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Chemistry Revision Quiz

Total questions: 109

Worksheet time: 1hrs 16mins

Name
Class
Date
1.

A substance that cannot be broken down any further without losing its properties.

a)

Compound

b)

Mixture

c)

Element

d)

Suspension

2.

The subatomic particle with a positive charge

a)

Proton

b)

Neutron

c)

Electron

3.

The subatomic particle/s found in the nucleus

a)

Electron

b)

Neutron

c)

Proton

4.

Atoms are mostly...

a)

Tightly packed

b)

Empty space

5.

The mass of an atom is found by adding which subatomic particles?

a)

Proton

b)

Neutron

c)

Electron

6.

The number of _______________ in an atom is represented by its atomic number.

a)

Protons

b)

Neutrons

c)

Electrons

7.

If an atom has 12 neutrons and 11 protons, what is its atomic mass?

(a)  

8.

Cations are...

a)

Positive

b)

Negative

c)

Neutral

d)

Non-metals

9.

Which of the following would produce an anion?

a)

Al

b)

Ca

c)

K

d)

F

10.

The number at the bottom of each square on the periodic table is the ...

a)

Atomic Number

b)

Atomic Mass

c)

Element Name

d)

Chemical Symbol

11.

How many protons does Helium (He) have?

a)

1

b)

2

c)

3

d)

4

12.

How many neutrons does Hydrogen (H) have?

(a)  

13.

15. What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

none of the above

14.

How many valence electrons does this element have?

(a)  

15.

What is the electrical charge of the ion form of this element?

(a)  

16.

How many electrons are in a gold atom?

a)

79

b)

118

c)

197

d)

275

17.

How many neutrons are in a gold atom?

a)

79

b)

118

c)

197

d)

275

18.

What is the name of this compound?


MgF2

a)

Manganese fluoride

b)

Magnesium fluorine

c)

Manganese fluorine

d)

Magnesium fluoride

19.

What is the chemical formula for Silver oxide?





(a)  

20.

Which is the correct formula for Calcium phosphate?


(Hint: Phosphate is PO43-)

a)

Ca(PO4)

b)

Ca3(PO4)2

c)

Ca2(PO4)3

d)

Ca12(PO4)2

21.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
22.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
23.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
24.
A chemical bond between oppositely charged ions.
a)
compound
b)
ion
c)
covalent bond
d)
ionic bond
25.
In this type of bond, electrons are delocalized in a "sea"
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nonpolar
26.

What is made when an atom gain an electron?

a)

Neutral(no charge)

b)

Positive ion

c)

Negative ion

27.

Which type of bond transfers electrons

a)

covalent bonds

b)

ionic bonds

c)

hydrogen bonds

28.

Identify the type of bonding between the oxygen and hydrogens in one water molecule.

a)

covalent bonding

b)

hydrogen bonding

c)

ionic bonding

29.

MgO is bonded together with what type of bond?

a)

ionic

b)

covalent

c)

metallic

d)

hydrogen

30.

C6H12O6 has what type of bond holding the atoms together?

a)

ionic

b)

covalent

c)

metallic

d)

Hydrogen

31.

Multiple Zn atoms are bonded together by what type of bond?

a)

ionic

b)

covalent

c)

metallic

d)

hydrogen

32.

Which of the following types of substance have a high melting point? (choose 2)

a)

metallic

b)

ionic

c)

covalent

d)

hydrogen

33.

Which of the following types of structure has a low melting point? (Choose 1)

a)

ionic

b)

covalent

c)

metallic

d)

hydrogen

34.
A positively or negatively charged particle.
a)
covalent bond
b)
compound
c)
ion
d)
chemical bond
35.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
36.
Which substance contains bonds that involve a transfer of electrons from one atom to another?
a)
CO2
b)
NH3
c)
KBr
d)
Cl2
37.
Which type of bond forms between two or more metals?
a)
Ionic
b)
Covalent
c)
Metallic
d)
Ironic
38.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1
39.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
40.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
41.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
42.
There are more metals than non metals in the periodic table.
a)
True
b)
False
43.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
44.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
45.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
46.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
47.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
48.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
49.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
50.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

51.

What particles have a charge of -1 and a very small mass?

a)

protons

b)

neutrons

c)

electrons

d)

shells

52.

The atomic number is

a)

the number of neutrons

b)

the number of neutrons and protons added together

c)

the number of electrons and protons added together

d)

the number of protons

53.

The atomic mass is

a)

protons and electrons added together

b)

protons and neutrons added together

c)

electrons and neutrons added together

d)

neutrons and electrons added together

54.

Elements in group 7 have how many electrons in their outer shell?

a)

1

b)

3

c)

5

d)

7

55.

Isotopes are atoms that have ...

a)

same number of protons but different number of electrons

b)

same number of neutrons but different number of protons

c)

same number of protons but different number of neutrons

d)

same number of electrons but different number of protons

56.

