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Final Exam Review (without organic)

Total questions: 66

Worksheet time: 50mins

Name
Class
Date
1.

Which of the following atoms will bond ionically with Na

a)

F

b)

S

c)

K

d)

O

2.

The atom Carbon has how many valence electrons?

a)

6

b)

12

c)

8

d)

4

3.

Which chemical needs a 2 in front of it in the following reaction: Mg + HCl --> MgCl2 + H2

a)

Mg

b)

HCl

c)

MgCl2

d)

H2

4.

A reaction has a change in enthalpy value of 253 kJ/mol. This is an example of

a)

an endothermic reaction

b)

an exothermic reaction

5.

Electron pairs that do not take part in a covalent bond are referred to as

a)

free electrons

b)

floating electrons

c)

electron pairs

d)

lone pair electrons

6.

What charge must X have in the ionic compound LiX

a)

+1

b)

-1

c)

+2

d)

+3

7.

In this chemical equation, the elements in red are the_______.

a)

Products

b)

Reactants

c)

Subscripts

d)

Coefficients

8.
What is a valence electron?
a)
an electron that is found in the outermost orbital of an atom. 
b)
an electron found in the innermost orbital of an atom.
c)
an electron found in the middle orbital.
9.

An ionic bond forms when

a)

valence electrons are shared back and forth (move between) two atoms.

b)

a sea of mobile electrons surround the cations and they then become negativly charged

c)

valence electrons are transferred from one atom to another, forming charged ions that are then pulled together by attraction between opposite charges

d)

none of the above

10.

Covalent bonds form when

a)

the electronegativity difference between two atoms is very large.

b)

electrons are completely transferred between two atoms.

c)

pairs of electrons are shared between two atoms.

d)

ions are held together by opposite charges.

11.

The pH Scale measures:

a)

Positive or negative ions

b)

Acids and Bases

c)

Electricity

d)

None of These

12.

In saltwater, the water is the:

a)

Solute

b)

Solvent

c)

Wet Stuff

d)

None of these

13.

Calcium carbonate has a pH of 9, it is a:

a)

Acid

b)

Base

c)

Neutral

d)

None of these

14.

used to separate a solid substance from a fluid by passing a mixture through a porous material such as filter

a)

filtration

b)

decantation

c)

distillation

d)

evaporation

15.

what is the common name of the compound dihydrogen monoxide?

a)

table salt

b)

water

c)

table sugar

d)

chalk

16.
The pH of a solution is tested, and it is found to be a basic solution. Of the following choices, what could the pH have been?
a)
3
b)
9
c)
7
d)
5
17.
Many cleaning solutions are bases. Which of the following is a property of most bases?
a)
feels slippery
b)
white color
c)
can only be liquid
d)
tastes sour
18.
Pure water has a pH of 7. Pure water _______.
a)
is a base
b)
is a neutral substance
c)
could be either an acid or a base
d)
is an acid
19.
Tastes Sour
a)
Acids
b)
Bases
c)
Salts
d)
All
20.
Forms hydroxide ions in water
a)
Acids
b)
Bases
c)
All
21.
pH less than 7.
a)
Acids
b)
Bases
c)
All
22.
What is a solution that has an excess of hydroxide (OH-) ions?
a)
pH
b)
acid
c)
neutral
d)
base
23.
Acids are found on the pH scale between which numbers?
a)
0-7
b)
7
c)
7-14
d)
19-42
24.
An acid/base reaction always produces:
a)
H2
b)
H2O
c)
NaCl
d)
H3O+
25.
BASE + ACID ----> SALT +?
a)
water
b)
oxygen
c)
hydrogen ion
d)
hydroxide ion
26.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
d)
lye
27.
Dilute solutions taste sour
a)
Acid
b)
Base
28.

What is the vocab term for the quantity of heat needed to raise the temperature of 1g of a substance by 1°C?

a)

Joule

b)

Specific Heat

c)

Heat Capacity

d)

calorie

29.

What is the standard unit for heat?

a)

Calorie

b)

calorie

c)

Joule

30.

How does energy flow?

a)

It goes from hot to cold

b)

It goes from cold to hot

c)

It transfers without any particular means

d)

It doesn't flow

31.

How does energy change in a reaction?

a)

It changes mass

b)

It increases

c)

It decreases

d)

It transfers

32.

Does the total energy change in a reaction?

a)

NEVER

b)

Yes, it increases

c)

Yes, it decreases

d)

Yes, but some increases and some decreases

33.

