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Chemistry Unit 1&2

Total questions: 137

Worksheet time: 1hrs 22mins

Name
Class
Date
1.

Which of these has a negative charge?

a)

Proton

b)

Neutron

c)

Electron

d)

Oatmeal

2.

Where are electrons found?

a)

Outside the nucleus

b)

Under my bed

c)

Inside the nucleus

d)

Inside a proton

3.

Neutrons have a ____________ charge.

a)

Neutral, or no charge

b)

Positive

c)

Negative

d)

Neutron? I don't know what that is!

4.

What is the smallest unit of matter?

a)

An element

b)

A drop of water

c)

A speck of dust

d)

An atom

5.
Which statement best describes an element?
a)
made from mixture 
b)
thousands in the world
c)

pure, made of only one type of atom

d)
can be separated 
6.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
7.

If an atom has 17 protons, 18 neutrons, and 17 electrons, what is the mass of this atom?

a)

17

b)

18

c)

35

d)

52

8.

A model of a beryllium atom is shown below. What type of particles are found in the cloud surrounding the atom's nucleus?

a)

Positively charge particles and negatively charge particles

b)

negatively charged particles only

c)

neutral particles and positively charge particles

d)

positively charge particles only

9.

What are the subatomic particles?

a)

Protons, Electrons, Neutrons

b)

Molecules, and atoms

c)

Electrons, Protons, Nucleus

d)

Nucleus, and Electrons

10.

What is this subatomic particle that has negative charge?

a)

Electron

b)

Neutron

c)

Proton

d)

Megatron

11.

This particle determines which element it is.

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mrs. Wagner

12.

The image shows the scientific notation of sodium. What is the atomic mass of Na?

a)

(a)11

b)

(b)12

c)

(c)23

d)

(d)34

13.

What is the smallest unit of matter? It is composed of protons and neutrons, held together in the nucleus, and electrons around the nucleus in different electron orbitals, which form an electron cloud.

a)

cell

b)

nucleus

c)

atom

d)

electron

14.

What is a subatomic particle without an electric charge, located in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

15.

What mass does a neutron have?

a)

1 amu

b)

0 amu

c)

-1 amu

d)

+2 amu

16.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

17.
In the Bohr model of the atom, what is the maximum number of electrons in the first shell?
a)
1
b)
2
c)
6
d)
8
18.
The number at the bottom of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element name
19.

Find the element:

Protons: 8

Neutrons: 9

Electrons: 10

a)

Carbon (C)

b)

Oxygen (O)

c)

Hydrogen (H)

d)

Titanium (Ti)

20.
The mass of one proton is equal to the mass of one...
a)
neutron
b)
electron
21.
All of the mass of an atom comes from what location?
a)
nucleus
b)
electron cloud
22.
What is the atomic mass of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
23.
Which of the following best describes the properties of metals?
a)
hard, brittle, and nonconductive
b)
liquid, dark, and conductive
c)
shiny, malleable, and conductive
d)
soft, oily, and very reactive
24.
Each row in the periodic table is called a 
a)
group
b)
period
c)
cluster
d)
unit
25.
Which property of an unknown element determines the other elements it reacts with?
a)
The total number of neutrons of the unknown element
b)
The total number of particles in the nucleus of the unknown element
c)
The number of protons of the unknown element
d)
The number of valence electrons of the unknown element
26.
Which statement best describes an electron?
a)
Smaller mass than a proton and a negative charge
b)
Smaller mass than a proton and a positive charge
c)
Greater mass than a proton and a negative charge
d)
Greater mass than a proton and a positive charge
27.

What is an electron in the outermost energy level that is available to be lost, gained or shared in the formation of a chemical compound

a)

valence electron

b)

cation

c)

anion

d)

proton

28.

a change in the chemical composition and identity of a substance

a)

Physical Change

b)

Chemical Change

c)

Physical and Chemical Change

d)

Matter

29.

a change that alters a substance without changing its chemical composition or its identity

a)

Chemical Change

b)

Physical Change

c)

Chemical and Physical Change

d)

Matter

30.

a physical property that does not depend on the amount of substance present

a)

chemical property

b)

physical property

c)

intensive property

d)

extensive property

31.

a physical property that depends on the amount of matter present

a)

chemical property

b)

physical property

c)

intensive property

d)

extensive property

32.

