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Chemistry II PreTest

Total questions: 75

Worksheet time: 2hrs 59mins

Name
Class
Date
1.

Which of the following is the strongest type of intermolecular force?

a)

London dispersion forces

b)

Dipole-dipole interactions

c)

Hydrogen bonding

d)

Ion-dipole interactions

2.

What is the trend in atomic radius as you move down a group in the periodic table?

a)

It increases

b)

It decreases

c)

It remains the same

d)

It first increases, then decreases

3.

Which of the following compounds is most likely to be ionic?

a)

CO2

b)

NaCl

c)

H2O

d)

CH4

4.

Which variable is kept constant in Boyle’s Law?

a)

Pressure

b)

Volume

c)

Temperature

d)

Number of moles

5.

What is the molecular geometry of methane (CH4)?

a)

Trigonal planar

b)

Tetrahedral

c)

Linear

d)

Bent

6.

Which of the following molecules is polar?

a)

CO2

b)

CCl4

c)

H2O

d)

BF3

7.

Which element has the highest electronegativity?

a)

Oxygen

b)

Fluorine

c)

Chlorine

d)

Nitrogen

8.

Which of the following best describes the bonding in an ionic compound?

a)

Sharing of electrons between atoms

b)

Transfer of electrons from one atom to another

c)

Overlapping of atomic orbitals

d)

Delocalized electrons

9.

Which gas law relates pressure and temperature at a constant volume?

a)

Boyle’s Law

b)

Charles’s Law

c)

Gay-Lussac’s Law

d)

Avogadro’s Law

10.

Which of the following molecules exhibit hydrogen bonding?

a)

HCl

b)

NH3

c)

CO2

d)

CH4

11.

As the atomic number of an element increases across a period, what generally happens to its ionization energy?

a)

It decreases

b)

It increases

c)

It remains the same

d)

It fluctuates randomly

12.

Which of the following best explains why NaCl has a high melting point?

a)

It has strong covalent bonds.

b)

It has strong ionic bonds.

c)

It has weak intermolecular forces.

d)

It has metallic bonding.

13.

A sample of gas occupies 4.0 L at 1.0 atm. If the pressure is increased to 2.0 atm at constant temperature, what will the new volume be?

a)

2.0 L

b)

4.0 L

c)

8.0 L

d)

1.0 L

14.

Which of the following molecules has a bent molecular geometry?

a)

CO2

b)

H2O

c)

CH4

d)

BF3

15.

Which change will increase the boiling point of a solution?

a)

Decreasing the amount of solute

b)

Increasing the amount of solute

c)

Decreasing the pressure

d)

Increasing the temperature

16.

A student observes that the vapor pressure of a solution is lower than that of the pure solvent. Which property explains this observation?

a)

Freezing point depression

b)

Boiling point elevation

c)

Raoult’s Law

d)

Henry’s Law

17.

A gas sample behaves non-ideally at high pressure and low temperature. Explain why this occurs using intermolecular forces.

a)

At high pressure and low temperature, intermolecular forces become significant, causing deviations from ideal behavior.

b)

At high pressure and low temperature, the gas molecules move faster, so intermolecular forces are negligible.

c)

At high pressure and low temperature, the volume of the gas increases, making intermolecular forces less important.

d)

At high pressure and low temperature, the gas behaves more ideally due to increased kinetic energy.

18.

Given the following data: 1.0 mol of an ideal gas at 273 K and 1.0 atm occupies 22.4 L. If the temperature is doubled and the pressure remains constant, what will be the new volume?

a)

11.2 L

b)

22.4 L

c)

44.8 L

d)

33.6 L

19.

Which of the following elements has the largest atomic radius?

a)

Sodium

b)

Oxygen

c)

Fluorine

d)

Chlorine

20.

What type of bond is formed when two atoms share electrons equally?

a)

Ionic bond

b)

Nonpolar covalent bond

c)

Metallic bond

d)

Polar covalent bond

21.

Which law states that the volume of a gas is directly proportional to its temperature at constant pressure?

a)

Boyle’s Law

b)

Avogadro’s Law

c)

Charles’s Law

d)

Dalton’s Law

22.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
23.

Match the following units to their names.

a)

Pressure

1.

mmHg

b)

Volume

2.

L

c)

Temperature

3.

K

d)

Pressure

4.

atm

e)

Moles

5.

mol

24.

The container has a volume of 4.0 L. The temperature of the gas is lowered to 150 K, and the pressure decreases to 1.25 atm. Calculate the number of moles of gas in the container.

