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Chemistry revised Paper 1 (Part 1) - Coggle Diagram
Chemistry revised Paper 1 (Part 1)
Atomic Structure and the Periodic Table
Atom basics
Tiny
Greeks believed the 'atomos' was the smallest thing in the world
So much so that 'atomos' meant 'uncuttable'
Made of 3 particles
Proton
Protons have a mass of 1
And a charge of +1
Neutron
Neutron has a mass of 1
And a charge of 0
Electron
Electrons have a mass of 1/2000 or 0.005
And a charge of -1
Atoms are infinitesimally small particles which make up everything in the universe
Compounds
Compounds are 2 or more elements that are bonded together
Periodic Table
The Periodic Table is a Graph that shows all 118 discovered 'elements' (types of atoms) in the world
Structure of the atom
The atom is made up of 2 parts
The Nucleus
The Nucleus is made up of protons and neutrons
and the shell
The shell is made up of electrons
Elements on the periodic table
The boxes containing elements on the periodic table have 4 parts
Symbol
Self explanatory, just avoid mishaps with symbols being different to names ( Potassium symbol= K)
Name
Self explanatory
The atomic number
Atomic Number = Protons = Electrons
Atomic number < Mass number
Mass number
Mass number= Protons + Neutrons
Mass number > Atomic Number
Must Learn Formula!
Hydrogen Gas
H2
Nitrogen Gas
N2
Oxygen Gas
O2
Ammonia
NH3
Water
H2O
Hydrochloric Acid
HCl
Carbon Dioxide
CO2
Sulfuric Acid
H2SO4
Please note all numbers should be written smaller than letters
Elements, Compounds and Mixtures
Definitions
Elements
Pure forms of atoms
e.g Hydrogen (H), Helium (He), Lithium (Li)
Compounds
2 or more elements that are chemically bonded
e.g Carbon Dioxide (CO2), Water (H2O), Sodium Chloride (NaCl)
Mixtures
A non chemically bonded mixture of several types of elements
Ink (C14H26N2O4S), Air (Annoying formula), Seawater (Also annoying formula)
Ways to seperate mixtures
Distillation
Heating the mixture at certain boiling points so that at each boiling point one element is extracted, until all of them are extracted
Evaporation
Heating the mixture so all liquids are gone, leaving only solids
Filtration
Pouring a liquid through filtration paper/ a sieve leaving the solid
Fractional Distilation
When you do regular distillation but extract different solids at different points
Plum Pudding Model and Rutherford's Experiment
Basis of the Plum Pudding Model
The plum pudding model is made up of two main parts
A 'pudding' of positive matter
Several negative 'plums' that are embedded in the positive matter
Rutherford's Experiment
The process
Rutherford and his student, Marsden, set up an 'alpha particle gun' to be fired at a thin sheet of gold foil
Their expectations were that all the strong alpha particles would go through the thin sheet
Result
They were partly correct in their predictions, with most going through, but some bounced off, which in today's circumstances, is like seeing a bullet bounce off a sheet of paper
History of the Atom
Ancient Greece (700BC-146BC)
Believed in 5 types of matter
Fire
Hot and Dry
Water
Cold and Wet
Earth
Cold and Dry
Air
Hot and Wet
Aether
Heavenly substance
Also created the word 'atomos'
Which means uncuttable
John Dalton (1860s)
Discovered the fact that atoms are tiny, solid spheres
J.J Thomson (1897)
Discovered the theory of the Plum Pudding Model
Tiny positive 'pudding' embedded with negative 'plums'
Lord Ernest Rutherford (1909)
Did the infamous 'Rutherford Experiment' (See separate branch)
Through this, he discovered the Proton
And through that, discovered the electron
Niels Bohr (1913)
He discovered that electrons don't float aimlessly round the proton 'nucleus', they orbit in 'shells'
James Chadwick (1932)
Discovered the 'Neutron'
A neutron is a neutrally charged particle that belongs in the nucleus, along with the protons and other neutrons
Groups, Periods and Electronic Structure
Which is which
Groups are vertical
There are 8 groups, plus a large chunk in the middle that are groupless
They are numbered: 1, 2, 3, 4, 5, 6, 7 and 0
Groups also show how many electrons are in the outer shells
e.g. Hydrogen has 1 electron
Periods are horizontal
Periods show two things:
1: How many shells they have
e.g. Hydrogen has 1 shell, but Chlorine has 3 shells
2: The amount of elements in each period show how many electrons should be in each shell at maximum
e.g. 1st shell has Hydrogen and Helium ; 2 elements meaning that rthe 1st shell can have no more than 2 electrons
Isotopes
Definition
An isotope is an atom with the original amount of protons and neutrons as a regular atom of that element but has more/less electrons
In short, same atomic number, different mass number
Rules
Metals can only lose electrons, giving them a + charge
Non-metals can only gain electrons, giving them a - charge
What group you are in shows how many electrons you lose, e.g. Berylium (A solid in Group 2) loses 2 electrons
With Non-Metals, Group 7 Chlorine doesn't gain 7 electrons, it gains 1. Group 6 Oxygen gains 2, Group 5 Nitrogen gains 3 etc.
