5.1.1 - A Simple Model Of The Atom, Symbols, Relative Atomic Mass, Electronic Charge And Isotopes Flashcards

1
Q

What are all substances made of

A

Atoms

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2
Q

What is an atom

A

The smallest part of an element that can exist

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3
Q

What are atoms of each element represented by

A

A chemical symbol (eg = Na or O)

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4
Q

How are compounds formed

A

From elements by chemical reactions

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5
Q

What do chemical reactions always involve

A
  • The formation of one or more new substances
  • a detectable energy change
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6
Q

What do compounds contain

A

Two or more elements chemically combined in fixed proportions

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7
Q

How are compounds represented

A

By formulae using the symbols of the atoms from which they were formed

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8
Q

What’s the only way compounds can be separated into elements

A

By chemical reactions

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9
Q

What does a micture consist of

A

Two or more elements/compounds not chemically combined together

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10
Q

What are the chemical proportions of each substance in a mixture like

A

Unchanged

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11
Q

How can mixtures be separated + examples

A

By physical processes
Eg = filtration, crystallisation, simple distillation, fractional distillation and chromotography

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12
Q

What do the physical processes for mixtures being separated not involve

A

Chemical reactions
No new substances are made

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13
Q

What does filtration separate

A

An insoluble solid from a liquid

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14
Q

What is filtration useful for separating

A

Separating sand from a mixture of sand and water OR an excess reactant from a reaction mixture

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15
Q

Why does filtration work

A

The filter paper has tiny holes/pores in it - they’re large enough to let small molecules + dissolved ions through but not larger particles of the un dissolved solid

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16
Q

Steps to filtration

A

1) one beaker has a micture of solid and liquid, the other has a funnel with filter paper in it
2) the solid and liquid mixtures poured into the filter funnel
3) the liquid drips through the filter paper but the solid particles are caught in the filter paper

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17
Q

What is crystallisation used for

A

To produce solid crystals from a solution

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18
Q

How does crystallisation work

A

When the solutions warmed, so,e of the solvent evaporates leaving crystals behind

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19
Q

Example of when crystallisation is used

A

To obtain copper Sulfate crystals from copper Sulfate solution

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20
Q

Steps to crystallisation

A

1) a solutions placed in an evaporating basin and heated with a Bunsen burner
2) the volume of the solution has decarsed because some waters evaporated - solid particles begin to form in the basin
3) all the water evaporates and leaves solid crystals behind

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21
Q

What’s simple distillation used for

A

To separate a solvent from a solution

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22
Q

What’s simple distillation useful for

A

For producing pure water from seawater

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23
Q

How does simple distillation work

A
  • The dissolved solute has a much higher boiling point than the solvent
  • when the solutions heated, solvent vapour leaves the solution
  • it moves away and is cooled/condensed
  • the remaining solution becomes more concentrated as the amount of solvent in it decreases
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24
Q

Steps to simple distillation

A

1) salty waters heated
2) the water vapour cools in the condenser and drips into a beaker
3)the waters condensed and is now in the beaker, the salt stays behind

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25
Q

What’s fractional distillation used to separate

A

To separate different liquids from a mixture of liquids

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26
Q

What’s fractional distillation useful for separating

A

Ethanol from a mixture of ethanol and water AND separating different fractions from crude oil

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27
Q

Why does fractional distillation work

A

Because the different liquids have different boiling points

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28
Q

How does fractional distillation work

A

When the mixtures heated -
1) vapour rises through a column which is hot at the bottom and cooler at the top
2) vapours condense when they reach the part of the column that’s below the temperature of their boiling point
3) each liquids led away from the column

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29
Q

What are the two ways to obtaining different liquids from the column

A

1) by collected different liquids from different parts of the column - the substance with the lowest boiling points collected at the top of the column
2) by continuing to heat the mixture to increase the temperatures in the column - the substance with the lowest boiling points collected first

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30
Q

Steps to fractional distillation

A

1) water and ethanol solution is heated
2) the ethanols evaporates first, cools and then condenses
3) the water left evaporates cools and then condenses

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31
Q

What does Papier chromatography separate

A

Mixtures of soluble substances - often coloured substances (eg = food colourings, inks, dyes or plant pigments)

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32
Q

What are the two phases in chromatography

A
  • stationary phase = paper
  • mobile phase = the solvent
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33
Q

What does a pure substance produce in chromatography

A

One spot

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34
Q

What does an impure substance produce in chromatography

A

Two or more spots

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35
Q

How do you know if two substances are likely the same in chromatography

A
  • if they produce the same number of spots and they’re the same colour
  • if the spots travel the same distance up the paper
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36
Q

What may lead to a scientific model being changed/replaced

A

New experimental evidence

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37
Q

What were atoms thought to be before the discovery of the electron + by who

A

Tiny spheres that couldn’t be divided
- by john dalton at the start of the 19th century

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38
Q

What discovery led to the plum pudding model

A

Discovery of the electron

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39
Q

Who + what year was the plum pudding model

A

1897 - J.J Thompson

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40
Q

What did the plum pudding model suggest

A

That the atoms a ball of positive charge with negative electrons embedded into it

41
Q

Who + when was the alpha particle experiment

A

1909 - Ernest Rutherford

42
Q

What conclusion did the alpha particle scattering experiment lead to

A
  • The mass of an atom was concentrated/positively charged at the centre (nucleus)
  • a ‘cloud’ of negative electrons surround the nucleus (most of the atoms empty space)
43
Q

What model replaced the plum pudding

A

Alpha particle scattering experiment

44
Q

What did the particles do in the alpha particle experiment

A
  • most when straight through the gold sheet
  • some were deflected at large angles
  • a small number were deflected backwards
45
Q

