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Practice Midterm Exam 2025

Total questions: 70

Worksheet time: 1hrs 8mins

Name
Class
Date
1.

What is this element?

a)

Beryllium (atomic #4)

b)

Boron (atomic #5)

c)

Carbon (atomic #6)

d)

Nitrogen (atomic #7)

2.

Protons are

a)

Negative

b)

Positive

c)

No charge

d)

Atomic Number

3.

Neutrons have

a)

Negative

b)

Positive

c)

No charge

d)

Atomic Number

4.

Electrons are are

a)

Negative

b)

Positive

c)

No charge

d)

Atomic Number

5.

What is represented by the letter Q?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutrons

6.

What is represented by the letter R?

a)

Nucleus

b)

Electron

c)

Proton

d)

Neutrons

7.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

8.

Nickel-59 has how many neutrons?

a)

30

b)

31

c)

32

d)

33

9.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

10.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

11.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

12.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

13.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

14.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

15.

Na has 1 valence electron. It will have a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

16.

Al has 3 valence electron. It will have a charge of _______

a)

+3

b)

-3

c)

+2

d)

-2

17.

Oxygen has 6 valence electron. It will have a charge of _______.

a)

+1

b)

-1

c)

+2

d)

-2

18.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
19.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
20.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
21.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
22.
How many valence electrons are in an atom of Sn?
a)
3
b)
8
c)
4
d)
1
23.
How many valence electrons are found in atoms of Calcium?
a)
4
b)
5
c)
2
d)
3
24.
How many valence electrons are found in atoms of Iodine?
a)
4
b)
7
c)
9
d)
1
25.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
26.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
27.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
28.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
29.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
30.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
31.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
32.

What type of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids?

33.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
34.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

35.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
36.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
37.
H2O
a)
Ionic Bond
b)
Covalent Bond
c)
Both bonds
d)
Neither bond
38.
Low melting point
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
39.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
40.
What is the rule for figuring out if it is ionic or covalent?
a)
Covalent bonds form between two metals.
b)
Ionic bonds form between two metals.
c)
Covalent bonds form between a metal and a non-metal.
d)
Ionic bonds form between a metal and a non-metal.
41.

In chemical compounds, covalent bonds form when

a)

the electronegativity difference between two atoms is very large.

b)

electrons are completely transferred between two metals.

c)

pairs of electrons are shared between two nonmetal atoms.

d)

two nonmetal atoms are attracted to each other by opposite charges.

42.

What two types of atoms make a covalent bond?

a)

2 nonmetals

b)

2 metals

c)

1 metal and 1 nonmetal`

43.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

44.

When electrons are lost by one atom and gained by another, so that they both get full outer shells.

a)

Covalent bond

b)

Ionic bond

c)

Pairing

d)

Compound

45.

____________ compounds are usually solid at room temperature and form a crystal structure.

a)

Ionic

b)

Covalent

c)

Molecule

d)

Solid

46.

Name the following Ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

47.

What is the correct formula for the compound, lithium oxide?

a)

LiO

b)

Li2O

c)

LiO2

d)

Li2O2

48.

What is the formula for manganese (III) oxide?

a)

MgO

b)

Mg2O3

c)

MnO

d)

Mn2O3

49.

The formula of calcium phosphate is:

a)

CaPO4

b)

Ca2(PO4)3

c)

Ca3PO4

d)

Ca3(PO4)2

50.

What is the name of Al(NO3)3?

a)

Aluminum trinitrate

b)

Monoaluminum nitrate

c)

Aluminum (III) nitrate

d)

Aluminum nitrate

51.

Name the following ionic compound: Cr(NO2)3

a)

Chromium nitrite

b)

Chromium nitride

c)

Chromium III nitride

d)

Chromium III nitrite

52.

What is the name of N2O3?

a)

Nitrogen trioxide

b)

Dinitrogen oxide

c)

Dinitrogen trioxide

d)

Nitrogen oxide

53.

What is the chemical formula for tetrasulfur pentoxide?

a)

SO

b)

S4O

c)

S4O5

d)

S5O4

54.

What is the name of C3Cl8?

a)

Carbon octachloride

b)

Tricarbon octachloride

c)

Carbon trichloride

d)

Octacarbon trichloride

55.

What is the name of Br6F10?

a)

Bromine fluoride

b)

Hexabromine fluoride

c)

Bromium decafluoride

d)

Hexabromine decafluoride

56.

What is the name of CO?

a)

Carbon Oxide

b)

Carbon Dioxide

c)

Carbon Monoxide

d)

Carbon II Oxide

57.

What is the name of S2Br6?

a)

sulfur hexabromide

b)

disulfur hexabromine

c)

disulfur hexabromide

d)

disulfur pentabromide

58.

The correct name of Cu3N2 is:

a)

copper (III) nitride

b)

copper (II) nitride

c)

copper nitride

d)

tricopper dinitride

59.

Roman numerals tell you the ____ of the metal cation(s) in an ionic compound.

a)

number

b)

mass

c)

type

d)

charge

60.

True or False: When naming ionic compounds, use prefixes to indicate subscripts

a)

True

b)

False

61.

Ionic compounds are written with

a)

cation (+ ion) first then anion (-ion)

b)

anion (-ion) first then cation (+ ion)

c)

either way is fine

d)

polyatomic ions first

62.

zinc (I) fluoride

a)

ZnF2

b)

ZnF

c)

Zn2F

d)

Zn2F4

63.

ammonium phosphate

a)

(NH4)3PO4

b)

NPO4

c)

NH4PO4

d)

NH4(PO4)3

64.

The formula for copper (II) hydroxide is

a)

Cu(II)OH

b)

Cu(OH)2

c)

Cu2OH

d)

CUOH2

65.

The chemical formula for tin (IV) oxide is written

a)

Sn2O4

b)

Ti2O4

c)

SnO2

d)

TiO2

66.
barium phosphide
a)
Ba3(PO4)2
b)
BaP
c)
Ba3P2
d)
Ba2P3
67.

Calcium nitrate is composed of a calcium cation (Ca2+) and a polyatomic nitrate anion (NO3–). What is its formula?

a)

Ca(NO3)

b)

Ca(NO3)2

c)

Ca2(NO3)

d)

Ca(NO3)3

68.

Name this ionic compound: Al2O3

a)

Dialuminum oxide

b)

Aluminum oxygen

c)

Oxygen Aluminide

d)

Aluminum oxide

69.

Name the following compound: FeO

a)

iron oxide

b)

iron (II) oxide

c)

iron (III) oxide

d)

ugly

70.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide

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