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Chemistry Final Review Ch. 5-8

Total questions: 75

Worksheet time: 48mins

Name
Class
Date
1.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
2.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
3.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
4.
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
5.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
6.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
7.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
8.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
9.
A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a)
covalent bond.
b)
ionic bond.
c)
charged bond.
d)
dipole bond.
10.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
11.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
12.
The force that hold two atoms together is called a ______. 
a)
Chemical Change
b)
Reaction
c)
Chemical Bond
d)
Physical Change
13.
How many electrons does chlorine need to gain in order to have a full outer shell? 
a)
7
b)
0
c)
1
d)
8
14.
A charged Particle is called an 
a)
isotope
b)
Ion
c)
Molecule
d)
Compound
15.
How does a selenium atom attain a noble gas electron configuration?
a)
it loses two electrons
b)
it gains two electrons
c)
it loses six electrons
d)
it gains six electrons
16.
Which of the following best describes a metallic bond?
a)
Metal cations are attracted to metal anions
b)
Metal atoms share pairs of valence electrons equally
c)
Metal atoms share pairs of valence electrons unequally
d)
Metal share a "sea" of valence electrons
17.
What is the name of the covalent molecule C4H10?
a)
Tetracarbon Decahydroxide
b)
Tetracarbon Decahydride
c)
Carbon Hydroxide
d)
Tetracarbon Decahydrogen
18.

Which of the following is NOT covalently bonded?

a)

K2S

b)

H2O

c)

I2

d)

CO2

19.
What is a cation?
a)
positive ion
b)
Neutral atom
c)
Two additional protons
d)
negative ion
20.
What is an anion?
a)
positive ion
b)
negative ion
c)
neutral atom
d)
2 neutrons taken away
21.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
22.
What element in period 2 has 7 valence electrons?
a)
Beryllium
b)
Chlorine
c)
Magnesium
d)
Fluorine
23.
Which element has the same number of electrons in the outermost energy level as lithium?
a)
Hydrogen
b)
Beryllium
c)
Carbon
d)
Magnesium
24.

What is a molecule?

a)

two elements bonded together (sharing electrons)

b)

a mixture of different substances

c)

smallest individual particles

d)

two elements bonded together (transferring electrons)

25.
How many total atoms are in the compound C2H8O ?
a)
11
b)
2
c)
8
d)
1
26.
Energy that is stored in bonds between atoms is:
a)
Mechanical energy
b)
Chemical energy
c)
Kinetic energy
d)
Nuclear energy
27.
What group of elements satisfies the octet rule without forming compounds?
a)
halogen
b)
noble gas
c)
alkali metal
d)
alkaline-earth metal
28.

Alkaline earth metals form ions with _____ charge

a)

-1

b)

+1

c)

+2

d)

-2

29.

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

30.

What type of chemical bond is represented in this diagram?

a)

double covalent bond

b)

single covalent bond

c)

ionic bond

d)

metallic bond

31.
11. Which of the following physical properties is not typical of metals?
a)
a) Sonorous
b)
b) Electrical Conductor
c)
c) Low melting point
d)
d) Maleable
32.

An alloy is a mixture of a(n) ____ and one or more other elements.

a)

metal

b)

organic compound

c)

ceramic

d)

plastic

33.

How does increasing the amount of carbon in steel affect its properties?

a)

Carbon makes the lattice harder and stronger.

b)

Carbon forms an oxide that protects the steel from rusting.

c)

Carbon makes the steel light enough to use for airplane parts.

d)

Carbon makes the steel softer and easier to cut.

34.

What does the element symbol in an electron dot diagram represent?

a)

the nucleus of the atom.

b)

the nucleus and all electrons.

c)

the nucleus and valence electrons.

d)

the nucleus and all non-valence electrons.

35.
The substances listed on the right side of a chemical equation are the
a)
Yields
b)
Reactants
c)
Products
d)
Precipitates
36.
The substances listed on the left side of a chemical equation are the
a)
Products
b)
Coefficients
c)
Precipitates
d)
Reactants
37.
In chemical reactions, what does the principle of conservation of mass mean?
a)
Matter is not created or destroyed.
b)
The total mass of the reactants is greater than the total mass of the products.
c)
The total mass of the reactants is less than the total mass of the products.
d)
Matter is not changed.
38.

A solid that is produced as a result of a chemical reaction in solution & separates from solution

a)

reactant

b)

yield

c)

precipitate

d)

coefficient

39.

An equation in which the reactants & products in a chemical reaction are represented by words:

a)

chemical equation

b)

word equation

c)

reversible reaction

d)

formula equation

40.

A chemical reaction in which the products re-form the original reactants:

a)

coefficient

b)

precipitate

c)

reversible reaction

d)

word equation

41.

An equation that represents the reactants and products of a chemical reaction by their formulas or symbols:

a)

formula equation

b)

word equation

c)

cofficient

42.

