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Year 8 Exams > Chemistry > Flashcards

Chemistry Flashcards

(60 cards)

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1
Q

What are the 3 states of matter?

A

Solid, liquid and gas

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2
Q

How do you convert the states of matter?

A

Solid to liquid(melting)
Liquid to solid(freezing)
Liquid to gas(evaporating)
Gas to liquid(condensing)
Melting and evaporarion are spead up with heat.
Freezing and condensing happens when heat is removed from the state.

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3
Q

Gas properties

A

The particles are constantly movung at random and are far apart

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4
Q

Solid particle properties

A

In an orderly pattern, vibrate at a fixed position and have very low energy with them all close together

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5
Q

Liquid particle properties

A

Reasonably close, randomly arranged and slip past each other with middle energy.

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6
Q

How to check purity of a metal using melting points?

A

In pure metals, during the shift in state, the metal will not gain heat however in non pure they will gradually gain heat.

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7
Q

Solute

A

The substance beong dissolved

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8
Q

Solvent

A

The substance doing the disolving such as water

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9
Q

Brownian motion

A

The random movement of microscopux particles suspended in a fluid caused by the collisions of the particles.

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10
Q

Sublimation

A

A transistion where a substance changes directly from solid to a gas without going through liquid state

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11
Q

Endothermic

A

A reaction/process requiring the absorption of heat

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12
Q

Exothermic

A

A reaction/process that is accompanied bu the release od heat

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13
Q

Why does a heat graph flatline during a change of state?

A

The thermal energy is used to change the state.

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14
Q

Proton

A

A part of an atom found in the nucleus that has a positive charge

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15
Q

Neutron

A

A particle found in the nucleus that has a neutral charge. This can vary between elements which changes their atomic weight.

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16
Q

How do we know how many protons and electrons in any element?

A

The atomic number = proton = electron

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17
Q

Periodic table

A

Groups= up / down
Period= along
Groups 1 to 8 with 8 maybe being 0
Middle area is called the transitional metals

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18
Q

The group names

A

Alkali metals
Alkaline earth metals
Transitin metals
Post-transition metals
Metalloids
Halogens
Noble Gases
Lathanides

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19
Q

Why are the elements placed where they are?

A

They are placed in order of atomic number based upon the number of protons it has.

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20
Q

Element vs compound vs mixture

A

An element is a pure substance that only has a single type of atom.
Compound is a 2 or more types of atom that have been chemically bonded
Mixtures are 2 or more types od atoms that have not been chemically bonded

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21
Q

Chemical vs physical change

A

A physical change changes the form an item is but is the same substance afterwoods.
A chemical change is a change into a completely new substance.

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22
Q

Ways of seperation

A

Sieving- a mixture of sand and gravel can be sepersted by seiving
Filtration-A method of seperating an insoluble solid from a liquid by stopping the solid passing through e.g filter paper.
Evaporation- evaporate a liquid and separating the liquid before condensing the vapours

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23
Q

Acids

A

Acids have a ph scale of less than 7 and will turn indicator paper green. A lower ph scale makes it more acidic

