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Honors Chemistry Final Exam Worksheet Extraction

Total questions: 80

Worksheet time: 40mins

Name
Class
Date
1.

What is the nuclear symbol of an atom which contains 28 protons, 28 electrons, and 34 neutrons?

a)

 ⁣6228Ni\!^{28}_{62}\mathrm{Ni}

b)

 ⁣2856Ni\!^{56}_{28}\mathrm{Ni}

c)

 ⁣2862Ni\!^{62}_{28}\mathrm{Ni}

d)

 ⁣3490Ni\!^{90}_{34}\mathrm{Ni}

2.

Element X has two isotopes, X-85.00 atomic mass units and X-86.00 atomic mass units. The atomic mass of X on the periodic table is 85.94 amu. Which isotope is the most abundant?

a)

X-86.00

b)

X-85.00

c)

The isotopes are equally represented in nature because the atomic mass on the periodic table is an average.

d)

There is not enough information given to answer this question.

3.

An atom of calcium-37 and an atom of calcium-42 differ in their total number of

a)

Electrons

b)

Neutrons

c)

Protons

d)

Positrons

4.

An unknown element has 2 common isotopes: X-85 (85.001 amu) and X-89 (88.995 amu). The relative abundance of the isotopes is 85.000% and 15.000% respectively. Determine the average atomic mass for element X.

a)

85.601 amu

b)

86.998 amu

c)

87.421 amu

d)

88.396 amu

5.

If an electron drops from n=2 to n=1 in the Bohr model, what type of electromagnetic radiation is emitted?

a)

Ultraviolet (UV)

b)

Visible

c)

Infrared (IR)

d)

Radio waves

6.

Which of the following elements has electrons in the d sublevel?

a)

Ne

b)

Mg

c)

S

d)

Sc

7.

Which orbital notation represents an atom of boron in its ground state?

a)

Diagram A

b)

Diagram B

c)

Diagram C

d)

Diagram D

8.

Which electron configuration represents an atom of nickel in the ground state?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p5

c)

1s2 2s2 2p6 3s2 3p4 3d8

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

9.

Gold-198 has a half-life of approximately 3 days. If a 100 g sample of gold-198 decays for 9 days, approximately how much gold-198 remains in the sample?

a)

12.5 g

b)

25 g

c)

33 g

d)

50 g

10.

In the nuclear equation given below, determine the missing piece:  ⁣92238U→ ⁣90234Th+  ______\!^{238}_{92}\mathrm{U} \rightarrow \!^{234}_{90}\mathrm{Th} + \;\_\_\_\_\_\_ .

a)

 ⁣24He\!^{4}_{2}\mathrm{He}

b)

 ⁣24Be\!^{4}_{2}\mathrm{Be}

c)

 ⁣22He\!^{2}_{2}\mathrm{He}

d)

 ⁣12H\!^{2}_{1}\mathrm{H}

11.

Which of the following are most directly involved in chemical bonding?

a)

Protons

b)

Neutrons

c)

Alpha particles

d)

Valence electrons

12.

What is the correct Lewis dot structure for nitrogen trifluoride (NF3)?

a)

Structure A

b)

Structure B

c)

Structure C

d)

Structure D

13.

The Lewis dot structure of a compound is shown: H—X with lone pairs around X. Which of the following elements does X represent in the structure?

a)

Carbon

b)

Nitrogen

c)

Chlorine

d)

Oxygen

14.

Which substance contains bonds that involve the transfer of electrons from one atom to another?

a)

CO2

b)

KBr

c)

NH3

d)

Cl2

15.

The correct formula between X and oxygen has a chemical formula of X2O. Which element would X most likely represent?

a)

Al

b)

Zn

c)

Li

d)

Mg

16.

What is the name of the compound FeCl3?

a)

Iron chloride

b)

Iron (I) chloride

c)

Iron (II) chloride

d)

Iron (III) chloride

17.

Which is the correct formula for dinitrogen trioxide?

a)

N2O2

b)

N2O3

c)

NO

d)

N2O5

18.

Which is the correct formula for magnesium phosphate?

a)

MgP

b)

Mg3P2

c)

MgPO4

d)

Mg3(PO4)2

19.

Which species cannot conduct an electric current?

a)

NaOH(aq)

b)

CH3(l)

c)

AlCl3(aq)

d)

HCl(aq)

20.

Use the chart below to determine the type of bonding that is most likely in compound A and D respectively.

a)

A is non-polar covalent and D is ionic.

b)

A is polar covalent and D is metallic.

c)

A is ionic and D is polar covalent.

d)

A is metallic and D is metallic.

21.

Which diagram best represents the structure of a water molecule?

a)

Diagram A

b)

Diagram B

c)

Diagram C

d)

Diagram D

22.

