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

Bonding Flashcards

(45 cards)

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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

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A

The weak forces between layers

20
Q

Describe properties and structure of diamond

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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

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A

Giant structures

22
Q

Describe the properties of silicon (IV) oxide

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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?

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A

3 - metallic, ionic, covalent

24
Q

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

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A

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

25
When don't and do ionic compounds conduct electricity
They don't in solid state They do in liquid and molten state
26
Why do ionic compounds conduct electricity in molten or liquid state
Because the IONS are free to move
27
As you go down the group 1 what happens to reactivity and why?
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
Why do noble gases not readily react
They have complete outer shells There is no need to lose or gain electrons Therefore they are inert
29
How is a covalent bond formed
the two non-metals share a pair of electrons
30
Why are simple molecular structures solid, liquid or gas and a low melting or boiling point
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
Why does a substance with a large molecular mass have a high boiling point
It means there are more covalent bonds in the structure Therefore more energy required to break more bonds
32
Why do giant covalent structures have high m.p and b.p
Because it has a large amount of strong covalent bonds which take large amounts of thermal energy to break
33
Do covalent compounds conduct electricity
Not usually
34
Draw a 2d metal lattice
35
What is metallic bonding (refer to electrostatic attraction)
The electrostatic attraction between positively charged metal ions and a sea of delocalised electrons
36
Why are metals electrical conductors
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
Why are metals malleable
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
What is a metal alloy
A mixture of a metal and one or more other elements Usually another metal and carbon
39
Why are metal alloys harder than pure metals
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
Uses of aluminium
Aircraft - low density/ resists corrosion Power cables - conducts electricity/ ductile
41
Uses of copper
water Pipes - maleable/ below hydrogen in reactivity series so it doesn't react with water Electrical wiring - excellent conductor of electricity
42
Uses of iron
Power cables - good electrical conductor Window frames - reistant to corrosion Aeroplanes - high strength to weight ratio
43
Uses of low carbon
Car bodies - malleable
44
Uses of high-carbon steel
Used for construction - strength
45
Uses of stainless steel
Cutlery - doesnt rust

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

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