To answer the question "Zn, Cd, and Hg do not show most of the properties of which of the following elements?", we need to analyze the electronic configurations and properties of these elements.
### Step-by-Step Solution:
1. **Identify the Elements**:
- The elements in question are Zinc (Zn), Cadmium (Cd), and Mercury (Hg).
2. **Determine the Electronic Configurations**:
- **Zinc (Zn)**: Atomic number 30, electronic configuration is [Ar] 4s² 3d¹⁰.
- **Cadmium (Cd)**: Atomic number 48, electronic configuration is [Kr] 5s² 4d¹⁰.
- **Mercury (Hg)**: Atomic number 80, electronic configuration is [Xe] 6s² 4f¹⁴ 5d¹⁰.
3. **Identify the Block of Elements**:
- These elements belong to the d-block of the periodic table, which consists of transition metals.
4. **Understand the Properties of Transition Metals**:
- Transition metals are characterized by having partially filled d-orbitals, which allow them to exhibit variable oxidation states, form colored compounds, and act as catalysts.
5. **Analyze the Properties of Zn, Cd, and Hg**:
- Zn, Cd, and Hg have fully filled d-orbitals (3d¹⁰ for Zn, 4d¹⁰ for Cd, and 5d¹⁰ for Hg).
- Because of this, they do not exhibit the typical properties of transition metals, such as variable oxidation states and the ability to form colored compounds.
6. **Conclusion**:
- Therefore, Zn, Cd, and Hg do not show most of the properties of transition metals.
### Final Answer:
Zn, Cd, and Hg do not show most of the properties of transition elements.
