Free Printable AP Chemistry Units 1-3 Review

1.

What is the chemical formula for the polyatomic ion sulfate?

a)

$S^2-$

b)

$SO_3^2-$

c)

$SO_4^2-$

d)

None of the above

2.

Which of the following represents the net ionic equation for the precipitation reaction between sodium carbonate and magnesium sulfate?

a)

Na₂CO₃ + MgSO₄ --> MgCO₃ + Na₂SO₄

b)

2Na⁺ + CO₃^-2 + Mg⁺² + SO₄^-2 --> Mg⁺² + CO₃^-2 + 2Na⁺ + SO₄^-2

c)

2Na⁺ + SO₄^-2 --> Na₂SO₄

d)

CO₃^-2 + Mg⁺² --> MgCO₃

3.

In this example, H⁺+ H₂O -> H₃O⁺the water acts as a(n)

a)

acid donating a proton

b)

acid accepting a proton

c)

base donating a proton

d)

base accepting a proton

4.

In the following example, CH₃CH₂COOH(aq) + H₂O(l) ⇄ CH₃CH₂COO^-(aq) + H₃O⁺(aq) what would be considered a conjugate acid-base pair?

a)

CH₃CH₂COOH(aq) and H₂O(l)

b)

CH₃CH₂COO^-(aq) and H₃O⁺(aq)

c)

CH₃CH₂COO^-(aq) and CH₃CH₂COOH(aq)

d)

CH₃CH₂COOH(aq) and H₃O⁺(aq)

5.

What is the oxidation number of N in NO₂^1-?

a)

0

b)

-1

c)

2

d)

3

6.

Identify the species reduced in the following reaction.

Fe_(s) + 2 Ag⁺_(aq)→ Fe²⁺_(aq) + 2 Ag_(s)

a)

Fe

b)

Ag+

c)

Ag(s)

d)

None of the above

7.

22.0 g of carbon tetrafluoride is equivalent to how many moles?

a)

4.00 moles

b)

0.250 moles

c)

0.500 moles

d)

132 x 10^23 moles

8.

Using the mass spectrum, determine the element's average atomic mass and likely identity.

a)

20.9 amu, Fluorine

b)

20.9 amu, Neon

c)

20.19 amu, Neon

d)

20.19 amu, Calcium

9.

Which of the following is NOT classified as a pure substance?

a)

Carbon

b)

Carbon dioxide

c)

Carbon monoxide

d)

Carbonated water

10.

Determine the percent composition of carbon in capsaicin ( $C_{18}H_{27}NO_3$ ), assuming the mass of Carbon = 12, H = 1, N=14, and O =16.

a)

305% C

b)

30.5% C

c)

216 % C

d)

21.6% C

e)

70.8% C

11.

True or false: $C_6H_8O_6\ and\ C_3H_4O_3$ have the same percent composition of both carbon and hydrogen?

a)

True

b)

False

12.

The ionization energies for random elements in Period 3 is given at left. Which element is most likely magnesium?

a)

Element 1

b)

Element 2

c)

Element 3

d)

Element 4

13.

What is the most likely identity of this element?

a)

Aluminum

b)

Magnesium

c)

Carbon

d)

Not enough information is given to determine this

14.

Would you predict the first ionization energy of atoms of iodine to be less than, equal to, or greater than that of atoms of fluorine? Pick the correct answer and best justification.

a)

Less than because iodine's electrons are farther from the nucleus and therefore experience less effective nuclear charge.

b)

Less than because the IE decreases down a group.

c)

Equal to because iodine and fluorine are both halogens.

d)

Greater than because iodine atoms experience a greater nuclear effective charge.

e)

Greater than because the trend increases down a group.

15.

Write the chemical formula for magnesium phosphate.

a)

MgP

b)

$Mg_3P_2$

c)

$MgPO_4$

d)

$Mg_3\left(PO_4\right)_2$

e)

$Mg_3PO_8$

16.

Determine the electron configuration for Sc in $Sc\left(NO_3\right)_3$ .

a)

$1s^22s^22p^63s^23p^64s^23d^1$

b)

$1s^22s^22p^63s^23p^64s^23d^4$

c)

$1s^22s^22p^63s^23p^6$

d)

$1s^22s^22p^63s^23p^64s^23d^2$

e)

$1s^22s^22p^63s^23p^64s^2$

17.

A hydrocarbon is analyzed and contains 86.2% carbon. What is its empirical formula?

a)

CH

b)

$CH_2$

c)

$C_2H$

d)

$CH_3$

18.

A substance melts at $750\degree C$ , is brittle, and does not conduct electricity in its solid state. Which of the following is the most likely identity?

a)

$C_6H_{12}O_{11}$

b)

$CO_2$

c)

$KCl$

19.

Which of the following molecules is nonpolar?

a)

$CH_3F$

b)

$CF_4$

c)

HF

20.

Which of the following substances will have the highest melting point? Hint - think about lattice energy and Coulomb's Law.

a)

NaCl

b)

NaF

c)

$MgCl_2$

d)

$MgF_2$

21.

Bronze is a(n) ______ alloy.

a)

Interstitial

b)

Intertwined

c)

Substitutional

d)

Superstitial

22.

Determine the formal charge on the central atom of the nitrate ion.

a)

+1

b)

0

c)

-1

d)

-2

23.

Phosphorus pentachloride will have which molecular geometry?

