Download Hybrid Orbitals – sp 3 Quiz

Hybrid Orbitals – sp3 Quiz
1. Based only on the number of unpaired electrons, how many bonds would a carbon atom
be expected to form?
a) 1
b) 2
c) 3
d) 4
2. In most compounds, carbon forms a total of ____ bonds.
a) 1
b) 2
c) 3
d) 4
3. Why can’t the bonds in CH4 be described by overlap of the atomic 2s and 2p orbitals of
the carbon atom?
a) There are not enough electrons.
b) The electrons in those orbitals are already paired.
c) The bond angles would be incorrect.
d) Carbon’s p orbitals can’t overlap with the s orbitals of the hydrogen atom.
4. What is hybridization of atomic orbitals?
5. Which cannot combine to form hybrid orbitals?
a) s and p orbitals
b) p and p orbitals
c) s, p and d orbitals
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6. What are carbon’s hybrid orbitals in CH4 called?
a) sp hybrids
b) sp2 hybrids
c) sp3 hybrids
d) sp3d hybrids
7. What spatial form do the four hybrid orbitals in a CH4 molecule take?
a) a tetrahedron
b) a square
c) an octahedron
d) a pyramid
8. What electron domain geometry leads to sp3 hybridization?
a) trigonal planar
b) trigonal pyramidal
c) tetrahedral
d) linear
9. The nitrogen atom in NH3 undergoes sp3 hybridization. Why does the nitrogen only form
three bonds instead of four?
10. In which molecule below is the central atom NOT sp3 hybridized?
a) CO2
b) H2O
c) CHCl3
d) PF3
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