Give the empirical formula for the ionic compounds formed between K, O and Na, p.

Answer

To determine the empirical formulas for the ionic compounds formed between potassium (K) and oxygen (O), as well as sodium (Na) and phosphorus (P), we can follow these steps:

### Step 1: Determine the Valence Electrons
- **Potassium (K)** is an alkali metal with **1 valence electron**.
- **Oxygen (O)** has **6 valence electrons**.
- **Sodium (Na)** is also an alkali metal with **1 valence electron**.
- **Phosphorus (P)** has **5 valence electrons**.

### Step 2: Formulate the Compound Between K and O
1. **Potassium (K)** will lose its 1 valence electron to achieve a stable electronic configuration, resulting in a **K⁺ ion**.
2. **Oxygen (O)** needs 2 electrons to complete its octet, so it will gain 2 electrons, resulting in an **O²⁻ ion**.
3. To balance the charges, we need **2 potassium ions** for every **1 oxide ion**:
- 2 K⁺ + O²⁻ → K₂O

### Step 3: Write the Empirical Formula for K and O
- The empirical formula for the ionic compound formed between potassium and oxygen is **K₂O**.

### Step 4: Formulate the Compound Between Na and P
1. **Sodium (Na)** will lose its 1 valence electron to become a **Na⁺ ion**.
2. **Phosphorus (P)** needs 3 electrons to complete its octet, so it will gain 3 electrons, resulting in a **P³⁻ ion**.
3. To balance the charges, we need **3 sodium ions** for every **1 phosphide ion**:
- 3 Na⁺ + P³⁻ → Na₃P

### Step 5: Write the Empirical Formula for Na and P
- The empirical formula for the ionic compound formed between sodium and phosphorus is **Na₃P**.

### Final Answer
- The empirical formulas are:
- For K and O: **K₂O**
- For Na and P: **Na₃P**

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