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Chemistry > Unit 1 - Atomic Structure And Periodic Table > Flashcards

Unit 1 - Atomic Structure And Periodic Table Flashcards

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1
Q

What is isotopes

A

Different form of the same element same number of protons but different number of neutrons

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2
Q

Relative mass of neutron

A

1

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3
Q

What is a mixture

A

Two or more elements or compounds mixed together

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4
Q

What is filtration

A

Separates insoluble solids from liquids

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5
Q

What is distillation

A

Separate solutions

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6
Q

What did jj Thompson come up with

A

Discovered electron , plum pudding model

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7
Q

What did John dalton discover

A

Atoms

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8
Q

What did Rutherford discover

A

Came up with alpha and beta particles and nucleus model

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9
Q

What did Neil Bohr discover

A

Suggested that all atoms were contained in shells

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10
Q

Who first developed the periodic table

A

Mendeleev

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11
Q

Properties of transition metals

A

Good conductors of heat and electricity
High density
High melting point
Form ions with different charges

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12
Q

What metals are in group 1

A

Alkali

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13
Q

Properties of alkali metals (group 1)

A

Low density, increasing reactivity as you go down, low melting and boiling pints

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14
Q

What is group 7 also known as

A

Halogens

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15
Q

Properties of halogens

A

Less reactive as you go down, high belting and boiling points

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16
Q

What did Chadwick discover

A

The neutron and isotopes have the same number of proteins and electrons but with different number of neutrons

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17
Q

What is a mass number

A

No of proteins and neutrons

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18
Q

Why do alkaline batteries stop working

A

A reactant is used up

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19
Q

Why can alkaline batteries not be recharged

A

The reaction is not reversible

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20
Q

Why did Mendeleev periodic table become more widely accepted

A

-Mendeleev had predicted properties of missing elements
- elements were discovered filled gaps
- properties of these elements matched his predictions

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21
Q

What is the modern name for the atomic weight

A

Relative atomic mass

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22
Q

What do you see when sodium reacts with chlorine

A

-Flame
-white solid forms

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23
Q

What ion do all acids produce in aqueous solutions

A

H+

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24
Q

Explain why carbon nanotubes conduct electricity

A

Contain delocalised electrons
So electrons can move through nanotube

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25
Q

Relative mass of neutron

A

1

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26
Q

Relative mass of proton

A

1

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27
Q

Why is the mass number different in two isotopes

A

Different number of neutrons

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28
Q

Relative mass of electron

A

0.0005

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29
Q

Explain why the alpha particle scattering experiment led to a change in model of the atom from the plum pudding model

A

-most alpha particles passes through gold foil
-so most of atom is empty space
-some particles were deflected
-so atom has a positively charged nucleus

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30
Q

Limitation of using a dot and cross diagram

A

Only 2 dimensional

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31
Q

Explain why ammonia has a low boiling point

A

-simple molecular structure
-has weak intermolecular forces
-so little energy needed to overcome the force

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32
Q

Control variables in electrolysis experiment

A

-temperature of solution
-size of electrode
-distance between electrodes

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33
Q

Hydrogen fuels can be used to power steam trains. Suggest why

A
  • hydrogen is oxidised to produce water
  • water is produced as steam
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34
Q

Explain why a mixture is used as the electrolyte

A

-Mixture has low melting point
-so less energy needed

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35
Q

Why must the positive electrode be continually replaced

A

-the electrode could react with oxygen
-the electrode is carbon
-so carbon dioxide is produced

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36
Q

Explain why sodium chloride solution cannot be used as the electrolyte to produce sodium metal

A

Hydrogen gas would be produced instead of sodium
Because sodium is more reactive than hydrogen

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37
Q

Why should hydrogen be burned off

A

To prevent it escaping into air
Because hydrogen is explosive

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38
Q

How could student separate insoluble silver iodide from mixture at end of reaction

A

Filtration

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39
Q

Why are reactions why a high atom economy used in industry

A

For economic reasons

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40
Q

Describe change Bohr made to nuclear model

A

Electrons orbit nucleus
And electrons are at specific distances from nucleus

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41
Q

Why did Mendeleev reversed order of some pairs

A

So properties matched rest of group

42
Q

Advantages of using hydrogen fuel cells

A

No toxic chemicals to dispose at end of cells life
Takes less time to refuel

43
Q

Disadvantages of the simple particle model for hydrogen gas

A

-Only two dimensional
-does not show the movement of particles

44
Q

Why should halogen gas experiment be done in a fume cupboard

A

Halogen is toxic

45
Q

Why does reactivity decrease as you go down the halogen group

A

The outer shell becomes further from the nucleus
So nucleus has less attraction for outer shell
So electron is gained less easily

46
Q

Why is burette used in the RPA

A

Can add drop by drop
More accurate than measuring cyclindor

47
Q

What is an element

A

Substance that is made up of only one type of atom

48
Q

Roughly how many different elements are there

A

100

49
Q

What is a compound

A

A substance made from more than one type of element chemically bonded together

50
Q

How are compounds represented

A

combining the chemical symbols of the 2 elements (Na and O) to create the chemical formula Na2O.

51
Q

What is a mixture

A

Contains two or more substances not chemically bonded together

52
Q

Does the properties of each substance in a mixture change

A

Being part of mixture doesn’t change the chemical properties of the substances that are in it

53
Q

5 processes that can be used to separate mixtures

A

Filtration.
Crystallisation.
Paper Chromatography.
Simple Distillation.
Fractional Distillation.