Color, hardness, malleability, solubility, electrical conductivity, density, melting point, and boiling point are examples of

a)

Physical Properties

b)

Chemical Properties

33.

Reactivity, flammability, and the ability to rust are examples of

a)

Physical Properties

b)

Chemical Properties

34.

He claimed that matter was made of small, hard particles that he called “atomos.”

a)

Democritis

b)

Dalton

c)

Moseley

d)

Einstein

35.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
36.
What is the Element's atomic number?
a)
Fe
b)
26
c)
55.847
d)
Iron
37.
Which state of matter has a fixed shape and volume and it's molecules move very slowly?
a)
Liquid
b)
Gas
c)
Solid
d)
Plasma
38.

Volume is a measurement of:

a)

the amount of particles a substance has.

b)

the space an object occupies

39.

Mass is a measurement of:

a)

the amount of particles a substance has.

b)

the space an object occupies

40.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
41.

Two or more elements chemically combined together are called a

a)

Element

b)

Compound

c)

Mixture

d)

Solution

42.

The simplest natural substance is called a(n)

a)

Element

b)

Compound

c)

Mixture

d)

Solution

43.

What state of matter does this picture show?

a)

Solid

b)

Liquid

c)

Gas

44.

Which state of matter has the highest energy?

a)

solid

b)

liquid

c)

gas

45.

A ___________ is a combination of many different elements not chemically combined.

a)

Element

b)

Compound

c)

Mixture

46.
a)
Element
b)
Compound
c)
Mixture
47.
a)
Element
b)
Compound
c)
Mixture
48.

Combination of two or more different kinds of substances that keep their own physical properties and can be easily separated.

a)

Solution

b)

Mixture

c)

Solubility

d)

Miscibility

49.

This is a type of mixture where one substance dissolves into another

a)

Solution

b)

Miscibility

c)

Compound

d)

Solubility

50.

This is a type of mixture where one substance dissolves into another

a)

Solution

b)

Miscibility

c)

Compound

d)

Solubility

51.

A mixture that appears to be evenly mixed throughout is a(n):

a)

Atom

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

52.

A mixture that does NOT appear to be evenly mixed throughout is a(n)______.

a)

Atom

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

53.
In which state does matter completely fill its closed container?
a)
Gas
b)
Liquid
c)
Solid
d)
Ice
54.
Which state of matter has a fixed shape and volume and it's molecules move very slowly?
a)
Liquid
b)
Gas
c)
Solid
d)
Plasma
55.

How would you find the volume of an irregular shaped object?

a)

use a ruler to measure its dimensions

b)

water displacement

c)

use a balance/scale

d)

use a timer

56.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
57.

5. Photosynthesis

a)

Physical change

b)

Chemical change

58.

Two or more elements chemically combined together are called a

a)

Element

b)

Compound

c)

Mixture

d)

Solution

59.

The simplest natural substance is called a(n)

a)

Element

b)

Compound

c)

Mixture

d)

Solution

60.

What state of matter does this picture show?

a)

Solid

b)

Liquid

c)

Gas

61.

Which state of matter has the lowest energy?

a)

solid

b)

liquid

c)

gas

62.
a)
Element
b)
Compound
c)
Mixture
63.
All of the following processes cause physical changes in matter except
a)
Burning
b)
Melting
c)
Freezing
d)
Boiling
64.
Which of the following indicates a PHYSICAL change?
a)
Change in temperature
b)
Change in shape
c)
Formation of a precipitate
d)
Change in color
65.
Which one of these is a chemical property?
a)
melting point
b)
boiling point
c)
color
d)
flammability
66.

Which process is an example of a physical change?

a)

Ice melting

b)

Milk souring

c)

metal rusting

d)

wood burning

67.