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

a)

coefficient

b)

precipitate

c)

subscript

43.

Which is NOT an indicator of a chemical change?

a)

Color Change

b)

Precipitate formed

c)

Production of Gas (Bubbles)

d)

Change of state

44.

H2, F2, O2, I2, Cl2, Br2, N2 are all

a)

polyatomic ions

b)

diatomic molecules

c)

noble gases

d)

transition metals

45.
What kind of reaction is this:
2H2O2 →2 H2O + O2
a)
Synthesis
b)
Decomposition
c)
Single Replacement 
d)
Combustion
46.
The reaction below is an example of?
AgNO3 + NaCl → AgCl + NaNO3
a)
Single Replacement
b)
Double Replacement
c)
Decomposition
d)
Combustion
47.
What kind of reaction is this:
4Fe  +  3O2 →   2Fe2O3 
a)
Synthesis
b)
Decomposition
c)
Single Replacement 
d)
Double Replacement
48.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
49.
Balance this equation-
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
50.

2H2O -> H2 + O2 is it balanced?

a)

No

b)

Yes

51.

2H2O -> 2H2 + O2 what is the correct word equation?

a)

water synthesizes into hydrogen and oxide

b)

hydrogen and oxygen gases react to form water

c)

water breaks down into hydrogen and oxygen gases

52.

(g) in a chemical equation means

a)

gravity

b)

gaseous

c)

great reactant

53.

When a chemical is written over the arrow in a chemical equation it means this is used

a)

extra reactant

b)

catalyst

c)

cation

d)

an impurity is produced

54.

When two chemicals combined to form a more complex chemical this reaction has occured

a)

synthesis

b)

combustion

c)

decomposition

d)

single replacement

55.

Which type of reaction has ions switching places in two compounds?

a)

single replacement

b)

combustion

c)

double replacement

d)

synthesis

56.

When a single binary compound decomposes this is produced

a)

a new compound

b)

a single element

c)

two elements

d)

an oxide

57.

The list of elements by ease they react

a)

activation list

b)

activity series

c)

reaction documentation

58.

When zinc metal is added to water

a)

it heats up

b)

it reacts

c)

it does not react

59.

When lead is added to acid

a)

no reaction

b)

lead replaces hydrogen

c)

lead oxide is formed

60.

When nickel is added to potassium chloride

a)

no reaction

b)

nickel and potassium react

c)

nickel replaces potassium

d)

nickel chloride is formed

61.

What follows an element’s symbol in a chemical formula to indicate the number of atoms of that element in one molecule of the compound?

a)

charge sign

b)

superscripted number

c)

number in parentheses

d)

subscripted number

62.

What is the correct name for the NO3- ion?

a)

nitrate

b)

nitrite

c)

nitride nitrite

d)

nitrogen oxide

63.

What is the correct formula for copper(I) cyanide?

a)

CuCy

b)

CuCy2

c)

CuCN

d)

Cu2CN

64.

What is the correct name for the compound P2Cl4.

a)

phosphorus chloride

b)

phosphorus tetrachloride

c)

diphosphorus chloride

d)

diphosphorus tetrachloride

65.

What is the correct formula for the compound made of magnesium (Mg2+) and nitrogen (N3-)?

a)

Mg2N3

b)

Mg3N2

c)

MgN2

d)

MgN

66.

Atoms have an oxidation number of zero in a(n)

a)

pure element.

b)

acid.

c)

ionic compound.

d)

molecular compound.

67.

What is the correct name for the compound Ni2O3 using the Stock system?

a)

nickel(II) oxide

b)

dinickel trioxide

c)

nickel trioxide

d)

nickel(III) oxide

68.

What is the oxidation number of phosphorus in the PO43- ion?

a)

-3

b)

0

c)

+5

d)

+8

69.

What is the correct formula for the compound platinum(VI) fluoride?

a)

PtF3

b)

PtF6

c)

Pt6F2

d)

Pt6F

70.

The molar mass of any compound is described in units of

a)

grams

b)

u

c)

moles

d)

grams per mole

71.

The simplest whole-number ratio of moles of each element in a compound is known as the

a)

percent composition.

b)

empirical formula.

c)

Stock formula.

d)

molecular formula.

72.

In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is equal to

a)

0

b)

10

c)

the number of atoms in the ion.

d)

the charge on the ion.

73.

The first part of the name of a binary ionic compound is the

a)

cation (positive ion).

b)

polyatomic ion (multiple element ion).

c)

oxyanion (ion w/ Oxygen).

d)

anion (negative ion).

74.

What is the molar mass of pure tin?

a)

1.00 g/mol

b)

47.88 g/mol

c)

118.71 g/mol

d)

237.42 g/mol

75.

How many moles of compound are there in 15.0 g of potassium dichromate, K2Cr2O7? (The molar mass of K2Cr2O7 is 294.2 g.)

a)

0.0510 mol

b)

11.0 mol

c)

15.0 mol

d)

294 mol

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