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Chemistry placement

Total questions: 115

Worksheet time: 1hrs 29mins

Name
Class
Date
1.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
2.

The Lewis structure of N2H2 shows __________.

a)

a nitrogen-nitrogen triple bond

b)

a nitrogen-nitrogen single bond

c)

each nitrogen has one lone pair

d)

each nitrogen has two lone pairs

e)

each hydrogen has one lone pair

3.

In the nitrite ion (NO2-), __________.

a)

both bonds are single bonds

b)

both bonds are double bonds

c)

both bonds are the same because of resonance

d)

there are 20 valence electrons

e)

there is one single and one double bond

4.

Resonance structures differ by __________.

a)

number and placement of electrons

b)

number of electrons only

c)

placement of atoms only

d)

number of atoms only

e)

placement of electrons only

5.

A valid Lewis structure of _______ cannot be drawn without violating the octet rule.

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

6.

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

a)

N

b)

C

c)

H

d)

O

e)

B

7.

Bond enthalpy is __________.

a)

always negative

b)

always positive

c)

sometimes positive and sometimes negative

d)

always zero

e)

unpredictable

8.

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable

9.

Of the possible bonds between carbon atoms (single, double, and triple), _____.

a)

a triple bond is longer than a single bond

b)

a double bond is stronger than a triple bond

c)

a single bond is stronger than a triple bond

d)

a double bond is longer than a triple bond

e)

a single bond is stronger than a double bond

10.

The ability of an atom in a molecule to attract electrons is best quantified by the ______.

a)

electronegativity

b)

paramagnetism

c)

diamagnetism

d)

electron change-to-mass ratio

e)

first ionization energy

11.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

12.

The formal charge on carbon in the molecule shown is _______.

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

13.

In the Lewis structure of ClF, the formal charge on Cl is _______ and the formal charge on F is _______.

a)

0,0

b)

-1, -1

c)

0, -1

d)

-1, 0

e)

+1, -1

14.

In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

15.

Using the table of average bond energies below, the ΔH for the reaction is _____ kJ.

a)

+160

b)

-160

c)

-217

d)

+217

e)

-63

16.

What follows an element’s symbol in a chemical formula to indicate the number of atoms of that element in one molecule of the compound?

a)

charge sign

b)

superscripted number

c)

number in parentheses

d)

subscripted number

17.

The chemical formula for an ionic compound represents one

a)

formula unit.

b)

ion.

c)

molecule.

d)

cation

18.

What is the correct notation for a calcium ion whose outer shell is a full octet?

a)

Ca1+

b)

Ca2+

c)

Ca1-

d)

Ca2-

19.

What is the correct name for the NO3- ion?

a)

nitrate

b)

nitrite

c)

nitride

d)

nitrogen oxide

20.

What is the correct formula for copper(I) cyanide?

a)

CuCy

b)

CuCy2

c)

CuCN

d)

Cu2CN

21.

What is the correct name for the acid CH3COOH?

a)

carbonic acid

b)

carbonate acid

c)

acetic acid

d)

acetous acid

22.

What is the correct name for the compound P2Cl4.

a)

phosphorus chloride

b)

phosphorus tetrachloride

c)

diphosphorus chloride

d)

diphosphorus tetrachloride

23.

What is the correct formula for the compound made of magnesium and nitrogen?

a)

Mg2N3

b)

Mg3N2

c)

MgN2

d)

MgN

24.

Oxidation numbers are used to indicate the

a)

charge on an ion.

b)

number of atoms or ions in a compound.

c)

type of bond holding particles together in a compound.

d)

distribution of electrons among the bonded particles in a compound.

25.

Atoms have an oxidation number of zero in a(n)

a)

pure element.

b)

acid

c)

ionic compound.

d)

molecular compound.

26.

What is the oxidation number of nickel in NiCO3?

a)

0

b)

+1

c)

+2

d)

+3

27.

What is the correct name for the compound Ni2CO3 using the Stock system?

a)

nickel(II) oxide

b)

dinickel trioxide

c)

nickel trioxide

d)

nickel(III) oxide

28.

What is the oxidation number of phosphorus in the PO3- ion?

a)

-3

b)

0

c)

+5

d)

+8

29.

