Periodicity Patterns

Question 1

What is the atomic radius?

Answer 1

The distance from the nucleus to the valence electron

Question 2

What properties affect the atomic radius?

Answer 2

Number of subshells - the more subshells the greater the radius
Number of electrons on the valence shell - the more electrons the lesser the radius

Question 3

Which group has the largest atomic radius?

Answer 3

Group 1

Question 4

Which group has the smallest atomic radius?

Answer 4

Group 7

Question 5

How does the atomic radius change across a period?

Answer 5

Decreases

Question 6

How does the atomic radius change down a group?

Answer 6

Increases

Question 7

What is ionisation energy?

Answer 7

The energy required to remove one mole of electrons from one mole of gaseous atoms (the energy required to remove valence electrons)

Question 8

What properties affect ionisation energy?

Answer 8

Number of subshells - the more subshells the lesser the ionisation energy required
Number of electrons on the valence shell - the more electrons the greater the ionisation energy required

Question 9

Which group has the highest ionisation energy?

Answer 9

Group 7

Question 10

Which group has the lowest ionisation energy?

Answer 10

Group 1

Question 11

How does ionisation energy change across a period?

Answer 11

Increases

Question 12

How does ionisation energy change down a group?

Answer 12

Decreases

Question 13

What is electronegativity?

Answer 13

A measure of the tendency of an atom to attract a bonding pair of electrons

Question 14

What properties affect electronegativity?

Answer 14

Number of subshells - the more subshells the lesser the electronegativity
Number of electrons on the valence shell - the more electrons the greater the electronegativity

Question 15

Which group has the highest electronegativity?

Answer 15

Group 7

Question 16

Which group has the lowest electronegativity?

Answer 16

Group 1

Question 17

How does electronegativity change across a period?

Answer 17

Increases

Question 18

How does electronegativity change down a group?

Answer 18

Decreases

Question 19

How do the properties of atoms change across a period?

Answer 19

The number of subshells stays the same but the number of electrons on the valence shell increase

Question 20

How do the properties of atoms change down a group?

Answer 20

The number of subshells increases but the number of electrons on the valence shell stays the same

Question 21

What molecules does ionic bonding occur between?

Answer 21

Metals and non metals (oppositely charged ions)

Question 22

How are electrons arranged during ionic bonding?

Answer 22

Donated and recieved

Question 23

What structure does ionic bonding result in?

Answer 23

Giant lattice

Question 24

What are the melting and boiling points of ionic compounds?

Answer 24

High - due to strong intermolecular forces

Question 25

Name a biologically important ionic compound.

Answer 25

Hydroxyapetite - the mineral component of bone that gives it its compressive strength

Question 26

Explain the solubility of ionic compounds.

Answer 26

Water soluble (negative ions interact with positive hydrogen, positive ions interact with negative oxygen)

Question 27

What molecules does covalent bonding occur between?

Answer 27

Non metals

Question 28

How are electrons arranged during covalent bonding?

Answer 28

Pairs of electrons are shared

Question 29

What are the melting and boiling points of covalent compounds?

Answer 29

Low - although there are strong intramolecular forces the intermolecular forces are weak

Question 30

What is carbon SP3 hybridisation?

Answer 30

Carbons 2S and 2P subshells combine to form an SP3 subshell which contains 4 electrons (more likely to complete its outer shell)

Question 31

What is a single carbon bond called?

Answer 31

Sigma

Question 32

What is a double carbon bond called?

Answer 32

Sigma-Pi