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Chemistry > C1 Atomic Structure > Flashcards

C1 Atomic Structure Flashcards

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1
Q

Element

A

A substance made up of only 1 type of atom

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2
Q

Significance of symbols used in equations

A

They show us what atoms are involved and how they are bonded together

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3
Q

Why mass is conserved in a chemical reaction

A

No new atoms have entered or left the system

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4
Q

Law of conservation of mass

A

Mass cannot be created or destroyed in a chemical reaction

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5
Q

Difference between plum-pudding and nuclear model of atom

A

Plum-pudding model - positive sphere with negative randomly placed in sphere

Nuclear - Central positive tiny nucleus with negative charges

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6
Q

Why model of atom changed overtime

A

Technology advanced

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7
Q

How evidence from scattering experiments changed the model of the atom

A

Alpha scattering led to plum-pudding model replaced with nuclear model

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8
Q

Relative charges and masses of subatomic particles

A

Relative charge

Protons = +1 Neutrons = 0 Electrons = -1

Relative mass

Protons and neutrons = 1

Electrons = 0.0005

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9
Q

Number of protons = atomic number

Number of electrons = atomic number

Number of neutrons = ?

A

Mass number - atomic number

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10
Q

Ion

A

Charged particles that have either lost or gained electrons

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11
Q

Isotope

A

Forms of element that have same number of protons but different numbers of neutrons

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12
Q

How to describe isotopes using atomic model

A

Atoms with same number of protons but different numbers of neutrons

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13
Q

Why ions have a charge

A

Because number of electrons does not equal number of protons

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14
Q

Relative size of atom and its nucleus

A

-10
Atom - diameter 10 m

                                   -15 Nucleus - diameter 10 m
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15
Q

Why chlorine doesn’t have a full mass number

A

Because of isotopes

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16
Q

The maximum number of electrons in the first 3 energy levels

A

First energy level - 2

Second energy level - 8

Third energy level - 18

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17
Q

Mixture

A

A compound made up of 2 or more elements not chemically bonded

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18
Q

Radius of an atom

A

0.1 nanometres

      -14 1 x 10       m
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19
Q

Why is the nucleus a positive charge

A

Because it has protons

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20
Q

Mass of electrons

A

Electrons have no mass

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21
Q

Atomic number

Mass number

A

23 -
Na
11 -

Page 12

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22
Q

Atomic number

A

Tells you how many protons there are

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23
Q

Mass number

A

Tells you total number of protons and neutrons in the atom

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24
Q

How to get number of neutrons

A

Mass number - Atomic number

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25
Q

Do elements consist of atoms with the same atomic number

A

True

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26
Q

What do number of protons in an element decide

A

What type of atom it is

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27
Q

The difference between isotopes

A

Same atomic number but different mass numbers

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28
Q

Example of a pair of isotopes

A

Carbon-12 - 6 neutrons

Carbon-13 - 7 neutrons

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29
Q

Abundances

A

Amounts

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30
Q

Relative atomic mass =

A

Sum of (isotopic abundance x isotopic mass number)
________________________________________________________

           Sum of abundances of all isotopes
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31
Q

Which part of an atom isn’t affected when a bond is made

A

The nuclei

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32
Q

What are compounds represented by

A

Formulas

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33
Q

What does the mixture air contain

A

Mainly nitrogen, oxygen, carbon dioxide, argon

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34
Q

Paper chromotography process

Steps 1-5

A

Draw line near bottom of filter paper

Add a spot of ink to line

Place sheet in beaker of solvent

Make sure ink isn’t touching the solvent

Place lid on top of container

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35
Q

Paper chromotography process

Steps 6-7

A

Solvent seeps up paper carrying ink with it

Each different dye in ink will move up at different rates

Each dye will form a spot in different place - 1 spot per dye in ink

36
Q

Paper chromotography process

8-10

A

If any dyes in the ink are insoluble they will stay on the baseline

When solvent has nearly reached top of paper, take paper out of beaker and leave to dry

The end result is a pattern called a chromatogram

37
Q

Why do you have to use pencil to draw a line near bottom of filter paper

A

Pencil marks are insoluble and won’t dissolve in solvent

38
Q

Why shouldn’t ink touch the solvent

A

Don’t want ink to dissolve into it

39
Q

Why do you need to place lid on top of container

A

To stop solvent from evaporating

40
Q

Methods of separating mixtures

A

Filtration

Crystallisation

Chromotography

Distallation

41
Q

2 ways to separate soluble solids from solutions

A

Evaporation

Crystallisation

42
Q

Evaporation method

A

Pour solution in evaporating dish

Slowly heat solution

Solvent will evaporate and solution becomes more concentrated

Crystals form

Keep heating evaporating dish until all you have left are dry crystals

43
Q

Crystallisation method

Steps 1-3

A

Pour solution into evaporating dish and gently heat solution

Some solvent will evaporate and solution will get more concentrated

Once some solvent evaporates or when you see crystals start to form (point of crystallisation) remove the dish from the heat and leave solution to cool

44
Q

Crystallisation method

Stels 4-6

A

The salt should start to form crystals as it becomes insoluble in cold highly concentrated solution

