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Worksheets

CHEMISTRY

Total questions: 85

Worksheet time: 1hrs 13mins

Name
Class
Date
1.

What is the formula of Copper (II) oxide?

a)

CUO

b)

CuO

c)

CuO2

d)

Cu2O

2.

What is the formula of nitric acid?

a)

H2SO4

b)

HNO3

c)

HCl

d)

hno3

3.

What is the formula of Copper (II) oxide?

a)

CUO

b)

CuO

c)

CuO2

d)

Cu2O

4.

What is the name of this chemical, H2SO4?

a)

Hydrogen sulfate

b)

Sulfuric acid

c)

Sulfate

d)

Sulfate hydrogen

5.

What is the chemical formula of Magnesium chloride?

a)

MgCl

b)

MgCl2

c)

MgC

d)

MgC2

6.

What is the chemical formula of sodium sulfate?

a)

SSO4

b)

SoSO4

c)

NaSO4

d)

Na2SO4

7.

What is the chemical formula of Magnesium chloride?

a)

MgCl

b)

MgCl2

c)

MgC

d)

MgC2

8.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
9.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
10.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
11.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
12.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
13.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
14.
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
15.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
16.
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
17.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
18.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
19.
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
20.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
21.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
22.

 In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces

a)

Higher

b)

The same

c)

Lower

23.

What explains the very high melting and boiling point of water?

a)

Dipole-dipole forces between water molecules

b)

London dispersion forces between water molecules

c)

Hydrogen bonds between water molecules

d)

Molecule-ion attractions between water molecules

24.

What type of intermolecular force is present in all substances, regardless of polarity?

a)

London dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

25.

Hydrogen bonding is a special type of what force?

a)

London dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

covalent force

26.

Which are the strongest intermolecular forces?

a)

hydrogen bonds

b)

London dispersion forces

c)

dipole-dipole forces

d)

molecule-ion attractions

27.

Which of these is not an intermolecular force?

a)

covalent bonding

b)

London dispersion forces

c)

hydrogen bonding

d)

dipole-dipole forces

28.

 Intermolecular forces are the forces that exist

a)

within molecules

b)

between molecules

29.

Forces that holds molecules together

a)

intramolecular forces

b)

intermolecular forces

30.

Which of the following has the lowest boiling point?

a)

PH3

b)

H2O

c)

SiH4

d)

NH3

31.

Hydrogen bonding is a special case of __________.

a)

london dispersion

b)

ion-dipole

c)

dipole-dipole

32.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, ion-dipole

b)

hydrogen bonding, london dispersion

c)

ion-dipole, london dispersion

33.

Forces that holds atoms together within the molecule

a)

intermolecular forces

b)

intramolecular forces

34.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

35.

Which of the following molecules is the weakest?

a)

F2

b)

H2O

c)

HCl

d)

SO2

36.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

37.

What intermolecular force present in a sample of pure HCl?

a)

dipole-dipole attraction

b)

H-bonds

c)

London dispersion forces 

d)

molecule-ion attraction

38.

Identify the IMF exist in NH3

a)

london dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

39.

Identify the IMF exist in CH4

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

40.

What type of bonding is present in water?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

41.

What type of bonding is present in potassium nitrate KNO3?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

42.

What type of bonding is present in iron?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

43.

What type of bonding is present in sodium?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

44.

What type of bonding is present in sodium chloride?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

45.

What type of bonding is present in chlorine Cl2?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

46.

What type of bonding is present in ammonia NH3?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

47.

What type of bonding is present in methane CH4?

a)

ionic

b)

covalent

c)

metallic

d)

ionic and covalent

48.

Which of the following compounds are covalent?

a)

carbon dioxide

b)

copper chloride

c)

calcium nitrate

d)

methane CH4

e)

ammonia NH3

49.

Which of the following compounds are ionic?

a)

carbon dioxide

b)

copper oxide

c)

calcium oxide

d)

nitrogen oxide

50.

What is an ion

a)

is compound or group of molecule that don't have any electric charge

b)

is an atom or group of atoms that has an electric charge

c)

is an atom or group of atoms that has no electric charge

d)

is an atom or group of atoms that don't have any electric charge

51.

What is Covalent bonding

a)

When a Nonmetal bonds with a Metal

b)

When a Metal bonds with a Metal

c)

When a Gas bonds with a Metal

d)

When a Nonmetal bonds with a Nonmetal

52.

What is Ionic bonding

a)

When a Nonmetal bonds with a Metal

b)

When a Metal bonds with a Metal

c)

When a Gas bonds with a Nonmetal

d)

When a Nonmetal bonds with a Nonmetal

53.

What is nonpolar bond

a)

In which the electrons are shared equally

b)

In which the number of electrons in both molecules are equal

c)

In which the number of electrons in both atoms are equal

d)

In which the electrons are shared unequally

54.