Different Element Groups
There are multiple Groups in the Periodic Table with different names, these are:
Alkali Metals (Group 1)
They react violently with metals
This causes flames to come from the reaction
This is what is used to make fireworks, with Alkali Metal Potassium being used regularly
Please note that despite being in that column regularly, Hydrogen is not an Alkali Metal, it is not even a metal
The Alkali Metals are soft, cuttable metals
They have to be stored in oil so they don't react with Oxygen and Water
Equations
Alkali Metal+ Oxygen= Metal Oxide
Alkali Metal + Water= Metal Hydroxide
They are all solid, apart from Hydrogen =, which isn't fully in group 1
Noble Gases (Group 8)
They have a full outer shell
They are unreactive
This means they have a lot of uses because of this including:
Balloons
Neon Lights
Halogens (Group 7)
They are 'diatomic' meaning they go in pairs (F2 (Fluorine), Br2 (Bromine))
They are all gases
They are highly reactive as they only need one electron
They regularly 'covalently bond' meaning they share an electron to each, resulting in the diatomicity
Most reactive are at the top (Fluorine) and least reactive at the bottom (Tennessine)
The lowest boiling point is at the top as well, with the highest at the bottom
States of Matter, Boiling Points and Melting Points
Liquids
Flexibility
In the middle between the two. Like solids, it is heavy and there is a large amount of restriction in the movement of particles. Like gases however, it can move around and be flexible enough to move around a contained area as much as it sees fit
Transitions to other states
Liquid to solid
Freezing
Liquid to gas
Evaporating
Gases
Flexibility
Very flexible, almost no chemical bonding between the particles, moves around freely and is very light
Transitions to other states
Gas to liquid
Condensing
Gas to solid
Deposition
Solids
Flexibility
Very brittle, little to no movement in the particles, cannot move from it's fixed position at all
Transition to other states
Solid to liquid
Melting
Solid to gas
Sublimating
Melting and boiling points
Compounds
Melting point
19oC
Boiling Point
14oC
State symbols
S= Solid
L= Liquid
AQ= Aqueous Solution
G= Gas
Ionic Bonding and Covalent Bonding
Ionic Bonding
Process
For example, take magnesium and Oxygen. Magnesium has 2 outer shell electrons, Oxygen has 6
Atoms want a full outer shell, so magnesium transfers it's 2
This gives oxygen it's full 8 electron outer shell, giving it a -2 charge, with electrons added
Magnesium then has +2 and is also stable, as they have emptied their outer shell, giving them greater stability as well
Covalent Bonding
Process
For example, take Nitrogen with 5 outer shell electrons and 3 Hydrogen atoms with 1 outer shell electron each
As usual, Nitrogen wants a full outer shell with 8 electrons
So, they collectively share their bonds with the 3 Hydrogen atoms, and the 3 coming to the Nitrogen's shell, give it the full outer shell
For reference, NH3 is Ammonia
Metals and Alloys
Any metal that isn't a metal alloy is called a pure ketal. A pure metal is a metal that only consists of that metal's atoms and de localised electron, the similar shape and size makes them easy to slide over each other and therefore, easily breakable
Any metal that isn't pure is called a metal alloy, this is when another metal or non-metal is added in the making of the metal, the shape and size of the alloy atoms means they can't slide over each other and they are therefore, harder to cut
Ionic Compound, Simple Covalent Compound and Giant Covalent Compound Structure and Properties
Ionic Compound
Structure
Giant Ionic lattice
Properties
High Melting Polint
High Boiling Point
Only conducts electricity when molten or dissolved
Ions need to be free to move
Examples
Sodium Chloride,
Lead Chloride
Potassium Hydride
Simple Covalent Compound
Structure
Covalent Bonding
Properties
Low Melting point
Does not conduct electricity
Examples
Water
Carbon Dioxide
Oxygen
Nitrogen
Hydrogen
Hydrochloric Acid
Giant Covalent Compounds
Examples
Graphite
Diamond
Carbon Nanotube (Buckminsterfullerene)
Structure
Giant Covalent Structure
Properties
High Melting Point
High Boiling Point
Doesn't conduct electricity
Does not dissolve