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Atoms, Elements, Ions, Isotopes

Total questions: 94

Worksheet time: 1hrs 3mins

Name
Class
Date
1.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
2.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
3.

How many electrons do the alkali metals have in their outer shell?

a)

1

b)

2

c)

8

d)

7

4.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

5.

Which gas is released when the alkali metals react with water?

a)

hydrogen

b)

oxygen

c)

hydroxide

d)

carbon dioxide

6.

What happens to the shielding affect as you go down the group?

a)

increases

b)

decreases

7.
True or False - Protons and Neutrons have about the same mass.
a)
True - They have about the same mass
b)
False - They do not have about the same mass
8.

Which scientist described a positively charged core (“nucleus”) in the middle of a lot of empty space?

a)

Chadwick

b)

Thomson

c)

Rutherford

d)

Bohr

9.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

10.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

11.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

12.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

13.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

14.

Which of the following is true for ionic bonding & ionic compounds? (3 correct statements)

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

15.

Which properties are all characteristics of ionic compounds?

a)

solids with high melting and boiling points

b)

soft solids which are highly malleable

c)

when solid, the ions are held in place so the compounds cannot conduct electricity

d)

conduct electricity when dissolved or molten

16.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting point and it conducts electricity when molten or dissolved

c)

A high boiling point and it conducts electricity when solid

17.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

18.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

19.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds which require a large amount of heat energy to overcome these strong bonds.

d)

They have weak bonds which require a little amount of heat energy to overcome these weak bonds.

20.

Which three of the following are features of ionic compounds? (click 3 boxes)

a)

They have bonds between metals and non-metals.

b)

They have bonds between two non-metals.

c)

They form simple molecular structures.

d)

They form giant ionic lattices.

e)

They involve the transfer of electrons.

21.

Be and F can combine to form BeF2, an ionic compound. Select ALL the true statements.

a)

Each Be atom loses two electrons from the outer shell.

b)

Each F atom gains two electrons from Be.

c)

The force holding the ionic compound together is electrostatic attraction.

d)

Each F ion has a charge of -1

22.

Select all the true statements:

a)

Each outer shell electron in Cl is represented by a cross.

b)

In Na, the total charge is -2.

c)

Na+ and Cl- are held together by electrostatic attraction.

d)

Na+ has a full outer shell of electrons.

23.

A single crystal of table salt (Sodium Chloride) is one giant ionic lattice, the Na+ and Cl- ions are held together in a (a)   lattice.

24.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

25.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

26.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

27.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

28.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
29.

Sodium Oxide is Na2O. Meaning there are 2 Na present for every O in the ionic compound. As the Oxygen ion has a charge of -2, what charge does each Sodium ion have?

a)

-1

b)

-2

c)

+2

d)

+1

30.

What is the correct formula for aluminium oxide? Aluminium is in group 3 and oxygen is in group 6.

a)

Al₂O₃

b)

AlO

c)

AlO₄

d)

Al₂O

e)

Al₃O₂

31.

Which Halogen has the lowest melting point?

a)

Fluorine

b)

Bromine

c)

Iodine

d)

Chlorine

32.

In an atom, there are three types of subatomic particles. ______ are positively charged, ______ are negatively charged, and ______ are neutral.

a)

Protons, Electrons, Neutrons

b)

Electrons, Protons, Neutrons

c)

Neutrons, Protons, Electrons

d)

Electrons, Neutrons, Protons

33.

The atomic number tells the number of ______ in an atom, which never changes.

a)

Protons

b)

Neutrons

c)

Electrons

34.

_______ is the average mass of all the isotopes of an element.

a)

Atomic Mass

b)

Atomic Number

c)

Chemical Symbol

d)

Element Name

35.

An atom of an element with a different number of neutrons and therefore a different atomic mass

a)

Isotope

b)

Ion

c)

Atom

d)

Particle

36.

Isotopes are atoms of the same element with different ____________.

a)

Number of Neutrons & Mass Number

b)

Number of Protons & Atomic Number

c)

Number of Protons, Neutrons, and Electrons

d)

Number of Electrons & Mass Number

37.

What is the ATOMIC MASS of the isotope Carbon-14?

a)

14

b)

6

c)

12

d)

20

38.

Carbon-14 has ____ protons, ____ electrons, and _____ neutrons.

a)

6, 6, 8

b)

6, 6, 6

c)

6, 6, 14

d)

6, 10, 14

39.

Isotopes of the same element have the same number of ________ but a different number of _______.

a)

protons, neutrons

b)

neutrons, protons

c)

protons, electrons

d)

electrons, neutrons

40.

An atom of phosphorus has an atomic number of 15 and a mass number of 31. How many neutrons does it contain?

a)

15

b)

16

c)

31

d)

46

41.

The identity of a chemical element is always determined by which of the following?

a)

the number of protons it has

b)

the number of neutrons it has

c)

the number of electrons it has

42.

By studying the picture, you can determine that Carbon-13 has ____ protons.

a)

6

b)

13

c)

12

d)

14

43.

Using the picture, you can determine that Carbon-13 has ____ neutrons.

a)

13

b)

6

c)

12

d)

7

44.

Atomic Mass is...

a)

protons + neutrons

b)

neutrons + electrons

c)

protons + electrons

45.

An element's atomic number _______ changes.

a)

always

b)

sometimes

c)

never

46.

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

a)

Protons

b)

Neutrons

c)

Electrons

47.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

48.

9 protons and 9 neutrons

a)

Fluorine-18

b)

Fluorine-9

c)

Fluorine-16

d)

Fluorine-18.998

49.
The photo above shows the isotopic notation for which isotope?
a)
Carbon 12
b)
Carbon 13
c)
Carbon 14
d)
Carbon 15
50.

