Clicker #1 How many unpaired electrons and valence electrons does Se have? A) 0; 14 B) 2; 6 C) 2; 14 D) 0; 6 E) 2; 4

Atomic Trends Atomic Radius: size of the orbital H F Fr decreasing increasing

Atomic Trends Atomic Radius: size of the orbital H F Fr decreasing increasing More protons = more attraction and smaller radius Orbitals are getting bigger and further from nucleus

Clicker #2 Which of the following elements has the largest atomic radius? A) Ca B) Al C) N D) Sr E) F

Atomic Trends Ionization Energy H F Fr increasing decreasing

Atomic Trends Ionization Energy H F Fr increasing decreasing Electron is at its lowest energy state when closest to the nucleus  takes more energy to take an electron away when closer to the nucleus

Clicker #3 Which of the following elements has the largest ionization energy? A)P B)Al C)Cl D)Ba E)K

Isoelectronic Series Same number of electrons Example: Which is larger Na + or Ne?

Isoelectronic Series Same number of electrons Example: Which is larger Na + or Ne? Same number of electrons but Na + has 11 protons and Ne has 10 protons.

Example Which is larger Cl - or Ar? Which has a higher ionization energy Cl - or Ar?

Example Which is larger Cl - or Ar? Which has a higher ionization energy Cl - or Ar?

BONDING “Forces” What is meant by a “chemical bond”? Why do atoms bond to form molecules? How do atoms bond to form molecules?

BONDING Two Types of Bonding Intramolecular (within a molecule) Intermolecular (between molecules)

Ionic Compounds Between a metal and a nonmetal Example: NaCl Na: [Ne]3s 1 Cl: [Ne]3s 2 3p 5

Ionic Compounds Between a metal and a nonmetal Example: NaCl Na: [Ne]3s 1 Na + : [Ne] Cl: [Ne]3s 2 3p 5 Cl - : [Ne] 3s 2 3p 6

Mg -> Mg + -> Mg 2+ Ionization energies of atoms are highly endothermic HOWEVER… Takes more energy to remove 2nd electron Once you get Mg 2+ (noble gas configuration) gives off energy OVERALL = EXOTHERMIC PROCESS

Bonding in H 2 Is this ionic?

Bonding in H 2 Covalent Bonding Sharing electrons Hydrogens share the electrons and have noble gas configuration Why isn’t He diatomic?

Bonding in H 2 Covalent Bonding Sharing electrons Hydrogens share the electrons and have noble gas configuration Why isn’t He diatomic? Already has a noble gas configuration

Therefore… Covalent bonding has same idea as ionic bonding… But Neither atom is “strong” enough to remove electron from the other atom

What about CO?