Free Printable AP Chem Sem 1 Review

1.

A mixture of elements was analyzed using a mass spectrometer. Based on the graph, which of the following is correct?

a)

The sample contains 4 elements, each with only one isotope.

b)

The sample contained one element with 4 different isotopes.

c)

There are 2 elements, one with 1 isotope and the other with 3 isotopes.

d)

The sample contained 100 elements with 4 different isotopes.

2.

Cl- and K+ are isoelectronic. Which of the following describes their relative sizes and best explains the difference?

a)

Cl- ion is larger; Cl- is more electronegative than K.

b)

Cl- ion is larger, Cl- has a lower effective nuclear charge.

c)

K+ ion is larger; K+ has more protons, so the ion is larger.

d)

K+ ion is larger; the K+ ion has a higher ionization energy.

3.

How many nitrogen atoms are there in 150 grams of dinitrogen trioxide, $N_2O_3$ ? (MM=76 g/mol)

a)

$6.0x10^{23}$

b)

$1.2x10^{23}$

c)

$1.2x10^{24}$

d)

$2.4x0^{24}$

4.

Which of the following best helps to account for the fact that the Cl^- ion is smaller than the S^2- ion?

a)

Cl^-has a larger nuclear mass than S^2- has.

b)

Cl^- has a larger nuclear charge than S^2- has.

c)

Cl^- has more electrons than S^2- has.

d)

Cl^- is more electronegative than S^2- is.

e)

Cl^- is more polarizable than S^2- is.

5.

A compound contains 1.10 mol of K, 0.55 mol of Te, and 1.65 mol of O. What is the simplest formula of this compound?

a)

KTeO

b)

KTe₂O

c)

K₂TeO₃

d)

K₂TeO₆

e)

K₄TeO₆

6.

Element, Z, with an e-configuration of $1s^2\ 2s^2\ 2p^6\ 3s^2\ 3p^6\ 4s^2\ 3d^{10}\ 4p^1$ forms a compound with fluorine. What is the charge of "Z" and the compound formed?

a)

$Z^+,ZF$

b)

$Z^-,FZ$

c)

$Z^{5^-},\ F_5Z$

d)

$Z^{3^+},\ ZF_3$

7.

A compound contains 30. percent sulfur and 70. percent fluorine by mass. The empirical formula of the compound is

a)

$SF$

b)

$SF_2$

c)

$SF_4$

d)

$SF_6$

e)

$S_2F$

8.

A sample of CaCO₃ (molar mass 100. g) was reported as being 30. percent Ca. Assuming no calcium was present in any impurities, the percent of CaCO₃ in the sample is

a)

30%

b)

40%

c)

70%

d)

75%

e)

100%

9.

Given the following values for electronegativity, arrange the following compounds in order of increasing bond polarity. $NF_3,NCl_3,NBr_3,NI_3$

a)

$NF_3<NI_3<NBr_3<NCl_3$

b)

$NCl_3<NI_3<NBr_3<NF_3$

c)

$NF_3<NBr_3<NI_3<NCl_3$

d)

$NCl_3<NBr_3<NI_3<NF_3$

10.

Consider the substance lithium sulfate, $Li_2SO_4$ , the attraction between the S and O would be considered ____________, while the attraction between Li and S would be considered ______________.

a)

a polar covalent bond, an ionic bond

b)

a nonpolar covalent bond, an ionic bond

c)

an ionic bond, a polar covalent bond

d)

a polar covalent bond, a polar covalent bond

11.

The Morse potential energy diagram is shown for the C=C and C=N bonds, identify the C=N bond shown on the graph and then explain the difference in the two curves.

a)

X is the C=N bond, the length of the bond is shorter because the atomic radius of N is smaller than that of C

b)

X is the C=N bond, the length of the bond is shorter because the atomic radius of N is larger than that of C.

c)

Z is the C=N bond, the length of the bond is shorter because the atomic radius of N is smaller than that of C.

d)

Z is the C=N bond, the length of the bond is shorter because the atomic radius of N is larger than that of C.

12.

Which of the following pairs of ions will require the least amount of energy to separate?

a)

$Li^+\ and\ F^-$

b)

$Na^+\ and\ Br^-$

c)

$Al^{_3+}and\ S^{2-}$

d)

$Mg^{2^+}and\ P^{3^-}$

13.

