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Grade 9 Chapter 5 and 6 revision

Total questions: 97

Worksheet time: 4hrs 6mins

Name
Class
Date
1.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
2.
Which has the greater EN: 
N or C?
a)
C
b)
N
3.
Which has the greater EN: 
H or F?
a)
H
b)
F
4.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
5.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
6.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
7.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
8.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
9.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
10.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
11.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
12.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
13.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
14.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
15.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
16.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
17.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

18.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
19.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
20.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
21.

Which property of elements increases across a period of the Periodic Table?

a)

metallic character

b)

number of electron shells

c)

number of outer shell electrons

d)

tendency to form positive ions

22.

Which of the following will have a larger radius than Zinc?

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

23.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

24.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium (He)

b)

Titanium (Ti)

c)

Calcium (Ca)

d)

Magnesium (Mg)

25.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
26.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
27.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
28.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
29.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

30.

A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

a)

chemical reactivity

b)

atomic radius

c)

energy levels

d)

orbit

31.
The core of an atom where most of the mass of an atom exists; contains protons and neutrons
a)
nucleus
b)
electron shell
c)
proton
d)
electron
32.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
33.
A negatively charged subatomic particle that exists in various energy levels outside the nucleus of an atom
a)
neutron
b)
electron
c)
proton
d)
subatomic particle
34.
The chart scientists use to organize and classify all the known elements
a)
elements chart
b)
the chart
c)
Periodic Table of the Elements
d)
Period table
35.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
36.
An electron that resides in the outermost shell, or principal quantum level, of an atom
a)
periodic trend
b)
electron shell
c)
ionic radius
d)
valence electron
37.
Put these in increasing order of atomic radii:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
38.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
39.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
40.
The general trend of metal ion size is that they decrease in size as you move from ______ to ______ on the PT.
a)
Right to left
b)
Left to right
c)
Diagonally
d)
Top to bottom
41.
The general trend of non-metal ion size is that they increase in size as you move from ______ to ______ on the PT.
a)
Left to right
b)
Bottom to top
c)
Top to bottom
42.
What element is the MOST reactive metal on the PT?
a)
Cu
b)
Mn
c)
F
d)
Fr
43.
Which element is a metalloid?
a)
S
b)
Br
c)
As
d)
Au
44.
Noble gases are characterized by...
a)
High reactivity
b)
Being solid at room temperature
c)
Low ionization energy
d)
Full valence shell of electrons
45.
Alkali metals are characterized by their...
a)
Formation of +2 charges
b)
High levels of reactivity
c)
Low melting points
d)
valence electrons in the "p" block
46.
Calcium belongs to which orbital block?  (s, p, d, or f)
a)
s
b)
p
c)
d
d)
f
47.
Metals are good conductors of heat and electricity.
a)
true
b)
false
48.

How does the ionization energy change across a period ?

a)

increases

b)

decreases

c)

stays the same

49.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
50.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
51.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
52.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
53.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
54.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
55.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
56.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
57.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
58.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
59.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
60.

Ability to attract other electrons

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Valence electrons

61.

measures the size of an atom

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Valence Electrons

62.

name this trend

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Valence Electrons

63.

name this trend

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Valence Electrons

64.

name this trend

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Valence Electrons

65.

How did Mendeleev arrange the elements?

a)

alphabetically by element name

b)

density

c)

atomic number

d)

atomic mass

66.

Which group of the periodic table is composed of inert (unreactive) gases?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

67.

Elements which are shiny, conduct electricity and heat are called:

a)

metal

b)

nonmetal

c)

metalloid

d)

radioactive

68.

Which element is not a metal?

a)

Hg

b)

Rh

c)

Al

d)

B

69.

What is on the left side of the dark line on the periodic table?

a)

Non-Metals

b)

Metals

c)

Metalloids

d)

Anions

70.

Which is a halogen?

a)

Helium

b)

Chlorine

c)

Oxygen

d)

Niobium

71.

