Which of the following elements typically forms two chemical bonds and has a Lewis dot structure with six valence electrons?

• A. Carbon (C)
• B. Nitrogen (N)
• C. Oxygen (O)
• D. Fluorine (F)

Answer: (C)

Verified step by step guidance

1. Identify the number of valence electrons for each element by looking at their group number in the periodic table. For example, Oxygen (O) is in group 16, so it has 6 valence electrons.
2. Recall that the number of bonds an element typically forms is related to how many electrons it needs to complete its octet. Elements tend to form bonds to reach 8 valence electrons.
3. For Oxygen, with 6 valence electrons, it needs 2 more electrons to complete its octet, so it typically forms 2 bonds.
4. Draw the Lewis dot structure for Oxygen by placing 6 dots around the symbol 'O' to represent its valence electrons, showing 2 unpaired electrons available for bonding.
5. Compare this with the other elements: Carbon has 4 valence electrons and typically forms 4 bonds; Nitrogen has 5 valence electrons and typically forms 3 bonds; Fluorine has 7 valence electrons and typically forms 1 bond.