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Chemistry > Topic 1: Atomic Structure and the Periodic Table > Flashcards

Topic 1: Atomic Structure and the Periodic Table Flashcards

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1
Q

What is an atom?

A

The smallest part of an element that can exist

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2
Q

Proton:
i) mass
ii) charge

A

i) 1
ii) +1

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3
Q

Neutron:
i) mass
ii) charge

A

i) 1
ii) 0

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4
Q

Electron:
i) mass
ii) charge

A

i) very small
ii) -1

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5
Q

What is the number of protons equal to?

A

The number of electrons

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6
Q

What does atomic number show?

A

Number of protons

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7
Q

What does the mass number show?

A

Number of protons + neutrons

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8
Q

What is an ion?

A

An atom without charge

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9
Q

What is an isotope?

A

Different forms of the same element with the same number of protons but a different number of neutrons

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10
Q

How do you calculate relative atomic mass?

A

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

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11
Q

What is a molecule?

A

Two or more atoms, held together by a chemical bond

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12
Q

What is a compound?

A

Two or more different elements, held together by chemical bonds

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13
Q

What is a mixture?

A

Two or more substances, not chemically bonded

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14
Q

In chromatography, why should the line be drawn with pencil?

A

Pencil marks are insoluble so won’t dissolve in the solvent

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15
Q

In chromatography, why should you make sure the ink isn’t touching the solvent?

A

To stop the ink dissolving into it

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16
Q

What is chromatography used to do?

A

Separate substances in a mixture

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17
Q

What is filtration used to do?

A

Separate insoluble solids from liquids

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18
Q

What is evaporation used to do?

A

Separate soluble solids from solutions

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19
Q

What is crystallisation used to do?

A

Separate soluble solids from solutions

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20
Q

When does crystallisation have to be used instead of evaporation?

A

If the salt decomposes when it’s heated

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21
Q

Explain how you would separate rock salt using filtration and crystallisation [4]

A
  1. Grind the rock salt to make sure the salt crystals are small, so will dissolve easily
  2. Put the mixture in water and stir - salt will dissolve, but the sand won’t
  3. Filter the mixture - the sand will collect on the paper but the salt will pass through in the solution
  4. Evaporate the water from the salt so that it forms dry crystals
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22
Q

What is rock salt a mixture of?

A

Sand and salt

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23
Q

What is simple distillation used to do?

A

Separate out solutions

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24
Q

What is the problem with simple distillation?

A

It can only be used to separate liquids with very different boiling points

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25
What is fractional distillation used to do?
Separate a mixture of liquids
26
What did the atomic theory (Democtritus) state? [2]
1. Everything is made from tiny particles, which can't be broken down any further 2. They are separated by empty space
27
What did John Dalton conclude? [2]
1. Atoms were solid spheres 2. Different types of spheres make up the different elements
28
What did the plum pudding model (J.J. Thomson) state?
The atom is a ball of positive charge with electrons stuck in it
29
Desscribe Rutherford's gold foil experiment and the results [3]
1. Fired alpha particles at thin gold foil 2. Expected particles to pass straight through or only be slightly deflected 3. Although most particles passed straight through, some were deflected more than expected and some were deflcted back the way they had come
30
What was concluded as a result of the gold foil experiment and why? [2]
1. Atoms contain a compact, positive nucleus in the centre - because some of the particles were deflected back 2. Rest of the atom is empty space - nearly all of the particles passed straight through
31
What was the model of the atom known as after the gold foil experiment?
Nuclear model
32
What did Bohr add to the nuclear model?
Electrons orbit the nucleus at specific distances
33
What did Chadwick discover?
The presence of neutrons in the nucleus
34
How many electrons maximum in the 1st shell?
2
35
How many electrons maximum in the 2nd shell?
8
36
Elements in the same group in the periodic table have what in common?
Same number of electrons in their outer shell (similar chemical properties)
37
How were elements classified in the early 1800s?
By atomic wight
38
What 2 changes did Mendeleev make to the early periodic table?
1. He left gaps in order to keep elements with similar properties in the same group 2. He switched the order of elements based on their properties, even if their atomic weights were no longer in order
39
What made it possible to explain why the order based on atomic weights is not always right on the periodic table?
The discovery of isotopes in the early 20th century
40
What kind of ions do metals form?
Positive ions
41
What kind of ions do non-metals form?
Not positive ions
42
Physical properties of metals [3]
1. Malleable 2. Great conductors of heat and electricity 3. High boiling and melting points
43
Physical properties of non-metals [4]
1. Dull in colour 2. Brittle 3. Poor conductor of electricity 4. Low boiling and melting points
44
What special properties do transition metals have? [3]
1. Elements can form more than one ion 2. Ions are often coloured 3. They make great catalysts
45
What is another name for group 1 metals?
Alkali metals
46
Alkali metal properties [3]
1. Soft 2. Low density 3. Low melting point
47
Alkali metal trends [2]
1. Increasing reactivity 2. Decreasing melting and boiling points
48
What do the alkali metals form with non-metals?
Ionic compounds
49
Ionic compounds: i) colour and state i) colour in water
i) white solids i) form colourless solutions
50
What does alkali metal + water produce?
Metal hydroxide + hydrogen gas
51
What does alkali metal + chlorine produce?
Metal chloride salts
52
What does alkali metal + oxygen produce?
Metal oxides
53
Lithium + oxygen forms?
Lithium oxide
54
What is the formula for lithium oxide?
Li₂O
55
Sodium + oxygen forms? [2]
1. Sodium oxide 2. Sodium peroxide
56
What is the formula for sodium oxide?
Na₂O
57
What is the formula for sodium peroxide?
Na₂O₂
58
Potassium + oxygen forms? [2]
1. Potassium peroxide 2. Potassium superoxide
59
What is the formula for potassium peroxide?
K₂O₂
60
What is the formula for potassium superoxide?
KO₂
61
What is another name for group 7?
Halogens
62
Halogen trends [2]
1. Decreasing reactivity 2. Increasing melting and boiling points
63
What will a more reactive halogen do?
Displace a less reactive one
64
What is fluorine?
Yellow gas
65
What is chlorine?
Green gas
66
What is bromine?
Red-brown liquid
67
What is iodine? [2]
1. Grey solid 2. Purple vapour
68
What is another name for group 0?
Noble gases
69
Noble gas properties [3]
1. Colourless gases 2. Unreactive 3. Non - flammable
70
Noble gas trend
Increasing melting and boiling points
71
How do group 1 metals differ to transition metals? [3]
1. More reactive 2. Less dense, strong, hard 3. Lower melting points

Chemistry (10 decks)

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