IONIC BONDS ION - charged atom 1. Bonds formed by transferring electrons between atoms 2. Electronegativity difference is approx. > 2.0 3. Metal + Nonmetal 4. Metal loses e- Nonmetal gains e- ION - charged atom 1. Cation (+ charge); metal Na+1 Ca+2 Al+3 Sodium Ion Calcium Ion Aluminum Ion 2. Anion (- charge); nonmetal I-1 S-2 P-3 Iodide Ion Sulfide Ion Phosphide Ion 3. Results in Noble Gas electron configuration for each atom K: 1s22s2p63s2p64s1 19 p+ 19 e- Cl: 1s22s2p63s2p5 17 p+ 17 e- e- e-

e- e- e- 19 p+ 18 e- K+1:1s22s2p63s2p6 17 p+ 18 e- Cl-1: 1s22s2p63s2p6 Now, both exhibit Noble Gas e- configuration “8 valence electrons” complete filled s & p orbitals Ionic compounds are composed of “ions”

NAMING IONIC COMPOUNDS IA + VIIA COMPOUNDS Combine in 1:1 ratio High melting point >5000C NAMING IONIC COMPOUNDS BINARY REGULAR METAL (1 charge) 1st: Name of element 2nd: Name changed to -ide ending SrI2 Strontium Iodide IRREGULAR METAL (2+ charges) 1st: Name of element common name w/ roman numeral or “derived name” 2nd: Name changed to -ide ending Pb3P2 Lead II Phosphide Plumbous Phosphide

Metallic Elements & Charges to Know +1 H +2 +3 Li Na Mg +6,2,3 +2,3 +2,3 +2,3 +1,2 Al K Ca Cr Fe Co Ni Cu Zn Ag Sn Ba Au Hg Pb +1,2 +2,4 U

Nonmetallic Elements & Charges to Know +4,-4 He Ne Ar Kr Xe Rn -3 -2 -1 C N O F Si P S Cl Br I

Elements & Charges to Know +1 H +4,-4 He Ne Ar Kr Xe Rn +2 +3 -3 -2 -1 Li C N O F Na Mg +6,2,3 +2,3 +2,3 +2,3 Al Si P S Cl +1,2 K Ca Cr Fe Co Ni Br Cu Zn+2 Ag+1 Sn I Ba Au Hg Pb +1,2 +2,4 U

POLYATOMICS radicals, polyatomic ions Group of 2+ elements combined together to make a group with an overall charge SO3-2 SO4-2 NO2-1 NO3-1 PO3-3 PO4-3 Sulfite Sulfate Nitrite Nitrate Phosphite Phosphate OH-1 CO3-2 HCO3- 1 Hydroxide Carbonate Hydrogen Carbonate or Bicarbonate C2H3O2-1 O2-2 Acetate Peroxide Halide Pattern ClO hypochlorite ClO2 chlorite ClO3 chlorate ClO4 perchlorate fluorine fluor bromine brom iodine iod

NaCl ine ide BaF2 ine ide 2nd: Element name, ending NH3: Ammonia NH4+1: Ammonium Ion Complete Molecule Itself Polyatomic Ion; needs Anion to complete cmpd. NH4Cl NH4C2H3O2 (NH4)2SiO3 Ammonium Ammonium Ammonium Chloride Acetate Silicate 2nd: Element name, ending changed to “–ide” 1st : Name of element NaCl ine ide Sodium Chlor BaF2 Barium ine ide Fluor

MULTIPLE CHARGED METALS IRREGULAR METALS Metals w/ 2 or more charges Use: 1) Roman Numeral to indicate the charge 2) Derivative Name Copper I Copper II Iron II Iron III Cuprous Cupric Ferrous Ferric -OUS lowest charge -IC highest charge

Fe2O3 FeO Fe2 O3 Fe O No subscripts +3 +2 -2 -2 charge “O” –2 = charge “Fe” +2 Charge on “Fe” = +3 Iron III Oxide Ferric Oxide Iron II Oxide Ferrous Oxide

. . . . . . . . . . Na3PO4 Mg(NO2)2 Sodium Phosphate Magnesium Nitrite REGULAR METAL FeSO4 Fe2(SO3)3 Iron II Sulfate Iron III Sulfite Ferrous Sulfate Ferric Sulfite IRREGULAR METAL Electron Dot Structure Use the total # of valence e-’s Cl: 1s22s2p63s2p5 Recall writing e- structure: & Hund’s Rule K: 1s22s2p63s2p64s1 . . . . . . K Cl . . Use chem. symbol & # valence e-: K . Cl .

ACIDS -- BASES Acid: 1st element, cation, is “H+1” Base: Metal + OH Anion, OH-1 Ca(OH)2 LiOH CuOH Calcium Hydroxide Lithium Hydroxide Copper I Hydroxide Cuprous Hydroxide Oxides IA Peroxides Li2O Lithium Li2O2 Na2O Sodium Na2O2 K2O Potassium K2O2 Oxide Peroxide O-2 O-1---> O2-2 NH4OH Ammonium Hydroxide MnO4-1: Permanganate MnO4-2: Manganate Mercury I or II Hg+2 Hg+1--Hg+1 Hg2+1

Halogen Acid Pattern F, Cl, Br, I 1 “O” 2 “O” 3 “O” 4 “O” -ClO3 -ClO -ClO2 -ClO4 Hypochlorite Chlorite Chlorate Perchlorate Hypochlorous Acid Chlorous Acid Chloric Acid Perchloric Acid -ITE Change ending to “OUS” -ATE Change ending to “IC”

Sn+2SO4-2 Sn+4SO4-2 Sn2(SO4)4 Sn(SO4)2 SnSO4 REVIEW HIGHLIGHTS Simple Ion: single atom or element w/ associated charge F-1 Ca+2 Sb+3 Complex Ion: group of elements w/ overall charge C2H3O2-1 NH4+1 OH-1 Molecule: covalent; nonmetal + nonmetal atoms combine in any ratio, not simplest ratio C2H6 C4H10 C4H8 Formula Unit: compound; ionic; metal + nonmetal atoms always combine in simplest ratio Tin II Sulfate Tin IV Sulfate Sn+2SO4-2 Sn+4SO4-2 Sn2(SO4)4 Sn(SO4)2 SnSO4 Reduce added subscript number to lowest form

IONIZATION ENERGY ELECTRON AFFINITY E required to remove e- from atom in its gaseous state Na + E ----------> Na+1 + e- Mg + E -----------> Mg+2 + 2e- Trend: increases L2R across row decreases down column ELECTRON AFFINITY E released when gaining an e- to an atom in its gaseous state O + 2e- ---------> O-2 + E Br + e- --------> Br-1 + E The Z=5, 6, 7, group 4A, & group 7A elements not easily gain or lose e- Tend to form Covalent Bonds

OXIDATION - REDUCTION “REDOX” Reduction: gain electron Oxidation: lose electron H2(g) + O2(g) --------> H2O(g) Both H2 & O2 are diatomics: charge on each 0 In the cmpd. H is +1 & O is -2 H: from 0 to +1 charge, loses e-, oxidized (reducing agent) O: from 0 to -2 charge, gain e-, reduced (oxidizing agent) Four IONs that play an important role in biochemical processes Na+1 Ca+2 K+1 Mg+2

REDOX – Reduction/Oxidation LEO the lion says GER-r-r-r-r-r Gain Electron Reduce Lose Electron Oxidize

REDOX – Reduction/Oxidation OIL RIG Oxidize Is Lose Reduce Is Gain