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G9 Quiz 2 Revision

Total questions: 191

Worksheet time: 3hrs 44mins

Name
Class
Date
1.

Rows on the periodic table are called...

a)

groups

b)

periods

c)

families

d)

shells

2.
How many PERIODS does the Periodic Table have?
a)
1
b)
7
c)
8
d)
18
3.
How many GROUPS does the Periodic Table have? 
a)
1
b)
5
c)
7
d)
18
4.
Which FAMILY  does Mercury belong to?
a)
Halogens
b)
Kardashians
c)
Transition Metals
d)
Alkali Metals
5.
Which FAMILY does Chlorine belong to?
a)
Alkali Earth Metals
b)
Halogens
c)
Noble Gases
d)
Jackson
6.
Is Plutonium artificially made?
a)
Yes
b)
No
c)
Maybe?
7.
Is Fluorine a solid, liquid or gas at room temperature? 
a)
Solid
b)
Liquid
c)
Gas
8.
Is Oxygen a Metal or Non-Metal? 
a)
Metal
b)
Non-metal
9.
Which PERIOD does Radon belong to? 
a)
18
b)
8
c)
6
d)
1
10.
Element from Period #2, Group #1?
a)
Lithium
b)
Beryllium 
c)
Helium 
d)
Lead
11.
Element from Group #17, Period #2?
a)
Fluorine
b)
Chlorine 
c)
Hydrogen
d)
Iodine
12.
Which of the element's listed is naturally RADIOACTIVE???
a)
Bismuth
b)
Aluminum
c)
Iron 
d)
Cesium
13.
How many NEUTRONS does Zinc have, MAN???
a)
35
b)
0
c)
30
d)
65
14.
How many PROTONS does Copper have? 
a)
27
b)
29
c)
0
d)
63.546
15.
Which way do PERIODS go? 
a)
Horizontally
b)
Verically
c)
Zig-zaggy
d)
Catty-wompus 
16.
What does this symbol mean? 
a)
Solid
b)
Radioactive 
c)
Artificially made
d)
Kardashian 
17.
What is the FAMILY name for GROUP 2 elements? 
a)
Alkali Metals 
b)
Alkali Earth Metals 
c)
Transition Metals 
d)
Kardashians
18.
Which element UNDER ATOMIC NUMBER 50 is artificially made? 
a)
Bromine 
b)
Tin
c)
Hydrogen 
d)
Technetium
19.
Who has ATOMIC NUMBER 20?
a)
Calcium
b)
Neon 
c)
Carbon 
d)
Krypton
20.
Who has an ATOMIC MASS of 195 (rounded)?
a)
Iridium
b)
Platinum
c)
Gold 
d)
Silver 
21.
What is the lightest element? 
a)
Hydrogen 
b)
Helium 
c)
Uuo 
d)
Francium
22.

The Periodic Table is organized by increasing

a)

charges

b)

atomic number

c)

mass number

d)

electronegativity

23.

The elements in the middle of the table are called the _____________ metals because their properties change from metallic to nonmetallic.

a)

positive

b)

negative

c)

magnetic

d)

transition

24.

The _________________ are a small group of elements that have both metallic and nonmetallic properties.

a)

Oxygen Group

b)

Nitrogen Group

c)

Metalloids

d)

Halogens

25.

The vertical columns on the periodic are called _______________.

a)

Rows

b)

Periods

c)

Groups

d)

Valence

26.

The horizontal rows of the Periodic Table are called ______________.

a)

Periods

b)

Groups

c)

Families

d)

Halogens

27.

The _______________electrons are the electrons on the outer most energy level of the atom.

a)

valence

b)

core

c)

excited

d)

ground state

28.

Elements of the same ______________ have the same number of valence electrons, which determines the elements chemical properties.

a)

Period

b)

Row

c)

Group

29.

This element does not match the properties of any other group so it stands alone. It is placed above Group 1 but it is not part of that group. It is very reactive, colorless, odorless, and a gas at room temperature.

a)

Hydrogen

b)

Helium

c)

Nitrogen

d)

Oxygen

30.

Group 1: These metals are extremely reactive. They all have one valence electron. They are shiny and silver in color. They are soft and can be cut with a knife.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline Metals

d)

Lanthanides

31.

