Which of the following shows the correct number of protons, neutrons, and electrons in a neutral cesium-134 atom?

55 protons, 79 neutrons, 55 electrons

134 protons, 55 neutrons, 134 electrons

79 protons, 55 neutrons, 79 electrons

55 protons, 79 neutrons, 79 electrons

55 protons, 55 neutrons, 55 electrons

The pressure, in atm, exerted by 1.85 mol of an ideal gas placed in a 3.00 L container at 35.0°C is given by which of the following expressions?

(1.85)(35.0)/(0.0821)(3.00) atm

(3.00)(1.85)/(0.0821)(35.0) atm

A pure liquid in an open vessel boils at the temperature at which the

vapor pressure of the liquid becomes equal to the atmospheric pressure on the surface of the liquid

molar entropy of the liquid becomes equal to that of the gas

molar heat capacity of the liquid becomes equal to that of the gas

vapor pressure of the liquid becomes equal to the equilibrium pressure at the triple point

average kinetic energy of the liquid molecules becomes equal to that of the gas molecules

Under which of the following conditions of temperature and pressure would 1.0 mol of the real gas CO₂(g) behave most like an ideal gas?

Temperature 800 K, Pressure 0.1 atm

Temperature 100 K, Pressure 100 atm

Temperature 100 K, Pressure 0.1 atm

Temperature 800 K, Pressure 100 atm

Temperature 800 K, Pressure 1 atm

Which of the following best helps to account for the fact that the F⁻ ion is smaller than the O²⁻ ion?

F⁻ has a larger nuclear charge than O²⁻ has

F⁻ has a larger nuclear mass than O²⁻ has

F⁻ is more electronegative than O²⁻ is

F⁻ has more electrons than O²⁻ has

F⁻ is more polarizable than O²⁻ is

At standard temperature and pressure, a 0.50 mol sample of H₂ and a separate 1.0 mol sample of O₂ has the same

average molecular kinetic energy

After completing an experiment to determine gravimetrically the percentage of water in a hydrate, a student reported a value of 38 percent. The correct value for the percentage of water in the hydrate is 51 percent. Which of the following is the most likely explanation for this difference?

The dehydrated sample absorbed moisture after heating.

Strong initial heating caused some of the hydrate sample to spatter out of the crucible.

The amount of the hydrate sample used was too small.

The crucible was not heated to constant mass before use.

Excess heating caused the dehydrated sample to decompose.

The mass percent of carbon in pure glucose, C₆H₁₂O₆, is 40.0 percent. A chemist analyzes an impure sample of glucose and determines that the mass percent of carbon is 38.2 percent. Which of the following impurities could account for the low mass percent of carbon in the sample?

Fructose, C₆H₁₂O₆, an isomer of glucose

The photoelectron spectra above show the energy required to remove a 1s electron from a nitrogen atom and from an oxygen atom. Which of the following statements best accounts for the peak in the upper spectrum being to the right of the peak in the lower spectrum?

Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

Nitrogen atoms have a half-filled p subshell.

There are more electron-electron repulsions in oxygen atoms than in nitrogen atoms.

Electrons in the p subshell of oxygen atoms provide more shielding than electrons in the p subshell of nitrogen atoms.

For element X represented above, which of the following is the most likely explanation for the large difference between the second and third ionization energies?

The electron removed during the third ionization is, on average, much closer to the nucleus than the first two electrons removed were.

The effective nuclear charge decreases with successive ionizations.

The shielding of outer electrons increases with successive ionizations.

The ionic radius increases with successive ionizations.

Based on the information above and periodic trends, which of the following is the best hypothesis regarding the oxide(s) formed by Rb?

Rb will form Rb₂O, Rb₂O₂, and RbO₂.

Rb will form only Rb₂O and RbO₂.

N₂ molecules absorb ultraviolet light but not visible light. I₂ molecules absorb both visible and ultraviolet light. Which of the following statements explains the observations?

Visible light does not produce transitions between electronic energy levels in the N₂ molecule but does produce transitions in the I₂ molecule.

More energy is required to make N₂ molecules vibrate than is required to make I₂ molecules vibrate.

More energy is required to remove an electron from an I₂ molecule than is required to remove an electron from a N₂ molecule.

The molecular mass of I₂ is greater than the molecular mass of N₂.

