Transcript November 12
Clicker #1 How many unpaired electrons and valence electrons does Se have? A) B) C) D) E) 0; 2; 2; 0; 2; 14 6 14 6 4 Atomic Trends Atomic Radius: size of the orbital decreasing H increasing Fr F Atomic Trends Atomic Radius: size of the orbital decreasing H increasing Fr F 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) B) C) D) E) Ca Al N Sr F Atomic Trends Ionization Energy increasing H decreasing Fr F Atomic Trends Ionization Energy increasing H decreasing Fr F 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) B) C) D) E) P Al Cl Ba 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 Clor Ar? Example Which is larger Cl- or Ar? Which has a higher ionization energy Clor 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) QuickTime™ and a TIFF (LZW) decompressor are needed to see this picture. Ionic Compounds Between a metal and a nonmetal Example: NaCl Na: [Ne]3s1 Cl: [Ne]3s23p5 Ionic Compounds Between a metal and a nonmetal Example: NaCl Na: [Ne]3s1 Cl: [Ne]3s23p5 Na+: [Ne] Cl-: [Ne] 3s23p6 Mg -> Mg+ -> Mg2+ Ionization energies of atoms are highly endothermic HOWEVER… Takes more energy to remove 2nd electron Once you get Mg2+ (noble gas configuration) gives off energy OVERALL = EXOTHERMIC PROCESS Bonding in H2 Is this ionic? Bonding in H2 Covalent Bonding Sharing electrons Hydrogens share the electrons and have noble gas configuration Why isn’t He diatomic? Bonding in H2 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?