Draw a Lewis structure for NH4* and answer the following questions based on your drawing. 1. For the central nitrogen atom: The number of lone pairs The number of single bonds = The number of double bonds= 2. The central nitrogen atom A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet. 4
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.
![**Lewis Structures**
Lewis Structures are used to describe the covalent bonding in molecules and ions.
**Task:**
Draw a Lewis structure for \( \text{NH}_4^+ \) and answer the following questions based on your drawing.
1. For the central nitrogen atom:
- The number of lone pairs = [ ]
- The number of single bonds = [ ]
- The number of double bonds = [ ]
2. The central nitrogen atom:
- A. Obeys the octet rule
- B. Has an incomplete octet
- C. Has an expanded octet
**Instructions:**
- Click "Submit Answer" after filling in your responses.
- You have 9 more group attempts remaining.
(Note: The task involves understanding Lewis structures, which represent molecules, focusing on lone pairs and bonding. For \( \text{NH}_4^+ \), the nitrogen atom typically forms single bonds with hydrogen atoms without double bonds or lone pairs.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F32bd268b-b979-4081-864c-934854ccb129%2Fdf90bced-79f0-4a5f-b2ec-2948314c07e4%2F2lf42oa_processed.jpeg&w=3840&q=75)
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