AP Chemistry 1.5 Structure and Arrangement of Atoms
AP Chemistry: Structure of Atoms Drill 1, Problem 5. What is the hybridization of the carbon atom in the Lewis structure?
|AP Chemistry||Structure and Arrangement of Atoms|
They're super energy-efficient.
The concept of hybridization derives from mixing the
originals of something into a new mix, or hybrid.
In chemistry, hybridization refers to the mixing of atomic orbitals.
Just as there's a path we can follow to define the orbit of a planet around the sun, there's
also a path we can follow to define the way an electron orbits the nucleus of an atom...also
called an atomic orbital.
Hybridization in chemistry refers to the mixing of atomic orbitals into hybrid orbitals which
allow electrons to form chemical bonds.
In fact, if atoms didn't "hybridize", some of these chemical bonds couldn't form because
they wouldn't have the right shape or structure.
Here, hybridization allows the Carbon to single bond to two chlorine atoms and double bond
to the single oxygen atom. Oooh... edgy.
Now onto the REAL question. How do we figure out what the hybridization of the carbon atom is?
When determining hybridization, we can just count the number of other atoms that the atom
in question is connected to.
Carbon is connected to two chlorine atoms, and one oxygen atom.
It doesn't matter that carbon is double-bound to oxygen; it is still only bound to three atoms.
Three atoms means three hybridized orbitals.
But wait, our answer choices aren't just numbers... in chemistry notation, we can add the exponents
in s and p to find the number of hybridized orbitals it represents.
Looking at answer C, we have the exponent in s...1 plus the exponent in p... 2. 1 plus
2 is... give us a second... oh, right. 3.
So our answer is C.
As in "carbonite."