Free Printable Chemistry Final Exam

1.

What is the volume of a piece of zinc with measurements 5.0 cm x 5.0 cm x 5.0 cm?

a)

15 cm³

b)

125 cm³

c)

15 cm

d)

125 cm

2.

What is the volume of the fluid in the graduated cylinder shown?

a)

12.0 ml

b)

13.0 ml

c)

13.5 ml

d)

12.5 ml

3.

Different substances can often be identified by their density. Density is a derived unit equal to:

a)

mass x volume

b)

volume / mass

c)

length x width x height

d)

mass /volume

4.

All of the following are physical changes except:

a)

Melting

b)

burning

c)

condensing

d)

vaporizing

5.

If the graph represents the energy of the reactants and products of a chemical reaction, which of the following is true of the reaction?

a)

there is an exothermic reaction

b)

there is an endothermic reaction

c)

the activation energy is lower than the energy released

d)

the total energy is higher than the starting energy

6.

Atoms in a _______ are closely packed vibrating particles.

a)

plasma

b)

liquid

c)

solid

d)

gas

7.

1 ml is the same as which af the following? (Mark all that apply)

a)

1 cc

b)

1 cm³

c)

1 $\mu l$

d)

1 dm³

8.

Increasing the temperature of a substance causes the particles to speed up and can cause all of the following except:

a)

condensing

b)

vaporizing

c)

melting

d)

boiling

9.

Which is NOT a chemical property?

a)

iron will react with oxygen

b)

white phosphorus is very flammable

c)

copper is malleable (can be bounded into sheets) and ductile (can be pulled into wire)

d)

lead is toxic

10.

Which is a Physical Change?

a)

iron is oxidized to become rust (iron oxide)

b)

carbon products are usually combustible

c)

Decomposition is a necessary reaction

d)

dissolving substances is often the 1st step in any procedure

11.

There are seven naturally occurring diatomic elements; which of the following is NOT a diatomic element?

a)

H

b)

O

c)

Cl

d)

N

e)

C

12.

A _________ is a pure substance made of different elements that are chemically combined into a new substance.

a)

mixture

b)

ion

c)

compound

d)

atom

13.

A material that is made of different substances that are NOT chemically combined is called a(an)

a)

compound

b)

mixture

c)

ion

d)

atom

14.

In a solution, the substance that causes the dissolving is known as a ________

a)

solute

b)

solvent

c)

suspension

d)

colloid

15.

_________ mixtures are evenly blended and appear to be the same throughout.

a)

homogeneous

b)

heterogeneous

16.

A mixture, like salt water, containing one substance dissolved in another, is known as a ____________ (mark all that apply).

a)

homogeneous mixture

b)

solution

c)

suspension

d)

colloid

17.

The two main parts of an atom are the:

a)

principle energy levels and sublevels

b)

nucleus and energy levels

c)

planetary electrons and energy levels

d)

nucleus and kernel

18.

The number of electrons in the 2nd principal energy level, n=2, of an atom is:

a)

4

b)

2

c)

8

d)

18

19.

An atom of beryllium contains 4 protons, 5 neutrons, and 4 electrons. What is the mass number of this atom?

a)

13

b)

9

c)

8

d)

5

20.

A substance that contains only one type of atom is known as a(n) ______(Mark all that apply)

a)

compound

b)

element

c)

Pure substance

d)

Mixture

21.

A can of baking powder reads: "Ingredients- cornstarch, sodium bicarbonate, calcium acid phosphate, and sodium aluminum sulfate." Baking soda is a

a)

compound

b)

mixture of compounds

c)

molecule

d)

mixture of elements

22.

A 220 g piece of metal was submerged in a graduated cylinder containing 50 ml of water. The level of the water rose to 150 ml. What is the density of the metal?

a)

2.2 g/ml

b)

0.45 ml/g

c)

320 g/ml

d)

20 g/ml

23.

Chlorine is represented by the electron dot structure shown in the picture. Which other atom(s) would have the same atomic dot structure? (Mark all that apply)

a)

Iodine

b)

Oxygen

c)

Sodium

d)

Fluorine

24.

Elements in the same column of the periodic table always have the same # of _______ as one another.

a)

Protons

b)

Neutrons

c)

Electrons

d)

Valence Electrons

25.

Which has the greater Electronegativity:

N or C?

a)

C

b)

N

26.

Which group of the periodic table is composed of inert (not reactive) gases?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

27.

If an atom loses two electrons what charge will it have?

a)

+ 2

b)

- 2

c)

+1

d)

-1

28.

Which two statements are correct about the figure shown?

a)

It is a covalent bond.

b)

Hydrogen atoms loss electrons and Carbon gains the atoms.

c)

It happens on metal and on another non-metal.

d)

The valence electrons are shared by both atoms.

29.

Predict the bond that will form between Be and F.

a)

Ionic

b)

Covalent

c)

metallic

30.

An electron dot diagram consists of the symbol representing the element and an arrangement of dots that usually shows

a)

the atomic number

b)

the atomic mass

c)

the number of neutrons

d)

the number of valence electrons

31.

