Ch. 4 - The Periodic Table III. Periodic Trends

A. Periodic Law When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

B. Chemical Reactivity Families within a group result in similar ______________ _____________

B. Chemical Reactivity _____________________________ ________________________________ ___________________________________

C. Other Properties Atomic Radius size ______________ © 1998 LOGAL First Ionization Energy Energy required to remove one ____________________. © 1998 LOGAL Melting/Boiling Point

D. Atomic Radius Atomic Radius K Na Li Ar Ne

D. Atomic Radius Atomic Radius Increases to the _______ and ________

D. Atomic Radius Atomic Radius Decreases to the ________ and _____

D. Atomic Radius Why larger going down? Higher _________ __________ have larger orbitals ________ - core e- block the attraction between the nucleus and the valence e- Why smaller to the right? ____________ nuclear charge without additional shielding pulls e- in tighter

E. Ionization Energy First Ionization Energy He Ne Ar Li Na K

E. Ionization Energy First Ionization Energy Increases _____ and to the _________

E. Ionization Energy Why opposite of atomic radius? In small atoms, e- are close to the nucleus where the attraction is ______________ Why small jumps within each group? _____________ e- configurations don’t want to lose e-

F. Melting/Boiling Point Highest in the ____________ of a period.

Examples Which atom has the larger radius? Be or Ba Ca or Br Ba Ca

Examples Which atom has the higher 1st I.E.? N N or Bi Ba or Ne Ne

Li or C Cr or Kr C Cr Examples Which atom has the higher melting/boiling point? Li or C Cr or Kr C Cr