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24
Q

Alkalis

A

Alkalis have a ph scale of more than 7 and will turn indicator blue-purple

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25
Neutralisation
Neutralisation produces water and a salt
26
Law of definite proportions
Also called Prouts low or the law of constant composition where elements in a chemical reaction will always have the same element afterwards.
27
Relative atomic mass
Atomic mass is calculated from the average weight of an atom. This only thinks of the relevant rounded ones You can use this to figure out compounds atomic weight by using their relative atomic mass and timesing it by the amount of each atoms it contains.
28
How to make a neutral ion compound
It must have the same positive and negative charge. E.g 2 aluminum ions are needed with a charge of +3 and 3 oxide ions with a charge of -2 each totally +6 and -6 which counters each other
29
How to predict salt names
HCl- produces salt ending in chloride H2SO4-produces salt ending in sulfate HNO3-produces salt ending nitrate Phosphoric acid-produces salt ending in phosphate
30
31
Properties of metals
Shiny , high melting points(exception mercury) good electricity conductor, good heat conductor, high density, malleable
32
Properties of non-metals
Dull, low melting points, poor conductors of electricity, poor conductors of heat, low density, brittle
33
Exceptions to standard metals and non-metals
Mercury has a low melting points Graphite has a high boiling point and is good at conducting electricity
34
Metals oxides
They act as a base and can neutralise an acid. These contain oxygen. They are solids and certain ones react with water to make an alkali solution
35
Non metal oxides
They contain oxygen. When dissolved into water, they make an acidic solution. They are often gases and have a ph scale lower than 7.
36
Reactions to make oxides
Substance+oxygen=oxides Magnesium + oxygen =MgO Calcium + oxygen=CaO Zinc + oxygen = H2O
37
Metals in group 1
Lithium, sodium,potassium,rubidium,Cesium and francium.
38
Properties of group 1 metals
Relatively soft Low density so first 3 float on water Shiny Low melting points compared to other metals Very reactive to water Reactivity increases going down the group
39
40
Group 2 metals
Beryllium, magnesium, calcium, strontium, barium and radium
41
Properties of group 2 metals
Silvery white appearance Less reactive than group 1 but still quite reactive Reactivity increases whilst going down the group
42
General equations for group 1
Oxygen= 4X+O2 = 2X2O Water= 2X+2H2O=2XOH+2H Chlorine= 2X +Cl2= 2XCl Acids=X+2H=X+(an aqueous substance)+H2
43
General equations of group 2 metals
Oxygen=2X+2O2=2XO Water=X+2H2O=X(OH)2+H2 Acid=X+2H+(an aqueous substance) = X2 +(not that aqueous substance a different one) +H2
44
Group 1 metals uses
Batteries-they give up electrons easily Medicine-have roles in the body that is unique to them Industrial processes-high Reactivity and ability to form various compounds.
45
Group 2 metals uses
Agriculture-to neutralise soil To extract titanium- high Reactivity and reducing agent properties Medicine- makes stomach easy to see
46
Reactivity series
Potassium-Most Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Hydrogen Tin Lead Copper Silver Gold Platinum-least
47
Reactivity series reactions
Potassium to carbon are very reactive metals Zinc and iron are less reactive Anything copper and below are unreactive.
48
Metals+oxygen=reactivity series
The reactivity with oxygen is how they are placed with the ones like potassium reacting vigorously with oxygen which is a reason why it has to be contained the way it is.
49
Protecting from oxidisation
You can create a barrier between it from water and oxygen by: Paint oiling greasing varnishing electroplating galvanisation
50
Metal+acid+reactivity scale
Metals higher up the reactivity scale will reacter more to acids displacing hydrogen and forming a salt if they are higher than hydrogen.
51
Reduction
The gain of electrons by an atom or molecule giving it a higher negative charge
52
Oxidation
The loss of electrons/gain of oxygen/loss of hydrogen. Opposite of reduction when talking about oxygen and electron loss.
53
Displacement reactions
If an element is higher in the reactivity scale than an element in a compound, when heat is added it will displace it.
54
Ore
A naturally occurring rock/mineral that contains a metal or metal compound that can be extracted
55
Alloy
A solid solution of 2 or more metals or a metal and a non metal
56
Alloy properties
Can include increased strength, hardness and corrosion resistant making them better uses for things like machinery such as using steel over iron
57
Key metal discovery dates
Around 8000 BC - Copper Around 3500 BC - bronze(alloy) Around 1200 BC - Iron Around 3800 BC - Lead Around 3500 BC - Tin(alloy) Around 750 BC - Mercury A lot of other metals were discovered more recently about 18th and 19th centuries.
58
Extraction method vs reactivity scale
It influences it as certain metals can be displaced or just found naturally whilst others that are highly reactive require a forcing of chemical reactions.
59
Electrolysis
Using electricity to break down ionic compounds by pushing DC current through an electrolyte. Positive ions will move to the negative electrode(cathode) Negative ions will move to the positive electrode(anode). This leaves simpler compounds or just the element
60
Reactive metal extraction
Metals that are highly reactive like sodium are extracted using electrolysis

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