General Principles And Processes Of Isolation Of Elements

Step 1: Understand the Structure of Ozone Molecule (O₃):
Ozone (O₃) is a molecule composed of three oxygen atoms. It has a bent structure, and the bonding in ozone involves both bonding pairs of electrons and lone pairs of electrons. The lone pairs are present on the central oxygen atom, and the bonding pairs are shared between the atoms.

Step 2: Determine the Electron Configuration in Ozone:
Ozone has a total of 18 valence electrons. These electrons are arranged as follows: - There are two bonds between the oxygen atoms, and one of the oxygen atoms has a lone pair of electrons. - The central oxygen atom has two lone pairs and forms two bonds with the outer oxygen atoms.

Step 3: Count the Lone Pairs and Bond Pairs:
- Lone pairs: The central oxygen atom in ozone has two lone pairs. - Bond pairs: There are three bond pairs between the oxygen atoms in the ozone molecule.

Step 4: Find the Ratio:
The ratio of lone pairs to bond pairs in the ozone molecule is:

Lone pairs : Bond pairs = 2 : 1

Final Answer:
The ratio of lone pairs to bond pairs of electrons in ozone molecule is 2:1.

Step 1: Understand the Statements:
We are given four statements about the oxides of halogens. Let's analyze them one by one:

Statement A: At room temperature, OF₂ is thermally stable.
This statement is incorrect. OF₂ is highly reactive and thermally unstable, decomposing easily at room temperature into oxygen and fluorine.

Statement B: The order of stability of oxides of halogens is I > Br > Cl.
This statement is correct. As we move down the halogen group, the oxides of iodine are more stable than those of bromine and chlorine. Iodine is the least electronegative halogen, leading to more stable oxides.

Statement C: I₂O₅ is used in the estimation of CO.
This statement is correct. Iodine pentoxide (I₂O₅) is used as an oxidizing agent in the estimation of carbon monoxide (CO).

Statement D: ClO₂ is used as a bleaching agent.
This statement is correct. Chlorine dioxide (ClO₂) is widely used as a bleaching agent, especially in paper and textile industries.

Step 2: Analyze the Correctness of Each Statement:
- Statement A is incorrect.
- Statement B is correct.
- Statement C is correct.
- Statement D is correct.

Final Answer:
The correct statements are B, C, and D.
Therefore, the correct option is A, C, and D only.

To solve the problem, we need to find the fractions of metal existing as and in the oxide with the formula .

1. Understand the oxidation states and formula:
Let the number of moles of be , and that of be . The total negative charge from 1 mole of oxygen atoms (as ) is -2. For the compound to be neutral, the total positive charge must also be +2.

2. Set up the equation for charge neutrality:

Simplifying:

3. Find the fractions:
Fraction of
Fraction of

Final Answer:
The fractions of metal that exist as and are 0.083 and 0.916 respectively.