Based on the structures shown above, which of the following statements identifies the compound with the higher boiling point and provides the best explanation for the higher boiling point?

Compound 2, because it forms hydrogen bonds, whereas compound 1 does not

Compound 1, because it has stronger dipole-dipole forces than compound 2

Compound 1, because it forms hydrogen bonds, whereas compound 2 does not

Compound 2, because it is less polarizable and has weaker London dispersion forces than compound 1

A mixture containing equal numbers of moles of ethyl acetate and butyl acetate was separated using distillation. Based on the diagrams shown above, which of the following identifies the substance that would be initially present in higher concentration in the distillate and correctly explains why that occurs?

Ethyl acetate, because it has a shorter carbon chain and weaker London dispersion forces

Ethyl acetate, because it has fewer C–C bonds to break

Butyl acetate, because it has more C–C bonds to break

Butyl acetate, because it has a longer carbon chain and weaker dipole-dipole attractions

The molecular formula and molar mass of two straight-chain hydrocarbons are listed in the table above. Based on the information in the table, which compound has the higher boiling point, and why is that compound's boiling point higher?

C₄H₁₀, because it has more electrons, resulting in greater polarizability and stronger dispersion forces

C₄H₁₀, because it has more hydrogen atoms, resulting in more hydrogen bonding

C₂H₆, because its molecules are smaller and they can get closer to one another, resulting in stronger dispersion forces

C₂H₆, because its molecules are more polar, resulting in stronger dipole-dipole attractions

At 298 K and 1 atm, Br₂ is a liquid with a high vapor pressure, and Cl₂ is a gas. Those observations provide evidence that under the given conditions, the

forces among Br₂ molecules are stronger than those among Cl₂ molecules

forces among Cl₂ molecules are stronger than the Cl–Cl bond

Br–Br bond is stronger than the Cl–Cl bond

Cl–Cl bond is stronger than the Br–Br bond

AP Chem Fall Final Exam Review Optional Practice

Quiz

•

Chemistry

•

11th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-1, HS-PS1-7, HS-PS1-3

+6

Standards-aligned

Jill Christman

Used 1+ times

FREE Resource

49 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Questions 1–3 refer to the following gases at 0°C and 1 atm. Which gas has an average atomic or molecular speed closest to that of N₂ molecules at 0°C and 1 atm?

Ne

Xe

O₂

CO

NO

Questions 1–3 refer to the following gases at 0°C and 1 atm. Which gas has the greatest density?

Ne

Xe

O₂

CO

NO

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Questions 1–3 refer to the following gases at 0°C and 1 atm. Which gas has the greatest rate of effusion through a pinhole?

Ne

Xe

O₂

CO

NO

Which gas has molecules with a pyramidal shape?

H₂(g)

HBr(g)

H₂S(g)

NH₃(g)

BH₃(g)

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which gas is the slowest to effuse through a small opening at 25 degrees Celsius and 1 atm?

H₂(g)

HBr(g)

H₂S(g)

NH₃(g)

BH₃(g)

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following ions has the same number of electrons as Br⁻?

Ca²⁺

Cl⁻

I⁻

K⁺

Sr²⁺

In solid methane, the forces between neighboring CH₄ molecules are best characterized as

covalent bonds

hydrogen bonds

ionic bonds

ion-dipole bonds

London (dispersion) forces

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AP Chem Fall Final Exam Review Optional Practice

49 questions

Questions 1–3 refer to the following gases at 0°C and 1 atm. Which gas has an average atomic or molecular speed closest to that of N₂ molecules at 0°C and 1 atm?

Questions 1–3 refer to the following gases at 0°C and 1 atm. Which gas has the greatest density?

Questions 1–3 refer to the following gases at 0°C and 1 atm. Which gas has the greatest rate of effusion through a pinhole?

Which gas has molecules with a pyramidal shape?

Which gas is the slowest to effuse through a small opening at 25 degrees Celsius and 1 atm?

Which of the following ions has the same number of electrons as Br⁻?

In solid methane, the forces between neighboring CH₄ molecules are best characterized as

Of the following electron configuration of neutral atoms, which represents an atom in an excited state?

Which of the following is a nonpolar molecule that contains polar bonds?

Which of the following shows the correct number of protons, neutrons, and electrons in a neutral cesium-134 atom?

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