CI CI...Si + A В D E (5

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Below is the perspective drawings for SiCl4.  Below the structure are arrows indicating the overall direction of polarity or a “0” if the molecule is non polar.  

**Molecular Polarity in Silicon Tetrachloride (SiCl₄)**

**Molecular Structure:**

The diagram displays the chemical structure of silicon tetrachloride (SiCl₄). A silicon (Si) atom is at the center with four chlorine (Cl) atoms bonded tetrahedrally around it. This symmetrical arrangement often suggests non-polarity due to the equal distribution of charge.

**Polarity Indicators:**

Below the molecular structure, there is a series of arrows labeled A to G, each representing potential dipole moments:

- **A:** No arrow, indicating no polarity.
- **B:** Arrow pointing right, with a positive sign (+) at the start.
- **C:** Diagonal arrow pointing upwards to the right, with a cross (x) at the end.
- **D:** Vertical arrow pointing upwards, with a positive sign (+) at the start.
- **E:** Vertical arrow pointing downwards, with a cross (x) at the top.
- **F:** Diagonal arrow pointing downwards to the left, with a cross (x) at the end.
- **G:** Arrow pointing left, with a positive sign (+) at the end.

**Question:**

What is the correct indication of polarity for this molecule?

**Analysis:**

Silicon tetrachloride is a symmetrical tetrahedral molecule. The dipoles of the Si-Cl bonds cancel each other out due to this symmetry, making the net dipole moment zero. Therefore, the correct answer is likely **A** (indicating no polarity).
Transcribed Image Text:**Molecular Polarity in Silicon Tetrachloride (SiCl₄)** **Molecular Structure:** The diagram displays the chemical structure of silicon tetrachloride (SiCl₄). A silicon (Si) atom is at the center with four chlorine (Cl) atoms bonded tetrahedrally around it. This symmetrical arrangement often suggests non-polarity due to the equal distribution of charge. **Polarity Indicators:** Below the molecular structure, there is a series of arrows labeled A to G, each representing potential dipole moments: - **A:** No arrow, indicating no polarity. - **B:** Arrow pointing right, with a positive sign (+) at the start. - **C:** Diagonal arrow pointing upwards to the right, with a cross (x) at the end. - **D:** Vertical arrow pointing upwards, with a positive sign (+) at the start. - **E:** Vertical arrow pointing downwards, with a cross (x) at the top. - **F:** Diagonal arrow pointing downwards to the left, with a cross (x) at the end. - **G:** Arrow pointing left, with a positive sign (+) at the end. **Question:** What is the correct indication of polarity for this molecule? **Analysis:** Silicon tetrachloride is a symmetrical tetrahedral molecule. The dipoles of the Si-Cl bonds cancel each other out due to this symmetry, making the net dipole moment zero. Therefore, the correct answer is likely **A** (indicating no polarity).
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