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Question 1

Metallic: Types of Elements

Answer 1

Metal elements

Question 2

Ionic: Types of Elements

Answer 2

Metals and Non Metals

Question 3

Covalent Molecular: Types of Elements

Answer 3

Non Metals

Question 4

Covalent Network: Types of Elements

Answer 4

Non Metals in Group 14 (Except oxygen)

Question 5

Metallic: Structure

Answer 5

Positive ions and delocalised electrons

Lattice of positive ions surrounded in by a sea of delocalised electrons

Question 6

Ionic: Structure

Answer 6

Positive and negative ions

Lattice of positive and negative ions

Question 7

Covalent Molecular: Structure

Answer 7

Neutral molecules

Molecules organised in a lattice; each molecule composed of atoms bonded together

Question 8

Covalent Network: Structure

Answer 8

Atoms

Atoms organised in a lattice

Question 9

Metallic: Bonding

Answer 9

Electrostatic attraction between delocalised electrons and positive metal ions, called metallic bonding

Strong

Non-Directional

Question 10

Ionic: Bonding

Answer 10

Electrostatic attraction between positive (cations) and negative ions (anions), called ionic bonding

Strong (electrostatic attraction of oppositely charged particles)

Non-Directional

Question 11

Covalent Molecular: Bonding

Answer 11

i. Within molecules, electrostatic attraction between shared electrons and nuclei called covalent bonding
ii. Weak bonds (intermolecular forces) between molecules.

Covalent bonds are strong (electrostatic attraction between shared electrons and nuclei) , intermolecular forces are weak (Weak Bonds)

Directional

Question 12

Covalent Network: Bonding

Answer 12

Electrostatic attraction between shared electrons and nuclei called covalent bonding

Strong (Covalent Bonds)

Question 13

Metallic: Properties

Answer 13

MP and BP: Most are high (Strong Electrostatic Attraction)

Electrical Conductivity: Good conductors in solid and liquid states (Electrons are free to move through the solid, Electron mobility explains it’s conductivity)

Hardness and Malleability: Most are hard, malleable, and ductile

Hard due to electrostatic attraction

Malleable and ductile due to sufficient force being able to cause a layer of atoms to slide over another and through the mobility of valence electrons

Question 14

Ionic: Properties

Answer 14

MP and BP: High (Electrostatic forces between ions)

Electrical Conductivity: Non-conductors in solid state, good conductors in liquid state and in aqueous solution (Ions are fixed in a solid, but can move freely and carry charges in aqueous state)

Hardness and Malleability: Hard and brittle

Hard due to strong electrostatic attraction

Brittle due to passing a layer of atoms over another causes ions of opposite charges to repulse (repulsion) each other (fracture)

Question 15

Covalent Molecular: Properties

Answer 15

MP and BP: Low (only a small amount of thermal energy required to overcome weak inter-molecular forces)

Electrical Conductivity: Non-conductors in solid and liquid states. Molecules are uncharged and electrons are held tightly within covalent bonds. No mobile charged particles. Only some covalent molecular substances that are aqueous can

Hardness and Malleability: Most are soft due to weak intermolecular forces

Very Malleable since only weak forces exist between molecules

Question 16

Covalent Network: Properties

Answer 16

MP and BP: Very High. Atoms held in a strong rigid structure by covalent bonds

Electrical Conductivity: Non-conductors in solid and liquid states (except graphite). Valence electrons are involved in bonding or ione pairs

Hardness and Malleability: Very hard and brittle

Strong covalent bonds through the lattice make it hard

Stressing the lattice makes it shatter (Brittle)