data. Know that a theory can evolve/change with new evidence. (2B,C,D)

P1. Understand the organization of the periodic table in terms of groups/families in columns (valence electrons), and periods in rows (energy levels) (5A & 5B).

P2. Develop the electron configuration for an element using the periodic orbital trends (s,p,d,f blocks on periodic table).

P3. Rationalize period and group trends of several

properties including: (5C)

P4. Identify and explain properties for each of the following

Chapter 6: Periodic Table and Periodic Law44. State the periodic law.

45. Distinguish between periods and groups in the periodic table.

46. Supply the information to complete the table belowsymbol name metal/

nonmetal/metalloid

Complete electronconfiguration

# valence electrons

elements with similar properties

formula of ion

FKCaO47. What is the trend for each of the following as you go across and down the periodic table?

Period Trend (left to right)

Group Trend (top to bottom)

metallic propertiesatomic radiusionic radius

shieldingelectronegativityionization energy reactivity48. Write the correct product in the following synthesis reaction given the following formulas:

ASSUME: all compounds are IONIC

M2X Y2B3 M2B

X2 + Y __________

49. Identify the following elementsa. has 7 valence electrons and in the 4th period.b. has the least amount of shielding in group 5A c. commonly found as the central atom in a tetrahedral molecule and has 1 inner core level d. isoelectronic with neon, located on the metalloid staircasee. only true metal in nitrogen family

50. Write the valence electron configuration for Magnesium Iron

Phosphorus Sulfur ion

Ionic Bonding UnitTARGET U F O Questions I

HaveSP1 Plan and carry

out experiments using the scientific methods (2E).

SP6 Use observational data to do the following (2H):



I1 Relate chemical bond formation to electron configuration & valence electrons. (6E;

7C)I2 Describe the

formation of positive and negative ions using the octet rule. (7C)

I3 Describe the formation of ionic bonds through electrostatic attraction. (7C)

I4 Account for the following physical properties of an ionic compound: (CRS VII D1)

I5 Illustrate at the atomic level the solvation (ionization, dissociation) of an ionic compound in water to form an electrolytic solution. (8A, (10E)

I6 Name and write formulas for ionic compounds and polyatomic ions (7A & 7B).

I7 Relate the physical properties of metals to metallic bonding (sea of electrons). (7D)thermal conductivityelectrical conductivitymalleabilityductility

I8 Explain how the unique properties of alloys can be used for separation: (7D)

Covalent Bonding UnitTARGET U F O Questions I

HaveSP6 Use

observational data to do the following (2H):

SP9 Gather, analyze, and report valid conclusions from data

C1 Apply the octet rule to atoms that bond covalently to form molecular compounds. (7C)

C2 Know the following exceptions to the octet rule, and identify molecules in which these exceptions occur: (7C)

C3 Know the seven diatomic elements (H2, O2, F2, Br2, I2, N2, and Cl2) and recognize that they are more stable than individual atoms of that element

(CRS VII A2).C4 Describe the

formation of single, double, and triple covalent bonds (7C).

C5 Write the names and formulas for binary molecular compounds

C6 Recognize that polyatomic ions are held together by covalent bond (7B).

C7 Name acidic solutions. (7A & 7B)

C8 Be able to draw Lewis structures for covalent compounds. Recognize unshared pairs and be able to substitute bond lines for shared pairs (7C).

C9 Use VSEPR bonding theory to explain bond angle formation and predict the shapes: (7E)

C10 Use electronegativity difference to determine bond type.