What element on the periodic table has 16 protons?

a)

germanium Ge

b)

phosphorus P

c)

oxygen O

d)

sulfur S

32.

Which element easily gives up 1 electron to form a cation with +1 charge?

a)

F

b)

Cl

c)

Mg

d)

Li

33.

Which atom will have the strongest affinity for electrons, becoming an anion with a -1 charge?

a)

K

b)

F

c)

O

d)

Fe

34.

Where on the periodic table do you find elements that form the strongest bases?

a)

left

b)

right

c)

middle

d)

inert gases

35.

If two atoms bond in such a way that one-member beomes a positive cation and the other a negative anion, what type of bond is formed?

a)

ionic bond

b)

covalent bond

c)

polar bond

d)

Vanderwaals bond

36.

Isotopes are atoms with different numbers of ________.

a)

protons

b)

neutrons

c)

electrons

37.

The first scientist to show that atoms emit tiny negative particles was

a)

J J Thomson

b)

Ernest Rutherford

c)

James Chadwick

d)

Neils Bohr

38.

The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is

a)

JJ Thomson

b)

Ernest Rutherford

c)

Neils Bohr

d)

John Dalton

39.

This scientist is responsible for the model that we use today to illustrate and help understand the atoms' energy levels.

a)

JJ Thomson

b)

Ernest Rutherford

c)

Neils Bohr

d)

John Dalton

40.

Which of the following parts of Dalton's atomic theory are no longer entirely correct? (Mark all that apply)

a)

atoms are small indestructible particles

b)

all atoms of an element are alike and different from atoms of other elements

c)

compounds are made of elements combined in different ratios of elements

d)

chemical reaction occur that rearrange elements but do not destroy them

41.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

42.

If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?

a)

12 neutrons

b)

12 electrons

c)

12 protons

d)

24 protons and neutrons

43.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

44.

Which Bohr model represents Neon?

a)

b)

c)

d)

45.

What atom matches this electron configuration?

1s²2s²2p⁶3s²

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

46.

Solve this equation for alpha decay.

₈₅²⁰⁹At = ___ + ₂⁴He

a)

₈₃²⁰⁵Bi

b)

₈₆²⁰⁹Rn

c)

₈₁²⁰⁷Tl

d)

₈₅²⁰⁸At

47.

According to the graph, what fraction of the original parent isotope still exists after 3 half lives?

a)

0,5000 g

b)

0,2500 g

c)

0,1250 g

d)

0.0625 g

48.

The total number of oxygen atoms indicated by the formula Fe₂ (CO₃)₃ is

a)

12

b)

6

c)

9

d)

3

e)

18

49.

The correct name for LiCl is

a)

lithium monochloride

b)

lithium chloride

c)

lithium I chloride

d)

monolithium monochloride

50.

What would be the proper chemical formula for combining Al³⁺ and l^- :

a)

Al l₃

b)

Al₃l

c)

Al l

d)

Al₃l₃

51.

What charge does a calcium (Ca) ion have?

a)

+1

b)

+2

c)

+3

d)

+4

52.

The chemical formula for an ionic compound of potassium and oxygen is

a)

KO.

b)

K₂O.

c)

K₂O₂.

d)

KO₂.

53.

Name the following ionic compound: BeCl₂

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

54.

Name the following ionic compound: MgSO₄

a)

magnesium sulfoxide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium oxide

55.

What is the chemical formula for Tetraphosphorous Pentachloride ?

a)

₄P₅Cl

b)

PCl

c)

P4Cl₅

d)

none of the above

56.

What is the name of N₂O₃

a)

Nitrogen trioxide

b)

Dinitrogen oxide

c)

Dinitrogen trioxide

d)

Nitrogen oxide

57.

Cu + 2Ag(NO₃) → 2Ag + Cu(NO₃)

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

58.

The correct name for FeO is

a)

iron III oxide

b)

iron II oxide

c)

iron monoxide

d)

iron I oxide

59.

Which of the following is NOT the correct chemical formula for the compound named?

a)

calcium sulfate CaSO₄

b)

beryllium oxide BeO

c)

ammonium chromate (NH₄)₂CrO₄

d)

lead(II) dinitrate Pb(NO₃)₂

60.

The correct formula for the ammonium ion is

a)

NH4

b)

N4H+

c)

NH4+

d)

Am+

61.

The carbonate ion has the formula CO₃^2-. What is the correct formula for sodium carbonate?

a)

Na(CO₃)₂

b)

Na₂(CO₃)₂

c)

Na₃(CO)₂

d)

Na₂CO₃

62.

A phosphorus atom needs to gain _____ electrons to achieve a noble gas configuration and has an oxidation number of ______

a)

5, -3

b)

3, -3

c)

3, -5

d)

3, +5

63.

What coeffiecient could be added in fron of the silver (Ag) reactant to balance the equation:

$\ldots Ag\ +\ H_2S\ \rightarrow\ Ag_2S\ +\ H_2$

a)

2

b)

3

c)

4

d)

none

64.

