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Chemistry GCSE > Topic 1 - Atomic Structure and the Periodic Table > Flashcards

Topic 1 - Atomic Structure and the Periodic Table Flashcards

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1
Q

What is the radius of an atom?

A

0.1 nm (1*10^-10m)

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2
Q

What are the main structures of an atom?

A

Nucleus

Electrons

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3
Q

Where is the nucleus?

A

In the middle of the atom

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4
Q

What is in the nucleus?

A

Protons

Neutrons

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5
Q

What is the radius of the nucleus?

A

1*10^-14m

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6
Q

What is the nucleus’s charge?

A

Positive (protons)

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7
Q

Where is the mass of the atom concentrated?

A

In the nucleus

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8
Q

How are electrons present in an atom?

A

They move around the nucleus in electron shells

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9
Q

What is the charge of an electron?

A

Negative (-1)

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10
Q

What is the charge of a proton?

A

Positive (+1)

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11
Q

What is the charge of a neutron?

A

Neutral (0)

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12
Q

What is the relative mass of a proton?

A

1 (same as neutron)

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13
Q

What determines the size of an atom?

A

The volume of the orbit of its electrons

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14
Q

What is the mass of an electron?

A

Practically 0

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15
Q

What is the charge of an atom?

A

Neutral - the number of protons and electrons is equal, cancelling each other out

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16
Q

How does an ion differ from an atom?

A

An ion has an overall charge because the number of protons isn’t equal to the number of electrons, while an atom is neutral

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17
Q

What does the atomic number tell us?

A

How many protons are in an atom (the smaller number)

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18
Q

What does the mass number tell us?

A

The total number of protons and neutrons in an atom (the bigger number)

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19
Q

What defines which element an atom is?

A

The number of protons in the nucleus

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20
Q

What is an element?

A

A substance which contains only atoms with the same number of protons

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21
Q

What are isotopes?

A

Different forms of the same element, with the SAME number of PROTONS but a DIFFERENT number of NEUTRONS (they have the same atomic number but a different mass number)

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22
Q

What is relative atomic mass?

A

The average mass taking into account the different masses and abundance’s of all isotopes that make up an element

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23
Q

What is the formula for relative atomic mass?

A

relative atomic mass = (sum of (isotope abundance*isotope mass number))/(sum of abundances of all the isotopes)

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24
Q

What are compounds?

A

Substances formed of +2 elements, the atoms of each being in a fixed proportion throughout the compound, where the atoms are held together by chemical bonds

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25
Q

What is involved in making bonds between atoms?

A

Electrons - their being given away, shared or taken - the nucleus isn’t affected

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26
Q

What is needed to separate original elements of a compound?

A

A chemical reaction

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27
Q

Which kinds of elements is a compound consisting of ions made out of?

A

A metal and a non-metal

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28
Q

What is ionic bonding?

A

The attraction of oppositely charged ions formed by a compound containing metals and non-metals

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29
Q

What is the electron exchange that takes place in ionic bonding?

A

The metal atoms lose electrons (forming positive ions) which the non-metal atoms gain (forming negative ions)

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30
Q

What does a compound of non-metals consist of?

A

Molecules

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31
Q

Which kind of bonding occurs between non-metals?

A

Covalent bonding

32
Q

What happens to electrons in covalent bonding?

A

Atoms share electrons between each other

33
Q

What is the formula for carbon dioxide?

A

CO2

34
Q

What is the formula for ammonia?

A

NH3

35
Q

What is the formula for water?

A

H2O

36
Q

What is the formula for sodium chloride?

A

NaCl

37
Q

What is the formula for carbon monoxide?

A

CO

38
Q

What is the formula for hydrochloric acid?

A

HCl

39
Q

What is the formula for calcium chloride?

A

CaCl2

40
Q

What is the formula for sodium carbonate?

A

Na2CO3

41
Q

What is the formula for sulfuric acid?

A

H2SO4

42
Q

What is the difference between a mixture and a compound?

A

While the parts of a compound are chemically bound, in a mixture the different parts (whether elements or compounds) are not chemically bound

43
Q

List the 5 physical methods of separating mixtures

A 
Filtration
Crystallisation
Simple distillation
Fractional distillation
Chromatography
(These DO NOT involve CHEMICALS reactions)
44
Q

What is the method for chromatography?

A

1) Draw a line near the bottom of a sheet of filter paper
2) Add a spot of ink to the line and place the sheet in a beaker of solvent (eg water)
3) The solvent depends on what’s being tested - if it dissolves well in water, that’s usually used.
4) Make sure the ink isn’t touching the solvent so it isn’t dissolved
5) Place a lid on top of the container to prevent the solvent Fromm evaporating
6) The solvent sweeps up the paper, carrying the ink with it
7) Each different dye in the ink will travel at a different rate, so the different dyes will separate out. Each dye will create a spot - 1 spot per dye
8) If any dyes are insoluble, they’ll stay baseline
9) When the solvent is close to the top of the paper, take it out and dry it

45
Q

What is the end result of chromatography called?

A

A chromatogram

46
Q

What use chromatography used to separate.

A

Inks and dyes

47
Q

What does filtration separate?

