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Periodic law and Bonding

Total questions: 36

Worksheet time: 27mins

Name
Class
Date
1.

Which of the following has a full valence shell?

a)

Oxygen

b)

Neon

c)

Barium

d)

Carbon

2.

Which type of bond has an equal sharing of electrons?

a)

Polar Covalent

b)

Non Polar Covalent

c)

Ionic

d)

Metallic

3.

Atoms gain or lose electrons to become stable by satisfying this rule.

a)

Lewis Structure rule

b)

Periodic Law

c)

octet rule

d)

Ionic Law

4.

This could be the dot diagram of

a)

Ne

b)

H

c)

C

d)

Ge

5.

What usually forms the positive ion?

a)

Metal

b)

Non Metals

c)

None

6.

Covalent compounds _________.

a)

Share electrons

b)

transfer electrons

c)

contain a sea of electrons

d)

conduct electricity

7.

What two types of atoms make a covalent bond?

a)

2 Non metals

b)

1 Non metal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

8.

Predict the bond that will form between Be and F.

a)

Ionic

b)

Covalent

9.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
10.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
11.
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
12.
Which type of bond creates a "sea" of electrons between atoms?
a)
Ionic Bonds
b)
Covalent Bonds
c)
Metallic Bonds
d)
Saving Bonds
13.
The picture depicts what kind of bond illustration? 
a)
metallic bond
b)
ionic bond
c)
covalent bond
d)
hydrogen bond
14.
All chemical bonds involve two atoms sharing electrons.
a)
True
b)
False
15.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
16.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
17.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
18.

Which is the correct Lewis Structure for oxygen?

a)
b)
c)
d)
19.

Does the following reference Polar, Nonpolar, or both:

"unequal sharing of electrons"?

a)

Polar

b)

Nonpolar

c)

Both

20.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

21.

The horizontal (side to side) rows in the Periodic Table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

22.
How many valence electrons?
a)
2
b)
3
c)
5
d)
10
23.

What is the name of the group that never reacts

a)

noble gases

b)

transition

c)

halogens

d)

borons

24.
Why does K become positive when it bonds to Cl to form KCl?
a)
Because it loses an electron to have a full valence shell 
b)
Because it gains an electron to have 2 valence electrons
c)
Because it loses an electron to become negatively charged
d)
Because Cl gives away its 7 electrons to Na to form an equal charge 
25.

Elements that are shiny, conduct electricity and heat are called:

a)

metal

b)

nonmetal

c)

metalloid

d)

radioactive

26.

What are the elements along the dark line on the periodic table called?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

27.

Atoms in the periodic table get bigger when going down a column or group. 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 neutrons.

28.

As you move across the periodic table atoms tend to get smaller because:

a)

the atoms have more mass.

b)

the atoms have more neutrons.

c)

the atoms have more protons.

d)

the atoms have energy levels.

29.

As we go from the left side to the right side on the periodic table, electronegativity:

a)

Increases

b)

Decreases

c)

Remains constant

30.

Which of the following elements has the highest electronegativity?

a)

Cl

b)

Si

c)

Mg

d)

Ca

31.

Atoms that have a high electronegativity:

a)

give up their electrons easily.

b)

hold on to their electrons tightly.

c)

have more electron shells.

d)

prefer to share their electrons.

32.

The energy required to remove the most loosely bound electron is the definition of:

a)

Electronegativity

b)

Electron Affinity

c)

Atomic Radius

d)

Ionization Energy

33.

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)

34.
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.
35.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
36.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 

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