How many valence electrons does Hydrogen have?

a)

1

b)

2

c)

3

d)

4

e)

5

68.

How many valence electrons does Beryllium have?

a)

1

b)

2

c)

3

d)

4

e)

5

69.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

70.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

71.
What do the numbers down the side tell us about the atoms in each row?
a)
number of protons
b)
number of electrons
c)
number of energy levels
d)
absolutely nothing
72.

The------ particle determines the identity of what element you have'

a)

electron

b)

proton

c)

neutron

d)

valence shell

73.
What is the atomic number of the atom pictured? 
a)
11
b)
12
c)
22
d)
23
74.
What is the atomic mass of the atom pictured? 
a)
11
b)
12
c)
22
d)
23
75.

WhIch sub atomic particle vary between isotopes of an element?

a)

protons, electrons, and atomic mass

b)

protons, electrons, and atomic number

c)

neutrons and electrons

d)

neutrons only

76.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
77.
What is the mass number and name of an element with 8 protons and 8 neutrons?
a)
16 - Carbon
b)
16 - Oxygen
c)
24 - Oxygen
d)
8 - Neon
78.
An element with a mass number of 10 and an atomic number of 6 has how many protons?
a)
5
b)
8
c)
6
d)
10
79.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
Electrons and megatrons
80.
In an atom, what is the number of protons equal to?
a)
The number of electrons.
b)
The number of neutrons.
c)
The number of molecules.
d)
The number of nuclei.
81.

The particles in atoms (protons, neutrons and electrons) are weighed in 'amu'. What does 'amu' stand for?

a)

Australian Macintosh Users

b)

Atomic Mass Units

c)

Andy's Maddening Ulcer

d)

Atomic Mega Ultras

82.

The mass number of an atom is equal to...

a)

Protons + Electrons

b)

Electrons + Neutrons

c)

Neutrons + Neutrons

d)

Protons + Neutrons

83.

What is the mass number of this Carbon atom?

a)

12

b)

6

c)

C

84.

What is the atomic number of this Carbon atom?

a)

12

b)

6

c)

C

85.

How many protons does this Carbon atom have?

a)

12

b)

6

c)

C

86.

How many neutrons does this Carbon atom have?

a)

12

b)

6

c)

18

87.

How are you finding chemistry so far?

a)

I'm finding it very challenging right now.

b)

It's a bit tricky but I will try to keep up.

c)

I have a few questions but overall it's OK.

d)

I'm getting it and could probably help other students who aren't getting it.

88.

What subatomic particles are coloured green in this image?

a)

protons

b)

neutrons

c)

electrons

89.

What two subatomic particles have approximately the same mass?

a)

electrons & neutrons

b)

protons & electrons

c)

neutrons & protons

90.

How would you calculate the number of neutrons in an atom?

a)

Atomic Number MINUS Atomic Mass

b)

Atomic Mass PLUS Atomic Number

c)

Atomic Mass MINUS Atomic Number

d)

Atomic Number PLUS Atomic Mass

91.

Use your periodic table to determine the number of Neutrons that Nitrogen has in its nucleus.

a)

6

b)

7

c)

8

d)

9

92.

Rate your understanding of Neutrons and Isotopes...

a)

Excellent

b)

Getting there!

c)

Developing

d)

Needs attention

e)

Poor

93.

find the number of neutrons in Cromo

a)

38

b)

18

c)

28

94.

find the numbers of neutrons of oxygen

a)

5

b)

8

c)

16

95.
What is the formula to solve for the neutron?
a)
Mass + Atomic Number= Neutrons
b)
Mass x Atomic Number = Neutrons
c)
Mass - Atomic Number = Neutrons
d)
Mass + Number of Protons = Neutron
96.
What is the charge of the neutron?
a)
Negative
b)
Positive
c)
electrical charge
d)
Neutral (no charge)
97.
An atom has 5 protons, 6 neutrons, and 5 electrons. What is the charge of the atom's nucleus?
a)
-5
b)
+6
c)
+5
d)
-6
98.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
99.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
5
100.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
101.
How is carbon-12 different from carbon-14?
a)
They have a different number of protons
b)
they have a different number of electrons
c)
they have a different number of neutrons
102.

