To determine what is not applicable to \( \text{TeCl}_4 \) (Tellurium Tetrachloride), we will analyze its electronic configuration, bonding, and geometry step by step.
### Step 1: Identify the Group and Valence Electrons
- Tellurium (Te) belongs to Group 16 of the periodic table, which includes elements like Oxygen, Sulfur, Selenium, and Polonium.
- As a Group 16 element, Tellurium has 6 valence electrons.
**Hint:** Remember that elements in the same group of the periodic table have similar properties, including the number of valence electrons.
### Step 2: Determine Bonding with Chlorine
- In \( \text{TeCl}_4 \), Tellurium forms bonds with 4 Chlorine atoms.
- Since it has 6 valence electrons and forms 4 bonds, 4 of these electrons are used for bonding.
**Hint:** The number of bonds formed by an element can often be determined by the number of valence electrons it has.
### Step 3: Calculate Lone Pairs
- After forming 4 bonds with Chlorine, Tellurium will have 2 remaining valence electrons.
- These 2 electrons will form 1 lone pair.
**Hint:** The lone pairs are the electrons that are not involved in bonding and can affect the shape of the molecule.
### Step 4: Determine Steric Number
- The steric number is calculated as the number of bond pairs plus the number of lone pairs.
- In \( \text{TeCl}_4 \), there are 4 bond pairs (from the 4 \( \text{Te-Cl} \) bonds) and 1 lone pair.
- Therefore, the steric number is \( 4 + 1 = 5 \).
**Hint:** The steric number helps in predicting the hybridization and geometry of the molecule.
### Step 5: Determine Hybridization
- A steric number of 5 indicates that the hybridization is \( \text{sp}^3\text{d} \).
- This involves one s orbital, three p orbitals, and one d orbital.
**Hint:** Hybridization can be determined based on the steric number, which reflects the number of regions of electron density around the central atom.
### Step 6: Determine Molecular Geometry
- The geometry corresponding to \( \text{sp}^3\text{d} \) hybridization is trigonal bipyramidal.
- With one lone pair, the molecular shape becomes seesaw.
**Hint:** The presence of lone pairs can distort the ideal geometry, leading to different molecular shapes.
### Conclusion
From the analysis, we can conclude:
- The geometry of \( \text{TeCl}_4 \) is not tetrahedral; it is trigonal bipyramidal with a seesaw shape due to the lone pair.
- Therefore, the statement that \( \text{TeCl}_4 \) is tetrahedral is **not applicable**.
### Final Answer
The option that is not applicable to \( \text{TeCl}_4 \) is that it is tetrahedral in shape.
