Topic 8- Group 7 Elements Part 2 Flashcards
How do halide ions become halogens?
What is this linked to?
What does it mean the larger the halide ion?
What is the reducing power like of halides?
What is the equation for the reaction of sodium chloride with concentrated sulfuric acid?
What type of fumes are produced?
What is this reaction not?
What is the chloride ion too weak to do?
Halide ions lose electrons to become halogens
Linked to size
The more easily it loses an electron
Increased reducing power as you go down the group
NaCl (s) + H2SO4 (l) —> NaHSO4 (s) + HCL (g)
Misty white fumes produced
Not a redox reaction
Chloride ion is too weak as a reducing agent to reduce the sulfur in sulfuric acid.
What is the first equation for the reaction of sodium bromide with concentrated sulfuric acid?
What is the second equation for the reaction of sodium bromide with concentrated sulfuric acid?
Describe the three gases produced in this reaction?
What two types of reactions is this reaction?
What is the first equation for the reaction of sodium iodide with concentrated sulfuric acid?
What is the second equation for the reaction of sodium iodide with concentrated sulfuric acid?
What is the third equation for the reaction of sodium iodide with concentrated sulfuric acid?
What is then produced if the reaction is then further reduced?
Describe the four gases produced in this reaction?
When do all of these reactions happen?
NaBr (s) + H2SO4 (l) —> NaHSO4 (s) + HBr (g)
2HBr + H2SO4 (l) —> SO2 (g) + 2H2O (l) + Br2 (l)
HBr- misty white fumes; SO2- choking gas; Br2- brown fumes
This reaction is both redox and exothermic
NaI (s) + H2SO4 (l) —> NaHSO4 (s) + HI (g)
2HI + H2SO4 (l) —> SO2 (g) + 2H2O (l) + I2 (s)
8HI + H2SO4 (l) —> H2S (g) + 4H2O (l) + 4 I2 (s)
Solid (yellow) sulfur is then produced
HI- misty fumes; SO2- choking gas; I2- purple fumes; H2S- bad egg smell
All of these reactions happen at the same time.