What is the atomic mass of the pictured isotope?

a)

2

b)

4

c)

6

51.

What is the name of the pictured isotope?

a)

Chlorine-18

b)

Chlorine-17

c)

Chlorine-35

52.

What is the name of the pictured isotope?

a)

Copper-29

b)

Copper-63

c)

Copper-34

53.
Two isotopes of carbon are carbon-12 and carbon-14.  These isotopes differ from one another by two protons.
a)
true
b)
false
54.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
55.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
56.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
57.
Found in the nucleus of the atom
a)
electrons only
b)
protons only
c)
neutrons and protons
d)
neutrons and electrons
58.
An element is defined by its number of 
a)
protons
b)
electrons
c)
neutrons
d)
protons + electrons
59.
Which of the subatomic particles is the lightest
a)
all have the same mass
b)
protons 
c)
neutrons 
d)
electrons
60.
Which of the subatomic particles is the heaviest?
a)
electrons 
b)
protons 
c)
neutrons 
d)
protons and neutrons have equal mass
61.
An atom with atomic number 6 would have how many protons?
a)
6
b)
12
c)
3
d)
cannot be determined 
62.
Most of an atom's mass is found in the
a)
electrons.
b)
nucleus.
63.

If a hydrogen atom has 1 proton, 1 electron, and 1 neutron, its mass number is ....

a)

1

b)

2

c)

3

d)

0

64.

How many neutrons are in an atom of carbon-14?

a)

6

b)

8

c)

10

d)

14

65.

How many protons does this isotope of titanium have?

a)

22

b)

26

c)

48

d)

70

66.

How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?

a)

2

b)

34

c)

36

d)

40

67.

Write the hyphen notation for the isotope that has 39 protons and 50 neutrons.

a)

Yttrium-11

b)

Tin-39

c)

Tin-89

d)

Yttrium-89

68.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
69.

Chromium has four naturally occurring isotopes (chromium-50, chromium-52, chromium-53, and chromium-54). What is the average atomic mass of Chromium?

a)

4

b)

51.996

c)

52.25

d)

Not enough information was given.

70.

An element has three isotopes. Given the abundances and relative masses, calculate the average atomic mass and determine (from the periodic table) which element it is.


Abundances | Relative masses

0.005% | 234.04 amu

0.720% | 235.04 amu

99.275% | 238.05 amu

a)

Uranium (#92, Atomic Mass: 238.03 amu)

b)

Fluorine (#9, Atomic Mass: 19.00 amu)

c)

Mercury (#89, Atomic Mass: 200.59 amu)

d)

Polonium (#84 209 amu)

71.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
72.

Rubidium has two naturally occurring isotopes, 85Rb (relative mass 84.9118 amu) and 87Rb (relative mass 86.9092 amu). The abundance of 87Rb is 27.8%, If rubidium has an average atomic mass of 85.47 amu, what is the % abundance of 85Rb (in percent)?

a)

27.9%

b)

72.1%

c)

74.63%

d)

34.29%

73.
What is the name of the pictured isotope?
a)
Carbon-12
b)
Carbon-13
c)
Carbon-14
d)
Carbon-15
74.

What element has the symbol K?

a)

Potassium

b)

Argon

c)

Copper

d)

Iron

75.

What element has the symbol K?

a)

Potassium

b)

Argon

c)

Copper

d)

Iron

76.

What element has the symbol Ca?

a)

Cadmium

b)

Carbon

c)

Mg

d)

Calcium

77.

What element has the symbol Ti?

a)

Helium

b)

Boron

c)

Aluminium

d)

Titanium

78.

What element has the symbol C?

a)

Cadmium

b)

Chromium

c)

Carbon

d)

Calcium

79.

What element has the symbol Be?

a)

Phosphorous

b)

Tin

c)

Boron

d)

Beryllium

80.

What element has the symbol N?

a)

Sodium

b)

Nitrogen

c)

Silicon

d)

Neon

81.

What element has the symbol Na?

a)

Nitrogen

b)

Helium

c)

Sodium

d)

Beryillium

82.

What symbol does Lithium?

a)

Li

b)

Na

c)

Si

d)

L

83.

What symbol does Magnesium have?

a)

Mg

b)

Na

c)

M

d)

Mo

84.

What symbol does hydrogen have?

a)

H

b)

He

c)

Hy

d)

Hi

85.

What symbol does Silicon have?

a)

S

b)

Sy

c)

Si

d)

St

86.

What symbol does sulfur have?

a)

Si

b)

S

c)

Ti

d)

D

87.

What symbol does Argon have?

a)

Ar

b)

A

c)

O

d)

N

88.

What symbol does Oxygen have?

a)

O2

b)

O

c)

No

d)

Ox

89.

What symbol does Neon have?

a)

N

b)

No

c)

Ne

d)

Ni

90.

If an atom has 22 protons and a mass number of 48, how may neutrons does it have?

a)

70

b)

22

c)

48

d)

26

91.

If an element has a mass number of 24 and 12 neutrons, how many protons does it have?

a)

24

b)

36

c)

12

d)

6

92.

If a stable atom has 10 protons, how many electrons does it have?

a)

5

b)

10

c)

15

d)

20

93.

Calcium has 20 electrons, what is its electron configuration?

a)

2, 8, 8, 2

b)

4, 8, 8

c)

2, 10, 8

d)

2, 8, 10

94.

Aluminium has 13 protons. What is its electron configuration?

a)

2, 8, 2, 1

b)

2, 10, 1

c)

2, 8, 3

d)

3, 10

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