Use the References to access important values if needed for this question. 1 What is the total number of valence electrons in the Lewis structure of SF? electrons 2 Draw a Lewis structure for SF6. • Do not include overall ion charges or formal charges in your drawing. • If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. M... с #[ ] در ?
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
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### Lewis Structure of \( \text{SF}_6 \)
#### 1. Determining Valence Electrons
**Question:**
What is the total number of valence electrons in the Lewis structure of \( \text{SF}_6 \)?
**Answer:**
\[ \_\_\_\_\_ \text{ electrons} \]
#### 2. Drawing the Lewis Structure for \( \text{SF}_6 \)
**Instructions:**
* **Do not include overall ion charges or formal charges in your drawing.**
* **If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule.**
**Drawing Area:**
Below the instructions, there is a drawing area where you can sketch the Lewis structure. This area is equipped with various tools for drawing atoms, bonds, and other necessary chemical symbols. The available tools include:
* A hand tool for selecting and moving items.
* An eraser to remove mistakes.
* Several types of bonds (single, double, triple) and electron pair notations.
* Elements from the periodic table to select and place atoms.
Use these tools to construct the Lewis structure of \( \text{SF}_6 \) by ensuring sulfur is the central atom surrounded by six fluorine atoms, connected via single bonds.
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**Note:** Remember, in \( \text{SF}_6 \), sulfur can accommodate more than eight electrons in its valence shell due to having access to the d-orbital. Therefore, sulfur can form six single bonds with six fluorine atoms.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a2edb2f-7c78-40b5-b7fe-b2ef3d716529%2F0c97de69-7464-4559-80b1-86d5e3824c35%2Fo7ct9wq_processed.png&w=3840&q=75)
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