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Chemistry GCSE Paper 1 > 1. Atomic Structure and the Periodic Table > Flashcards

1. Atomic Structure and the Periodic Table Flashcards

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1
Q

What is the radius of an atom?

A

0.1nm (1x10^-10 m)

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2
Q

What is the nucleus of an atom?

A

Middle of the atom, contains protons and neutrons, has a radius of 1x10^-14m which is around 1/10000 of the radius of the atom, positive charge because of protons and almost the whole mass is concentrated in the nucleus.

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3
Q

What are the electrons of an atom?

A

Move around the nucleus in electron shells, negatively charged and tiny, volume of their orbits determines the size of the atom and have virtually no mass.

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4
Q

What is the relative mass of a proton, neutron and electron?

A

Proton= 1, Neutron= 1 and Electron= Very small (0)

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5
Q

What is the charge of a proton, neutron and electron?

A

Proton= +1, Neutron= 0 and Electron= -1

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6
Q

What is the charge of an atom?

A

Neutral- have the same number of protons as electrons. Charge on the electrons is the same size as the protons but opposite.

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7
Q

What does the atomic number tell you?

A

How many protons there are.

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8
Q

What does the mass number tell you?

A

The total number of protons and neutrons in the atom.

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9
Q

How do you calculate the number of neutrons?

A

Subtract the atomic number from the mass number.

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10
Q

What decides what type of atom it is?

A

The number of protons.

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11
Q

What is an element?

A

A substance that only contains atoms with the same number of protons.

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12
Q

What are isotopes?

A

Different forms of the same element, which have the same number of protons but a different number of neutrons. (Same atomic number but different mass number.)

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13
Q

What is relative atomic mass (Ar)?

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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14
Q

How do you calculate relative atomic mass?

A

sum of (isotope abundance x isotope mass number)/sum of total abundances.

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15
Q

What are compounds?

A

Substances formed from two or more elements chemically bonded together.

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16
Q

How do metal atoms form positive ions?

A

By losing electrons.

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17
Q

How do non-metals form negative ions?

A

By gaining electrons.

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18
Q

What’s a disadvantage of using word equations?

A

You can’t tell what has happened to each of the atom straight away.

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19
Q

What is a mixture?

A

A substance made up of elements and compounds not chemically bonded together.

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20
Q

What are five methods of seperating mixtures?

A

Filtration, crystallisation, simple distillation, fractional distillation and chromatography.

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21
Q

Explain how to carry out a paper chromatography practical?

A
  1. Draw a line in pencil 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. Make sure the ink isn’t touching the solvent.
  3. Place a lid on the container to stop the solvent from evaporating.
  4. The solvent will seep up the paper carrying the ink with it. Each dye in the ink will move up the paper at a different rate so the dyes will seperate out.
  5. When the solvent has nearly reached the top of the paper, take the paper out of the beaker to dry.
  6. The end result is a pattern of spots called chromatogram.
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22
Q

Chromatography practical: What solvents can be used?

A

Depends on what’s being tested. Water or ethanol.

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23
Q

What is filtration?

A

Used to seperate an insoluble solid from a liquid reaction mixture. Can also be used in purification. (Solid impurities seperated out).

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24
Q

How can you seperate a soluble salt from a solution with evaporation?

A
  1. Pour the solution into an evaporating dish.
  2. Slowly heat the solution. The solvent will evaporate and the solution will become more concentrated. Crystals will start to form.
  3. Keep heating until all you have left is dry crystals.
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25
Q

Why can’t evaporation always be used to seperate soluble salts from a solution?

A

Can only be used if the salt doesn’t decompose when heated.

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26
Q

How can you seperate a soluble salt from a solution with crystallisation?

A
  1. Pour the solution into an evaporating dish and gently heat the solution. Some of the solvent will evaporate.
  2. At the point of crystallisation (when you see crystals start to form), 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. You could also use a drying oven or a desiccator.
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27
Q

What is rock salt?

A

A mixture of salt and sand.

28
Q

What makes it easy to seperate rock salt?

A

Salt dissolves in water and sand doesn’t - their difference in physical properties.

29
Q

Describe how you would seperate rock salt.

A
  1. Grind the mixture to make sure that the salt crystals are small and will dissolve easily.
  2. Put the mixture in water and stir. The salt will dissolve but the sand won’t.
  3. Filter the mixture. The grains of sand won’t fit through the tiny holes in the filter paper, so they will collect on the paper. The salt passes through the filter paper as it is part of the solution.
  4. Evaporate the water from the salt so that it forms dry crystals. (Could also use crystallisation).
30
Q

Explain how you would carry out simple distillation.

A
  1. The solution is heated. The part of the solution that has the lowest boiling point will evaporate first.
  2. The vapour is then cooled, condenses and is colleced.
  3. The rest of the solution is left behind in the flask.
31
Q

What is a problem with simple distillation?

A

Can only be used to seperate things with very different boiling points.

32
Q

What is fractional distillation?

A

Seperating a mixture of liquids with similar boiling points.

33
Q

Describe how fractional distillation works.

A
  1. Put your mixture in a flask and stick a fractionating column on top. Then heat it.
  2. The liquids will evaporate at different temperatures as they have different boiling points.
  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 a higher boiling point may also start to evaporate but the column is cooler towards the top so they will only get part of the way before condensing and running back towards the flask.
  5. When the temperature of the first liquid has been collected, raise the temperature until the next one reaches the top.
34
Q

How did John Dalton describe the atom?

A

Start of the 19th century - as solid spheres. Thought that different spheres made up different elements.

35
Q

How did JJ Thomson disprove this?

A

1897, due to his measurements of charge and mass, he concluded that an atom must contain smaller negatively charged particles (electrons). The new theory was know as the ‘plum pudding model’. It showed the atom as a ball of positive charge with electrons stuck in it.

