honors chemistry final exam study guide and review packet › chemistry › 820 › pdf ›...

Honors Chemistry Name_______________________________________ Block____________

Honors Chemistry Final Exam Study Guide and Review Packet

Final Exam Preparation

There are many benefits to preparing for and taking a final exam. Keep in mind that you are trying to

gain an understanding of the “big picture” when studying for a cumulative exam. You are most likely to

remember information when it makes sense to you. A value in studying for an exam of large scope is it

allows you to review earlier information with the benefit of knowledge gained later. The knowledge

gained later can frequently help you to gain a clearer picture of topics that may have confused you the

first time around. Learning that comes from reevaluation can make a major difference in your overall

understanding. This difference is a reason why studying for exams is worthwhile.

Study tips:

❖ Review your chemistry journal (class notes & reading notes).

❖ Organize and review your worksheets, labs, problem sets.

❖ Review your study guides.

❖ Study sequentially.

❖ Divide your study time into short, intense sections. This can be more effective than studying

continually for a long period of time.

❖ “Guess the test questions.” You should ask yourself what is most important when studying.

What questions would you ask if you were writing the exam?

❖ Practice, practice, practice.

o Go over the review packet.

o Go over end of chapter problems in your textbook.

o Do the multiple choice questions from the on-line resources.

http://infohost.nmt.edu/~chem/heagy/UnOfficialACSPracticeTest01A.pdf

http://cemast.illinoisstate.edu/downloads/ACS_PRACTICE_EXAM.pdf

o Do the ACS practice test (you may borrow a printed copy and return it by exam day).

o Study with a friend. Quiz each other. Practice explaining topics to one another.

❖ Do the practice problems using the periodic table, reference sheet, and calculator you will use on

the exam.

Significant Figures Review

1. a. Sketch graduated cylinders with proper markings to match the following measurements.

5 mL 5.3 mL 5.28 mL

b. Which measurement is the most precise?__________ Explain.

c. The uncertainty of the least precise measurement is the ____________ place.

d. What is the total volume of the measurements? Show work.

Round your final answer to the appropriate place.

2. An object has a mass of 19.355g and a volume of 11.5 mL.

a. The measurement with the least number of significant figures has ________sig. figs.

b. Determine the density of the object. Show work. Round your final answer to the appropriate

number of significant figures.

http://infohost.nmt.edu/~chem/heagy/UnOfficialACSPracticeTest01A.pdf


Ch. 1 Water - A Natural Wonder

Read the bullet points on pages 56-57 (Ch. 1 sec. 13 Outcomes Review).

1. Compare the substances: nitrogen gas, water, and sodium chloride. Fill in the table.

N2 H2O NaCl

Classify as element

or compound.

Make a particle level

drawing.

Show 6 molecules in the gas phase. Show H-bonding between 6

molecules in the liquid phase.

Show the solid crystal structure. Include 6

formula units.

Describe forces of

attraction between

particles.

Rank in order of

lowest to highest

boiling point.

Rank in order of

lowest to highest

melting point.

Molar mass

How many moles

are in 145 g of the

substance?

2. Compare the elements nitrogen, oxygen, phosphorus, and sulfur. Fill in the table.

Nitrogen Oxygen Phosphorus Sulfur

Number of valence

electrons

Core charge

Electron

configuration

Number of unpaired

electrons

Rank in order of

smallest to largest

atomic radius

Rank in order of

lowest to highest

electronegativity


Ch. 2 Aqueous Solutions and Solubility

Read the bullet points on pages 138 (Ch. 2 sec. 15 Outcomes Review).

1. Potassium nitrate, KNO3.

a. Draw a picture of a solid crystal lattice b. Draw a picture that shows the particles

for the ionic compound KNO3. when KNO3 is dissolved.

c. Is dissolving a chemical or physical change? Explain.

d. Will this solution conduct electricity? Explain.

e. The overall process of dissolving KNO3 is endothermic. Draw an energy diagram for

this process.

• Label each part of the diagram.

• Show ∆Elattice and ∆Esolvation and ∆Enet.

