IIIIII The Periodic Table

Chemical Reactivity zAlkali Metals zAlkaline Earth Metals zTransition Metals zHalogens zNoble Gases

Chemical Reactivity zPeriod/Row zFamilies/Groups/Columns yElements in the same family has the SAME # of valence electrons

zAtomic Radius is the distance from the nucleus to the outermost orbital yIncreases to the LEFT and DOWN Atomic Radius

zWhy larger going down? yHigher energy levels have larger orbitals zWhy smaller to the right? yIncreased nuclear charge Atomic Radius

zWhich atom has the larger radius? yBe orBa yCa orBr Ba Ca Examples

zIonization Energy- the energy required to remove 1 electron from the parent atom zWhy opposite of atomic radius? yIn small atoms, e - are close to the nucleus where the attraction is stronger Ionization Energy

zFirst Ionization Energy yIncreases UP and to the RIGHT Ionization Energy

zWhich atom has the higher 1st I.E.? yNorBi yBa orNe N Ne Examples

zMelting/Boiling Point – the temperature at which a substance changes states yHighest in the middle of a period. Melting/Boiling Point

zWhich atom has the higher melting/boiling point? yLiorC yCrorKr C Cr Examples

Ionic Radius zThe distance between the center of the nucleus and the outer edge of the ion Cations/Metals -lose elections, so they have a positive charge -small Atoms -neutrally charged elements -medium Anions/Nonmetals -gain electrons, so they have a negative charge -large

Electronegativity * The measure of how strongly an atom attracts electrons when it is combined with another element Increases from left to right (except for noble gases) due to increased nuclear charge Increases as you move up a group due to the shorter distance between the nucleus and valence electrons. Increases UP and to the RIGHT

zWhich particle has the largest electronegativity? ySorP yAlorGa S Al Examples