The Periodic Table
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- Created on: 13-10-20 15:02
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- The Periodic Table
- The Periodic Table
- metalloids are after transition metals (B, Si, Ge, As, Sb, Te)
- Metallic Properties
- metallic structure is regular lattice of cations and sea of delocalised electrons
- elements on the left are metals as they have lower ionisation energies
- Large atomic radii, low ionisation energy, less exothermic electron affinity, low electronegativity
- Electron Configurations
- group number = valence electrons
- period number = number of main energy levels
- s-block = group 1 and 2. p-block = groups 13-18. d-block = transition metals
- Physical Properties
- Atomic Radius
- Half the internuclear distance of a molecules of an element
- increases down the group as more orbitals
- Decreases across period as charge increases
- Ionic Radius
- ionic radius of positive ions is smaller and ionic radius of negative ions is larger
- less electron electron repulsion in cations
- More electron electron repulsion in anions
- the greater the charge the smaller / bigger the radius
- ionic radius of positive ions is smaller and ionic radius of negative ions is larger
- First Ionisation Energy
- decreases down the group as atomic radii increases
- increases across a period because nuclear charge increases
- First Electron Affinity
- Exothermic for most elements
- more exothermic across the period due to increase charge and decrease in atomic radius
- decreases down the group because radius increases
- Exothermic for most elements
- Electronegativity
- Decreases down a group as atomic radii increase
- Increases across a period as increased radius is smaller
- Group 1
- Alkali metals
- Highly reactive, soft, low melting point
- melting point decreases down the group as ions get larger
- Reactions more vigorous down the group
- React rapidly with oxygen and tarnish in air
- Form basic, soluble oxides
- React with water to form a metal hydroxide and hydrogen gas
- Group 17
- Halogens
- Diatomic molecules
- Melting point increases down the group
- masses increase and London forces get stronger
- Reactivity decreases down the group
- decrease in electron affinity
- React with alkali metals to form salts
- Salts usually white or colourless
- chloride, bromides and iodides soluble in water to form colourless neutral solutions
- Salts usually white or colourless
- Oxides of Period 2 and 3
- metallic oxides are basic, non-metallic oxides are acidic
- Aluminium oxide is amphoteric
- Magnesium oxide is not very soluble as it have high charges on the ions
- NO and N2O are neutral
- NO can be oxidised in the atmosphere to NO2 which can react with water to produce nitric acid
- metallic oxides are basic, non-metallic oxides are acidic
- Atomic Radius
- The Periodic Table
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