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combined trilogy chemistry GCSE AQA > bonding, structure and properties of matter > Flashcards

bonding, structure and properties of matter Flashcards

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1
Q

what is ionic bonding?

A

form between metals and non-metals. It involves the transfer of electrons in the outer shells.

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2
Q

what is covalent bonding?

A

When atoms share pairs of electrons, they form covalent bonds. These are STRONG bonds

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3
Q

Examples of covalently bonded substances with giant covalent structures:

A

diamond and silicon dioxide.

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4
Q

What are the three types of structure that can be formed by
covalent bonding?

A

Small molecules, very large molecules, giant covalent molecules.

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5
Q

What are the limitations of using dot and cross diagrams to
represent covalent bonds?

A

It shows the electrons differently, when they are the same and it does not show the bond angles or shape of the molecule.

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6
Q

The electrons in the outer shell of metal atoms are delocalised and are free to move throughout the structure.
The sharing of delocalised electrons lead to ….

A

strong metallic bonds.

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7
Q

How are atoms arranged in a metal?

A

Giant structures of atoms, arranged in a regular pattern,
delocalised electrons.

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8
Q

Why are metallic bonds so strong?

A

Sharing of delocalised electrons.

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9
Q

What are delocalised electrons?

A

They are free-moving electrons within structure; not associated with a particular atom.

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10
Q

Why are the particles that make up a metal described as positively charged?

A

The metal atoms lose outer shell electrons and therefore there are more protons (+) than electrons (−).

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11
Q

solids (s) =

A

Close together, regular pattern, vibrate on the spot.

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12
Q

liquids (l) =

A

Close together, random arrangement, move around each other.

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13
Q

gases (g) =

A

Far apart, random arrangement, move quickly.

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14
Q

aqueous solution (aq) =

A

water that contains one or more dissolved substance.

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15
Q

solid → liquid =

A

melting

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16
Q

liquid → gas =

A

evaporation

17
Q

gas → liquid =

A

condensation

18
Q

liquid → solid =

A

freezing

19
Q

gas → solid =

A

deposition

20
Q

solid → gas =

A

sublimation

21
Q

Melting and freezing take place at ….

A

the melting point

22
Q

Boiling and condensing take place at ….

A

the boiling point

23
Q

The stronger the forces between the particles the ….

A

higher the melting and boiling point of the substance.

24
Q

What factor affects the amount of energy needed to change
state?

A

Forces between molecules.

25
Q

Describe the structure of ionic compound

A

Regular, giant ionic lattice

26
Q

Why do ionic compounds have high melting and boiling points?

A

Strong electrostatic forces of attraction between ions.

27
Q

Why can ionic compounds conduct electricity when melted or dissolved in water?

A

Ions are free to move, carry the charge.

28
Q

Why do small molecules have low melting and boiling points?

A

Weak forces between molecules/ intermolecular forces.

29
Q

What happens to the melting and boiling points as small
molecules get bigger? Why?

A

Increases, intermolecular forces get bigger.

30
Q

What are polymers?

A

Very large molecules made of repeating units.

31
Q

Why are polymers normally solid at room temperature?

A

Intermolecular forces relatively strong.

32
Q

What is an alloy?

A

Mixture of two elements, one of which is a metal.

33
Q

Why are metals good conductors of electricity?

A

Electrical charge carried by delocalised electrons.

34
Q

In a diamond, how many covalent bonds does each carbon make?

A

4

35
Q

Diamond does not conduct electricity. Why?

A

No delocalised electrons.

36
Q

In graphite, how many covalent bonds does each carbon make?

A

3

37
Q

Why is graphite soft?

A

Layers can slide over each other, weak forces between layers, no covalent bonds between layers.

38
Q

How is graphite similar to metals?

A

It contains delocalised electrons.

combined trilogy chemistry GCSE AQA (6 decks)

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