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Chemistry Paper 1 > 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 nanometers

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2
Q

What is the relative mass of a proton?

A

1

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3
Q

What is the relative mass of a neutron?

A

1

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4
Q

What is the relative mass of an electron?

A

0

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5
Q

What is the relative charge of a proton?

A

+1

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6
Q

What is the relative charge of a neutron?

A

0

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7
Q

What is the relative charge of an electron?

A

-1

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8
Q

What is the mass number?

A

The total number of protons + neutrons

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9
Q

What is the atomic number?

A

The number of protons and electrons.

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10
Q

What is an isotope?

A

Different forms of the same element which have the same number of protons but different numbers of neutrons.

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11
Q

What is the relative atomic mass (same as the mass number)?

A

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

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12
Q

What is a mixture?

A

Two substances that are mixed but not chemically joined.

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13
Q

What are the are the properties of a mixture like?

A

Just a mixture of the properties of the desperate parts.

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14
Q

How can mixtures be separated?

A

Without a chemical reaction.

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15
Q

What does chromatography do?

A

It separates substances in a solution.

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16
Q

When does chromatography work?

A

When substances are aqueous in the same solvent.

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17
Q

What is chromatogram?

A

The picture made by chromatography. Hey

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18
Q

What is filtration?

A

A method which separates insoluble from soluble substances.

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19
Q

What is crystallisation?

A

A method used to obtain s soluble substance from a solution.

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20
Q

What is simple distillation?

A

A method used to separate out a liquid from a solution.

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21
Q

What did John Dalton describe atoms at the start of the 19th century?

A

Solid spheres and that different spheres made up different elements.

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22
Q

What did JJ Thompson conclude from his experiments in 1879?

A

That atoms aren’t solid spheres.

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23
Q

What did JJ Thompson’s measurements of charge and mass show?

A

An atom must contain even smaller negatively charged particles- electrons.

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24
Q

What did the plum pudding model show?

A

The atom as a ball of positive charge with electrons stuck in it.

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25
Q

Which famous experiments did Rutherford and his student Marsden conduct in 1909?

A

The alpha particle scattering experiments.

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26
Q

How did Rutherford and Marsden carry out the alpha particle scattering experiments?

A

The fired positive ply charged alpha particles at an extremely thin sheet of gold foil.

27
Q

What did Rutherford and Marsden expect the alpha particles to do?

A

To pass straight through the sheet or to be slightly deflected at most.

28
Q

Why did Rutherford and Marsden have the expectations that they had?

A

Because the positive charge of the atom was thought to be very spread out through the pudding of the atom.

29
Q

What actually happened to the alpha particles?

A

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

30
Q

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

A
  • The Nuclear model of the atom.

- There is a positively nucleus at the centre where the mass is concentrated and surrounded by a ‘cloud’ of electrons.

31
Q

How are Rutherford’s backed up by what he saw in his experiments?

A

When alpha particles came near to the concentrated mass of the nucleus , they were deflected.
If fired directly at the nucleus, they were deflected backwards.
Otherwise the passed through the empty space.

32
Q

How did other scientists reason that there couldn’t be a ‘cloud ‘ of electrons?

A

Because the electrons in a ‘cloud’ would be attracted to the nucleus causing the atom to collapse.

33
Q

What did Neil Bohr’s nuclear model of the atom suggest and what did he propose?

A

That all the electrons were contained in ‘shells’.

That electrons orbit the nucleus in fixed shells and aren’t anywhere in between.

34
Q

How were elements arranged in the early 1800s?

A

By atomic mass.

35
Q

What were the two obvious ways to categorise elements in the early 1800s?

A
  • Their physical and chemical properties.

- Their relative atomic mass.

36
Q

How did Mendeleev arrange the periodic table?

A

Mainly in order of atomic mass but did switch that order if the properties meant that it should be changed.

37
Q

What happened with Tellurium and Iodine in terms of organisation on the periodic table?

A

iodine has a smaller relative atomic mass but is placed after tellurium as it has similar properties to the elements in that group.

38
Q

Why did Mendeleev leave gaps in his periodic table?

A

To make sure that elements, to be discovered in the future, with similar properties stayed in the same groups.

39
Q

What did some of the gaps that Mendeleev left in the periodic table indicate?

A

The existence of undiscovered elements.

40
Q

What sort of ions do metals from?

A

Positive ions.

41
Q

What sort of ions do non-metals form?

A

Negative ions.

42
Q

Why do metals form positive ions and non-metals form negative ions?

A

For metals to form positive ions it requires less energy to lose 1 than to gain lots.
For non-metals it requires less energy for them to gain 1 electron than to gain lots.

43
Q

What are the general properties of metals?

4

A
  • Strong
  • Malleable
  • Heat and electricity conductors
  • High boiling and melting points
44
Q

What are the general properties of non-metals?

5

A
  • Dull looking
  • Brittle
  • Not always solid
  • Don’t conduct electricity
  • Lower density
45
Q

What are the properties of transition metals?

11

A
  • Shiny
  • Malleable
  • sonorous
  • Water proof
  • Conduct electricity
  • Coloured Compounds
  • Ductile (can be drawn into wires)
  • High melting points
  • Conduct heat
  • Often make good catalysts
  • insoluble
46
Q

Why can transition metals have different numbers of ions?

A

Because they have different numbers of electrons on their outer shells.

47
Q

Why are transition metal compounds coloured?

A

The electrons are able to move around and emit different colours.

48
Q

What are the properties of the Alkali Metals (group 1 elements)?
(8)

A
  • Shiny
  • Low melting points
  • Soft
  • Low density
  • Form white compounds
  • Good conductors of heat and electricity
  • Insoluble
  • Malleable
49
Q

What happens as you go down group 1?

3

A
  • Reactivity increases
  • Lower melting and boiling points
  • High relative atomic mass
50
Q

What are alkali metals like compared to transition metals?

A

Group 1 are much more reactive, less dense, less strong, less hard and have lower melting points.

51
Q

What are group 7 known as?

A

The halogens

52
Q

What are the halogens?

A

Non-metals with coloured vapours.

53
Q

What is fluorine like?

A

It is very reactive and a yellow, poisonous gas.

54
Q

What is chlorine like?

A

It is fairly reactive and a poisonous, dense, green gas.

55
Q

What is bromine like?

A

It is a dense, poisonous, brown, volatile liquid.

56
Q

What is iodine like?

A

It is a dark, grey, crystalline solid or a purple vapour.

57
Q

What do all group 7 elements exist as?

A

Molecules

58
Q

What happens as you go down group 7?

A

The halogens become:

  • Less reactive (its harder to gain an extra electron because the shell is further away from the nucleus).
  • Have higher melting and boiling points.
  • Have higher relative atomic masses.
59
Q

What will more reactive halogens do to less reactive halogens?

A

Displace them.

60
Q

Why are all the Nobel gases inert (they don’t react much)?

A

They all have 8 electrons in their outer shell, making them stable.
Helium has two.

61
Q

What sort of gases are noble gases?

A

Monatomic gases- single atoms are not bonded to each other.

62
Q

Describe al the noble gases.

A

They are all colourless, non-flammable gases at room temperature.

63
Q

What happened as you go down the noble gases?

A
  • The boiling points and relative atomic masses increase.
  • The increase in boiling point is due to an increase in the number of electrons meaning there are greater intermolecular forces.

Chemistry Paper 1 (4 decks)

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