Which of the following classifications describes the element with the noble gas configuration [Ar]4s23d104p5[\mathrm{Ar}]4s^23d^{10}4p^5 ?

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Gas

23.

Given boron’s electron configuration of [He]2s22p1[\mathrm{He}]2s^22p^1 , which of the following represents its electron-dot structure? Select the correct diagram among options a–d.

a)

a

b)

b

c)

c

d)

d

24.

What is the total number of electrons in the N 3−^{3-} ion?

a)

10

b)

14

c)

16

d)

18

25.

Use the following diagram to answer: Which element in the chart has the highest electronegativity?

a)

A

b)

C

c)

D

d)

E

26.

Use the following diagram to answer: Which element in the chart would be solid, malleable and conductive?

a)

A only

b)

A, C, D, and E

c)

B only

d)

C, D, and B

27.

Use the following diagram to answer: Which ranking lists the elements on the chart from largest to smallest atomic radius?

a)

A, C, B, D, E

b)

E, D, B, C, A

c)

C, D, E, A, B

d)

B, E, D, C, A

28.

Use the following diagram to answer: Which element in the chart will lose 1 electron when it reacts?

a)

A

b)

B

c)

C

d)

D

29.

Which process is the opposite of sublimation?

a)

Melting

b)

Deposition

c)

Vaporizing

d)

Decomposition

30.

A substance has particles that are close together with no regular arrangement. The particles vibrate and slide past each other. The substance is difficult to compress and flows easily. Which state of matter is the substance displaying?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

31.

Consider the Haber-Bosch reaction and select the stressors that will induce the reaction to produce more ammonia: N 2_2 (g) + 3H 2_2 (g) ⇌\rightleftharpoons 2NH 3_3 (g) + 92 kJ; I. Add nitrogen; II. Increase the temperature; III. Decrease the temperature; IV. Increase the pressure.

a)

I only

b)

IV only

c)

I, III, and IV

d)

I, II, and IV

32.

Consider the following potential energy diagram. Which letter represents the activation energy in the presence of a catalyst?

a)

A

b)

B

c)

C

d)

D

33.

Given the thermochemical equation H 2_2 (g) + Cl 2_2 (g) →\rightarrow 2HCl(g) ΔH=−185.2 kJ\Delta H = -185.2\,\mathrm{kJ} , which statement best describes the enthalpy of the reaction?

a)

The reaction is exothermic and releases energy to the environment.

b)

The reaction is exothermic and absorbs energy from the environment.

c)

The reaction is endothermic and releases energy to the environment.

d)

The reaction is endothermic and absorbs energy from the environment.

34.

The graph represents the uniform heating of a substance. Which line segment represents the liquid and gas phases coexisting?

a)

AB

b)

BC

c)

CD

d)

DE

35.

Use this heating curve to determine the boiling point of this substance.

a)

30 °C

b)

55 °C

c)

90 °C

d)

120 °C

36.

A 226.00 g sample of ice at −18.0 °C is heated to a temperature of 85.0 °C. Determine the total amount of heat absorbed by the ice.

a)

47.7 kJ

b)

75.5 kJ

c)

97.3 kJ

d)

164 kJ

37.

Consider the following phase diagram for questions #37 and #38. What is the phase change that takes place as a substance moves from B to A?

a)

Condensation

b)

Boiling

c)

Melting

d)

Freezing

38.

Consider the following phase diagram for questions #37 and #38. What is the boiling point of this liquid at 0.8 atm pressure?

a)

81.0 K

b)

83.5 K

c)

86.0 K

d)

87.5 K

39.

A student has a beaker containing 55.0 g of water at 100.0 °C. How much heat is required to convert the water to steam (gas)?

a)

124,000 J

b)

11,100 J

c)

2,200 J

d)

330 J

40.

A sample of aluminum absorbs 9.86 J of heat, and its temperature increased from 23.2 °C to 30.5 °C. What is the mass of the sample? The specific heat of aluminum is 0.90 J/g·°C.

a)

72 g

b)

8.1 g

c)

6.7 g

d)

1.5 g

41.

How many moles of nitrogen gas, N2, are present in a 48.0 liter container at a pressure of 0.750 atm and a temperature of 35.0 °C?

a)

0.702 mol

b)

1.42 mol

c)

12.53 mol

d)

0.0141 mol

42.

Which graph best shows the change in the volume of 1 mole of nitrogen gas as pressure increases and temperature remains constant?

a)

a

b)

b

c)

c

d)

d

43.

A diver finds the best corals at a depth of 10.0 m. The diver’s lung capacity is 5.40 L. The surface air temperature is 33.0 °C and the pressure is 760.0 mmHg. What is the volume of the diver’s lungs at 10.0 m at a temperature of 20.0 °C and a pressure of 1059.3 mmHg?

a)

4.05 L

b)

1.66 L

c)

3.71 L

d)

2.35 L

44.

