Zusammenfassung der Ressource
Chemical Periodicity
- Periodicity is the repeating pattern of properties in elements.
- This regularity allows elements to be placed in groups
- Each element has similar, though gradually varying, properties
- These properties are both chemical and physical
- Electron structure
- Electrons orbit the nucleus at certain fixed distances- SHELLS
- Each shell can hold up a certain number of electrons
- Shell 1- 2 Electrons
- Shell 4- 2 Electrons
- Shell 3- 8 Electrons
- Shell 2- 8 Electrons
- Electrons fill up the nearest shells first
- Number of electrons in the outer shell= group number
- All chemical reactions are the result of changes in the outer shell of electrons
- All elements in a group have the same number of electrons in the outer shell
- Therefore elements in any group have similar characteristics
- However, as groups descends, more shells are added
- More shells means more distance from the positively charged nucleus
- Therefore it is harder to gain electrons but easier to lose them
- GROUP 0- NOBLE GASES
- Highly unreactive
- Do not form compounds
- Full outer shell of electrons
- Colourless gases
- Down the group they become
- Denser
- Gain a higher boiling point
- USES
- Helium
- Airships
- Party balloons
- Neon
- Filling gas discharge tubes for neon signs
- Cryogenic refrigeration
- Argon
- Inside lightbulbs to stop filament oxidation
- Food packaging to stop rotting
- Krypton
- Lasers
- Killing Superman
- Xenon
- Flash camera bulbs
- Strobe lights
- GROUP 1 ALKALI METALS
- Relatively low density
- Potassium, Sodium and Lithium float on water
- Shiny when first cut
- Tarnish rapidly upon oxidation
- Soft- can be cut by a knife
- Low melting points
- Silvery metals
- Caesium is pale-gold colour
- Very reactive- most reactive metal group
- Stored under oil or under Argon atmosphere
- They react with water to give Oxides
- They react with water to give Hydroxides AND Hydrogen
- These reactions are very vigorous
- Lithium fizzes around on the surface of the water and seems to dissolve
- Sodium fizzes around in a molten ball, appearing to dissolve
- This is because Sodium has a lower boiling point than Lithium AND the reaction is more exothermic
- Potassium fizzes around in a molten ball, igniting the Hydrogen from the reaction and producing a purple flame
- The presence of Hydroxide products can be shown using an indicator
- Hydroxides are alkaline, thus why the metals are also known as the 'alkali metals'
- As the group descends...
- The metals become more reactive
- Become softer
- Increase in density
- The metals want to lose an electron to have a full outer shell
- The further they are from the protons, the easier they can lose the electron
- The more shells they have, the further they are from the protons.
- As they descend the group, the become MORE reactive
- GROUP 7- THE HALOGENS
- Halogens are reactive non-metals
- They are diatomic molecules
- They have poisonous vapours
- Halogens and their properties
- Fluorine
- Pale yellow
- Highly toxic
- Very reactive
- GAS
- Chlorine, Cl2
- Pale green gas
- Dense
- Toxic
- GAS
- Bromine, Br2
- Dense
- Dark red
- LIQUID
- Gives off red/brown vapour
- Toxic and Corrosive
- Iodine
- Dark grey
- SOLID
- Sublimes to give a purple vapour
- Forms a brown solution in water and a purple one in Hexane
- Astatine is radioactive and very unstable
- They are ALL poor conductors of heat and electricity
- On descending the group...
- They become less reactive
- They are trying to ATTRACT electrons, unlike the Alkali metals
- This means they want to be nearer the protons and the nucleus
- Therefore they want fewer shells between them and the nucleus
- Their colour becomes darker
- Their melting and boiling points INCREASE