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Chemistry Paper 1 > C1 - Atomic Structure > Flashcards

C1 - Atomic Structure Flashcards

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1
Q

Define atom.

A

The smallest part of an element that can still be recognized as that element.

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2
Q

Define element.

A

A substance made of only one type of atom.

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3
Q

Define compound.

A

A substance made of two or more different atoms chemically bonded together.

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4
Q

Define molecule.

A

A substance made of more than one atom chemically bonded together (can be atoms of the same element!).

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5
Q

State the masses of the subatomic particles.

A

Protons: 1
Neutrons: 1
Electrons: almost 0

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6
Q

State the relative charges of the subatomic particles.

A

Protons = +1
Neutrons = 0
Electrons = -1

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7
Q

What is the plum pudding model of the atom?

A

A ball of positive charge with negative electrons studded into it.

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8
Q

What did Rutherford’s alpha scattering experiment prove?

A

Atoms have a small dense nucleus with a positive charge.

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9
Q

How did Bohr adapt the model of the atom?

A

He said electrons orbit the nucleus at specific distances.

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10
Q

What did Chadwick’s work give evidence of?

A

That the nucleus also contained neutrons as well as protons.

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11
Q

What is the atomic number of an atom?

A

The number of protons in an atom.

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12
Q

How were elements arranged in the early attempts of the periodic table?

A

By atomic weight.

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13
Q

How are elements in the periodic table arranged?

A

By atomic number.

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14
Q

What do you know about elements in the same group?

A

They have similar properties (reactions) as they have the same number of electrons in the outer shell.

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15
Q

What are periods in the periodic table?

A

The rows in the periodic table.

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16
Q

What are groups in the periodic table?

A

The columns, numbered 1,2,3,4,5,6,7,8/0

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17
Q

Why did Mendeleev swap the order of some elements?

A

So they were in the same group as elements they had similar chemical properties with.

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18
Q

What is crystallization?

A

When a solution is heated until crystals start to form then left to cool until all the water evaporates.

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19
Q

What does distillation do?

A

Separates mixtures of liquids with different boiling points.

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20
Q

What is an isotope?

A

An atom with the same number of protons but a different number of neutrons.

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21
Q

What type of ions do metals form?

A

Positive ions as they lose electrons to get a full outer shell. Cations.

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22
Q

What type of ions do non-metals form?

A

Negative ions as they gain electrons to get a full outer shell. Anions.

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23
Q

What is group 1 called?

A

Alkali metals.

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24
Q

What is group 7 called?

A

Halogens.

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25
Q

What is group 0 called?

A

The noble gases.

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26
Q

State the trend in melting points of the alkali metals.

A

Gets lower as you go down the group.

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27
Q

Explain why the group 1 elements are called alkali metals.

A

They are metals that form alkalis when they react with water.

28
Q

What is a displacement reaction?

A

A reaction in which a more reactive element takes the place of a less reactive element in a compound.

29
Q

Why does the following reaction not proceed: KBr + I2

A

Iodine is less reactive than Bromine so cannot displace it.

30
Q

What are the properties of the transition metals? 5 points.

A
  1. They are good conductors of heat electricity.
  2. They are malleable.
  3. They have high melting points (but mercury is a liquid at room temperature).
  4. They are usually hard and tough.
  5. They have high densities.
31
Q

What is an ion?

A

Atoms with a charge.

32
Q

What is a cation?

A

Metal atom which has lost an electron to therefore, have a positive charge.

33
Q

What is an elements atomic mass?

A

Number of protons + number of neutrons

34
Q

What is an elements atomic number?

A

Number of protons.

35
Q

Who discovered the plum pudding model?

A

J.J. Thomson.

36
Q

Explain the alpha-particle scattering experiment.

A

They fired positively charged atoms at a thin piece of gold foil. Most atoms passed straight through, proving the plum pudding model to be wrong. Some repelled proving the nucleus had a positive charge.

