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Chemistry > C1 atomic structure and the periodic table > Flashcards

C1 atomic structure and the periodic table Flashcards

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1
Q

what is the radius of an atom?

A

about 0.1 nanometers

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2
Q

what does the nuclear symbol of an atom tell you?

A

its atomic (proton) number and mass number

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3
Q

what does the atomic number tell you?

A

how many protons there are

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4
Q

what are isotopes?

A

different forms of the same element, which have the same number of protons but a different number of neutrons

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5
Q

why is relative atomic mass used instead of mass number when referring to the element as a whole?

A

because elements can exist as a number of different isotopes

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6
Q

what is relative atomic mass?

A

an average mass taking into account the different masses and abundances of all the isotopes that make up the element

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7
Q

what is the formula to work out the relative atomic mass of an element?

A

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

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8
Q

substitute the formula for this question:
copper has two stable isotopes. Cu-63 has an abundance of 69.2% and Cu-65 has an abundance of 30.8%. Calculate the relative atomic mass of copper.

A

……………………………(69.2 x 63) + (30.8 x 65)
relative atomic mass = _______________
………………………………………….69.2 + 30.8

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9
Q

what are compounds?

A

substances formed from two or more elements, the atoms of each are in fixed proportions throughout the compound and they’re held together by chemical bonds

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10
Q

are the nuclei of the atoms affected when a bond is made?

A

no

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11
Q

do metal atoms lose or gain electrons? do they form positive or negative ions?

A

metal atoms lose electrons to form positive ions

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12
Q

do non-metal atoms lose or gain electrons? do they form positive of negative ions?

A

non-metal atoms gain electrons to form negative ions

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13
Q

what is the chemical formula for ammonia?

A

NH3

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14
Q

what is the chemical formula for hydrochloric acid?

A

HCl

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15
Q

what is the chemical formula for sulfuric acid?

A

H2SO4

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16
Q

balance the equation H2SO4 + NaOH -> Na2SO4 + H2O

A

H2SO4 + 2NaOH -> Na2SO4 + 2H2O

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17
Q

name five physical methods that can be used to separate a mixture

A
  1. filtration
  2. crystallisation
  3. simple distillation
  4. fractional distillation
  5. chromatography
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18
Q

what are the steps of paper chromatography?

A
  1. draw a pencil 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, e.g. water
  3. make sure the ink isn’t touching the solvent
  4. place a lid on top of the container to stop the solvent evaporating
  5. the solvent seeps up the paper, carrying the ink with it
  6. each different dye in the ink will move up the paper at a different rate, so the dyes will separate out
  7. if any of the dyes in the ink are insoluble in the solvent you’ve used, they’ll stay on the baseline
  8. when the solvent has nearly reached the top of the paper, take the paper out of the beaker and leave it to dry
  9. the end result is a pattern of spots called a chromatogram
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19
Q

what can filtration be used for?

A

filtration separates insoluble solids from liquids. It can be used if your product is an insoluble solid that needs to be separated from a liquid reaction mixture. It can also be used in purification.

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20
Q

what are two ways to separate soluble solids from solutions?

A

evaporation and crystallisation

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21
Q

what are the three steps of using evaporation to separate soluble solids from solutions?

A
  1. pour the solution into an evaporating dish
  2. slowly heat the solution. The solvent will evaporate and the solution will get more concentrated. Eventually, crystals will start to form
  3. keep heating the evaporating dish until all you have left are dry crystals
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22
Q

what are the 4 steps of using crystallisation to separate soluble solids from solutions?

A
  1. pour the solution into an evaporating dish and gently heat the solution
  2. once some of the solvent has evaporated, or when you see crystals start to form (the point of crystallisation) remove the dish from the heat and leave the solution to cool
  3. the salt should start to form crystals as it becomes insoluble in the cold, highly concentrated solution
  4. filter the crystals out of the solution, and leave them in a warm place to dry
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23
Q

when would you use crystallisation over evaporation when separating soluble solids from solutions?