What did Niels bohr suggest about the atom

A

That the electrons orbit the nucleus at specific distances

46
Q

What did later experiments lead to

A

The positive charge of any nucleus could be divided into smaller particles that have the same positive charge - the proton

47
Q

What did James Chadwick show the existence of + when

A

The neutrons within the nucleus about 20 years after the nucleus became an accepted scientific idea

48
Q

The relative charges of
1) proton
2) electron
3) neutron

A

1) +1
2) -1
3) 0

49
Q

What’s the number of electrons equal to

A

The number of protons

50
Q

Do atoms have an overall electrical charge

51
Q

What is the atomic number

A

The number of protons in an atom

52
Q

What do all atoms of a particular element have

A

The same number of protons

53
Q

What is an atoms radius

A

0.1 nm (1x10^-10 nm)

54
Q

What is the nucleus radius

A

1 x 10^-14 m)

55
Q

Where’s almost all the mass in an atom

A

The nucleus

56
Q

Relative masses of
1) proton
2) neutron
3) electron

A

1) 1
2) 1
3) very small (1/2000)

57
Q

What is the sum of protons and neutrons in an atom

A

The mass number

58
Q

What’s an isotope

A

The same elements each with a different number of neutrons

59
Q

What is the top number

A

The mass number

60
Q

What’s the bottom number

A

The atomic number

61
Q

How to find out how many neutrons are in an element

A

Atomic number - mass number

62
Q

What’s the relative atomic mass

A

An average mass that takes into account the different masses/abundances of all the isotopes of the element

63
Q

How to find the relative atomic mass

A

Sum of (isotope abundance x isotope mass number) / sum of abundances of all the isotopes

64
Q

What do electrons move around the nucleus in

A

In electron shells

65
Q

How were elements originally arranged

A

By their atomic weight

66
Q

What was bad about elements being in order of atomic weight

A

Periodic tables weren’t complete and many elements were placed in the wrong group

67
Q

What did Mendeleev do with the periodic table in 1869

A
  • he left gaps for elements that hadn’t been discovered yet
  • put the elements in order of atomic weht but moved them round if their properties meant it should be changed
68
Q

What happened with the gaps he left in the table

A

Elements with properties predicted by him were discovered and they filled i the gaps

69
Q

What did the knowledge of isotopes explain

A

Why the the order based on atomic weight wasnt always correct

70
Q

What are metals

A

Elements that react to form positive ions

71
Q

What are non-metals

A

Elements that dont form positive ions

72
Q

Physical properties of a metal

A
  • strong but malleable
  • good at conducting heat/electricity
  • high boiling/melting points
73
Q

Physical properties of non-metals

A
  • dull
  • brittle
  • aren’t always solids at room temperature
  • don’t conduct electricity
  • lower density
74
Q

Why do non-metals have different properties to metals

A

They don’t have metallic bonding

75
Q

How do atoms react to form a full outer shell

A

By losing, gaining or sharing electrons

76
Q

Why do some metals feel a weaker attraction to their nucleus

A

They don’t have many electrons to remove OR they’re far away from the nucleus

77
Q

What does a weaker attraction to the nucleus mean (to do with energy)

A

Not much energys needed to remove the electrons

78
Q

Why is forming positive ions for non-metals difficult

A

They have lots of electrons to remove to get a full outer shell OR they’re outer electrons are close to their nucleus so they feel a strong attraction to it

79
Q

What is the name for group 0

A

Noble gases

80
Q

Why are group 0 unreactive + don’t form molecules easily

A

They have full outer shells

81
Q

What happens to the boiling point as you go down the noble gases

82
Q

Why do the noble gases increase in boiling point

A

An increase in the number of electrons leads to greater intermolecular forces

83
Q

Order if noble gases from smallest boiling point to highest

A

Helium
Neon
Argon
Krypton
Xenon
Radon

84
Q

What are group 1 elements called

A

The alkali metals

85
Q

What happens as you go down the alkali metals

A

Increases reactivity
Lower melting/boiling points
Higher relative atomic mass

86
Q

Why are the alkali metals very reactive

A

They have one outer electrons to remove in their outer shell

87
Q

Why does tye reactivity increase in the alkali metals

A

The outer electrons more easily lost because the attraction between the nucleus and electron gets weaker - electrons further away from nucleus as you go down group

88
Q

Properties of alkali metals

A

Soft
Low density

89
Q

What happens when group 1 metals react with water

A
  • react vigoursly to produce hydrogen gas and metal hydroxides
  • as you go down the group the reactions get more vigorous
  • as yiu go down the group the amount of energy given out increases
90
Q

What happens when group 1 reacts with chlorine

A
  • they react vigorously when heated in chlorine gas to form white metal chloride salts
  • as you go down the group the reactions get more gets more vigorous
91
Q

What happens when group 1 reacts with oxygen

A
  • they form a metal oxide
92
Q

What are group 7 known as

93
Q

Why do the halogens have similar reactions

A

They all have seven electrons on their outer shell

94
Q

What happens as you go down the halogens

A
  • less reactive
  • higher melting/boiling points
  • higher relative atomic mass
95
Q

Why do the halogens become less reactive

A

It’s harder to gain a full outer shell because the outer shells become further away from the nucleus

96
Q

How can halogens get a full outer shell

A

By sharing electrons by covalent bonding with other non-metals

97
Q

What do the compounds that are formed when halogens react with the non-metals have

A

Simple molecular structures

98
Q

In ionic bonding with halogens and metals what do the compounds formed have

A

Ionic structures

99
Q

What can a displacement reaction occur between

A

A more reactive halogen and the salt of a less reactive one