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GCSE - Chemistry > Chemistry Higher 3 GCSE > Flashcards

Chemistry Higher 3 GCSE Flashcards

(71 cards)

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1
Q

arrangement of particles in solid, liquid, gas

A

regular, random, random

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2
Q

relative distance between particles in solid, liquid, gas

A

very close, close, far apart

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3
Q

main movement of particles in solid, liquid, gas

A

vibrate in fixed positions, move around each other and move quickly in all directions

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4
Q

at what state can you not compress a substance

A

solid or liquid
Because there is no space for the particles to move into. A substance in its solid shape has a fixed shape and cannot flow, because the particles vibrate around in fixed positions and cant move from place to place.

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5
Q

what is an atom

A

a small piece of matter

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6
Q

how big is an atom

A

Helium atoms are the smallest and they are 62pm (62 *10-12 (to the power of -12))

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7
Q

what are electrostatic forces

A

forces of attraction between positive and negative charges.

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8
Q

limitations of the particle model

A

doesn’t show:
forces between the particles
the size of particles
the space between particles

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9
Q

relative mass of an electron

A

0.0005

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10
Q

isotopes

A

different number of neutrons

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11
Q

ion

A

different number of electrons

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12
Q

Atomic model

A

DaTe RnBo

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13
Q

relative atomic mass/ formula mass

A

the mean mass of an atom/ formula compared to 1/12 the mass of a 12 6 Carbon atom

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14
Q

pure

A

consists of only 1 element

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15
Q

what is an alloy

A

a mixture of a metal and one or more element

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16
Q

how do you know what a substance is impure

A

the m.p is often less than that of a pure substance

it melts over a range of temperatures

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17
Q

how can you find the m.p

A

heat slowly

stir the substance as you melt it

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18
Q

How does crystallisation work

A

You have to heat a solution, until it becomes a saturated solution. Then allow to cool, and crystallisation should form

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19
Q

stationary phases in PC

A

absorbent paper

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20
Q

mobile phases in PC

A

solvent like water or propane

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21
Q

stationary phases in TLC

A

thin layer of silica or alumina powder spread over the glass plate

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22
Q

Thin layer chromatography method

A
  1. put solvent in the chromatography tank to a depth of 1cm. (make sure there are no naked flames if it is flammable)
  2. add a small amount of the sample to the baseline
  3. let the solvent travel through the powder and take out the plate before it reaches the top
  4. analyse the pattern
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23
Q

gas chromatography stationary phase

A

silica or alumina powder in metal column

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24
Q

gas chromatography mobile phase

A

unreactive carrier as like nitrogen

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25
what is the solvent front
how far the water/ solvent has actually reached
26
explanation for gas chromatography
the sample is turned into a gas and injected into the column. The carrier gas pushes the sample through the column. The different components take different times to travel through the column, depending on how strongly they bond to the stationary phase.
27
advantages of TLC
quicker more sensitive- so less sample large range of stationary phases to choose from
28
what ions do metals form
they form positive ions as they lose electrons
29
what ions do non-metals form
they form negative ions as they gain electrons
30
do metals react with each other
no, but non-metals can react with each other
31
metal oxides produce what
alkaline solutions
32
non-metal oxides produce what
acidic solutions
33
structure and bonding in ionic compounds
ions are held together by ionic bonds, which act in all directions. ionic bonds are strong electrostatic forces between the oppositely charged ions
34
structure and bonding in covalent compounds
involve electrostatic forces, but the forces are between the nucleus of each bonded atom and the shared electrons. The covalent bonds are strong, but the IMF are weak
35
2 types of polymers
thermosoftening - tangled chains that are easy to seperate | thermosetting- chains joined with covalent bonds- called cross linking
36
metallic bonds
electrons leave their outer shells of the metal atoms, forming a 'sea of delocalised electrons' around the positively charged ions. They have strong electrostatic forces of attraction between the delocalised electron and the ions
37
Why can carbon form so many compounds
its atoms have 4 electrons, so it can form 4 covalent bonds
38
What can carbon form
CHAINS AND RINGS
39
What is an allotrope
different forms of the same element in different arrangements
40
Diamond
exists as a giant covalent structure, in which each carbon atom is joined to 4 others. Can't transfer electricity. High melting point and very hard
41
Graphite
Giant covalent structure where each carbon atom is joined to 3 others. Has 1 delocalised electron that can carry the charge
42
why is graphite slippery
even though the covalent bonds between in the graphite are strong. The forces between the layers is quite weak, so the layers can easily slide over each other
43
Graphene
A layer of graphite Transparent Strong Conducts electricity
44
Fullerenes
Large family of carbon allotropes. Nanotube: a sheet of graphene rolled into a tube. Buckyball: Graphene closed to make a hollow ball.
45
what elements are in the solid state at r.t
metals ionic compounds giant covalent
46
Brittle
Cracks under pressure
47
Malleable
be bent
48
how big are nanoparticles
1nm- 100 nm
49
nanoparticles uses
paints | cosmetics
50
what is a mole
a unit for amount of substance
51
What is Avogadro's constant
6.02 * 10 (-23) / mol | The number of entities in one mol
52
acid + carbonate
salt + water + carbon dioxide
53
acid + metal
salt + hydrogen
54
dilute acid
contains a low ratio of acid to volume of solution
55
concentrated acid
contains a higher ratio of acid to volume of solution
56
weak acids
they partially ionise
57
strong acids
they fully ionise
58
explanation behind weak and strong acids
acids release Hydrogen ions in aqueous solutions. As the concentration of H+ ions increases by a factor of 10, by pH decreases by 1.
59
electrolysis of water anode
4H+(aq) + 4e- -> 2H2 (g)
60
electrolysis of water cathode
4OH-(aq) -> 2H20(l) + O2(g) + 4e-
61
when is hydrogen produced
at the anode, unless there is an atom of a metal less reactive than hydrogen, then it will form
62
when is oxygen produced
at the cathode, unless there is a group 7 element there (bromine, chlorine, iodine?)
63
non-inert electrodes
will change
64
inert electrodes
will not change
65
in electroplating, what is the cathode
the object you want to coat
66
in electroplating, what is the anode
the metal you want to coat with
67
in electroplating, what is the electrolyte
has atoms of the metal you want to coat with
68
how does electroplating work
atoms lose electrons at the anode and then they gain electrons at the cathode, so they move and stay on the cathode.
69
how is copper purified
both electrodes are made from copper. The anode is the impure one and the cathode is the pure one. Copper(2) sulfate solution is usually used as the electrolyte. The cathode will gain copper atoms, and the anode will lose the electrons.
70
what type of particle is present in covalent bonding
a molecule
71
why might a covalent compound have a low melting point
because it still had weak intermolecular forces

GCSE - Chemistry (33 decks)

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