25.

What is the standard temperature?

a)

0K

b)

0oC

c)

173 K

d)

173.15 K

26.

What creates pressure?

a)

Gas molecules spinning

b)

Gas molecules colliding with container walls

c)

Potential energy

d)

Electrons

27.

If the pressure of a gas is doubled while the temperature remains constant, what happens to the volume of the gas?

a)

It doubles

b)

It remains the same

c)

It is halved

d)

It quadruples

28.

A 2.5-liter sample of gas is at STP. When the temperature is raised to 273°C and the pressure remains constant, what will be the new volume of the gas?

a)

A) 1.25

b)

B) 2.5

c)

C) 5.0

d)

D) 10.

29.

Why do equal numbers of small and large gas particles occupy the same volume?

a)

Large expanses of space exist between gas particles.

b)

Large particles move more slowly than smaller particles.

c)

There are fewer collisions between smaller gas particles.

30.

Match the bonds with the amount of electrons

a)

Triple bond

1.

6 electrons (3 pairs) shared

b)

Double bond

2.

4 electrons (2 pairs) shared

c)

Single bond

3.

2 electrons (1 pairs) shared

31.

Why do elements bond? (a)  

Choose from the below words

To gain new properties

To create a new element

To become stable

To get bigger

32.

Atoms of two or more elements chemically bonded together are called (a)   .

Choose from the below words

Molecule

Compound

Element

Ion

33.

Match the following

a)

C02

1.

non polar covelant

b)

H20

2.

polar covelant

c)

NaCl

3.

ionic

34.

Match the symbol and charge to the correct metal Cation

a)

Chromium (II)

1.

Cr2+

b)

Copper (I)

2.

Cu+

c)

Titanium(II)

3.

Ti2+

d)

Mercury (II)

4.

Hg2+

e)

Lead (IV)

5.

Pb4+

35.

Match the following

a)

Complete transfer of electrons

1.

ionic

b)

unequal sharing of electrons

2.

polar covelant

c)

equal sharing of electrons

3.

non-polar covelant

36.

When bonding, (a)   give up electrons and become positive (b)   .

Choose from the below words

metals

cations

nonmetals

anions

37.

Two nonmetals from Region 3 combine. This is most likely a (a)   .

Choose from the below words

Covalent Bond

Ionic Bond

Metallic Bond

38.

Match the following pertaining to the strength of IMFs and the kinetic energy (temperature) of the molecules.

a)

IMFs >> KE

1.

solid

b)

IMFs = KE

2.

liquid

c)

IMFs << KE

3.

gas

39.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
40.

Attractions between polar molecules are weaker than attractions between nonpolar molecules.

a)

True

b)

False

41.

Which state of matter has the weakest intermolecular attraction between particles?

a)

Solid

b)

Liquid

c)

Gas

42.

A student places a piece of I2 (s) in 50.0 mL of H2O (l), and another piece of I2 (s) of the same mass in 50.0 mL of C6H14 (l), then shakes the mixtures. The results are shown above. What do the results indicate about the intermolecular interactions of the substances?

a)

I2 (s) and H2O (l) have similar intermolecular interactions, and I2 (s) and C6H14 (l) do not.

b)

I2 (s) and C6H14 (l) have similar intermolecular interactions, and I2 (s) and H2O (l) do not.

c)

I2 (s), H2O (l), and C6H14 (l) all have similar intermolecular interactions.

d)

I2 (s), H2O (l), and C6H14 (l) all have three completely different types of intermolecular interactions.

43.

In this scenario, the ice is undergoing an ____________ change?

a)

Exothermic,

because heat energy is leaving the ice.

b)

Endothermic,

because heat energy is leaving the ice.

c)

Exothermic,

because heat energy is entering the ice.

d)

Endothermic,

because heat energy is entering the ice.

44.

What happens to the boiling point of a solution when a nonvolatile solute is added?

a)

It decreases

b)

It fluctuates randomly

c)

It remains unchanged

d)

It increases

45.

What is the correct coefficient for O2 when this reaction is balanced?

a)

3

b)

5

c)

6

d)

10

46.

Which of the following is NOT soluble in water?

a)

NaSO4

b)

AgBr

c)

Ca(NO3)2

d)

BaSO4

47.

What is the oxidation state of S in Na2SO4?

a)

-2

b)

+2

c)

+4

d)

+6

48.

Which of the following would require resonance structures to satisfactorily describe the bonding?

a)

H2O

b)

NO3-

c)

CO2

d)

OH-

49.

