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Final Exam (1b, 2b, 3b) Review -- June 2025

Total questions: 55

Worksheet time: 1hrs 20mins

Name
Class
Date
1.

Name the type of Van Der Waals force that exists between I2 (diatomic Iodine) molecules.

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

Hydrogen Bonds

2.

Which of the following molecules can produce hydrogen bonding?

a)

CBr4

b)

NO2

c)

H2S

d)

NH3

3.

Hydrogen bonding can occur between molecules when those molecules contain Hydrogen (H) covalently bonded to N, O, or F.

a)

TRUE

b)

FALSE

4.

Which is the second strongest intermolecular force, after hydrogen bonding?

a)

dipole-dipole attraction

b)

London dispersion forces

5.

Avogadro's number defines...

a)

Amedeo Avogadro's home phone number.

b)

the number of things (6.022 x 10^23) within a mole of a substance.

c)

the number of things (2.54 x 10^3) within a mole of a substance.

d)

the number of protons within an atom.

6.

For any given element, one mole weighs as much as that element’s atomic mass in ____________.

a)

Newtons

b)

Pounds

c)

Grams

d)

Kilograms

7.

The percent composition by mass of Hydrogen (H) in water (H2O) is approximately...

a)

11%

b)

89%

c)

15%

d)

55%

8.

Will this PH3 molecule be polar or nonpolar?

a)
polar
b)
nonpolar
9.

What is the molecular formula for a molecule with (a) the empirical formula CH2OCH_2O , and, (b) a molecular molar mass of approximately 90 g/mol?

a)

CH2OCH_2O  

b)

C2H4O2C_2H_4O_2  

c)

C3H6O3C_3H_6O_3  

d)

C4H8O4C_4H_8O_4  

10.

What is the approximate percent composition by mass of carbon (C) in CO2CO_2  ?

a)

~ 60%

b)

~ 40%

c)

~ 73%

d)

~ 27%

11.

What is the empirical formula of glucose (C6H12O6) ?

a)

C6H12O6

b)

C3H6O3

c)

C12H6O12

d)

CH2O

12.

How many oxygen atoms in Mg(NO3)2

a)
1
b)
2
c)
3
d)
6
13.

Which of the following molecules is nonpolar despite having polar bonds?

a)

H2O

b)

CO2

c)

NH3

d)

CH3Cl

14.

How many TOTAL electron domains are around the N in the middle?

a)

1

b)

2

c)

3

d)

4

15.

How many TOTAL electron domains are around the middle oxygen?

a)

2

b)

3

c)

4

d)

5

16.

Find the molar mass of the following compound:

(NH4)2CO3

a)

303.3 g/mole

b)

102.9 g/mole

c)

74.1 g/mole

d)

160.0 g/mole

e)

96.0 g/mole

17.

What is Avogadro's Number?

a)

6.023 x 1023

b)

6.023 x 10-23

c)

6.023

d)

6.023 x 10100

18.

Which of the metals listed below can have more than one kind of ionic charge (or oxidation state)?

a)

lithium (Li)

b)

iron (Fe)

c)

Calcium (Ca)

19.

The aluminum ion is Al3+ while the sulfide ion is S2-. What would be the correct formula for aluminum sulfide?

a)

AlS

b)

Al2S3

c)

Al3S2

d)

AlS+1

20.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
21.

Which of the following best describes (according to the Brønsted-Lowry theory), what an acid can do?

a)

accept protons

b)

donate protons

c)

increase the concentration of OH- ions in water

22.

What is the relationship between pH and pOH in a solution?

a)

pH + pOH = 7

b)

pH + pOH = 14

c)

pH - pOH = 7

d)

pH - pOH = 14

23.

What is molarity (M)?

a)

The number of moles of solute dissolved per liter of solution

b)

The number of moles of solute dissolved per kilogram of solvent

c)

The number of grams of solute dissolved per liter of solution

d)

The number of grams of solute dissolved per kilogram of solvent

24.

What does a higher Ka value indicate about an acid?

a)

The acid is weaker

b)

The acid dissociates less completely

c)

The acid is stronger

25.

What causes acid rain?

a)

Interaction of water vapor with sulfur oxides and nitrogen oxides

b)

Interaction of water vapor with oxygen

c)

Interaction of water vapor with methane

26.

