AQA AS Chemistry INORGANIC
Study online at https://quizlet.com/_69tzn0
1. Write the simplest ionic Cl2 + 2I- —> 2Cl- + I2
equation for when chlo-
rine water reacts with aq
potassium iodide soluion
2. Define periodicity A REPEATING pattern/trend for all periods of physical/chemical prop-
erties
3. for group 2, what happens As you go down a group, reactivity INCREASES because atomic radius
to reactivity and why? increases, weaker EFA and electron easier to remove
4. Colour of fluorine pale yellow gas
5. colour of chlorine pale green gas
6. Colour of bromine and Br2 ’Browny orange liquid
bromide Br- ’ions Yellow solution
7. Colour of iodine solid Black
8. which is the best oxidising Fluorine
agent of group 7? Why? Most electronegative element (smallest size, least shells and shield-
ing) therefore easily gains electrons
9. which is the strongest re- iodide ions
ducing agent of the halide Highest ionic radius, most shells and shielding, so least EFA therefore
ions? WHY? more easily loses electrons
10. Define disproportionation The simultaneous oxidation and reduction of the same species
11. how to test for ammonium
compounds (include eq)
, AQA AS Chemistry INORGANIC
Study online at https://quizlet.com/_69tzn0
12. Test for sulfates (include
eq)
13. What is an exception for Mg, is MUCH lower than expected because of a structural difference
group 2 melting points compared to other group 2 metals
14. Write ionic equation for Ba (2+) (aq) + SO4 (2-) (aq) --> BaSO4 (s)
formation of BaSO4
15. Write the ionic equation H+ (aq) + OH- (aq) --> H2O (l)
for a neutralisation reac-
tion.
16. Define reducing agent •Readily donates electrons
•Substance that is oxidised
17. Define oxidizing agent something that removes electrons from something else and itself is
reduced
18. Why does group 4 have -giant covalent (strong) macromolecular lattice structure that needs
the highest melting point? lots of energy to break
19. Describe melting point group 1 - 3: increases (because metallic bonding strengthens as
across a period more delocalised electrons and smaller ionic radius)
group 4: peaks (because strong macromolecular lattice covalent
structure)
group 5 - 8: decreases (because weak(er) simple molecular struc-
ture)
20. Describe electrical con- increases up to group3 and then decreases
ductivity across a period
Study online at https://quizlet.com/_69tzn0
1. Write the simplest ionic Cl2 + 2I- —> 2Cl- + I2
equation for when chlo-
rine water reacts with aq
potassium iodide soluion
2. Define periodicity A REPEATING pattern/trend for all periods of physical/chemical prop-
erties
3. for group 2, what happens As you go down a group, reactivity INCREASES because atomic radius
to reactivity and why? increases, weaker EFA and electron easier to remove
4. Colour of fluorine pale yellow gas
5. colour of chlorine pale green gas
6. Colour of bromine and Br2 ’Browny orange liquid
bromide Br- ’ions Yellow solution
7. Colour of iodine solid Black
8. which is the best oxidising Fluorine
agent of group 7? Why? Most electronegative element (smallest size, least shells and shield-
ing) therefore easily gains electrons
9. which is the strongest re- iodide ions
ducing agent of the halide Highest ionic radius, most shells and shielding, so least EFA therefore
ions? WHY? more easily loses electrons
10. Define disproportionation The simultaneous oxidation and reduction of the same species
11. how to test for ammonium
compounds (include eq)
, AQA AS Chemistry INORGANIC
Study online at https://quizlet.com/_69tzn0
12. Test for sulfates (include
eq)
13. What is an exception for Mg, is MUCH lower than expected because of a structural difference
group 2 melting points compared to other group 2 metals
14. Write ionic equation for Ba (2+) (aq) + SO4 (2-) (aq) --> BaSO4 (s)
formation of BaSO4
15. Write the ionic equation H+ (aq) + OH- (aq) --> H2O (l)
for a neutralisation reac-
tion.
16. Define reducing agent •Readily donates electrons
•Substance that is oxidised
17. Define oxidizing agent something that removes electrons from something else and itself is
reduced
18. Why does group 4 have -giant covalent (strong) macromolecular lattice structure that needs
the highest melting point? lots of energy to break
19. Describe melting point group 1 - 3: increases (because metallic bonding strengthens as
across a period more delocalised electrons and smaller ionic radius)
group 4: peaks (because strong macromolecular lattice covalent
structure)
group 5 - 8: decreases (because weak(er) simple molecular struc-
ture)
20. Describe electrical con- increases up to group3 and then decreases
ductivity across a period
