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2025 Chemistry Practice Final

Total questions: 57

Worksheet time: 3hrs 51mins

Name
Class
Date
1.

A theory is a ___

a)

Proposed explanation for an observation

b)

Well-tested explanation for a broad set of observations

c)

Summary of the results of many observations

d)

Procedure used to test a proposed explanation

2.

Which step in the scientific method requires you to use your senses to obtain information?

a)

Revising a hypothesis

b)

Designing an experiment

c)

Making an observation

d)

Stating a theory

3.

All of the following are physical properties of matter except ___

a)

Mass

b)

Color

c)

Melting point

d)

Ability to rust

4.

Which state of matter has a definite volume and takes the shape of its container?

a)

Solid

b)

Liquid

c)

Gas

d)

Both b and c

5.

Which of the following is a physical change?

a)

Corrosion

b)

Explosion

c)

Evaporation

d)

Rotting of food

6.

Which of the following is a homogeneous mixture?

a)

Salt water

b)

Beef stew

c)

Sand and water

d)

Soil

7.

Which of the following is true about compounds?

a)

They can be physically separated into their component elements

b)

The have compositions that vary

c)

They are pure substances

d)

They have properties similar to those of the component elements

8.

Which of the following is a chemical property?

a)

Color

b)

Hardness

c)

Freezing point

d)

Ability to react with oxygen

9.

The smallest particle of an element that retains the properties of that element is a(n) ___

a)

Atom

b)

Electron

c)

Proton

d)

Neutron

10.

Dalton’s atomic theory included which idea?

a)

All atoms of the same element are the same size.

b)

Atoms of different elements always combine in one-to-one ratios.

c)

Atoms of the same element are always identical.

d)

Individual atoms can be seen with a microscope.

11.

All atoms are ___

a)

Positively charged, with the number of protons exceeding the number of electrons

b)

Negatively charged, with the number of electrons exceeding the number of protons

c)

Neutral, with the number of protons equaling the number of electrons

d)

Neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons

12.

An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ___.

a)

152 protons and 76 electrons

b)

76 protons and 0 electrons

c)

38 protons and 38 electrons

d)

76 protons and 76 electrons

13.

Isotopes of the same element have different ___

a)

Numbers of neutrons

b)

Numbers of protons

c)

Numbers of electrons

d)

Atomic numbers

14.

What is the maximum number of orbitals in the p sublevel?

a)

2

b)

3

c)

4

d)

5

15.

What types of atomic orbitals are in the third principle energy level?

a)

s and p only

b)

p and d only

c)

s, p, and d only

d)

s, p, d, and f

16.

What is the next atomic orbital in this series 1s 2s 2p 3s 3p?

a)

2d

b)

3d

c)

3f

d)

4s

17.

What is the electron configuration of potassium?

a)

1s2 2s2 2p4 3s2 3p2 4s1

b)

1s2 2s2 2p10 3s2 3p3

c)

1s2 2s2 3s2 3p6 3d1

d)

1s2 2s2 2p6 3s2 3p6 4s1

18.

Each period in the Periodic Table corresponds to ___

a)

A principle energy level

b)

An energy sublevel

c)

An orbital

d)

A suborbital

19.

Which of the following elements is a transitional metal?

a)

Cesium

b)

Copper

c)

Tellurium

d)

Tin

20.

Atomic size generally ___

a)

Increases as you move from left to right across a period

b)

Decreases as you move from top to bottom within a group

c)

Remains constant within a period

d)

Decreases as you move from left to right across a period

21.

In which of the following groups of ions are the charges all shown correctly?

a)

Li+1, O2-, S+2

b)

Ca+2, Al+3, Br-1

c)

K+2, F-1, Mg+2

d)

Na+1, I-1, Rb-1

22.

Which is the element with the lowest electronegativity value?

a)

Cesium

b)

Magnesium

c)

Calcium

d)

Fluorine

23.

Which of the following elements has the smallest first ionization energy?

a)

Sodium

b)

Calcium

c)

Potassium

d)

Magnesium

24.

How many valence electrons are in an atom of phosphorous?

a)

2

b)

3

c)

4

d)

5

25.

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

a)

Orbital electrons

b)

Valence electrons

c)

Anions

d)

Cations

26.

What is the net charge of the ionic compound calcium fluoride?

a)

-2

b)

-1

27.

An ionic bond is between ___

a)

A cation and an anion

b)

Valance electrons and cations

c)

The ions of two different metals

d)

The ions of two different nonmetals

28.

According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?

a)

Pairs of valence electrons

b)

Inner shell electrons

c)

Mobile electrons

d)

The electrons closest to the nuclei

29.

What type of ions have names ending in -ide?

a)

Only cations

b)

Only anions

c)

Only metal ions

d)

Only gaseous ions

30.

When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ___

a)

Prefix

b)

Suffix

c)

Roman numeral following the name

d)

Superscript after the name

31.

What is the correct formula for potassium sulfite?

a)

KHSO3

b)

KHSO4

c)

K2SO3

d)

K2SO4

32.

