1. electrons are attracted to the nucleus and repelled by other electrons

2. Z eff = Z - S, Z is atomic number, s is inner core electrons

3. average electrical feild for one electron

periods = decreasing due to higher Z eff

groups = increasing due to higher n

1. nuclear charge AKA how many electrons it has gained/lost

2. number of electrons it has overall

3. what orbitals the electrons are in

increases down groups because of an overall increase in size

1. same number of electrons

2. sizes go down as charge gets higher because the higher the charge, the more electrons lost

1. amount of energy needed to remove otuer electron

2. increases with each new electron removed

 3. increases dramatically in inner core electrons

1. decreases as you go down groups smaller atoms are less willing to give up their electrons

2. increases across periods because of higher Zeff

1. easier to remove from p orbitals than s orbitals.

 2. easier to remove from filled orbital shells (/\,\/)

1. the ease with which an atom gains an electron

2. more (-) an affinity is, the easier it will lose electron

3. (+) affinity is unstable and will not form 

1. across periods increases

2. same discontinuities as Ionization

1. Shiny

2. good conductor of heat and electricity

3. cations in aqueous solutions

4. metal oxides are basic

5. tend to lose electrons

6. malleable

1. not shiny

2. brittle

 3. poor condutor

4. non-metal oxides are molecular and acidic

5. aniona in aqueous soutions

6. gain electrons

1. characteristics of both metals and non-metals

2. e.g. silicon is shinny but a poor conductor and brittle

1. soft metallic

2. only compunds in nature

3. decreasing melting points and densities

4. decreasing ionization energies

5. exo rxns with water

 6. bright colors in flames

7. rxns with O: Li-nothing, K, Rb,Cs-superoxides, others-peroxides

1. Higher densities and melting points than alkalis

2. lower ionization energues than alkalis

3. rxn-ness increases top to bottom

4. rxn w/ H2O: Mg-Steam only, Be-nothing, everything else easily.

1. O,Se,S = non-metals

2. Te = ,etaliod

3. Po = Metal

1. 2 allotropes O₂, O₃ (dioxygen and ozone)

2. 3 anions O^-2,O₂^-2,O₂^-1 (oxide, peroxide, superoxide)

3. tends to take elctrons

1. weaker oxidizer than O

2. allotrop S8 = ring shaped, most stable

1. non-metals

2. large (-) affinities

3. easily oxidized

4. react w/ metals = halidies

1. large ionization energies

2. (+) affinities

3. unreactive

4. monotomic gases

5. Xe = XeF2, XeF4 and XeF6

6. Kr = KrF2

7. HArF - unstable, synthesized in 2000

1. Periods- increases because the atomic number increases (total electrons) while the s stays the same

2. Groups- stays basically the same

1. Doesnt really belong to any group

2. Very hard to take it's electron --no sheilding effect/repulsion from other electrons