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Classification of Matter Quiz

Total questions: 136

Worksheet time: 7hrs 19mins

Name
Class
Date
1.

What is a mixture that has a uniform composition called?

a)

Heterogeneous Mixture

b)

Homogeneous Mixture

c)

Compound

d)

Element

2.

Which type of matter cannot be physically separated?

a)

Mixture

b)

Pure Substance

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

3.

What is an example of a compound?

a)

NaCl (s)

b)

Soil

c)

Mg

d)

H₂

4.

Which of the following is an element?

a)

NaCl (aq)

b)

Soil

c)

Mg

d)

NaCl (s)

5.

What is an example of a diatomic molecule?

a)

Mg

b)

H₂

c)

Na

d)

Al

6.

How many diatomic molecules are there according to the periodic table diagram?

a)

5

b)

6

c)

7

d)

8

7.

Which element is atomic number 1?

a)

Nitrogen

b)

Oxygen

c)

Hydrogen

d)

Helium

8.

Which group of atoms forms a "seven" on the periodic table?

a)

N, O, F, Cl, Br, I

b)

H, He, Li, Be, B

c)

C, N, O, F, Ne

d)

Na, Mg, Al, Si, P

9.

What do compounds contain?

a)

Only one type of element

b)

Two or more different elements chemically combined

c)

Only metals

d)

Only non-metals

10.

What is a mixture?

a)

A single element

b)

A compound chemically combined

c)

Two or more different substances not chemically combined

d)

A single compound

11.

Which of the following is an example of a mixture?

a)

H2O

b)

NaCl

c)

Mg & Zn & NaCl

d)

CO2

12.

What does filtration physically separate?

a)

Soluble solid from a liquid

b)

Insoluble solid from a liquid or aqueous solution

c)

Gas from a liquid

d)

Liquid from another liquid

13.

Which of the following is an example of filtration?

a)

Mixing salt and water

b)

Separating sand from salt water

c)

Dissolving sugar in water

d)

Boiling water

14.

What is the process called that physically separates two or more liquids based on their boiling points?

a)

Filtration

b)

Distillation

c)

Evaporation

d)

Sedimentation

15.

What is the process called when a solid turns into a gas without passing through the liquid phase?

a)

Melting

b)

Freezing

c)

Sublimation

d)

Condensation

16.

Which phase of matter has a definite volume but takes the shape of its container?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

17.

What type of process is boiling, where heat is added to change a liquid into a gas?

a)

Exothermic

b)

Endothermic

c)

Isothermal

d)

Adiabatic

18.

In which phase of matter are particles in constant motion and have an indefinite volume?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

19.

What is a physical change?

a)

A change that alters the chemical properties of a substance

b)

A change that does not change the chemical properties of a substance

c)

A change that creates a new substance

d)

A change that only occurs at high temperatures

20.

Which of the following is an example of a physical change?

a)

Burning wood

b)

Rusting iron

c)

Melting ice

d)

Baking a cake

21.

Which process is NOT a phase change?

a)

Boiling

b)

Cutting

c)

Freezing

d)

Melting

22.

What is a chemical change?

a)

A reaction where a new substance is formed

b)

A reaction where no new substance is formed

c)

A physical change in appearance

d)

A change in temperature only

23.

Which of the following is an example of a chemical change?

a)

Melting

b)

Freezing

c)

Rusting

d)

Boiling

24.

Which process involves the formation of a new substance?

a)

Evaporating

b)

Burning

c)

Dissolving

d)

Cutting

25.

When counting significant figures, where should you start?

a)

At the first zero

b)

At the first nonzero digit

c)

At the last digit

d)

At the decimal point

26.

How many significant figures does the number 3006 have?

a)

2

b)

3

c)

4

d)

5

27.

When are zeros trailing after the last nonzero digit considered significant?

a)

Always

b)

Only if a decimal point is present

c)

Never

d)

Only if they are between nonzero digits

28.

When multiplying or dividing numbers, to how many significant figures should you round the answer?

a)

The greatest number of significant figures in any of the numbers

b)

The least number of significant figures in any of the numbers

c)

The average number of significant figures in the numbers

d)

The total number of significant figures in all the numbers combined

29.

What is the freezing/melting point of water in degrees Celsius?

a)

0°C

b)

100°C

c)

273°C

d)

-273°C

30.

What is the boiling/condensation point of water in degrees Celsius?

a)

0°C

b)

100°C

c)

273°C

d)

-273°C

31.

