CH 1010 Chapter 3 Part 2

Ml

= (2l -1)

n=1

l=0, s-level, ml =0, 1 shell

s-level

spherical orbital 1 shell 1 sub orbital

n=2

l=1, p-level, ml = -1, 0, 1; sub shells: 1, 3, with 4 shells

p-level

second lowest energy level, 4 shells, 1/3 sub shell

n=3

l=2, d-level, ml = -2, -1, 0, 1, 2. Sub shells: 1, 3, 5, with 9 shells

d-level

third lowest energy level, 9 shells, 1/3/5 sub shell

n=4

l=3, ml= -3,-2,-1, 0, 1, 2, 3. Subshells 1, 3, 5, 7 with 16 shells

f-level

fourth lowest energy level, 16 shells, 1/3/5/7 sub shell

degenerate

orbitals in the same sub shell are _______

different

For a given shell, the subshells are NOT degenerate, the subshells have ____ energies

n

Principle Quantum Number

l

Angular Momentum Quantum Number

ml

Magnetic Quantum Number

smaller

As n increases, the energy differences between shells becomes _______

overlap

There is an ________ or penetration of the n=4 and higher shells

4s, 3d

The __ sub shell is lower in energy than the __ sub shell

5s, 4d

The __ sub shell is lower in energy than the __ sub shell

6s, 4f, 5d

The __ sub shell is lower in energy than the __ which is lower than the __ sub shell

Stern-Gerlach Experiment 1922

A fundamental property of electrons is spin. All electrons have the same amount. There are only two possible spin orientations, aligning with an external magnetic field or against. "Spin up or Spin down." The different spins are deflected differently by the magnetic field.

Ms

the fourth quantum number (spin), independent of ml, l, and n. Either equal to -1/2 or +1/2.

Pauli Exclusion Principle

no two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers (ml, n or l). Electrons that occupy the same orbital have thee identical quantum numbers (ex. 2, 1, 3)

2

No orbital can contain more than _ electrons. (one up one down)

electron configuration

Arrangement of electrons in the orbitals of an atom is called an atoms _____ ______

ground state

the lowest energy state of an atom or other particle

excited state

the higher energy state of an atom or other particle

Aufbau Principle

Lowest energy orbitals fill up first, then higher energy orbitals. (Do not pair first!)

Hund's Rule

For degenerate orbitals (with the same energy), the lowest energy arrangement is attained when the number of electrons with the same spin is maximized.

condensed notation

Show closest Noble Gas configuration in brackets, with valence electrons

valence electrons

Determines properties and chemical behaviors of element. Outermost shell, largest n. Most loosely held, involved in bonding.

core electrons

inner shells, filled orbitals, used to provide shielding for valence electrons from the positive charges from nucleus.

s-block

1-2 column, 1s for 1st period, 2s for second period, etc. holds two electrons.

d-block

3-12 column, mostly metals, 3d follows 4s, 4d follows 5s, 5d follows 4f and 6s, 6d follows 5f and 7s. Holds 10 electrons.

p-block

13-18 column, includes noble gases, holds 6 electrons.

f-block

transition metals, between s block and d block, holds 14 electrons.

4

How many unpaired electrons are found in the ground state of iron?

Anomalous electron configurations

Result from the unusual stability of half-filled and full-filled sub shells. These occur where the sub shell energy differences are small. (ex. 4s v. 3d)