What is the volume of 6.5 L of a gas at 35 °C when it is heated to 49 °C?

a)

4.6 L

b)

6.2 L

c)

6.8 L

d)

9.1 L

45.

How many moles is 1.2 L of nitrogen gas at STP?

a)

0.053 mol

b)

1.0 mol

c)

18.2 mol

d)

282 mol

46.

A student buys a balloon in Harris Teeter where the temperature is 19 °C and takes it outside where the temperature is 35 °C. What happens to the volume of the balloon when the student takes it outside?

a)

The volume remains unchanged.

b)

The volume decreases.

c)

The volume increases.

d)

The volume decreases, then increases.

47.

Oxygen gas from the decomposition of potassium chlorate was collected by water displacement. The barometric pressure during the experiment, which is the same as the total pressure of the system, was measured at 723.0 mmHg and the temperature was measured at 20.0 °C. What is the partial pressure of the oxygen gas (dry gas) collected? The vapor pressure of water at 20.0 °C is 17.5 mmHg.

a)

17.5 mmHg

b)

693 mmHg

c)

705.5 mmHg

d)

745.5 mmHg

48.

The pressure of a gas is…

a)

determined by the number of collisions of the gas particles on the side of the container.

b)

determined by the melting point of the gas.

c)

is measured in Kelvin.

d)

always equal to 1 atm.

49.

Which kelvin temperature is equivalent to 24 °C?

a)

226 K

b)

249 K

c)

273 K

d)

297 K

50.

A student mixes two colorless solutions together. They observe that the color changes to pink and the beaker feels cold. Based on these observations, what type of change has occurred?

a)

A chemical change that is endothermic.

b)

A chemical change that is exothermic.

c)

A physical change that is endothermic.

d)

A physical change that is exothermic.

51.

When N2O5 is heated under certain conditions, O2 and NO2 are produced. What type of reaction is this?

a)

Combustion

b)

Decomposition

c)

Double replacement

d)

Synthesis

52.

Consider the following unbalanced equation: C4H10 (l) + O2 (g) → CO2 (g) + H2O (l). What is the coefficient of C4H10 once the equation is balanced with the lowest coefficients?

a)

1

b)

2

c)

6

d)

13

53.

The following equation is an example of a ______ reaction. CH3OH (l) + O2 (g) → CO2 (g) + H2O (l)

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

54.

Which is the correct balanced chemical equation for the reaction between aluminum and silver nitrate to form aluminum nitrate and silver.

a)

Al(s) + AgNO3(aq) → AlNO3 (aq) + Ag (s)

b)

3Al(s) + AgNO3(aq) → Al3NO3 (aq) + Ag (s)

c)

Al(s) + 3AgNO3(aq) → Al(NO3)3 (aq) + 3Ag (s)

d)

Al(s) + 3AgNO3(aq) → 3Al(NO3)3 (aq) + 3Ag (s)

55.

When the reaction ___ Ca(ClO3)2 → ___ CaCl2 + ___ O2 is correctly balanced, what is the coefficient of CaCl2?

a)

1

b)

2

c)

3

d)

4

56.

Use the solubility rules to predict the precipitate for the following reaction: NiCl2(aq) + Li2S(aq) → NiS + LiCl

a)

NiCl2

b)

Li2S

c)

NiS

d)

No precipitate formed

57.

According to the activity series of metals, which of the following metals will replace all of the other metals listed?

a)

Cu

b)

Ag

c)

Mg

d)

Na

58.

What is the net ionic equation for: CoCl2(aq) + NaOH (aq) → NaCl (aq) + Co(OH)2(s)

a)

Co + 2OH → Co(OH)2

b)

Na + Cl → NaCl

c)

Co2+ + 2OH− → Co(OH)2

d)

Na+ + Cl− → NaCl

59.

Which of the following is a neutralization reaction?

a)

H2S(g) + Ca(ClO3)2(s) → HClO3 + CaS

b)

H2SO4(aq) + Ca(NO3)2(aq) → HNO3 + CaSO3

c)

H2SO4(aq) + Ca(OH)2(aq) → HOH + CaSO4

d)

SO2(g) + CaO(s) → no reaction

60.

For the reaction: 2 HNO3 + Mg(OH)2 → Mg(NO3)2 + 2 H2O, how many grams of magnesium nitrate are produced from 0.800 moles of nitric acid (HNO3)?

a)

59.3 g

b)

37.0 g

c)

592 g

d)

818 g

61.

Which of the following correctly labels the enthalpy of reaction for the endothermic potential energy diagram?

a)

A

b)

B

c)

C

d)

D

62.

