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Atomic Structure And The Periodic Table Flashcards

(68 cards)

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1
Q

The amount of what subatomic particle dictates what element the atom is?

A

The number of protons.

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2
Q

Define isotopes

A

Isotopes

are atoms of the same element, with the same number of protons but a different number of neutrons.

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3
Q

How do you find the Relative Atomic Mass?

A

Sum of (isotope abundance x isotope mass number)
————————————————
Sum of abundances of all isotopes

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4
Q

Atoms join together to make…

A

Compounds
——————-
Compounds are substances formed by two or more elements, the atoms are in fixed proportions through the compound and held together by chemical bonds.

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5
Q

Properties of a compound are same/different from the properties of the original elements?

A

Different

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6
Q

Formula of ammonia

A

NH
3

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7
Q

Formula of sodium carbonate

A

Na CO
2 3

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8
Q

Formula of sulfuric acid

A

H SO
2 4

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9
Q

Balance this symbol equation

Mg + O 2 -> MgO

A

2Mg + 02 -> 2MgO

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10
Q

How are compounds formed?

A

Ionic or covalent bonding
(Giving away, taking or sharing electrons)

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11
Q

Are there Chemical bonds between compounds?

A

Yes!
————————————————A chemical reaction is needed to separate the original elements of a compound.

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12
Q

Formula of sodium chloride

A

NaCl

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13
Q

Formula of carbon monoxide

A

CO

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14
Q

Formula of calcium chloride

A

CaCl
2

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15
Q

Properties of a mixture are same/different from the properties of the origin elements

A

It’s just a mixture of properties of the separate parts- the chemical properties aren’t affected by it being a part of a mixture.

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16
Q

Are there Chemical bonds between different parts of mixtures?

A

No
———————————————-The parts of a mixture can be either elements or compounds and can we separated by physical methods.

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17
Q

When is paper chromatography needed?

A

To separate compounds out of a mixture

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18
Q

In chromatography- what do you use to draw a line
A) pencil
B) pen
Why?

A

Pencil because it leaves insoluble marks, so they won’t dissolve in solvent

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19
Q

In chromatography, should ink be touching the solvent?

A

No! Otherwise it will dissolve into it.

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20
Q

How do we stop the solvent from evaporating in chromatography?

A

Placing a lid on top of the container

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21
Q

What is the aim of paper chromatography? (What will happen?)

A

Each dye will move up at separate rate and will form a spot in different places. 1 spot per dye.
If they are insoluble, they’ll stay at baseline.

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22
Q

What is the end result of paper chromatography called?

A

The end result is a pattern of spots called a chromatogram

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23
Q

When is filtration needed?

A

To separate insoluble solids from liquids in a mixture or in purification

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24
Q

When is evaporation used compared to when crystallisation is used?

A

They’re used for separating soluble solids from solutions.
Evaporation is used when salt doesn’t decompose when heated and it’s quick
Crystallisation is used when you want nice, big salt crystals.