Which molecule has the smallest bond angle?

a)

$H_2S$

b)

$PCl_3$

c)

$XeF_2$

d)

$CBr_4$

14.

Which molecule has an expanded octet?

a)

$H_2S$

b)

$PCl_3$

c)

$XeF_2$

d)

$CBr_4$

15.

Which molecule is not $sp^3$ hybridized?

a)

$H_2S$

b)

$PCl_3$

c)

$XeF_2$

d)

$CBr_4$

16.

Galvanized steel can be formed by reacting steel (an alloy of iron, Fe, and carbon, C) with molten zinc, Zn, to form a corrosion resistant alloy on the surface of the steel. Which of the following images best represents galvanized steel?

a)

b)

c)

d)

17.

Based on the resonance structures shown above, what are the bond orders of the two carbon-oxygen bonds?

a)

1 and 1.5

b)

1 and 2

c)

1.5 and 1.5

d)

1.5 and 2

18.

Which of the following molecules contains exactly three sigma (σ) bonds and two pi (π) bonds?

a)

C₂H₂

b)

CO₂

c)

HCN

d)

SO₃

e)

N₂

19.

Which of the following molecules contains polar covalent bonds but is a nonpolar molecule?

a)

CH₃Cl

b)

CH₂Cl₂

c)

NH₃

d)

CCl₄

e)

N₂

20.

Which of the following incorrectly identifies the type or types of intermolecular forces present in the substance?

a)

Ozone, $O_3$ , London dispersion forces

b)

Carbon disulfide, $CS_2$ , London dispersion forces

c)

Ammonia, $NH_3$ , hydrogen bonding, dipole-dipole interactions, and London dispersion forces

d)

Hydrogen cyanide, HCN, dipole-dipole interactions and London dispersion forces

21.

Which of these ions would have the strongest ion -dipole with water?

a)

Lithium

b)

Scandium

c)

Copper

d)

Zinc

22.

A substance is found to have no odor, has a high melting point and as a solid it doesn’t conduct electricity but will when placed into water. What will happen to this substance if it was hit with a hammer?

a)

bend because it has metallic interactions

b)

break because it has ionic interactions

c)

bend because it has dipole-dipole interactions

d)

break because it has covalent network interactions

23.

Which of the following best explains why the molar volume of a liquid and a solid of the same substance are similar while the volume of the same substance as a gas is much greater?

a)

particles are very close together as a gas, but as a solid and a liquid they are further apart

b)

gas particles are smaller while the particles as a solid and a liquid are close to the same size

c)

particles are far away from each other as a gas but are very close together as a solid and a liquid

d)

gas particles are larger while the particles as a solid and a liquid are close to the same size

24.

A 0.50 L tank was used to combine 1.0 L of helium gas, He, at a pressure of 2.0 atm with 1.0 L of neon gas, Ne, at a pressure of 4.0 atm. What is the final pressure of the system? Assume that the temperature remains constant.

a)

2.0 atm

b)

6.0 atm

c)

12.0 atm

d)

24.0 atm

25.

Which of the following pairs can form a hydrogen bond between them?

a)

$H_2S+H_2O$

b)

$H_2O+LiCl$

c)

$HF+HCl$

d)

$NH_3+CH_3OH$

26.

Based on the information in the table above, which liquid, CS₂(l) or CCl₄(l), has the higher equilibrium vapor pressure at 25°C, and why?

a)

CS₂(l), because it has stronger London dispersion forces

b)

CS₂(l), because it has weaker London dispersion forces

c)

CCl₄(l), because it has stronger London dispersion forces

d)

CCl₄(l), because it has weaker London dispersion forces

27.

Consider the Maxwell-Boltzmann distribution for the two gases as shown. Which of the following statements is true?

a)

Gas A is hotter than gas B

b)

Gas A is cooler than gas B

c)

There is a greater number of particles of gas A.

d)

Gas A is a diatomic while gas B is monatomic.

28.

Which of the following behaves most like an ideal gas at the conditions indicated?

a)

H₂(g) molecules at 10^-3 atm and 200^oC

b)

O₂(g) molecules at 20 atm and 200^oC

c)

SO₂(g) molecules at 10^-3 atm and 200^oC

d)

NH₃(g) molecules at 20 atm and 300^oC

29.

Under which of the following circumstances would a solution be most likely to form?

a)

Strong solvent-solvent interactions

b)

Strong solute-solute interactions

c)

Strong solute-solvent interactions

d)

Weak solute-solvent interactions

30.

