Hybridization Numbers

quantum numbers

represents the properties of electrons

Heisenberg Principle

We can never know the precise location and speed of a particle at a given time. We can only approximate the location of an electron

Pauli Exclusion Principle

No two electrons can be in the same exact orbital and have the same spin

S orbital

spherical, n=1 (energy level) 1s, at energy level n=2, it is called 2s

P orbital

there are three p orbitals, have two lobes centered on an axis

D orbital

at energy levels > 2, there are five orbitals

F orbital

at energy levels > 3, there are 7, orbital shape gets more complex as the energy level increases

each orbital

can hold 2 electrons with opposite spins

as energy levels increase

The number of orbitals at each energy level and the orbital shapes get more complex, and the electrons in the orbitals get farther from the nucleus

n = principal quantum number

Represents the energy level and size of the orbital. As this number increases, the orbital is larger, and the electron inside has more energy and is less tightly bound to the nucleus

m_s = spin quantum number

represents the spin value of the electron, in an orbital with two electrons, one has a spin of +1/2 and the other has a spin of -1/2. Can equal either +1/2 or -1/2

l = shape quantum number

related to the shape of the orbital. Can equal 0 to n-1.

• 0 =s, 1 = p, 2 = d, 3 = f

m_l = orientation quantum number

this number is related to the orientation of the orbital in space. Can equal values from -l to l. Example: if l = 2, m_l can equal -2, 0, +2

atomic radius

• measure of an atom’s size

• decreases across a period (left to right), increases down a group (top to bottom)

electronegativity

• increases across a period (left to right)

• decreases down a group (top to bottom)

• measure of an atom’s ability to attract electrons

ionization energy

• increases across a period (left to right)

• decreases down a group (top to bottom)

• minimum energy required to remove an electron