Chem Chapter 3 Flashcards
What is left to right on the periodic table? What is up and down?
Period is left to right
Group is up and down
Period trends
Increasing mass
Increasing energy
Increasing Effective Nuclear Charge
Smaller atomic size and ionic size
Atomic radius decreases
Group trends
Bigger
Atomic radius increases
Element groups from left to right
Metals (alkali metals and alkali earth metals)
Metalloids
Non metals (chalogens, halogens, nobel gases)
Coulombs Law
Attraction and repulsion between particles
Electron Configuration
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d
Effective Nuclear Charge
Z - # of inter-core e-
Inter-core e coresponds with the period
Aufbau Principle
Energy levels fill from lowest to highest
Hunds Rule
Full each orbital once before doubling up
Magnetism Types
Diamagnetic: no unpaired e-
Paramagnetic: some unpaired e-
Ferromagnetic: large domains of aligned magnetic fields (iron)
Metals and Nonmetals anions or cations?
Metals cations (give up e-)
Nonmetals anions (e- hungry)
Groups and their ions
Group 1: +1
Group 2: +2
Al: +3
Chalogens -2
Halogens: -1
Cations and Anions
Cations: become smaller and positive (K+)
Anions: become bigger and negative (Cl-)
Ionization Energy
Minimum energy needed to move an e- into gas phase
Endothermic because it needs energy
Element + ionization energy = x+ + e-
Electron affinity
Addition of an e- to valence shell in the gas phase
The more negative, the larger the EA
Element + e- = element- + energy
Increase from left to right
