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GCSE Chemisty > C1 atomic structure and the periodic table > Flashcards

C1 atomic structure and the periodic table Flashcards

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1
Q

Element

A

A substance that cannot be broken down chemically

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2
Q

Compound

A

A substance that contains at least two different elements chemically combined and fixed proportions

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3
Q

Elements

A

Are made up of atoms that are all the same

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4
Q

Compounds

A

Are made from atoms or charged atoms of different elements which are been chemically joined together

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5
Q

Mixtures

A

Can be easily separated because of the chemicals in them or not join together.

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6
Q

Mixture of separation techniques

A

Filtration, crystallisation, simple distillation, fractional distillation and chromatography.

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7
Q

Democritus

A

400 BC
Describe the materials has been made of small particles which could not be divided. These particles were atoms. He had no evidence

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8
Q

John Dalton

A

1803

He described an atom a billiard ball which could not be divided

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9
Q

J.J. Thomson

A

1897
Who describes atoms using a plum pudding model. The negative electrons were thought to be embedded in a ball of positive charge (protons)

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10
Q

Geiger and Marsden

A

1909
They conducted an experiment with gold leaf and alpha particles. This showed that the atom had a positively charged nucleus in the centre where most of the mass of the atom is concentrated and much of the atom was empty space

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11
Q

Niels Bohr

A

1913

He confirmed previous experiments although explained that electrons orbiting the nucleus

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12
Q

James Chadwick

A

1920
Term proton was used for positively charged atoms
1932
Neutron discovered

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13
Q

Atoms

A

Is made up of a nucleus that is surrounded by electrons

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14
Q

Electron shells

A

Electrons occupy the space around the nucleus in shells. The space between the nucleus and the electron shells is empty space.

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15
Q

Atomic radii

A

A typical atomic radius is about 0.1 nm (1×10 to the -10 m)
However the radius of an atom increases within a group of elements. The atomic radii a Li,Na,K increase as more electrons are added to the atom

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16
Q

The atomic number

A

The number of protons/ electrons in an atom

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17
Q

Relative atomic mass

A

Number of protons and neutrons

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18
Q

Isotopes

A

A form of an element that has the same number protons but different number of neutrons

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19
Q

Relative abundance calculation

A

Ar = (mass of first isotope x % Of first isotope) + (Mass of first isotope x % of first isotope) /100

20
Q

Electron shell formation

A

2,8,8,18,18,32,32

21
Q

Periodic table

A

The periotic table is arranged in order of proton number
Rows show how many shows how many electron shells it has
Columns show how many electrons it has and that shell

22
Q

Row

Column

A

Period

Group

23
Q

Group 1
Group 7
Group 0/8

A

Highly reactive metals
The halogens-react with group 1 metals to make Salts
Are are unreactive-noble gases

24
Q

Döbereiner

A

1829
Noticed that sometimes three elements have similar properties. These were called Döbereiner triads
1860
I need a list of more accurate atomic weight was published

25
Q

John Newlands

A

1865
Noticed that when he put elements in atomic weight order some of them seem to be in the wrong place there was often a pattern of similar properties every eight element. He called his new theory the law of octaves. He noticed the patterns but did not make predictions

26
Q

Dimitri Mendeleev

A

1869
Decided to swap some elements around so that the patterns of chemical behaviour fitted better
was able to imagine that were undiscovered elements
Left gaps in his table for later discoveries
Put eka infront of names , 3 elements were discovered in his lifetime

27
Q

Periodic table modern day

A

1932
Theory developed and supported with evidence- isotopes explained why order was wrong. Discovery of neutron explained why it had to be by number of protons

28
Q

Physical properties of metals

A 
Lustrous
Hard
High density
High tensile strength
High melting point and boiling point 
Good conductors of heat
Good electrical conductor
29
Q

Physical properties of nonmetals

A 
Dull
Soft, brittle, liquid or gas
Low density
Low or no tensile strength or gas
Low melting point and boiling point
Poor or no thermal conductivity
Poor or non conductors of electricity
30
Q

Chemical properties of metals

A

Result of reactions with oxygen or acids to make salts and hydrogen gas

Form basic oxides

31
Q

Chemical properties of nonmetals

A

Result of reaction with oxygen
Eg carbon with oxygen to make CO2

Form acidic (or neutral) oxides

32
Q

Metals and nonmetals in the periodic table

A

Metals are on the left hand side and non metals are on the right hand side

33
Q

Positions of elements in the table

A

If it makes a positive ion it is a metal

Nonmetals make negative ions

34
Q

Stable atoms

A

The noble gases or stable atoms as they have a full outer shell

35
Q

What can happen to the electrons in the outer shell

A

They can be transferred to the outer shell of another atom
They can have electrons are added to the outer shell from another atom
They can be shared with another atom

36
Q

Group 0

A

All unreactive

All gases

37
Q

Why does helium stay as a gas at lower temperatures?

A

Exist as single atoms not molecules

The smaller the atom it is it is for them to keep moving around rapidly

38
Q

Why do elements in group 0 exist as single atoms?

A

They do not make compounds with other elements and are unreactive. This is because they have 8 electrons in their outer shell

39
Q

Properties of group 1 elements

A

They are less dense than water so they would float
React vigorously with water to produce hydrogen
Burn in water to form oxides (sodium)

40
Q

Reaction trends of alkali metals

A

Lithium reacts vigorously with water
Sodium reacts very vigorously with water sometimes an orange flame produced
Potassium reacts extremely vigorously with water and produces a lilac flame

41
Q

What is an ion

A

When an atom loses or gains an electron

42
Q

Halogens

A 
Are non metals
Exist as a pair of atoms
React vigorously with group 1 metals
Make gases or liquids such as acids
Are solid or gas at room temp
43
Q

Reactivity

A

1 increases down group

7 increases up the group

44
Q

Trends across the table

A

Metal to non metal
Across and down depend on atomic structure and electronic structure
Period 2&3 outer electrons increase by 1 from group 1
Group 2 with 2 outer electrons up to group 7 with 7 outer electrons
Group 1 lose electron to form +ions easier
Group 7 gain 1 electron to form ions

45
Q

Transition elements

A

Are metals and have typical metallic properties
Found in the middle part of the periodic table
Less reactive than elements in group 1
Often catalysts

46
Q

A catalyst

A

An element or compound that changes the rate of a chemical reaction without taking part in the reaction as a reactant. Catalysts are unchanged by the reaction.

47
Q

Ions and coloured compounds

A

A compound that contains the transition element is often coloured
Can form 2 types of positive ions.

GCSE Chemisty (10 decks)

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