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Chemical Bonds and the periodic table

Total questions: 55

Worksheet time: 55mins

Name
Class
Date
1.

What type of bond is formed when electrons are transferred from one atom to another?

a)

Metallic bond

b)

Hydrogen bond

c)

Ionic bond

d)

Covalent bond

2.

What type of bond is found in metals?

a)

Metallic bond

b)

Covalent bond

c)

Hydrogen bond

d)

Ionic bond

3.

Describe the properties of metallic bonds.

a)

Metallic bonds are not characterized by delocalization of electrons

b)

Metallic bonds are formed between non-metal atoms

c)

Metallic bonds are formed between metal atoms and are characterized by the delocalization of electrons, high electrical and thermal conductivity, malleability, and ductility.

d)

Metallic bonds have low electrical and thermal conductivity

4.

The 3 types of chemical bonds are ________, ________, and ______. (Choose 3)

a)

ionic

b)

valence

c)

covalent

d)

metallic

e)

atomic

5.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
6.

A bond between two nonmetal atoms is a __________ bond.

a)

ionic

b)

nuclear

c)

metallic

d)

covalent

7.

Which of the following is NOT a covalent bond?

a)

K2S

b)

H2O

c)

I2

d)

CO2

8.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

9.
What is the name for an ion with a negative charge?
a)
cation
b)
anion
c)
onion
d)
union
10.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

11.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
12.
What is the name for an ion with a positive charge?
a)
cation
b)
anion
c)
onion
d)
union
13.

Complete the general equation:

Metal + Acid ->

a)

Salt + Water

b)

Salt + Hydrogen

c)

Salt

14.

Complete the equation:

Sodium + Hydrochloric Acid ->

a)

Sodium Hydroxide + Hydrogen

b)

Sodium Chloride + Hydrogen

c)

Chloric Sodium + Hydrogen

d)

Sodium Chloride + Water

15.
A displacement reaction will occur when...
a)
a more reactive metal displaces a less reactive metal from its compound.
b)
A less reactive metal displaces a more reactive metal from its compound
c)
Displacement only occurs when two of the same metals are reacted 
d)
Displacement reactions will only occur in metals above iron in the reactivity series
16.

The following are example(s) of transition metals (check all that apply):

a)

sodium

b)

gold

c)

cobalt

d)

boron

e)

plutonium

17.

Why do transition metals get different rules for their names and formulas?

a)

atoms are larger

b)

cations have many different charges

c)

they have more protons

d)

they are rare elements

18.

What is the correct name for this compound?

a)

fluorine chlorine

b)

iron chloride

c)

iron(II) chloride

d)

iron(I) chloride

19.

What is the formula for iron(III) oxide?

a)

FeO

b)

Fe(III) O

c)

Fe2O3

d)

Fe3O2

20.

What is the name of this compound? Na2S

a)

nitrogen(II) sulfide

b)

sodium(II) sulfide

c)

sodium sulfide

d)

sodium(I) sulfide

21.
What would be the proper chemical formula for combining Al3+ and l- :
a)
Al l3
b)
Al3l
c)
Al l
d)
Al3 l3
22.

Correct diagram for HF

a)
b)
c)
d)
23.

Correct diagram for CF4

a)
b)
c)
24.

What type of forces act between the ions in an ionic compound?

a)

Electrostatic

b)

Frictional

c)

Gravitational

d)

Magnetic

25.
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
26.

Which alkali metal is most reactive out of the following

a)

rubidium

b)

potassium

c)

sodium

d)

lithium

27.

How many electrons do the alkali metals have in their outer shell?

a)

1

b)

2

c)

8

d)

7

28.

What happens to the melting point of the alkali metals as you move down the group?

a)

decreases

b)

increases

29.

How does a group 1 metal atom form an ion?

a)

lose 1 electron

b)

lose 2 electrons

c)

gain 1 electron

d)

gain 2 electrons

30.

Which of the following is NOT a property of group 1 metals?

a)

More dense than water

b)

less dense than water

c)

low melting point

d)

soft

31.

What is the formula of a group 1 metal oxide?

a)

M2O

b)

MO

c)

MO2

d)

Mo

32.

What group are the Halogens?

a)

6.9

b)

7

c)

8

d)

3

33.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

34.

Which of the halogens could able to make the strongest ionic bond with Sodium metal?

a)

Iodine

b)

Bromine

c)

Chlorine

d)

Flourine

35.

Complete the following equation: Iodine + Potassium Bromide -->

a)

Potassium Iodine + Bromine

b)

Iodine + Potassium Bromide

c)

No reaction

36.

Complete the following equation: Bromine + Potassium Iodide -->

a)

Potassium Iodine + Bromine

b)

Iodine + Potassium Bromide

c)

No reaction

37.

Which of the following is NOT a property of noble gases?

a)

They have a complete outer shell.

b)

They are highly reactive.

c)

They are colorless, odorless, and tasteless.

d)

They exist as monatomic gases at room temperature.

38.

What is the primary use of Helium (He)?

a)

In light bulbs as a filament

b)

In refrigeration systems

c)

In balloons and airships as a lifting gas

d)

In fireworks to produce colors

39.

Why are noble gases generally unreactive?

a)

They have low atomic masses.

b)

They have low melting points.

c)

They have a complete outer electron shell.

d)

They have high melting points.

40.

Which noble gas is used in light bulbs to prevent the tungsten filament from oxidizing?

a)

Neon

b)

Xenon

c)

Argon

d)

Radon

41.

Which noble gas has the highest boiling point?

a)

Helium

b)

Neon

c)

Argon

d)

Radon

42.

Fe2+ and Fe3+ are both ions of iron. What is different about them?

a)

they have different numbers of protons

b)

they have different numbers of neutrons

c)

they have a different charge

d)

they are different elements

43.

Where are the transition metals located on the periodic table?

a)

blue square

b)

red square

c)

yellow square

44.

The table shows information about two metals. One metal is cobalt and the other is potassium. Suggest which metal is cobalt.

(a)  

45.

Metal X: Reacts vigorously with oxygen to form a white compound.

Metal Y: Reacts slowly with oxygen to form a red compound.

Metal Z: Reacts slowly with oxygen to form a white compound.


Which metal is most likely to be a transition metal?

(a)  

46.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

47.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

48.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds.

d)

They have many weak bonds.

49.

Which two elements would NOT form an ionic bond?

a)

calcium and lithium

b)

calcium and oxygen

c)

lithium and oxygen

d)

calcium and carbon

50.

Compound X conducts electricity in aqueous solution or molten state. It also has a high melting point and boiling point.

What is X?

a)

CCl4CCl_4

b)

MgCl2MgCl_2

c)

CO2CO_2

d)

NH3NH_3

51.

Compound X has high melting and boiling point. Which of the following explains the statement.

a)

Compound X has strong covalent bond between ions.

b)

Compound X has strong electrostatic force between ions.

c)

Compound X has strong electrostatic force between molecules.

d)

Compound X has strong covalent bond between atoms and giant lattice structure.

52.

What is the property of the compound?

a)

Can conduct electricity in solid state

b)

Exists as liquid at room temperature

c)

Has low melting and boiling points

d)

Soluble in water

53.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
54.

H2O, Cl2, NH3

Do the bonds above require a high temperature to melt?

a)

Yes, because they have strong forces holding them together.

b)

No, those are ionic bonds.

c)

No, those are all covalent bonds that have weaker forces holding them together.

d)

Yes, because they are metallic bonds.

55.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly

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