wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Honors Chemistry Final Exam Review

Total questions: 68

Worksheet time: 2hrs 2mins

Name
Class
Date
1.

The molar volume of a gas at STP occupies _____________.

a)

22.4 L

b)

0˚C

c)

1 kiloPascal

d)

12 grams

2.

Chemical equations must be balanced to satisfy ____.

a)

The law of definite proportions

b)

The law of multiple proportions

c)

The law of conservation of mass

d)

Avogadro's principle

3.

What are the coefficients that will balance the skeleton equation below?

AlCl3 + NaOH → Al(OH)3 + NaCl

a)

1,3,1,3

b)

3,1,3,1

c)

1,1,1,3

d)

1,3,3,1

4.

How many moles of aluminum are needed to react completely with 1.2 mol of FeO?

2Al(s) + 3FeO(s) → 3Fe(s) + Al2O3(s)

a)

1.2 mol

b)

0.8 mol

c)

1.6 mol

d)

2.4 mol

5.

What is the name of H2SO4?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

6.

If 2.00 L of a gas in a container at room temperature exerts a pressure of 4.00 atm. If the pressure doubles and the temperature remains the same, the volume would become ________.

a)

16.0 L

b)

2.00 L

c)

4.00 L

d)

1.00 L

7.

A sample of gas occupies 52.0 mL at 20℃ and 1.00 atm. What volume will it occupy at 40℃ and 1.00 atm?

a)

62.4 mL

b)

44.8 mL

c)

55.5 mL

d)

48.7 mL

8.

When an equation is used to calculate the amount of product that could form during a reaction, then the value obtained is called the ____.

a)

Actual yield

b)

Percent yield

c)

Minimum yield

d)

Theoretical yield

9.

The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?

a)

Combustion reaction

b)

Single replacement reaction

c)

Double replacement reaction

d)

Decomposition reaction

10.

The specific heat of ethanol is 2.44J/g˚C. How many kilojoules of energy are required to heat 50.0g of ethanol from -20.0˚C to 68.0˚C?

a)

10.7 kJ

b)

8.30 kJ

c)

2.44 kJ

d)

1.22 kJ

11.

Which is the most likely ∆H for an endothermic reaction?

a)

0 kJ

b)

-16 kJ

c)

+16 kJ

d)

There is no such thing as an endothermic reaction

12.

An ionic bond is between

a)

metal and metal

b)

metal and nonmetal

c)

nonmetal and nonmetal

13.

A covalent bond is between

a)

metal and metal

b)

metal and nonmetal

c)

nonmetal and nonmetal

14.

Which Lewis dot matches the electron configuration?

 1s21s^2   2s22s^2   2p22p^2   2p62p^6   3s13s^1  

a)
b)
c)
15.

What is the correct structural formula for a molecule of Nitrogen trihydride (NH3)?

a)
b)
c)
16.

Which name represents the formula  Fe2O3Fe_2O_3  ?

a)

Iron (III) oxide

b)

Iron (II) oxide

17.

1s22s22p63s23p63d104s24p3

Which element does this configuration belong to?

a)

Arsenic

b)

Calcium

c)

Lithium

d)

Aluminum

18.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
19.

Which scientist proposed the Planetary Model of the atom?

a)

Bohr

b)

Dalton

c)

Rutherford

d)

Thomson

20.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
21.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
22.
Calculate 7.987 m - 0.54 m and give your answer with the appropriate number of significant figures.
a)
7.45 m
b)
7.447 m
c)
7.4 m
d)
7.5 m
23.

Predict the products for this reaction: Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

24.

Identify the type of rxn:

PbCl2 + 2AgNO3 → Pb(NO3)2 + 2AgCl

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

25.

What is the name for MgF2 ?

a)

magnesium fluoride

b)

magnesium difluoride

c)

magnesium(II) fluoride

d)

magnesium fluorite

26.

Select the correct formula for sulfur hexachloride.

a)

S2Cl6

b)

S6Cl

c)

SCl6

d)

SCl2

27.

What is the percent by mass of fluorine in calcium fluoride?

a)

24%

b)

49%

c)

51%

d)

65%

28.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

29.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
30.

How much SOCl2 should be produced when 16.2 g SO2 reacts with 13.7 g PCl5 according to the following equation? SO2 + PCl5 --> SOCl2 + POCl3

a)

7.87 g

b)

30.1 g

c)

26.4 g

d)

19.8 g

31.

Calculate the volume that a 0.323-mol sample of a gas will occupy at -8°C and a pressure of 0.900 atm.

a)

7.18 L

b)

7.81 L

c)

4.63 L

d)

4.36 L

32.