• Indicate if each ∆E is positive or negative.

2. Aqueous solutions of copper (II) nitrate and potassium phosphate mixed.

a. Write a balanced equation for the reaction.

b. Show what ions are present. Remember that ionic compounds in the aqueous phase have the ions

separated from each other. In the solid phase the ions form a crystal lattice. You do not need to show

the water molecules. Draw enough ions to make 2 Cu3(PO4)2 formula units.

+

c. Which ions are the spectator ions?

d. Write the net ionic equation.

3. _____Na2CO3 (aq) + _____Ca(NO3)2 (aq) _____CaCO3 (s) + _____NaNO3 (aq)

a. Balance the equation.

b. You make up a problem. Solve it. Then give it to a study partner.

________________ of _______M Na2CO3 is mixed with __________ of _______M Ca(NO3)2. (you choose the volume) (you choose the molarity) (you choose the volume) (you choose the molarity)

Determine how many grams of are CaCO3 formed in the reaction. Hint: limiting reactant.


4. Write the name for each formula. Check your spelling!

a. Cu2SO4 ________________________________

b. P2O5 ________________________________

c. HNO2 ________________________________

d. C7H16 ________________________________

5. Write the formula for each name.

a. lead (II) phosphide __________________________

b. aluminum carbonate __________________________

c. xenon hexachloride __________________________

d. butane __________________________

e. perchloric acid __________________________

6. a. Draw a Lewis structure for chlorous acid, HClO2.

b. Write a chemical equation to show the dissociation of chlorous acid in water.

c. In the equation in part b, label the Bronsted-Lowry acid, Bronsted-Lowry base, conjugate acid,

conjugate base.

d. Draw a molecular level drawing to show the particles present in a solution of chorous acid.

Make a key.

e. Describe what is happening when this system is at equilibrium.

f. Describe 3 ways to shift this equilibrium to the right.

g. When acids are added to water the resulting mixture feels warm. Explain why. (Hint: think about

what attractions are overcome and what attractions are made.)

7. You make up a problem. Solve it. Then give it to a study partner.

(you choose the volume) _______ of 0.10 M HCl is mixed with ( you choose the volume) ______ of 0.25 M NaOH.

What is the resulting pH and pOH of the solution?


Ch. 6 Chemical Readtions

Read the bullet points for section 6.9 on page 421 (Ch. 6 sec. 12 Outcomes Review).

1. Make a practice problem for each type of reaction listed below. Make a molecular level drawing for

each. Trade with a study partner.

a. synthesis

b. decomposition

c. combustion

d. single replacement

e. precipitation (double replacement)

f. acid-base neutralization

2. Silver Bullion “The cupellation assay was used formerly, for the determination of silver in many of its alloys. This method has been

replaced in the majority of mints and assay offices by volumetric methods. The chief of these is the "Gay Lussac" assay,

which was introduced into the Paris mint in 183o, and has since been adopted in most offices. An exact weight of the

bullion is dissolved in nitric acid, and very nearly all the silver is precipitated at once by the addition of a known volume

of a standard solution of salt. When the precipitate has settled, the remaining silver is precipitated by the further addition

of a small quantity of a more dilute solution of salt, the precipitate forming a white cloud in the supernatant liquid. The

quantity of this silver is judged by the appearance of the white cloud.” http://gluedideas.com/Encyclopedia-Britannica-

Volume-2-Annu-Baltic/Wet-Assaying.html

a. Write a balanced chemical equation (include phases) for the reaction between silver metal and

nitric acid. The products of the reaction are silver nitrate, nitrogen dioxide, and water.

______________________________________________________________________

Element reduced: _______ Element oxidized: ____________

Reducing agent: ________ Oxidizing agent:_____________

Reduction half-reaction: _______________________________________________________

Oxidation half-reaction: _______________________________________________________

b. Write a balanced chemical equation (include phases) for the reaction between silver nitrate and

sodium chloride.

