GCSE chemistry unit 1 Flashcards

1
Q

what is the relative mass of an electron?

A

1/1840 or negligible

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2
Q

what are the charged of a) protons b) neutrons and c) electrons.

A

protons +1 or positive
neutrons 0 or neutral
electrons -1 or negative

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3
Q

The relative mass of protons and neutrons are both 1, where are they held?

A

in the nucleus, the charge here is positive.

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4
Q

electron orbit the _______ in energy levels.

A

Nucleus.

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5
Q

what shell has the highest energy level (out of shell 1, shell 2, shell 3 or shell 4) and how many electrons are on it?

A

Shell 4 and it holds the maximum of 18 electrons. shells 2 and 3 hold the maximum of 8 electrons and the 1st shell contains 2 electrons.

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6
Q

m
X
z

m- relative atomic mass- number of protons added to number of neutrons.
z- atomic number- this shows the number of protons (the number of electrons is the same.)
X- this is the chemical symbol e.g. C is carbon.

how many Protons neutrons and electrons does sodium have?
23
Na
11

A
protons = 11 because the atomic number is 11 
neutrons = 12 because 23 take 11 is 12. 
electrons = 11 because the number of protons is always the same on any atom unless its an ion.
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7
Q

what is most of an atom made up of?

A

empty space.

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8
Q

what is the charge of any atom?

A

neutral, there are the same amount of protons and electrons so the charges cancel each other. if any electrons are added or taken away it becomes a charged ion.

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9
Q

an element is made up of all the same type of atom. The periodic table is ordered by atomic mass. what makes atoms different?

A

the number of subatomic protons in its nucleus.

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10
Q

what is an isotype?

A

an isotype is an atom with a normal amount of protons and electrons but a changed amount of neutrons. this means the atomic number is still the same but it has a different atomic mass.

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11
Q

the group number is the same number as the number of electrons on the outer shell (vertical columns) what do the periods show?

A

the number of shells.

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12
Q

what is group 1 on the periodic table.

A

alkali metals

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13
Q

if a halogen (grp 7) gains an electron during ionic bonding it will have the same atomic structure as a group 8/0 element which can also be called….

A

noble gases

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14
Q

what is the middle section of the periodic table called?

A

transition metals

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15
Q

which side of the periodic table are metals found on??

A

the left side- there are lots of them and they take up 3/4 of the space.

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16
Q

what happens as the number of electrons on the outer shell gets closer to 8 or 0?

A

it becomes more reactive.

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17
Q

metal atoms loose electrons as they do not have many electrons on their out shells. this makes them into positively charged____

A

cations.

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18
Q

non-metal atoms gain the electrons because its easier to fill up their shell rather than get rid of all their electrons.this makes them into negatively charged _____

A

anions

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19
Q

to work out the charge of an ion: for a metal the charge is the group number, and for a non-metal ___ ______ __ ___ _____ ______ _____ _

A

Non-metal= group number minus 8

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20
Q

why do oppositely charged ions attract each other?

A

because of strong electrostatic forces.

21
Q

when 2 ions of opposite charges bond the charges must balance. for example sodium oxide: Na+ and O2- how many sodium would be needed to cancel out the negative charge from the oxygen?

A

2

22
Q

what is covalent bonding?

A

when atoms share electrons to get a full outer shell.

23
Q

what sort of atoms does a covalent bond form between?

A

2 non-metals

24
Q

when non-metals are bonded in a covalent bond what are they called?

A

a molecule.

25
Q

list some properties of gases or liquids bonded by a covalent bond :)

A
  • low melting points (the covalent bond is strong but there are weak intermolecular forces actually holding them together therefore only a low temperature is needed to separate the molecules when they are melted/boiled)
  • don’t conduct electricity.
26
Q

when drawing covalent bonds: you use dots for one atom and crosses for the atom, which shell do you draw?

A

you only have to draw the outer shell.

27
Q

when drawing a letter diagram for covalent bonding how do you decide how many lines to put in-between the atoms?

A

the number of lines is the number of electrons shared, this makes the difference between single double and triple covalent bond.

28
Q

how are metallic bonds formed?

A

they are formed by the attraction between free electrons and the positive metal ions.

29
Q

The bond is strong therefore the melting/boiling point is high. what are some other properties of metallic bonds?

A

they are good conductors of heat and electricity because free electrons can carry a charge or heat energy through the metal. these free electron also make the metal able to slide over each other because of its linear layers. the free electrons keep these layers together when the metal is doing this (ductile and malleable.)

