We are asked to use valence bond theory to write a hybridization and bonding scheme for CO2.
Carbon → Central atom → Group 4A → 4 valence electrons
O → Group 6A → 6 valence electrons
2 atoms +0 lone pairs = 2 groups
AX2 → Linear
Subshell Total # of orbitals
s _ 1 orbital
p _ _ _ 3 orbitals
d _ _ _ _ _ 5 orbitals
Use valence bond theory to write a hybridization and bonding scheme for CO2.
Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.
1. The Lewis structure for CO2 has a central _____ atom attached to _____ atoms through _____.
2. Carbon dioxide has a _____ electron geometry.
3. The carbon atom is _____ hybridized.
4. Carbon dioxide has _____ π bonds and _____ δ bonds.
You can only use the following words:
two C(s)-O(s) ; two C(p)-O(p) ; trigonal planar ; two O(sp2)-C(sp) ; two O(sp)-C(sp2) ; carbon and oxygen ; sp2 ; a single and a double bond ; oxygen ; two single bonds ; linear ; tetrahydral ; carbon ; sp ; two double bonds ; sp3
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Hybridization concept. You can view video lessons to learn Hybridization. Or if you need more Hybridization practice, you can also practice Hybridization practice problems.