Open Question
Write the electron configuration for Ne. Then write the Lewis symbol for Ne and indicate which electrons from the electron configuration are included in the Lewis symbol.
11. Bonding & Molecular Structure
Lewis Dot Symbols
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In the Lewis structure for Cl—F, how many valence electrons, bonding pairs, and lone pairs are present?
A
10 valence electrons, 1 bonding pair, 4 lone pairs
B
16 valence electrons, 1 bonding pair, 7 lone pairs
C
12 valence electrons, 2 bonding pairs, 5 lone pairs
D
14 valence electrons, 1 bonding pair, 6 lone pairs
Verified step by step guidance1
Step 1: Determine the number of valence electrons for each atom. Chlorine (Cl) is in group 17 and has 7 valence electrons. Fluorine (F) is also in group 17 and has 7 valence electrons.
Step 2: Add the valence electrons from both atoms to find the total number of valence electrons in the molecule. This is calculated as 7 (from Cl) + 7 (from F) = 14 valence electrons.
Step 3: Draw the Lewis structure by placing the atoms and connecting them with a single bond, which represents a bonding pair of electrons. This bond uses 2 of the 14 valence electrons.
Step 4: Distribute the remaining valence electrons to satisfy the octet rule for each atom. After the bonding pair, there are 12 valence electrons left. Place 6 electrons (3 pairs) around each atom as lone pairs.
Step 5: Verify the structure by ensuring that each atom has a complete octet. Chlorine and Fluorine should each have 8 electrons around them, including the shared bonding pair.
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