QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for NH^2− .
What is the electronic geometry?
What is the molecular geometry?
Is the molecule polar or non-polar?
What is the hybridization?
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Answer
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Step 1:: Determine the total number of valence electrons in the NH^2− ion.
The nitrogen atom (N) is in the 5th period and group 15 of the periodic table, so it has 5 valence electrons. The hydrogen atoms (H) each have 1 valence electron, and there are two of them. The negative charge on the ion adds one additional electron. Therefore, the total number of valence electrons is: \text{Total valence electrons} = 5 (\text{N}) + 2 (2 \times 1 (\text{H})) + 1 (\text{negative charge}) = 8 \text{ valence electrons}
Step 2:: Draw the Lewis structure for the NH^2− ion.
Step 3:
Place the nitrogen atom (N) in the center of the structure.
Step 4:
Place the two hydrogen atoms (H) around the nitrogen atom, each sharing one electron with the nitrogen atom.
Step 5:
Place the remaining 4 electrons as lone pairs on the nitrogen atom.
Step 6:
Add a negative charge to the ion. The Lewis structure for NH^2− is: ```lua H : N : H -
Final Answer
Add a negative charge to the ion. The Lewis structure for NH^2− is: ```lua H : N : H -
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