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25
How long do you hear the solution in crystallisation?
To the point of crystallisation (when crystals start to form)
26
Name the four steps to separating rock salt:
1) Grinding (dissolve easily) 2) Dissolving (salt will dissolve, sand won’t) 3) Filtering (Sand won’t pass through, salt will as part of the solution) 4) Evaporation/Crystallisation
27
What is rock salt?
A mixture of salt and sand. Salt is soluble Sand is insoluble
28
What is simple distillation used for? (2)
Separating solution of liquids with very different boiling points Or To get pure water from sea water
29
What evaporates first in distillation/ fractional distillation
The liquid with the lowest boiling point
30
How is the vapour cooled in distillation/ fractional distillation
Using a condenser, where vapour turns back to liquid after being cooled using water
31
What is fractional distillation used for?
Mixtures of liquids with very similar boiling points.
32
When is a fractionating column needed? Why?
When doing fractional distillation. This is needed because liquids with higher boiling points may also start evaporating, but the column would be cooled at the top, so they’ll condense and go back down again.
33
Who discovered the plum pudding model?
JJ Thomson
34
What was the plum pudding model?
It showed the atom as a ball of positive charge with electrons stuck inside.
35
What we’re the results of Rutherfords’ experiment?
Most Alpha particles went through. Done deflected Few rebound.
36
What does it mean if most alpha particles went through the gold foil in Rutherford’s experiment?
There is a large empty space between the nucleus and the outside of the atom.
37
What does it mean if some alpha particles deflected when sent towards the gold foil in Rutherford’s experiment?
The centre is positively charged
38
What does it mean if few alpha particles rebounded when sent at the gold foil in Rutherford’s experiment?
The centre is very small and dense
39
Why were Rutherford and Bohr’s findings easily accepted?
Because their findings were backed up and supported by evidence and work from other scientists.
40
What did Bohr suggest?
That electrons were in shells, different distances away from the nucleus.
41
What was Bohr’s model called?
The Nuclear Model
42
What did Chadwick do?
Provide evidence for neutral particles in the nucleus. (Neutrons)
43
Plum pudding model vs Nuclear model? What 4 points can you compare?
Space Density and centre Positive charge Location of electrons
44
Plum pudding model vs Nuclear model? Space
There is no empty space in plum pudding model There is empty space between the nucleus and electrons in the nuclear model
45
Plum pudding model vs Nuclear model? Density and centre
Plum pudding- everything has the same mass and density Nuclear- centre is small and dense
46
Plum pudding model vs Nuclear model? Positive charge
Plum pudding- the atom is a ball of positive charge Nuclear- the centre is positively charged
47
Plum pudding model vs Nuclear model? Location of electrons
Plum pudding- electrons are embedded in ball Nuclear- electrons are in electron shells, fixed distances away from nucleus.
48
Similarities with Mendeleev’s periodic table and Newlands’: 3 points
Both arrange elements in order of increasing atomic mass Both arrange in groups according to similar properties Both have places which have 2 elements
49
Differences with Mendeleev’s periodic table and Newlands’: 3 piints
In Mendeleev’s, the metals and non- metals are well separated with metals on the left, non metals on the right Mendeleev’s groups hydrogen with metals Furthermore, there are gaps and sometimes the order of increasing number isn’t followed
50
Why was Mendeleev’s periodic table readily accepted?
Because Mendeleev could predict the properties of undiscovered elements by looking at their location in the periodic table, these predictions were later proven to be true.
51
Do metals form positive/negative ions when react?
Positive- easy to lose electrons
52
Do non-metals form positive/negative ions when react?
Negative- easy to gain electrons
53
Why do elements react?
To gain a full outer electron shell
54
What are some features of a typical metal (3)
Strong but malleable Good at conducting heat and electricity High boiling and melting points
55
What are some features of a typical non-metal (3)
Dull looking Brittle Don’t generally conduct electricity Lower density
56
What are similar about transition metals and ‘proper metals’? (3)
Conduct heat and electricity Dense Strong Shiny
57
What are the unique properties of transition metals? (3)
Can have more than one ion Form coloured compounds Often make good catalysts React slower with oxygen and water More dense Harder Higher melting points (except mercury)
58
What are some properties of group 1 metals? (3)
Form 1+ ions Form white compounds Low melting and boiling points Soft Alkali metals Low density Very reactive
59
What happens to reactivity going down group 1? Why? (5 marks)
Increases Needs to lose an electron Forces of attraction decrease The more shielded the nucleus Outer most electron is more easily lost
60
What happens to reactivity going down group 7? (5 points)
Decreases Needs to gain electron More electron shells in between The more shielded the nucleus The weaker the forces of attraction Harder to gain an electron
61
What happens to melting and boiling points going down group 1?
Lower
62
What happens to melting and boiling points going down group 7?
Higher- more energy needed to separate it
63
Finish the **displacement** reaction- Cl2+ 2KI ->
Cl2+ 2KI -> I2 + 2KCl
64
What colour is fluorine?
Reactive, poisonous yellow gas
65
What colour is chlorine?
Reactive, poisonous dense green gas
66
What colour is bromine?
Dense, poisonous, red brown, volatile liquid
67
What colour is iodine?
Dark grey crystalline solid or purple vapour
68
What happens to melting and boiling points going down group 0?
Increases More electrons, greater intermolecular forces need to be overcome

Chemistry (2 decks)

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