A

when the salt decomposes when it’s heated

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24
Q

what is rock salt?

A

a mixture of salt and sand

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25
Q

what is simple distillation used for?

A

separating out a liquid from a solution

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26
Q

what are the steps of simple distillation?

A
  1. the solution is heated. the part of the solution that has the lowest boiling point evaporates first
  2. the vapour is then cooled, condenses and is collected
  3. the rest of the solution is left behind in the flask
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27
Q

what is a problem with simple distillation?

A

you can only use it to separate things with very different boiling points

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28
Q

what process do you use to separate a mixture of liquids with similar boiling points?

A

fractional distillation

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29
Q

what are the steps of fractional distillation?

A
  1. you put your mixture in a flask with a fractionating column on top and heat it
  2. the different liquids will all have different boiling points, so they will evaporate at different temperatures
  3. the liquid with the lowest boiling point evaporates first. When the temperature on the thermometer matches the boiling point of this liquid, it will reach the top of the column
  4. liquids with higher boiling points might also start to evaporate, but the column is cooler towards the top so they will only get part of the way up before condensing and running back down towards the flask
  5. when the first liquid has been collected, you raise the temperature until the next one reaches the top
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30
Q

what was the plum pudding model?

A

it was a model that showed the atom as a ball of positive charge with negative electrons embedded in it

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31
Q

what were atoms believed to be at the start of the 19th century? who described them as this?

A

at the start of the 19th century John Dalton described atoms as solid spheres, and said that different spheres made up the different elements

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32
Q

what was the first subatomic particle to be discovered? who discovered it?

A

JJ Thomson discovered electrons

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33
Q

when was the ‘plum pudding’ model first introduced?

A

1897

34
Q

what was the expected outcome of the alpha particle scattering experiment and why?

A

they were expecting the particles to pass straight through, or be very slightly deflected at most. this was because the positive charge of each atom was thought to be very spread out through the ‘pudding’ of the atom.

35
Q

what were the results of the alpha scattering experiment?

A

while most of the particles did go straight through the gold sheet, some were deflected more than expected, and a small number were deflected backwards.

36
Q

Who did the alpha particle scattering experiment? when did they do it?

A

Ernest Rutherford and his student Ernest Marsden in 1909

37
Q

what did Ernest Rutherford do in the alpha scattering experiment?

A

fire positively charged alpha particles at an extremely thin sheet of gold

38
Q

what was Rutherfords new idea for the model of the atom based on the Alpha particle scattering experiment?

A

He came up with the nuclear model of the atom - a tiny, positively charged nucleus at the centre, where most of the mass is concentrated. A ‘cloud’ of negative electrons surrounds this nucleus, so most of the atom is empty space.

39
Q

what was the problem with Rutherford’s nuclear model of the atom?

A

electrons in a ‘cloud’ around the nucleus of an atom, as Rutherford described, would be attracted to the nucleus, causing the atom to collapse

40
Q

what was Niels Bohr’s solution to the problems with Rutherford’s nuclear model?

A

He suggested that all the electrons orbited the nucleus in fixed shells, each one a set distance from the nucleus

41
Q

who discovered neutrons?

A

James Chadwick

42
Q

how were elements arranged in the early 1800s?

A

atomic mass

43
Q

when did Dmitri Mendeleev create his Table of Elements?

A

1869

44
Q

How did Dmitri Mendeleev organise the elements?

A

mainly in order of atomic mass, but he did switch the order if the properties meant it should be changed

45
Q

why were gaps left in Dmitri Mendeleev’s Table of Elements?

A

to make sure that elements with similar properties stayed in the same groups. Some of these gaps indicated the existence of undiscovered elements and allowed Mendeleev to predict what their properties might be. when they were found and they fitted the pattern

46
Q

who came up with the modern day periodic table?

A

Dmitri Mendeleev

47
Q

how are elements laid out in the periodic table?

A

in order of increasing atomic (proton) number

48
Q

where are metals and non-metals found on a periodic table?

