Match the shapes of the following molecules based on the hybridization of the ce
ID: 1001535 • Letter: M
Question
Match the shapes of the following molecules based on the hybridization of the central atom, keeping in mind, the number of lone pairs or empty orbitals if any on the central atom.
1. Tetrahedral
2. Trigonal Planar
3. Pyramidal
4. Bent (V-Shaped)
5. Linear
Boron trifloride (BF3)
Ammonia (NH3)
Water (H2O)
Methane (CH4)
Methyl Anion (CH3-)
Methyl Cation (CH3+)
Ammonium Cation (NH4+)
Hydronium Ion (H3O+)
Carbon Dioxide (CO2)
Ethane (C2H6)
Ethene (C2H4)
Ethyne (C2H2)
Explanation / Answer
We can clasify the geometry of a molecule in: electron pair geometry (EPG) which take into consideration the lone pair of electrons, and the molecular geometry (MG) that accounts for bonding electrons only. Nonetheless, the hybridization is the same for any of the geometry, EP (electro pair) or M (molecular), that you decide to use.
a. The B atom in BF3 molecule has a sp2 hybridization (this is an exception to octete rule). EP and M geometry are both Trigonal Planar (there is none lone pair electron on the Boron atom).
b. Th N atom in NH3 molecule has a sp3 hybridization. EP geometry is tetrahedral (there is one lone electron pair on the nitrogen atom) and M geometry is Trigonal pyramidal.
c. The O atom in H2O molecule has a sp3 hybridization. EP geometry is tetrahedral (there are 2 pairs of lone electrons on the oxygen atom) and M geometry is bent.
d. The C atom in CH4 molecule has a sp3 hybridization. EP and M geometry are both tetrahedral (there is no lone pair electron on the carbon atom).
The geometry arragenment in all molecules obeys to minimize the repulsion of the atoms an the electron pairs.
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