Which of the following would have the highest concentration of sodium ions?

a)

2.0 moles of sodium phosphate, $Na_3PO_4$ , dissolved in 500. mL of solution.

b)

1.0 mole of sodium sulfate, $Na_2SO_4$ dissolved in 250. mL of solution

c)

4.0 moles of sodium chloride, $NaCl,$ dissolved in 500 mL of solution.

d)

3.0 moles of sodium phosphate, $Na_3PO_4,$ dissolved in 1000. mL of solution.

31.

Of the following mixtures of liquids, predict which pair would be immiscible.

a)

$Br_2+CCl_4$

b)

$CH_3OH+CH_3COOH$

c)

$C_6H_6+C_8H_{18}$

d)

$C_8H_{18}+CH_3OH$

32.

Based on the results of the paper chromatography experiment shown above, which of the following can be concluded about the dye?

a)

It has weak intermolecular forces.

b)

It has a small molar mass.

c)

It has a stronger attraction for the stationary phase than it has for the mobile phase.

d)

It has a weaker attraction for the stationary phase that it has for the mobile phase.

33.

Which of the following techniques should be used to separate a homogeneous mixture of the following liquids?

a)

Thin Layer Chromatography

b)

Distillation

c)

Column Chromatography

d)

Filtration

34.

0.27 grams of Aluminum metal, Al, will react with 0.010 L of 6.0 M hydrochloric acid, HCl, solution according to the following balanced equation:

$2Al(s)+6HCl(aq)🡪2AlCl_3(aq)+3H_2(g)$

How many moles of hydrogen gas, $H_2$ , can be formed?

a)

0.015 moles

b)

0.018 moles

c)

0.030 moles

d)

0.045 moles

35.

If the net ionic equation below were performed and 15.0 ml of 0.40 M potassium iodide, KI, was needed to reach the endpoint of the titration, calculate the amount of moles of arsenic pentoxide, $As_2O_5$ , that were present in the initial sample.

$As_2O_5+4H^+++4I^--🡪As_2O_3+2I_2+2H_2O$

a)

6.0 moles

b)

0.0015 moles

c)

0.0060 moles

d)

0.024 moles

36.

Complete the following half reactions with the appropriate number of electrons and then determine the total number of electrons transferred in the balanced chemical equation.

a)

2 electrons

b)

5 electrons

c)

7 electrons

d)

10 electrons

37.

A 25 mL sample of an unknown concentration of hydrochloric acid, HCl was titrated with 50. mL of an aqueous solution of 0.30 M barium hydroxide, $Ba(OH)_2$ , until the reaction reached the equivalence point. What was the concentration of the unknown hydrochloric acid solution?

a)

0.15 M

b)

0.30 M

c)

0.60 M

d)

1.2 M

38.

Which of the following incorrectly classifies the strength of the acids or bases?

a)

$H_2SO_3,$ Weak Acid

b)

$HBr,\$ Strong Acid

c)

$Al(OH)_3,\$ Strong Base

d)

$KOH,\$ Strong Base

39.

$Fe\left(s\right)\ +\ 2HCl\left(aq\right)\ \longrightarrow\ \ FeCl_2\left(aq\right)\ +\ H_2\left(g\right)$

When a student adds 30.0 mL of 1.00 M HCl to 0.56 g of powdered Fe, a reaction occurs according to the equation above. When the reaction is complete at 273 K and 1.0 atm, which of the following is true?

a)

HCl is in excess, and 0.100 mol of HCl remains unreacted.

b)

HCl is in excess, and 0.020 mol of HCl remains unreacted.

c)

0.015 mol of FeCl₂ has been produced.

d)

0.22 L of H₂ has been produced.

40.

What mass of Au is produced when 0.0500 mol of Au₂S₃ is reduced completely with excess H₂?

a)

9.85 g

b)

19.7 g

c)

39.4 g

d)

48.9 g

41.

NH₃(aq) + HCl(aq) ⇄ NH₄⁺(aq) + Cl^-(aq)

The Brønsted-Lowry bases in the reaction represented above are

a)

NH₃(aq) and NH₄⁺(aq)

b)

NH₃(aq) and Cl^-(aq)

c)

HCl(aq) and NH₄⁺(aq)

d)

HCl(aq) and Cl^-(aq)

AP Chem Sem 1 Review

Total questions: 41

Worksheet time: 50mins

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