54
Q

What can crystallisation be used to separate

A

Used to dissolve a soluble solid from a liquid

55
Q

Process of simple distillation

A

Place our solution with our dissolved solid into the flask, heat the solution with a Bunsen burner. Heat the solution until it boils. The liquid starts to evaporate turning into a vapour. Vapour rises up the glass tube the flask into the condenser (condenser is cold as a result of cold tap water circulating around it). This cause the vapour to condense turning back to a liquid. We collect the liquid in a beaker and left with crystals in the flask.

56
Q

Ways to used simple distillation in real life

A

Can be used to make drinking water from sea water

57
Q

Disadvantage of simple distillation

A

Great amount of energy is required for simple distillation

58
Q

What is simple distillation used to separate

A

A solvent from a solution

59
Q

What is filtration used to separate

A

Seperates an insoluble solid from a liquid

60
Q

Process of filtration

A

Pouring our mixture into the filter paper, the solid material cannot pass through the paper so it’s trapped.

61
Q

Process of crystallisation

A

Leave the solution for a few days for the solution to evaporate. This will leave behind solid crystals

62
Q

How do you make crystallisation happen faster and a disadvantage of doing it

A

By gently heating our solution to evaporate the water. However certain chemicals will break down if we heat them

63
Q

Example of filtration (RPA)

A

Can be used to separate copper oxide from sulphuric acid

64
Q

Example of crystallisation in real life

A

Crystallisation of water to form ice cubes and snow

65
Q

What does paper chromatography allow us to do

A

Separate substances based on their different solubilities

66
Q

Process of paper chromatography

A

Draw a pencil line near the bottom, we put a dot of as many colours we can fit on our pencil line. Place bottom of paper into a solvent. The solvent will rise up the paper and carry the ink up with it

67
Q

What phase do we call the paper in paper chromatography

A

The stationary phase because the paper does not move

68
Q

What phase do we call the solvent in paper chromatography

A

The mobile phase because the solvent moves

69
Q

What will a pure compound produce in photo chromatography

A

A single spot in any solvent

70
Q

What will the compounds in a mixture look like in photo chromatography

A

Will separate into different spots depending on the solvent

71
Q

Why do we draw our starting line for photo chromatography in pencil

A

If we drew the line in pen, the ink could dissolve in the solvent and move up the paper

72
Q

What is required in fractional distillation in the mixture of solutions

A

That they have different boiling points then it will work

73
Q

What does fractional distillation separate

A

Two liquids

74
Q

Process of fractional distillation

A

Heat our mixture, both liquids will start to evaporate but the one with the lower boiling point will evaporate easier. Vapours move up the fractionating column, they then condense and drip back into flask to evaporate again. This repeated process will increase amount of the lower boiling point chemical in fractionating column. The lower boiling point chemical will then mostly be the one being collected in the beaker

75
Q

Disadvantages of fractional distillation

A

Won’t be useful for separating large volumes of liquid, might need to carry out several round of fractional distillation if boiling points are close together

76
Q

Which particles have the same relative mass

A

Proton and neutron

77
Q

One reason why platinum may be used for jewellery

A

Un reactive

78
Q

Observations when sodium is added to water

A

Bubbles, moves around, catches fire

79
Q

What may lead to a scientific model being changed

A

New experimental evidence

80
Q

What is the plum pudding model

A

Positive ball of charge with negative electrons

81
Q

What is the alpha scattering experiment

A

Fired alpha particles at a thin layer of gold foil

82
Q

What did scientists discover by the alpha scattering model

A

-Most of alpha particles went straight through the foil therefore atoms are mainly empty space
-some alpha particles were deflected so the centre of the atom must have a positive charge
-because some alpha particles bounced back the mass of the atom must be concentrated in the centre

83
Q

Differences between plum pudding model and nuclear model

A

-nuclear model have mainly empty spaces however plum pudding has none
-nuclear model electrons orbit nucleus however plum pudding model electrons are embedded in the mass of positive charge

84
Q

Radius of an atom

A

0.1 nm or 0.0000000001 or 1 × 10 -10 m)

85
Q

Radius of a nucleus

A

1 × 10-14 m

86
Q

Relative the size of atoms to objects that can be seen in real life

A

If the nucleus were the size of a blueberry, the atom would be about the size of a football stadium

87
Q

How to calculate relative atomic mass

A

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

88
Q

How are elements arranged in the periodic table

A

In order of increasing atomic number

89
Q

Problems with the early periodic table

A

Early periodic tables were incomplete, since many elements were unknown.

90
Q

Physical properties of metals

A

Shiny , high melting points, good conductors of electricity, good conductors of heat, high density, malleable

91
Q

What does malleable mean

A

Capable of being hammered or pressed into a new shape without being likely to break or return to the original shape

92
Q

Properties of non metals

A

Dull, low melting points, poor conductors of electricity, poor conductors of heat, low density, Brittle

93
Q

What does brittle mean

A

Easily broken

94
Q

Describe the trend in boiling point going down group 0

A

Boiling point increases

95
Q

How quick does alkali metals react with oxygen

A

The further down the group the quicker it reacts

96
Q

What happens when alkali metals react with water

A

Alkaline solution produced
Gas being produced
Bubbles
Fizzing

97
Q

Name of process when an acid and alkali react

A

Neutralisation

98
Q

Litmus paper is an example of a what?

A

Indicator

99
Q

Which ions do all acids produce in aqueous solution

A

H plus

100
Q

Why are alloys harder than pure metals

A

Atoms are different sizes, this distorts layers, so layers can’t slide over each other as easily as a pure metal

101
Q

Why is rubidium more reactive than potassium

A

Outer shell further from nucleus
So less electrostatic attraction between nucleus and outer shell
So electrons are more easily lost

Chemistry (7 decks)

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