Which is an alkali metal?

a)

Magnesium

b)

Iron

c)

Sodium

d)

Europium

72.

A horizontal row of elements in the periodic table is called:

a)

column

b)

group

c)

period

d)

family

73.

A vertical column in the periodic table is called:

a)

row

b)

group

c)

period

d)

table

74.

In the modern periodic table elements are arranged by:

a)

valence electrons

b)

atomic number

c)

alphabetical order

d)

atomic mass

75.

How many valance electrons does iodine have?

a)

6

b)

16

c)

7

d)

17

76.

The majority of elements on the periodic table are:

a)

radioactive.

b)

nonmetals.

c)

metals.

d)

gases.

77.

What period and group is arsenic?

a)

Period 3, Group 4A

b)

Period 3, Group 5A

c)

Period 4, Group 5A

d)

Period 4, Group 4A

78.

Metalloids are typically described as:

a)

the same as nonmetals

b)

the same as metals

c)

having characteristics of metals and nonmetals

d)

radioactive

79.

An electron that resides in the outermost shell of an atom is called:

a)

periodic trend

b)

electron shell

c)

ionic radius

d)

valence electron

80.

The group B elements are known as the:

a)

Rare Earth Metals

b)

Transition Metals

c)

Alkaline Earth Metals

d)

Alkali Metals

81.

Which atom has the largest atomic radius?

a)

magnesium

b)

chlorine

c)

barium

d)

selenium

82.

Atoms in the periodic table get bigger when going down a column or group. This is because:

a)

The atoms have more mass.

b)

The atoms have more protons.

c)

The atoms have more energy levels.

d)

The atoms have more neutrons.

83.

As you move across the periodic table atoms tend to get smaller because:

a)

the atoms have more mass.

b)

the atoms have more neutrons.

c)

the atoms have more protons.

d)

the atoms have energy levels.

84.

What is the measure of the size of an atom ( generally defined as the distance from the nucleus to the outermost electron orbit)?

a)

electronegativity

b)

atomic radius

c)

ionization energy

d)

electron affinity

85.

Order the following from smallest to largest atomic radii:

Ra, Be, Ca, Rb, H

a)

Ra, Be, Rb, H, Ca

b)

Rb, H, Ca, Be, Ra

c)

Ra, Rb, Ca, Be, H

d)

H, Be, Ca, Rb, Ra

86.

In the late 1700s, he compiled a list of all elements that were known at the time. The list contained 33 elements organized in four categories.

a)

Antoine Lavoisier

b)

Johann Dobereiner

c)

▪ Alexandre Emile Beguyer de Chancourtois

d)

John Newlands

e)

▪ Dmitri Mendeleev

87.

he suggested that elements be arranged in “octaves” because he noticed (after arranging the elements in order of increasing atomic mass) that certain properties repeated every 8th element.

a)

Antoine Lavoisier

b)

Johann Dobereiner

c)

Alexandre Emile Beguyer de Chancourtois

d)

John Newlands

e)

Dmitri Mendeleev

88.

he organized the elements into a periodic table in order of increasing atomic mass into columns with similar properties,

a)

Antoine Lavoisier

b)

Johann Dobereiner

c)

Alexandre Emile Beguyer de Chancourtois

d)

John Newlands

e)

Dmitri Mendeleev

89.

He rearranged the elements in order of increasing atomic number.

a)

Antoine Lavoisier

b)

Henry Moseley

c)

Alexandre Emile Beguyer de Chancourtois

d)

John Newlands

e)

Dmitri Mendeleev

90.

In the modern periodic table elements are arranged by:

a)

valence electrons

b)

atomic number

c)

alphabetical order

d)

atomic mass

91.

What period and group is Arsenic (As)?

a)

Period 3, Group 14

b)

Period 3, Group 15

c)

Period 4, Group 15

d)

Period 4, Group 14

92.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

93.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

94.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
95.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
96.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

97.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

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