C11 Compare and contrast the polarity of the

bond and the polarity of the molecule. (CRS VII I7)

Chapters 8 & 9: Ionic Compounds & Covalent BondingNaming and Writing Polyatomic Ions pp.919 Table C-8Naming and Writing Ionic Compound Formula pp.221-227Naming Molecules and Writing Molecular Compound Formulas pp.248-251

Name the ionic compounds listed below: Name the molecular compounds:51. MgO _________________________ 58. N2O3 _________________________52. BaS _________________________ 59 PCl3 _________________________53. K3P_________________________ 60.SiO2 _________________________54. Na3N _________________________ 61. P2O5 _________________________55. SnCl4 _________________________ 62. CS2 _________________________56. Mn2O3 _________________________ 57. PbS _________________________

Naming compounds with polyatomic ions:63. NaClO2 _________________________ 64.Na2CO3 _________________________65. BaSO4 _________________________ 66.NaHCO3 _________________________67. BaSO3 _________________________ 68.(NH4)3PO4_________________________69. From the list below choose the symbols of the elements that usually have positive ionic charges

Fe C N Na Sr Se Mn Mg Al As H O Ca Ag At

Name or give formulas for these ionic compounds:70.NH4OH ___________________________________71. iron (III) chloride ___________________________________72. silver acetate ___________________________________73. Ca(OH)2 ___________________________________74. CoPO4 ___________________________________75. mercury (II) oxide ___________________________________76. NaClO3 ___________________________________77. (NH4)2SO4 ___________________________________78. Fe2S3 ___________________________________Write the chemical formula or name for the following: 79. dinitrogen tetraoxide______________________ 86. PI3 ______________________80. mercury (II) bromide______________________ 87. ZnO ______________________81. silver sulfide______________________ 88. Li2CO3 ______________________82. strontium iodide______________________ 89. Cu2O ______________________83. disulfur dichloride_____________________ 90. N2H4 ______________________84. chromium (III) nitrate_____________________ 91. KBr ______________________85. calcium carbonate______________________ 92. Fe(C2H3O2)3____________________

Ionic Bond Formation and Ionic Compound Properties pp.211-220Metallic Bonds and Properties of Metals pp.228-231Covalent Bond Formation, Bond Types, Characteristics pp.241-247; Properties pp.266Be familiar with polyatomic ions93. Draw a molecular picture of a compound of salt.

94. Draw a molecular picture of a compound of water.

95. Types of What What types Which have From what Given the

Elements Involved

happens to electrons?

of compounds are made?

higher melting points?

do you decide how to write the formula?

formula, what needs to be added

to the elements to

name?IONICCOVALENTLewis Dot Structures pp.252-258 Molecular Shapes pp.259-262; Table 9-3 pg. 260Polar and Non-polar Molecules pp.26596. State the octet rule.

97. Explain the formation of the ionic compound—why some elements form ionic compounds and others molecules.

98. Describe the formation of the sodium ion and chloride ion using e- dot structures.

99. Use the definition of electronegativity to describe the formation of a covalent bond. Why do some elements form polar and others nonpolar covalent bonds? Use examples to help you with your explanation.

100. Draw electron dot structures for the following ionic compounds:magnesium phosphide sodium oxide

101. Fill in the table below regarding molecules.formula electron

dotshape

Polar or nonpolar Molecule

formula electron dot

shapepolar or nonpolar molecule

CBr4 CSe2

AsF3 F2

H2S HCl

102. Explain the relationship between polar covalent bonds and polarity of the molecules. Use CO2 and CO as examples.

103. Which of the following would have the greatest ionic character?

CI4 NaCl FrF O2

104. Which of the following descriptions are that of ionic compounds, and which are those of covalent molecules? Complete the chart below.

Conduct Electricity 2 or more nonmetals Crystals High Melting pointsVan der Waals forces Cation/anion Transfer electrons Share electronsDouble bonds Electronegativity difference greater than 1.7 Partial chargesTetrahedral H2O NaCl Lone Pairs

Ionic Covalent

Chemical Reactions UnitTARGET U F O Questions I

HaveSP2 Write or select

a hypothesis that can be tested or supported in a lab situation (2B).