What is the correct formula for the compound platinum(VI) fluoride?

a)

PtF3

b)

PtF6

c)

Pt6F2

d)

Pt6F

30.

The formula mass of any coumpound is described in units of

a)

grams

b)

u

c)

moles

d)

grams per mole.

31.

The molar mass of water is equal to

a)

1 g of O plus 2 g of H.

b)

1 g of O plus 1 g of H.

c)

the mass of 1 mol of O plus the mass of 1 mol of H.

d)

the mass of 1 mol of O plus the mass of 2 mol of H.

32.

What is the molar mass of pure tin?

a)

1.00 g/mol

b)

47.88 g/mol

c)

118.71 g/mol

d)

237.42 g/mol

33.

How many moles of compound are there in 15.0 g of potassium dichromate, K2Cr2O7? (The molar mass of K2Cr2O7 is 294.2 g.)

a)

0.0510 mol

b)

11.0 mol

c)

15.0 mol

d)

294 mol

34.

What is the mass percentage of cobalt in cobalt(II) fluoride, CoF2?

a)

33.33%

b)

39.20%

c)

60.80%

d)

96.93%

35.

What is the mass of 4.80 mol of barium hydride, BaH2?

a)

4.80 g

b)

29.0 g

c)

139 g

d)

669 g

36.

Which of the following molecular formulas does not have the corresponding empirical formula XY2Z?

a)

X2Y4Z2

b)

XYZ

c)

X6Y12Z6

d)

X3Y6Z3

37.

The simplest whole-number ratio of moles of each element in a compound is known as the

a)

percent composition.

b)

empirical formula

c)

Stock formula.

d)

molecular formula.

38.

What is the empirical formula for a compound that contains 12.62% Li, 29.17% S, and 58.21% O?

a)

LiSO2

b)

LiS2O6

c)

Li2SO4

d)

Li2SO3

39.

What is the molecular formula for the compound with a formula mass of 58.12 u and an empirical formula of C2H5?

a)

C2H5

b)

C4H10

c)

C6H15

d)

C8H20

40.

What is the molecular formula for the compound that is made up of 30.45 g N and 69.55 g O, and has a formula mass of 92.02 u?

a)

NO

b)

N2O2

c)

NO2

d)

N2O4

41.

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.

42.

Using the Stock system of nomenclature, Cr2(SO4)3 is named

a)

chromium(II) sulfate.

b)

chromic sulfate.

c)

dichromium trisulfate.

d)

chromium(III) sulfate.

43.

In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is equal to

a)

0.

b)

10.

c)

the number of atoms in the ion

d)

the charge on the ion.

44.

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

a)

cation

b)

polyatomic ion.

c)

oxyanion.

d)

anion.

45.

The empirical formula may not represent the actual composition of a(n)

a)

ionic compound.

b)

crystal.

c)

salt.

d)

molecular compound.