What is the formula to convert Kelvin to Celsius?

a)

K = °C + 273

b)

°C = K + 273

c)

K = °C - 273

d)

°C = K - 273

32.

If an object is 150 K, what is its temperature in Celsius?

a)

-123°C

b)

123°C

c)

-150°C

d)

150°C

33.

What is the formula for calculating density?

a)

Density = Mass x Volume

b)

Density = Mass / Volume

c)

Density = Volume / Mass

d)

Density = Mass + Volume

34.

If an object has a density of 0.3456 g/cm³ and a volume of 112.4 cm³, what is its mass?

a)

38.85 g

b)

32.45 g

c)

40.12 g

d)

35.67 g

35.

What is the mass of an aluminum sample with a volume of 251 cm³ and a density of 2.70 g/cm³?

a)

678 g

b)

500 g

c)

700 g

d)

600 g

36.

According to Table S, what is the density of aluminum?

a)

2.70 g/cm³

b)

1.74 g/cm³

c)

0.97 g/cm³

d)

2.34 g/cm³

37.

What is the formula for calculating percent error?

a)

% error = (measured value + accepted value) / accepted value x 100

b)

% error = (measured value - accepted value) / accepted value x 100

c)

% error = (measured value x accepted value) / accepted value x 100

d)

% error = (measured value / accepted value) x 100

38.

A student measures the mass of a sample as 48.9 grams and the volume as 5.00 cubic centimeters. What is the calculated density of the sample?

a)

9.18 g/cm³

b)

8.96 g/cm³

c)

10.00 g/cm³

d)

7.50 g/cm³

39.

What is the percent error of the student's calculated density?

a)

2.46%

b)

5.00%

c)

1.50%

d)

3.00%

40.

What is the direction of heat flow?

a)

Cold to hot

b)

Hot to cold

c)

Upward

d)

Downward

41.

What does average kinetic energy represent?

a)

Pressure

b)

Volume

c)

Temperature

d)

Mass

42.

What is the characteristic of liquids in terms of shape and volume?

a)

Definite shape and volume

b)

Definite volume, takes shape of container

c)

No definite shape or volume

d)

Expands indefinitely

43.

Which radioactive particle has this symbol?

a)

Alpha

b)

Beta

c)

Gamma

d)

Nuclear

44.

What is the name of this isotope?

a)

Magnesium

b)

Magnesium-22

c)

Magnesium-12

d)

Magnesium-10

45.

How many protons are in the nucleus of this isotope?

a)

22

b)

12

c)

34

d)

10

46.

How many neutrons are in the nucleus of this isotope?

a)

22

b)

12

c)

34

d)

10

47.

What number belongs in the blank?

a)

9

b)

2

c)

17

d)

0

48.

Which type of nuclear reaction splits a large unstable nucleus into smaller ones?

a)

Fission

b)

Fusion

49.

Which type of nuclear reaction combines smaller particles into a larger one?

a)

Fission

b)

Fusion

50.

A beta particle is also called _____.

a)

an isotope

b)

a mass number

c)

an electron

d)

a fusion

51.

What type of decay is shown in this equation?

a)

alpha decay

b)

beta decay

c)

gamma emission

52.

What particle completes this reaction?

a)
b)
c)
d)
53.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
54.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
55.
What is the missing isotope that will balance the following nuclear equation?
94Be  +  11H →  _____  +  42He
a)
105B
b)
105Ne
c)
63Li
d)
63C
56.
 Which statement describes particles of an ideal gas, based on the kinetic molecular theory? 
a)
Gas particles are separated by distances smaller than the size of the gas particles.
b)
Gas particles do not transfer energy to each other when they collide.
c)
Gas particles have no attractive forces between them. 
d)
Gas particles move in predictable, circular motion.
57.
Which electron configuration represents an excited state for an atom of calcium? 
a)
2-8-7-1
b)
2-8-7-2
c)
2-8-7-3
d)
2-8-8-2
58.

