Periodic Trends In Bonding And Structure

Question 1

Metals and non metals on the periodic table

Answer 1

Changeover from metal to non metal takes place on diagonal line
Elements near divide show in between properties, metalloid
More metals than non metals

Question 2

Metallic bonding

Answer 2

Each atom has donated outer shell electrons to a shared pool of delocalised electrons
Cations consist of nucleus, inner electron shells
Cations in fixed positions, maintain metal structure and shape
Delocalised electrons, mobile
Giant metallic lattice

Question 3

Properties of metals

Answer 3

Strong metallic bonds
High electrical conductivity
High melting and boiling points
Insoluble

Question 4

Electrical conductivity of metals

Answer 4

Conduct in solid and liquid states

Delocalised electrons move through structure carrying charge

Question 5

Metallic bonding

Answer 5

Strong electrostatic attraction between cations and delocalised electrons

Question 6

Melting and boiling points in metals

Answer 6

Most have high melting and boiling points
Depends on strength of metallic bonds holding atoms together
High temperatures are necessary to provide the large amount of energy needed to overcome the strong electrostatic attraction between cation, electrons

Question 7

Solubility of metals

Answer 7

Metals do not dissolve

Any interactions would lead to a reaction rather than dissolving

Question 8

Giant covalent structures

Answer 8

Boron, carbon, silicon

No intermolecular forces, network of strong covalent bonds only

Question 9

Giant covalent lattice

Answer 9

Billions of atoms are held together by a network of strong covalent bonds

Question 10

Giant covalent properties

Answer 10

High melting and boiling point
Insoluble in almost all solvents
Non conductors except graphite, graphene

Question 11

Melting and boiling points of giant covalent structures

Answer 11

High melting and boiling points

Covalent bonds are strong, high temperatures needed to break them

Question 12

Solubility of giant covalent structures

Answer 12

Insoluble in almost all solvents

Covalent bonds holding atoms in the lattice are too strong to be broken

Question 13

Electrical conductivity of giant covalent structures

Answer 13

Non conductors in diamond, silicon
All 4 outer shell electrons involved in covalent bonding, non available for conducting, electricity
Graphene, graphite have free electrons, conduct electricity

Question 14

Giant covalent lattice

Answer 14

Billions of atoms are held together by a network of strong covalent bonds

Question 15

Graphene

Answer 15

Single layer of graphite

Hexagonally arranged carbon atoms linked by strong covalent bonds, 1 free electrons

Question 16

Graphite

Answer 16

Parallel layers of hexagonally arranged carbon atoms, stack of graphene layers
Strong covalent bonds and weak London forces, 1 spare electron

Question 17

Periodic trends in melting points

Answer 17

Melting point increases from Group 1-14(giant metallic, giant covalent)
Sharp decrease in melting point between Group 14-15
Melting points comparatively low from Group 15-18 (simple molecular)