The difference between a chemical and physical change is that...

a)

A chemical change makes a new substance and a physical change doesn't

b)

A physical change makes a new substance and a chemical change doesn't

c)

There is no difference between a chemical and physical change

d)

A chemical change makes something new and a physical change can only be measured microsopically

103.
What can you conclude about carbon-14 from its name?
a)
It has 14 electrons
b)
it has 14 neutrons
c)
it has 14 protons
d)
it has an atomic mass of 14 u
104.

What differentiates the isotopes of an element?

a)

number of protons

b)

number of neutrons

c)

number of electrons

d)

atomic number

105.

Using the atomic masses and relative abundance of the isotopes of nitrogen given below, determine the average atomic mass of nitrogen.

N-14: 14.003 amu; 99.63% N-15: 15.000 amu; 0.37%

a)

14.003 amu

b)

14.007 amu

c)

14.506 amu

d)

15.000 amu

106.

Element A has 15 protons. Determine the number of neutrons in its isotope with mass number 33.

a)

15

b)

18

c)

33

d)

48

107.

The atomic mass of an element depends upon the ___.

a)

relative abundance of protons in that element

b)

mass and relative abundance of each isotope of that element

c)

mass of each isotope of that element

d)

mass of each electron in that element

108.

The atomic mass of an element is the ___.

a)

average of the mass number and the atomic number for the element

b)

weighted average of the masses of the isotopes of the element

c)

total mass of the isotopes of the element

d)

total number of subatomic particles in the nucleus

109.

What does the 1.0079 stand for?

a)

atomic number

b)

hydrogen

c)

atomic mass

d)

mass number

110.

Select the element with the largest atomic radius

a)

Potassium

b)

Scandium

c)

Gallium

d)

Arsenic

111.

Select the element most likely to gain an electron

a)

Bromine

b)

Fluorine

c)

Chlorine

d)

Iodine

112.

Select the sequence that correctly orders from smallest to largest atomic radius

a)

Sn, Y, Ru

b)

Cu, Ga, Br

c)

Al, S, Na

d)

F, N, Li

113.

Select the group that is the most reactive metals

a)

Transition Metals

b)

Alkali Earth Metals

c)

Alkali Metals

d)

Halogens

114.

Select the element with the highest ionization energy

a)

Sodium

b)

Aluminum

c)

Phosphorous

d)

Chlorine

115.

Select the element Alkali Earth Metal found in Period 4

a)

Calcium

b)

Potassium

c)

Titantium

d)

Krypton

116.

Select the element below that is least reactive

a)

Hydrogen

b)

Chlorine

c)

Lithium

d)

Neon

117.

Select the element that is a metalloid

a)

Gallium

b)

Boron

c)

Oxygen

d)

Magnesium

118.

Select the element that has 3 valence electrons

a)

Calcium

b)

Sodium

c)

Aluminum

d)

Sulfur

119.

What element is found in Group 5 period 4?

a)

Zirconium

b)

Magnesium

c)

Strontium

d)

Vanadium

120.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

121.

Which element is most likely to lose an electron?

a)

Zinc

b)

Arsenic

c)

Bromine

d)

Potassium

122.
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
123.
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
124.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

125.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

126.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

127.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

128.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

129.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

130.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
131.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
132.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
133.

Ions are formed when atoms gain or lose ___.

a)

electrons

b)

protons

c)

neutrons

d)

atomic mass

134.

Which element in period 4 has the highest electronegativity?

a)

potassium

b)

calcium

c)

copper

d)

bromine

135.

The common charge on an atom in group 17 would be....

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

136.

What type of elements are poor conductors of heat and electricity?

a)

transition metals

b)

inner transition metals

c)

metals

d)

nonmetals

137.

What type of elements are malleable and ductile?

a)

noble gases

b)

nonmetals

c)

metals

d)

halogens

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