Topic 4 Inorganic Chem Flashcards
Most reactive group 2 metal
Barium, at bottom
3 physical properties of group 2 metals
High melting and boiling points
Low density
Form white compounds
How does reactivity change down group 2 and why
Increases as electrons are lost more easily
What happens to first ionisation energy down g2 and why
Decreases:
Shielding increases
Increased atomic radius
Lower effective nuclear charge
What kind of reaction do G2 elements have with oxygen
Redox reaction
Mg + Water
Cold - No reaction
Hot - MgOH + Hydrogen
Steam - MgO + Hydrogen
Which G2 doesnt react with water
Beryllium
Products of G2 oxide + Dilute Acid
Salt and Water
Product of G2 oxide + water
Metal Hydroxide
Solubility of hydroxides g2
Increases down the group
Mg(OH)2 is sparingly soluble
Solubility of sulphates
Decreases down the group
G2 hydroxide + dilute acid
salt (-ate) + water
Reason for trend in thermal stability of G1 and G2 Carbonates and nitrates
G2 more thermally stable as you go down group. Cations get bigger so have less of a polarising effect on the carbonate. C-O bond is not weakened so is harder to break down.
G1 carbonates only lithium decomposes. Only lithium has high enough charge densitiy
2 Properties of halogens
low melting and boiling points
Exist as diatomic molecules
Trend in boiling point in halogens - why?
Increases down the group as the size of the atom increases and therefore there are stronger london forces between molecules
Trend in oxidising agent ability down group 7
Decreases as Cl has the strongest enc so best acceptor so reduces best so best oxidising agent
Trend in reducing agent ability of halides
Increases down the group. I has the weakest enc so will lose electrons easiest
Displacement reaction for halogens
when more reactive displaces less
Color of chlorine in water and organic solvent
pale green/yellow , pale green/yellow
Color of bromine in water and organic solvent
orange, orange
color of iodine in water and organic solvent
brown, violet
Chlorine with water reaction
Disproportionation
HCl+ HClO formed
Chlorine + Cold, dilute alkali
NaClO formed - Bleach
Chlorine + Hot, dilute alkali
NaClO3 formed
