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AQA GCSE - Chemistry > 2.1 - Structure And Bonding > Flashcards

2.1 - Structure And Bonding Flashcards

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1
Q

What is a compound?

A

Two or more elements chemically combined

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2
Q

What is a chemical bond?

A

An attraction between particles

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3
Q

What do substances that have that consist of simple molecules?

A

Low melting and boiling points

Weak intermolecular forces

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4
Q

What is ionic bonding?

A

When a non-metal and a metal combine by transfer of electrons

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5
Q

What happens when the metal element loses electron(s) in ionic bonding?

A

It produces a full outer shell and becomes a positive ion - this is because it has lost electron(s) meaning it has more protons which are positive

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6
Q

What happens when the non-metal gains electron(s) in ionic bonding?

A

It produces a full outer shell and becomes a negative ion - this is because it has gained electron(s) meaning it will have more electrons which are negative

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7
Q

Why do the ions bond in ionic bonding?

A

Negatively charged ions are attracted to positively charged ions as oppositely charged ions attract

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8
Q

What is the attraction between the ions in ionic bonding?

A

They have a strong electrostatic attraction between positive and negative ions

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9
Q

What is the melting point of an ionic bond?

A

High melting point

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10
Q

Can ionic bonds conduct electricity?

A

They conduct when dissolved in water or molten as the bond between the ions are broken and are free to move

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11
Q

What is covalent bonding?

A

When a non-metal and another non-metal combine by sharing electrons

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12
Q

What are substances made from covalent bonds called?

A

Molecules

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13
Q

What are the force like in simple covalent bonding?

A

They have weak intermolecular forces but strong bonds between atoms where electrons are shared

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14
Q

What is the melting and boiling points in simple covalent bonding?

A

Low melting and boiling points

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15
Q

Do simple covalent bonds conduct electricity?

A

They can’t conduct as they have no charge

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16
Q

Which 3 Giant covalent structures do you need to know about?

A

Diamond, Silicon Dioxide and Graphite

17
Q

What is the structure of a normal giant covalent bond?

A

Repeating 3D structure
Each carbon has 4 bonds (diamond)
Strong bonds between atoms
Hard materials

18
Q

What is the melting and boiling points in giant covalent bonding?

A

High Melting and Boiling Points

19
Q

Do normal giant covalent structures conduct electricity?

A

They don’t conduct electricity as they have no free atoms therefore no delocalised electrons. It is also insoluble in water

20
Q

What is the structure of Graphite?

A

Hexagonal rings of carbon 1 atom thick in layers

Each carbon has three bonds

21
Q

Can Graphite conduct electricity?

A

Yes as each carbon only has three bonds meaning it has one free electron per carbon atom not involved in bonding. This electron is delocalised and free to move allowing graphite to conduct electricity

22
Q

What are the forces between the layers in Graphite?

A

It has weak intermolecular forces so the layers can slide over each other - component in lubricants

23
Q

What are fullerenes?

A

A form of carbon (allotropes) made up of balls cages or tubes

24
Q

What can fullerenes be used for?

A

Drug delivery
Lubricants
Catalysts
In nanotubes e.g tennis racket

25
Q

Properties of a fullerene?

A

Strong but light

Large surface area

26
Q

What is metallic bonding?

A

When a metal and another metal element are combined

27
Q

How are metals bonded?

A

The outer electrons in the metal lattice become delocalised leaving a lattice of positively charged electrons
The electrostatic attraction between the positively charged metal ions and the negatively charged sea of delocalised electrons creates a strong metal bond

28
Q

What is the melting and boiling points in metallic bonding?

A

Hight melting and boiling points

29
Q

Can metallic structures conduct electricity?

A

Yes as delocalised electrons carry the electrical charge

30
Q

Properties of metals?

A

Malleable and ductile as layers cans slide over each other

Shiny and sonorous (ding!)

31
Q

What are alloys?

A

Made from two or more metals with different sizes distorting the atom layers

32
Q

What properties of alloys make them better than metals?

A

They can’t slide over each other making them much harder

33
Q

What is a shape memory alloy?

A

They can return to their original shape when heated after being deformed

34
Q

Give an example of a shape memory alloy?

A

Nitinol

Made from Nickel and Titanium

AQA GCSE - Chemistry (19 decks)

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