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GCSE AQA Chemistry > C1 - Atomic Structure > Flashcards

C1 - Atomic Structure Flashcards

1
Q

What is the plum pudding model

A

A ball of positve charge with negative electrons studded into it

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2
Q

What did the gold foil experiment prove

A

Atoms have dense nuclei with a positive charge

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3
Q

What did chadwick discover

A

Neutron

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4
Q

What did bohr discover

A

Electrons are in shells

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5
Q

History of atom timeline

A

Dalton said atoms were balls
Thompson Plum Pudding Model
Rutherford alpha scattering
Rutherford nuclear model (stereotypical model)
Bohr model - electrons in shells
Chadwick nucleus
Current nuclear model

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6
Q

Why did mendelev leave gaps in the periodic table

A

For elements that had not been discovered yet

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7
Q

What is an atom?

A

The smallest part of an element that can exist

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8
Q

What is an element?

A

A substance made of only one type of atom

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9
Q

What is a compound?

A

A substance made of two or more different atoms chemically bonded

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10
Q

How are compounds formed?

A

From chemical reactions

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11
Q

What is involved in a chemical reaction?

A

The formation of one or more new substances and an energy change

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12
Q

What is a molecule?

A

A substance made of more than one atom chemical bonded

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13
Q

What is a mixture?

A

A substance made of more than one thing not chemically bonded together

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14
Q

How can mixtures be separated?

A

Physical processes (filtration, crystallisation, simple distillation, fractional distillation and chromatography)

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15
Q

Name the three subatomic particles

A

Protons, neutrons, electrons

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16
Q

State the relative masses and charges of the subatomic particles

A

Mass: Proton :1, neutrons:1, electrons:0

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17
Q

What is the plum pudding model

A

A ball of positive charge with negative electrons studded into it

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18
Q

What did the gold foil experiment (alpha particle scattering) prove?

A

That atoms have sense nuclei with a positive charge

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19
Q

What did Chadwick discover?

A

The neutron

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20
Q

What did Bohr’s experiments show?

A

That electrons are in specific shells

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21
Q

What is the atomic number of an atom?

A

The number of protons in an atom

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22
Q

What is the mass number of an atom?

A

The number of protons + the number of neutrons

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23
Q

In the electron shell model, how are the subatomic particles arrange in an atom?

A

Protons and neutrons in the nucleus, electrons orbiting in shells

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24
Q

Why is the number of electrons in an atom equal to the number of protons

A

As their charges cancel out

25
How many electrons can go in the first shell?
2
26
How many electrons can go in the second and third shells?
8
27
What are the groups in the periodic table?
The columns numbered (1, 2, 3, 4, 5, 6, 7, 0)
28
What can the group tell you about the electrons in an atom
How many electrons are in the outer shell E.g. carbon is in group 4 so has 4 electrons in the outer shell
29
What are periods in the periodic table?
The rows
30
What can the period tell you about the electron in an atom?
How many shells an atom has. E.g. Carbon is in the second period so has two shells.
31
Why do atoms have no overall charge?
The number of protons and neutrons are equal
32
Approximately how large are atoms?
Radius is 0.1 nm
33
How large is the nucleus compared to the whole atom?
About 1/10,000 the size
34
What are isotopes?
Atoms of the same element with a different number of neutrons
35
What is abundance?
The % of atoms in a sample with a particular mass
36
What is the relative atomic mass of an element?
An average value for the mass that takes account of the abundance of the isotopes of the element
37
In the modern periodic table, how are the atoms arranged?
By their atomic number and in groups according to their chemical properties
38
Why do elements in the same group have similar properties?
Because they have the same number of electrons in their outer shell
39
Before the discovery of protons, neutrons and electrons, how did scientists organise the elements?
By atomic weight
40
Why did Mendeleev leave gaps in his periodic table?
For elements that had not been discovered yet
41
Which discovery meant that their organising elements by atomic weight was not always correct?
Isotopes
42
Where are the metals on the periodic table found?
To the left and bottom of the periodic table
43
What is an ion?
An atom which has lost or gained electrons
44
What kinds of ions do metals and non-metals form?
Metals form positive, non-metals form negative
45
What name is given to elements in group 0?
Noble gases
46
Why are the group 0 elements so unreactive?
They gave full outer shells so do not need to lose or gain electrons
47
How does the boiling points of group 0 change down the group?
Increases down the group
48
Explain why the group 1 elements are called alkali metals
They are metals that form alkalis when they react with water
49
What are the products of the alkali metals in a reaction with: oxygen, water, halogens
Oxygen: Metal oxide
50
Explain why group 1 elements get more reactive down the group
More electrons, more shielding, weaker electrostatic from the nucleus to the outer shell, easier to lose an electron
51
What name is given to elements in group 7?
Halogens
52
How does the boiling point of group 7 elements change down the group?
Increases down the group
53
Explain why the group 7 elements get less reactive down the group?
More electrons, more shielding, weaker electrostatic attraction from the nucleus to the outer shell, harder to gain an electron
54
What is a displacement reaction?
Where a more reactive element displaces a less reactive one from a compound
55
Where are the transition metals found in the periodic table?
In the middle
56
Compare the melting point, density, strength, hardness and reactivity of transition metals with group 1 metals
Higher for all but reactivity
57
What is distinctive about the ions formed by transition metals?
Can form ions with different charges
58
What is distinctive about compounds formed from transition metals?
They are coloured
59
What can transition metals be used for?
Catalysts

GCSE AQA Chemistry (18 decks)

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