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Review: metallic, ionic, covalent

Total questions: 44

Worksheet time: 2hrs 49mins

Name
Class
Date
1.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
2.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
3.
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.
4.

Why are metals malleable?

a)

They are shiny

b)

The electrons are held tightly within the lattice structure making it strong

c)

The electrons are delocalized and able to move between the atoms

d)

The electrons are shared between two metal ions and this holds the atoms together

5.
Magnesium bromide is an ionic compound with the chemical formula 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
6.

Which of the following pairs of elements would NOT react to form an IONIC compound?

a)

sulfur and phosphorus

b)

sodium and iodine

c)

iron and oxygen

d)

aluminum and bromine

7.
Ionic compounds are ordinarily found as
a)
plasma
b)
liquids
c)
gasses
d)
crystalline solids 
8.

How are compounds with metallic bonds similar to ionic compounds?

a)

Both tend to have double and triple bonds.

b)

Both tend to have low boiling point

c)

Both tend to have poor conductivity.

d)

Both tend to have high melting points.

9.

How are compounds with metallic bonds similar to ionic compounds?

a)

They both have repeating structures

b)

They both have high mp and bp

c)

Both tend to have poor conductivity.

d)

Both tend to have low melting points.

10.

Nonmetals tend to form ions by

a)

destroying electrons

b)

gaining electrons

c)

losing electrons

d)

sharing electrons

11.

In metallic bonds, the force of attraction is between

a)

positive and negative ions

b)

cations and electrons

c)

two different metals

d)

neutrons and electrons

12.

Metals are used to make electric wires because metals (choose all that apply)

a)

are ductile

b)

are shiny

c)

have free moving electrons

d)

form a lattice

13.

How does a metallic lattice differ from an ionic crystal?

a)

A metallic lattice is less flexible

b)

A metallic lattice can change shape without breaking

c)

A metallic lattice shatters when struck

14.

An alloy of iron and carbon is

a)

more likely to rust than pure iron

b)

weaker than pure iron

c)

a mixture of two METALS

d)

known as steel

15.

True or False: A metallic bond may form between a metal and any other element

a)

True

b)

False

16.

What are some benefits of alloys? (choose all that apply)

a)

they can be stronger than pure metal

b)

they may not rust/corrode as easily

c)

they don't have electrons

d)

they form covalent bonds

17.
Which type of bonding allows for the conduction of electricity in the solid state?
a)
Metallic
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
18.

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

19.

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.

20.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
21.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
22.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
23.
The ability of a material to deform, usually by stretching along its length. This property allows us to make wires.
a)
conductivity
b)
ductility
c)
malleability
d)
hardness
24.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
25.
Large molecules made up of smaller molecules.
a)
monomer
b)
polymer
c)
hydrocarbon
d)
plastic
26.
Small molecules that make up larger molecules.
a)
monomer
b)
polymer
c)
synthetic
d)
plastic
27.
Petroleum based product 
a)
plastic
b)
synthetic
c)
inorganic
d)
organic
28.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
29.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
30.
a)
2
b)
8
c)
3
d)
13
31.

Covalent compounds may be (multi select)

a)

3 atom molecules

b)

large repeating structures

c)

small 2 atom molecules

d)

single atoms

32.
a)
7
b)
8
c)
9
d)
10
33.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
34.

Is this correct way to draw the Lewis Dot Structure for Carbon?

a)

Yes

b)

No, too many electrons

c)

No, not enough electrons

d)

No, dots are in wrong places

35.

Which of these is incorrect?

a)
b)
36.
In a stable atom the amount of electrons is electron is equal to
a)
neutrons
b)
protons
c)
atomic mass
d)
neutrons + protons
37.

Which area would be most useful in determining the identity of an element?

a)

Area 1

b)

Area 2

c)

Area 3

d)

Area 4

38.

Which statement best explains why protons are used to identify an element?

a)

Protons are the most easily identified subatomic particles

b)

Positive charges are more easily detected during an investigation than negative and neutral charges

c)

The number of protons is unique to each element and remains constant

d)

Protons alone cannot be used to identify an element. The number of electrons and neutrons must also be known.

39.

What is a cation's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element

40.

What is an anion's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element's charge

41.
In general, what can be said of the melting points of metals?
a)
They are low.
b)
They are high.
c)
They are lower than nonmetals.
d)
They do not have melting points.
42.

Identify the compound if hydrogen and chlorine are chemically combined.

a)

HCl

b)

HCl7

c)

H1Cl1

d)

H1Cl7

43.

Valence electrons are 'shared' between 2 atoms

a)

ionic bonding

b)

covalent bonding

c)

metallic bonding

44.

Select the covalent compounds

a)

lithium fluoride

b)

nitrous oxide

c)

carbon dioxide

d)

methane

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