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chem chapter 8 bonding

Total questions: 50

Worksheet time: 45mins

Name
Class
Date
1.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

2.

The negative ions tend to _____________ electrons.

a)

lose

b)

gain

3.

Valence electrons are found

a)

in the innermost energy level of an atom

b)

in the middle energy levels of an atom

c)

in the outermost energy levels of an atom

4.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

5.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
6.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
7.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
8.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
9.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
10.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

11.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

12.
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.
13.
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
14.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
15.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
16.

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 moving electrons.

17.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
18.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
19.

Electrons that are free to move in metals are called (a)   electrons

20.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

21.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

22.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
23.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
24.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
25.
Molten compound does NOT conduct electricity.
a)
ionic compound
b)
covalent compound
26.
Have a high m.p. (1000°C-3000°C)
a)
ionic compounds
b)
covalent compounds
27.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
28.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
29.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
30.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
31.
electrolytes
a)
ionic compounds
b)
covalent compounds
32.

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

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

33.

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

34.
What type of bond forms between two or more atoms that are charged (+/-)?
a)
Covalent bond
b)
Incomplete bond
c)
Ionic bond
d)
Metallic bond
35.

The particle formed when two or more atoms bond covalently is...

a)

structural formula

b)

molecule

c)

hybridization

d)

oxyacid

36.

Any acidic compound that contains oxygen is called a(n)...

a)

hybrid

b)

molecule

c)

structural formula

d)

oxyacid

37.
CaCO3 represents a chemical
a)
Symbol
b)
Formula
c)
Subscript
d)
Reaction
38.

A small whole number that appears in front of a formula in a chemical equation

a)

coefficient

b)

precipitate

c)

subscript

39.
Name the compound: HoI3
4 lines
40.
What name results when Ca+2  and  Br- ions bond?
a)
calcium bromine
b)
calcium boron
c)
calcium boride
d)
calcium bromide
41.
Fe+3   +    S-2
a)
FE+4(S)=3
b)
Fe2S4
c)
Fe2S3
d)
Fe3S2
42.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
43.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
44.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2PO3
d)
Mg3(PO3)2
45.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
46.
Name KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
47.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
48.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
49.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
50.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O

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