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Final Exam Practice

Total questions: 75

Worksheet time: 38mins

Name
Class
Date
1.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
2.
How many significant figures does the following number have: 100.3
a)
4
b)
3
c)
5
d)
2
3.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
4.
Which lists metric units, in order, from smallest to largest?
a)
milligram, centigram, gram
b)
kilogram, gram, centigram
c)
decagram, hectogram, milligram
d)
kilogram, hectogram, decagram
5.

When Joselyn went to the store she bought 2.7kg of salt water taffy. What does Joselyn need to do to find out how many grams she bought?

a)

Divide by 1000

b)

Multiply by 1000

c)

Divide by 100

d)

Multiply by 100

6.

Which of the following would be considered a physical change?

a)

Cutting paper

b)

pH test

c)

Burning marshmellow

d)

Roasting a Turkey

7.

Which of the following would be considered a physical property?

a)

Colour

b)

Flammability

c)

pH

d)

Reactivity

8.
No Definite Shape and No Definite Volume
a)
Gas
b)
Liquid
c)
Solid
9.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
rust
10.
Digesting your food is an example of 
a)
chemical change
b)
physical change
11.

In which type of bond do atoms share electrons unequally?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

d)

Polar covalent bond

12.

Which of the following is a chemical change?

a)

Boiling water

b)

Dissolving sugar in water

c)

Rusting of iron

d)

Melting ice

13.

Which group do the alkaline metals belong to?

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

14.

Atoms of the same element that have different numbers of neutrons are called __________.

a)

Compounds

b)

Molecules

c)

Isotopes

15.

The number of protons in an atom is the __________.

a)

Mass number

b)

Atomic number

c)

Atomic mass

16.

The __________ is the number of protons and neutrons in an atom.

a)

Mass number

b)

Atomic number

c)

Atomic mass

17.

True or false?  Elements in the same group/family have similar properties.

a)
True
b)
False
18.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

19.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

20.

How many protons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

21.

How many neutrons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

22.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
23.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

24.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
25.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
26.

How many atoms are there in H2SO4 ?

a)

6

b)

5

c)

7

d)

3

27.

How many Nitrogen atoms are in the in H2C3O4N5?

a)

2

b)

3

c)

4

d)

5

28.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

29.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

30.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

31.
MgS 
a)
Magnesium sulfide
b)
Monomagnesium monosulfide
c)
Magnesium monosulfide
32.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
33.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
34.

What type of bond is formed between nitrogen and oxygen?

a)

Metallic

b)

No bond will form

c)

Ionic

d)

Covalent

35.

What is happening to the electrons during a covalent bond?

a)

The electrons are being shared

b)

One element is taking electrons, another is giving away electrons

c)

The electrons don't move

d)

Both atoms give away electrons

36.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
37.
Metals and nonmetals form which kind of bond?
a)
Polar covalent
b)
Ionic
c)
Non-polar covalent
d)
Metallic
38.

What is a valence electron?

a)

an electron that is found in the outermost energy level of an atom

b)

an electron found in the innermost energy level of an atom

c)

an electron found in the middle energy level

d)

an electon found in the nucleus

39.
__Na + __Cl2 --> __NaCl
a)
1,1,2
b)
2,1,2
c)
2,1,1
d)
already balanced
40.
__NaClO3 --> __NaCl + __O2
a)
2,2,2
b)
2,2,3
c)
3,2,2
d)
1,2,3
41.
__BF3 + __Li2SO3 --> __B2(SO3)3 + __LiF
a)
2,3,1,3
b)
2,3,1,6
c)
4,4,2,12
d)
3,3,1,9
42.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
43.

What id the molar mass of UF6?

a)

101 g/mol

b)

238 g/mol

c)

257 g/mol

d)

352 g/mol

44.

Calculate the molar mass of CO2.

a)

14 g/mol

b)

28 g/mol

c)

36 g/mol

d)

44 g/mol

45.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

46.

Calculate the molar mass of NH4NO2

a)

50 g/mol

b)

60 g/mol

c)

64 g/mol

d)

78 g/mol

47.

Which of the following is NOT a property of noble gases?

a)

They have a complete outer shell.

b)

They are highly reactive.

c)

They are colorless, odorless, and tasteless.

d)

They exist as monatomic gases at room temperature.

48.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
49.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
50.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
51.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
52.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
53.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
54.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
55.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

56.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

57.

you have an unknown compound with an Empirical Formula of CF2. The Molecular formula mass of the compound is 192 g/mol. What is the Molecular Formula of the compound?

a)

C4F8

b)

C8F4

c)

C3F6

d)

C2F4

58.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
59.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
60.
What is the percent composition of Benzene, C6H6?
a)
C = 50%
H = 50%
b)
C = 85.7 %
H = 14.3%
c)
C = 92.2%
H = 7.8%
d)
C = 71.9%
H = 28.1%
61.
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
62.
Acids are found on the pH scale between which numbers?
a)
0-7
b)
7
c)
7-14
d)
19-42
63.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
64.

What is the molarity of a solution containing 20.0 grams of CaCl2 in 600ml of solution?

a)

0.0003M

b)

0.11M

c)

0.30M

d)

0.18M

65.

Which of the following is not a way to increase the rate of solvation?

a)

Increasing the temperature of the solution

b)

Increasing the surface area of the solute

c)

Mixing the solution thoroughly

d)

Cooling down the solvent

66.

If 70g of CaCl2 is dissolved in 100g of water at 20°C, what kind of solution is created?

a)

unsaturated

b)

saturated

c)

supersaturated

d)

none of the above

67.

Consider the reaction NH3 + H2O ⇌ NH4+ + OH-. Which species is the acid?

a)

NH3

b)

H2O

c)

NH4+

d)

OH-

68.

How would you define an Arrhenius base?

a)

a substance that donates an H+

b)

a substance that ionizes to produce OH-

c)

a substance that accepts an H+

d)

a substance that ionizes to produce H+

69.

In the reaction below, what species is the conjugate acid? CO32−+H2O↔HCO3−+OH−CO3^{2-} + H2O \leftrightarrow HCO3^{-} + OH^{-}

a)

CO32−CO3^2-

b)

OH−OH^{-}

c)

HCO3−HCO3^{-}

d)

H2O

70.

What is the pH of a 3.6x10−43.6x10^{-4} M solution of HCl?

a)

3.4

b)

5.7

c)

7.8

d)

10.8

71.

When electrons move to a higher energy level, they are in a/an ___________.

a)

Photon

b)

Ground State

c)

Excited State

d)

Energy

72.

how many electrons fit into a P orbital

a)

2

b)

3

c)

6

d)

4

73.

Identify the element

a)

Sulfur

b)

Oxygen

c)

Selenium

d)

Phosphorus

74.
 Groups contain the same amount of ___________________ electrons, and periods contain the same number of ____________________shell.
a)
 atom/ electron
b)
valence/electron
c)
electron /valence
d)
protons/neutrons  
75.

The octet rule states that, to be a stable compound, atoms want:

a)

to be like a noble gas.

b)

more protons than electrons

c)

less than eight valence electrons

d)

more electrons than protons

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