In which of the following arrangements, the order is according to the property indicated against it?

Options

A. Basic strenght:`SbH_(3) gt AsH_(3) gt PH_(3) gt NH_(3)`
B. `IE_(1):N gt O gt C gt B`.
C. Oxidising power : `PbO_(2) gt SnO_(2) gt SiO_(2) gt CO_(2)`
D. Acid strength: `HI gt HCl gt HF`

Explanation

To determine the correct arrangement of compounds based on the indicated properties, we will analyze each option step by step.

### Step 1: Analyze Basic Strength
The first arrangement given is for basic strength: \( \text{SbH}_3, \text{AsH}_3, \text{PH}_3, \text{NH}_3 \).

1. **Understanding Basic Strength**: Basic strength generally decreases down a group in the periodic table due to the increase in atomic size, which leads to a decrease in electron density and the ability to donate electrons.
2. **Order of Basic Strength**:
- \( \text{NH}_3 \) (ammonia) has the highest basic strength due to its small size and high electron density.
- \( \text{PH}_3 \) (phosphine) is next as it is larger than ammonia but still has some basic character.
- \( \text{AsH}_3 \) (arsine) follows, as it is larger than phosphine.
- \( \text{SbH}_3 \) (stibine) has the least basic strength due to its larger size and lower electron density.

**Conclusion**: The correct order of basic strength is \( \text{NH}_3 > \text{PH}_3 > \text{AsH}_3 > \text{SbH}_3 \).

### Step 2: Analyze Ionization Energy
The second arrangement is for ionization energy: \( \text{B}, \text{C}, \text{N}, \text{O} \).

1. **Understanding Ionization Energy**: Ionization energy generally increases across a period from left to right due to increasing nuclear charge and decreasing atomic radius.
2. **Order of Ionization Energy**:
- \( \text{N} \) has a higher ionization energy than \( \text{O} \) due to its half-filled 2p subshell, which is more stable and requires more energy to remove an electron.
- The order is \( \text{N} > \text{O} > \text{C} > \text{B} \).

**Conclusion**: The correct order of ionization energy is \( \text{N} > \text{O} > \text{C} > \text{B} \).

### Step 3: Analyze Oxidizing Power
The third arrangement is for oxidizing power: \( \text{PbO}_2, \text{SnO}_2, \text{SiO}_2, \text{CO}_2 \).

1. **Understanding Oxidizing Power**: The oxidizing power generally decreases down a group as the stability of higher oxidation states decreases.
2. **Order of Oxidizing Power**:
- \( \text{PbO}_2 \) has the highest oxidizing power as lead in +4 oxidation state can easily reduce to +2.
- \( \text{SnO}_2 \) follows, then \( \text{SiO}_2 \), and finally \( \text{CO}_2 \) has the least oxidizing power.

**Conclusion**: The correct order of oxidizing power is \( \text{PbO}_2 > \text{SnO}_2 > \text{SiO}_2 > \text{CO}_2 \).

### Step 4: Analyze Acid Strength
The fourth arrangement is for acid strength: \( \text{HF}, \text{HCl}, \text{HBr}, \text{HI} \).

1. **Understanding Acid Strength**: Acid strength increases down the group due to the weakening of the H-X bond as the size of the halogen increases.
2. **Order of Acid Strength**:
- \( \text{HI} \) is the strongest acid, followed by \( \text{HBr} \), \( \text{HCl} \), and \( \text{HF} \) being the weakest.

**Conclusion**: The correct order of acid strength is \( \text{HI} > \text{HBr} > \text{HCl} > \text{HF} \).

### Final Summary
1. Basic Strength: \( \text{NH}_3 > \text{PH}_3 > \text{AsH}_3 > \text{SbH}_3 \)
2. Ionization Energy: \( \text{N} > \text{O} > \text{C} > \text{B} \)
3. Oxidizing Power: \( \text{PbO}_2 > \text{SnO}_2 > \text{SiO}_2 > \text{CO}_2 \)
4. Acid Strength: \( \text{HI} > \text{HBr} > \text{HCl} > \text{HF} \)