1.1- Formulae and Equations Flashcards
(a) Formulae of some common substances
Water
Oxygen
Hydrogen
Nitrogen
Carbon dioxide
Sulfur Dioxide
Hydrochloric acid
Sulfuric acid
Nitric acid
Sodium hydroxide
Sodium carbonate
Ammonia
Water- H₂O
Oxygen- O₂
Hydrogen- H₂
Nitrogen- N₂
Carbon dioxide- CO₂
Sulfur Dioxide- SO₂
Hydrochloric acid- HCl
Sulfuric acid- H₂SO₄
Nitric acid- HNO₃
Sodium hydroxide- NaOH
Sodium carbonate- Na₂CO₃
Ammonia- NH3
(a) Charges on some common ions
Ammonium
Hydroxide
Sulphate
Nitrate
Carbonate
Ammonium- NH4+
Hydroxide- OH-
Sulphate - SO42-
Nitrate- NO3-
Carbonate- CO32-
Oxidation numbers
Rules:
The oxidaton state of atoms in elements is always 0.
In compounds, the sum of the oxidation state is always 0.
In ions the sum of the oxidation states is equal to the charge on the ion.
(b)
Oxidation states
Rules:
Fluorine(F):
-1
Oxygen(O):
-2
Hydrogen(H):
+1 (except in H-)
Chlorine(Cl):
-1
(c)
Write an ionic equation for the reaction between nitric acid (HNO3 ) and sodium hydroxide (NaOH). Include state symbols.
Reaction equation: HNO3 + NaOH → NaNO3 + H2O
Rewrite the equation with the aqueous ions: H + + NO3 - + Na+ + OH- → Na+ + NO3 - + H2O
Cancel any ions appearing on both side to get the ionic equation and add in state symbols: H + (aq) + OH- (aq) → H2O(l)
(c)
Write an ionic equation for the reaction between silver nitrate and sodium chloride. Include state symbols.
Reaction equation: AgNO3 + NaCl → AgCl + NaNO3
Rewrite the equation with aqueous ions (note, AgCl is a solid): Ag+ + NO3 - + Na+ + Cl- → AgCl + Na+ + NO3 - Cancel any ions appearing on both side to get the ionic equation: Ag+ (aq) + Cl- (aq) → AgCl(s)
