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Chemistry > C1 - Atomic Structure And The Periodic Table > Flashcards

C1 - Atomic Structure And The Periodic Table Flashcards

1
Q

What is the definition of an element?

A

A substance where all atoms are the same

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2
Q

What is the definition of a compound?

A

A substance containing 2 or more elements chemically combined in fixed proportions

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3
Q

What is the definition of a mixture?

A

Different compounds and elements that are however not chemically combined

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4
Q

If you want to separate a mixture you can use a chemical/ physical seperating technique?

A

Physical

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5
Q

What are 4 physical methods of seperating a mixture?

A

Filtration
Crystallisation
Distillation
Chromatography

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6
Q

What is the definition of a molecule?

A

A molecule is any elements chemically combined
Eg O^2

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7
Q

Filtration is used to separate an insoluble/ soluble solid from a liquid/gas

A

Insoluble solid
Liquid

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8
Q

What three pieces of equipment are needed to perform filtration?

A

Conical flask
Filter paper
Filter funnel

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9
Q

Crystallisation is used to separate an insoluble/ soluble solid from a liquid.

A

Soluble solid

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10
Q

What does the state symbol (aq) mean?

A

Dissolved in water

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11
Q

How can we make crystallisation happen faster?

A

Gently heat the solution

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12
Q

What are the 2 main stages of simple distillation?

A

Evaporation and condensation

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13
Q

What is fractional distillation used for?

A

To separate a range of different liquids

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14
Q

In fractional distillation the liquids must have different _________ points.

A

Boiling

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15
Q

When the thermometer temperature is rising steadily in fractional distillation, what does this mean?

A

There is a mixture of the liquids condensing into the beaker

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16
Q

When the temperature on the thermometer stops rising in fractional distillation what does this mean.

A

One of the liquids is condensing as a pure substance

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17
Q

What is a solvent?

A

A liquid that will dissolve substances

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18
Q

What do we call the paper in chromatography?

The __________ phase

A

Stationary

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19
Q

What do we call the solvent during paper chromatography?

The ______ phase

A

The mobile phase
Because it moves

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20
Q

In paper chromatography…
A pure/ impure compound will produce a single spot in all solvents.

A

Pure

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21
Q

True or false

In paper chromatography…

A more soluble substance travels less far along the mobile phase than a substance that is less soluble.

A

False, a more soluble substance travels further than a substance that is less soluble.

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22
Q

In paper chromatography…
Why do we draw the starting line in pencil and not in pen?

A

Because the pen ink could dissolve in the solvent and move up the paper

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23
Q

Why did Rutherford use gold in his alpha particle scattering experiment?

A

Gold can be hammered into very thin few only a few atoms thick

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24
Q

Alpha particles has a negative/positive charge.

A

Positive

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25
Who proposed the plum pudding model?
J . J Rutherford
26
Who proposed that electrons orbit the nucleus at specific distances?
Niels Bohr
27
What do we call the orbits of electrons?
Shells
28
Who discovered that the nucleus also contains neutral particles?
James Chadwick
29
What is the radius of an atom?
0.1 nanometres
30
How many metres (in standard form) is 0.1 nanometres?
1 x 10^ -10 m
31
What is the radius of a nucleus in an atom? In metres
1 x 10 ^ -14 m
32
What is the relative charge of a proton?
+1
33
What is the relative charge of a neutron?
0
34
What is the relative charge of an electron?
-1
35
The number of protons in an atom, are___ greater/equal/less___ than the number of electrons in the atom.
Equal
36
What is the overall charge of an atom?
0
37
What is the relative mass of a proton?
1
38
What is the relative mass of a neutron?
1
39
What is the relative mass of an electron?
Nearly 0 Very small
40
All the atoms of the same element all have the same number of neutrons/ electrons/ protons.
Protons
41
When an atom contains a different number of neutrons to other atoms of the same element, what is this atom called?
An isotope
42
What are ions?
Ions are atoms which have an overall charge because they have lost or gained electrons.
43
What does the word abundance mean in regards to how common each isotope is?
It means how common each isotope is
44
What is the equation to calculate relative atomic mass?
(Mass no x percentage abundance of is 1) + (Mass no x percentage abundance of is 2) _______________________________________________________________________ 100
45
The larger/ smaller of the 2 numbers either side of the element in the periodic table is the atomic number.
Smaller
46
How many electrons can the first shell in an atom hold? (Max)
2
47
How many electrons can the second shell in an atom hold? (Max)
8
48
The number of electrons in the outer shell of the atom tells us the____ mass/ atomic/ group/element number of that element in the periodic table.
It tells us the group number
49
What group of the periodic table are elements with a full outer shell found in?
Group 0
50
What is the name for group 0 in the periodic table?
The noble gases
51
Who developed the first modern periodic table?
Dmitri Mendeleev
52
In the modern periodic table the elements are arranged in order of…
Atomic number
53
Atomic number is the no of neutrons/protons/electrons in the atom.
No of protons
54
What kind of ions do metals always form?
Metals always form positive ions
55
What are the group 1 elements called in the periodic table?
They are called the alkali metals
56
All group 1 metals have ___ electron in their outer shell.
1
57
Are group 1 metals hard or soft?
Soft
58
Group 1 metals react slowly/ quickly with oxygen.
Quickly
59
What can be observed during the reaction of lithium with water?
Fizzing, alkali pH
60
What can we observe during the reaction the reaction of sodium with water?
Fizzing, alkaline pH
61
What can we observe during the reaction of potassium with water?
Extremely rapid, fizzing, catching fire, alkaline pH
62
What does effervescence mean?
Fizzing/ bubbles in a liquid
63
In covalent bonding, electrons are_______.
Shared
64
What are the group 7 elements called?
The halogens
65
The melting and boiling points increase/decrease as we move down group 7.
Increase
66
Fluorine and chlorine are both solids/liquids/gases at room temperature sine their boiling points are lower than room temperature.
Gases
67
Do the molecules get smaller or bigger moving down group 7?
Bigger
68
Are the halogen metals or non metals?
Non- metals
69
What is an ion?
An ion is an atom with an overall charge
70
What is the most reactive element in group 7?
Fluorine
71
Do the halogens get more or less reactive as we move down group 7?
They get less reactive
72
A ______ reactive halogen can displace a _____ reactive halogen from and aqueous solution of its salt.
More, less
73
We find metals on the ____ side of the periodic table.
Left
74
We find non metals on the _____ side of the periodic table.
Right
75
All of the ______ elements are metals.
Transition elements
76
Do alkali metals have a low or high density?
Low density
77
Are alkali metals soft or hard metals?
Soft metals
78
Are the transition metals soft or hard?
Hard metals
79
Do transition elements have high or low melting points?
High melting points
80
Do transition elements have a high or low density?
High density
81
What is copper used to make?
Used to make pipes to carry water
82
What colour is iron oxide?
Reddish
83
What colour is copper sulphate?
Blue
84
What is a catalyst?
Chemical added to increase the rate of reaction is however not used up in the reaction.

Chemistry (13 decks)

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