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2nd Evaluation Grade9 Term2

Total questions: 47

Worksheet time: 36mins

Name
Class
Date
1.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

2.

Metals tend to

a)

gain electrons

b)

lose electrons

3.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
4.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
5.

When a nonmetal gains electrons, it becomes this type of ion.

a)

Anion

b)

Cation

6.

When a metal loses electrons, it becomes this type of ion.

a)

anion

b)

cation

7.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
8.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
9.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
10.

The Lewis Dot structure for aluminum would have ______ electrons.

a)

13

b)

3

c)

8

d)

27

11.

Valence electrons are those that are

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

in the outermost energy level of the atom.

d)

unable to become involved in chemical bonding.

12.

Which of the following is not a way that ions can form?

a)

gaining electrons

b)

gaining protons

c)

losing electrons

d)

All of the above are ways that ions can form.

13.

Oxygen has six valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

14.

Which of the following best describes the correct arrangement of the electrons in a Lewis dot structure for phosphorus?

a)

five single electrons

b)

two pairs of electrons and one single electron

c)

three pairs of electrons and one single electron

d)

three single electrons and one pair of electrons

15.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

16.

Most elements are most stable when their outermost energy levels contain ________ electrons.

a)

2

b)

6

c)

8

d)

18

17.

Look at the Periodic table. Which of the following elements would you expect to form an ion that has the same charge as the oxide ion?

a)

calcium

b)

boron

c)

sulfur

d)

chlorine

18.

Which of the following pairs of atoms and/or ions is isoelectronic?

a)

Na and K

b)

Cl and Cl-1

c)

Ne and Na+1

d)

O-2 and S-2

19.

Which of the following tend to gain electrons when forming ions?

a)

metalloids

b)

metals

c)

nonmetals

d)

cations

20.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
21.
Which has the greater EN: 
N or C?
a)
C
b)
N
22.
Which has the greater EN: 
H or F?
a)
H
b)
F
23.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
24.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
25.
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)
26.
Based on electronegativity trends in the periodic table, which of the following is the most likely value for the electronegativity of silicon?
a)
2.44
b)
1.23
c)
2.22
d)
2.03
27.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
28.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
29.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
30.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
31.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
32.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
33.
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.
34.
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.
35.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
36.

How does the ionization energy change across a period ?

a)

increases

b)

decreases

c)

stays the same

37.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

38.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

39.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
40.

How ionic bonds are made?

a)

As a result of attraction between neutrons and negative ions

b)

As a result of attraction between positive and negative ions

c)

As a result of attraction between electrons

d)

As a result of attraction between molecules

41.

Choose which of the following compounds contain IONIC Bonds (you may choose more than one answer)

a)

H2O

b)

SO2

c)

AlCl3

d)

H2

e)

MgI2

42.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
43.
Refer to the image. Which diagrams correctly represent the transfer of electrons in ionic bonding?
a)
Diagram 3 and 4
b)
Diagram 1 and 2
c)
Diagram 1 and 4
d)
Diagram 2 and 3
44.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

45.

Which of the following compounds is considered ionic?

a)

CO2

b)

NaCl

c)

H2

d)

SCl2

46.

FeCl3 is considered a(n):

a)

Ionic Compound

b)

Covalent Compound

c)

Metallic Compound

d)

Element

47.

Select the correct Lewis structure for Li2O:

a)
b)
c)
d)

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