Module 3 P1

Question 1

How are the elements arranged in the periodic table?

Answer 1

• In order of increasing atomic number
• in periods
• in groups

Question 2

How were elements arranged in Mendeleev’s original periodic table?

Answer 2

In order of increasing atomic mass

Question 3

What do periods show in the periodic table?

Answer 3

Repeating trends in physical and chemical properties.

Elements in the same period have the same number of shells

Question 4

What is periodicity?

Answer 4

The repeating pattern seem across different periods

Question 5

What do groups show in the periodic table?

Answer 5

Elements with similar chemical properties because elements in the same group have the same number of electrons in their outer shell

Question 6

What is an advantage of numbering the groups in the periodic table as 1-7 + 0 rather than 1-18?

Answer 6

The group number matched the number of electrons in the highest energy shell

Question 7

What is a disadvantage of numbering the groups in the periodic table as 1-7 + 0 rather than 1-18?

Answer 7

Doesn’t include the d block

Question 8

What is an advantage of numbering the groups in the periodic table as 1–18 rather than 1-7 + 0?

Answer 8

The numbers each column in the s, p and d blocks sequentially

Question 9

Which groups are in the s block in the periodic table?

Answer 9

Groups 1 and 2 plus hydrogen and helium

Question 10

Which groups are in the p block in the periodic table?

Answer 10

Groups 13 to 18

Question 11

Why are group 18 elements inert?

Answer 11

Their sub shells are filled

Question 12

Which groups in the p block can share electrons to form covalent bonds?

Answer 12

Groups 14-17

Question 13

Which groups in the p block are capable of gaining electrons to form negative ions?

Answer 13

Groups 16 and 17

Question 14

Key points about ionisation energies:

Answer 14

• endothermic
• always use the gas state symbol
• the lower the ionisation energy, the easier it is to form an ion
• measured in KJmol^-1

Question 15

Which factors affect an element’s ionisation energy?

Answer 15

• atomic radius
• nuclear charge
• shielding

Question 16

How do successive ionisation energies show shell structure?

Answer 16

A large increase/ jump in the ionisation energy required indicates that the electron is in a new shell/energy level.

Question 17

What do the peaks and troughs on ionisation energy graphs show?

Answer 17

Evidence of sub-shells

Question 18

What is another name for shell?

Answer 18

Energy level - the principal quantum number (n)

Question 19

What is an atomic orbital?

Answer 19

A region around the nucleus that can hold up to two electrons with opposite spins

Question 20

What shape is an a orbital?

Answer 20

Spherical

Question 21

How many s orbitals are there in each s sub-shell?

Answer 21

One

Question 22

What is the shape of a p orbital?

Answer 22

Figure of 8/ dumb-bell shape

Question 23

How many p orbitals is there in one p sub-shell?

Answer 23

3

Question 24

How many d orbitals is there in one d sub-shell?

Answer 24

5

Question 25

How many f orbitals is there in one f sub-shell?

Answer 25

7

Question 26

What are the four types of electron orbitals?

Answer 26

s, p, d, f

Question 27

How many electrons can fit in each orbital?

Answer 27

2

Question 28

Give the order in which the orbitals fill up in an electron

Answer 28

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

Question 29

In box diagrams, why do all the boxes on an energy level fill up before electrons are paired in orbitals?

Answer 29

Electrons repel each other

Question 30

Why must two electrons in an orbital have opposite spins?

Answer 30

To help counteract the repulsion between the negative charges