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Worksheets

Review

Total questions: 152

Worksheet time: 4hrs 19mins

Name
Class
Date
1.

What is the name of this element?

a)

Oxygen

b)

Tin

c)

Sulfur

d)

Magnesium

2.

What is the atomic number of this element?

a)

8

b)

15.999

3.

What is the chemical symbol of this element?

a)

O

b)

Ox

c)

Oy

d)

Og

4.

What is a row of elements on the periodic table called?

a)

period

b)

group

5.

What is a column of elements on the periodic table called?

a)

period

b)

group

6.

The elements in a group have the same or similar properties.

a)

True

b)

False

7.

Which group has 2 valence electrons?

a)

Transition Metals

b)

Alkaline Earth Metals

8.

Which group has the magnetic elements iron, cobalt, and nickel?

a)

Transition Metals

b)

Alkaline Earth Metals

9.

What particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

d)

Protons, neutrons, and electrons

10.

The atomic number is equal to _.

a)

the number of protons

b)

the number of neutrons only

c)

the total number of protons and neutrons

d)

the number of protons, neutrons, and electrons

11.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

d)

115

12.

What is the mass number of this Neon atom?

a)

10

b)

11

c)

21

d)

20

13.

What changes when an atom becomes an ion?

a)

The number of electrons

b)

The number of protons

c)

The number of neutrons

d)

Both the number of neutrons and electrons

14.

What is the charge on a lithium atom that loses 1 electron?

a)

+1

b)

0

c)

-1

d)

-2

15.
How many neutrons does B (Boron) contain?
a)
5
b)
11
c)
6
d)
10.811
16.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

17.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
18.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
19.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
20.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
21.

Draw a water molecule.

22.

Which property describes water attracted to water?

a)

cohesion

b)

adhesion

c)

solvent

23.

Which of the following is not a state of matter?

a)

liquid

b)

gas

c)

frozen

d)

solid

24.

The pH of water is ______.

a)

acidic (1-6)

b)

neutral (7)

c)

basic (8-14)

25.

Atoms are made up of

a)

protons

b)

neutrons

c)

electrons

d)

all of the above!

26.

Electrons have a _____. charge.

a)

positive

b)

neutral (zero)

c)

negative

d)

strong

27.

True or False:

Pollution is any substance that is GOOD for the environment.

a)

True

b)

False

28.

Which of the following is an example of light pollution?

a)

lights from a city

b)

the sound from a loud engine

c)

battery acid

d)

wind

29.

Ionic bonds are ____ than covalent bonds.

a)

weaker

b)

stronger

c)

equal to

30.

Radio waves are the longest electromagnetic waves.

a)

True

b)

False

31.

More H (mickey ears) means a solution is more _____.

a)

acidic

b)

basic

c)

neutral

32.

Which property says water is attracted to other elements?

a)

cohesion

b)

adhesion

c)

solvent

33.

Covalent bonds share ELECTRONS

a)

True

b)

False

34.

Car batteries and cell phones can be recycled with paper and water bottles.

a)

True

b)

False

35.

Which state of matter is shown in the picture?

a)

liquid

b)

gas

c)

frozen

d)

solid

36.

Which of the following does NOT involve a physical change?

a)

mixing

b)

melting

c)

grinding

d)

decomposing

37.

Which of the following processes does NOT involve a change in chemical properties?

a)

rusting

b)

fermenting

c)

boiling

d)

burning

38.

In the measurement 0.503 L, which digit is the estimated digit?

a)

5

b)

the 0 immediately to the left of the 3

c)

3

d)

the 0 to the left of the decimal point

39.

How many significant figures are in the measurement 811.40 grams?

a)

two

b)

three

c)

four

d)

five

40.

Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.

a)

10 mm 2

b)

11 mm2

c)

11.0 mm2

d)

11.00 mm2

41.

What is the measurement 1042 L rounded off to two significant digits?

a)

1.0 x 103 L

b)

1040 L

c)

1050 L

d)

1.1 x 103 L

42.

What is the metric system prefix for the quantity 0.000 001?

a)

centi-

b)

deci-

c)

kilo-

d)

micro-

43.

What is the SI unit of mass?

a)

liter

b)

joule

c)

candela

d)

kilogram

44.

Which of the following mass units is the largest?

a)

1 cg

b)

1 dg

c)

1 mg

d)

1 ng

45.

