Free Printable Spring Final Exam Review

1.

What is the mass number of the following element?

a)

20 amu

b)

2882 amu

c)

Ca

d)

40. amu

2.

Going across a period from left to right, the size of the atomic radii...

a)

stay the same

b)

are unpredictable

c)

increases

d)

decreases

3.

The number of neutrons in an atom of Bi-211 is

a)

128

b)

209

c)

83

d)

2

4.

Malleable, shiny, and ductile describe

a)

nonmetals

b)

halogens

c)

sulfur

d)

alkali metals

5.

Mendeleev's periodic table was organized based on

a)

atomic number

b)

atomic mass

c)

valence electrons

d)

x-ray results

6.

The most electronegative element on the periodic table is

a)

potassium

b)

hydrogen

c)

fluorine

d)

oxygen

7.

For Gold (Au), 79 represents

a)

mass number

b)

number of electrons

c)

atomic number

d)

avg atomic mass

8.

In general, which properties are common to elements within a single group on the periodic table?

a)

atomic number and atomic weight

b)

chemical properties and ability to bond to other atoms

c)

color and luster

d)

boiling point and freezing point

9.

Horizontal rows of the periodic table are called

a)

periods

b)

columns

c)

groups

d)

families

10.

Which is an example of a nonmetal?

a)

copper

b)

phosphorus

c)

mercury

d)

cadmium

11.

Valence electrons are

a)

outer level electrons

b)

found only in metals

c)

the amount of electrons short of a full level

d)

always "s" orbit electrons

12.

What phase change occurs during condensation?

a)

solid to liquid

b)

liquid to gas

c)

liquid to solid

d)

gas to liquid

13.

Changing a subscript in a correctly written chemical formula will

a)

change the electron configuration of that element

b)

change the charges on the other ions in the compound

c)

change the formula so that it no longer represents the same compound

d)

have no effect on the formula

14.

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

a)

cation

b)

polyatomic ion

c)

oxyanion

d)

anion

15.

The oxidation number for Mg in MgO is

a)

+1

b)

-1

c)

-1

d)

+2

16.

Formula for silicon dioxide

a)

$SO_2$

b)

$SiO_2$

c)

$Si_2O_2$

d)

SiO

17.

$N_2O_4$

a)

Nitride oxide

b)

Mononitrogen hexoxide

c)

Dinitrogen tetroxide

d)

Nitrogen oxide

18.

CO

a)

Monocarbon oxide

b)

Carbon dioxide

c)

Carbon monoxide

d)

Chlorine oxide

19.

Molar mass of carbon dioxide (CO2)

a)

44.0 g/mol

b)

28.0 g/mol

c)

40 g/mol

d)

12.0 g/mol

20.

What is the mass of 0.240 mol glucose, $C_6H_{12}O_6$ ?

a)

750 g

b)

.00133 g

c)

180 g

d)

43.2 g

21.

What part is the cation in sodium oxide?

a)

S

b)

Na

c)

Oxygen

d)

moles

22.

How many atoms are present in the compound (NH4)3N?

a)

9

b)

11

c)

16

d)

13

23.

To balance a chemical equation, you should adjust the

a)

coefficients

b)

subscripts

c)

formulas of the products

d)

number of products

24.

In a chemical equation, the symbol (aq) indicates that the substance is

a)

water

b)

dissolved in water

c)

an acid

d)

insoluble

25.

In a reaction, the ions of two compounds exchange places in aqueous solution to form two new compounds. This reaction is called a

a)

synthesis reaction

b)

decomposition reaction

c)

single displacement reaction

d)

double displacement reaction

26.

What type of chemical reactions is: CaO(s) + H2O(l) → Ca(OH)2(s)

a)

synthesis

b)

decomposition

c)

single replacement

d)

combustion

27.

Balance this chemical equation: __ AgNO3 + __ CuCl2 → __ AgCl + __ Cu(NO3)2

a)

2,2,1,2

b)

1,2,1,2

c)

1,3,1,2

d)

2,1,2,1

28.

Balance this chemical equation: ___ PbO2 → ___ PbO + ___ O2

a)

2,2,1

b)

3,3,1

c)

4,2,2

d)

1,1,1

29.

What is generally found on the left side of the equation?

a)

reactants

b)

products

c)

coefficients

d)

subscripts

30.

Balance the equation and choose the type of reaction: __ Cs + __ N2 --->__ Cs3N

a)

2,2,2 synthesis

b)

2,3,1 decomposition

c)

3,2,3 single replacement

d)

6,1,2 synthesis

31.

Balance the following chemical equation: ___ BaCO3 -->___ BaO + ___ CO2

a)

2,2,2

b)

2,2,3

c)

1,1,1

d)

3,2,1

32.

In the equation 6CO2 + 6H2O → C6H12O6 + 6O2, the mole ratio of water to oxygen is

a)

2:1

b)

1:1

c)

3:2

d)

6:8

33.

For the reaction represented by the equation N2 + 3H2→ 2NH3, how many moles of nitrogen are required to produce 18 mol of NH3?

a)

9

b)

18

c)

27

d)

36

34.

In the reaction represented by the equation 2Na + 2H2O → 2NaOH + H2, how many grams of hydrogen are produced if 120. g of Na and 80.0 g of H2O are available?

a)

5.21 g H2

b)

2.60 g H2

c)

4.48 g H2

d)

2.23 g H2

35.

Reaction: 2As2O3 + 3C → 3CO2 + 4As

If 8.0 mol As2O3 reacts with excess carbon, the theoretical yield of the above reaction is

a)

32 mol As

b)

16 mol As

c)

8 mol As

d)

4 mol As

36.

For the reaction 2H2 + O2 → 2H2O, how many moles of water can be produced from 6.0 mol of oxygen?

a)

6.0 mol H2O

b)

2.0 mol H2O

c)

12 mol H2O

d)

3.0 mol H2O

37.

Given the reaction represented by the following unbalanced equation: N2O(g) + O2(g) → NO2(g) What is the mole ratio of NO2 to O2?

a)

2:3

b)

3:4

c)

4:3

d)

1:2

38.

The volume of 1 mole of a gas at STP is

a)

760 mL

b)

22.4 L

c)

100 mL

d)

dependent on the type of gas

39.

How many mL are in 3 L?

a)

100

b)

1000

c)

3000

d)

3

40.

Convert 2000 grams to kg:

a)

2 kg

b)

20 kg

c)

2000 kg

d)

4000 kg

41.

What word describes when water is attracted to other substances?

a)

Cohesion

b)

Adhesion

c)

Capillary action

d)

Surface tension

42.

When water molecules stick easily to other water molecules, this is called what?

a)

Cohesion

b)

Adhesion

c)

Solution

d)

Polar molecule

43.

The fact that ice floats on liquid water is due to the fact that water's solid form is _____________ than its liquid form.

a)

Less polar

b)

More polar

c)

Less dense

d)

More dense

44.

Water is a universal solvent because it...

a)

It can be found anywhere

b)

It freezes when it gets cold

c)

floats when frozen

d)

Dissolves most substances

45.

$O_2\left(g\right)\ +\ 2\ H_2\ \left(g\right)\ \rightarrow\ 2\ H_2O\ \left(g\right)\ +\ Energy$

a)

endothermic

b)

exothermic

46.

$6\ CO_2+\ 6\ H_2O\ +\ Energy\ \rightarrow\ C_6H_{12}O_6\ +\ 6\ O_2$

a)

endothermic reaction

b)

exothermic reaction

Spring Final Exam Review

Total questions: 46

Worksheet time: 28mins

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