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Chapter 1: Q16P (page 2)

Give each atom the appropriate formal charge:

Short Answer

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We have to give each atom appropriate formal charge:

Step by step solution

01

Lewis structure

1. A pair of shared electrons is shown by a line.

2. H- one covalent bond

Halogens- one covalent bond

O- two covalent bonds

N- three covalent bonds

C- four covalent bonds

02

Explanation final answer

a) Oxygen can form two covalent bonds then by increasing the bond it will get positive charge.

b) Carbon can form four covalent bonds then by decreasing the bond it will get negative charge.

c) Nitrogen can form three covalent bonds then by increasing the bond it will get positive charge.

d) Nitrogen and boron can form three covalent bonds then by increasing the bond it will get positive charge.

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Most popular questions from this chapter

For each of the given species:a. Draw its Lewis structure.b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.

1.H2CO2

2. HCN

3. CCl4

4. H2CO3

The compounds commonly known as “amino acids” are actually -aminocarboxylic acids (Section 21.0). What carbonyl compounds should be used to synthesize the two amino acids shown here?

Determine the partial negative charge on the fluorine atom in a C-F bond. The bond length is 1.39 1.39A* , and the bond dipole moment is 1.06D. The charge on an electron is 4.80⨯10-10esu.

Which of the following molecules would you expect to have a dipole moment of zero? To answer parts g and h, you may need to review the Problem Solving Strategy on p. 39.

Explain why HCI has a smaller dipole moment than HF,even though the H -CI bond is longer than the H-F bond.
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