C4.1 Predicting Chemical Reactions

Column on the far left of the periodic table Alkali metals as they react with water to form alkaline solutions Shiny when freshly cut Good conductors of electricity Solid at room temperature Soft Density increases going down the group Melting point decreases going down the group React rapidly with oxygen in air and water so stored in oil 1 electron in the outer shell, lose it in reactions, forming 1+ charge ion Ionic equation: M -> M+ + e- Easier to lose its outer electron, the more reactive the element is Reactivity increases going down the group

Typical properties of non metals, brittle, poor conductor of electricity Diatomic molecules with weak intermolecular forces Density increases down the group Melting points and boiling points increase down the group Called halogens as they react with metals to make salts Reactivity decreases going down the group 7 electrons in the outermost shell The easier it is for a halogen to gain an outer electron, the more reactive it is

Halogens react with halides in solution Halogen will displace a less reactive halogen from its halide ions in solution The more reactive halide gives an electron to the less reactive halide

Compound containing a halogen and another element, typically hydrogen or a metal

Column on far right of periodic table Unreactive Full outer shell All noble gases have 8 electrons in their outer shell except for helium with 2 electrons Monatomic Single atoms with weak forces of attraction between them Very low boiling points Attractive forces get stronger down the group Boiling point increases down the group Density increases down the group Low densities

Between groups 2 and 3 All metals so they are shiny when freshly cut, good conductors of electricity, strong, malleable Stronger and harder than group 1 Higher densities than group 1 Higher melting points than group 1 (except mercury) Less reactive than alkali metals Can form positive ions of more than 1+ Uses: Good catalysts as they are inert Used to stain glass, colour paint, glaze pottery

Metals form positive ions in reactions, more easily this happens, more reactive the metal Metal reacts if it is more reactive than hydrogen (before copper on reactivity series) Forms metal hydroxide and hydrogen Metals react with acids to produce a salt and hydrogen

More reactive metal can displace a less reactive metal from solutions or its compounds

Reactivity of metal Rate of hydrogen production

Elements in group 0 don’t react Reactive non-metals may form covalent bonds with each other Metals may form ionic compounds with reactive non-metals Metals in group 1 and 2 are more reactive than transition metals and other metals Metals in group 1 and 2 become reactive down the group Non metals in group 7 become less reactive down the group

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