Group 2: Slightly less reactive because they have 2 valence electrons. They are silver colored and more dense that Group 1 metals.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline-earth Metals

d)

Actinides

32.

Groups 3-12: These metals have a moderate range of reactivity and a wide range of properties. They are shiny and good conductors of heat and electricity. They have higher densities and melting points than Groups 1 and 2. These have 1 or 2 valence electrons.

a)

Transition Metals

b)

Alkali Metals

c)

Alkaline-earth Metals

d)

Lanthanides

33.

Elements with atomic numbers 57-70 and 89-102: These metals were taken out and placed at the bottom of the table so the table wouldn't be so wide. Some are shiny and reactive. Others are radioactive and unstable. Elements 95-103 do not exist in nature but have been manufactured in the lab.

a)

Alkali Metals

b)

Alkaline-earth Metals

c)

Lanthanides and Actinides

d)

Boron Group

34.

Group 13: Contains on metalloid and 4 metals. They are reactive. All have 3 valence electrons (Group # minus 10).

a)

Boron Group

b)

Nitrogen Group

c)

Oxygen Group

d)

Carbon Group

35.

Group 14: Contains one nonmetal, two metalloids, and two metals. These all have 4 valence electrons (Group # minus 10) and have varied reactivity.

a)

Boron Group

b)

Carbon Group

c)

Nitrogen Group

d)

Oxygen Group

36.

Group 15: Contains two nonmetals, two metalloids, and one metal. They have varied reactivity. These elements have 5 valence electrons (Group # minus 10).

a)

Boron Group

b)

Carbon Group

c)

Nitrogen Group

d)

Oxygen Group

37.

Group 16: Contains three nonmetals, one metalloid, and one metal. They are a reactive group. These elements all have 6 valence electrons (Group # minus 10).

a)

Boron Group

b)

Carbon Group

c)

Nitrogen Group

d)

Oxygen Group

38.

Group 17: All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend to form salts with metals. Example NaCl: sodium chloride which is known as table salt. These elemtns have 7 valence electrons (Group # minus 10).

a)

Boron Group

b)

Oxygen Group

c)

Nitrogen Group

d)

Halogens

39.

Group 18: Unreactive nonmetals. All are colorless, odorless gases at room temperature. These elements have a full outer energy level, usually 8 valence electrons, except for Helium which only has 2 valence electrons.

a)

Nitrogen Group

b)

Oxygen Group

c)

Noble Gases

d)

Halogens

40.

The elements on the right side of the Periodic Table are classified as ________________.

a)

Metals

b)

Nonmetals

41.

The elements on the left side of the periodic table are classified as ________________.

a)

metals

b)

nonmetals

42.

The periodic table is organized by _________________

a)

Atomic Number

b)

Mass Number

c)

Average Atomic Mass

d)

Alphabetical Order

43.

The periodic table is broken into Rows and Columns.


The Rows are called _____

a)

Periods

b)

Groups

44.

The periodic table is broken into Rows and Columns.


The Columns are called _____

a)

Periods

b)

Groups

45.

Who is considered the Father of the Periodic Table?

a)

Dimitri Mendeleev

b)

John Dalton

c)

Antoine Levoisier

d)

Mr. Hanrahan

46.

What do you call the electrons that are the furthest away from the nucleus?

a)

Valence Electrons

b)

Exterior Electrons

c)

Outer Electrons

d)

Perimeter Electrons

47.

What is the largest group on the periodic table?

a)

Transition Metals

b)

Noble Gases

c)

Metalloids

d)

Alkaline Earth Metals

48.

Which of the following is NOT a metalloid?

a)

Aluminum

b)

Silicon

c)

Boron

d)

Arsenic

49.

Which of the following is a Metal?

a)

Sodium

b)

Carbon

c)

Oxygen

d)

Argon

50.

Which of the following is a Nonmetal?

a)

Sulfur

b)

Gold

c)

Iron

d)

Calcium

51.

What is the name of the group that contains unreactive nonmetals, each with 8 valence electrons?

a)

Noble Gases

b)

Halogens

c)

Alkaline Earth Metals

d)

Rare Earth Metals

52.

