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Chemical Bonding

Total questions: 74

Worksheet time: 38mins

Name
Class
Date
1.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

2.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

3.

Always a solid at room temperature

a)

Ionic compounds

b)

Covalent compounds

4.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

5.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

6.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

7.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

8.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

9.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

10.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

11.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

12.

MgO

a)

ionic

b)

covalent

c)

metallic

13.

NaCl

a)

ionic

b)

covalent

c)

metallic

14.

If two fluorine atoms bond they will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

15.

Hydrogen and Chlorine will from a _________ bond

a)

ionic

b)

covalent

c)

metallic

16.

Cations have a _____________ charge.

a)

positive

b)

negative

c)

neutral

17.

Anions have a ____ charge.

a)

positive

b)

negative

c)

neutral

18.

In ionic bonding, valence electrons are _______.

a)

shared

b)

transferred

c)

destroyed

19.

In covalent bonding, valence electrons are ______.

a)

shared

b)

transferred

c)

destroyed

20.

Why do all bonds form?

a)

filling the outermost energy level to be stable

b)

to make all atoms the same

c)

to make other atoms unstable

d)

to make all atoms different

21.

Why don't noble gases form bonds?

a)

They all have a full octet

b)

Noble gases do form bonds

c)

They only bond when with eachother

d)

none of these answers are correct

22.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
23.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
24.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
25.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
26.

What kind of bond will Potassium form with Sulfur?

a)

ionic

b)

covalent

c)

metallic

d)

no bond

27.

In ionic bonds, metals tend to

a)

share valence electrons

b)

gain valence electrons

c)

lose valence electrons

d)

keep their electrons

28.

Bond that forms when electrons delocalize forming the "electron sea."

a)

covalent bond

b)

hydrogen bond

c)

metallic bond

d)

ionic bond

29.

This type of bond typically forms between a metal and another metal.

a)

covalent

b)

hydrogen

c)

metallic

d)

ionic

30.

In an electron dot diagram, the dots represent...

a)

nucleus

b)

inner shell electrons

c)

valence electrons

d)

protons

31.

True or False...When writing formulas for IONIC compounds, the total amount of positive charge must equal the total amount of negative charge (making the compound neutral).

a)

True

b)

False

32.
NaCl
a)
Ionic
b)
Covalent
c)
Metallic
d)
Polyatomic Ion 
33.
Which is most likely to form a negative ion?
a)
an element from group 17
b)
a metal
c)
an element from group 1
d)
an element with atoms that have eight valence electrons
34.

Identify the types of bonds shown in the image.

a)

A. Covalent , B. Ionic, C. Metallic

b)

A. Covalent , B. Metallic, C. Ionic

c)

A. Ionic , B. Covalent, C. Metallic

d)

A. Ionic , B. Metallic, C. Covalent

35.

What happens when two negatively charged ions are pushed together?

a)

they will repel (move apart)

b)

they will be attracted to each other (move together)

36.

What happens when two oppositely charged ions are pushed together?

a)

they will repel (move apart)

b)

they will be attracted to each other (move together)

37.

How does magnesium become an magnesium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

38.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
39.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
40.

In metallic bonds electrons :

a)

are shared

b)

move around the nuclei randomly

c)

are transferred

41.

Malleability and ductility are characteristics of compounds with

a)

covalent bonds

b)

metallic bonds

c)

ionic bonds

d)

alloy bonds

42.

Alloys are important because

a)

their properties are often superior to the component elements

b)

their properties are a blend of the component elements

c)

they never corrode

d)

they are less expensive than their component elements.

43.

Why are metals good conductors?

a)

they have mobile electrons

b)

they have mobile atoms

c)

they have crystal structures that can rearrange

d)

they have mobile protons

44.

Malleability means

a)

the ability to be drawn into a wire

b)

the electrons of metals are mobile

c)

the ability to be hammered into a shape

d)

the ability to be a conductor of electricity

45.

