Bonding Flashcards

1
Q

Definition of ionic bonding

A

Electrostatic forces of attraction between positive and negative electrons.

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2
Q

Properties of of ionic bonding

A

High boiling and melting points.

Can conduct electricity when molten or dissolved beacause ions are free to move.

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3
Q

Definition of covalent bonding

A

Bond between two non-metals formed by a shared pair of electrons between two atoms with a strong force of attraction.

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4
Q

Simple molecules

A

Low melting and boiling points.
Weak covalent bonds.
Can’t conduct electricity because there are no electrons or ions to move.

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5
Q

Giant molecules

A

Lattice structures.
High melting and boiling points.
Strong covalent bonds so difficult to overcome with lots of heat needed.
Can’t conduct electricity except graphite.

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6
Q

Diamond

A

Hard
Each atom is joined to 4 other ones
Does not conduct electricity

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7
Q

Graphite

A

Soft and slippery
Layers are weak and can be easily separated
Need to be broken down

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8
Q

C60 Fullerene

A

Soft
Low melting and boiling points.
Can conduct electricity.
Each carbon atom joined to 3 other carbon atoms and the 4th is delocalised and free to move.
Small amounts of heat to overcome them so weak covalent bonds.

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