What is the name of the group that contains highly reactive metals, each with 1 valence electron?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Rare Earth Metals

53.

What is the name of the group that contains reactive metals, each with 2 valence electrons?

a)

Transition Metals

b)

Halogens

c)

Alkaline Earth Metals

d)

Rare Earth Metals

54.

What is the name of the group that contains highly reactive nonmetals, each with 7 valence electrons?

a)

Noble Gases

b)

Halogens

c)

Alkaline Earth Metals

d)

Metalloids

55.

What is the name of the group that contains radioactive metals, that can each form multiple ions?

a)

Alkali Metals

b)

Noble Gases

c)

Alkaline Earth Metals

d)

Inner Transition Metals

56.

What does the Atomic Number of an element represent?

a)

# of Protons

b)

# of Neutrons

c)

# of Electrons

d)

# of Neutrinos

57.

What element is Period 6, Group 2?

a)

Yrituim

b)

Barium

c)

Osmium

d)

Hafnium

58.

What element is Period 4, Group 8?

a)

Os

b)

Ca

c)

Fe

d)

Ti

59.

What element is Period 6, Group 18?

a)

Radon

b)

Tungsten

c)

Cesium

d)

Xenon

60.

What element is Period 3, Group 16?

a)

Scandium

b)

Germanium

c)

Oxygen

d)

Sulfur

61.

What element is Period 5, Group 6?

a)

Tantalum

b)

Molybdenum

c)

Arsenic

d)

Barium

62.

What is the Period number of Silicon?

a)

2

b)

3

c)

13

d)

14

63.

What is the Period Number of Bromine?

a)

4

b)

5

c)

16

d)

17

64.

What is the Group Number of Titanium?

a)

4

b)

5

c)

6

d)

7

65.

What is the Group Number of Argon?

a)

3

b)

4

c)

17

d)

18

66.

What element has the same Period Number and Group Number?

a)

Na

b)

W

c)

N

d)

O

67.

What state is Calcium?

a)

solid

b)

liquid

c)

gas

68.

What state is Hg?

a)

solid

b)

liquid

c)

gas

69.

What state is N?

a)

solid

b)

liquid

c)

gas

70.

What state is Xe?

a)

solid

b)

liquid

c)

gas

71.

What state is K?

a)

solid

b)

liquid

c)

gas

72.
Which of these is a property of metals?
a)
It's malleable
b)
It can't conduct electricity
c)
They are used in food
d)
It's very brittle
73.
Where are the non-metallic elements found in the periodic table?
a)
In the middle
b)
In the top rows
c)
On the left-hand side
d)
On the right-hand side
74.
Which of these grouping of elements could have the characteristic of luster (shiny)?
a)
Metal
b)
Nonmetal
c)
metalloids
d)
Both metals and metalloids
75.
Which element is a metalloid?
a)
Titanium
b)
Selenium
c)
Potassium
d)
Polonium
76.
Which elements are found on the left to middle of The Periodic Table? 
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Candles
77.
Which of the following would help a student classify an unknown element as a metal, metalloid, or non-metal?
a)
Measure its conductivity
b)
Determine its density
c)
Find its melting point
d)
Observe its color
78.
All of the following are properties used to classify elements as metals, non-metals, and metalloids EXCEPT —
a)
texture
b)
conductivity
c)
luster
d)
malleability
79.
Which type of elements touch the zigzag line?
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Metals and Metalloids
80.
Some students conducted a laboratory investigation to learn more about the physical properties of different elements. They observed four samples and recorded their observations in the table . Based on these observations, which sample is most likely a nonmetal?
a)
Sample 1
b)
Sample 2
c)
Sample 3
d)
Sample 4
81.
A student is given a sample of an unknown substance. He is asked to determine if it is classified as a metal, a metalloid, or a nonmetal. He discovered that the unknown element conducted some heat and electricity, had a shiny luster, and broke easily. This element is most likely a 
a)
metal
b)
nonmetal
c)
metalloid
d)
cannot be determined
82.

What subatomic particles are in the nucleus?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Photons

83.

What subatomic particle has a negative charge?

a)

Electrons

b)

Neutrons

c)

Protons

d)

Nucleus

84.

