chem periodic trends

Coulombic attraction

Between oppositely charged particles

Distance and attractive force

Farther distance less attraction

Alkali metals attraction

More shells less attraction

Number of protons and attraction

More protons more attraction

Weakest element

Francium

Higher charge =

Greater attraction

Atomic radius

-Attraction increases down and left

-atoms to left have less protons = weaker coulombic attraction bigger atoms

-atoms at bottom more energy lvls = bigger distance from nucleus to valence electrons + weaker coulombic attraction bigger atoms

Ionization energy

Amount energy required to remove highest energy valence electron

Increase up and right

Hardest to take e- from helium

Atoms to right have more protons greater coulombic attraction=harder to remove valence e

Ionic radius

Size of ions (cation and anion radius)

Cation radius

Increase down and left

Metals only

Ion with larger pos charge smaller than ion with smaller pos charge

Atom to right =more protons so stronger coulombic attraction on remaining e-

Anion radius

Non metals only

increases down and left

Atoms right have more protons = stronger coulombic attraction on e

Nonmetals in same period have same e # after gain

Add electrons increase electron repulsion’s

Strongest element

Fluorine

Electronegativity

Ability of atom in molecule to attract shared electrons to itself to attract electrons in bind

Increases up and right

EXCLUDES NOBLE GASES

Metal reactivity

Increases left and down

Lose valence when reacting=easier to remove so it’s more reactive

left metals less protons = weaker coulombic attraction more reactive

Bottom atoms more energy lbls larger distance to valence e weaker pulmonic attraction more reactive

Nonmetal reactivity

increases right and down

EXCLUDE NOBLE GASES

Gain valence when react= easier for valence e to be attracted to nicked more reactive

Right Nonmetals more protons stronger CA more reactive

Bottom have more energy lvl a = bigger distance to e weaker CA less reactive nonmetals

Shielding

Outer electrons shielded from nucleus by core electrons

Causes outer e to not experience same effect of nuclear charge

Coulomb’s law

Opposite charges attracted

Like charge repel

Attraction strength based on atomic radius and charge protons

Effective coulombic attractions

Directly proportional to charge

Inversely proportional to distance between