46.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
47.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
48.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
49.
What is the ionic compound formed between Ba and P?
a)
Ba2P3
b)
Ba3P2
c)
BaP
d)
Ba2P2
50.
When a test instrument is calibrated, does its accuracy, precision, or reliability improve?
a)
precision
b)
accuracy
c)
reliability
d)
all of the above
51.
What is the density of an object having a mass of 8.0 g and a volume of 25 cm3?
a)
0.32 g/cm3
b)
3.1 g/cm3
c)
200 g/cm3
d)
2.0 g/cm3
52.
Which group of measurements  is the most precise? (Each group of measurements is for a  different object)
a)
2.0 g, 3.0 g, 4.0 g
b)
1 g, 3 g, 5 g
c)
2 g, 2.5 g, 3 g
d)
2 g, 3 g, 4 g
53.
The weight of an object _____.
a)
depends on its location
b)
is always the same
c)
is not affected by gravity
d)
is the same as its mass
54.
What is the result of adding 2.5 x 103 and 3.5 x 102?
a)
2.9 x 102
b)
6.0 x 103
c)
2.9 x 103
d)
6.0 x 105
55.
Which of the following mass units is the largest?
a)
dg
b)
cg
c)
ng
d)
mg
56.
Which of the following volumes is the smallest?
a)
one deciliter
b)
one microliter
c)
one liter
d)
one milliliter
57.
Which of the following measurements (of different masses) is the most accurate?
a)
3.122 22 g
b)
3.100 00 g
c)
3.1000 g
d)
Cannot be determined
58.
What is the volume of a salt crystal measuring 2.44 x 10-2 m by 1.4 x 10-3 m by 8.4 x 10-3 m?
a)
2.9 x 10-4 m3
b)
2.9 x 10-5 m3
c)
2.9 x 10-7 m3
d)
2.9 x 10-6 m3
59.
Express the sum of 7.68 m and 5.0 m using the correct number of significant figures.
a)
12.7 m
b)
10 m
c)
13 m
d)
12.68 m
60.
Express the product of 4.0 x 10-2 m and 8.1 x 102 m using the correct number of significant figures.
a)
3.24 x 101 m2
b)
3 x 101 m2
c)
3.2 x 101 m2
d)
3.0 x 101 m2
61.
An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.
a)
20
b)
10
c)
5
d)
25
62.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
63.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
64.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
65.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
66.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
67.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
68.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
69.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
70.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
71.
Bonus question: What element is this an atom of?
a)
nitrogen
b)
lithium
c)
beryllium
d)
carbon
72.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
73.
What is the mass number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
74.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
75.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
76.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
77.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
78.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
79.
What is the chemical formula for Fluorine trisulfide ?
a)
S3F
b)
FS3
c)
FS
d)
none of the above
80.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
81.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
82.
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
83.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
84.
What is the charge on a Hydrogen ion?
a)
+1
b)
1
c)
2
85.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
86.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
87.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
88.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

89.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

90.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

91.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

92.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

93.

How would you classify the matter in the picture above?

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

94.

How would you classify the matter in the picture above?

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

95.

Tap water (water, salt & minerals) is an example of a(n):

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

96.

Chicken noodle soup is an example of a(n):

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

97.

Which of the following is a physical property?

a)

Heat of combustion

b)

Boiling point

c)

Flammability

d)

Reactivity

98.

Which of the following is NOT a sign that a chemical change has occurred?

a)

Change in color

b)

Change in shape

c)

Formation of a gas

d)

Change in odor

99.

Which of the following is a physical property?

a)

Combustion

b)

Electronegativity

c)

Color

d)

PH Level

100.

Which of the following is a physical change?

a)

Burning a match

b)

Vinegar reacting with baking soda

c)

Melting butter

d)

Cooking an egg

101.

Which of the following is an example of a chemical change?

a)

Ripping paper in half

b)

Boiling an egg

c)

Cracking an egg

d)

Dissolving sugar in water

102.

Something that takes up space and has mass.

a)

Volume

b)

Matter

c)

Mass

d)

Density

103.

The ___________ of an atom is a unique number that describes how many protons an element has.

a)

atomic number

b)

valence electron

c)

nucleus

d)

electron cloud

104.

A __________ is an electron in the outermost energy level of an atom.

a)

valence electron

b)

proton

c)

neutron

d)

nucleus

105.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
106.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
107.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
108.

Resonance structures differ by __________.

a)

number and placement of electrons

b)

number of electrons only

c)

placement of atoms only

d)

number of atoms only

e)

placement of electrons only

109.

Of the possible bonds between carbon atoms (single, double, and triple), _____.

a)

a triple bond is longer than a single bond

b)

a double bond is stronger than a triple bond

c)

a single bond is stronger than a triple bond

d)

a double bond is longer than a triple bond

e)

a single bond is stronger than a double bond

110.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

111.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

112.

Long wavelength has _________ frequency and ___________ energy.

a)

High; High

b)

High; Low

c)

Low; Low

d)

Low; High

113.

Which color has the highest energy?

a)

Green

b)

Orange

c)

Yellow

d)

Red

114.

What is the first noble gas before Silicon?

a)

Aluminum

b)

Magnesium

c)

Argon

d)

Neon

115.

Which of the following is NOT an example of a physical change?

a)

crumpled paper

b)

pencil sharpening

c)

glass breaking

d)

mold growing on cheese

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