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Eddie's iGCSE Chemistry - rates of reaction > Bonding > Flashcards

Bonding Flashcards

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1
Q

What are the properties of covalent bonds

A

Low melting and boiling point due to weak intermolecular forces These intermolecular forces are increased with molecular size e.g. there are bigger forces between C2H6 than CH4

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2
Q

Why do covalent bonds have a shared pair of electrons

A

To gain a noble gas configuration

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3
Q

What is an ionic bond

A

The type of bonding that occurs between a metal and a non-metal An electrostatic attraction between type oppositely charged ions

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4
Q

What does the electrostatic attraction cause

A

The formation of +ve and -ve ions with stable noble gas configurations

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5
Q

Properties of ionic bonding

A

Ionic lattices - ionic solids are often crystalline The ions are arranged in a giant 3D lattice pf alternating +ve and -ve ions Strong electrostatic attraction between the anions and cations, this causes high melting and boiling points

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6
Q

What is metallic bonding

A

The bonding found between two metals

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7
Q

What is a metallic bond

A

Electrostatic attraction between metals ions and a sea of delocalised electrons

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8
Q

Why are metallic bonds good conductors

A

The electrons are free to move

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9
Q

Why do metallically bonded compounds have high melting and boiling points

A

Because the electrostatic attraction between positive metal ions and delocalised electrons is strong

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10
Q

How does electrostatic attraction change is the metal becomes more malleable

A

The electrostatic attraction weakens

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11
Q

What is the difference between ionic and covalent bonds?

A

Ionic bonds are crystalline solids whereas covalent bonds are liquids or gases Ionic has high b.p./m.p. and covalent has low b.p./m.p. Ionic bonds are soluble in water and covalent bonds aren’t Ionic bonds aren’t soluble in organic solvent but covalent bonds are Ionic bonds conduct electricity in molten or solution state whereas covalent bonds do not

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12
Q

Why can ionic bonds conduct electricity in molten or solution state

A

Because the ions are free to move and carry charge

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13
Q

Why can’t covalent bonds conduct electricity

A

There are no charged particles to carry charge

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14
Q

Define allotropy

A

The substance has more than one form that can occur in a physical state

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15
Q

Examples of carbon allotropes

A

Diamond, graphite, graphene, buckminsterfullerene (C60)

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16
Q

Describe the properties of graphite

A

Electrically conductive Black, opaque, shiny density 2.25g/cm3

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17
Q

Describe the properties of diamond

A

Electrical insulator Transparent, shiny, sparkles Hardest known substance 3.52g/cm3

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18
Q

Describe bonding of graphite

A

Layered structure Hexagonal patterns within layers Strong bonds within layer Weak forces between layers Spare electron per carbon atoms leads to electrical conductivity between layers

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19
Q

Why is graphite a good lubricant

A

The weak forces between layers

20
Q

Describe properties and structure of diamond

A

Tetrahedral arrangement Each C atom bonds with four others Strong bonds with no spare electron making it a good insulator Shape of diamond makes it very hard

21
Q

What structures do graphite and diamond have

A

Giant structures

22
Q

Describe the properties of silicon (IV) oxide

A

High mpt and bpt Isn’t electrically conductive Hard but not as hard as diamond which is 8 times harder

23
Q

How many types of bonding are there?

A

3 - metallic, ionic, covalent

24
Q

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

A

Strong electrostatic forces of attraction between oppositely-charged ions require a lot of energy to break

25
Q

When don’t and do ionic compounds conduct electricity

A

They don’t in solid state They do in liquid and molten state

26
Q

Why do ionic compounds conduct electricity in molten or liquid state

A

Because the IONS are free to move

27
Q

As you go down the group 1 what happens to reactivity and why?

A

Reactivity increases with a larger electron configuration The outer electrons are further away from the nucleus The attraction between the nucleus and valence electron gets weaker This allows it to react more readily

28
Q

Why do noble gases not readily react

A

They have complete outer shells There is no need to lose or gain electrons Therefore they are inert

29
Q

How is a covalent bond formed

A

the two non-metals share a pair of electrons

30
Q

Why are simple molecular structures solid, liquid or gas and a low melting or boiling point

A

They have strong covalent bonds but weak intermolecular forces When a covalent substance melts or boils its the weaker intermolecular forces that break Less energy is required to break these molecules apart, so they have a lower m.p or b.p

31
Q

Why does a substance with a large molecular mass have a high boiling point

A

It means there are more covalent bonds in the structure Therefore more energy required to break more bonds

32
Q

Why do giant covalent structures have high m.p and b.p

A

Because it has a large amount of strong covalent bonds which take large amounts of thermal energy to break

33
Q

Do covalent compounds conduct electricity

A

Not usually

34
Q

Draw a 2d metal lattice

A
35
Q

What is metallic bonding (refer to electrostatic attraction)

A

The electrostatic attraction between positively charged metal ions and a sea of delocalised electrons

36
Q

Why are metals electrical conductors

A

There are free electrons able to move and carry charge

Electrons entering the other end of the metal cause a delocalised electron to displace

Hence electrons can flow so electricity is conducted

37
Q

Why are metals malleable

A

There are layers of +ve ions that can slide over one another when a force is applied.

The metallic bonding allows the metal to change shape without shattering

38
Q

What is a metal alloy

A

A mixture of a metal and one or more other elements

Usually another metal and carbon

39
Q

Why are metal alloys harder than pure metals

A

The alloy is made up of atoms of different size

This means that the layers of atoms cannot slide over each other easily

This makes the metal harder

40
Q

Uses of aluminium

A

Aircraft - low density/ resists corrosion

Power cables - conducts electricity/ ductile

41
Q

Uses of copper

A

water Pipes - maleable/ below hydrogen in reactivity series so it doesn’t react with water

Electrical wiring - excellent conductor of electricity

42
Q

Uses of iron

A

Power cables - good electrical conductor

Window frames - reistant to corrosion

Aeroplanes - high strength to weight ratio

43
Q

Uses of low carbon

A

Car bodies - malleable

44
Q

Uses of high-carbon steel

A

Used for construction - strength

45
Q

Uses of stainless steel

A

Cutlery - doesnt rust

Eddie's iGCSE Chemistry - rates of reaction (16 decks)

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