A

Insolubles solids from liquids

48
Q

Where can filtration be used?

A

In purification, when removing solid impurities in the reaction mixture

49
Q

List two methods which can be used to separate soluble solids from solutions.

A

Evaporation

Crystallisation

50
Q

When can evaporation be used?

A

If the salt doesn’t break down when heated

51
Q

What is the method for evaporation?

A

1) Pour the solution into the evaporation dish
2) Slowly heat the solution. The solvent will evaporate, and the solution will get more concentrated, eventually creating crystals
3) Keep heating the dish until only dry crystals are left

52
Q

What’s is the method for crystallisation?

A

1) Pour the solution into the evaporation dish and gently heat, so some of the solvent evaporates and the solution becomes more concentrated
2) Once some of the solution has evaporated/some crystals begin to form, remove the dish from the heat and leave it to cool
3) The salt should start to form crystals as it becomes insolubles in the cold, highly concentrated solution
4) Filter the crystals out and leave them somewhere warm to dry

53
Q

How can rock salt (or any other mixture containing soluble and insoluble solids) be separated?

A

By a combination of filtration and crystallisation

54
Q

Give the method for separating rock salt.

A

1) Grind - makes salt crystals small, easier to dissolve
2) Dissolve - put mixtures into water and stir (salt dissolves, sand doesn’t)
3) Filter - the sand won’t fit through the holes in the filter paper, so only the salt will pass through (part of solution)
4) Evaporate - evaporate water from solution to form dry salt crystals

55
Q

What is simple distillation used for?

A

Separating out a liquid from a solution

56
Q

Give the method for simple distillation.

A

1) Heat the solution - the liquid with the lowest boiling point will evaporated first
2) The vapour will pass throughout then condenser and will condense back into a liquid
3) Collect the liquid
4) The rest of the solution is left in the flask

57
Q

What is the limitation of simple distillation?

A

It can only separate liquids with very different boiling points

58
Q

Which kind of distillation is used for liquids with similar boiling points?

A

Fractional distillation

59
Q

Give the method for fractional distillation.

A

1) Put the mixture into the flask and insert the fractionating column on top.
2) Heat the flask - the different liquids have different boiling points and Willa evaporate at different temperatures
3) First the liquid with the lowest boiling point will evaporate - when the temperature on the top thermometer matches the boiling point of the liquid, it will reach the top of the column
4) Liquids with higher boiling points may also evaporate, but as the fractionating column is cooled at the top they will condense and trickle back into the flask
5) Once the first liquid is collected, the temperature is raised until the next one reaches the top

60
Q

How did John Dalton describe atoms?

A

As solid spheres, with different spheres making up different elements (at the beg. of 19th c.)

61
Q

What did J J Thompson discover in 1897?

A

Atoms weren’t solid spheres and contained negatively charged electrons

62
Q

What was J J Thompson’s theory?

A

The “plum pudding model” - that the atom was a ball of positive charge with electrons stuck in it

63
Q

Which experiments did Ernest Rutherford conduct in 1909?

A

The alpha particle scattering experiments where positively charged alpha particles were fired at a thin sheet of gold

64
Q

How did Rutherford’s experiment prove the plum pudding model wrong?

A

Rather than the alpha particles passing straight through or only being slightly deflected by the gold sheet, many particles were deflected more than expected, with something being deflected backwards - as Thomson’s model had the positive charge spread out through the atom, it couldn’t be right

65
Q

What did Rutherford’s atom model introduce?

A

A positively charged nucleus at the centre of the atom with a cloud of negatively charged electrons surrounding it, leaving most of the atom to be empty space.

66
Q

How did the alphas particle scattering experiments support Rutherford’s atom model?

A

Alpha particles near the concentrated, positively charged nucleus would be deflected (if directly then backwards), otherwise passing through empty space

67
Q

What did Bohr introduce to the theory of atomic structure?

A

That electrons orbit the nucleus in fixed shells, each shell a fixed distance from the nucleus. Otherwise, all the electrons would be attracted to the nucleus, causing the atom to collapse

68
Q

What did James Chadwick introduce to the theory of the atomic structure?

A

The existence of neutral particle should in the nucleus, called neutrons

69
Q

What do electrons occupy?

A

Shells/energy levels

70
Q

Which energy levels are filled first?

A

The lowest ones, closest to the nucleus

71
Q

How many electrons are allowed in each shell?

A

1st: 2
2nd: 8
3rd: 8

72
Q

When are atoms stable?

A

When they have a full outer electron shell, like noble gases (Group 0)

73
Q

What is the electronic structure of magnesium? (Atomic no. = 12)

A

2, 8, 2

74
Q

How were elements arranged in the early 1800s?

A

By their physical and chemical properties, and by their relative atomic mass - some elements were placed in the wrong group because they were placed in order of Mr, not taking properties into account

75
Q

What dude Dmitri Mendeleev do in 1869?

A

He placed the known elements into a Table of Elements, prioritising putting elements into groups according to properties over in the order of Mr, while taking Mr into account. He also left gaps in the table for elements yet to be discovered.

Chemistry GCSE (2 decks)

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