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Chemistry > Year 9 Term 2 > Flashcards

Year 9 Term 2 Flashcards

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1
Q

Metal atoms lose electrons during reactions and will always…

A

Form positive ions

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2
Q

Non-metal atoms gain electrons and always…

A

Form negative ions

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3
Q

Group one elements form

A

1+ ions

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4
Q

Group 2 elements form

A

2+ ions

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5
Q

Group 6 elements form

A

2- ions

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6
Q

Group 7 elements form

A

1- ions

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7
Q

Do compounds have a charge

A

No because charges must cancel out when working out the overall formula

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8
Q

What do ionic compounds contain

A

Metals and non-metals

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9
Q

What does dissolve mean

A

When some solids are out into a liquid like water, they appear to get smaller, some solids seem to disappear. This is called dissolving

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10
Q

Decanting

A

Insoluble solid from liquid

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11
Q

Filtration

A

Insoluble solid from liquid

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12
Q

Evaporation

A

Solute from a solution

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13
Q

Distillation

A

Solvent from a solution

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14
Q

Fractional distillation

A

Mixture is miscible liquids

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15
Q

Separating funnel

A

Mixture of miscible liquids

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16
Q

Chromatography

A

Mixture of miscible liquids

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17
Q

Soluble solute + solvent —>

A

Solution

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18
Q

Insoluble solute + solvent —>

A

Solute + solvent

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19
Q

What is chromatography

A

Separating the different inks in a pen. Each colour travels different distances. All inks in pen are water soluble and travel up chromatography paper. The greater the distance travelled, the more soluble it is

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20
Q

Why do elements react

A

Because they want a full outer shell

21
Q

How do elements react

A

By gaining or losing an electron(s) from/to the outer shell

22
Q

Why are Nobel gases unreactive

A

Because they have a full outer shell so don’t need to gain/lose and electron

23
Q

Ionic bonding

A

Metals and non-metals
Outer electrons become delocalised
Produces positive ions and delocalised electrons

24
Q

Giant covalent bonds

A

Non-metals
Share electrons
Particles = atoms

25
Q

Covalent simple molecular bonding

A

Non-metals
Share electrons
Particles= molecules

26
Q

How are ions held together

A

They are held together by strong forces of attraction between oppositely charged ions. The electrostatic force of attraction is called the ionic bond

27
Q

Why are ions in a giant structure held together so strongly

A

The force exerted by an ion on the other ions acts equally in all directions

28
Q

Why are metals always positively charged

A

Because they lose an electron

29
Q

Why are non-metals always negatively charged

A

Because they gain an electron

30
Q

Does solid sodium chloride conduct electricity?

A

No because it needs to be able to move freely (liquid) and solid can’t.

31
Q

Does sodium chloride dissolved in distilled water conduct electricity

A

Yes because it can move freely and contains ions. Because they can move and carry a charge

32
Q

Can distilled water conduct electricity

A

No because it doesn’t contain ions so doesn’t conduct

33
Q

Does molten sodium chloride conduct electricity

A

Yes because it can move freely and contains ions so can carry a charge

34
Q

To conduct electricity particles need to…

A

Be able to move freely and particles need to have a charge

35
Q

Ionic compounds conduct electricity when molten or dissolved in water because…

A

They can move freely because it’s a liquid and can conduct electricity because it’s an ionic compound. Charged particles can carry a charge

36
Q

Ionic compounds do not conduct when solid because

A

They are solid so vibrate about a fixed point so the ions cannot move to terminals

37
Q

Ionic compounds have high melting and boiling points because

A

There is a strong force of attraction between ionic bonds so a lot of energy is needed to break attraction

38
Q

What is a covalent bond

A

A shared pair of electrons

39
Q

How to draw a covalent bond

A

Only draw the outer shell

Cl-Cl the line represent the covalent bond between the atoms

40
Q

Can covalent compounds conduct electricity

A

No because they don’t have an overall charge

41
Q

Do simple molecular substances conduct electricity

A

No because they aren’t electrically charged, they are neutral

42
Q

Why do simple molecular substances have a low melting and boiling point

A

Because there are weak forces between the molecules

43
Q

Why do covalent substances not conduct electricity

A

Because the molecules don’t have an overall charge - don’t contain free ions or electrons

44
Q

Why do diamond and graphite have a high melting and boiling point

A

Because there are many strong covalent bonds to break

45
Q

Why is diamond hard and why is graphite soft

A

Diamond is hard because the atoms are held together by many strong covalent bonds
Graphite is soft because the layers of atoms can slide

46
Q

Why can’t diamond conduct electricity and why can graphite conduct electricity

A

Diamond can’t because there are no free electrons/ ions

Graphite can because it has an outer delocalised electron

47
Q

What does delocalised mean

A

Free to move if there is a delocalised electron, it can conduct electricity

48
Q

Buckminster fullerene

A

Arranged in pentagons, hexagons and spheres

Chemistry (13 decks)

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