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chemistry act

Total questions: 77

Worksheet time: 50mins

Name
Class
Date
1.

An electron is:

a)

Positively charged

b)

Negatively charged

c)

Neutral

2.

The atomic number of an element tells us:

a)

The number of protons

b)

The number of neutrons

c)

The number of protons plus neutrons

d)

The atomic mass

3.

An ice cube melting is an example of a:

a)

Physical change

b)

Chemical change

4.

Beryllium's atomic number is 4 and its atomic mass is 9. How many neutrons will a beryllium atom have?

a)

4

b)

5

c)

9

d)

13

5.

Which of these is NOT a physical property?

a)

Colour

b)

Melting Point

c)

Hardness

d)

Flammability

6.

In a Bohr-Rutherford Diagram, the innermost shell has a maximum of how many electrons?

a)

1

b)

2

c)

8

d)

18

7.

Soda with ice cubes is an example of a:

a)

Homogeneous mixture

b)

Heterogeneous mixture

c)

Element

d)

Compound

8.

Calcium's atomic number is 20. A calcium ion has a charge of +2. How many electrons does a calcium ion have?

a)

18

b)

20

c)

22

d)

40

9.

Where would you tend to find non-metals on the periodic table?

a)

In the left-most groups

b)

In the middle of the table

c)

In the right-most groups

d)

At the bottom of the table

10.

A rotting apple is an example of a:

a)

Physical change

b)

Chemical change

11.

Boron's atomic number is 5. How many valence electrons will a boron atom have?

a)

1

b)

2

c)

3

d)

5

12.

If an ion is positively charged, it is referred to as a:

a)

Anion

b)

Cation

13.

The charge of an ion is -3. This means the atom must have:

a)

Gained 3 protons

b)

Lost 3 protons

c)

Gained 3 electrons

d)

Lost 3 electrons

14.

Is solubility (ability to dissolve) a physical property or a chemical property?

a)

Physical Property

b)

Chemical Property

15.

A sulfur atom has 16 protons and 16 neutrons. What is its atomic mass?

a)

16

b)

24

c)

32

d)

48

16.

Fill-in-the-blank: Elements in the same ____________ have similar chemical properties.

a)

group

b)

row

c)

period

17.

Here is the Bohr-Rutherford diagram for a neutral Nitrogen atom. To have a completely filled outer shell, it will need to:

a)

Lose 3 electrons

b)

Gain 3 electrons

c)

Lose 5 electrons

d)

Gain 5 electrons

18.

Which of the following describe ionic bonding?

a)

It involves the transfer of electrons

b)

It involves sharing of electrons.

c)

It involves transfer of protons.

d)

It involves sharing of protons.

19.

From the periodic table, which pair of elements can combine to form ionic bonds?

a)

Ca and O

b)

H and N

c)

H and Cl

d)

Xe and Fe

20.

Bond that is formed when electrons are equally shared.

a)

non polar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

metallic bond

21.

Which of the following pairs of atoms is most likely to form a covalent compound?

a)

Ba and Cl

b)

Na and O

c)

Mg and Br

d)

C and O

22.

In Ionic Bonding, metals most likely to

a)

lose electron

b)

lose proton

c)

gain electron

d)

gain proton

23.

Atoms need to be bonded in order to attain the stability needed like that of _______.

a)

alkali metals

b)

alkaline earth metals

c)

noble gases

d)

semi metals

24.

What is the chemical formula of Sulfur Hexafluoride?

a)

S6F

b)

S6F6

c)

SF6

d)

6SF

25.

What is the chemical name of SO2

a)

monosulfur dioxide

b)

disulfur monoxide

c)

sulfur dioxide

d)

disulfur oxide

26.

What is the chemical name of the ionic compound formed from the attraction between K+1 and S2- ions?

a)

Potassium Sulfide

b)

Potassium disulfide

c)

dipotassium monosulfide

d)

dipotassium sulfide

27.

In metallic bond, it results from

a)

the attraction between cations and anions

b)

the sharing of electrons between non metals

c)

the attraction between the free moving electrons and the positive ions.

28.

Predict the formula of the ionic compound that forms from Potassium and Chlorine

a)

 KCl2KCl_2  

b)

 KClKCl  

c)

 P2ClP_2Cl  

d)

 PClPCl  

29.

Ionic compounds ...

a)

do not conduct electricity

b)

conduct electricity when dissolved in water

c)

conduct electricity when melted

d)

are malleable

30.

Which of the following is a correct lewis structure for carbon dioxide CO2?

a)
b)
c)
d)
31.

The electrons involved in the formation of a chemical bond are called

a)

valence electrons

b)

kernels

c)

lewis electrons

d)

dipoles

32.

Elements in group 6A tend to form

a)

1+ ions

b)

2- ions

c)

8- ions

d)

6- ions

33.

Which property does a covalent bond have?

a)

Forms alloys

b)

Consists of metals only

c)

Is a good conductor of heat

d)

Has a low melting point

34.

