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Ionic and Metallic Bonds

Total questions: 25

Worksheet time: 14mins

Name
Class
Date
1.

An atom that has gained or lost electrons is called ...

a)

a polyatomic ion

b)

an isotope

c)

an ion

d)

a neutral atom

2.

Atoms that lose electrons become...

a)

anions

b)

cations

c)

neutral atoms

d)

polyatomic ions

3.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
4.
Nitrogen will ____ electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
5.

Which of the following is NOT a property of ionic compounds?

a)

They are crystalline.

b)

They conduct electricity when in solution.

c)

They have high boiling points.

d)

They are insoluble in water.

6.

Magnesium bromide is an ionic compound with the formula unit MgBr₂. What does the "2" tell you?

a)

There are 2 bromide ions for every magnesium ion

b)

Bromide has a 2- charge

c)

Bromide has a 2+ charge

d)

There are 2 magnesium ions to every bromide ion

7.

Which types of elements become cations?

a)

nonmetals

b)

metals

c)

only transition metals

d)

metalloids

8.

Atoms gain or lose electrons to become stable by satisfying this rule.

a)

Lewis Structure Rule

b)

Periodic Law

c)

Octet Rule

d)

Ionic Law

9.
What do you call a bond that forms when electrons are transferred from one atom to another?
a)
a compound bond
b)
an ionic bond
c)
a crystal bond
d)
an atomic bond
10.

Based in sulfur's charge, what would be copper's charge in Cu2S?

a)

+1

b)

+2

c)

-1

d)

-2

11.

Ionic compounds have a _____.

a)

neutral charge

b)

positive charge

c)

negative charge

d)

various charges

12.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
13.

What does malleable mean?

a)

able to be flattened

b)

will break easily

c)

able to be pulled into a wire

d)

is shiny

14.
How many valence electrons does aluminum have?
a)
13
b)
14
c)
3
d)
4
15.

In the picture shown, #2 is likely __________.

a)

Carbon

b)

Magnesium

c)

Nitrogen

d)

Oxygen

16.

Look at the following electron configuration: 1s22s22p63s1

What charge will the ion of this element likely form?

a)

+2

b)

-2

c)

+1

d)

-1

17.

Why do ions form?

a)

Atoms become more stable when sharing electrons.

b)

Atoms become more stable by gaining or losing protons.

c)

Atoms become more stable with a Noble Gas electron configuration.

d)

Atoms become more stable as Transition Metals.

18.
When magnesium and chlorine react, they form an ionic compound. What is the charge of the ionic compound?
a)
+1
b)
+2
c)
-3
d)
0
19.

What is the formula unit for a compound of calcium and chlorine?

a)

CaCl

b)

Ca2Cl

c)

CaCl2

d)

ClCa

20.
Group 17 always has ions with a charge of ____.
a)
+1
b)
+2
c)
-1
d)
-2
21.

An electronegativity difference greater than 1.7 results in ________.

a)

Nonpolar Covalent bonding

b)

Metallic bonding

c)

Ionic bonding

d)

Polar Covalent bonding

22.

Nitrogen and oxygen react. Their bond is __________.

a)

Polar Covalent

b)

Metallic

c)

Ionic

d)

Nonpolar Covalent

23.
Lithium and fluorine react. Their bond is __________.
a)
Covalent
b)
Metallic
c)
Ionic
24.

In metals, the _______ electrons form a shared sea of electrons.

a)

negative

b)

core

c)

valence

d)

positive

25.

Due to low electronegativity, metals will ____ electrons.

a)

gain

b)

lose

c)

retain

d)

repel

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