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Chemistry final review 23

Total questions: 84

Worksheet time: 1hrs 20mins

Name
Class
Date
1.

A catalyst is

a)

the product of a combustion reaction

b)

not used up in a reaction

c)

one of the reactants in a single-replacement reaction

d)

a solid product of a reaction

2.

What is the mass of 1.2 x 1024 atoms of C?

a)

2.0 grams

b)

24 grams

c)

0.17 grams

d)

1.4 x 1025 grams

3.

What is the molar mass of table salt (NaCl)? Read all options! Be careful!

a)

58.44 amu

b)

35.45 g/mol

c)

22.99 g/mol

d)

58.44 g/mol

4.

Determine the mass of 4.20 moles of C6H12

a)

353 g

b)

0.0499 g

c)

337 g

d)

2.53 x 1024 g

5.

What physical state symbol should be included for oxygen?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

6.
The numbers needed to balance the equation are:
a)
2, 7, 6, 4
b)
2, 1, 3, 2
c)
3, 1, 1, 3
d)
2, 3, 1, 3
7.
The numbers needed to balance the equation are:
a)
1, 1, 1, 2
b)
1, 1, 2, 2
c)
1, 1, 1, 1
d)
2, 3, 1, 3
8.

What physical state symbol should be included for water?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

9.

When two substances react to form products, the reactant which is used up is called the

a)

determining reagent

b)

excess reagent

c)

limiting reagent

d)

catalytic reagent

10.

Avogadro's number of representative particles is equal to

a)

mole

b)

kilogram

c)

kelvin

d)

gram

11.

In every balanced equation, each side of the equation has the same amount of

a)

molecules

b)

coefficients

c)

molecules

d)

atoms of each element

12.

What is the molar mass of (NH4)2CO3?

a)

96g

b)

144g

c)

598g

d)

66g

13.

What does the symbol Δ above the arrow in a chemical equation mean?

a)

water added to equation

b)

heat added to equation

c)

solid added to equation

d)

element added to equation

14.

How many valence electrons does a helium atom have?

a)

3

b)

4

c)

6

d)

2

15.

Which of the following elements forms an ion with a 1- charge?

a)

fluorine

b)

hydrogen

c)

potassium

d)

sulfur

16.

chemical reactions

a)

occur only in living organisms

b)

create and destroy atoms

c)

only occur outside living organisms

d)

produce new substances

17.

what does -ite or -ate ending in a polyatomic ion mean?

a)

sulfur is in the formula

b)

nitrogen is in the formula

c)

oxygen is in the formula

d)

bromine is in the formula

18.

a net ionic equation

a)

shows spectator ions

b)

shows only the particles in volved in the reaction

c)

is not necessarily balanced with respect to mass and charge

d)

shows dissolved ionic compounds as dissociated free ions

19.

How many valence electrons are in a silicon atom?

a)

3

b)

5

c)

4

d)

2

20.

How many moles of CaBr2 are in 5.0 grams of CaBr2?

a)

2.5 x 10-2 mol

b)

3.8 x 10-3 mol

c)

4.8 x 10-2 mol

d)

5.5 x 10-9 mol

21.

Which of the following combinations of symbol and explanation of symbol is correct when used in a chemical equation?

a)

(g), grams

b)

(l), liters

c)

(aq), dissolved in water

d)

(s), solid product

22.

molecular compounds are usually

a)

composed of two or ore transition elements

b)

composed of positive and negative ions

c)

two or more nonmetallic elements

d)

exceptions to the law of definite proportions

23.

When the name of an anion that is part of an acid ends in -ite, the acid name includes the suffix ____.

a)

-ous

b)

-ic

c)

-ite

d)

-ate

24.

The reaction 2Fe + 3Cl2 → 2FeCl3 is an example of which type of reaction?

a)

combustion reaction

b)

single-replacement reaction

c)

combination reaction

d)

decomposition reaction

25.

What is the volume, in liters, of 0.500 mol of C3H8 gas at STP?

a)

0.0335 L

b)

11.2 L

c)

22.4 L

d)

34.6 L

26.

what is the name given to the electrons in the highest occupied energy level of an atom?

a)

orbital electrons

b)

anions

c)

cations

d)

valence electrons

27.

What is the molar mass of AuCl3 ?

a)

96g

b)

130g

c)

232.5g

d)

303.6g

28.

how are chemical formulas of binary ionic compounds generally written?

a)

cation on the left anion on the right

b)

anion on the left cation on the right

c)

roman numerals first, then anion, then cation

d)

subscripts first, then ions

29.

how are bases named?

a)

like monatomic elements

b)

like polyatomic ions

c)

like ionic compounds

d)

like molecular compounds

30.

them chemical formula of an ionic compound shows

a)

how many atoms of each element a molecule contains

b)

the lowest whole-number ration between ions in an ionic compound

c)

which molecules the ionic compound contains

d)

how atoms bond

31.

What type of ions have names ending in -ide?

a)

only cations

b)

only anions

c)

only metal ions

d)

only gases

32.

The equation Mg(s) + 2HCl(aq)→ MgCl2(aq) + H2(g) is an example of which type of reaction?

a)

single-replacement

b)

combustion

c)

double-replacement

d)

combination

33.

How many valence electrons does Carbon have?

a)

4

b)

5

c)

6

d)

8

34.
Positively charged particles found in the nucleus of an atom are called
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
35.
What is the law of Conservation of Mass?
a)
A measure of how much mass is created or destroyed. 
b)
Mass can neither be created nor destroyed during a chemical reaction. 
36.
Negatively charged particles found outside of the nucleus are called
a)
electron
b)
protons
c)
neutrons
d)
nucleons
37.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

38.
Chemical Formulas ...
a)
are written in alphabetical order 
b)
represent the destruction or creation of atoms 
c)
represent how atoms are arranged in a chemical reaction 
39.

