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The shape of ClO₃⁻ according to valence shell electron repulsion theory will be
- a)Planar triangle
- b)Pyramidal
- c)Tetrahedral
- d)Square planar
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
The shape of ClO₃⁻ according to valence shell electron repulsion theor...
Explanation:
Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the shapes of molecules based on the repulsion between their valence electrons. According to VSEPR theory, the ClO₃⁻ ion has a trigonal pyramid shape with a bond angle of approximately 107°.
Steps to determine the shape of ClO₃⁻ using VSEPR theory:
1. Determine the Lewis structure of ClO₃⁻:
- Chlorine (Cl) has 7 valence electrons and oxygen (O) has 6 valence electrons.
- There are three oxygen atoms bonded to the central Cl atom in ClO₃⁻.
- The total number of valence electrons is 7 + (3 x 6) + 1 = 22.
- The Lewis structure of ClO₃⁻ is:
O
/ \
O O
| |
Cl O⁻
2. Determine the electron group geometry:
- The ClO₃⁻ ion has four electron groups around the central Cl atom (three single bonds and one lone pair of electrons).
- The electron group geometry is therefore tetrahedral.
3. Determine the molecular geometry:
- To determine the molecular geometry, we need to take into account the lone pair of electrons on one of the oxygen atoms.
- The lone pair of electrons repels the bonding pairs, causing the ClO₃⁻ ion to adopt a trigonal pyramid shape.
- The bond angle between the Cl-O bonds is approximately 107°.
Conclusion:
According to VSEPR theory, the ClO₃⁻ ion has a trigonal pyramid shape with a bond angle of approximately 107°.
Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the shapes of molecules based on the repulsion between their valence electrons. According to VSEPR theory, the ClO₃⁻ ion has a trigonal pyramid shape with a bond angle of approximately 107°.
Steps to determine the shape of ClO₃⁻ using VSEPR theory:
1. Determine the Lewis structure of ClO₃⁻:
- Chlorine (Cl) has 7 valence electrons and oxygen (O) has 6 valence electrons.
- There are three oxygen atoms bonded to the central Cl atom in ClO₃⁻.
- The total number of valence electrons is 7 + (3 x 6) + 1 = 22.
- The Lewis structure of ClO₃⁻ is:
O
/ \
O O
| |
Cl O⁻
2. Determine the electron group geometry:
- The ClO₃⁻ ion has four electron groups around the central Cl atom (three single bonds and one lone pair of electrons).
- The electron group geometry is therefore tetrahedral.
3. Determine the molecular geometry:
- To determine the molecular geometry, we need to take into account the lone pair of electrons on one of the oxygen atoms.
- The lone pair of electrons repels the bonding pairs, causing the ClO₃⁻ ion to adopt a trigonal pyramid shape.
- The bond angle between the Cl-O bonds is approximately 107°.
Conclusion:
According to VSEPR theory, the ClO₃⁻ ion has a trigonal pyramid shape with a bond angle of approximately 107°.
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Community Answer
The shape of ClO₃⁻ according to valence shell electron repulsion theor...
It has one lone pair electron
( valence electron of chlorine+charge/2)
7+1/2=4
lone pair= 4-3(here 3 oxygen atom )
= 1
ClO3^- has 1 lone pair and 3 shared pair electron. so, pyramidal geometry.
( valence electron of chlorine+charge/2)
7+1/2=4
lone pair= 4-3(here 3 oxygen atom )
= 1
ClO3^- has 1 lone pair and 3 shared pair electron. so, pyramidal geometry.
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