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Quarter 3 CBA Review

Total questions: 63

Worksheet time: 11hrs 57mins

Name
Class
Date
1.

What is the correct formula for Calcium Phosphate?

a)

Ca3(PO4)2

b)

Ca3(PO4)

c)

Ca2(PO4)

d)

Ca2(PO4)2

2.

What is the correct name for the compound with the formula (NH4)3PO4

a)

Ammonium Pyrophosphite

b)

Ammonium Phoporylate

c)

Ammonium Phosphite

d)

Ammonium Phosphate

3.

The correct name for the compound with the formula PbSO3 is

a)

Lead (II) Sulfite

b)

Lead (III) Sulfite

c)

Lead Sulfite

d)

Lead Sulfate

4.

What is the correct name of the compound P2O5

a)

phosphorous oxide

b)

diphosphorous pentoxide

c)

phosphorous pentoxide

5.

What formula represents dinitrogen trioxide?

a)

N3O2

b)

NO2

c)

N2O3

6.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
7.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
8.

Why are chemical equations always balanced? Select ALL that apply.

a)

Matter cannot be created.

b)

Matter cannot be destroyed.

c)

Matter can only be rearranged/conserved.

d)

Matter doesn't matter.

9.

In a chemical reaction, if the reactants are heated, the reaction usually happens

a)

slower

b)

faster

c)

at the same rate

d)

in a smaller volume

10.
The left side of the equation below is called
a)
Products
b)
Reactants
11.
The right side of the equation below is called the
a)
products
b)
reactants
12.
A chemical reaction that absorbs heat
a)
Single replacement
b)
Exothermic
c)
Endothermic
d)
Decomposition
13.
What type of reaction is illustrated below?
2HI --> H2  +  I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
14.

What type of reaction is illustrated below?

Zn + H2S --> ZnS + H2

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

15.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
16.

Which one shows that a chemical reaction has occurred?

a)

dissolving

b)

melting

c)

formation of a gas

d)

bending

17.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
18.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
19.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

20.

Combustion reactions will always involve

a)

Oxygen and a solid

b)

Liquid nitrogen and heat

c)

Oxygen and heat/energy released

d)

CO and H2O

21.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
22.

A chemical reaction or process that absorbs heat from the surroundings

a)

Endothermic

b)

Exothermic

23.

A chemical reaction or process that releases heat.

a)

Endothermic

b)

Exothermic

24.

What is the oxidation number of O in the molecule O2 ?

a)

0

b)

-2

c)

+1

d)

+2

25.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
26.

Categorize

Fe + O2 → Fe2O3

a)

Redox

b)

Neutralization (Acid-Base)

c)

electrolysis

d)

Precipitation

27.

Categorize

FeS + HCl → H2S + FeCl2

a)

neutralization (acid-base)

b)

precipitation

c)

redox

d)

electrolysis

28.

Categorize: (Mark ALL correct answers.)

Zn(OH)2 + HNO3 ---> H2O + Zn(NO3)2

a)

Neutralization

b)

Redox

c)

electrolysis

d)

Acid-base

e)

Precipitation

29.

What is collision theory?

a)

Molecules must collide in the correct orientation with enough energy to bond.

b)

Molecules need enough energy to collide and react.

c)

Atoms constantly collide and react.

d)

The minimum energy needed for atoms to react

30.

What factors effect rate of reaction?

a)

Temperature, Concentration, Time, Pressure and Energy

b)

Surface Area, Concentration, Catalyst, Energy, and Pressure

c)

Temperature, Pressure, Concentration, Catalyst, and Surface area

d)

Pressure, Surface area, Density, Temperature, and Energy

31.

Redox is short for ___

a)

reverse deoxygenation

b)

reduction-oxidation

c)

red oxygen

d)

redone exactly

32.

Mark all the ways that the following reaction can be classified.

HCl + NaOH → NaCl + H2O

a)

Neutralization

b)

Combustion

c)

Double Replacement

d)

Decomposition

e)

Acid-Base

33.
Find the percentage composition of  Mg in Mg3(PO4)2.
   

a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
34.
Calculate the molar mass of Mg(OH)2.
a)
33.2 g/mol
b)
41.3 g/mol
c)
86.9 g/mol
d)
58.3 g/mol
35.
How many grams of Hydrogen are there in 25 moles of water?
a)
25 g
b)
450 g
c)
18 g
d)
50 g
36.
What is Avogadro's number?
a)
6.02×1023
b)
6.02×1024
c)
6.02×1027
d)
6.02×1020
37.

What is the molar mass of table salt (NaCl)?

a)

116.886 g/mol

b)

35.453 g/mol

c)

22.990 g/mol

d)

58.443 g/mol

38.

How many moles are in 16.94g of water (H2O)?

a)

16.94

b)

0.9403

c)

305.2

d)

1.063

39.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
40.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
41.

How many liters are in 3.2 moles of CO2 gas at STP?

a)

22.4 Liters

b)

71.68 Liters

c)

5 liters

d)

85.0 Liters

42.

22.4 Liters of O2 gas at STP is equal to

a)

3 moles

b)

1 mole

c)

.5 moles

43.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
44.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
45.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
46.

What is ionic bonding?

a)

Bonding that is the result of two elements sharing electrons

b)

Bonding involving only one atom

c)

Bonding that is the result of an exchange of electrons between a metal and a nonmetal

d)

Bonding between two metals

47.

What is Covalent Bonding?

a)

Bonding that is the result of two nonmetals sharing electrons

b)

Bonding between two metals

c)

Bonding that is the result of a nonmetal and a metal exchanging electrons

d)

Bonding between more than two elements

48.

This Lewis Dot Structure for water is correct

a)

True

b)

False

49.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

50.

Choose all of the covalent molecules below.

a)

H2O

b)

C

c)

Br2

d)

CCl4

51.

What is the shape of this molecule?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Pyramidal

e)

Trigonal Planar

52.

WHat is the shape of this molecule?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Pyramidal

e)

Trigonal Planar

53.

What is the shape of this molecule?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Pyramidal

e)

Trigonal Planar

54.

Check all the properties of metallic bonding.

a)

Malleable

b)

Ductile

c)

Conducts electricity as a solid

d)

Shiny

e)

Good conductor of heat

55.

How does an atom become a charged ion?

a)

gaining or losing protons

b)

gaining or losing electrons

c)

gaining or losing neutrons

d)

by electrical shock

56.

What is a positively charged ion called?

(a)  

57.

How does an atom get a negative charge?

a)

Gain protons

b)

Lose protons

c)

Gain electrons

d)

Lose electrons

58.

Determine the oxidation number or charge of the following element:

Aluminum (Al)

(a)  

59.

Determine the oxidation number or charge of the following element: Lithium (Li)

(a)  

60.

Reduction is the ___________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

61.

What are the seven diatomic elements?

a)

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

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

62.

What are diatomic elements?

a)

Elements that form two-atom molecules when not combined in a compound.

b)

Two elements that combine with one atom from each element.

c)

Elements that are always in pairs no matter what.

63.
Bonds between two nonmetal atoms are 
a)
covalent.
b)
ionic.
c)
incomplete.
d)
complete.

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