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Chemistry Review

Total questions: 65

Worksheet time: 1hrs 9mins

Name
Class
Date
1.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
2.
Which units of measurement are used for volume?
a)
grams
b)
centimeters
c)
grams/milliliter
d)
milliliter
3.

What is the molecular (molar) mass of one mole of HCl?

a)

79.92 grams per mole of HCl

b)

36.46 grams per mole of HCl

c)

35.45 grams per mole of HCl

d)

1.01 grams per mole of HCl

4.

When compared, a mole of oxygen and a mole of sulfur, how many atoms each has?

a)

oxygen has 16 grams of atoms

b)

sulfur has 32.06 grams of atoms

c)

both contains 6.02 x 1023 atoms

d)

A

5.

The molar mass of CO2 is

a)

12.01 g/mol

b)

16.00 g/mol

c)

44.01 g/mol

6.

How many significant digits are in the measurement 0.0029 g (grams)?

a)
b)
c)
d)
7.

How many significant digits are in the measurement of 3.40 m (meters)?

a)
b)
c)
d)
8.

How many significant digits are there in the measurement of 60 s (seconds)?

a)
b)
c)
d)
9.

carbon dioxide

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

10.

Identify the following:

a)

element

b)

compound

c)

mixture of elements

d)

mixture of compounds

e)

mixture of elements and compounds

11.

Which of the following is a homogeneous mixture?

a)

rice pudding

b)

carbonated water with bubbles

c)

magnesium

d)

air

12.

Which of the following is a pure substance?

a)

table salt

b)

Salad

c)

sugar

d)

table salt and suger

13.
Mixture, such as mixed nuts or dry soup mix, in which different materials are unevenly distributed and are easily identified.
a)
suspension
b)
homogeneous mixture
c)
heterogeneous mixture
d)
colloid
14.

What is the molar mass of AuCl3?

a)

96.55 g

b)

130.00 g

c)

232.50 g

d)

303.32 g

15.
Law of conservation of mass states that 
a)
matter is created
b)
matter is destroyed
c)
matter is neither created nor destroyed
d)
matter does not change
16.

100g of white powder reacts with 77g of clear liquid. The reaction bubbles and changes color producing a yellow liquid that has a mass of 90g. What can be concluded?

a)

97g of gas was produced

b)

This experiment violates the conservation of mass

c)

87g of gas was produced

d)

The excess reactant is destroyed & disappears during the reaction

17.
Which subatomic particle has a positive (+) charge?
a)
Neutron
b)
Proton
c)
Electron
18.
Which subatomic particle has a neutral or no charge?
a)
Proton
b)
Electron
c)
Neutron
19.

What is the mass number?

a)

the number of protons

b)

the number of neutrons

c)

the number of protons and electrons

d)

the number of protons and neutrons

20.
How many neutrons in this species?
a)
146
b)
238
c)
92
d)
148
21.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
22.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
23.
This particle determines what element you have - the elements identity.
a)
electron
b)
proton
c)
neutron
d)
valence shell
24.

How many electrons does this element have?

a)

34

b)

28

c)

31

d)

other

25.

What is the correct symbol for an atom with 9 protons and 10 electrons?

a)

F-

b)

Ne

c)

F+

d)

other

26.

What is the correct symbol for an atom with 56 protons and 54 electrons?

a)

Ba-2

b)

Ba+2

c)

Ba-

d)

Ba+

27.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
28.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
29.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
30.

In 1s2, the 1 means

a)

there is 1 electron

b)

the electrons are in the 1st energy level

c)

the shape is circular

d)

there is a -1 charge

31.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
32.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
33.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

34.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

35.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

36.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

37.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

38.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
39.

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.

40.

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.

41.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

42.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

43.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

44.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

45.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
46.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
47.
What is the abbreviated electron configuration for barium?
a)
[Xe] 6s2
b)
[Rn] 6s2
c)
[Ar] 4s2 3d10 4p5
d)
[He] 2s2 3p1
48.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
49.

What is the shorthand configuration for Lead?

a)

[Xe]6s24f145d106p2

b)

[Xe]6s25d106p2

c)

[Rn]6s25d106p2

d)

[Rn]6s24f145d106p2

50.

A beam of light has a wavelength of 600 nm in air. What is the frequency of the light (c = 3x108 m/s)?

a)

5 x 1014 Hz

b)

2 x 1014 Hz

c)

3 x 1014 Hz

d)

6 x 1014 Hz

51.

Find the frequency of an electromagnetic wave with a wavelength 2.75 × 10–8 m.

a)

1.10 Hz

b)

1.09 × 1016 Hz

c)

9.17 × 1015 Hz

d)

9.17 × 1016 Hz

52.

What is the variable λ used for?

a)

frequency

b)

wavelength

c)

Energy

d)

speed of light

53.

What is the variable c used for?

a)

frequency

b)

wavelength

c)

Energy

d)

speed of light

54.

The frequency of light is 7.14 x 1014 Hz. What is the energy?

a)

4.73 x 10-19 J

b)

1.20 x 10-48 J

c)

1.13 x 10-17 J

d)

4.97 x 10-49 J

55.

When bombarded with light, lithium emits a light with a frequency of 4.29 x 1014 Hz. Calculate the wavelength and use the chart to predict the color.

a)

blue

b)

green

c)

yellow

d)

red

56.

Which wave has a greater frequency?

a)

A

b)

B

57.

How are frequency and wavelength related?

a)

As frequency increases, wavelength gets shorter

b)

As frequency increases, wavelength gets longer

c)

As frequency increases, wavelength gets lower

d)

As frequency increases, wavelength gets higher

58.
What are the units of frequency?
a)
m/s
b)
s
c)
Hz
d)
m
59.
Which sample of O2 contains a total of 3 x 1023 molecules?
a)
1.0 moles
b)
2.0 moles
c)
16.0 grams
d)
32.0 grams
60.
What is the mass of 3.0 x 1023 atoms of neon?
a)
1.0 g
b)
0.5 g
c)
10.0 g
d)
20.0 g
61.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
62.
What is the Molar mass of the Baking Soda? (NaHCO3)
a)
84 g
b)
84 amu
c)
52 g
d)
52 amu
63.

How many moles are there in 108 grams of H2O?

a)

7 moles

b)

6 moles

c)

5 moles

d)

4 moles

64.
Vitamin C, also known as ascorbic acid, is water soluble and cannot be produced by the human body. Each day, a person's diet should include a source of Vitamin C, such as orange juice. Ascorbic acid has a molecular formula of C6H8O6 and a gram-formula mass of 176 grams per mole.
Determine the number of moles of vitamin C in an orange that contains 0.171 grams of vitamin C.
a)
1 mole
b)
.005 mole
c)
.001 mole
d)
.0001 mole
65.

During a test, a propane lantern is operated for three hours and consumes 5.0 moles of propane (C3H8) from the lantern's tank.

Calculate the total mass of propane consumed during the lantern test.

a)

88 g

b)

132 g

c)

225 g

d)

220 g

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