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Chemistry 2023 Fall Final

Total questions: 75

Worksheet time: 57mins

Name
Class
Date
1.

Which part of an atom is most directly involved in chemical bonding?

a)

nucleus

b)

electron

c)

proton

d)

neutron

2.

Which element has the highest electronegativity?

a)

nitrogen

b)

iodine

c)

fluorine

d)

selenium

3.

Which set of tools will provide the most precise measurements for calculating the density of an irregularly shaped rock?

a)

flask and beaker

b)

flask and balance

c)

balance and graduated cylinder

d)

beaker and graduated cylinder

4.

Which of these is an example of a chemical change?

a)

Methane is burned in air.

b)

Solid gold is melted to make jewelry.

c)

A bar of copper is stretched into a long copper wire.

d)

Iron is coated with bronze to prevent rusting.

5.

Which element on the periodic table has a total of 16 protons?

a)

germanium (Ge)

b)

phosphorus (P)

c)

oxygen (O)

d)

sulfur (S)

6.

The half-life of cobalt-60 is 5.27 years. Approximately how much of a 199 g sample will remain after 20 years?

a)

10.0 g

b)

12.5 g

c)

40.0 g

d)

50.0 g

7.

The reaction shown represents the oxidation of ammonia (NH3 ). How many grams of water (H2O) will be formed when 34 grams of ammonia reacts with an excess of oxygen (O2)?

a)

51 grams

b)

54 grams

c)

64 grams

d)

110 grams

8.

The equation represents an incomplete chemical reaction. Al + Cl2==> What is the product of the chemical reaction?

a)

Al2Cl3

b)

AlCl

c)

AlC12

d)

AlC13

9.

Two measuring tools are shown. Measuring Tools What is the most appropriate tool for measuring 30.0 mL of a sodium chloride solution?

a)

the beaker because it is more stable and the liquid is less likely to spill

b)

the beaker because it is calibrated to hold large amounts of liquid

c)

the graduated cylinder because it is calibrated to measure the liquid more precisely

d)

the graduated cylinder because it will be nearly filled with liquid

10.

Isotopes of an element have different numbers of

a)

protons

b)

neutrons

c)

electrons

d)

positrons

11.

What is the molarity of a 0.5 L sample of solution that contains 60.0 g of sodium hydroxide (NaOH)?

a)

0.8M

b)

1.5 M

c)

3.0M

d)

6.0M

12.

Which element has the highest electronegativity?

a)

beryllium (Be)

b)

fluorine (F)

c)

silver (Ag)

d)

silicon (Si)

13.

A chemical equation is shown. What is the molar ratio for the chemical reaction when the equation is balanced?

a)

1: 2: 5

b)

2: 1 : 1

c)

4: 3: 1

d)

4:3:2

14.

Which characteristic of an exothermic reaction differs from that of an endothermic reaction?

a)

An exothermic reaction absorbs heat as the reaction progresses.

b)

The activation energy is higher in an exothermic reaction.

c)

An exothermic reaction releases heat as the reaction progresses.

d)

The products in exothermic reactions have more potential energy than the reactants.

15.

Which illustration represents the region in which an electron of a hydrogen atom is most likely found at ground state?

a)

F

b)

G

c)

H

d)

J

16.

Magnesium (Mg) and oxygen (O2) react to form magnesium oxide (MgO). Which type of chemical reaction does the equation represent?

a)

decomposition

b)

double replacement

c)

single replacement

d)

composition

17.

Based on the graph, what change occurred when ice at 0°C was heated at a constant rate?

a)

Molecules broke apart into atoms.

b)

Elements dissociated into ions.

c)

Intermolecular attractions were decreased.

d)

Chemical energy was stored.

18.

What is the percent composition by mass of sulfur in ammonium sulfate, (NH )2S0 4?

a)

6.7%

b)

24%

c)

28%

d)

32%

19.

The chemical equation shows methane (CH4) burned in the presence of oxygen gas (O2). Which type of reaction does this equation represent?

a)

composition

b)

single replacement

c)

double replacement

d)

combustion

20.

The diagram represents the Lewis electron-dot structure of a neutral element. Which element does this Lewis electron-dot structure most likely represent?

a)

Na

b)

Mg

c)

Cl

d)

Ar

21.

A student fills a flask with 5.0 moles of nitrogen gas and then seals the flask. Which change will happen when the student warms the flask?

a)

The temperature of the nitrogen gas will decrease.

b)

The pressure inside the flask will increase.

c)

The volume inside the flask will decrease.

d)

The molar mass of the nitrogen gas will increase.

22.

Which statement best describes the Bohr model of the atom?

a)

Electrons are arranged in energy clouds.

b)

Electrons have properties similar to waves.

c)

Electrons orbit around the nucleus in set paths.

d)

Electrons make up most of the mass of an atom.

23.

What is the approximate percent composition of phosphorus in phosphoric acid (H3PO4)?

a)

29.5%

b)

31.6%

c)

65.3%

d)

98.0%

24.

Which of these is an example of a homogeneous mixture?

a)

a bowl of noodle soup

b)

a container of water and sand

c)

a glass of salt water

d)

a bottle of oil and vinegar

25.

A student sets up an experiment to investigate the effect of temperature on the volume of 50 grams of gas inside a balloon. Which statement correctly describes the design of the experiment?

a)

The temperature is an experimental control, and the volume is the independent variable.

b)

The volume is an experimental control, and the temperature is the dependent variable.

c)

The mass of the gas is an experimental control, and the temperature is the independent variable.

d)

The temperature is an experimental control, and the mass of the gas is the dependent variable.

