Ch 3: Bonding (3%)

principal, n, energy, size, closer, lower, n, 1, infinity

The ___________ quantum number, ___, corresponds to the _______ level of a given electron in an atom and is essentially a measure of its _____. The smaller the number, the _______ the shell is to the nucleus, and the ________ its energy. The possible values of ___ range from ___ to _______.

subshells, azimuthal, l, 0, n-1, l, s, p, d, f, increases, azimuthal

Within each electron shell, there can be several _________, which are described by the ___________ quantum number ___, which ranges from ___ to ______ for a given energy shell. The ___-values 0, 1, 2, and 3 correspond to the ___, ___, ___, and ___ subshells, respectively. Just as with the principal quantum number, energy __________ as the __________ quantum number increases.

orbitals, magnetic, ml, -l, +l, atomic orbital, shape, s-orbital, p-orbital

Within each subshell, there may be several _________, which are described by the _____________ quantum number ___, which ranges from ___ to ___ for a given subshell. Each type of ________ ________ has a specific _______, which describes the probability of finding an electron in a given region of space. A ___-________ is spherical and symmetrical, centered around the nucleus. A ___-________ is composed of two lobes symmetrically about the nucleus and contains a node at the nucleus (an area where the probability of finding an electron is zero).

2, spin, ms, ms, +1/2, -1/2

Each orbital can hold ___ electrons, which are distinguished by the ______ quantum number ___. The only values of ___ are ____ and ____.

molecular orbitals

the combination of two atomic orbitals forms these

bonding orbital

molecular orbital where the signs of the wave functions are the same, indicating a lower-energy (more stable) molecule

antibonding orbital

molecular orbital where the signs of the wave functions are different, indicating a higher-energy (less stable) molecule

1, 0

How many sigma bonds are in single bonds?

How many pi bonds are in single bonds?

1, 1

How many sigma bonds are in double bonds?

How many pi bonds are in double bonds?

1, 2

How many sigma bonds are in triple bonds?

How many pi bonds are in triple bonds?

weaker, stronger

Pi bonds are _________ than sigma bonds, but the strength is additive, making double and triple bonds _________ overall than single bonds.

hybrid orbitals

the combination of different types of orbitals forms these

sp3

the hybrid orbital of a molecule with tetrahedral geometry (109.5° bond angles)

25%, 75%

How much s character does sp³ have?

How much p character does sp³ have?

sp3

the hybrid orbital of a carbon atom with all single bonds

sp2

the hybrid orbital of a molecule with trigonal planar geometry (120° bond angles)

33%, 67%

How much s character does sp² have?

How much p character does sp² have?

sp2

the hybrid orbital of a carbon atom with one double bond

sp

the hybrid orbital of a molecule with linear geometry (180° bond angles)

50%, 50%

How much s character does sp have?

How much p character does sp have?

sp

the hybrid orbital of a carbon atom with one triple bond

sp

the hybrid orbital of a carbon atom with two double bonds