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Working scientifically > C1 - Atomic Structure and the Periodic Table > Flashcards

C1 - Atomic Structure and the Periodic Table Flashcards

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1
Q

What are the subatomic particles in an atom?

A

Neutron

Proton electron

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2
Q

What is the size of an atom?

A

0.1 nm

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3
Q

What is the relative charge of a neutron?

A

0

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4
Q

What is the relative charge of a proton?

A

+1

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5
Q

What is the relative charge of an electron?

A

-1

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6
Q

What is the relative mass of an electron?

A

Very small

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7
Q

What is the relative mass of a proton?

A

1

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8
Q

What is the relative mass of a neutron?

A

1

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9
Q

What is the atomic number?

A

The number of protons

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10
Q

What is the mass number?

A

The number of protons and neutrons

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11
Q

How many electron does an atom have?

A

The same as protons

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12
Q

What is the overall charge on an atom?

A

0

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13
Q

What are isotopes?

A

Atoms that have the same proton number but different number of neutrons

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14
Q

What is an element?

A

Substances made up of atoms with the same atomic number

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15
Q

How do you calculate the relative atomic mass?

A

Sum of (isotope abundance x isotope mass number) / total abundance

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16
Q

What is a compound?

A

A substance made up of two or more different elements chemically bonded together in fixed positions

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17
Q

What is a molecule?

A

When two or more non-metals are covalently bonded

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18
Q

Why does a chemical reaction need to be balanced?

A

Because there need to be an equal number atoms on both sides

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19
Q

What is a mixture?

A

A substance made up of different elements or compounds that are not chemically bonded to each other and can be serrated by physical methods.

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20
Q

How do we separate compounds?

A

By chemical reaction

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21
Q

In a mixture, do the substances keep their properties or are they changed?

A

They keep

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22
Q

Why should we draw the baseline in paper chromatography with pencil?

A

Because the pencil contains graphite which is not soluble in water so it will not smudge the results

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23
Q

Which substances in a sample are moved further in paper chromatography?

A

The ones that are more soluble in the solvent

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24
Q

Which substances in a sample remain at the baseline?

A

The insoluble substances

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25
Why does the solvent need to be below the baseline?
Before the paper can even suck up the solvent, the sample will all dissolve in the solvent and nothing will rise up
26
What is the solvent front?
The distance that the solvent has travelled
27
How do you calculate the Rf value?
Distance travelled by the spot / distance travelled by the solvent
28
What will change the Rf value of a substance?
The solvent used
29
If you have a pure substance, how many spots are expected to be seen in the chromatography?
one
30
What are the different physical separation techniques?
Filtration, simple and fractional distillation, chromatography, crystallisation, evaporation
31
What is filtration used for?
To separate insoluble says from liquids
32
What is the solid left on the filter paper called?
Residue
33
What is the liquid that goes through the filter paper called
Filtrate
34
What is evaporation used for?
To separate soluble salts from liquids
35
Describe the developments in the atomic model
``` Atoms are solid spheres Plum pudding model Nuclear model Bohr's model Nucleus has protons Chadwick discovered neutrons ```
36
Why is the solid sphere model incorrect?
The atom is not a solid sphere but made up of loads of empty space
37
Why is the plum pudding model incorrect?
Electrons are not inside the nucleus
38
Why is the nuclear model incorrect?
Because atoms contained shells
39
What is another word for shell?
Energy level
40
How many electrons can go in the first, second and third shell?
2 8 8
41
What is the lowest shell?
The first one | The one that is closest to the nucleus
42
How were the elements in the old periodic table arranged?
According to increasing atomic weight/mass
43
How did Mendeleev arrange the elements in this Table of Elements?
He arranged elements according to their properties as well as atomic weight
44
Why did Mendeleev leave gaps in his table?
Elements were not discovered yet
45
What explained why elements cannot be strictly ordered by atomic weight?
The discovery of isotopes
46
How are the elements in the modern periodic table arranged?
Increasing proton/atomic number | In Groups and Periods
47
What does the Group tell you about the electronic structure of an element?
How many outer shell electrons it has
48
What does the Period tell you abut the electronic structure of an element?
The number of shells
49
Why do elements in the same group have the same chemical properties?
Because they have the same number of electrons in the outer shell
50
Do metals form positive or negative ions?
Positive
51
Do non-metals form positive or negative ions?
Negative
52
How do metals gain a full outer shell?
By losing electrons
53
How do non-metals gain a full outer shell?
By gaining electrons
54
What does it mean when metals are more reactive?
They can lose the electrons more easily
55
What does it mean when non-metals are more reactive?
They can gain electrons more easily
56
Metals get more reactive towards...
as you go down the group
57
Non-metals get more reactive towards...
as you go up the group
58
What is the appearance of metals like?
Shiny
59
What is the appearance of non-metals like?
Dull
60
What is the strength of metal like?
Strong but malleable
61
What is the strength of non-metal like?
Brittle
62
What is the melting and boiling points of metals like?
High
63
What is the melting and boiling points of non-metals like?
Low
64
What is a better conductor of electricity, metals or non-metals?
Metals
65
Name one exception of a metal that has low melting and boiling points
Mercury
66
How does the reactivity of the Group 1 elements change as you go down the group?
Increases
67
How do the melting and boiling points of the Group 1 elements change as you go down the group?
Decrease
68
How does the relative atomic mass of the Group 1 elements change as you go down the group?
Increase
69
Name properties of the Group 1 metals
They are softer than other metals They are very reactive They have lower melting points
70
What is the charge on an ion formed by a Group 1 element?
1+
71
What are the products of alkali metals with water?
Metal hydroxide + hydrogen
72
What are the products of alkali metals with chlorine?
Metal chloride
73
What is the product of the reaction of alkali metals with oxygen?
Metal oxide
74
What is another word for the Group 0 elements?
Noble gases
75
Why are noble gases so stable?
They have a full outer shell of electrons
76
How do the boiling points of Group 0 elements change as you go down the group?
Increases
77
What is the state of Group 0 elements at room temperature?
Gases
78
What is the colour of the noble gases?
Colourless
79
What is the appearance of fluorine like?
Yellow gas
80
What is the appearance of chlorine like?
Green gas
81
What is the appearance of iodine like?
purple vapour
82
What is the appearance of bromine like?
red-brown liquid
83
How does the reactivity of the Group 7 elements change going down the group?
Decreases
84
How does the molecular mass of the Group 7 elements change going down the group?
Increases
85
How do the melting and boiling points of the Group 7 elements change going down the group?
Increase
86
What is another word for Group 7 elements?
Halogens
87
Are halogens monoatomic or diatomic?
Di
88
Are noble gases mono or di atomic?
Mono
89
What type of a bond do halogens form with non-metals?
Covalent
90
What type of bond do halogens form with metals?
Ionic
91
What is the charge on the ion formed from a halogen?
1-
92
What is a displacement reaction?
When a more reactive halogen/element replaces a less reactive one

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