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Worksheets

Solids

Total questions: 40

Worksheet time: 35mins

Name
Class
Date
1.

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

2.
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
3.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
4.

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

5.
Ionic compounds are ordinarily found as
a)
plasma
b)
liquids
c)
gasses
d)
crystalline solids 
6.

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.

7.

Which is an example of an metallic solid?

a)

Quartz

b)

NaCl

c)

Ammonia

d)

Iron

8.
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
9.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
10.
Which type of bonding allows for the conduction of electricity in the solid state?
a)
Metallic
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
11.

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 delocalised electrons.

12.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
13.
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
14.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

15.

Metals have...

a)

High meting points because metallic bonds are weak

b)

Low melting points because metallic bonds are weak

c)

High melting points because metallic bonds are strong

d)

All of the above

16.

What is the 'quick clue' that a solid is ionic? It involves....

(m = metal, nm = nonmetal)

a)

m & nm

b)

m & m

c)

nm & nm

d)

Clue? I have no clue!

17.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
18.

What is the name of the 3D pattern that forms when ions bond together?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

an ionic chalice

19.

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 molten (melted) and dissolved in water

20.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

21.

When can an ionic compound conduct electricity?

a)

when dissolved in water

b)

as a solid

c)

as a crystal

d)

when warmed slightly

22.

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

a)

conduct electricity when molten (melted)

b)

conduct electricity when in solution

c)

have high boiling points

d)

are insoluble in water

23.

When dissolved in water, which has a solution that is a good conductor of electricity?

a)

ionic compounds

b)

covalent compounds

c)

metallic compounds

d)

ALL

24.

Which solids are usually hard AND brittle?

a)

ionic compounds

b)

covalent network solids

c)

metallic

d)

covalent molecular solids

25.

Which could be a white crystalline solid that....

- melts at 801°C

- doesn't conduct electricity when solid

- conducts electricity when dissolved in water

- dissolves easily in water

a)

C6H12O6(s)

b)

NaCl(s)

c)

SiO2(s)

d)

Cu(s)

26.
Why are Covalent Compounds normally gases or liquids? 
a)
They have very high melting points
b)
They have normal melting points
c)
They have low melting points
d)
They do not have a specific melting point 
27.
What are covalent compounds mainly comprised of (made of)? 
a)
Metals
b)
Non-metals
c)
Metals and Non-metals
d)
Metalloids 
28.
Decide which is example is NOT a covalent compound
a)
H2O
b)
CO2
c)
SO4
d)
CaCl2
29.
Why are covalent compounds non-conductive to electricity? 
a)
They do NOT contain charged atoms (ions) 
b)
They contain ions, but have equal charges in those ions
c)
They contain metals, which give away electrons
d)
They bond by transferring electrons 
30.
True or False: 
ALL covalent compounds are insoluble in water (cannot dissolve in water) 
a)
True
b)
False
c)
Tu eres loco, Hagerman
d)
The illuminati 
31.
Covalent compounds tend to be.... 
a)
Solids 
b)
Solids and liquids
c)
Gases only
d)
Liquids and gases 
32.
Why do covalent compounds have low melting points? 
a)
They have weak forces ("bad relationships = break up)
b)
They have strong forces that allow them to physically melt
c)
They have slow chemical reactions which cause them to melt 
d)
They have isomers that change shapes into gases or liquids 
33.
Why is rain water conductive to electricity but distilled (pure) water is not? 
a)
Rain water contains covalent compounds, which are conductive to electricity 
b)
Distilled water contains ions, which have charges
c)
Distilled water is pure water, H2O, which is covalent.  Covalent compounds lack a charge
d)
Rain water is a mixture of pure water and other salts.  Salts lack a charge
34.

Which of the following materials is an example of a 3-D covalent lattice?

a)

Copper

b)

Diamond

c)

Carbon dioxide

d)

Potassium chloride

35.

The two types of bonding in graphite are

a)

Covalent and ionic

b)

Metallic covalent

c)

Ionic and metallic

d)

Covalent and weak intermolecular forces

36.

Diamond is hard to the presence of:

a)

Directional intermolecular forces in 3 dimensions

b)

Directional dipole-dipole forces in 3 dimensions

c)

Directional hydrogen bonding in 3 dimensions

d)

Directional covalent bonding in 3 dimensions

37.

What statement is incorrect about graphite

a)

It conducts electricity

b)

It can be used as a lubricant

c)

It is slippery

d)

It's melting point is 300 C

38.

Silicon carbide, SiC, has a similar structure to diamond. What type of properties would you expect?

a)

Hard, good electrical conductor, high melting point

b)

Hard, good electrical conductor, low melting point

c)

Soft, good electrical conductor, high melting point

d)

Hard, poor electrical conductor, high melting point

39.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
40.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

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