8.2 Chemical Earth Research Paper
8.2 Chemical Earth
8.2.1 The living and non-living components of the Earth contain mixtures * Construct word and balanced formulae equations of chemical reactions as they are encountered
Combustion reaction (burning) element + oxygen → oxide
e.g. 4Na (S) + O2 (g) → Na2O (s)
Reaction with hydrogen element + hydrogen → hydride
e.g. Ca (s) + H2 (g) → CaH2 (s)
Reaction between an oxide and water metallic oxide + water → hydroxide
* metallic oxide is also known as “basic oxide”
e.g. Na2O (s) + H2O (l) → 2NaOH (aq) non-metallic oxide + water → acid
* non-metallic oxide is known as “acidic oxide”
e.g. SO2 (g) + H2O (l) → H2SO3 (aq)
Reaction between active metals and water active metal + water (liquid or gas) → hydroxide + hydrogen gas
e.g. 2K (s) + 2H2O (l) → 2KOH (aq) +H2 (g) …show more content…
Thermal decomposition of gold oxide * 2. Light decomposition (photolysis) of silver bromide * 3. Electrolytic decomposition of molten lead (II) bromide * Synthesis reaction is the formation of a compound from its elements or a more complex compound from simpler compounds. * Application of decomposition reaction in the real world: * Rust is an oxide of iron that forms when iron structures are exposed to oxygen in the air. * The ammonia industry synthesises ammonia directly by combining nitrogen and hydrogen gases at high temperatures and pressures over a catalyst. * Examples: * 1. Synthesis of iron (III) chloride using heat energy * 2. Synthesis of hydrogen chloride using light * Explain that the amount of energy needed to separate atoms in a compound is an indication of the strength of the attraction, or bond, between them
The stronger the chemical bonding in a compound, the more energy is required to break the compound into atoms. Alternatively, the stronger the chemical bonding in a compound the more energy is released when the compound is formed from its
8.2.1 The living and non-living components of the Earth contain mixtures * Construct word and balanced formulae equations of chemical reactions as they are encountered
Combustion reaction (burning) element + oxygen → oxide
e.g. 4Na (S) + O2 (g) → Na2O (s)
Reaction with hydrogen element + hydrogen → hydride
e.g. Ca (s) + H2 (g) → CaH2 (s)
Reaction between an oxide and water metallic oxide + water → hydroxide
* metallic oxide is also known as “basic oxide”
e.g. Na2O (s) + H2O (l) → 2NaOH (aq) non-metallic oxide + water → acid
* non-metallic oxide is known as “acidic oxide”
e.g. SO2 (g) + H2O (l) → H2SO3 (aq)
Reaction between active metals and water active metal + water (liquid or gas) → hydroxide + hydrogen gas
e.g. 2K (s) + 2H2O (l) → 2KOH (aq) +H2 (g) …show more content…
Thermal decomposition of gold oxide * 2. Light decomposition (photolysis) of silver bromide * 3. Electrolytic decomposition of molten lead (II) bromide * Synthesis reaction is the formation of a compound from its elements or a more complex compound from simpler compounds. * Application of decomposition reaction in the real world: * Rust is an oxide of iron that forms when iron structures are exposed to oxygen in the air. * The ammonia industry synthesises ammonia directly by combining nitrogen and hydrogen gases at high temperatures and pressures over a catalyst. * Examples: * 1. Synthesis of iron (III) chloride using heat energy * 2. Synthesis of hydrogen chloride using light * Explain that the amount of energy needed to separate atoms in a compound is an indication of the strength of the attraction, or bond, between them
The stronger the chemical bonding in a compound, the more energy is required to break the compound into atoms. Alternatively, the stronger the chemical bonding in a compound the more energy is released when the compound is formed from its