CR1 Represent chemical reactions with equations. (7B, 8D)

CR2 Classify chemical reactions as: (10H)

CR3 Predict products of the following given the reactants: (10H)

CR4 Classify equations involving heat (kJ or energy) written in the equation as endothermic or exothermic. (11C)

CR5 Illustrate and explain how water interacts with some ionic solids to form hydrated ions. (10A; CRS VII I2)

CR6 Write complete ionic and net ionic equations for chemical reactions in aqueous solutions. (7B; 8D; 10B)

CR7 Predict whether reactions in aqueous solutions will produce a precipitate, aqueous ions, or a gas using

solubility rules. (10B)

CR8 Apply the law of conservation of mass to chemical reactions by balancing chemical equations (8D).

Chapter 10: Chemical ReactionsEndothermic and Exothermic Energy in Reactions pp.247; pp.500Be able to interpret an energy diagramWriting and Balancing Chemical Reactions Equations pp.278-283Classify each of the following reactions as one of the five reaction types. If energy is present, state if the reaction is endothermic or exothermic. Balance the equations.

105. CuO + H2 ----> Cu + H2O106. Na(cr) + O2(g) ----> Na2O(cr)107. H2O2 + energy ----> H2O + O2

1087 Pb(NO3)2(aq) + Na2CrO4(aq) ----> NaNO3(cr) + PbCrO4(cr)109. Ag + S ----> Ag2S110. NbI2(cr) + I2(cr) ----> NbI5(cr)111. C4H8 + O2 ----> CO2 + H2O + energy112. Li(cr) + H2O(l) ----> LiOH(aq) + H2(g)113. K + H2O ----> KOH + H2

114. C7H14(l) + O2(g) ----> CO2(g) + H2O(g)115. HCl + NaOH ----> H2O + NaCl116. Complete the graphs:

Endothermic Exothermic

Predict the products for the following reactions:117. Single replacement: Mg + AgNO3

118. Combustion of C3H7OH:119. Synthesis of calcium phosphide:120. Decomposition of aluminum oxide:121. Decomposition of magnesium carbonate: (yields a gas and an oxide compound)122. Single replacement: Ni + MgCl2123. Double replacement: Li2CO3 + MoBr4 124 Your favorite class is _____________________________.

Page PAGE 1 of NUMPAGES 16

4. How would you dilute acid with water? ____________________________________________________________

Scientific Methods as a Systematic Approach pp.10-135. List the steps involved in the scientific method. __________________________________________6. What is the difference between a hypothesis, a theory and a scientific law? _________________________

_____________________________Proper Use and Selection of Lab Equipment and Correct Scale InterpretationSee HYPERLINK "http://lhs.lps.org/staff/squiring/chemistry/Intro/UseOfLabEquipment.pdf" http://lhs.lps.org/staff/squiring/chemistry/Intro/UseOfLabEquipment.pdfSee HYPERLINK "http://www.hmpublishing.com/Brown/Chapter%204.pdf" http://www.hmpublishing.com/Brown/Chapter%204.pdf

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Clues1. Refers to how close a series of measurements are to one another; but the measurements may not be accurate.2. _____ factor - a ratio of equivalent values used to 3. A ratio that compares the mass of an object to its volume.express the same quantity in different units; changes the units of a quantity. 4. ___ error - the ratio of an error to an accepted value.5. ____ unit - a unit defined by a combination of base units.6. _______ figures - the number of all known digits reported in measurements plus one estimated digit.7. A visual representation of information that can reveal patterns in data.8. Refers to how close a measured value is to an accepted value.

Chapter 3: Matter: Properties and ChangesProperties of Matter: Intensive vs. Extensive / Physical vs. Chemical pp.55-59; pp.61-6226. State whether each of the following is a homogeneous or heterogeneous mixture:

a. oxygen dissolved in water ___________________________________b. carbon mixed with sand ___________________________________

c. apples juice ___________________________________d. vegetable soup ___________________________________e. sour milk ___________________________________

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2010Fall_HonorsReview