If the temperature changes by 100 K, by how much does is change in  °C\degree C ?

a)

0 °C\degree C  

b)

37 °C\degree C  

c)

100 °C\degree C  

d)

273  °C\degree C  

46.

Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?

a)

°C\degree C 93

b)

34 °C\degree C

c)

-61 °C\degree C

d)

-34 °C\degree C

47.

What is the density of an object having a mass of 8.0 g and a volume of 25 cm3 ?

a)

0.32 g/cm3

b)

2.0 g/cm3

c)

3.1 g/cm3

d)

200 g/cm3

48.

An example of an extensive property of matter is

a)

temperature.

b)

pressure.

c)

mass.

d)

hardness.

49.

Which of the following are considered physical properties of a substance?

a)

color and odor

b)

melting and boiling points

c)

malleability and hardness

d)

all of the choices

50.

Which state of matter expands when heated and is easy to compress?

a)

gas

b)

liquid

c)

solid

d)

plasma

51.

Which of the following is a physical change?

a)

corrosion

b)

explosion

c)

evaporation

d)

rotting of food

52.

Which of the following CANNOT be classified as a substance?

a)

table salt

b)

air

c)

nitrogen

d)

gold

53.

Which of the following is a heterogeneous mixture?

a)

air

b)

salt water

c)

steel

d)

soil

54.

Which of the following is true about homogeneous mixtures?

a)

They are known as solutions.

b)

They consist of two or more phases.

c)

They have compositions that never vary.

d)

They are always liquids.

55.

Which of the following is true about compounds?

a)

They can be physically separated into their component elements.

b)

They have compositions that vary.

c)

They are substances.

d)

They have properties similar to those of their component elements.

56.

Which of the following materials is a substance?

a)

air

b)

gasoline

c)

stainless steel

d)

silver

57.

What distinguishes a substance from a mixture?

a)

Substances are compounds, and mixtures are not.

b)

Mixtures are groupings of elements, and compounds are not.

c)

Samples of the same substance can have different intensive properties.

d)

Mixtures can be separated physically, while compounds cannot.

58.

The first figure in a properly written chemical symbol always is

a)

boldfaced.

b)

capitalized.

c)

italicized.

d)

underlined.

59.

Which of the following is a chemical property?

a)

color

b)

hardness

c)

freezing point

d)

ability to react with oxygen

60.

All of the following changes to a metal are physical changes EXCEPT

a)

bending.

b)

melting.

c)

rusting.

d)

polishing.

61.

What must be done to be certain that a chemical change has taken place?

a)

Check for the production of bubbles before and after the change.

b)

Demonstrate that a release of energy occurred after the change.

c)

Check the composition of the sample before and after the change.

d)

Demonstrate that energy was absorbed by the reactants after the change.

62.

Which of the following does NOT indicate that a chemical change may have taken place?

a)

fracture formation

b)

gas production

c)

precipitate formation

d)

energy transfer

63.

What happens to matter during a chemical reaction?

a)

Matter is neither created nor destroyed.

b)

Some matter is destroyed.

c)

Some matter is created.

d)

Some matter is destroyed and some is created.

64.

How many significant figures are in the measurements 0.0034 kg?

a)

two

b)

four

c)

five

d)

This cannot be determined.

65.

How many significant figures are in the measurement 40,500 mg?

a)

two

b)

three

c)

four

d)

five

66.

How many significant figures are in the measurement 811.40 grams?

a)

two

b)

three

c)

four

d)

five

67.

Express the sum of 7.68 m and 5.0 m using the correct number of significant digits.

a)

12.68 m

b)

12.7 m

c)

13 m

d)

10 m

68.

Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.

a)

10 mm2

b)

11 mm2

c)

11.0 mm2

d)

11.00 mm2

69.

What is the measurement 111.009 mm rounded off to two significant digits?

a)

111 mm

b)

111.0 mm

c)

111.01 mm

d)

110 mm

70.

What is the SI unit of mass?

a)

liter

b)

joule

c)

candela

d)

kilogram

71.

What is the temperature -34 degrees Celcius expressed in kelvins?

a)

139 K

b)

207 K

c)

239 K

d)

339 K

72.

If the temperature changes by 100 K, by how much does it change in degrees Celsius?

a)

0 degrees Celsius

b)

37 degrees Celsius

c)

100 degrees Celsius

d)

273 degrees Celsius

73.

