CHEM TYPES OF SOLIDS L2

Type of solid (E.g NaCL, Kl, FeCl2) (m-nm)

IONIC

A 3D lattice of alternativing positive and negative ions held together by strong ionic bonds.

Ions are the charged molecules

Type of solid (E.g Cu, Mg, Na, Fe) (m-m) STRUCTURE

METALLIC (conducts electricity)

Either

A 3D lattice of atoms held together by strong metallic bonds

OR

A 3D lattice of Cations in a “sea” of delocalised(free to move) electrons held together by strong metallic bonds.

brittle

Shatters when hit.

Electrical conductors require..

free- moving charged particles

• delocalised e-

• ions

Malleability

Doesn’t shatter when hit, bendy, can be moulded into different shapes.

Brittleness of ionic solids explanation

1. Structure + force applied

2. Ions displaced + ‘like’ charges align

3. Replusions + shatter

Metals are malleable because….

The metallic bonds are non-directional, allowing the atoms to move without disrupting the bond.

Melting/boiling point depends on

The strength of the named attractive forces between the named particles.

Type of solid

(E.g CCl4, H20, CO2)

Structure

MOLECULAR

molecules held together by weak intermolecular forces.

• cannot conduct electricity

Type of solid

(E.g Cdia, Cgra, Si, Sio2)

(nm-nm)

STRUCTURE

GIANT COVALENT NETWORK

A 3D lattice of atoms held together by strong covalent bonds

Exception- Cgra

Graphite is made up of 2D layers where each C atom is bonded to 3 other C atoms. Each C atom has a delocalised electrons.

Ductile

Can be drawn into wire(s)

Dissolving template

1. Structure(solid + solvent)

2. Attractions

3. Pull apart and surronded

Polarity of solvents

1. Water

2. Cyclohexane

nonmetal-nonmetal (CCI4,H20,CO2,CH4)

Molecular solid

Structure:molecules, weak intermolecular forces.

Melting: low, small energy overcome weak bonds.

Conductivity: molecules, not charged, no response to electric field.

Malleability: soft, easily deformed, small energy to overcome weak forces.

Soluability: polar dissolves polar

metal-metal

AI, Mg, Zn, Pb,Cu

Metallic solid

Structure: 3D lattice of nuclea in metallic bonds. Sea of elections. STRONG

Melting: moderate-high, metallic bonds between atoms, requires a large amount of heat energy.

Conductivity: Good delocalised electrons free to move.

Malleability: attraction non-directional able to rearrange without break

Solubility: Insoluble

non-metal - non-metal

Diamond,Silicon, Graphite

C,Si,SiO

Giant Covalent Network

Structure:lattice of atoms, strong covalent bonds

Melting: High, large amount heat energy to overcome bonds.

Conductivity: No charged particles free to move, Graphite can ( 1 fee delocalised e-)

Malleability: No, Strong bonds

Graphite(3 carion,2d,weak,layers slide)

Solubility: INSOLUABLE

metal - non-metal

NaCI, MgO,CuO

Ionic solid

Structure: Positive + Negative ions held by strong ionic bonds.

Melting: high, strong bonds bt ions : large amount heat to overcome.

Conductivity: >Solid, fixed, unable to move, non conducting

> Liquid,bonds overcome, ions free to move, conductors

Malleability: hard, like charges align + repel.

Solubility:Polar solvents