37
Q

Why did Mendeleev leave gaps in his periodic table?

A

To leave spaces for the elements that had not been discovered yet.

38
Q

Why was Mendeleev’s table widely accepted?

A

Mendeleev had predicted the properties of missing elements by leaving gaps. When these elements were discovered they matched his predictions.

39
Q

What would happen if the plum pudding model was proved to be correct in the alpha particle scattering experiment?

A

The positively charged helium nucleus would travel straight through the atom with no reflection as charge would be spread evenly.

40
Q

What happened in the alpha scattering particle experiment that led to a change in the model of the atom?

A

Particles deflected off the foil at an angle which showed the positive charge was concentrated in the middle of the atom. Most particles passed straight through proving the atom to be mostly empty space.

41
Q

What did J.J. Thompson discover?

A

The existence of electrons. This led to the plum pudding model.

42
Q

What was the order of the people who made discoveries of the atom?

A
  • John Dalton
  • J.J. Thompson
  • Ernest Rutherford
  • Neils Bohr
  • James Chadwick
43
Q

What did John Dalton say about the atom?

A

Atoms were indivisible.
Those of the same element were the same. Compounds are combinations of different types of atoms.

44
Q

Do compounds have the same properties as their constitute elements?

A

No.

45
Q

Do mixtures have the same properties as their constitute elements?

A

Yes.

46
Q

What is simple distillation?

A

Used to separate a liquid from it’s solution, by boiling the solution and then condensing the gas in a condenser, so the chemical can be obtained in its liquid form,

47
Q

What is the purpose of the fractionating distillation column?

A

Containing glass beads, helps to separate out the compounds. As it is cold at the top and hot at the bottom, the liquids will condense at different heights of the column.

48
Q

What is chromatography used for?

A

To separate a mixture of substances dissolved in a solvent.

49
Q

What is a solvent?

A

Substance that dissolves the solute.

50
Q

What is a solute?

A

Gets dissolved by the solvent.

51
Q

What is the radius of an atom?

A

0.1nm

52
Q

Compare the boiling points of metals and non-metals.

A

Metals - high
Non-metals - low

53
Q

Compare the appearance of metals and non-metals.

A

Metals - shiny
Non-metals - dull

54
Q

Compare the conductivity of metals and non-metals.

A

Metals - conduct heat and electricity
Non-metals - don’t conduct (exception of graphite)

55
Q

Compare the malleability of metals and non-metals.

A

Metals - malleable
Non-metals - brittle

56
Q

Compare the densities of metals and non-metals.

A

Metals - high density
Non-metals - low density

57
Q

Define miscible/ immiscible.

A

Able to be mixed / unable to mixed.

58
Q

What do the elements in the same period have in common?

A

Number of energy levels.

59
Q

What is the trend in the properties of the noble gases down the group?

A

Higher boiling points down the group as atoms get heavier.

60
Q

What are the properties of noble gases?

A

Unreactive (full outer shell), low boiling points, gases.

61
Q

Compare Group 1 metals with transition metals.

A

Both - shiny when polished, conductors, form ionic compounds with non-metals.
Transition metals - less reactive, harder, higher densities.

62
Q

Why would ordering elements in atomic weight be incorrect?

A

Isotopes aren’t considered.

63
Q

What 4 substances can react with an acid to form a soluble salt?

A

Metal oxide
Metal hydroxide
Metal carbonate
Alkali

64
Q

What is the dish called in the formation of copper sulfate crystals?

A

Evaporating basin

65
Q

Why is chlorine more reactive than iodine?

A

Chlorine’s outer shell electron is closer to the nucleus.
Chlorine has greater attraction for outer shell electrons.
So will gain an electron more easily.

66
Q

Why do the boiling points of the halogens increase down the group?

A

Size of molecules increases.
Increases strength of intermolecular forces.
More energy is needed to overcome these forces.

Chemistry Paper 1 (6 decks)

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