What is the quantity 0.0075 meters expressed in centimeters?

a)

0.075 cm

b)

0.75 cm

c)

7.5 cm

d)

70.5 cm

74.

What is the quantity 987 milligrams expressed in grams?

a)

0.000987 g

b)

0.987 g

c)

9.87 g

d)

98,700 g

75.

Which of the following is NOT among Democritus's ideas?

a)

Matter consists of tiny particles called atoms.

b)

Atoms are indivisible.

c)

Atoms retains their identity in a chemical reaction

d)

Atoms are indestructible.

76.

Dalton's atomic theory included which idea?

a)

All atoms of all elements are the same size.

b)

Atoms of different elements always combine in one-to-one ratios.

c)

Atoms of the same element are always identical.

d)

Individual atoms can be seen with a microscope.

77.

Why did J.J. Thomson reason that electron must be a part of the atoms of all elements?

a)

Cathode rays are negatively charged particles.

b)

Cathode rays can be deflected by magnets.

c)

An electron is 2000 times lighter than a hydrogen atom.

d)

Charge-to-mass ratio of electrons was the same, regardless of the gas used.

78.

All atoms are

a)

positively charged, with the number of protons exceeding the number of electrons.

b)

negatively charged, with the number of electrons exceeding the number of protons.

c)

neutral, with the number of protons equaling the number of electrons.

d)

neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons.

79.

As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?

a)

Protons, electrons, and neutrons are evenly distributed throughout the volume of the atoms.

b)

The nucleus is made of protons, electrons, and neutrons.

c)

Electrons are distributed around the nucleus and occupy almost all the volume of the atoms.

d)

The nucleus is made of electrons and protons.

80.

The atomic number of an element is the total number of which particles in the nucleus?

a)

neutrons

b)

protons

c)

electrons

d)

protons and neutrons

81.

What does the number 84 represent in the name krypton-84?

a)

the atomic mass

b)

the mass number

c)

the sum of the protons and electrons

d)

atomic numbers

82.

In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?

a)

In, 49 protons, 49 electrons

b)

Zn, 30 protons, 60 electrons

c)

Cs, 55 protons, 132.9 electrons

d)

F, 19 protons, 19 electrons

83.

How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?

a)

50 protons, 50 electrons, 75 neutrons

b)

75 electrons, 50 protons, 50 neutrons

c)

120 neutrons, 50 protons, 75 electrons

d)

70 neutrons, 75 protons, 50 electrons

84.

Which of the following statements is NOT true?

a)

Atoms of the same element can have different masses.

b)

Atoms of isotopes of an element have different numbers of protons.

c)

The nucleus of an atoms has a positive charge.

d)

Atoms are mostly empty space.

85.

Which of the following sets of symbols represents isotopes of the same element?

a)

4291 J   4292 J   4093 J_{42}^{91}\ J\ \ \ _{42}^{92}\ J\ \ \ _{40}^{93}\ J

b)

1950 L  2050 L  2150 L_{19}^{50}\ L\ \ _{20}^{50}\ L\ \ _{21}^{50}\ L

c)

3884 M   3886 M   3887 M_{38}^{84}\ M\ \ \ _{38}^{86}\ M\ \ \ _{38}^{87}\ M

d)

59138 Q   55133Q   54133 Q_{59}^{138}\ Q\ \ \ _{55}^{133}Q\ \ \ _{54}^{133}\ Q

86.

How is the number of neutrons in the nucleus of an atom calculated?

a)

Add the number of electrons and protons together.

b)

Subtract the number of electrons from the number of protons.

c)

Subtract the number of protons from the mass number.

d)

Add the mass number to the number of electrons.

87.

Which of the following statements is NOT true?

a)

Protons have a positive charge.

b)

Electrons are negatively charged and have a mass of 1 amu.

c)

The nucleus of an atom is positively charged.

d)

Neutrons are located in the nucleus of an atom.

88.

The atomic mass of an element depends upon the

a)

mass of each electron in that element.

b)

mass of each isotope in that element.

c)

relative abundance of the protons in that element.

d)

mass and relative abundance of each isotope of that element.

89.

What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?

a)

2d

b)

3d

c)

3f

d)

4s

90.

What is the electron configuration of potassium?

a)

1s22s22p23s23p24s1

b)

1s22s22p103s23p3

c)

1s22s23s23p64s1

d)

1s22s22p63s23p64s1

91.