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Trigonal bipyramidal

d)

Octahedral

24.

What is the bond hybridization of the central carbon in dichloromethane?

a)

sp

b)

$sp^2$

c)

$sp^3$

d)

$sp^2d^1$

25.

How many pi bonds are in capsaicin?

a)

24

b)

23

c)

4

d)

5

26.

Draw a Lewis structure for C₂H₄.

27.

Which molecule will not have resonance structures?

a)

$H_2O$

b)

$O_3$

c)

$HCN$

d)

$SO_3$

28.

What is the strongest type of intermolecular force this molecule will experience?

a)

London dispersion forces (LDF)

b)

Hydrogen bonding

c)

Dipole-dipole interactions

29.

Which molecule will experience the strongest London dispersion forces?

a)

$CH_4$

b)

$C_2H_6$

c)

$C_3H_8$

30.

Which of the following substances will experience a repeating network of covalent bonds?

a)

Glass

b)

Copper

c)

Brass Alloy

d)

Silicon dioxide

31.

Which household ingredient would you expect to experience the greatest intermolecular forces?

a)

Olive oil

b)

Salad dressing

c)

Honey

d)

Chocolate syrup

32.

Which of the following statements is NOT true about an ideal gas?

a)

It experiences completely inelastic collisions

b)

The movement of its particles is completely random.

c)

It has essentially no volume.

d)

It experiences no attractive or repulsive forces between molecules.

33.

Which of the following substances contains both ionic and

covalent bonds?

a)

NH₃

b)

CH₄

c)

NaOH

d)

C₂H₅OH

34.

Dinitrogen monoxide, N₂0, has two double bonds. The general structure is N=N=O. What is the formal charge on the oxygen atom in this molecule?

a)

zero

b)

positive one (+1)

c)

positive two (+2)

d)

negative one (-1)

35.

What is the molecular geometry in the structure A?

a)

Tetrahedral

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Octahedral

36.

Which structure is more likely to correspond with the actual Lewis diagram for the sulfate ion?

a)

Structure A; single bonds are more stable than double bonds

b)

Structure A; it has the most unshared pairs of electrons

c)

Structure B; there are more possible resonance structures

d)

Structure B; fewer atoms have formal charges

37.

Which is correct for the hybridization and molecular geometry of phosphorus tribromide?

a)

sp³, tetrahedral

b)

sp³, trigonal pyramidal

c)

sp², trigonal pyramidal

d)

sp², trigonal planar

38.

Which best describes the bonding in the cyanide ion (CN^-)?

a)

3 (sigma) bonds

b)

2 (sigma) bonds and I (pi) bond

c)

1 (sigma) bond and 2 (pi) bonds

d)

3 (pi) bonds

39.

What is the molecular formula of a compound with an empirical formula of CH₂O and a molar mass of 180 g/mol?

a)

C₂H₄O₂

b)

C₃H₆O₃

c)

C₁₂H₂₄O₁₂

d)

C₆H₁₂O₆

40.

What is the hybridization of the central atom in sulfur hexafluoride (SF₆)?

a)

sp

b)

sp³d²

c)

sp²

d)

sp³

41.

Which of the following would form an insoluble compound (precipitate?)

a)

$Fe\left(NO_3\right)_3$

b)

$CaSO_4$

c)

$NH_4Cl$

d)

$KNO_3$

42.

Na₂SO₄ (aq) + Ba(NO₃)₂ (aq) $\longrightarrow$ 2NaNO₃ (aq) + BaSO₄ (s)

This reaction is a(n)...

a)

acid-base reaction

b)

oxidation-reduction reaction

c)

precipitation reaction

43.

Which of the following gases is expected to behave least ideally at a given temperature and pressure?

a)

HCI

b)

NH₃

c)

Xe

d)

He

44.

Which of the following is the best explanation of how ions in KCI interact with a water molecule in the process of dissolution?

a)

The K ions are attracted to the oxygen end of the water molecule and the CI ions are attracted to the hydrogen end.

b)

The K ions are attracted to the hydrogen end of the water molecule and the CI ions are attracted to the oxygen end.

c)

Both the K⁺ and CI^-ions are attracted to the oxygen end of the water molecule.

d)

Both the K⁺ and CI^- ions are attracted to the hydrogen end of the water molecule.

45.

The Maxwell-Boltzmann distributions of molecular speeds in samples of two different gases at the same temperature. Which gas has the smaller molar mass?

a)

Gas A

b)

Gas B

c)

smaller Both gases have the same molar mass

d)

it cannot be determined unless the pressure of each sample is known.

46.

Which of the following is most likely to be a solid at room temperature?

a)

N₂

b)

CaS

c)

CH₄

d)

HF

47.

The total pressure in the container to the right is 7.50 atm. Calculate the partial pressure of argon in the container.

a)

.94 atm

b)

4.69 atm

c)

1.88 atm

d)

6.00 atm

48.

Real gases behave most ideal gas at what conditions?

a)

High T, Low P

b)

High P, Low T

c)

High V, Low T

49.

Name a property that increases as IMF increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

50.

Which curve in this Maxwell-Boltzmann distribution represents the highest proportion of particles moving the fastest (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

All particles are moving at the same speed

51.

Why are asymmetrical molecules containing polar bonds polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

AP Chemistry Units 1-3 Review

Total questions: 51

Worksheet time: 29mins

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