______________________________________________________________________

c. The U.S. Brilliant Uncirculated Silver Eagle Dollar coin has a mass of 31.1 g (also known as a

troy ounce) and is 99.9% pure silver. (http://www.govmint.com)

If an exact weight of the bullion is assayed, what volume of 0.750 M NaCl must be added to

precipitate out all of the silver ions?

http://gluedideas.com/Encyclopedia-Britannica-Volume-2-Annu-Baltic/Wet-Assaying.html

http://gluedideas.com/Encyclopedia-Britannica-Volume-2-Annu-Baltic/Wet-Assaying.html

http://www.govmint.com/


Ch. 3 Origin of Atoms

Read the bullet points on pages 197-198 (Ch. 3 sec. 8 Outcomes Review).

mp = 1.00728 amu mn = 1.00866 amu

1. Carbon-14 has a mass of 14.003241amu.

a. Calculate the nuclear binding energy in units of kJ/mol.

b. The half life of carbon-14 is 6730 years. What fraction of a sample is left after 12,000 years?

c. Write a balanced equation to show 14C undergoing beta decay.

2. Write balanced equations to show 236Np undergoing electron capture followed by alpha decay

followed by beta decay.

3. Determine the average atomic mass of silicon based on the following data.

Isotope Atomic Mass (amu) % Abundance 28Si 27.9769271 92.2297 29Si 28.9764949 4.6832 30Si 29.9737707 3.0872


Ch. 4 Structure of Atoms

Read the bullet points on pages 269-270 (Ch. 4 sec. 12 Outcomes Review). 1. Emission Spectra

The energy for each principal energy level for the H atom is given in the following table.

n Energy in eV

5 -0.54

4 -0.85

3 -1.50

2 -3.40

1 -13.6

Suppose an electron in an excited state can return to the ground state in two steps. It first falls to an intermediate state,

emitting radiation of wavelength λ1 and then to the ground state, emitting radiation of wavelength λ2. The same electron can

also return to the ground state in one step, with the emission of radiation of wavelength λ3.

a. How are the three wavelengths related?

b. How are the frequencies of the three radiations related?

c. How are the energies of the three radiations related?

d. Make an energy level diagram to illustrate your answer.

e. Support your answer with calculations.

2. Photoelectric Effect. For a certain solar cell made of hydrogenated amorphous silicon wafers (abbreviated Si-H), the

threshold energy is 1.9 eV. (1.602 x 10 -19 J = 1 eV)

a. Calculate the threshold wavelength.

b. In what region of the EM spectrum is this wavelength?

c. Which of the following types of radiation would knock an electron from the Si-H wafer? Explain. blue

light, yellow light, microwaves, UV, x-rays, radio waves

d. If the incident light has a wavelength of 475 nm, determine the kinetic energy of the ejected electron in units of eV.

e. How is KE related to temperature (in Kelvin)?

f. If much of the energy above the threshold energy is dissipated as heat, what would happen to the temperature of the

Si-H wafers?

g. “Efficiency is defined as the ratio of output electric energy to the incident light energy. A silicon wafer alone

produces very little electric energy, usually on the order of less than 5 percent. This efficiency can be improved by a

number of methods.” Suggest strategies for improving the efficiency.


Ch. 5 Structure of Molecules

Read the bullet points on pages 340-341. (Ch. 5 sec. 12 Outcomes Review).

1. a. Draw Lewis diagrams for the following compounds:

1-hexanol and 2,3-dimethyl-2-butanol

b. Compare the boiling points, melting points, solubility in water.

c. Draw 2 more structural isomers of 1-hexanol.

2. Given the structure for phenylalanine,

a. Identify the amino group, carboxylic acid group,

benzyl group.

b. What is the chemical formula of phenyalanine?

c. Determine the oxidation number of each atom?

d. Determine the molecular geometry of each central

atom.

e. Determine the ideal bond angle about each central atom.

f. Identify any chiral carbons.

g. How many sigma bonds?

h. How many pi bonds?

3. Give an example of each type of isomer. (Draw a pair of structures for each type of isomer.)

a. structural

b. diastereomers

c. enantiomers

4. a. Draw several valid Lewis structures of the bromate, BrO3- ion.

b. What is the oxidation number of Br?_____ of O?_______

c. Based on formal charge, which structure is the best structure?