A

metals are found to the left and non-metals to the right

49
Q

what does the group number tell you about an element?

A

how many electrons there are in the outer shell

50
Q

do elements with similar properties share the same group or period?

A

group

51
Q

if you know the properties of one element, can you predict properties of other elements in that group?

A

yes

52
Q

in group one (the alkali metals) does reactivity increase or decrease as you go down the group?

A

increase

53
Q

in group 7 (the halogens) does reactivity increase or decrease as you go down the group?

A

decrease

54
Q

are there more metal or non-metal elements?

A

metal

55
Q

do metals form positive or negative ions? do non-metals form positive or negative ions?

A

metals form positive ions and non-metals form negative ions

56
Q

what are some properties of metals?

A
  • they’re strong (hard to break), but can be bent or hammered into different shapes (malleable)
  • they are good conductors of heat and electricity
  • they have high boiling and melting points
57
Q

what are some properties of non-metals?

A
  • dull-looking
  • more brittle
  • aren’t always solids at room temperature
  • don’t generally conduct electricity
  • often have a lower density
58
Q

what are the alkali metals?

A

lithium, sodium, potassium, rubidium, caesium and francium

59
Q

describe the group 1 elements

A

reactive, soft metals that have a low density

60
Q

what are the trends for the alkali metals as you go down group 1?

A
  • increasing reactivity
  • lower melting and boiling points
  • higher relative atomic masses
61
Q

why does reactivity increase as you go down group 1?

A

the outer electron is more easily lost as the attraction between the nucleus and electron decreases, because the electron is further away from the nucleus the further down the group you go

62
Q

how many electrons do the alkali metals have in their outer shells?

A

1`

63
Q

what happens when group 1 metals are put in water?

A

they react very vigorously

64
Q

describe the reaction of lithium, sodium or potassium with water

A

they float and move around the surface of the water, fizzing furiously

65
Q

what does the reaction between group 1 metals and water produce?

A

hydrogen and a hydroxide

66
Q

what are the word and balanced symbol equations for the reaction between sodium and water?

A

sodium + water -> sodium hydroxide + hydrogen

2Na + 2H2O -> 2NaOH + H2

67
Q

what happens when a group 1 metal reacts with chlorine?

A

it forms a salt

68
Q

what are the word and balanced symbol equations for the reaction between sodium and chlorine?

A

sodium + chlorine -> sodium chloride

2Na + Cl2 -> 2NaCl

69
Q

what do group 1 metals react with oxygen to form?

A

a metal oxide

70
Q

what are all non-metals with coloured vapours?

A

halogens

71
Q

what colour is flourine gas?

A

yellow

72
Q

what colour is chlorine gas?

A

green

73
Q

what colour is bromine? what state is it?

A

it is a red-brown volatile liquid

74
Q

what colour is iodine as a solid? what colour is it as a gas?

A

it is a dark grey solid or a purple vapour

75
Q

are the halogens diatomic?

A

yes

76
Q

what are the trends as you go down group 7 (the halogens)?

A
  • become less reactive
  • have higher melting and boiling points
  • have higher relative atomic masses
77
Q

why do halogens become less reactive as you go down the group?

A

it becomes harder to gain an extra electron because the outer shell is further from the nucleus so it’s less attracted to it

78
Q

what are the group 0 elements?

A

the noble gases

79
Q

what group is all inert, colourless gases

A

group 0, the noble gases

80
Q

why are the noble gases unreactive?

A

they have a full outer shell. As their outer shell is energetically stable they don’t need to give up or gain electrons to become more stable

81
Q

do the boiling points of the noble gases increase or decrease as you move down the group? why?

A

the boiling points increase because as you go down the group the number of electrons in each atom increases, which leads to greater intermolecular forces between the atoms. This increases the boiling point as the intermolecular forces are stronger and harder to overcome

82
Q

what is the formula for sodium carbonate?

A

Na2CO3

Chemistry (16 decks)

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