Which subatomic particle has the least mass?

a)

Electron

b)

Neutron

c)

Proton

85.

Which subatomic particle has no charge?

a)

Electron

b)

Neutron

c)

Proton

86.

Neutrons have the same mass as which subatomic particle?

a)

Electrons

b)

Protons

87.

Which part of the atom has the most mass?

a)

The electrons

b)

In the nucleus

c)

It is evenly spread out

d)

On the outside

88.

Atomic number is a measure of the...

a)

Number of electrons

b)

Number of neutrons

c)

Number of protons

d)

Number of protons and neutrons

89.

To have a charge of zero, what two particles must be balanced in an atom?

a)

Protons and Electrons

b)

Protons and neutrons

c)

Electrons and neutrons

90.

What subatomic particle is different between isotopes?

a)

Electrons

b)

Protons

c)

Neutrons

91.

Mass number is a measure of an atom's

a)

Electrons and protons

b)

Electrons and neutrons

c)

Neutrons and protons

92.

What is the Atomic Number of Nitrogen?

a)

7

b)

14.007

c)

14

d)

21

93.

What is the Atomic Mass of Nitrogen?

a)

7

b)

14.007

c)

14

d)

21

94.

What is the Mass Number of Nitrogen?

a)

7

b)

14.007

c)

14

d)

21

95.

How many electrons are in an atom of Nitrogen?

a)

7

b)

14.007

c)

5

d)

2

96.

How many VALENCE electrons are in an atom of Nitrogen?

a)

7

b)

14.007

c)

5

d)

2

97.

How many energy levels of electrons are in an atom of Nitrogen?

a)

7

b)

14

c)

5

d)

2

98.

How many electrons are in the first energy level of an atom of Nitrogen?

a)

7

b)

14

c)

5

d)

2

99.

What period is Nitrogen in on the Periodic Table?

a)

7

b)

15

c)

5A

d)

2

100.

What group is Nitrogen in on the Periodic Table?

a)

7 (7B)

b)

15 (5A)

c)

5 (5B)

d)

2

101.

How many electrons will Nitrogen gain to fill its outer shell?

a)

2

b)

3

c)

5

d)

8

102.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
103.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
104.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
105.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

106.

What is the atomic number of Barium, Ba? (enlarge the periodic table)

a)

20

b)

38

c)

56

d)

88

107.

What is the atomic number of Nickel? (enlarge the periodic table)

a)

110

b)

28

c)

46

d)

78

108.

How many protons are in a sodium atom, Na? (tap to enlarge the periodic table)

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons

109.

An element has the mass number 12 and atomic number 6. The number of neutrons in it is:

a)

6

b)

10

c)

4

d)

8

110.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

111.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

112.

How many neutrons does C-14 [atomic #6] contain? (tap to enlarge the image)

a)

6

b)

7

c)

14

d)

8

113.

How many neutrons does an atom of the isotope Neon-22 have? (tap to enlarge the image)

a)

12

b)

10

c)

22

d)

20

114.

How many neutrons does an atom of Nitrogen-13 have? (tap to enlarge the image)

a)

6

b)

7

c)

13

d)

5

115.

Isotopes have different numbers of

a)

protons

b)

neutrons

c)

electron

d)

properties

116.

The number in Kr-84 represents what about Krypton?

a)

The number of electrons

b)

The number of protons

c)

The mass number

117.

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

a)

0

b)

1

c)

10

d)

5

118.

How many electrons are in an atom with an atomic number of 50? You will need a periodic table to help you.

a)

5

b)

8

c)

50

d)

2

119.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
120.

How many neutrons does the isotope of lithium - 8 have?

a)

8

b)

3

c)

4

d)

5

121.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
122.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
123.

Which of the following is a property of an acid

a)

bitter taste

b)

sour taste

c)

slippery feeling

d)

turns red litmus blue

124.

Which of the following is a property of a base?

a)

feels soapy

b)

corrodes metals

c)

causes burns on skin

d)

tastes sour

125.

Which would cause burns to the skin?

a)

HCl (hydrochloric ACID)

b)

NaOH (sodium hydroxide BASE)

126.