How many calories of heat are required to raise the temperature of 225g of Al from 20°C to 100°C? (specific heat of Al = 0.21 cal/g°C)

a)

590 calories

b)

3800 calories

c)

38000 calories

d)

85000 calories

34.

A 100 g piece of heated steel cools from 50°C to 20°C. How much heat is released to the surroundings?

a)

300 J of heat are released

b)

300 cal of heat are released

c)

The amount cannot be calculated because the heat capacity isn't known

d)

The amount cannot be calculated because the system isn't closed

35.

During a phase change temperature...

a)

may increase or decrease

b)

increase

c)

decreases

d)

stays the same

36.

The symbol for specific heat is .......

a)

C

b)

q

c)

m

d)

T

37.
A material was cooled from 100ºC to 40ºC.  What is the temperature change?
a)
60ºC
b)
40ºC
c)
-60ºC
d)
-40ºC
38.

The specific heat of copper is 0.39 J/g °C. What is the temperature change when 100 Joules of heat is added to 20 grams?

a)

12.82 °C

b)

24.12°C

c)

351 °C

39.

Calculate the ∆H for the following reaction: 2H2O2 → 2H2O + 1 O2

You are given these two equations:

2H2 + O2 → 2H2O ∆H = -572 kJ

H2 + O2 → H2O2 ∆H = -188 kJ

a)

∆H = -948 kJ

b)

∆H = -196 kJ

c)

∆H = -384 kJ

d)

∆H = -188 kJ

40.

Refer the the following question:

2N2 + 3H2 --> 2NH3 + 46 kJ

How much energy would be produced if only 14.0 g of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

41.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
42.

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

a)

Limiting Reactant

b)

Excess Reactant

c)

Highly Reactant

d)

Super Reactant

43.

A limiting reactant is a reactant that.....

a)

runs out during a chemical reaction

b)

causes a reaction to stop

c)

determines the amount of products that can be made

d)

all of these

44.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of iron can be made from 6 moles H2 and excess Fe2O3?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

45.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 3 moles of Fe2O3?
a)
6 moles Fe
b)
4 moles Fe
c)
2 moles Fe
d)
1 moles Fe
46.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron (Fe) can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
47.
Write the formula for copper (I) phosphide?
a)
Cu3P
b)
CuP
c)
Cu1P
d)
CuP3
48.
Write the formula for vanadium (IV) carbonate
a)
V(CO3)2
b)
V4C
c)
V(CO3)4
d)
V4(CO3)
49.
Name this compound:
Li2SO3
a)
Lithium sulfate
b)
Lithium sulfite
c)
Lithite sulfide
d)
Sulfur lithite
50.
What is the formula for copper (II) sulfate?
a)
Cu2SO4
b)
CuSO3
c)
CuS
d)
CuSO4
51.
What is the formula for silver nitrate?
a)
Ag3NO
b)
AgNO3
c)
Ag(NO3)2
d)
Ag2NO3
52.
What is the formula for iron (III) chloride
a)
FeCl
b)
FeCl3
c)
FeClO3
d)
Fe3Cl
53.

What is the formula for potassium sulfite?

a)

K2SO4

b)

KSO3

c)

KSO4

d)

K2SO3

54.
What is the formula for manganese (II) chloride?
a)
MgCl2
b)
MnCl2
c)
Mn2Cl
d)
MnCl
55.
Name this compound: 
NH4F
a)
Ammonia fluoride
b)
Ammonium fluorite
c)
Ammonia fluorate
d)
Ammonium fluoride
56.
What is the formula for lead (II) iodide
a)
PbI
b)
PbI2
c)
Pb2I
d)
LbI2
57.
What is the formula for barium hydroxide?
a)
BaOH
b)
Ba(OH)2
c)
BaOH2
d)
Ba2(OH)2
58.

What is the fomula of carbonic acid?

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

59.

What is the formula of chlorous acid?

a)

HClO3

b)

HClO2

c)

HClO

d)

HCl

60.

The correct name of the acid with the chemical formula HI is ___.

a)

iodic acid

b)

hydroiodic acid

c)

iodous acid

d)

hypoiodous acid

61.

The correct name of the acid with the formula H2SO3 is ____;

a)

sulfuric acid

b)

hydrosulfuric acid

c)

sulfurous acid

d)

persulfuric acid

62.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
63.

State the name of the acid with the formula H2S

a)

sulfuric acid

b)

sulfurous acid

c)

hydrosulfuric acid

d)

hydrosulfurous acid

64.

State the name of the acid with the formula HC2H3O2

a)

acetic acid

b)

acetous acid

c)

hydrogen acetate

d)

hydrogen dicarbon trihydrogen dioxygen

65.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
66.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide

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