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Science Revision > Yr10 chemistry atoms, ions bonds n stuff > Flashcards

Yr10 chemistry atoms, ions bonds n stuff Flashcards

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1
Q

Ions are _____ particles

A

charged

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2
Q

In an ionic compound, the metal is the ______ ion

A

positive

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3
Q

In an ionic compound, the non-metal is the ______ ion

A

negative

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4
Q

Are ionic compounds soluble in water?

A

yes

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5
Q

Are ionic compounds conductive in water?

A

yes

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6
Q

Are ionic compounds conductive as a solid?

A

yes

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7
Q

Why are ionic compounds (not?) soluble in water?

A

Water has a slight charge which is attracted to the ions

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8
Q

Why are ionic compounds (not?) conductive as a solid?

A

Ions can’t move, and to conduct electricity, the substance needs to be charged (which ions are) and be able to move (which solids can’t)

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9
Q

Why are ionic compounds (not?) conductive as water?

A

To conduct electricty substances need to be charged and able to move. Ions in water are charged, and because they have dissolved they can move.

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10
Q

What are the properties of ionic compounds? (and why?)

A

Hard, but brittle. this is because of the strong forces of attraction. They are brittle because they are made of layers which can snap apart.

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11
Q

do ionic compounds have high/low melting/boiling points? why?

A

High melting points
This is because ionic solids contain strong forces of electrostatic attraction and a lot of energy is needed to break these bonds

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12
Q

How are ionic solids arranged?

A

In a lattice

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13
Q

Why does magnesium oxide have a higher melting point that sodium chloride?

A

Because the bonds are stronger. Oxygen ions are -2 ions, magnesium ions are +2 compared to sodium and chloride’s +1 / -1

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14
Q

What do most ionic compounds look like?

A

White powder (exception copper sulfate)

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15
Q

Why does ionic bonding happen?

A

All atoms “want” a full outer shell of electrons like a noble gas. Metals need to lose electrons while non-metals need to gain them. Metals will “give” non-metals their electrons, so in the end all the atoms- now ions- are balanced. They are ions because they now have an uneven number of protons and electrons

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16
Q

What is another word for a negative ion?

A

anion

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17
Q

What is another word for a positive ion?

A

cation

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18
Q

Describe the arrangement of ions in an ionic lattice

A

It is an assembly of positive and negative ions held together by forces of electrostatic attraction, arranged in a regular array. Ionic bonds are non-directional, with every ion attracted to all its neighbours.

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19
Q

What does isoelectronic mean?

A

ions with the same electronic configuration

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20
Q

What is the word for atoms with the same electronic configuration?

A

isoelectronic

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21
Q

What is group one called?

A

The alkali metals

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22
Q

Group seven are the…

A

halogens

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23
Q

Which word should you never use when describing bonds?

A

weak

24
Q

Which word should you never use when describing forces?

A

strong

25
Q

Why is an alloy not a compound?

A

The different elements in the alloy are not chemically bonded, but are “set” into the metal

26
Q

What is one layer of graphite called?

A

Graphine

27
Q

What is diamond’s melting point like and why?

A

Very high. this is because each carbon atom has four strong covalent bonds, each of which need a lot of energy to overcome

28
Q

What is diamond’s conductivity like and why?

A

It cannot conduct electricity as nothing in diamond’s structure can move.

29
Q

Give a description of diamond’s structure

A

Each carbon has four strong bonds. It is a regular repeating structure

30
Q

What is diamond’s hardness like and why?

A

Very hard- the hardest substance on earth. This is because of its structure (CHECK)

31
Q

What are diamond’s industrial uses like and why?

A

Drill heads (very hard) and jewelry (you can cut along a line of atoms in diamond, and can make very sharp, precise cuts (CHECK))

32
Q

What is graphite’s melting point like and why?

A

Very high, not as high as diamond, but each carbon still have three strong covalent bonds that need lots of energy to overcome.

33
Q

What is graphite’s conductivity like and why?

A

Very conductive, because delocalised electrons can move.

34
Q

What is graphite’s hardness like and why?

A

Very soft. Layers slide and break of easily because of weak intermolecular forces between layers

35
Q

What are graphite’s industrial uses and why?

A

Pencil led- due to softness and layers breaking easily
Lubricant- better than liquid, graphite lubricant won’t melt or run out the machine

36
Q

What is another example of a giant covalent structure like diamond?

A

silicon, silicon dioxide

37
Q

What is the formula for sulphuric acid?

A

H2SO4

38
Q

What is the formula for sulphate?

A

SO₄²⁻

39
Q

What is the formula for carbonate?

A

CO₃²⁻

40
Q

What is the formula for hydrogencarbonate?

A

HCO₃⁻

41
Q

What is the charge of sulfide?

A

-2

42
Q

Remember to use the correct formulas for things like magnesium! (mg not m)

A

qwertyuiopasdfghjklzxcvbnm

43
Q

What is a nanometre?

A

a millionth of a millimetre
OR 1 x 10^-9 metres

44
Q

what does nanoscience refer to?

A

it refers to structures that are 1 - 100 nm in size

45
Q

why do nanoparticles have different properties to their larger versions?

A

they have a larger SA : V ratio

46
Q

Give some examples of uses for nanotechnology

A

medicine, electronics, energy production

47
Q

Give some disadvantages of nanotechnology

A

concerns about toxicity, environmental concerns with microplastics in the food chain,

48
Q

What are polymers

A

Polymers are plastics- long chainlike molecules linked together by strong covalent bonds. All polymers are solids at room temperature

49
Q

What are polymers made of, and how do they effect the plastic produced?

A

Monomers undergo polymerisation to make a polymer. If you modify the monomer, you modify the polymer.

50
Q

What are the three allotropes of carbon?

A

diamond, graphite and fullerenes

51
Q

Give two examples of fullerenes

A

Buckminster fullerene and carbon nanotubes

52
Q

What are the properties of carbon nanotubes?

A

They are graphene rolled into a cylinder.
they are good conductors of heat and electricity
very strong
used as catalysts
large SA

53
Q

What are the properties of buckminster fullerenes/ buckyballs?

A

Made up of 60 carbon atoms, each of which forms a double bond and two singles
Simple molecular
Much lower melting points than diamond or graphite

54
Q

What are fullerenes?

A

Hollow 3D shapes made of carbon

55
Q

What are some applications of buckminster fullerene?

A

Delivering harmful drugs in a “cage” straight to cancer cells
Sieves for large particles like viruses
Lubricant- non stick coating for machinery, like ball bearings
Chemical sponges for toxic substances

Science Revision (59 decks)

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