Which list of symbols represents nonmetals, only?

a)

B, Al, Ga

b)

Li, Be, B

c)

C, Si, Ge

d)

P, S, Cl

59.
Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right? 
a)
Both electronegativity and atomic radius increase.
b)
Both electronegativity and atomic radius decrease. 
c)
Electronegativity increases and atomic radius decreases.
d)
Electronegativity decreases and atomic radius increases.
60.
What is the total amount of heat required to completely melt 347 grams of ice at its melting point? 
a)
334 J
b)
1450 J
c)
116000 J
d)
784000 J
61.
What is the charge of the nucleus of an oxygen atom?
a)
0
b)
-2
c)
+8
d)
+16
62.
Which Lewis electron-dot diagram represents a nitrogen atom in the ground state?
a)
1
b)
2
c)
3
d)
4
63.
What is the most likely electronegativity value for a metallic element?
a)
1.3
b)
2.7
c)
3.4
d)
4
64.
Every chlorine atom has
a)
7 electrons
b)
17 neutrons
c)
a mass number of 35
d)
an atomic number of 17
65.
Which substance can not be broken down by a chemical change?
a)
ammonia
b)
methanol
c)
propane
d)
phosphorus
66.

At standard pressure and temperature, what will be the physical state of bromine?

a)

liquid

b)

gas

c)

solid

d)

plasma

67.
Which property can be defined as the ability of a substance to be hammered into thin sheets?
a)
conductivity
b)
malleability
c)
melting point
d)
solubility
68.
Which list of elements consists of a metal, a metalloid, and a noble gas?
a)
aluminum, sulfur, argon
b)
magnesium, sodium, sulfur
c)
 sodium, silicon, argon
d)
silicon, phosphorus, chlorine
69.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

70.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
71.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
72.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
73.
Which two subatomic particles make up the nucleus of an atom?
a)
Protons and Electrons
b)
Neutrons and Electrons
c)
Electrons and Protons
d)
Protons and Neutrons
74.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
75.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
76.
Where is most of the mass in an atom located?
a)
in the nucleus
b)
in the protons
c)
in the neutrons
d)
in the electrons
77.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

78.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

79.

What is the difference between Neon-20 and Neon-22?

a)

They have different numbers of electrons.

b)

They have different numbers of neutrons.

c)

Only 1 is radioactive.

d)

No difference.

80.

Which is the correct symbol for Fluorine-18?

a)
b)
c)
d)
81.

How many protons are in this isotope?

a)

9

b)

21

c)

12

82.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

83.

During a flame test, sodium chloride produces an intense yellow flame. This yellow color is produced when electrons in excited atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

move to lower energy states within the atoms

84.

An atom that has 8 protons and 10 neutrons is an isotope of the element

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

85.

Which electron configuration represents the atoms of a bromine atom in the excited state?

a)

2-8-18-7

b)

2-8-18-8

c)

2-8-17-8

d)

2-8-18-7-1

86.

Under which conditions does a gas behave least like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and low pressure

d)

low temperature and high pressure

87.
The mass of a proton is approximately equal to the mass of
a)
an alpha particle
b)
a beta particle
c)
a neutron
d)
a positron
88.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

89.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

90.
The most dangerous type of radiation is the ____. 
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
91.

What is the charge of a neutron?

a)

+1

b)

-1

c)

0

d)

+2

92.

Which scientist is known for the discovery of the nucleus?

a)

Bohr

b)

Rutherford

c)

Thomson

d)

Dalton

93.

Which term represents the strength of the attraction an

atom has for the electrons in a chemical bond?

a)

electrical conductivity

b)

electronegativity

c)

first ionization energy

d)

specific heat capacity

94.

Which term represents the amount of energy required

to remove the most loosely bound electron from an

atom in the gaseous state?

a)

atomic radius

b)

electronegativity

c)

First ionization energy

d)

electrical conductivity

95.

As the elements in Period 2 of the Periodic Table are

considered in order from left to right, which property

generally decreases?

a)

atomic radius

b)

electronegativity

c)

ionization energy

d)

nuclear charge

96.

Which sequence correctly places the elements in order

of increasing ionization energy?

a)

H -> Li -> Na -> K

b)

I -> Br -> Cl -> F

c)

O -> S -> Se -> Te

d)

H -> Be -> Al -> Ga

97.

In a given period of the Periodic Table, the element

with the lowest first ionization energy is always in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

98.

Which of these elements has physical and chemical

properties most similar to silicon (Si)?

a)

germanium (Ge)

b)

lead (Pb)

c)

phosphorus (P)

d)

chlorine (Cl)

99.

As the atomic number of elements within Group 2

increases, the metallic character of each successive

element

a)

decreases

b)

increases

c)

remains the same

100.

Which atom has the greatest attraction for the

electrons in a chemical bond?

a)

hydrogen

b)

oxygen

c)

silicon

d)

sulfur

101.

Which element is a noble gas?

a)

Argon

b)

chlorine

c)

hydrogen

d)

magnesium

102.

