Chemical Properties.

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Presentation transcript:

Chemical Properties

Syllabus Statements 3.3 Chemical properties 3.3.1 Discuss the similarities and differences in the chemical properties of elements in the same group. 3.3.2 Discuss the changes in nature, from ionic to covalent and from basic to acidic, of the oxides across period 3.

The IB expect you to be able to answer questions about: Group 0 – the noble gases Group I – the alkali metals Group VII – the halogens

Group VII – the halogens Fluorine – yellowish gas

Chlorine – pale yellow-green gas

Bromine – red-brown liquid (orange in solution)

Iodine – purple/black crystalline solid

The halogens are coloured (learn the colours!) They exist as diatomic elements, X2 Their melting and boiling points increase as you go down the group (gas liquid solid) They are very reactive Reactivity decreases as you go down the group (why?) They may form ionic compounds with metals, or covalent compounds with other non-metals.

Reaction with group I metals Halogens react with group I metals to form an ionic halide The halogen gains one electron from the metal to form a halide ion with a charge of 1- Electrostatic forces hold the halide ion and the metal ion together