As the pH of a solution gets lower, the solution becomes more _____.

a)

acidic

b)

basic (or alkaline)

c)

neutral

d)

ionic

27.

In the reaction:

HCO31– + H2O ↔ CO32– + H3O+

the hydrogen carbonate ion (HCO31–) is acting as a(n) ______.

a)

acid

b)

base

c)

indicator

d)

conjugate

28.

Strong acids necessarily have _________ conjugate bases.

a)

strong

b)

weak

29.

True or false: bases are sometimes called alkaline.

a)

True

b)

False

30.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

31.

At 25 degrees Celsius, a base has an [OH-] = 1 x 10^-4. What is its pH?

a)

12

b)

6

c)

10

d)

4

32.

CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the complete combustion of 110 g of CH4?

a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
33.

Identify the limiting reagent when 6.00 g of HCl combines with 5.00 g of Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 

a)
Mg
b)
H2
c)
MgCl2
d)
HCl
34.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
35.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
36.

How many moles of water (H2O) could form from 5.00 moles of hydrogen (H2) when oxygen (O2) is in excess?

a)

5.00 moles

b)

10.00 moles

c)

2.50 moles

d)

No Reaction

37.

You react 5.00 moles of iron (Fe) with excess oxygen (O2) and collect 385 grams of iron (III) oxide (Fe2O3). What is your % yield?

a)

96.5% yield of iron (III) oxide

b)

399 gram of iron (III) oxide

c)

104% yield of iron (III) oxide

d)

82.4% yield of iron (III) oxide

38.

Are CH4 molecules able to hydrogen bond with one another?

a)
yes
b)
no
39.

PCl5 + ___ H2O → ___ HCl + H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

40.
Which side of a chemical equation is the reactant side?
a)

Usually Left

(reaction arrow points from)

b)

Usually Right

(reaction arrow points at)

41.

Which equation is balanced?

a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
42.
Which of the following equations are correctly balanced?
a)
12CO2 +H2O --> C6H12O6 + O2
b)
CO2 + 9H2O --> C6H12O6 + O2
c)
CO2 + H2O --> 3C6H12O6 + O2
d)
6CO2 + 6H2O --> C6H12O6 + 6O2
43.

What type of reaction is represented by the equation H2 + O2 ⟶ H2OH_2\ +\ O_2\ \longrightarrow\ H_2O ?

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

44.

Classify the following reaction: 2KClO3→2KCl+3O22KClO_3\rightarrow2KCl+3O_2

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

e)

Combustion reaction

45.

What type of reaction is CuSO4+Fe→FeSO4+CuCuSO_4+Fe\rightarrow FeSO_4+Cu ?

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

e)

Combustion reaction

46.

Identify the reaction type: C3H8+5O2→3CO2+4H2OC_3H_8+5O_2\rightarrow3CO_2+4H_2O

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

e)

Combustion reaction

47.

Determine the type of reaction for AgNO3+NaCl→AgCl+NaNO3AgNO_3+NaCl\rightarrow AgCl+NaNO_3

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

e)

Combustion reaction

48.

What type of reaction is 2Na+Cl2→2NaCl2Na+Cl_2\rightarrow2NaCl ?

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

e)

Combustion reaction

49.

Determine the type of reaction for 2NaN3 → 2Na + 3N22NaN_3\ \rightarrow\ 2Na\ +\ 3N_2

a)

Synthesis reaction

b)

Decomposition reaction

c)

Single replacement reaction

d)

Double replacement reaction

e)

Combustion reaction

50.

When an organic combustion reaction has relatively little oxygen available as a reactant, there is a ________ chance of obtaining CO (cabon monoxide) as a product.

a)

higher

b)

lower

51.

Choose The Best Answer:

In single displacement reactions, the displacing atom ...

a)

can be a metal

b)

can be a nonmetal

c)

can be either a metal or nonmetal

52.

When something is reduced, it __________.

a)

gains electrons

b)

loses electrons

c)

moves non-valence electrons to valence shells

53.

What is the empirical formula if you have 46.65% nitrogen and 53.35% oxygen by mass?

a)

NO

b)

N2O4

c)

N2O3

d)

N2O5

54.

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

55.

What words best describe a London Dispersion Force?

a)

temporary intermolecular bond, instantaneous, induced

b)

permanent intermolecular bond

c)

asymmetric molecule, polar molecule

d)

Londinium, Britannium

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