What type of hybridization does C have in CH2OH?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

50.

What is the formal charge of Cl?

a)

0

b)

+1

c)

-1

d)

-2

51.

Which Lewis dot structure shows exactly two unshared pairs of valence electrons?

a)

H2S

b)

CO2

c)

NH3

d)

CBr4

52.

What is ionization energy?

a)

How well an atom attracts electrons in a chemical bond

b)

The relative size of an atom

c)

An atom that has gained or lost an electron

d)

The amount of energy it takes to remove an electron from the valence shell of an atom

53.

Which of the following subshells has the lowest energy?

a)

4d

b)

5s

c)

5p

d)

5f

54.

Which of the following is NOT isoelectronic with the other species?

a)

S2-

b)

Br-

c)

Kr

d)

Sr2+

55.

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

56.

How many nitrogen atoms are there in 150 grams of dinitrogen trioxide, N2O3N_2O_3 ? (MM=76 g/mol)

a)

6.0x10236.0x10^{23}

b)

1.2x10231.2x10^{23}

c)

1.2x10241.2x10^{24}

d)

2.4x0242.4x0^{24}

57.

Element, Z, with an e-configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p11s^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+,ZFZ^+,ZF

b)

Z−,FZZ^-,FZ

c)

Z5−, F5ZZ^{5^-},\ F_5Z

d)

Z3+, ZF3Z^{3^+},\ ZF_3

58.

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%

59.

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)

60.

Match the generic Lewis Valence Electron Dot Structure with the elements that would have the same Lewis structure.

a)

1.

Na

b)

2.

Mg

c)

3.

Al

d)

4.

C

e)

5.

N

61.

Reorder the following steps for drawing lewis structures

a)

The Valence electrons

charge - add/subtract if there is a charge

b)

Place the lower Electronegative atom in the centre and draw in bonds

c)

Add remaining electrons as Lone pairs (terminal atoms first).

d)

If any atoms dont have an Octet, use electrons to create double bonds.

e)

Check each atom has the same number of electrons as it started with (formal charge)

1)
2)
3)
4)
5)
62.
Question Image

Match the correct part of the chemical equation with its descriptor.

a)

A

1.

Reactants

b)

B

2.

Yields

c)

C

3.

Products

d)

D

4.

Subscript

e)

E

5.

Coefficient

63.

Rohan and Emma are learning about photosynthesis! Looking at the balanced equation for photosynthesis: 6 H2O + 6 CO2 → C6H12O6 + 6 O2, how many molecules of water are needed on the reactant (starting materials) side?

a)

12

b)

6

c)

18

d)

24

64.

2 Al2O3 → 4 Al + 3O2

Setup the equation to solve for mass of Al2O3 from 96.5 g Al.

a)96 g
b)32 g
c)96.5 g
d)27 g
e)108 g
f)102 g
g)204 g
1
2
3
1)
2)
3)
65.

1 C5H12 + 8 O2 → 5O2 + 6 H2O

Setup the equation to solve for mass of H2O from 3 mol of O2.

a)6 mol
b)256 g
c)32 g
d)3 mol
e)8 mol
f)18 g
g)108 g
1
2
3
1)
2)
3)
66.

Choose the correct path on the mole map chart to solve the following problem:

H3PO4 + 5 HCl --> PCl5 + 4H2O

How many grams of PCl5 will be produced from 58.3 grams of H3PO4?

A
B
C
D
E
F
G
67.

In a chemical equation, "dissolved in water" is represented by which of the following symbols?

a)

(s)

b)

(l)

c)

(g)

d)

(aq)

68.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
69.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
70.
What are the products of this reaction?
Cu+ AgNO3--> 
a)
Cu(NO3)2+Ag
b)
CuNO3 + Ag
c)
CuAg+NO3
d)
Cu+ AgNO3
71.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
72.

What is the name of the compound HgCl2

a)

mercury (II) chloride

b)

mercury chlorite

c)

Monomercury dichloride

d)

mercury dichloride

73.
K +  and  N-3
a)
KN
b)
KN3
c)
K3N3
d)
K3N
74.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
75.
When adding a subscript to a polyatomic ion, you should...
a)
multiply any subscripts on the polyatomic ion by the subscript you are adding
b)
put parentheses around the polyatomic ion before adding a subscript
c)
write the new subscript next to any subscripts on the polyatomic ion
d)
put the polyatomic ion in square brackets before adding the subscript

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