Which of the following categories includes the majority of the elements?

a)

metalloids

b)

liquids

c)

metals

d)

nonmetals

92.

Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a)

Pt

b)

V

c)

Li

d)

Kr

93.

What element has the electron configuration 1s22s22p63s23p2?

a)

nitrogen

b)

selenium

c)

silicon

d)

silver

94.

Which of the following is true about the electron configuration of the noble gases?

a)

The highest occupied s and p sublevels are completely filled.

b)

The highest occupied s and p sublevels are partially filled.

c)

The electrons with the highest energy are in the d sublevel.

d)

The electrons with the highest energy are in an f sublevel.

95.

Atomic size generally

a)

increases as you move from left to right across a period.

b)

decreases as you move from top to bottom within a group.

c)

remains constant within a period.

d)

decreases as you move from left to right across a period.

96.

What element in the second period has the largest atomic radius?

a)

carbon

b)

lithium

c)

potassium

d)

neon

97.

Which of the following elements has the smallest atomic radius?

a)

sulfur

b)

chlorine

c)

selenium

d)

bromine

98.

What is the element with the lowest electronegativity value?

a)

cesium

b)

rubidium

c)

calcium

d)

fluorine

99.

What is the element with the highest electronegativity value?

a)

cesium

b)

oxygen

c)

calcium

d)

fluorine

100.

What is the energy required to remove an electron from an atom in the gaseous state called?

a)

nuclear energy

b)

ionization energy

c)

shielding energy

d)

electronegative energy

101.

Which of the following elements has the smallest first ionization energy?

a)

boron

b)

carbon

c)

aluminum

d)

silicon

102.

As you move from left to right across the second period of the periodic table

a)

ionization energy increases.

b)

atomic radii increase.

c)

electronegativity decreases.

d)

atomic mass decreases.

103.

If your partner gets chemical in their eye, what should be done first?

a)

Call 911

b)

Flush your eyes with water for 15 min

c)

Clean up the spill immediately to prevent slips

d)

Help them to the eye wash station

104.

What is the name of the instrument in the image?

a)

buret clamp

b)

beaker tongs

c)

crucible tongs

d)

beaker holder

105.

An egg got boiled, what kind of change occurred?

a)

physical because it is still an egg

b)

chemical because it no longer has the same properties

c)

chemical because it was a liquid and now is a solid

d)

physical because it has the same properties as before the boil

106.

Which of the following pairs is incorrect?

a)

proton--atomic number

b)

mass number--protons + neutrons

c)

atomic mass--neutrons + protons

d)

cation--positive ion

107.

62.14 g/ml--What type of data?

a)

quantitative

b)

qualitative

c)

empirical

d)

precise

108.

How many significant figures in 0.001060

a)

7

b)

6

c)

4

d)

3

109.

What prefix is used for 10-12?

a)

pico

b)

tera

c)

giga

d)

micro

110.

Which sublevel is displayed in the diagram and how many electrons does it hold?

a)

s-2

b)

d-10

c)

p-6

d)

f-14

111.

Which of the following used gold foil experiment to discover a dense center of an atom?

a)

Rutherford

b)

Thompson

c)

Dalton

d)

Democritus

112.

The average distance from the nucleus is described as which of the following terms?

a)

Sublevel

b)

Orbital

c)

Atomic radius

d)

Principle energy level

113.

What is a Lewis valence e-dot structure?

a)

a representation of the valence electrons arranged around the nucleus of an atom

b)

a model to predict the mass of the molecule

c)

a representation of the protons in an atom

d)

a list of where all the electrons are located in an atom

114.

How would you draw a Lewis dot diagram for the following atom of Arsenic. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

a)

b)

c)

d)

115.

Which of the following is the correct e-dot diagram?

a)

b)

c)

d)

116.

Which particles are represented by the dots in Lewis valence e-dot structures?

a)

core electrons

b)

valence electrons

c)

protons

d)

all electrons

117.

What is the ground state electron configuration for arsenic?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

b)

1s2 2s2 2p6 3s2 3p6 4s2 4p3 4d10

c)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

d)

1s2 2s2 2p6 3s2 3p6 4s2 4p3

118.

Which element has the ground state electronic configuration, 1s2 2s2 2p6 3s2 3p6 4s1?

a)

calcium

b)

potassium

c)

phosphorus

d)

bromine

119.