In metals, the valence electrons are

a)

attached to the most positive ions

b)

shared by all of the atoms

c)

are bonded to the least electronegative element

d)

shiny

46.
A three dimensional pattern of repeating ions is called a _________ ________
a)
crystal lattice
b)
ionic lattice
c)
iceberg lettuce
d)
covalent molecule
47.

Metallic bonds include a "sea" of free moving _______.

a)

electrons

b)

atoms

c)

molecules

d)

protons

48.
Ionic bonds are between _______ and ________. 
a)
nonmetals and nonmetals 
b)
metals and metals 
c)
metals and nonmetals
d)
none
49.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
50.

MgO dissolves in water and the solution conducts electricity.

Mg is a metal. O is a non-metal.

What type of bond holds the molecule together?

a)

ionic

b)

covalent

c)

metallic

51.

SO2 does not conduct electricity in water or by itself. Identify the following compound as metallic, ionic or covalent:

a)

ionic

b)

covalent

c)

metallic

52.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
53.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
54.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

55.

These compounds generally have low melting and boiling points.

a)

Ionic compounds

b)

Covalent compounds

56.

The name for a single unit of an ionic compound is

a)

molecule

b)

crystal latticde

c)

formula unit

d)

alloy

57.

Roman numerals are used in naming certain ions because

a)

bad question - Roman numerals are never used

b)

non-metals can often have many different charges

c)

it is easier than looking on the periodic table

d)

there are multiple cations that can form from that element

58.

Isoelectronic means

a)

elements have the same number of valence electrons

b)

atoms and ions have the same number of valence electrons

c)

atoms and ions have the same total number of electrons

d)

atoms and ions are the same size

59.

This force holds ions together in a compound

a)

electrostatic

b)

metallic

c)

molecular

d)

strong nuclear

60.

Another name for covalent compounds is

a)

allotrope

b)

metallic

c)

ionic

d)

molecular

61.

Which of the following properties does not belong to an alloy as compared to its pure metal?

a)

Stronger

b)

More corrosion resistant

c)

Harder

d)

More malleable

62.

A mixture of metals is called an (a)   .

63.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
64.

what are the 2 types of alloys

a)

substitutional

b)

additional

c)

interstitial

d)

intracellular

65.

the biggest difference between substitutional and interstitial alloys are

a)

substitutional alloys have a minor size difference while interstitial alloys have a large size difference

b)

substitutional alloys have a major size difference while intercellular alloys have a minor size difference

c)

substitutional are liquds found to be highly conductive while interstitial are liquids that are highly flamable

d)

none of the above

66.

Which of the following statements is best explain why pure metals are malleable causing its shape can be easily changed?

a)

There are empty spaces between metal atoms. When force applied layers of atoms slide and fill the empty spaces

b)

The metal atoms arranged in orderly manner. When force applied atoms will vibrate and move faster.

c)

There are no empty spaces between metal atoms. When force applied layers of atoms slide and pure metal change shape

d)

There are empty spaces between metal ions. When force applied layers of ions slide and fill the empty spaces

67.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
68.
What charge will a sulfide ion have?
a)
3+
b)
2+
c)
2-
d)
3-
69.
Metals __________ electrons when they become ions
a)
lose
b)
gain
c)
neither
70.

Non-metals ________ electrons when they become ions.

a)

lose

b)

gain

c)

neither

71.

Which of the following groups on the Periodic Table will only form ions with positive charges?

a)

Group 2

b)

Group 15

c)

Group 17

d)

Group 18

72.

Which of the following pairs of atoms and/or ions is isoelectronic?

a)

Na and K

b)

Cl and Cl-1

c)

Ne and Na+1

d)

O-2 and S-2

73.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

74.

Atoms and ions that are isoelectronic have

a)

the same charge.

b)

the same number of electrons.

c)

the same number of protons.

d)

no charge since the number of protons and electrons is equal.

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