Sodium reacts with chlorine to produce sodium chloride (table salt). Which of the equations below is the proper balanced equation?

a)

$Na\ +\ Cl\ \rightarrow\ NaCl$

b)

$Na\ +\ Cl_2\ \rightarrow\ 2NaCl$

c)

$Na\ +\ Cl_2\ \rightarrow\ NaCl$

d)

$2Na\ +\ Cl_2\ \rightarrow\ 2NaCl$

65.

Methane and oxygen react in a combustion reaction releasing carbon dioxide. Complete the balanced equation.

$CH_4\ +\ 2O_2\ =>\ CO_2\ \ +\$

a)

$CH_4+2O_2\ =>\ CO_2\ +H_2$

b)

$CH_4+2O_2=>CO_2\ +2H_2O\$

c)

$2CH_4+2O_2=>CO_2\ +4H_2+CO$

66.

Which of the following is a synthesis reaction?

a)

$2Mg\ +\ O_2\ \rightarrow\ \ 2MgO$

b)

$2Al+6HCl\rightarrow2AlCl_3\ +3H_2$

c)

$2ZnS+3O_2\rightarrow2ZnO+2SO_2$

d)

$PCl_5\ \rightarrow\ PCl_3\ +Cl_2$

67.

Which of the following is a single replacement reaction?

a)

$2Mg\ +\ O_2\ \rightarrow\ \ 2MgO$

b)

$2Al+6HCl\rightarrow2AlCl_3\ +3H_2$

c)

$Na_2S+2HCl\rightarrow2NaCl+H_2S$

d)

$PCl_5\ \rightarrow\ PCl_3\ +Cl_2$

68.

Which of the following is a double replacement reaction?

a)

$2Mg\ +\ O_2\ \rightarrow\ \ 2MgO$

b)

$2Al+6HCl\rightarrow2AlCl_3\ +3H_2$

c)

$Na_2S+2HCl\rightarrow2NaCl+H_2S$

d)

$PCl_5\ \rightarrow\ PCl_3\ +Cl_2$

69.

What type of reaction is the equation C + O₂→ CO₂?

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

70.

Number of H in 3(NH₄)₂CrO₄

a)

4

b)

6

c)

8

d)

24

71.

Balance this equation:
P₄+O₂--> P₂O₃

a)

3 P₄+ O₂--> 2 P₂O₃

b)

P₄+ O₂--> 2 P₂O₃

c)

P₄+ 3 O₂--> 2 P₂O₃

d)

P₄+ 2 O₂--> 3 P₂O₃

72.

How many atoms of aluminum are on each side of the following equation: 4Al + 3O₂--> 2Al₂O₃

a)

2

b)

6

c)

1

d)

4

73.

What type of reaction is this?

2 C₆H₁₄ + 19 O₂ → 12 CO₂ + 14 H₂O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

74.

1 mole of water has a mass of _____ grams.

a)

6.02 x 10^23

b)

18.0

c)

1.0

75.

What is the molar mass of $C_4H_{10}$ , butane?

a)

14

b)

40

c)

58

76.

What is the percent by mass of sodium(Na) in NaCl?

a)

39%

b)

61%

c)

35%

d)

65%

77.

What is the molar mass of AuCl₃?

a)

96 g

b)

130 g

c)

232.5 g

d)

303.3 g

78.

2 KClO₃ → 2 KCl + 3 O₂

How many moles of oxygen are produced when 8 moles of KClO₃ decompose completely?

a)

8 mol

b)

4 mol

c)

12 mol

d)

10 mol

79.

How many moles are present in 32.3 grams of carbon dioxide (CO₂)?

a)

44.01 moles

b)

1421.52 moles

c)

32.3 moles

d)

0.73 moles

80.

What is the mass in grams of 5.90 mol C₈H_{18? (Molar mass 114 g/mol)}

a)

.0512 g

b)

19.4 g

c)

673 g

d)

389 g

81.

SiO₂ + 3C → SiC + 2CO

I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?

a)

_{96 g}

b)

0.67 g

c)

2.67 g

d)

48 g

82.

How many grams are in 3 moles of nitrogen? (N - 14.01 molar mass)

a)

14.01

b)

4.67

c)

6.98x10^-23

d)

42.03

83.

How many grams are in 1 mole of sucrose sugar? ( $C_{12}H_{22}O_{11}$ ) C = 12.0, H = 1.0, O = 16.0

a)

342

b)

$6.022\times10^{23}$

c)

$2.7\times109$

d)

$45$

84.

What percent of $C_3H_8O\$ is Hydrogen? (Molecular Mass = 60; 1 C=12.0, 1 H = 1.0, 1 O = 16.0 ) this is a simple percentage problem

a)

60%

b)

13%

c)

27%

85.

What grade do you think you should get in this class?

a)

A- mastery understanding

b)

B - on track understanding most material

c)

C - approaching understanding

d)

D - below, completing but not understanding

Chemistry Final Exam

Total questions: 85

Worksheet time: 1hrs 25mins

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