Which of the following molecules has a central atom with precisely two unshared pairs of electrons?

a)

ammonia NH3

b)

methane CH4

c)

water H2O

d)

hydrocyanic acid HCN

120.

Around the central atom in a covalently bonded molecule, there are four pairs of electrons: three shared pairs and one unshared pair. The geometry of this molecule is best described as —

a)

linear

b)

trigonal planar

c)

trigonal pyramidal

d)

tetrahedral

121.

Which of the following molecules would be expected to exhibit a tetrahedral geometry?

a)

NH3

b)

CH2O

c)

H2O

d)

CH4

122.

The following picture shows a covalent molecule. What molecule listed below has the same shape?

a)

BH3

b)

H2O2

c)

NH3

d)

Na3P

123.

What is the shape of a CO2 molecule?

a)

linear

b)

tetrahedral

c)

trigonal planar

d)

bent

124.

The Lewis Dot Structures of two atoms are depicted below. What type of bonding would be seen between these two atoms?

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

No bonds would form

125.

Which of the electron dot structures correctly illustrates diatomic nitrogen with a triple bond?

a)

b)

c)

d)

126.

Based on their Lewis Dot Diagram, which of the following elements is a metal?

a)

b)

c)

d)

127.

Choose the correct Lewis Dot diagram for H2O?

a)

b)

c)

d)

128.

Choose the correct Lewis Dot diagram for KCl.

a)

b)

c)

d)

129.

What is the molecular shape of a CCl4 molecule?

a)

bent

b)

linear

c)

trigonal planar

d)

tetrahedral

130.

How many atoms are in a tetrahedral molecule?

a)

2

b)

3

c)

4

d)

5

131.

Any atom that is electrically neutral must contain —

a)

more protons than electrons

b)

equal numbers of electrons and protons

c)

fewer neutrons than nucleons

d)

equal numbers of nucleons and neutrons

132.

Choose the correct Lewis Dot diagram for CH4?

a)

b)

c)

d)

133.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

134.

Elements in a .................. have similar chemical properties.

a)

period

b)

group

c)

row

135.

Which group of the periodic table is composed of inert (not reactive) gases?

answer choices

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

136.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
137.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
138.

How many protons are in one carbon atom?

a)

1

b)

6

c)

12.01

d)

12

139.

How many electrons are in one carbon atom?

a)

1

b)

6

c)

12.01

d)

12

140.

What is the atomic mass of Neon?

a)

10

b)

20.18

c)

10.18

d)

20

141.
How many protons are in Beryllium?
a)

4

b)

9

c)

5

d)

2

142.

What is the atomic mass of Copper?

a)

63.546

b)

29

c)

29.546

d)

92

143.
How many neutrons are in a Gold atom?
a)

79

b)

196

c)

118

d)

275

144.

How many electrons does a Copper atom have?

a)

63

b)

29

c)

92

d)

34

145.

What is the atomic mass of Gold?

a)

79

b)

196.97

c)

79.97

d)

275

146.

What is the atomic mass of Helium

a)

4.0026

b)

2.0026

c)

4

d)

1

147.

What is the atomic mass of Hydrogen?

a)

1.008

b)

2

c)

1

d)

0

148.

Match the following

a)

Group 18

1.

Noble Gases

b)

Group 1

2.

Alkali Metals

c)

Group 2

3.

Alkaline Earth Metals

d)

Groups 3-12

4.

Transition metals

e)

Group 17

5.

Halogens

149.

Match the following

a)

Elements

1.

Contain only one type of atom

b)

Molecules

2.

at least 2 atoms combined together

c)

Compounds

3.

At least 2 DIFFERENT atoms combined together

d)

Mixture

4.

2 or more substances that are NOT chemically combined

150.

Match the following

a)

Located in the nucleus; have a positive charge; and a mass of 1 amu

1.

Protons

b)

Located outside of the nucleus; have a negative charge; and a mass of 1/2000th of an amu

2.

electrons

c)

located in the nucleus; have no charge; and no charge

3.

neutrons

151.

Elements with similar qualities are located in the same

(a)  

152.

Match the following

a)

Periods

1.

Horizontal rows on the periodic table

b)

Groups

2.

vertical columns on the periodic table

c)

Families

3.

The specific names for the group of elements within a vertical column on the periodic table

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