Which set of chemical name and chemical formula for the same compound is correct?

a)

Ammonium sulfite, (NH4)2S

b)

Iron (III) phosphate, FePO4

c)

Lithium carbonate, LiCO3

d)

Magnesium dichromate MgCrO4

33.

Which of the following formulas represents a molecular compound?

a)

ZnO

b)

Xe

c)

SO2

d)

BeF2

34.

What is the name of H2SO3?

a)

Hyposulfuric acid

b)

Hydrosulfuric acid

c)

Sulfuric acid

d)

Sulfurous acid

35.

What is the formula for phosphoric acid?

a)

H3PO3

b)

H3PO4

c)

HPO2

d)

HPO4

36.

What is the correct name for CoCl2?

a)

Cobalt (I) chlorate

b)

Cobalt (I) chloride

c)

Cobalt (II) chlorate

d)

Cobalt (II) chloride

37.

What is the correct name for Sn3(PO4)2?

a)

Tritin diphosphate

b)

Tin (II) phosphate

c)

Tin (III) phosphate

d)

Tin (IV) phosphate

38.

The expression of 5008km in scientific notation is __.

a)

5.008 5.008x1035.008x10^3 km

b)

50.08 x104x10^4 km

c)

5.008 5.008x10−35.008x10^{-3} km

d)

5.008 5.008x1045.008x10^4 km

39.

What is the measurement 111.009mm rounded off to four significant figures?

a)

111mm

b)

111.0mm

c)

111.01mm

d)

110mm

40.

What is the quantity 7896 millimeters expressed in meters?

a)

7.896m

b)

78.96m

c)

789.6m

d)

789,600m

41.

How many moles of silver atoms are in 1.8x10^20 atoms of silver?

a)

3.0x10^{-4} moles Ag

b)

3.3x10^{-3} moles Ag

42.

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

a)

144g

b)

138g

c)

96g

d)

78g

43.

What is the mass in grams of 5.90 mol C8H18?

a)

0.0512g

b)

19.4g

c)

389g

d)

673g

44.

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

a)

0.0335L

b)

11.2L

c)

16.8L

d)

22.4L

45.

What is the percent composition of chromium in BaCrO4?

a)

4.87%

b)

9.47%

c)

20.5%

d)

25.2%

46.

Which of the following is not an empirical formula?

a)

C2N2H8

b)

C3H6O

c)

BeCr2O7

d)

Sb2S3

47.

What is the empirical formula for a compound that is 40% sulfur and 60% oxygen by weight?

a)

SO

b)

SO2

c)

SO3

d)

S6O4

48.

Which of the following is NOT a true statement concerning what happens in all chemical reactions?

a)

The ways in which atoms are joined together are changed

b)

New atoms are formed as products

c)

The starting materials are named reactants

d)

The bonds of the reactants are broken and new bonds of the products are formed

e)

In a word equation representing a chemical reaction, the reactants are written on the left and the products on the right.

49.

In the balanced chemical equation for the following reaction, what is the coefficient in front of fluorine?

nitrogen trifluoride  -> nitrogen  +  fluorine

a)

1

b)

2

c)

3

d)

5

e)

6

50.

In order to predict whether or not a single-replacement reaction takes place, we need to consult a chart which shows the ____________.

a)

periodic table

b)

activity series of metals

c)

common ion chart

d)

table of electronegativities

e)

orbital energy level diagram

51.

Predict the products for the following reaction: Potassium + Zinc nitrate →

a)

potassium zinc + nitrogen

b)

potassium nitride + zinc

c)

potassium nitrate + zinc

d)

potassium nitrite + zinc

e)

No Reaction

52.

Which of the following accurately represents the correct balanced equation for the following reaction: Sodium + Nitrogen →

a)

S + N → SN

b)

Na + N → NaN

c)

3 Na + N → Na3N

d)

6 Na + N2 → 2 Na3N

e)

4 Na + N2 → 2 Na2N

53.

How many moles of oxygen react with 2.4 moles of iron according to the following reaction? 4 Fe + 3 O2 → 2 Fe2O3

a)

1.2 mol

b)

1.8 mol

c)

2.4 mol

d)

3.2 mol

e)

4.8 mol

54.

How many grams of Cr are needed to react with an excess of CuSO4 to produce 27.0 g Cu?

a)

0.00548 g

b)

14.7 g

c)

18.0 g

d)

33.2 g

e)

81.5 g

55.

Which type of stoichiometric calculation does not require the use of the molar mass of a substance?

a)

mass-mass problems

b)

mass-volume problems

c)

mass-particle problems

d)

volume-volume problems

56.

If 50 molecules of hydrogen reacts with 50 molecules of oxygen to produce 50 molecules of water, which of them would be the limiting reactant in this reaction? 2 H2 + O2 → 2 H2O

a)

50 molecules of H2

b)

50 molecules of O2

c)

50 molecules of H2O

d)

none of these is limiting

57.

How many molecules of Chlorine can be produced when 0.98 L of HCl reacts with excess O2 at STP?

a)

6.72 x 10^21 molecules

b)

1.32 x 10^22 molecules

c)

2.63 x 10^22 molecules

d)

5.38 x 10^22 molecules

e)

1.05 x 10^23 molecules

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