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Worksheets

Final Review

Total questions: 61

Worksheet time: 2hrs 55mins

Name
Class
Date
1.

What is the atomic number of Carbon?

a)

14

b)

6

c)

12

d)

4

2.

The mass number of an element is the sum of:

a)

#protons + #neutrons

b)

#protons + #electrons

c)

#neutrons + #electrons

d)

#protons + #electrons + #neutrons

3.

How many neutrons are in the isotope C-13?

a)

13

b)

6

c)

7

d)

12

4.

How many total electrons does Br- have?

a)

35

b)

79

c)

36

d)

7

5.

How many valence electrons does Bromine have?

a)

7

b)

35

c)

36

d)

8

6.

How many significant figures does 0.00310 contain?

(a)  

7.

How many significant figures should the answer to the following have: 28.01+1.2528.01+1.25  

(a)  

8.

Answer the following in the appropriate amount of sig. fig. 25.05.012\frac{25.0}{5.012}  

(a)  

9.

Which IMFs does the following contain (select all that apply):

a)

dispersion

b)

dipole-dipole

c)

hydrogen bonding

d)

ion-dipole

10.

Which compound has the higher boiling and melting point? CH4 or C2H6

a)

CH4

b)

C2H6

11.

Classify the type of solid: CaI2

a)

atomic

b)

molecular

c)

ionic

12.

What is the formula when calcium and sulfur are combined?

a)

Ca2S2

b)

CaS

c)

CaS2

d)

Ca2S

13.

What is the formula when potassium and sulfate (SO42-) are combined?

a)

K(SO4)2

b)

K2SO4

c)

KSO4

14.

What is the name of the following formula: Cu3N

a)

copper (III) nitride

b)

copper (I) nitride

c)

copper nitride

d)

copper nitrate

15.

What is the name of the formula: S2Cl4

a)

sulfur chloride

b)

sulfur (II) chloride

c)

disulfur tetrachloride

16.

Name the following compound: HClO2

(a)  

17.

Write the full electronic configuration for nitrogen

(a)  

18.

Convert 123 millimeters to liters.

a)

0.123 L

b)

1.23 L

c)

123000 L

19.

Write the electronic configuration of Br-

(a)  

20.

Calculate molar mass of Co(NO2)2

(a)  

21.

Draw Lewis Dot Structure for KI

22.

Draw Lewis Dot structure for HCN

23.

Draw Lewis Dot Structure for CCl4

24.

What is the formula for AlBr3

a)

aluminum tribromide

b)

aluminum bromide

c)

aluminum (III) bromide

d)

aluminum (III) tribromide

25.

Convert 3.50 moles of Li2O to mass of Li2O.

a)

80.3

b)

2.11x1024

c)

0.117 g

d)

105 g

26.

How many moles of barium hydroxide are needed to react with 4.05 moles of HCl? 2 HCl + Ba(OH)2 --> BaCl2 + 2 H2O

a)

4.05

b)

8.10

c)

2.03

27.

Classify the following reaction:

2 HCl + Ba(OH)2 --> BaCl2 + 2 H2O

a)

Acid-Base Neutralization

b)

Acid-Metal

c)

Single Replacement

d)

Double Replacement

28.

Balance the following equation:

__ V2O5 + __ HCl --> __ VOCl3 + __ H2O

(a)  

29.

Define a strong acid & strong base

a)

completely dissociates

b)

partially dissociates

c)

good conductor of electricity

d)

poor conductor of electricity

30.

Identify the following: HNO2 (aq)

a)

monoprotic

b)

diprotic

c)

weak acid

d)

weak base

31.

Classify the following as an Arrhenius acid or base:

Ba(OH)2

a)

acid

b)

base

32.

Classify the following as an Arrhenius acid or base:

HCN

a)

acid

b)

base

33.

A sample of neon gas occupies a volume of 2.8 L at 1.8 atm. What will its volume be at 3.2 atm?

(a)  

34.

A balloon full of air has a volume of 4.27 L at 18 degrees Celsius. What is the volume at 42 degrees Celsius?

(a)  

35.

Predict the products of the following reaction:

2 HBr + Ca(OH)2 -->

4 lines
36.

Predict the products of the following reaction:

2 HBr + Ca -->

4 lines
37.

Predict the products of the following reaction:

H2SO4 + CaO -->

4 lines
38.

Equivalence point is reached when _________

a)

precipitate occurs

b)

moles of H+ equals moles of OH-

c)

rate of vaporization equals rate of condensation

39.

Describe an acidic solution

a)

[H3O+] is greater than [OH-]

b)

[H3O+] is less than [OH-]

c)

pH is greater than 7

d)

pH is less than 7

40.

Calculate [OH-] when [H3O+] = 4.35 x 10-4

(a)  

41.

Calculate pH when [H3O+] = 2.54x10-5

(a)  

42.

Calculate the percent of O in acetic acid (HC3H2O3)

(a)  

43.

If 5.02 moles of gas at a pressure of 788 mmHg hold a volume of 154 L, what is the temperature (in K)?

(a)  

44.

What is the mass percent of a sucrose solution containing 12.5 g sucrose and 412 g of water.

(a)  

45.

What is the mass of solute in 145 g of a solution with 23.4% percent mass of solute.

(a)  

46.

How much 6.0 NaNO3 solution should you use to make 0.585 L of a 1.2 M NaNO3 solution?

(a)  

47.

123 mL of a 3.41 M NaOH solution is diluted to 345 mL. What is the molarity of the diluted solution?

(a)  

48.

What is the volume of a 5.36 M solution that contains 39.1 moles?

(a)  

49.

Convert 23.8 cm to inches

(a)  

50.

Which conversion factor converts mass to moles and vice versa

a)

molar mass

b)

molar ratio

c)

molar volume

d)

molarity

51.

Which conversion factor converts moles of 1 compound to moles of another compound?

a)

molar mass

b)

molar ratio

c)

molar volume

d)

molarity

52.

Which conversion factor converts moles to L when given concentration?

a)

molar mass

b)

molar ratio

c)

molar volume

d)

molarity

53.

Calculate the mass percent of carbon in carbon tetrafluoride.

a)

12.0%

b)

7.81%

c)

78.1%

d)

24.1%

54.

What is the percent by mass of N in (NH4)2S? (work needed)

a)

47.1%

b)

68.1%

c)

44.1%

d)

41.1%

55.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
56.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
57.

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

a)

5.14 %

b)

13.4 %

c)

8.47 %

d)

11.8 %

58.

What is the concentration, in percent by volume, of 15.3 mL of solute in 2650 mL of solution?

a)

0.58%

b)

0.0058%

c)

5.8%

d)

58%

59.

What is the state of matter characterized by having neither a definite shape nor a definite volume?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

60.
A chemical change
a)
doesn't really change much.
b)
creates a new substance
c)
is a change in the state of matter
61.
Water vapor cooling and turning into water droplets/steam is an example of......
a)
Condensation
b)
Melting
c)
Freezing
d)
Evaporation

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