What is polar bond

a)

In which the electrons are shared equally

b)

In which one molecule gives away all of it's electron away

c)

In which one compound gives away all of it's electron away

d)

In which the electrons are shared unequally

55.
_Al + _HCl →_H2 + _AlCl3
a)
2 Al + 2 HCl → 2 H2 + 6 AlCl3
b)
3 Al + 3 HCl → 6 H2 + 2 AlCl3
c)
1 Al + 1 HCl → 3 H2 + 1 AlCl3
d)
2 Al + 6 HCl → 3 H2 + 2 AlCl3
56.
__Na + __Cl2 --> __NaCl
a)
1,1,2
b)
2,1,2
c)
2,1,1
d)
already balanced
57.
_P4+_O2 →  _P2O3
a)
3 P4+1 O2 → 2 P2O3
b)
1 P4+1 O2 → 2 P2O3
c)
1 P4+ 3 O2 → 2 P2O3
d)
1 P4+ 2 O2 → 3 P2O3
58.
How many F atoms are in this compound?
6MgF2 
a)
2
b)
6
c)
8
d)
12
59.
How many Al atoms are in this compound?         4Al2O3
a)
2
b)
8
c)
6
d)
4
60.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
61.
In a chemical reaction, bonds are broken and new bonds are formed that create new substances. The bonds that are broken are called what?
a)
Reactants
b)
Products
c)
Atoms
d)
Catalysts
62.

What is the BEST definition of a chemical reaction?

a)

A change in matter that produces one or more NEW substances

b)

When two things combine and EXPLODE.

63.

A substance that is formed as the result of a chemical reaction is a __________________

a)

Product

b)

Reactant

c)

Starters

d)

Enders

64.

Which of the following is an ester

a)

HCOOCH2CH3

b)

CH3CO2CH3

c)

CH3OCOCH3

d)

CH3CH3COOH

65.

Which of the following is a carboxylic acid

a)

CH3CH2COOCH3

b)

CH3CH2COOH

c)

HOOCCH2CH2COOH

d)

CH3COOCH2CH3

66.

Which of the following is an nitrile

a)

CH3CH2NH2

b)

CH3CH2CN

c)

CH3CH2OH

d)

CH3CHO

67.

Which of the following is an amine

a)

CH3CH2NH2

b)

CH3NH2

c)

CH2(NH2)CH2CH2CH3

d)

(CH3)3CNH2

68.

which of the following is an alcohol

a)

CH3CH(OH)CH2CH3

b)

(CH3)2CHCOOH

c)

CH3COCH2CH3

d)

CH3CH2CH2OH

69.

What is the functional group described in the picture?

Note: The amino (N, NH, NH2) is attached directly to the alkyl group/s.

a)

AMIDE

b)

NITRILE

c)

ARENE

d)

AMINE

70.

What is the functional group described in the picture?

Note: The amino (N, NH, NH2) is attached directly to the alkyl group/s.

a)

ALDEHYDE

b)

ESTER

c)

CARBOXYLIC ACID

d)

AMINE

71.

What is the functional group described in the picture?

Note: Contains the carboxyl group

(-COOH) or -(C=O)-OH

a)

ALDEHYDE

b)

ESTER

c)

CARBOXYLIC ACID

d)

AMINE

72.

What is the functional group described in the picture?

Note: Have carboxyl group (–COO-)

a)

ALDEHYDE

b)

ESTER

c)

CARBOXYLIC ACID

d)

AMINE

73.

What is the functional group described in the picture?

Note: The carbonyl group is located at the terminal end of the molecule.

a)

ALDEHYDE

b)

ESTER

c)

CARBOXYLIC ACID

d)

AMINE

74.

which of the following is an alkene

a)

CH3CH2CH2CH3

b)

(CH3)2CHCH3

c)

CH3CH2CH=CH2

d)

CH3CH2CH2=CH3

75.

What is the functional group described in the picture?

Note: Two alkyl groups attached to the same oxygen atom

a)

ALKYL HALIDE

b)

ALCOHOL

c)

ETHER

d)

KETONE

76.

What is the functional group described in the picture?

a)

ALKYL HALIDE

b)

ALCOHOL

c)

ETHER

d)

KETONE

77.

An electron is

a)

positively charged

b)

neutral

c)

negatively charged

78.

If an atom has 7 protons and 7 electrons, its electric charge is ---

a)

-7

b)

-14

c)

0

d)

+7

79.

Atoms that gain an electron have an electric charge of ---

a)

-1.

b)

-2.

c)

+1.

d)

+2.

80.

Ionic bonds form between ---

a)

nonmetals.

b)

metals and nonmetals.

81.

Covalent bonds form between ---

a)

nonmetals.

b)

metals and metals

c)

metals and nonmetals

82.

What are valence electrons?

a)

sum of the protons and neutrons

b)

protons minus electrons

c)

electrons in the inner shells

d)

electrons in the outer shell

83.

Alkyl halide has .... Functional group

a)

-Halide

b)

-OH

c)

-COOH

d)

=O

84.

the name of this compaund C4H10

a)

METHANE

b)

HEXENE

c)

BUTANOIC ACID

d)

BUTANE

85.

What below is NOT considered matter?

a)

Carbon atoms

b)

Gravity

c)

Bacteria

d)

Air

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