An atom of which element has the largest atomic

radius?

a)

Fe

b)

Mg

c)

Si

d)

Zn

103.
A nuclear reaction where a nucleus splits into two smaller nuclei is... 
a)
Fission
b)
Fusion
c)
Gamma decay
d)
Beta decay
104.
What would two different isotopes of an atom have in common?
a)
Number of neutrons 
b)
Number of protons
c)
Atomic weight 
d)
Atomic mass
105.
What happens when the number of protons in an atom changes? 
a)
The number of electrons changes too 
b)
Usually nothing happens, unless the atom is radioactive 
c)
The atomic nucleus explodes
d)
It becomes a completely different atom, with different properties 
106.
When nuclei decay, massive amounts of __________ is released.
a)
energy
b)
jello
c)
protons
d)
neutrons
107.

Which list of symbols represents nonmetals, only?

a)

B, Al, Ga

b)

Li, Be, B

c)

C, Si, Ge

d)

P, S, Cl

108.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
109.
According to the Combined Gas Law, pressure and volume are inversely related which means that
a)
When pressure increases, volume increases
b)
When pressure decreases, volume decreases
c)
When pressure increases, volume decreases
d)
When pressure doubles, volume triples
110.
According to the Combined Gas Law, volume and temperature are directly related. This means that
a)
When volume increases, temperature increases
b)
When volume increases, temperature decreases
c)
When volume double, pressure triples
d)
When volume doubles, volume is reduced by 1/2
111.
If 6L of gas at 293K is compressed to 4L, what is the new temperature? 
a)
195K
b)
439.5K
c)
0.082K
d)
12.2K
112.
4L of a gas is contained at 300 kPa and 200K. What will its volume be in L at 140 kPa and 100K?
a)
4.3L
b)
4.8L
c)
6.2L
d)
8.5L
113.

A student measures the mass and volume of a sample of aluminum at room temperature, and calculates the density of Al to be 2.85 grams per cubic centimeter. Based on Table S in the Chemistry Reference Table, what is the percent error for the student's calculated density of Al?

a)

2.7%

b)

5.3%

c)

5.6%

d)

95%

114.

A phase change is a...

a)

physical change

b)

chemical change

115.

During which phase change does a substance absorb energy?

a)

freezing

b)

condensation

c)

evaporation

d)

deposition

116.

During which phase change does a substance release energy?

a)

condensation

b)

evaporation

c)

melting

d)

sublimation

117.

Which phase change is endothermic?

a)

condensation

b)

deposition

c)

melting

d)

freezing

118.

Which phase change is exothermic?

a)

sublimation

b)

evaporation

c)

melting

d)

freezing

119.

What is happening to the kinetic energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

120.

What is happening to the potential energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

121.

What is happening to the kinetic energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

122.

What is happening to the potential energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

123.

At what time interval is the substance melting?

a)

AB

b)

BC

c)

CD

d)

DE

124.

At what time interval is the substance evaporating?

a)

AB

b)

BC

c)

CD

d)

DE

125.

When temperature increases, kinetic energy...

a)

increases

b)

decreases

c)

stays constant

126.

Which particle diagram shows a solid?

a)
b)
c)
127.

Which particle diagram shows a liquid?

a)
b)
c)
128.

Which particle diagram shows a gas?

a)
b)
c)
129.

Which formula would you use to calculate the heat absorbed when ice is melted at its melting point?

a)
b)
c)
130.

Which formula would you use to calculate the heat absorbed when water is heated from 10°C to 20 °C?

a)
b)
c)
131.

Which formula would you use to calculate the heat absorbed when water is boiled at 100°C?

a)
b)
c)
132.

Which formula would you use to calculate the heat released when water is frozen at 0°C?

a)
b)
c)
133.

Which formula would you use to calculate the heat released when water vapor condenses to a liquid?

a)
b)
c)
134.

How much heat is released when 20.0 grams of water is cooled from 65°C to 55°C?

a)

300 J

b)

836 J

c)

6,680 J

d)

10,800 J

135.

What is the total number of joules released when a 10.00-gram sample of water changes from liquid to solid at 0°C?

a)

4.18 x 103 J

b)

3.34 x 103 J

c)

2.26 x 103 J

d)

2.73 x 103 J

136.

The temperature of a sample of water changes from 55°C to 77°C when the sample absorbs 1,103.5 joules of heat. What is the mass of the sample?

a)

7 grams

b)

12 grams

c)

50 grams

d)

72 grams

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