AP Chem Ch 7-9 Flashcards
(63 cards)
Principle QN (n)
Energy level
Integer from 1-7
Quantum numbers
Four numbers that describe an electron
- Principle QN (n)
- Angular momentum QN (l)
- Magnetic QN (ml)
- Spin QN (ms)
Angular momentum QN (l)
From 0 to n-1 When l = 0, s orgbital 1 --> p 2--> d 3 --> f
Magnetic QN (ml)
From -l to l
So when l = 0, one possibility for S orbital
When l = 1, 3 possibilities in p orbital
Spin QN
+/- 1/2
Pauli exclusion principle
No two electrons can be in the same spot
Aufbau principle
Build up – put electrons into lowest energy orbital available
Hund’s Rule
Lowest Energy confirmation generates unpaired electron – result of energy required to pair the electron in the same orbitals.
This means first do it unpaired and then pair them up
Auger emission
When a core electron is ejected, a higher energy may relax into that electron hole, resulting in an emission of energy
Exceptions to normal electron configuration
Chromium and molybendium fill up d orbital half way and have only one S electron
Copper, silver, gold all fill up the d orbital and have one in the S
Pd has no s electrons, 10 d
Homogenous magnetic field
Orient dipoles– spins align. Observed splitting of the 5s energy level with the S going to 2 different energy states. Pauli connected this to the spin in the electrons with the +1/2 and -1/2, the 2 intrinsic states of electron.
Periodic trend key factors
Number of protons, number of electrons, effective nuclear charge, down the group, across the period, shielding, distance from the nucleus
Electron affinity
The amount of energy to add an electron
Energy associated with this rxn:
X + e- –> X-
Atomic radius / size periodic trend
Increases down and to the left. Francium the biggest, helium the smallest
Ionization energy
Amount of energy required to remove an electron
M–> M+ + e-
Increases top right
Helium has the most because very hard to remove an electron
Francium the least, easier.
Increases across the period mostly, but some exceptions as move from a metal to a non metal
Electronegativity
How much an element wants an electron
Measured in Paulings, arbitrary unit for how much an element wants the electron
Increase top right. Fluorine has the most, a 4.0
Effective nuclear charge
Number of protons - inner electrons
Aluminum is +3
Chrlorine +7
Why does IE increase left to right?
Effective nuclear charge increases because number of protons increases, so while shielding stays the same because same energy level, it is harder to remove an electron against this extra positive charge from the nucleus while the atom is smaller as well.
Decreases as go down a row because it is easier to remove an electron from a bigger atom (shielding effect in effect)
Why does oxygen have lower IE than nitrogen?
Nitrogen has the p orbital half way full, so it is more stable, so it thus harder to remove that electron than from oxygen
Ionic bonding
Involves the transfer of electrons and is the positive / attractive force that results from the charged species
Electrostatic interactions
Interactions of charged particles –> forces keeping electrons around electrons –> force that makes ionic bonds ionic.
Anion
Negative ions. Non metal
Cation
Positive ions. Metal
Bond energy
Energy required to break a bond
E= (2.3110^-19 Jnm) q1 q2 / d where d is the distance between 2 nuclei