Which groups tend to not form ions? Check all that apply

a)

1A

b)

4A

c)

3A

d)

7A

e)

8A

40.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin(IV) Selenide

c)

Tin selenide

d)

Tin(II) triselenide

41.

What is the name of the following compound: Mn2O3

a)

manganese oxide

b)

manganese(II) oxide

c)

manganese(III) oxide

d)

magnesium oxide

42.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper(I) bromide

d)

copper(II) bromide

43.

Which is the correct formula for the compound: lead(II) fluoride

a)

Pb2F

b)

PbF2

c)

PbF

d)

PbF7

44.

What is the what charge of lead in the compound: lead(IV) iodide

a)

+1

b)

+4

c)

+6

d)

-1

45.

LiBr is called

a)

lithium bromine

b)

lithium(I) bromine

c)

lithium bromide

d)

lithuim(I) bromide

46.

What is the name of the following compound: NaCl

a)

sodium chloride

b)

sodium(I) chloride

c)

sodium chlorine

d)

sodium(I) chlorine

47.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium(II) chloride

c)

beryllium chloride

d)

beryllium dichloride

48.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium(II) sulfate

d)

cesium(II) sulfide

49.

The name of FeCl₂ is

a)

iron chloride

b)

iron(II) chloride

c)

iron(I) chloride

d)

iron dichloride

50.

What is the name of the following compound: K2SO4

a)

potassium sulfur

b)

potassium sulfate

c)

potassium(I) sulfate

d)

potassium(II) sulfide

51.
What is the formula for copper (II) hydroxide?
a)
CuOH
b)
Cu(OH)2
c)
Cu2OH
d)
Cu2O
52.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
53.

If I gain electrons I become

a)

Positive because I've added to my atom

b)

negative because I've added electrons

c)

same because i'm balanced

d)

equal because now I have electrons

54.
What is the correct term for "atom with more protons than electrons"?
a)
positive ion (cation)
b)
negative ion (anion)
c)
neutral atom
d)
stable atom
55.
How many valence electrons for Ca?
a)
1
b)
2
c)
3
d)
4
56.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
57.
If an atom does not have a stable octet, what will it do?
a)
form bonds with other atoms
b)
nothing
c)
fall apart
d)
gain or lose protons
58.

Select each compound that can be produced by combustion reactions. (more than 1 answer)

a)

Oxygen

b)

Carbon Dioxide

c)

Water

d)

Glucose

e)

Carbon

59.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

60.

Identify the type of chemical reaction pictured above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

61.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

62.

Identify the type of reaction...

(NH4)2CrO4 +2 KOH −> 2NH4OH + K2CrO4\left(NH_4\right)_2CrO_4\ +2\ KOH\ ->\ 2NH_4OH\ +\ K_2CrO_4

a)

Composition

b)

Decomposition

c)

Single Replalcement

d)

Double Replacement

e)

Combustion

63.

Identify the type of chemical reaction pictured above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

64.

Identify the type of reaction...

C4H10 + O2 −>C_4H_{10}\ +\ O_2\ ->

a)

Composition

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

65.

Identify the type of reaction...

N2O5 +H2O −>N_2O_5\ +H_2O\ ->

a)

Composition

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

66.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

67.

Find the mass of 5.82 mol of MgCl2. Round to the nearest tenth.

a)

552.9 g

b)

436.8 g

c)

55.2 g

d)

555.9 g

68.

Determine the number of moles in 1.50 grams of copper metal.

a)

1.50 grams

b)

0.023 moles

c)

42.4 moles

d)

6.02x1023

69.

How many grams does 0.50 moles of silicon dioxide (SiO2) weigh?

a)

2.0 g

b)

0.50 g

c)

60.1 g

d)

30.0 g

70.

Determine the number of moles of KNO3 that are in 784 g of the compound.

a)

7.7 mol

b)

6.9 mol

c)

10.6 mol

d)

7.8 mol

71.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

72.

Which of the following dimensional analysis setups will correctly convert 27.76 g of Li to atoms of Li?

a)

A

b)

B

c)

C

d)

D

73.

How many moles are in 98.3 grams of aluminum hydroxide, Al(OH)3?

a)

1.26 moles

b)

0.8 moles

c)

7,670 moles

d)

1.63 x 10-22 moles

74.

How many formula units are in 2.5 moles of NaCl?

a)

1.5 x1024 formula units

b)

1.5 formula units

c)

4.2 formula units

d)

4.2 x10-24 molecules

75.

How many moles of Fe are reacted to produce 50 moles of FeCl3?

a)

36.67 moles Fe

b)

75 moles Fe

c)

25 moles Fe

d)

50 moles Fe

76.

Which reactant is the limiting reagent and why?

2H2(g) + O2(g) → 2H2O(l)

a)

Hydrogen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.

b)

Oxygen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.

77.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
78.

4NH3+6NO --> 5N2 + 6H2O


What is the limiting reactant if 10 moles of NH3 react with 30.0 moles of NO?

a)

NH3

b)

NO

c)

N2

d)

water

79.

The limiting reactant

a)

slows the reaction down

b)

is used up first

c)

is the reactant that is left over

d)

controls the speed of the reaction

80.
Is the following compound an acid or a base? 
Ca(OH)2
a)
Acid
b)
Base
81.

When the polyatomic ion in an acid ends in -ate, the root name of the polyatomic ion is followed by the ending -_____.

a)

ide

b)

ic

c)

ous

d)

ite

82.

The cation in an acid is always

a)

a metal

b)

hydrogen

c)

hydroxide

d)

negatively charged

83.
Nitrous Acid
a)
HNO2
b)
H2NO2
c)
HNO3
84.
Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide

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