Periodic trends

what increases/decreases as the principal quatum number increases?

radius increases

electric field decreases

valence electrons not held as strongly

what is sheilding?

electrosn shield eachother from the nuclesu

what are z, z-eff

z is the full attractive force of the nucleus

s-eff is the effective nuclearn sharge after shilding takes effect

trend of z-eff

bottom right

why are noble gasses so stable

have a ns² np^6 configuration

what are isoelectric elements

when an element gains to loses an electront o form the noble gas configuration

periodic trend of atomic radius

bottom left

why does atomic radius increase down

electrons added to new shells. Zeff doesnt chaneg muhc but electrons are farther away from the nucleus, resulting in less atrraction

why does atomic radius decrease across a period

nuclear charge (z) increases but electrons are added to the same valence shell so more attractio

Ionic radius quick rules

• cations are smaller that thier neutral atoms (opposite for anions)

• for isoelectric ions/atoms sinze decreases as Z increases (F- >Ne >Na+)

• right most and left most halogens and alkali metals will ahve similar radius inversly (nuetral will be name as anion, neutral will be same as cation)

ionizatione nergy trend

top right

ionization eneergy

energy needed to remove an electron from a agss

Why do some have a higher inonization

will ahve a filled 3s or a half filled 3p

Why do some have a higher inonization

will have an unpaired spin electron that if removed will have a filled 3s or half filled 3p

second inization energy main rules

• removing electron from a cation

• will need more ionization energy than the first

• follows same blips

nd ionizatione nergy

removing the electron from a core shell of a cation takes SIGNIFICATNLY more energy then 1st ionization energy

electron affinity

the energy change when an electron is added to a neutral atom, typically resulting in the formation of an anion.

electrona ffinity trend

amgnitude increases top right