Filter crystals out of solution and leave them in warm place to dry

45
Q

Distallation

A

Used to separate mixtures which contain liquids

2 types - simple and fractional

46
Q

What is simple distallation and fractional distallation used for

A

Simple distallation - used to separate out solutions

Fractional distallations - used to separate a mixture of liquids

47
Q

Simple distallation process

A

Solution heated

Vapour is cooled, condenses (turns back into a liquid) and is collected

Rest of solution is left behind in the flask

48
Q

Fractional distillation process

Steps 1-4

A

Put mixture in flask

Stick a fractionating column on top then heat it

Different liquids will have different boiling points so will evaporate at different temperatures

The liquid with lowest boiling point evaporates first

49
Q

Fractional distillation process

Steps 4-7

A

When temperature of thermometer matches boiling point of this liquid it will reach top of the column

Liquids with higher boiling points mights also start to evaporate

But the column is cooler towards the top so will only get part of the way up before condensing and run back down towards flask

When the first liquid has been collected raise temperature until the next one reaches the top

50
Q

How would you know what separation technique to use for a given mixture?

A

Dependent on the properties of the mixture components

51
Q

How do the chemical properties of a mixture relate to the chemical it is made from

A

The chemical property of each substance in a mixture does not change

52
Q

How fractional distillation can separate miscible liquids with similar boiling points

A

A mixture of liquids is boiled and the resulting vapors travel up a fractionating column and separate

53
Q

Properties of an element

A

Atomic radius

Electronegativity

Ionization energy

54
Q

Properties of a mixture

A

No fixed composition

No fixed melting points

No fixed boiling points

55
Q

Properties of a compound

A

Pure substance

Fixed melting point

Fixed boiling point

56
Q

John Dalton

A

1803

Described atoms as solid spheres

Said different spheres are made up of different elements

57
Q

J J Thomson

A

1897

Plum pudding model

A ball of positive charge with electrons scattered over it

58
Q

Ernest Rutherford

A

1909

Nuclear model

Tiny positive charged nucleus at the centre, electrons orbit the nucleus

59
Q

Niels bohr

A

1913

Rutherford-bohr model

Positive charged nucleus with electrons surrounding it

60
Q

Erwin Schrodinger

A

1926

Quantum model

Stated electrons don’t move in set paths around the nucleus but in waves

Electrons orbit positive nucleus in waves

61
Q

Ernest Rutherford and his student Ernest Mardon’s experiment

A

Alpha particle scattering experiment

They fired positively charged alpha particles at a thin sheet of gold

They expected particles to pass straight through the sheet or slightly deflected

Some particles went straight through the gold sheet but some were deflected more than expected and a small number were deflected backwards

So this disproved plum pudding model

62
Q

Why did Rutherford expect particles to go straight through sheet

A

Positive charge of atom was thought to be very spread out through the ‘pudding of an atom’

63
Q

Why was the nuclear model atom mostly an empty space

A

A ‘cloud’ of negative electrons surrounds nucleus

64
Q

Proton, electron, neutron,

Order of discovery

A

Electron, proton, neutron (earliest to latest)

Electron - J J Thomson 1897

Proton - Ernest Rutherford early 20th century

Neutron - James Chadwick 1932

65
Q

What are the energy levels which electrons orbit called

A

Shells

66
Q

How many electrons are allowed in each shell

A

2 - 1st shell

8 - 2nd shell

8 - 3rd shell

67
Q

Electronic structure of Nitrogen

Nitrogen has atomic number 7 (so 7 protons)

A

The first shell can only take 2 electrons and the 2nd takes maximum of 8

So electronic structure of nitrogen would be 2, 5

68
Q

Electronic structure of magnesium

Atomic number 12 (so has 12 protons so it has 12 electrons)

A

1st shell takes 2, 2nd shell takes 8, 3rd shell takes 8

2, 8, 2

69
Q

Atom

A

Smallest part of an element

70
Q

What do elements in same group have in common

A

Same chemical properties

71
Q

Reactants

Products

A

Reactants - substances you start with

Products - the new substances made in chemical reaction

72
Q

Hydrogen + oxygen ———-> water

Reactants?

Products?

A

Reactants - hydrogen + oxygen

Products - water

73
Q

Aqueous solution (aq)

A

Substances dissolved in water

74
Q

Precipitate

A

Solid formed in reaction between 2 solutions

75
Q

How did Niels Bohr discover electrons 1914

A

He noticed light given out when atoms were heated had specific amounts of energy

76
Q

Why does sand become residue rocksalt separation technique

A

Sand grains are insoluble so cannot pass through filter paper

77
Q

Why does yellow dye move further up the paper chromotogram technique

A

The yellow dye is more soluble in water than the red dye

78
Q

Molecules

A

Pairs of atoms

79
Q

Filtration use

A

Separates an insoluble solid from a liquid

80
Q

Crystallisation use

A

Separates a soluble solid from a liquid

81
Q

Simple distallation use

A

Separates a liquid from a dissolved solid

82
Q

Fractional distallation use

A

Separates two or more liquids which have different boiling points

83
Q

Chromotography use

A

Separates two or more dissolved solids from a solution

84
Q

Reading on thermometer during simple distallation

A

100°C

85
Q

Diamater of indium atom in metres

A

-10
3.10 x 10 m

86
Q

Diamater of indium atom in metres

A

-10
3.10 x 10 m

Chemistry (10 decks)

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