Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of neutral NBr3?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
After drawing the Lewis structure of CHF, determine whether the molecule is polar or nonpolar.
A
Polar
B
Nonpolar
C
Cannot be determined
D
Ionic
Verified step by step guidance1
Step 1: Draw the Lewis structure of CHF by first counting the total valence electrons. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, and fluorine (F) has 7, giving a total of 12 valence electrons.
Step 2: Arrange the atoms with carbon as the central atom, since it is less electronegative than fluorine. Connect carbon to hydrogen and fluorine with single bonds, using 2 electrons per bond.
Step 3: Complete the octet for fluorine by adding the remaining electrons as lone pairs around it. Carbon will have 8 electrons around it (including bonding pairs), and hydrogen will have 2 electrons (bonding pair).
Step 4: Determine the molecular geometry around the central carbon atom. Since carbon is bonded to two atoms and has no lone pairs, the shape is linear.
Step 5: Assess the polarity by considering the difference in electronegativity between carbon, hydrogen, and fluorine. Fluorine is highly electronegative, creating a dipole moment. Because the molecule is linear but the atoms bonded are different, the dipoles do not cancel, making CHF a polar molecule.
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