Final answer:
c) 12 shared electrons, 0 lone pairs. The molecule H2C=CH2 has 12 shared electrons and 0 lone pairs, as all valence electrons are used in bonding, satisfying the octet rule for the carbon atoms with no remaining electrons for lone pairs.
Step-by-step explanation:
To determine how many shared electrons and lone pairs there are in the molecule H2C=CH2, we first need to account for the valence electrons. Each carbon (C) atom contributes four valence electrons, and each hydrogen (H) atom contributes one valence electron. The molecule has two C atoms and four H atoms, resulting in a total of 12 valence electrons (2 x 4 + 4 x 1).
When we draw the Lewis structure for the molecule, a double bond between the carbon atoms will fulfill the octet requirement for both carbons without creating any lone pairs on them. Each hydrogen atom is satisfied with a single bond (two shared electrons). The double bond consists of four shared electrons, and each single bond consists of two shared electrons. Therefore, this molecule has four single bonds and one double bond, which is equal to:
4 single bonds x 2 electrons = 8 shared electrons from single bonds
1 double bond x 4 electrons = 4 shared electrons from the double bond
Adding these together gives us a total of 12 shared electrons. There are no lone pairs on this molecule since all electrons are used for bonding.
Thus, the correct answer is option (c) 12 shared electrons, 0 lone pairs.