When you have an ion of an atom, O-2 for example, what has changed in the atomic structure?

a)

Number of protons

b)

Number of neutrons

c)

Number of electrons

57.

What two subatomic particles must be equal for an atom to have no charge (neutral).

a)

protons and neutrons

b)

protons and electrons

c)

electrons and neutrons

58.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
59.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
60.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
61.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
62.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

63.
The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?
a)
0
b)
3
c)
5
d)
7
64.
What is the shape of s orbitals?
a)
Dumbbell shaped
b)
Peanut shaped
c)
Spherical shaped
d)
Hybrid structure
65.
What shape are P Orbitals? 
a)
Cloverleaf shaped
b)
Spherical shaped
c)
Hybrid structure
d)
Dumbell shaped
66.

As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?

a)

Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.

b)

The nucleus is made of protons, electrons, and neutrons.

c)

Electrons are distributed around the nucleus and occupy almost all the volume of the atom.

d)

The nucleus is made of electrons and protons.

67.

Which of the following sub-shells is lowest in energy?

a)

4s

b)

3d

c)

4p

d)

5s

68.

In order for electrons to occupy the same orbital they must have opposite spins.

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli’s Exclusion Principle

d)

Heisenberg’s Uncertainty Principle

69.

In Bohr's model of the atom, where are the electrons and protons located?

a)

The electrons move around the protons, which are in the center of the atom.

b)

The electrons and protons move throughout the atom.

c)

The electrons occupy fixed positions around the protons, which are at the center of the atom.

d)

The electrons and protons are located throughout the atom, but they are not free to move.

70.

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

a)

s and p only

b)

p and d only

c)

s, p, and d only

d)

s, p, d, and f

71.

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

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

72.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

73.

Nickel-59 has how many neutrons?

a)

30

b)

31

c)

32

d)

33

74.

Bromine-80 has how many neutrons?

a)

41

b)

42

c)

44

d)

45

75.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

76.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

77.

9 protons and 9 neutrons

a)

Fluorine-18

b)

Fluorine-9

c)

Fluorine-16

d)

Fluorine-18.998

78.

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

79.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

80.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

81.
Giant lattice structure held together by attraction between  positive and negatively charged ions 
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
82.
Elements such as  Silicon, diamond and graphite.  Compounds include  SiO2
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
83.
Low melting and boiling points which increase with increasing molecule size due to increased intermolecular forces.
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
84.
Melting points are very high – a large amount of energy is needed to break all the covalent bonds
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
85.
Conductors due to delocalised electrons
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
86.
Melting points are generally high – lots of energy is needed to overcome the attractions between positive ions and delocalised electrons.  
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
87.
Formulae of these might include H2O
each molecule contains 1 O and 2H atoms 
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
88.
Compounds containing a metal and non-metal.
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent 
89.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
90.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
91.
Which elements tend to lose electrons?
a)
metals
b)
nonmetals
92.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
93.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
94.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
95.
Atoms form ions in order to become
a)
isotopes
b)
stable
c)
metals
d)
nonmetals
96.

Many alloys are softer than the elements that are in them.

a)

True

b)

False

97.

Why are alloyed metals usually stronger?

a)

They have atoms of different metals in them, which makes it easier for the layer to move past each other...less likely to break

b)

They have atoms of different metals in them, which makes it harder for the layer to move past each other...less likely to break

98.

An alloy is made of __________ size particles while a pure metal is made up of _________ size particles.

a)

same, different

b)

different, same

c)

same, same

d)

different, different

99.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
100.

What charge do electrons have?

a)

Positive

b)

Neutral

c)

Negative

101.

Which two particles are contained in the nucleus of an atom?

a)

Protons and Neutrons

b)

Protons and Electrons

c)

Electrons and Neutrons

102.

Haw many maximum electrons can be present in the "M" shell of an atom?

a)

2

b)

8

c)

18

d)

32

103.

An atom has atomic number 4 the number of electrons in its outermost orbit will be ?

a)

2

b)

6

c)

4

d)

1

104.

How many energy shells/levels does this atom have?

a)

1

b)

2

c)

3

d)

4

105.
How many neutrons does a sodium atom have? (Use the image to help you)
a)
23
b)
11
c)
12
d)
34
106.
The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.
a)
9
b)
10
c)
19
d)
28
107.

The electronic configuration of 17Cl is

a)

2,8,8,1

b)

2,8,6

c)

2,8,8

d)

2,8,7

108.

Which of the following is the electronic Configuration of Sodium 11Na

a)

2,8

b)

2,8,1

c)

2,1,8

d)

8,1,2

109.

Which of the following is the correct arrangement of electrons in different shells for an element with atomic number 17 ?

a)

2,8,7

b)

8,8,1

c)

2,8,1,6

d)

2,8,2,5

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