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The Periodic Table (Module 3.1)

Total questions: 44

Worksheet time: 32mins

Name
Class
Date
1.

How are the elements organized in the modern periodic table?

a)

Atomic numbers

b)

Atomic mass

c)

Reactivity

d)

Neutron number

2.

Atomic numbers are also the number of ..... in an element

a)

Protons

b)

Neutrons

c)

Electrons

d)

Neutrons and protons

3.

Metals can be found in the periodic table from groups...

a)

1 - 16

b)

14 - 18

c)

1 - 13

d)

1 - 2

4.

Non-metals can be found in the periodic table from groups ....

a)

1 - 16

b)

14 - 18

c)

1 - 13

d)

17 -18

5.

Elements in the same group have the same...

(a)  

6.

Which sub-shell has the LOWEST energy level?

a)

4s

b)

3d

7.

Elements in groups 1-2 have outer electrons in...

a)

s - orbitals

b)

p - orbitals

c)

d - orbitals

d)

f - orbitals

8.

Elements in groups 13 - 18 have outer electrons in...

a)

s - orbitals

b)

p - orbitals

c)

d - orbitals

d)

f - orbitals

9.

Elements in groups 3 - 12 have outer electrons in...

a)

s - orbitals

b)

p - orbitals

c)

d - orbitals

d)

f - orbitals

10.

The first ionization energy is a measure of how easily an atom uses an electron and forms a...

a)

+1 ion

b)

-1 ion

c)

Radicle

d)

Compound

11.

Which factors affect ionization energy?

a)

Atomic radius

b)

Nuclear charge

c)

Electron screening/shielding

d)

Metal or non-metal

12.

Ionization reactions are...

a)

Exothermic

b)

Endothermic

13.

Successive ionization energies get more and more...

a)

Exothermic

b)

Endothermic

c)

Reactive

d)

Acidic

14.

If there is a big change in successive ionization energy it means the (a)   has changed

15.

The ionization energy increases across a period due to...

a)

Atomic radius decrease

b)

Nuclear charge increases

c)

Electron shielding decrease

d)

Reactivity increase

16.

Electrons that are spin-paired have lower ionization energy due to...

(a)  

17.

The ionization energy decreases down a group due to...

a)

Atomic radius increase

b)

Electron shielding increase

c)

Nuclear charge decreases

d)

Atomic radius decreases

18.

The ionization energy decreases down a group despite...

a)

Atomic radius increase

b)

Electron shielding increase

c)

Nuclear charge increases

d)

Atomic radius decreases

19.

A giant metallic lattice structure consists of...

a)

Positive ions

b)

Negative ions

c)

Delocalised electrons

d)

Delocalised neutrons

20.

Giant metallic structures have (a)   melting and boiling points

21.

Metals are good conductors of electricity due to...

(a)  

22.

Boron, carbon, and silicon are all examples of what type of structure?

(a)  

23.

What structure does the majority of non-metal have?

(a)  

24.

Molecule of Nitrogen in its standard state, has how many nitrogen atoms?

a)

1

b)

2

c)

4

d)

8

25.

Molecule of Oxygen in its standard state, has how many oxygen atoms?

a)

1

b)

2

c)

4

d)

8

26.

Molecule of Fluorine in its standard state, has how many fluorine atoms?

a)

1

b)

2

c)

4

d)

8

27.

Molecule of Phosphorus in its standard state, has how many phosphorus atoms?

a)

1

b)

2

c)

4

d)

8

28.

Molecule of Sulfur in its standard state, has how many sulfur atoms?

a)

1

b)

2

c)

4

d)

8

29.

A high melting point is caused by strong...

a)

Intermolecular forces

b)

Intramolecular forces

c)

Metallic bonds

d)

Covalent bonds

30.

As you go down group two, the reactivity...

(a)  

31.

Down group 2, the ionization energy...

(a)  

32.

Group 2 elements ...

a)

Reactive metals

b)

Strong reducing agents

c)

2+ ions

d)

Have relatively high melting and boiling points

33.

When group 2 elements are reacted with oxygen, what is formed?

(a)  

34.

Reactions between group 2 elements and water produce?

a)

Metal hydroxide

b)

Hydrogen

c)

Metal Oxide

d)

Oxygen

35.

Reactions between group 2 elements and dilute acids produce?

a)

Salt

b)

Hydrogen gas

c)

Metal oxides

d)

Water

36.

Reactions between group 2 oxides and water produce?

(a)  

37.

The solubility and alkalinity of group 2 hydroxides... down the group

(a)  

38.

What are some uses of group 2 compounds?

a)

Neutralizing acidic soils

b)

Indigestion remedies

c)

Building and construction use

d)

Dental hygiene products

39.

What are the properties of halogens?

a)

Low melting and boiling points

b)

High melting and boiling points

c)

Exist as diatomic atoms

d)

Have a high density

40.

Which halogen is liquid in its standard state?

(a)  

41.

In which orbital can the halogens' outer electrons be found?

(a)  

42.

Which halogen has the lowest boiling point?

a)

Fluorine

b)

Chlorine

c)

Bromine

d)

Iodine

43.

Which halogen is the most reactive?

a)

Fluorine

b)

Chlorine

c)

Bromine

d)

Iodine

44.

What causes halogen reactivity to decrease?

a)

Atomic radius increases

b)

Electron shielding increases

c)

Ability to gain electrons decreases

d)

Nuclear charge decreases

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