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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

Compounds contain 2 or more elements chemically combined in…

A

Fixed proportions

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2
Q

What is an ion?

A

A charged particle formed when an atom (or group of atoms) loses or gains electrons.

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3
Q

What do state symbols show?

A

The physical state of a substance

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4
Q

What are the 4 state symbols?

A

Solid = (s)
Liquid = (l)
Gas = (g)
Aqueous solution = (aq)

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5
Q

How are aqueous solutions formed?

A

When a substance dissolves in water

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6
Q

What is a pure substance?

A

A substance consisting of only one element or one compound

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7
Q

What are the 5 physical separation techniques (used to separate mixtures)?

A
  • filtration
  • crystallisation
  • simple distillation
  • fractional distillation
  • chromatography
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8
Q

What does insoluble mean?

A

Unable to dissolve in a particular solvent

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9
Q

What is a solution?

A

Mixture formed by a solute and a solvent

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10
Q

What is a solvent?

A

The liquid a solute dissolves in to form a solution

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11
Q

What is a solute?

A

The dissolved substance in a solution

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12
Q

What is filtration used for?

A

To separate an in insoluble solid from a liquid

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13
Q

What equipment is needed to carry out filtration?

A
  • beaker (containing a mixture of solid and liquid)
  • conical flask
  • filter paper
  • filter funnel
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14
Q

What is the name for a liquid that has passed through a filter (in filtration)?

A

Filtrate

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15
Q

What is crystallisation used for?

A

To separate a soluble solid from a liquid

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16
Q

What does soluble mean?

A

Able to dissolve in a particular solvent

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17
Q

What is the process of crystallisation?

A

allowing the solvent to evaporate slowly by gently heating the solution to leave behind solid crystals

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18
Q

What are the steps in carrying out crystallisation?

A
  1. Place solution in evaporating basin over a Bunsen burner/boiling water bath
  2. Gently heat solution until all solvent has evaporated, leaving solid crystals behind
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19
Q

What equipment is needed to carry out crystallisation?

A
  • Bunsen burner/boiling water bath (heat)
  • evaporating basin
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20
Q

What is simple distillation used for?

A

To separate a solvent from a solution

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21
Q

What are the 2 stages of simple distillation?

A
  1. evaporate the liquid into vapour by heating the solution
  2. condense the vapour back to a liquid by cooling
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22
Q

What equipment/apparatus is needed to carry out simple distillation?

A
  • flask
  • Bunsen burner
  • thermometer
  • condenser
  • beaker
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23
Q

What are the steps in carrying out simple distillation?

A
  1. Heat the solution (in flask) using Bunsen burner until it boils/all the liquid has evaporated and formed vapour
  2. Vapour rises up glass tube and thermometer reading increases
  3. Vapour passes through condenser and is cooled back to liquid
  4. Liquid is collected in beaker
  5. Left with solid crystals in flask and liquid in beaker
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24
Q

How does the condenser work in simple distillation?

A

condenser surrounds glass tube and keeps it cool as cold water continuously runs through condenser

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25
Q

What is fractional distillation used for?

A

To separate a mixture of different liquids into fractions

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26
Q

In fractional distillation, what must the different liquids being separated have?

A

Different boiling points

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27
Q

What equipment/apparatus is needed to carry out fractional distillation?

A
  • a flask containing a mixture of different liquids
  • fractionating column
  • thermometer
  • heater
  • condenser
  • beakers
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28
Q

What is a fractionating column?

A

tall column full of small glass beads/rods that is cooler at the top than at the bottom

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29
Q

What examples of mixtures is fractional distillation useful for separating?

A
  • Ethanol and water
  • crude oil into fractions
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30
Q

What is paper chromatography used for?

A

To separate mixtures of soluble substances

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31
Q

What equipment is needed to carry out paper chromatography?

A
  • chromatography paper
  • pencil line
  • solvent
  • ink/dye dots
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32
Q

What is the paper called in paper chromatography?

A

The stationary phase

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33
Q

What is the solvent called in paper chromatography?

A

The mobile phase

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34
Q

What will a pure substance produce on a chromatogram?

A

One spot

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35
Q

What will an impure substance/mixture produce on a chromatogram?

A

Two or more spots

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36
Q

Why is the starting line in paper chromatography drawn with a pencil?

A

If a pen was used, the pen ink would dissolve in the solvent and move up the paper

37
Q

Who created the plum pudding model?

A

JJ Thompson

38
Q

What conclusions were drawn from the alpha particle scattering experiment?

A
  • most of an atom is empty space
  • the mass of an atom is concentrated at its centre (nucleus)
  • the nucleus is positively charged
39
Q

What replaced the plum pudding model after the alpha particle scattering experiment?

A

The nuclear model

40
Q

Who carried out the alpha particle scattering experiment and created the nuclear model?

A

Ernest Rutherford

41
Q

Who adapted the nuclear model by suggesting that electrons orbit the nucleus at specific distances?

