Periodic Table
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- Created by: Abc312
- Created on: 30-03-18 14:53
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- Periodic Table
- How it is organised
- The columns are called groups
- The group number tells you the electrons in the outer shell
- The elements in each group have similar properties
- This is because the electrons in the outer shell control how it reacts
- As you go down the group you can make predictions in the reactivity trends
- The rows are called periods
- Each new row represents another full shell of electrons
- They are laid out in increasing atomic numbers.
- The metals are on the left of the table and the non-metals are on the right
- The columns are called groups
- Metals and Non-metals
- Most elements are metals
- Metals form positive ions when they react
- This is because they don't have to lose many electrons to get a full outer shell
- Metals form positive ions when they react
- Metals are on the left of the table and non-metals are on the right
- Most metals are strong, malleable, good heat and electricity conductors and have high boiling and melting points
- Transition metals are in the middle of the periodic table
- They have the same properties of other metals
- They can form multiple ions which normal metals cannot
- They are often coloured
- They make good catalysts in reactions
- Most elements are metals
- Group 1 Elements
- They are :
- They are also known as the alkali metals
- Lithium
- Sodium
- Potassium
- Rubidium
- Caesium
- Francium
- They all have one electron in the outer shell
- This makes them very reactive because they easily form 1+ ions
- They are soft and have a low density
- As you go down the group...
- Reactivity increases
- The outer electron is more easily lost because the electron is further away from the nucleus so the attraction is weaker
- Lower melting and boiling points
- Reactivity increases
- Reaction with water
- React vigorously with water
- Producing hydrogen gas and a metal hydroxide
- A metal hydroxide is a salt that dissolves in water to make alkaline solutions
- Producing hydrogen gas and a metal hydroxide
- The more reactive the metal is the more violent the reaction
- The further down the table the more energy is released
- Potassium releases enough energy to ignite hydrogen
- Lithium
- Produces Lithium hydroxide and hydrogen
- Sodium
- Produces sodium hydroxide and hydrogen
- Potassium
- Produces potassium hydroxide and hydrogen(but it ignites it)
- React vigorously with water
- They only ever make ionic compounds which are usually white solids that dissolve in water to form colourless solutions
- Reaction with chlorine
- Group 1 reacts vigorously when heated in chlorine gas
- This produces metal chloride salts
- Lithium
- Produces lithium chloride
- Sodium
- Produces sodiumchloride
- Potassium
- Produces potassium chloride
- Group 1 reacts vigorously when heated in chlorine gas
- Reaction with oxygen
- They react with oxygen to make a metal oxide which differs depending on the metal
- Oxide - one oxygen atom
- Peroxide- two oxygen atoms
- Superoxide- three oxygen atoms
- Reacting with oxygen is why group 1 metals tarnish in the air
- Sodium
- Makes a mixture of sodium oxide and sodium peroxide
- Lithium
- Makes lithium oxide
- Potassium
- Makes a mixture of potassium peroxide and potassium superoxide
- They react with oxygen to make a metal oxide which differs depending on the metal
- They are :
- Group 7 Elements
- Known as the halogens
- They are :
- Fluorine
- Chlorine
- Bromine
- Iodine
- Astatine
- They all exist in pairs of atoms
- They are :
- They are all non-metals with coloured vapours
- Fluorine- Very reactive poisonous yellow gas
- Chlorine- Fairly reactive poisonous dense green gas
- Bromine- Dense poisonous, red-brown volatile liquid
- Iodine- Dark grey crystalline solid or a purple vapour
- As you go down Group 7 they...
- Are less reactive
- It is harder to gain an extra electron because the shells are further away from the nucleus
- Higher melting and boiling points
- Are less reactive
- They bond by ionic bonding and covalent bonding
- Ionic bonding with metals
- They form 1- ions called halides
- Covalent bonding with other non-metals
- Ionic bonding with metals
- Displacementreactions can happen between a more reactive halogen and the salt of a less reactive one
- Eg. chlorine reacts with potassium iodide and will displace iodine to make iodine and potassium chloride
- Known as the halogens
- Group 0 elements
- Also known as noble gases
- They are:
- Helium
- Neon
- Argon
- Krypton
- Radon
- They are:
- They have a full outer shell
- This means that they don't want to give up or gain electrons
- This means that they are inert- unreactive
- This also means that they are non-flammable
- This means that they are inert- unreactive
- This means that they don't want to give up or gain electrons
- As you go down the group the boiling points increase
- Because more electrons in the atom leads to greater intermolecular forces which need to be overcome
- They are monatomic gases- travel alone.
- Colourless gases at room temperature.
- Also known as noble gases
- Transitionmetals
- Comparison to Group 1
- Group 1 metals are more reactive than transition metals
- Transition metals are denser, stronger and harder than group 1.
- They have lower melting points
- For example manganese melts at 2000C but sodium melts at 98C
- Except for mercury which is a liquid at room temperature
- These are metals in the middle of the periodic table
- Can form ions with different charges
- Eg. Coppercan form Cu+ and Cu2+ ions
- They are often used as catalysts
- They form coloured compounds
- Eg. Potassium chromate(VI) is yellow and potassium(VII) manganate is purple
- Comparison to Group 1
- How it is organised
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