30
Q

limestone’s quarried out of the ground- its great for building and can also be used as a solid conditioner to neutralise acidic soils. limestone is calcium carbonate (CaCO3), when heated it thermally decomposes to make __________

A

calcium oxide (CaO) and carbon dioxide (CO2)

31
Q

the calcium oxide, also known as quick lime, then has _____ added to it to make slaked lime/______ _______ (limestone cycle.)

A

you add water (H2O) which make calcium hydroxide (Ca(OH)2 (s))

32
Q

when we dissolve calium hydroxide in water it makes calcuim hydroxide solution (Ca(OH)2(aq)) also known as lime water, what happens if you bubble carbon dioxide through this?

A

when you bubble CO2 through limewater/ calcium hydroxide solution it goes cloudy which is where lots of small bits of lime stone are being made. and then the limestone cycle restart: calcium carbonate - calcium oxide - calcium hydroxide - calcium hydroxide solution.

33
Q

what is mortar, cement, and concrete. what are they used for and what are their properties?

A

Mortar - cement + sand. used to join bricks together because of its strong sticky properties.
Cement- Made by heating powdered limestone with clay. used to bind materials and good because it doesn’t break easily.
concrete- made from cement + sand +water +crushed rocks. used to make buildings and its great because its very strong.

34
Q

where does limestone come into the making of glass?

A

limestone is used to make the glass stronger. Sand is heated and powdered limestone is added. glass can be used to make buildings and its good because its transparent.

35
Q

calcium carbonate can also react with acid to make a calcium slat, carbon dioxide and…

A

water

36
Q

what happens in a displacement reaction?

A

A more reactive metal takes the place of a less reactive metal when they are bonding with another substance.

37
Q

what is reduction?

A

the removal of oxygen from a compound.

38
Q

what is an ore?

A

a rock containing enough metal to make it economically viable to extract.

39
Q

What does ‘native’ mean?

A

unreactive metals found as elements in nature.

40
Q

explain the reactivity series.

A

list of metals (also carbon and hydrogen) listed in order from most reactive to least reactive. (don’t worry you will be given this in the exam as well as a periodic table.)

41
Q

List properties of metals (8)

A
  • they are solid at room temperature (except mercury)
  • they make a ringing sound when hit.
  • ductile (drawn into wires)
  • malleable (easily bent.)
  • conducts heat
  • conducts electricity
  • some are magnetic (3)
  • high melting points.
42
Q

what are a positive and negative environmental point for quarrying?

A

positive: can create habitats (e.g. peregrine falcon) after the quarrying site has closed down.
negative: may destroy habitats
increase of lorries may produce more CO2 which can cause global warming.

43
Q

economic effects of quarrying limestone?

A

positive: creates money from selling rock
boosts employment
more money in local circulation for locals to spend in pubs etc
negative: costs alot to set up
house prices may drop

44
Q

negative and positive effects from quarrying that affect people (social)

A

positive: creates jobs for people
produces more local building material.
shop owners benefit from more money in circulation
may be a tourist attraction.
negative: creates noise pollution and ruins the view.

45
Q

Metal high up in the reactivity series take alot of ____ for them to break down (thermally decompose)

A

heat

46
Q

what happens in a blast furnace?

A

Metal oxide/carbonate + carbon ——— copper + carbon dioxide
a displacement reaction occurs.
the carbon is a reducing agent as it removes the oxygen from the (e.g.) copper oxide
the (e.g.) copper oxide is an oxidising agent as it gives oxygen to the carbon- when reduction and oxidisation occurs it is called a redox reaction.
this produces CO2

47
Q

explain phytomining

A

where plants are planted in areas where low grade copper ores are in the soil. the plants are then burned and the ash dissolved in acid the electrolysis occurs. you can use low grade ores however it takes a long time for plants to grow and create CO2

48
Q

Explain bioleaching.

A

bacteria absorb copper compounds and then produce leachates which contain copper compounds.
it does take a long time however its good for the environment and can use low grade coppers.

49
Q

Electrolysis means electricity and splitting, how does it work to get pure copper?

A

is the breaking down of substances using electricity. when you do ths you are left with cation and anions. there are two sticks in the electrolyte: cathode (-) which is made up of pure copper and the anode (+) which is made up of impure copper. The copper compound breakdown off the anode and because it is a positive metal ion is attracted to the negatively charged cathode. therefore copper builds up on the cathode electrode. Oxidation happens at the cathode