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Chemistry- AQA- GCSE > Yr9 recap test > Flashcards

Yr9 recap test Flashcards

1
Q

What did the discovery of the electron lead to?

A

The plum pudding model

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2
Q

What did the plum pudding model suggest about atoms?

A

That the atom was a ball of positive charge with negative electrons embedded in it

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3
Q

What did the results from the Rutherford and Marsden’s alpha scattering experiments lead to?

A

The plum-pudding model being replaced by the nuclear model.

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4
Q

In the nuclear atom model, what is the centre of the atom called?

A

The nucleus

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5
Q

What did the ‘alpha scattering’ experiment show?

A

. That all the mass of the atom was in the nucleus
. That all the positive charge of the atom was in the nucleus

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6
Q

How are electrons placed in the nuclear model?

A

The electrons were thought to orbit the nucleus, like planets around the sun.

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7
Q

What happened to most of the alpha particles in the ‘alpha scattering’ experiment? What did it prove?

A

Most of the alpha particles directed at thin gold foil passed through showing that
that all the mass of the atom was in the nucleus.

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8
Q

What happened to a few of the alpha particles in the ‘alpha scattering experiment’? What did it prove?

A

A few alpha particles were deflected or bounced back, suggesting the positive charge was concentrated at the
centre of each gold atom.

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9
Q

How did Neils Bohr adapted the nuclear model?

A

By suggesting that electrons orbit the
nucleus at specific distances

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10
Q

Where are electrons on the Bohr model?

A

The electrons are on energy levels or shells

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11
Q

What did later experiments (after Bohr) lead to?

A

The idea that the positive charge of any nucleus could be subdivided into a whole
number of smaller particles, each particle having the same amount of positive charge. The name proton was
given to these particles.

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12
Q

What did the experimental work of James Chadwick provide the evidence to show?

A

The existence of neutrons within the
nucleus.

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13
Q

How long after the nucleus was discovered was neutrons discovered?

A

About 20 years after the nucleus became an accepted scientific idea.

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14
Q

What did the discovery of neutrons help explain?

A

The existence of isotopes

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15
Q

What is the nucleus of the atom made up of?

A

Protons and neutrons

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16
Q

What orbits around the nucleus of an atom?

A

Electrons

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17
Q

In an atom what is the number of electrons equal to?

A

The number of protons in the
nucleus.

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18
Q

Do atoms have an overall electric charge?

A

NO

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19
Q

What do all atoms of a particular element have?

A

The same number of protons

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20
Q

Where is most of the mass of an atom

A

The nucleus

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21
Q

What is an atom’s mass number?

A

The total number of protons and neutrons in an atom

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22
Q

What is the radius of an atom?

A

0.1 nm (1x 10-10 m)

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23
Q

What is the radius of the nucleus of an atom?

A

1/10 000 of that of the atom (about 1 x 10-14 m)

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24
Q

What is the atomic number of an element?

A

The number of protons in an atom

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25
Q

How are elements arranged in the modern periodic table.

A

In order of their atomic number (proton number)

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26
Q

How do you work out the number of neutrons in an atom?

A

Subtract the atomic number from the mass number

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27
Q

What are isotopes?

A

Atoms of the same element can have different numbers of neutrons

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28
Q

Do isotopes of an element have the same chemical properties

A

YES because they have the same electronic structure.

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29
Q

What is the relative atomic mass?

A

An average value that takes account of
the abundance of the isotopes of the element.

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30
Q

What is the relative atomic mass calculation

A
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31
Q

What do elements in the same group in the periodic table have?

A

The same number of electrons in the highest energy levels (outer electrons) and this gives them similar properties.

32
Q

What are the elements in Group 0 of the periodic table called?

A

The noble gasses

33
Q

Why are group 0 elements inert?

A

Their atoms have a stable arrangement of electrons.

34
Q

How are elements in the periodic table arranged?

A

In order of atomic number

35
Q

What are columns in the periodic table known as?

A

Groups

36
Q

How did the periodic table get it’s name?

A

Because similar properties occur at regular intervals.

37
Q

Elements in the same group in the periodic table have…

A

…the same number of electrons in their outer shell (outer electrons) and this gives them similar chemical properties.

38
Q

What does the atomic number of an element give?

