Group 17 Elements
Chapter Name : The P- Block Elements |
Sub Topic Code : 102_12_07_18_08 |
Topic Name : Group 17 Elements |
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Sub Topic Name : Chemical Properties |
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Introduction
• All the halogens exhibit –1 oxidation state. However, chlorine, bromine and iodine exhibit + 1, + 3, + 5 and + 7 oxidation states. • The oxidation states of +4 and +6 occur in the oxides and oxoacids of chlorine and bromine. • The fluorine atom has no d orbitals in its valence shell and therefore cannot expand its octet. • Being the most electronegative, it exhibits only –1 oxidation state. • All the halogens are highly reactive. They react with metals and non-metals to form halides. • F2 is the strongest oxidising halogen and it oxidises other halide ions in solution or even in the solid phase.
Pre-Requisites:
Periodic table, elements, chemical Properties
Activity:
See weeds have iodine in them.
Real Life Question:
Where does chlorine gas come from?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
|---|---|
| group | Group is the vertical column on the periodic table which contains elements having the similar properties. |
Learning aids / Gadgets
| Gadgets | How it can be used |
|---|---|
| Chlorine disinfectant | Chlorine is used as a disinfectant. |
Real life uses :
Chlorine is used as a disinfectant.
Places to visit :
Beach.
Practical examples around us
| Examples | Explainations |
|---|---|
| Sea weed, chlorine disinfectant | Sea weed has iodine in it. |
What you learn in Theory:
• All the halogens exhibit –1 oxidation state. However, chlorine, bromine and iodine exhibit + 1, + 3, + 5 and + 7 oxidation states. • The oxidation states of +4 and +6 occur in the oxides and oxoacids of chlorine and bromine. • The fluorine atom has no d orbitals in its valence shell and therefore cannot expand its octet. • Being the most electronegative, it exhibits only –1 oxidation state. • All the halogens are highly reactive. They react with metals and non-metals to form halides. • F2 is the strongest oxidising halogen and it oxidises other halide ions in solution or even in the solid phase.
What you learn in Practice:
• All the halogens exhibit –1 oxidation state. However, chlorine, bromine and iodine exhibit + 1, + 3, + 5 and + 7 oxidation states. • The oxidation states of +4 and +6 occur in the oxides and oxoacids of chlorine and bromine. • The fluorine atom has no d orbitals in its valence shell and therefore cannot expand its octet. • Being the most electronegative, it exhibits only –1 oxidation state. • All the halogens are highly reactive. They react with metals and non-metals to form halides. • F2 is the strongest oxidising halogen and it oxidises other halide ions in solution or even in the solid phase.