A

Niels Bohr

42
Q

Which 2 other discoveries about the atom were made after Niels Bohr?

A
  • the nucleus contains small positively charged particles - protons
  • the existence of neutrons within the nucleus
43
Q

Who provided the evidence to show the existence of neutrons?

A

James Chadwick

44
Q

What is the relative charge of a proton?

A

+1

45
Q

What is the relative charge of a neutron?

A

0

46
Q

What is the relative charge of an electron?

A

-1

47
Q

What is the radius of an atom?

A

0.1 nm or 1x10-10m

48
Q

What is the radius of a nucleus?

A

1x10-14m

49
Q

What is the relative mass of a proton?

A

1

50
Q

What is the relative mass of a neutron?

A

1

51
Q

What is the relative mass of an electron?

A

Very small

52
Q

What is the equation to calculate relative atomic mass?

A

(Mass number of isotope 1 x percentage abundance of isotope 1)+(mass number of isotope 2 x percentage abundance of isotope 2)/100

53
Q

How did the early periodic tables attempt to arrange the elements?

A

By atomic weight (relative atomic mass)

54
Q

Who developed the first modern Periodic-Table?

A

Dmitri Mendeleev

55
Q

What type of element reacts to form positive ions?

A

Metals

56
Q

What type of element reacts to form negative ions?

A

non-metals

57
Q

What is the atomic number?

A

number of protons/electrons in an element

58
Q

What is the mass number?

A

Total number of protons and neutrons

59
Q

How are the elements in the periodic table arranged?

A

By atomic number

60
Q

What are isotopes?

A

Atoms of the same element with different numbers of neutrons

61
Q

What does the group number of an element represent?

A

Number of electrons in its outer shell

62
Q

What are the 5 properties of a typical non metal (when solid)?

A
  • poor conductivity electricity
  • poor conductor heat
  • dull
  • low density
  • brittle
63
Q

What are the 5 properties of a typical metal (when solid)?

A
  • good conductor electricity
  • good conductor heat
  • shiny
  • high density
  • malleable
64
Q

What are the elements in group 0 called?

A

Noble gases

65
Q

Why are the noble gases unreactive?

A

all have a full outer shell

66
Q

Why are the noble gases, gases at room temperature?

A

All have low boiling points under room temperature

67
Q

What do the boiling points of the noble gases increase with?

A

Increasing relative atomic mass (going down the group)

68
Q

What are the elements in group 1 called?

A

Alkali metals

69
Q

How many electrons do all group 1 elements have in their outer shell?

A

1

70
Q

What does the reaction between an alkali metal and oxygen in the air produce?

A

Metal oxides

71
Q

What are 4 properties of the alkali metals?

A
  • soft (can be cut with a knife)
  • relatively low melting points
  • low densities
  • reactive
72
Q

What does the reaction between an alkali metal and chlorine produce?

A

Metal chlorides

73
Q

What does the reaction between an alkali metal and water produce?

A

Metal hydroxide and hydrogen (compounds that dissolve in water to produce alkaline solutions)

74
Q

What happens when a group 1 element reacts?

A

each of its atoms loses its outer electron to form a positively charged ion

75
Q

Why does the reactivity of group 1 elements increase going down the group?

A

Going down group 1:
- outer electron becomes further from nucleus
- attraction between nucleus and outer electron decreases
- outer electron lost more easily

76
Q

How do group 1 metals react with chlorine and water?

A

Vigorously

77
Q

What are the 3 trends for alkali metals as you go down group 1?

A
  • increasing reactivity
  • lower melting and boiling points
  • higher relative atomic mass
78
Q

What are the group 7 elements called?

A

The halogens

79
Q

Why do the elements in group 7 all have similar reactions?

A

All have 7 electrons in outer shell

80
Q

What do all group 7 elements form and consist of?

A

Molecules made up of 2 atoms covalently bonded

81
Q

What are the 3 trends for the halogens going down group 7?

A
  • decreasing reactivity
  • higher melting and boiling points
  • higher relative atomic mass
82
Q

What do group 7 elements form when they react with other non metal elements?

A

Covalent compounds

83
Q

What do group 7 elements form when they react with metals?

A

Ionic compounds

84
Q

Why does the reactivity of the halogens decrease going down the group?

A
  • outer shell is further from nucleus
  • harder to gain an electron
85
Q

How can a displacement reaction occur between 2 halogens?

A

More reactive halogen can displace a less reactive halogen from an aqueous solution of its salt

86
Q

Where are the transition metals found on the periodic table?

A

middle

87
Q

What are the 6 properties of transition metals that you would expect of a ’typical metal’?

A
  • hard
  • strong
  • shiny
  • high density
  • good conductors
  • relatively low reactivity
88
Q

What are the 3 special properties of transition metals?

A
  • can form ions with different charges
  • form coloured compounds
  • good catalysts

Chemistry Paper 1 (6 decks)

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