36
Q

What were the alpha particle scattering experiments?

A

In 1909, Ernest Rutherford and his student Ernest Marsden fired positively charged alpha particles at an extremely thin sheet of gold. Most particles passed straight through the sheet as expected. However, some were deflected more than expected and a small number were deflected backwards.

37
Q

What idea did Rutherford come up with to explain his evidence?

A

The nuclear model of the atom. Tiny positively charged nucleus in the centre where most of the mass was concentrated. A ‘cloud’ of negative electrons surrounding this, so most of the atom is empty space. When alpha particles come near the concentrated, positive nucleus, they were deflected. If they were fired directly at the nucleus they were deflected backwards. Otherwise, they passed through the empty space.

38
Q

How did scientists disprove Rutherford’s model?

A

Realised that electrons in the ‘cloud’ around the nucleus of an atom would be attracted to the nucleus causing the atom to collapse.

39
Q

What was Bohr’s nuclear model?

A

Suggested that all the electrons were contained in shells. Electrons orbit the nucleus at fixed distances. It was supported by many experiements and helped to explain other scientist’s observations at the time.

40
Q

What was a further experiment by Rutherford?

A

Showed that the nucleus could be divided into smaller particles which has the same charge as a hydrogen nucleus called protons.

41
Q

What did James Chadwick discover?

A

Neutrons (neutral particles).

42
Q

How many electrons are allowed in each cell?

A

2,8,8…etc

43
Q

How were the elements ordered in the early 1800s?

A

Relative atomic mass. However some elements were placed in the wrong groups as their properties were not taken into account.

44
Q

How did Dmitri Mendeleev order the elements in 1869?

A

Mainly in order of atomic mass but did switch the order if the properties meant it should be changed. He also left gaps to make sure that when elements with the same properties were discovered, they could stay in the right group. When they were found and fitted the pattern, it confirmed Mendeleev’s ideas.

45
Q

How are elements arranged in the modern periodic table?

A

Increasing atomic (proton) number. This meant that there are repeating patterns in the properties of the elements.

46
Q

Describe the columns of the periodic table.

A

Called groups. Formed by elements with similar properties. Group number tells you how many electrons there are in the outer shell.

47
Q

Why is it useful to know the properties of one element?

A

You can predict the properties of elements in the same group.

48
Q

Describe the rows in the periodic table?

A

Called periods. Represents the number of shells.

49
Q

What are properties of metals?

A

Have metallic bonding causing them to have similar physical properties.

  1. They’re strong but malleable.
  2. They are good conductors of heat and electricity.
  3. Have high boiling and melting points.
50
Q

What are properties of non-metals?

A

Dull-looking, brittle, aren’t always solid at room temp, don’t generally conduct electricity, often have lower density.

51
Q

What are properties of transition metals?

A
  1. Can have more than one ion.
  2. Often coloured so form colourful compounds, eg. potassium chromate(VI), which is yellow, potassium(VII) manganate is purple.
  3. Often make good catalysts.
52
Q

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

A
  1. Increasing reactivity- the outer electron is more easily lost as the attraction between the nucleus and electron decreases.
  2. Lower melting and boiling points.
  3. Higher relative atomic mass.
53
Q

What are properties of the alkali metals?

A

Very reactive as they have one electron on their outer shell, soft and low density.

54
Q

What ions do alkali metals form?

A

1+.

55
Q

What do alkali metals generally react to form?

A

Ionic compounds (white solids that dissolve to form colourless solutions).

56
Q

Describe alkali metal’s reaction with water.

A

React vigorously to produce hydrogen gas and metal hydroxides (salts that dissolve in water to produce alkaline solutions). The more reactive the metal is, the more violent the reaction. The amount of energy given out by the reaction increases as you go down the group.

57
Q

Describe alkali metal’s reaction with chlorine.

A

React vigirously when heated with chlorine gas to form white metal chloride salts. Reaction with chlorine gets more vigorous as you go down the group.

58
Q

Describe alkali metal’s reaction with oxygen.

A

React to form metal oxides. Form a dull metal.

59
Q

Compare the properties of alkali metals to transition metals.

A

Group 1 metals are more reactive than transition metals (react more vigorously with water, oxygen or Group 7 elements). Also much less dense, strong and hard than transition metals and have a much lower melting point.

60
Q

What coloured vapours do the group 7 elements form?

A

Fluorine: very reactive, poisonous yellow gas. Chlorine: fairly reactive, poisonous dense green gas. Bromine: dense, poisonous, red-brown volatile liquid. Iodine: dark grey crystalline solid or a purple vapour.

61
Q

Describe the trends as you go down group 7.

A
  1. Become less reactive, harder to gain an extra electron, outer sheel further away from nucleus.
  2. Have higher melting and boiling points.
  3. Have higher relative atomic masses.
62
Q

Why do group seven elements react in similar ways?

A

They all have 7 electrons in their outer shell.

63
Q

What ions do halogens form?

A

1- ions (halides).

64
Q

Describe group 0 elements.

A

Noble gases, eg. helium, neon, argon..etc. Have 8 electrons in their outer energy level (apart from helium which has two) giving them a full outer shell. Their outer shell is energetically stable so doesn’t need to give up of gain electrons.

65
Q

What are properties of Group 0 elements?

A
  1. Inert, don’t react.
  2. Exist as monatomic gases.
  3. Colourless gases at room temperature.
  4. Non-flammable (as they are inert).
66
Q

Describe the trends of Group 0 elements as you go down the group.

A

Boiling points increase along with increasing relative atomic masses. Due to the increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome.

Chemistry GCSE Paper 1 (5 decks)

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