Periodicity

Question 1

Name the 4 types of bonding structures

Answer 1

Metallic
Monatomic
Covalent molecular
Covalent network

Question 2

In the first 20 elements, name the elements with metallic bonding

Answer 2

Li Be Na Mg Al K Ca

Question 3

In the first 20 elements, name the elements with monatomic bonding

Answer 3

He Ne Ar

Question 4

In the first 20 elements, name the elements with covalent molecular

Answer 4

H2 N2 O2 F2 Cl2 P4 S8 and fullerenes

Question 5

In the first 20 elements, name the elements with covalent networks

Answer 5

B C (diamond and graphite) Si

Question 6

The noble gases are what type of elements

Answer 6

Monatomic

Question 7

What kind of forces are between the atoms of noble gases

Answer 7

London dispersion forces

Question 8

Describe London dispersion forces

Answer 8

Weak forces of attraction between atoms and molecules when temporary dipoles are formed within atoms or molecules

Question 9

What do the halogens Hydrogen, Nitrogen, oxygen exist as?

Answer 9

Individual diatomic molecules

Question 10

Hydrogen etc have London dispersion forces between the molecules, what are these?

Answer 10

Intermolecular forces

Question 11

Hydrogen etc have strong covalent bonds between the atoms in a molecule, what are these known as?

Answer 11

Intramolecular forces

Question 12

Sulfur and phosphorus have strong London dispersion forces. What state are they in at room temp?

Answer 12

Solids

Question 13

Carbon can exist as fullerenes, describe these.

Answer 13

Large individual covalent molecules, which have molecules with 60 carbon atoms or more.

Question 14

What shake can fullerene molecules be?

Answer 14

Ball or tube-shaped

Question 15

Why do fullerenes have high melting points?

Answer 15

Large London dispersion forces between molecules

Question 16

Carbon can exist as covalent networks in the form of?

Answer 16

Diamond and graphite

Question 17

The carbon atoms in diamond are bonded to …

Answer 17

4 other carbons in a large, strong, three-dimensional network. That is very hard.

Question 18

The structure of diamond results in diamond having?

Answer 18

A very high melting point

Question 19

Why is diamond a non-conductor of electricity?

Answer 19

It has no delocalised electrons

Question 20

Graphite forms a network that each carbon is bonded to? Can it conduct electricity?

Answer 20

Three other carbons, which results in graphite having delocalised electrons, and do conducts electricity.

Question 21

The carbon atoms in graphite form what kind of shape? What are they held together by?

Answer 21

Hexagonal plates which are held together by London dispersion forces

Question 22

The layers in graphite can be easily seperated, what does this result in?

Answer 22

Graphite’s not as hard as diamond

Question 23

Boring and Silicon are covalent networks, describe their properties.

Answer 23

High melting and boiling points

Question 24

What patterns exist when going down a group, or across a period?

Answer 24

Covalent radii, ionisation energy, electronegativity

Question 25

Describe the covalent radius

Answer 25

Is half the distance between the nuclei of two atoms, joined by a covalent bond

Question 26

What happens to the covalent radius going down a group and why?

Answer 26

Covalent radius increases as the number of occupied electron shells increases and shields the outer electrons from the pull of the nucleus

Question 27

What happens to the covalent radius going across a period?

Answer 27

Decreases as there is no increased shielding as the electrons are added to the same shell, stronger nuclear charge

Question 28

What is ionisation energy?

Answer 28

The energy required to remove one mole of electrons from one mole of atoms in the gaseous state

Question 29

What happens to the first ionisation energy going down a group?

Answer 29

Decreases going down a group as the outer electrons get further away from the nucleus and are shielded by from the pull of the nucleus by shells of the inner electrons

Question 30

What happens to the first ionisation energy across a period?

Answer 30

Generally increases as the outer electrons are held more tightly by the nucleus as electrons are added to the same energy level and energy he charge on the nucleus increases

Question 31

What is electronegativity?

Answer 31

A measure of the attraction an atom has for the electrons of the bond

Question 32

What happens to electronegativity going down a group?

Answer 32

Decreases as atoms get bigger and the attraction of the nucleus for bonding electrons decreases

Question 33

What happens to electronegativity going across a period?

Answer 33

Increases as the atoms get smaller, and the attraction of the nucleus for the bonding electrons increases