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Emmanuel College Chemistry > Paper 1- Unit 2 Bonding > Flashcards

Paper 1- Unit 2 Bonding Flashcards

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1
Q

A covalent bond is

A

shared pair of electrons

between two non-metals

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2
Q

An ionic bond is

A

strong

(electrostatic) attraction

between positive and negative ions

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3
Q

A metallic bond is

A

strong

(electrostatic) attraction

between positive metal ions (in a lattice)

and negative delocalised electrons

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4
Q

Why do simple covalent substances have low melting points

A

weak (intermolecular) forces of attraction

between molecules

easily overcome

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5
Q

Explain why simple covalent substances are poor conductors of electricity

A

electrons aren’t free moving

to carry an electrical charge

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6
Q

The larger the covalent molecule the higher the boiling point. Explain why.

A

Larger molecules have stronger attraction
Between the molecules
More energy needed
To separate

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7
Q

Describe the structure of diamond

A

Giant covalent
Carbon atoms
Covalently bonded
To 4 other carbons

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8
Q

Explain why diamond had a high melting and boiling point

A

4
strong covalent bonds
broken
lots of energy needed to overcome

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9
Q

Describe the structure of graphite

A

Carbon atoms
In layers
Weak forces of attraction (between)

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10
Q

Explain why graphite is soft and slippery

A

Layers
Slide over each other
(due to) weak forces between layers

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11
Q

Explain why graphite is an electrical conductor

A

Free (unbonded) electron can move

Carry electrical charge throughout the structure

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12
Q

Explain why ionic substance have high melting and boiling points

A

Strong (electrostatic) attraction
between positive and negative ions
Takes lots of energy
To separate ions

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13
Q

Explain why ionic substance are conductors when molten or dissolved but not liquid

A

Ions can’t move in solid
(when molten or dissolved) Ions able to move
Can carry an electrical charge

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14
Q

Describe the structure of a metal

A 
Free (delocalised) electrons
Positive metal ions
In a (giant) lattice
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15
Q

Explain why metals have high melting and boiling points

A 
Strong (electrostatic) attraction
(between) positive metal ions
Negative free (delocalised) electrons
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16
Q

Explain why metals conduct electricity

A 
Free (delocalised) electrons can move
Carry electrical charge
Throughout the (giant) metal lattice
17
Q

What is graphene?

A

a single layer of graphite

18
Q

Why does graphene conduct electricity?

A 
free electron (delocalised)
can travel through the single layer
and carry an electrical charge through it

Emmanuel College Chemistry (15 decks)

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