What types of chemical compounds would corrode a metal?

a)

acids

b)

bases

127.

Which types of substances have pH values that are LOW (below 7)?

a)

acids

b)

bases

128.

Which types of substances have pH values that are HIGH (above 7)?

a)

acids

b)

bases

129.

A pH of 7 is considered to be

a)

acidic

b)

basic

c)

neutral

130.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

131.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

132.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

133.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

134.

Which of the following is a property of a base?

a)

bitter taste

b)

reacts with metals

c)

salty

d)

sour taste

135.

Bases have many uses. They are mainly used to make

a)

cleaning products

b)

soaps

c)

concrete

d)

all of the answer choices

136.

All bases have a sour taste.

a)

True

b)

False

137.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

138.

The strongest bases have pH values close to

a)

0

b)

14

c)

7

d)

5

139.

Which of the following is a base?

a)

baking soda in water

b)

orange juice

c)

vinegar

d)

lemonade

140.

If the substance is neutral, what would the pH be?11

a)

3

b)

5

c)

7

d)

9

e)

11

141.
If an acid is combined with a base of equal strength, the result will most likely be
a)
a neutral solution.
b)
a stronger acid.
c)
impossible to tell without testing the pH.
d)
a stronger base
142.
Which of the following is a base?
a)
orange juice
b)
water
c)
vinegar
d)
dishwashing detergent
143.
Pure water has a pH of 7. Pure water _______.
a)
is a base
b)
is a neutral substance
c)
could be either an acid or a base
d)
is an acid
144.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
145.

A bond between a nonmetal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

146.

What is Covalent Bonding?

a)

Bonding that is the result of two nonmetals sharing electrons

b)

Bonding between two metals

c)

Bonding that is the result of a nonmetal and a metal exchanging electrons

d)

Bonding between more than two elements

147.

Which particle is responsible for bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

148.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

149.

Potassium Chloride is...

a)

Ionic

b)

Covalent

150.

Water (H2O) is...

a)

Ionic

b)

Covalent

151.

Ammonium (NH4) is...

a)

Ionic

b)

Covalent

152.
Share electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
153.
Gain or lose electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
154.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
155.
This picture shows a...
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
156.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

157.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

158.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

159.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

160.

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

161.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
162.

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

163.

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.

164.

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

165.

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

166.

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

167.

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.

168.

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.

169.

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.

170.

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

171.

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.

172.

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.

173.

Match the following to form true statements:

a)

When solid, ionic compounds

1.

cannot conduct electricity

b)

When melted ionic compounds

2.

can conduct electricity

c)

Ionic compounds have

3.

high melting and high boiling points

d)

There are many strong bonds

4.

between ions in an ionic compound.

e)

Elements in group 1 of the periodic table form ions

5.

with a charge of 1+

174.

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

175.

This is an image of the giant ionic lattice representing Sodium Chloride, what is represented by the +?

a)

Cl ion

b)

Cl atom

c)

Na atom

d)

Na ion

176.

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

177.

Is the following compound ionic or covalent?

Exists as a solid, liquid or gas

a)

Ionic

b)

Covalent

178.

Is the following compound ionic or covalent?

A material that has a low boiling point

a)

Ionic

b)

Covalent

179.

Is the following compound ionic or covalent?

A material with a high melting point

a)

Ionic

b)

Covalent

180.

Is the following compound ionic or covalent?

PBr5

a)

Ionic

b)

Covalent

181.

Is the following compound ionic or covalent?

LiBr

a)

Ionic

b)

Covalent

182.

Is the following compound ionic or covalent?

A material that has a low boiling point

a)

Ionic

b)

Covalent

183.

Is the following compound ionic or covalent?

A material that forms a crystal lattice

a)

Ionic

b)

Covalent

184.

Is the following compound ionic or covalent?

A material that is hard and brittle

a)

Ionic

b)

Covalent

185.

Is the following compound ionic or covalent?

A material that SHARES electrons

a)

Ionic

b)

Covalent

186.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

187.
Molten compound conducts electricity.
a)
ionic compound
b)
covalent compound
188.
Molten compound does NOT conduct electricity.
a)
ionic compound
b)
covalent compound
189.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
190.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
191.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

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