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Chemistry > Bonding (Ionic, Simple Covalent, Giant Covalent, Metallic) > Flashcards

Bonding (Ionic, Simple Covalent, Giant Covalent, Metallic) Flashcards

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1
Q

Describe how ions are formed through electron loss or gain

A

Ionic bonding occurs between metals and non-metals

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2
Q

Explain metal ions

A

Metal atoms lose electrons = positive ions

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3
Q

Explain non-metal ions

A

Non- metal atoms gain electrons = negatove ions

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4
Q

Finish the sentence: The oppositely charged ions strongly….

A

Attract each other (ELECTROSTATIC ATTRACTION) in an ionic compound, this is ionic bonding

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5
Q

State the charges of these metal ions:

Ag

A

Silver +

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6
Q

Cu

A

Copper 2+

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7
Q

Fe

A

Iron (ii) 2+

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8
Q

Fe

A

Iron (ii) 3+

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9
Q

Pb

A

Lead 2+

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10
Q

Zn

A

Zinc 2+

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11
Q

And these non-metal ions:

H

A

Hydrogen +

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12
Q

OH

A

Hydroxide -

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13
Q

NH4

A

Ammonium +

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14
Q

CO3

A

Carbonate 2-

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15
Q

NO3

A

Nitrate -

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16
Q

SO4

A

Sulfate 2-

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17
Q

What is the is the formula for the ionic compound Magnesium+2 Chloride-1

A

MgCl2

18
Q

Iron 2+ sulphate 2- (SO4)

A

FeSO4

19
Q

Aluminium 3+ oxide 2-

A

Al2O3

20
Q

What is an ionic bond?

A

An ionic bond is the strong electrostatic attraction between oppositely charged ions

21
Q

Why do giant ionic lattices have a high melting and boiling point?

A

The strong electrostatic attraction between the oppositely charged ions takes a lot of energy to overcome

22
Q

State and explain why ionic compounds only conduct electricity when dissolved or molten?

A 
As solids ions are bonded together in lattice so cannot carry charge,
When molten (liquid) ions can break free of the lattice and are able to move, these ions are charged particles and so can carry an electric current.
When dissolved ions are free to move and can carry an electric current
23
Q 
Simple Covalent (molecular) Bonding:
Describe covalent bonds
A

A covalent bond is formed between atoms sharing a pair of electrons

24
Q

What is a covalent bond?

A

An electrostatic attractions between pairs of shared electrons and and the nuclei of the atoms

25
Q

Explain why simple covalent structures have a low melting and boiling point

A

There is a weak intermolecular attraction between the molecules which don’t take much energy to overcome

26
Q

Why do simple covalent structures not conduct electricity?

A

There is nothing to carry a charge ie. no delocalised electrons etc.

27
Q

Giant Covalent Bonding:

Describe the structure of diamond

A 
Made of carbon in a giant covalent lattice structure, each carbon is covalently bonded to four others 
High mpt + bpt
Very strong
A giant covalent lattice
DOES NOT conduct electricity
28
Q

Describe the structure of Graphite

A

A carbon allotrope, each carbon is covalently bonded to three others, each carbon atom has a delocalised electron free to carry charge - can conduct electricity. Weak attraction between layers so layers can easily slide off.
High mpt + bpt
Each individual layer is very strong
Graphite is the only non-metal that conducts electricity

29
Q

Describe the structure of Buckminster fullerene

A

Fullerenes are an allotrope of carbon
It contains 60 Carbon atoms
Each is bonded to three other atoms by two single and one double bond
Lower mpt + bpt than giant structures due to the weak intermolecular attraction
Used as delivery for drugs and used as lubricants

30
Q

Metallic Bonding:

Describe a metallic lattice

A

A giant structure of tightly packed layers which form a regular lattice structure

31
Q

What are the properties of metals?

A 
Sonorous
Malleable
Strong
Conduct Heat
Conduct Electricity
High mpt + bpt
32
Q

Why are metals malleable?

A

The ions are arranged in layers which can slide over each other, this makes it malleable

33
Q

Why can metals conduct electricity and heat?

A

In each atom the outer electrons are delocalised, the metal ions are attracted to the delocalised electrons - strong electrostatic attraction

34
Q

What is reduction?

A

A gain of electrons

35
Q

What is oxidation?

A

A loss of electrons

36
Q

What does the acronym OIL RIG stand for?

A

Oxidation Is Less Reduction Is Gain

37
Q

Has Mg2+ oxidised or reduced?

A

Oxidised - lost electrons

38
Q

Has Cl- oxidised or reduced?

A

Reduced - Gained electrons

39
Q

What is the electronic configuration of
19
F
9

A

2,7

40
Q

What are allotropes?

A

Different forms of the same element e.g.. diamond and graphite = carbon

Chemistry (3 decks)

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