When the temperature of a gas increases the particles

a)

speed up and move closer together.

b)

speed up and move farther apart.

c)

slow down and move closer together.

d)

slow down and move farther apart.

33.

How many neutrons does this isotope of titanium have?

a)

48

b)

22

c)

26

d)

70

34.

Which of these elements has the lowest ionization energy?

a)

oxygen

b)

fluorine

c)

sulfur

d)

chlorine

35.

A rigid plastic container holds methane gas at 0.9 atm pressure when the temperature is 22.0°C. How much more pressure will the gas exert if the temperature is raised to 44.6°C?

a)

0.97 atm

b)

1.82 atm

c)

0.97oC

d)

1.82oC

36.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

37.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
38.

Which atom has the largest atomic radius?

a)

potassium

b)

calcium

c)

rubidium

d)

strontium

39.

What molecular geometry is the structure shown here?

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

40.

For which of the following would hydrogen bonding occur between molecules?

a)
b)
c)
d)
41.

How many mL of stock solution of 2.0 M NaCl do you need to prepare 100.0 mL of 0.150 M NaCl?

a)

7.5 mL

b)

15 mL

c)

1300 mL

d)

200 mL

42.
What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?
a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
43.

2Fe2O3 + C → Fe + 3CO2

You react 28.00 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2?

a)

58.83%

b)

308%

c)

6435%

d)

15.5

44.

When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

45.

Which compound has both ionic and covalent bonds?

a)

CH4

b)

CO

c)

CaCl2

d)

MgSO4

46.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

47.

What is the concentration (M) of hydronium ions if the pH is 4.23?

a)

5.9 x 10-6 M

b)

5.9 x 10-5 M

c)

5.9 x 10-9 M

d)

5.9 x 10-8 M

48.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

5.0

c)

2.5

d)

7

49.

A solution that contains all of the solute it can hold at a given temperature is

a)

diluted.

b)

saturated.

c)

supersaturated.

d)

unsaturated.

50.

CH4 + 2 O2 → CO2 + 2 H2O

How many moles of carbon dioxide are produced from the combustion of 110. g of CH4?

a)

13.7 mol

b)

2.75 mol

c)

6.11 mol

d)

6.85 mol

51.

At 30'C, which substance has the lowest solubility?

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

52.

Which of the following molecules have this molecular shape?

a)

CH4

b)

CO2

c)

PCl5

d)

BF3

53.
What is Specific Heat?
a)
The  amount of thermal energy required to increase the temperature of 1kg of a material by 1°C.
b)
The  amount of radiant energy required to increase the temperature of 1kgof a material by 1°C
c)
The  amount of energy required to increase the temperature of 1kgof a material by 1°C.
d)
The  amount of friction  required to increase the temperature of 1kgof a material by 1°C.
54.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

55.

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

a)

12.82 °C

b)

24.12°C

c)

1.95 °C

d)

5128 °C

56.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
57.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

58.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

59.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

60.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

61.

Valence electrons are

a)

the number of electrons in the outer most energy shell.

b)

the number of protons in the nucleus.

c)

the atomic mass.

d)

total number of electrons.

62.

How many valence electrons does phosphorus (P).

a)

3

b)

5

c)

15

d)

31

63.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
64.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
65.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
66.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
67.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
68.

What is the atomic mass of an element with 16 protons, 13 neutrons, and 16 electrons?

a)

13 amu

b)

16 amu

c)

29 amu

d)

45 amu

Similar Resources on Wayground

Year 10 Chemistry Revision

64 questions

Year 10 Chemistry Revision

quiz

Worksheet

•

10th - 11th Grade

Yr10 - Chemical Reactions - Revision

70 questions

Yr10 - Chemical Reactions - Revision

quiz

Worksheet

•

10th Grade

Chemical formulas

67 questions

Chemical formulas

quiz

Worksheet

•

10th - 12th Grade

môn của a sa yêu quý

66 questions

môn của a sa yêu quý

quiz

Worksheet

•

10th - 11th Grade

Common Assessment -Cycle 1-Review

70 questions

Common Assessment -Cycle 1-Review

quiz

Worksheet

•

9th - 10th Grade

Honors Chem Chapter 9

65 questions

Honors Chem Chapter 9

quiz

Worksheet

•

10th Grade

Ch. 16 - Atoms and The Periodic Table

69 questions

Ch. 16 - Atoms and The Periodic Table

quiz

Worksheet

•

8th - 12th Grade

23-24 Midterm Exam Review - Unit 5 & 6

65 questions

23-24 Midterm Exam Review - Unit 5 & 6

quiz

Worksheet

•

9th Grade