5. a. Draw resonance structures for the nitrate ion.

b. Describe the molecular geometry, bond angle, localized orbitals, delocalized orbitals, bond order,

polarity.

http://www.newworldencyclopedia.org/entry/File:L-phenylalanine-skeletal.png

Ch. 7 Chemical Energetics- Enthalpy

Read the bullet points on pages 491. (Ch. 7 sec. 12 Outcomes Review).

1. Describe an exothermic and endothermic reaction in terms of energy of bond making

and bond breaking.

2. a. Draw the energy diagram for an endothermic and exothermic reaction.

b. Does the temperature of the surroundings increase or decrease in an endothermic

reaction?

c. Does the enthalpy of the system increase or decrease in an endothermic reaction?

3. If it takes 5.8 joules of energy to heat a piece of metal that weighs 1.6 grams from

23°C to 41°C, what is the specific heat of this metal? Is this metal pure gold (cAu = 0.13

J/gC)? Why or why not?

4. The equation for the fermentation of glucose to alcohol and carbon dioxide is:

C6H12O6 2 C2H5OH + 2 CO2 ∆H = - 67 kilojoules

a. Is this reaction endothermic or exothermic? Why?

b. How much heat is released when 25 moles of glucose is fermented?

5. For the reaction of dry ice subliming at room temp, describe each of the following

a. Free energy, ∆G.

b. Enthalpy, ∆H.

c. Entropy, ∆S.

d. Work, w.

e. Internal energy, ∆E

6. Make a sketch of each type of diagram.

a. Heating curve (label solid, liquid, gas, melting, boiling)

b. Phase diagram (label solid, liquid, gas, triple point, critical point, normal

melting point, normal boiling point)

7. Solve the following gas law problems. Report all answers using the correct significant figures!

State the relationship ( or formula) and the numerical answer

__________

_______ moles

Calculate the number of moles of nitrogen gas present if it occupies 25.3

Liters at 58.2 °C and 2.04 atmospheres of pressure?

__________

_______ L

A balloon containing 4.0 liters of air at 45 C is warmed to

90 C. What is the new volume of the balloon if the pressure remains

constant?

__________

_______ atm

A gas sample has a pressure of 1.4 atm and a volume of 5.5 L. What is the

new pressure, if the gas volume increases to 11.0 L at constant

temperature?

__________

___________

molecules

You are scuba-diving in the Caribbean. The captain of the boat hands you a

tank of pure compressed oxygen gas that has a volume of 15 liters at STP.

How many molecules of oxygen are in the tank?

__________

_______ mmHg

The vapor pressure of water at 25 °C is 23.5 mmHg. A sample of

hydrogen is collected over water and the pressure inside the eudiometer is

equilibrated with the atmospheric pressure. Determine the partial pressure

of hydrogen when the atmospheric pressure is 763.0 mmHg. Draw a

picture to show how the pressure is equilibrated.

_________ atm

_________ atm

A 0.020 mol sample of solid sodium hydrogen carbonate is placed in a 1.0

L evacuated flask, which is then sealed and heated to 350 K. The solid

sodium hydrogen carbonate decomposes completely according to the

balanced equation,

2 NaHCO3 (s) Na2O(s) + 2CO2 (g) + H2O (g)

a. What is the total pressure (in atm) in the flask at the end of the

reaction? Report your answer using 2 sig figs.

b. What is the partial pressure of the carbon dioxide?

__________

_______ L

On a cold day, a person intakes 476 mL of air at 780 mm and –2.0 °C.

What is the volume of this air in the lungs at 757 mm and 35°C?

______________

Compare the effusion rates of carbon monoxide and oxygen gas at 25°C.

Which one is faster? By how much?