A

The number of protons or
electrons

39
Q

Elements in the same period…

A

… have the same
number of shells

40
Q

As you go down a group…

A

…the number of shells
increases

41
Q

How did scientists attempted to classify the elements before the discovery of protons, neutrons and electrons?

A

By arranging them
in order of their atomic weights.

42
Q

What was wrong with early periodic tables?

A

The tables were incomplete and some elements were placed in inappropriate groups if the strict order of atomic weights was followed.

43
Q

What made it possible to explain why the
order based on atomic weights was not always correct?

A

Knowledge of isotopes

44
Q

How did Mendeleev overcome some of the problems of early periodic tables?

A

By leaving gaps for elements that he thought had not been discovered.

45
Q

What did Mendeleev predict about the undiscovered elements?

A

Their properties

46
Q

What do metals react to form?

A

Positive ions

47
Q

What do non-metals react to form?

A

Not positive ions (hydrogen is exeption)

48
Q

Where are metals found on the periodic table?

A

To the left and towards the bottom of the
periodic table.

49
Q

Where are non-metals found on the periodic table?

A

Towards the right and top of the periodic table.

50
Q

What happens to the boiling point of group 0 elements as you go down the group?

A

The boiling points of the noble gases increase with increasing relative atomic mass (going down the group).

51
Q

Do group 1 elements have high or low density?

A

They are metals with low density (the first
three elements in the Group are less
dense than water)

52
Q

How are group 1 metals safely stored?

A

They are stored under oil to prevent them
from reacting with oxygen or water.

53
Q

How do group 1 elements react with non-metals?

A

They react with non-metals to form ionic
compounds in which the metal ion carries a
charge of + 1.

54
Q

What does the compound produced when group 1 elements react with non-metals look like?

A

The compounds are white
solids which dissolve in water to form
colourless solutions.

55
Q

How do group 1 metals react with water?

A

Group 1 metals react with water releasing
hydrogen and form hydroxides which
dissolve in water to give alkaline solutions.
(this is why they are known as alkali metals)

56
Q

Describe how group 1 elements react with water?

A

They react vigorously with water fizzing and
moving around on the surface of the water.

57
Q

What happens to the reactivity of group 1 elements as you go down the group?

A

In group 1, the further down the group an element is the more reactive it becomes

58
Q

Why does reactivity increase as you go down group 1?

A

As the atoms get larger the outer electron is
further from the nucleus.
Thus the outer electron is less attracted to the nucleus and so can more easily be lost.

59
Q

What id the name given to group 7 elements?

A

Halogens

60
Q

What do the halogens have?

A

Coloured toxic vapours

61
Q

Are group 7 elements diatomic?

A

YES

62
Q

What do group 7 elements form when reacted with metals?

A

Ionic salts with metals in which the chloride, bromide or iodide ion carries a charge of -1

63
Q

What do group 7 elements form when reacted with non-metals?

A

Molecular compounds

64
Q

In group 7, does the relative molecular mass of the elements increase or down the group?

A

Increase due to increased intermolecular forces

65
Q

What is a displacement reaction?

A

When more reactive halogen can displace a less reactive halogen
from an aqueous solution of its salt.
E.g. Cl2 + 2 NaBr  Br2 + 2 NaCl

66
Q

In group 7, does the reactivity of the elements increase or decrease going down the group?

A

Decrease because…
Going down the group:
* The atoms get bigger
* and so outer shell electrons are
further from nucleus
* Outer electrons less strongly
attracted to nucleus
* can less easily gain electrons.

67
Q

Where are the transition metals in the periodic table?

A

between Groups 2 and 3

68
Q

Compared with the elements in Group 1, do transition metals have higher or lower melting points?

A

Higher (except mercury)

69
Q

Compared with the elements in Group 1, do transition metals have higher or lower densities?

A

Higher

70
Q

Compared with the elements in Group 1, are transition metals stronger?

A

YES

71
Q

Compared with the elements in Group 1, are transition metals harder?

A

YES

72
Q

Compared with the elements in Group 1, are transition metals less reactive?

A

Yes, are much less reactive and so do not react as vigorously with water or oxygen

73
Q

Many transition elements have ions with…

A

…different charges

74
Q

Many transition elements form…

A

…coloured compounds

75
Q

Many transition elements are useful as…

A

…catalysts

Chemistry- AQA- GCSE (2 decks)

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