Determining the hybridization state requires that you know how many regions of electron density there are. This does not mean how many bonds! For the carbon with the arrow, there are 4 bonds (2 single bonds and 1 double bond) but only 3 regions of electron density. The double bond only occupies 1 region of electron density. If you look at the terminal -CH3 carbon on the molecule, you\'ll notice that it also has 4 bonds (4 single bonds). This carbon has 4 regions of electron density since each bond occupies its own region. Once you know how many regions, it\'s simply a matter of adding exponents. The only hybridization states of carbon are sp, sp2, and sp3. If you add the exponents of each, you get 2, 3, and 4, respectively. These correspond to electron density regions. If it has 3 regions of electron density (not necessarily 3 bonds!), then it\'s sp2 hybridized (s1p2= 3). Carbon can only form 4 bonds (this rule never changes), so it can have at most 4 regions of electron density. Since there are only single, double, and triple bonds (no quadruple bond), the minimum regions of electron desity for carbon is 2 (i.e. triple and single bond, or double and double bond). Just remember, count regions (not bonds!) and add exponents. Solution Determining the hybridization state requires that you know how many regions of electron density there are. This does not mean how many bonds! For the carbon with the arrow, there are 4 bonds (2 single bonds and 1 double bond) but only 3 regions of electron density. The double bond only occupies 1 region of electron density. If you look at the terminal -CH3 carbon on the molecule, you\'ll notice that it also has 4 bonds (4 single bonds). This carbon has 4 regions of electron density since each bond occupies its own region. Once you know how many regions, it\'s simply a matter of adding exponents. The only hybridization states of carbon are sp, sp2, and sp3. If you add the exponents of each, you get 2, 3, and 4, respectively. These correspond to electron density regions. If it has 3 regions of electron density (not necessarily 3 bonds!), then it\'s sp2 hybridized (s1p2= 3). Carbon can only form 4 bonds (this rule never changes), so it can have at most 4 regions of electron density. Since there are only single, double, and triple bonds (no quadruple bond), the minimum regions of electron desity for carbon is 2 (i.e. triple and single bond, or double and double bond). Just remember, count regions (not bonds!) and add exponents..

1. Determining the hybridization state requires that you know how many regions of electron density
there are. This does not mean how many bonds! For the carbon with the arrow, there are 4 bonds
(2 single bonds and 1 double bond) but only 3 regions of electron density. The double bond only
occupies 1 region of electron density. If you look at the terminal -CH3 carbon on the molecule,
you'll notice that it also has 4 bonds (4 single bonds). This carbon has 4 regions of electron
density since each bond occupies its own region.
Once you know how many regions, it's simply a matter of adding exponents. The only
hybridization states of carbon are sp, sp2, and sp3. If you add the exponents of each, you get 2, 3,
and 4, respectively. These correspond to electron density regions. If it has 3 regions of electron
density (not necessarily 3 bonds!), then it's sp2 hybridized (s1p2= 3). Carbon can only form 4
bonds (this rule never changes), so it can have at most 4 regions of electron density. Since there
are only single, double, and triple bonds (no quadruple bond), the minimum regions of electron
desity for carbon is 2 (i.e. triple and single bond, or double and double bond).
Just remember, count regions (not bonds!) and add exponents.
Solution
Determining the hybridization state requires that you know how many regions of electron density
there are. This does not mean how many bonds! For the carbon with the arrow, there are 4 bonds
(2 single bonds and 1 double bond) but only 3 regions of electron density. The double bond only
occupies 1 region of electron density. If you look at the terminal -CH3 carbon on the molecule,
you'll notice that it also has 4 bonds (4 single bonds). This carbon has 4 regions of electron
density since each bond occupies its own region.
Once you know how many regions, it's simply a matter of adding exponents. The only
hybridization states of carbon are sp, sp2, and sp3. If you add the exponents of each, you get 2, 3,
and 4, respectively. These correspond to electron density regions. If it has 3 regions of electron
density (not necessarily 3 bonds!), then it's sp2 hybridized (s1p2= 3). Carbon can only form 4
bonds (this rule never changes), so it can have at most 4 regions of electron density. Since there
are only single, double, and triple bonds (no quadruple bond), the minimum regions of electron
desity for carbon is 2 (i.e. triple and single bond, or double and double bond).
Just remember, count regions (not bonds!) and add exponents.