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Draw the Lewis Structure for ClO4- (Perchlorate Ion) - Class 11 Chemistry Video Lecture
FAQs on Draw the Lewis Structure for ClO4- (Perchlorate Ion) - Class 11 Chemistry Video Lecture
| 1. How do you draw the Lewis Structure for ClO4- (Perchlorate Ion)? |  |
Ans. To draw the Lewis Structure for ClO4- (Perchlorate Ion), we first determine the total number of valence electrons. Chlorine (Cl) contributes 7 valence electrons, and each oxygen (O) contributes 6 valence electrons. Since there are four oxygen atoms, the total number of valence electrons is 7 + (6 * 4) + 1 (extra electron due to the negative charge) = 32.
Next, we arrange the atoms, with chlorine (Cl) at the center and the four oxygen (O) atoms surrounding it. Each oxygen atom forms a single bond with the central chlorine atom, and each oxygen atom also has two lone pairs of electrons. The remaining electrons are placed on the chlorine atom, ensuring that it satisfies the octet rule.
The final Lewis Structure for ClO4- is as follows:
O
/
Cl-O
\
O
| 2. What is the charge on ClO4- (Perchlorate Ion)? | |
Ans. The charge on ClO4- (Perchlorate Ion) is -1. This means that the ion has one extra electron compared to the number of valence electrons in the neutral ClO4 molecule.
| 3. What is the shape of ClO4- (Perchlorate Ion)? | |
Ans. The shape of ClO4- (Perchlorate Ion) is tetrahedral. The central chlorine atom is surrounded by four oxygen atoms, which are arranged in a tetrahedral geometry.
| 4. What is the hybridization of the central chlorine atom in ClO4- (Perchlorate Ion)? | |
Ans. The central chlorine atom in ClO4- (Perchlorate Ion) undergoes sp3 hybridization. This means that one 3s orbital and three 3p orbitals of chlorine mix to form four sp3 hybrid orbitals, which are involved in bonding with the four oxygen atoms.
| 5. Is ClO4- (Perchlorate Ion) polar or nonpolar? | |
Ans. ClO4- (Perchlorate Ion) is a polar molecule. The oxygen atoms are more electronegative than the chlorine atom, which leads to an uneven distribution of electron density. This results in a net dipole moment, making the molecule polar.
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Dec 26, 2024 Last updated |
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