26.

What is the approximate mass of 1.50 moles of ammonia (NH3)?

a)

10.0 grams

b)

15.0 grams

c)

17.0 grams

d)

25.5 grams

27.

What is the total number of electrons in all s orbitals of a neutral atom of phosphorus?

4 lines
28.

Which process represents a chemical change?

a)

oxidation

b)

sublimation

c)

evaporation

d)

condensation

29.

Which pair of arrows correctly represents how atomic radii change, from smallest electronegativity to largest electronegativity, on the periodic table of the elements?

a)

red and blue arrows

b)

blue and green arrows

c)

purple and green arrows

d)

yellow and purple arrows

30.

What are the products of the decomposition of mercury(II) oxide (HgO)? 2 answers

a)

Hg2 and O2

b)

Hg2 and O

c)

Hg and O2

d)

HgO and O2

31.

The electron configuration of a neutral atom of calcium is shown. How many valence electrons are in the atom?

a)

6

b)

8

c)

2

d)

10

32.

What quantities of nitrogen gas (N2) and oxygen gas (O2) will react completely to produce 2 moles of dinitrogen pentoxide (N2O5)?

a)

4 moles of N2 and 10 moles of O2

b)

4 moles of N2 and 5 moles of O2

c)

2 moles of N2 and 10 moles of O2

d)

2 moles of N2 and 5 moles of O2

33.

According to the quantum mechanical model of the atom, what is the maximum number of electrons that can occupy the second energy level?

a)

8

b)

18

c)

10

d)

6

34.

A gas has a volume of 3.0 L at a pressure of 3.0 atm. What will be the final volume of the gas if the pressure is increased to 5.0 atm at a constant temperature?

a)

0.56 L

b)

1.8 L

c)

3.0L

d)

5.0L

35.

The chemical equation represents the reaction between sodium (Na) and oxygen (O2). What is the product of this reaction?

a)

Na2O

b)

NaO

c)

NaO2

d)

Na2O2

36.

The diagram shows the Lewis electron-dot structure of Element X at ground state. Which of these could be the atomic number of Element X? choose 2

a)

2

b)

6

c)

16

d)

46

37.

How many atoms are in 3.50 moles of calcium (Ca)?

a)

140.28

b)

3.5

c)

2.1 x 10^24

d)

8.4 x 10^25

38.

The chemical equation shows the production of calcium oxide (CaO) and carbon dioxide (CO2) from CaCO3.. How should this reaction be classified?

a)

decomposition

b)

composition

c)

single replacement

d)

double replacement

39.

Which of these gives an example of a chemical change?

a)

burning a piece of wood

b)

cracking an egg

c)

folding a piece of paper

d)

melting an ice cube

40.

Which of these describes how gallium forms a 3 + ion?

a)

The gallium loses 3 electrons.

b)

The gallium loses 3 protons.

c)

The gallium gains 3 electrons.

d)

The gallium gains 3 protons.

41.

During the production of aspirin, 2.6 g of aspirin can be formed from 2.0 g of salicylic acid. What is the percent yield if only 1.7 g of aspirin is produced?

a)

35%

b)

65%

c)

77%

d)

85%

42.

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

43.

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

44.

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

45.

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

a)

1 cc

b)

1 cm3

c)

1 μl\mu l  

d)

1 dm3

46.

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

47.

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

48.

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

a)

solute

b)

solvent

c)

suspension

d)

colloid

49.

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

a)

homogeneous

b)

heterogeneous

50.

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

51.

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

52.

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

53.

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

54.

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

55.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
c)

metallic

56.

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

a)

F

b)

Cl

c)

Mg

d)

Li

57.

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

a)

K

b)

F

c)

O

d)

Fe

58.

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

a)

left

b)

right

c)

middle

d)

inert gases

59.

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

60.

Isotopes are atoms with different numbers of ________.

a)

protons

b)

neutrons

c)

electrons

61.

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

62.

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

63.

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

a)

20

b)

10

c)

35

d)

25

64.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

65.

Solve this equation for alpha decay.

85209At = ___ + 24He

a)

83205Bi

b)

86209Rn

c)

81207Tl

d)

85208At

66.

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

67.

The correct name for LiCl is

a)

lithium monochloride

b)

lithium chloride

c)

lithium I chloride

d)

monolithium monochloride

68.
What would be the proper chemical formula for combining Al3+ and l- :
a)
Al l3
b)
Al3l
c)
Al l
d)
Al3 l3
69.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
70.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
71.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
72.

Cu + 2Ag(NO3) → 2Ag + Cu(NO3)

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

73.

The correct formula for the ammonium ion is

a)

NH4

b)

N4H+

c)

NH4+

d)

Am+

74.

Which of the following is a double replacement reaction?

a)

2Mg + O2 →  2MgO2Mg\ +\ O_2\ \rightarrow\ \ 2MgO  

b)

2Al+6HCl→2AlCl3 +3H22Al+6HCl\rightarrow2AlCl_3\ +3H_2

c)

Na2S+2HCl→2NaCl+H2SNa_2S+2HCl\rightarrow2NaCl+H_2S

d)

PCl5 → PCl3 +Cl2PCl_5\ \rightarrow\ PCl_3\ +Cl_2  

75.
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

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