When two atoms share electrons, a chemical bond is formed. What is this type of bond called?

a)

Polyatomic bond

b)

Crystalline bond

c)

Ionic bond

d)

Covalent bond

35.

What property does a metallic bond have?

a)

Forms molecules

b)

Includes only nonmetals

c)

Is a poor conductor of heat

d)

Is a solid at room temperature.

36.

Which characteristic does an ionic bond have?

a)

It is made of metals only

b)

It has low melting points

c)

It is ductile and malleable

d)

It has high melting points.

37.

What type of bond do hydrogen and carbon form?

a)

Metallic

b)

Covalent

c)

Ionic

d)

Nonpolar

38.
An ionic bond
a)
Shares electrons
b)
Transfers electrons
c)
Has a sea of electrons
39.
A covalent bond
a)
Shares electrons
b)
Transfers electrons
c)
Has a sea of electrons
d)

Transfers neutrons

40.
Identify the correct Lewis structure for HCl
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
41.

Identify the correct Lewis structure for COH2.

a)

Option 1

b)

Option 2

c)

Option 3

d)

Option 4

42.

Identify the correct Lewis structure for MgF2.

a)

Option 1

b)

Option 2

c)

Option 3

d)

Option 4

43.
Which of these is covalent?
a)
option 1
b)
option 2
c)
option 3
d)
option 4
44.
What charge does a Boron ion have?
a)
+1
b)
+2
c)
+3
d)
-3
45.
How many valence electrons does carbon have?
a)
4
b)
2
c)
3
d)
5
46.
How many valence electrons does hydrogen have?
a)
2
b)
1
c)
3
d)
4
47.
A ___________ is an ion with a positive (+) charge.
a)
solute
b)
anion
c)
cation
d)
ion
48.

An ___________ is an ion with a negative (-) charge.

a)
solute
b)
anion
c)
cation
d)
ion
49.

Covalent substances like sugar tend to (select all that may apply):

a)

Have low melting and boiling points

b)

Not conduct electricity very well

c)

Not normally dissolve in water

d)

Have high melting and boiling points

50.

Which of these elements does not bond to form molecules: oxygen, chlorine, neon, or sulfur?

a)

Oxygen

b)

Chlorine

c)

Neon

d)

Sulfur

51.

What type of bond is formed between the following atoms: CCl₄?

a)

Ionic

b)

Covalent

52.
What type of bond is formed between the following atoms: Fe₂O₃
a)
Ionic
b)
Covalent
53.

What type of bond is formed between the following atoms: AlBr₃?

a)

Ionic

b)

Covalent

54.

What type of bond is formed between the following atoms: HF?

a)

Ionic

b)

Covalent

55.

What type of bond is formed between the following atoms: CO₂?

a)

Ionic

b)

Covalent

56.

What type of bond is formed between the following atoms: CO₂?

a)

Ionic

b)

Covalent

57.

What type of bond is formed between the following atoms: NO₂?

a)

Ionic

b)

Covalent

58.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
59.
Rutherford discovered the...
a)
electron
b)
proton
c)
neutron
d)
nucleus
60.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
61.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
62.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
63.
An ______________ is the same element, with the same number of protons, but different numbers of neutrons
a)
Atom
b)
Isotope
c)
Atomic Number
d)
Mass Number
64.
The smallest particle into which an element can be divided and still be the same substance
a)
neutron
b)
atom
c)
electron
65.
What scientist first developed 4 rules for atomic theory, and helped kick start modern chemistry?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
66.
Niels Bohr suggested that electrons.......
a)
are found in specific orbits
b)
electrons are scattered throughout the atom
c)
electrons move according to their energy level
d)
electrons are positive
67.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
68.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
69.
What is the atomic mass (rounded to the nearest whole number) of this element
a)
196
b)
196.95
c)
197
d)
79
70.
Because atoms are neutral, the number of protons will be equal to the number of __________ in an atom.
a)
Positrons
b)
Neutrons
c)
Electrons
d)
Nuclei
71.
The three main subatomic particles are electrons, protons and ____________.
a)
photons
b)
neurons
c)
neutrons
d)
quarks
72.
What are the two main parts of the atom?
a)
nucleus and cytoplasm
b)
nucleus and electron cloud
c)
core and electron cloud
d)
protons and neutrons
73.
The conservation of ___ explains the process of nuclear decay reactions.
a)
mass
b)
definite
c)
multiple
74.
Identify letter A
a)
Nucleus
b)
Neutrons
c)
Protons
d)
Electrons
75.
Identify letter B
a)
Nucleus
b)
Neutrons
c)
Protons
d)
Electrons
76.
Identify letter C
a)
Nucleus
b)
Neutrons
c)
Protons
d)
Electrons
77.
Identify letter D
a)
Nucleus
b)
Neutrons
c)
Protons
d)
Electrons

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