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IGCSE Chemistry > Atomic structure, types of bondings > Flashcards

Atomic structure, types of bondings Flashcards

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1
Q

The reason why the boiling point of nitrogen is very low even though the bond between the atoms in a nitrogen molecule is very strong is [2]

A

Weak intermolecular and low amount of energy required to break bonds between molecules; [1 mark]
covalent bonds don’t break [1 mark]

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2
Q

The difference in electrical conductivity between solid and liquid strontium chloride is

A

Ions cannot move in solid
OR
Ions can move in liquid; [1 mark]

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3
Q

The difference in electrical conductivity between liquid strontium chloride and liquid sulfur chloride is

A

No ions in sulfur chloride
OR
Sulfur chloride is covalent
OR
Sulfur chloride only contains molecules
OR
Only strontium chloride has ions; [1 mark]

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4
Q

Diamond is an example of

A

Giant covalent structure

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5
Q

Give an example of an ionic compound

A

Sodium chloride

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6
Q

Explain how simple covalent molecules have low melting and boiling points even though covalent bonds are strong [3]

A

1) Intermolecular forces that hold covalent molecules together
2) Intermolecular force is weak
3) Requires low energy to break

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7
Q

What is an ionic bonding?

A

Metal atom will transfer electrons to non metal so both can form a full outershell for stability

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8
Q

Why do diamond and graphite have high melting point [3]

A

1) It has billions of covalent bonds, it is 1 molecule for the entire structure.
2) Every carbon is bonded 4 times
3) No intermolecular forces

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9
Q

Why is graphite slippery

A

Weak forces of attraction between layers so it can slide over each other

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10
Q

What is the formation of positive ions called

A

Cation

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11
Q

Formation of negative ions

A

Anion

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12
Q

Define ionic bond

A

Strong electrostatic attraction between oppositely charged ions

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13
Q

5 properties of ionic compound

A

1) High melting & boiling point
2) good electrical conductivity when aqueous or
molten and poor when solid
3) Hard; [1 mark]
4) Soluble in water / insoluble in organic solvents; [1 mark]
5) Brittle

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14
Q

Draw the giant lattice of ionic compound

A

regular arrangement of
alternating positive and negative ions

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15
Q

Ionic bonds are formed between

A

Metals & non-metals

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15
Q

Explain why ionic structures have high melting points and boiling points [2]

A

Lots of strong electrostatic forces,
requires lots of energy to break

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15
Q

Explain why ionic structures have good electrical conductivity when aqueous or
molten but poor when solid [2]

A

1) Ions can flow around freely in an aqueous state which conducts electricity
2) Charges are immobile in solid state

16
Q

Covalent bonding

A

When non-metals & non metals react and overlap pairs of electrons to get a full outershell

17
Q

3 properties of covalent bonded compounds

A

1) Low melting & boiling point
2) Poor electrical conductivity
3) Covalent compounds are not soluble in water

18
Q

Explain why covalent structures have poor electrical conductivity points [2]

A

1) There are no charged molecules flowing around
2) There are no free electrons

19
Q

Negative ion

A

Anion

20
Q

Positive ion

A

Cation

21
Q

metallc bonding

A

the electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocalised electron

22
Q

3 properties of metallic bonding

A

1) good electrical conductivity
2) malleable and ductile
3) High melting and boiling points

23
Q

Why are metallic bonding strong

A

Strong attraction between the positive metal ions and sea of delocalised electrons

24
Q

Explain why metallic bonding have good electrical conductivity

A

delocalised electrons carry charge and move around structure freely

25
Q

Explain why metallic bonding are malleable and ductile

A

Pure metals are arranged in layers and are the same size
2) Layers slide past each other when a force is extered

26
Q

Describe diamond structure [3]

A

1) 1 carbon is bonded 4 more times
2) All covalent bonds are strong and identical
3) No intermolecular forces

27
Q

Describe graphite structure

A

1) 1 carbon is bonded 3 more times that form layers of hexagons leaving 1 delocalised electron per carbon atom

2) Covalent bonds between layers are strong

3) Layers are attracted to each other by weak intermolecular forces

28
Q

Why is graphite used as a lubricant

A

Layers can slide past each other

29
Q

Why is graphite used as a electrode [3]

A

1) good conductor of electricity
2) chemically stable
3) Have high melting & boiling point

30
Q

Why is diamond used as a cutting tool

A

Diamond have lots of strong covalent bonds making it a hard material that can cut through other materials

31
Q

Describe the giant covalent structure of silicon(IV) oxide, SiO2 [2]

A

1) Each Silicon atom forms covalent bonds with 4 Oxygen atoms and each Oxygen atom in turn forms covalent bonds with 2 Silicon atoms

2) tetrahedral arrangement

32
Q

Describe the similarity in properties between diamond and silicon(IV) oxide, related to their structures [4]

A

1) both have tetrahedral arrangement
2) SiO2 has lots of very strong covalent bonds and no intermolecular forces like diamond
3) both have high boiling & melting points
4) Both are hard
5) Silicion oxide can form acidic oxide

33
Q

Define lattice

A

A repeating pattern of particles

34
Q

Define electrostatic forces

A

he attractive or repulsive force between two electrically charged objects.

35
Q

Ammonium

A

NH4

36
Q

Hydroxide

A

OH

37
Q

Nitrate

A

NO3

38
Q

Sulfate

A

SO4

39
Q

Carbonate

A

CO3

40
Q

Hydrgoen carbonate

A

HCO3

IGCSE Chemistry (10 decks)

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