A3 Inorganic Chemistry Flashcards
How do all electronic configurations of Group 2 elements end
S (^2)
What happens to all group 2 elements in redox reactions
Oxidised to form 2+ ions
General symbol equation for Group 2 elements reacting with dilute acid
General symbol equation for Group 2 elements reacting with water
General symbol equation for Group 2 elements reacting with oxygen
State and explain the reactivity of Group 2 elements
- Reactivity increases down group
- More shells
- More sheilding
- Nuclur attraction decreases
- Ionisation energy decreases
- Less energy required to remove outer-shell electron
Down Group 2, what happens to elements reducing power
Strong reducing agents
State how solubility changes down the group and so the effect this has on the solution produced
- Solubility increases
- More alkaline solutions form
- Solutions have higher pH
General symbol equation for metal oxide reacting with water
What property of group 2 compounds make them useful
They are basic
What is the use of calcium hydroxide in commerce, and what is the equation
- Neutralise soil acids in agriculture
What is the use of magnesium hydroxide and calcium carbonate in commerce, and what are their equations
- Antacids to treat indigestion
What electronic configurations do all group 7 elements end with
s(^2)p(^5)
What happens to all group 7 elements in redox reactions
Reduced to form 1- ions
How do all group 7 elements exist
Diatomic molecules
Why does the boiling point of group 7 elements decrease down the group
- London forces become stronger
- More energy needed to break London forces
State and explain the trend in reactivity down the group 7
- Reactivity decreases
- More shells
- Atomic radius increases
- More sheilding
- Nuclear attraction decreases
- Ionisation energy decreases
- More energy required to attract outer-shell electron
Colour of chlorine regular
Colourless
Colour of chlorine aqueous
Colourless
Colour of chlorine organic
Colourless
Colour of bromine regular
Red-Brown
Colour of bromine aqueous
Orange
Colour of bromine organic
Brown
Colour of iodine regular
Dark grey
Colour of iodine aqueous
Orange
Colour of iodine organic
Violet
Define Disproportionation
The reduction and oxidation of the same element in the same reaction
Equation for chlorine reacting with cold, dilute aqeous sodium hydroxide, to form bleach
Chemical formula and name for bleach
- NaClO
- Sodium Chlorate (I)
When chlorine is used to form bleach, what are the conditions required for sodium hydroxide
- Cold
- Dilute
Equation for chlorine used for water treatment
Formula and name of acid created when chlorine is used for water treatment (not HCl)
- Chloric (I) acied
- HClO
Benefits of using chlorine for sterelising drinking water
Kills bacteria
Risks with using chlorine for sterelising drinking water
- Chlorine gas is toxic
- Chlorinated hydrocarbons formed which are carcinogenic
How to test for halide ions and result
- Add HNO3
- Add AgNO3
- Add ammonia
- Chloride ppt dissolved in dilute ammonia
- Bromide ppt dissolved in concentrated ammonia
- Iodide ppt insoluble in concentrated ammonia
Equation for halide ion test
How to test for carbonate ions, and result
- Add HCl
- Bubble gas through limewater
- Limewater turns cloudy
Equation for carbonate ion test
How to test for sulfate ions
- Add HCl to remove any carbonates
- Add BaCl2
- White ppt will form
Equation for sulfate ion test
How to test for ammonium ions and result
- Add NaOH
- Gently heat
- Ammonia gas produced
- Turns damp litmus blue
Equation for ammonium ion test