Useful Information

Equations Constants

c = λ ν c = 2.998 108 m/s

Ephoton = h ν h = 6.626 10−34 J s

ΔE = n h ν NA = 6.022 1023 mol−1

KE = ½ m u2 me = 9.1094 10−31 kg

λmatter = h /(m u) mp = 1.6726 10−27 kg

En = −RH(z2/n2) mn = 1.6749 10−27 kg

∆E = − RH(z2/nf2 − z2/ni

2) RH = 13.6 eV

qlost = −qgained RH = 2.178 10-18 J

q = Cp ∆T R = 62.4 mmHg L mol−1 K−1

∆E = q + w R = 8.314 L kPa mol−1 K−1

∆Hp = ∆E + Pext ∆V R = 0.08206 L atm mol−1 K−1

w = − Pext ∆V

qp = ∆Hp

q = m cp ∆T (specific heat)

q = n C˚p ∆T (molar heat capacity)

∆T = Tf - Ti

TK = TC + 273.15

PV = nRT

A

B

B

A

MM

MM

r

r

A

B

B

A

MM

MM

u

u

2

1

2

1

T

T

u

u

2

3RTKE

3rms

RTu

MM

Hrxn = )(H)(H if

i

iif

i

i reactantnproductn

Hrxn = (reactants) ( )BH BH products

N(t) = N(0)e−λt = N(0)(½)n

f(n) = (½)n

n = t / ϫ

ϫ = ln(2)/λ

ΔE = Δm c2

The Periodic Table of Elements 1A 8A

1

H

1.008

2A 3A 4A 5A 6A 7A 2

He 4.003

3

Li 6.941

4

Be 9.012

5

B 10.81

6

C 12.01

7

N 14.01

8

O 16.00

9

F 19.00

10

Ne 20.18

11

Na 22.99

12

Mg 24.31

13

Al 26.98

14

Si 28.09

15

P 30.97

16

S 32.07

17

Cl 35.45

18

Ar 39.95

19

K 39.10

20

Ca 40.08

21

Sc 44.96

22

Ti 47.88

23

V 50.94

24

Cr 52.00

25

Mn 54.94

26

Fe 55.85

27

Co 58.93

28

Ni 58.69

29

Cu 63.55

30

Zn 65.39

31

Ga 69.72

32

Ge 69.72

33

As 74.92

34

Se 78.96

35

Br 79.90

36

Kr 83.80

37

Rb 85.47

38

Sr 87.62

39

Y 88.91

40

Zr 91.22

41

Nb 92.91

42

Mo 95.94

43

Tc (98)

44

Ru 101.1

45

Rh 102.9

46

Pd 106.4

47

Ag 107.9

48

Cd 112.4

49

In 114.8

50

Sn 118.7

51

Sb 121.8

52

Te 127.6

53

I 126.9

54

Xe 131.3

55

Cs 132.9

56

Ba 137.3

57

La 138.9

72

Hf 178.5

73

Ta 181.0

74

W 183.8

75

Re 186.2

76

Os 190.2

77

Ir 192.2

78

Pt 195.1

79

Au 197.0

80

Hg 200.6

81

Tl 204.4

82

Pb 207.2

83

Bi 209.2

84

Po (209)

85

At (210)

86

Ru (222)

87

Fr (223)

88

Ra 226.0

89

Ac 227.0

104

Rf (261)

105

Db (262)

106

Sg (263)

107

Bh (262)

108

Hs (265)

109

Mt (266)

110

(269)

111

(272)

112

(277)

114

(289)

58

Ce 140.1

59

Pr 140.9

60

Nd 144.2

61

Pm (145)

62

Sm 150.4

63

Eu 152.0

64

Gd 157.3

65

Tb 158.9

66

Dy

162.5

67

Ho 164.9

68

Er 167.3

69

Tm 168.9

70

Yb 173.0

71

Lu 175.0

90

Th 232.0

91

Pa 231.0

92

U 238.0

93

Np 237.0

94

Pu (244)

95

Am (243)

96

Cm (247)

97

Bk (247)

98

Cf

(251)

99

Es (252)

100

Fm (257)

101

Md (258)

102

No (259)

103

Lr (260)

honors chemistry final exam study guide and review packet › chemistry › 820 › pdf ›...

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