Chemistry- Definitions and key terms

Definitions and key terms

aluminium oxide

Al₂O₃

2Na_(s) + 2H₂O_(l) →

2NaOH_(aq)+H_2(g) (fizzing)

Sodium + cold water →

sodium hydroxide +hydrogen gas

magnesium +cold water →

magnesium hydroxide + hydrogen gas

Mg_(s)+ H₂O_(g)→

MgO_(s)+ H_2(g)

magnesium +oxygen → magnesium oxide

white flame and white solid smoke

sodium +oxygen → sodium oxide

yellow flame and white solid

Aluminium + oxygen → aluminium oxide

white flame and white solid smoke

Silicon + oxygen → silicon oxide

white flame and white solid smoke

Phosphorus + oxygen → phosphorous oxide

white flame and white solid smoke

Sulfur + oxygen → sulfur dioxide

blue flame and acidic choking gas

VO₂⁺

+5, yellow

VO²⁺

+4, blue

V³⁺

+2, green

V²⁺

violet

addition of zinc to vanadium

will reduce through successive oxidation state, going from yellow to violet

Lewis acid

electron pair donator

Lewis base

electron pair donator

metal ions with water

hydrated with H₂O ligands around central metal ions

weaker ions in solution

2⁺ ions, (Fe²⁺, Cu²⁺ ) as they dissociate

stronger ions in solution

3⁺ ions, (Fe³⁺, Al³⁺),

metal ions in solution

acidic

why are 3+ ions in solution stronger acids than 2+ ions?

they dissociate more and have a greater attractive power to OH^- (basic ions)

metal ions in solution + NaOH →

salt + water

neutralisation reaction

metal ions in solution act as acid

[Fe(H₂O)₆]²⁺ + 2OH^- →

[Fe(H₂O)₄(OH)₂] + 2H₂O

green precipitate formed

[Cu(H₂O)₆]²⁺ +2OH^- →

[Cu(H₂O)₄(OH)₂] + 2H₂O

blue precipitate

[Fe(H₂O)₆]³⁺ + 3OH^- →

[Fe(H₂O)₃(OH)₃] + 3H₂O

purple precipitate

[Al(H₂O)₆]³⁺ + 3OH^- →

[Al(H₂O)₃(OH)₃] +3H₂O

white precipitate