In this lesson, we will learn how to link the hybridization of an atom in a molecule to the oxidation state and geometry of bonds and electron pairs.
Q1:
Iodine heptafluoride can be produced by the reaction of fluorine with iodine pentafluoride at high temperature as shown in the equation: F()+IF()IF()257ggg
What is the hybridization of the I atom in IF5?
What term describes the bonding geometry in IF5?
What is the smallest angle between IF bonds in IF7?
What term describes the bonding geometry in IF7?
Q2:
Nitrogen dioxide contains an unpaired electron and has trigonal planar electron-pair geometry.
Which type of hybridized orbital does the unpaired electron occupy?
Which term best describes the magnetic behavior of this molecule?
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