Given the balanced equation: CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g), what is the total number of moles of CO2 formed when 4.0 moles of HCl is completely consumed?

a)

1.0 mol

b)

2.0 mol

c)

4.0 mol

d)

5.0 mol

63.

How many grams of carbon monoxide will be produced from 19.53 g of iron react according to the following reaction: 3 Fe + 4 CO2 → 4 CO + Fe3O4

a)

13 g

b)

98 g

c)

130 g

d)

390 g

64.

How many grams of iron will be required to react completely with 2.52×10232.52 \times 10^{23} particles of carbon dioxide according to the reaction: 3 Fe + 4 CO2 → 4 CO + Fe3O4.

a)

12.5 g

b)

17.5 g

c)

20.9 g

d)

27.8 g

65.

A student reacts 5.00 g of barium hydroxide with excess iron(III) chloride in lab according to the balanced chemical equation: 3Ba(OH)2 + 2FeCl3 → 2Fe(OH)3 + 3BaCl2. They collect the iron(III) hydroxide precipitate, wash it thoroughly with deionized water, and then dry the precipitate. Data: Mass of the filter paper: 0.81 g; Mass of the filter paper with dry precipitate: 2.75 g. The calculated theoretical yield is 2.08 g. What is the student’s percent yield for the lab?

a)

55.0 %

b)

93.3 %

c)

75.6 %

d)

132 %

66.

Calculate the percent of oxygen in Ca(OH)2, calcium hydroxide.

a)

22%

b)

28%

c)

43%

d)

70%

67.

Benzene has the molecular formula C6H6. What is the percent composition of carbon in benzene?

a)

92.3 %

b)

50.0%

c)

12.0%

d)

7.71%

68.

Which of the following is the correct nuclear notation for an element with 20 protons, 20 neutrons, and 18 electrons?

a)

2020Ca2+^{20}_{20}\mathrm{Ca}^{2+}

b)

2040Ca^{40}_{20}\mathrm{Ca}

c)

2040Ca2+^{40}_{20}\mathrm{Ca}^{2+}

d)

1840Ca2+^{40}_{18}\mathrm{Ca}^{2+}

69.

How many electrons are in an atom of 14N^{14}\mathrm{N} ?

a)

7

b)

14

c)

10

d)

4

70.

A hydrate is a compound that includes water molecules within its crystal structure. During an experiment to determine the percent by mass of water in a hydrated crystal, a student collected the following data: Mass before heating 4.10 g; Mass after heating 3.70 g. What is the percent by mass of water in this crystal?

a)

0.40 %

b)

9.8%

c)

11%

d)

90.0%

71.

What is the molar mass of aluminum acetate, Al(C2H3O2)3?

a)

86 g/mol

b)

150 g/mol

c)

118 g/mol

d)

204 g/mol

72.

As the number of effective collisions between reacting particles increases, the rate of the reaction…

a)

Decreases

b)

Increases

c)

Does not change

d)

Cannot be determined given the information

73.

Which change would most likely increase the rate of a chemical reaction?

a)

Decreasing the concentration of the reactants

b)

Decreasing the surface area of the reactants

c)

Adding a catalyst to the reaction mixture

d)

Cooling the reaction mixture

74.

Which factors must be equal in a reversible chemical reaction when it is at equilibrium?

a)

The amounts of the reactants and products

b)

The potential energies of the reactants and products

c)

The activation energies of the forward and reverse reactions

d)

The rates of the forward and reverse reactions

75.

What is the pH of a solution that is 1.45×10−13 M1.45 \times 10^{-13}\,\mathrm{M} [H3O+]?

a)

2.84

b)

12.84

c)

-2.84

d)

-12.84

76.

What is the pH of 0.040 M0.040\,\mathrm{M} [OH−]?

a)

0.80

b)

1.09

c)

12.60

d)

13.20

77.

What is the correct name for H3PO4?

a)

Hydrophosphoric acid

b)

Phosphoric acid

c)

Trihydrogen phosphate

d)

Hydrogen triphosphate

78.

According to the solubility graph, what is the approximate number of grams of potassium nitrate KNO3 that can be dissolved at a temperature of 10 °C?

a)

89 g

b)

20 g

c)

10 g

d)

0 g

79.

Which of the following substances would show a decrease in solubility when temperature increases?

a)

Fe (s)

b)

CO2 (g)

c)

KI (s)

d)

C2H5OH (l)

80.

When dissolving a cube of sodium chloride in water, which of the following changes will cause the cube to dissolve more quickly?

a)

Agitating the mixture

b)

Pouring out half of the water

c)

Increasing the pressure on the solution

d)

Decreasing the temperature of the solution

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