Write the electron configuration for K and Br. Circle the Valence Electrons

A John Modica Production NOMENCLATURE OF IONIC COMPOUNDS A John Modica Production

Ionic Compounds Mg O Because electrons are negatively charged… an atom becomes positively or negatively charged as it loses or gains an electron, respectively. Any atom or group of atoms with a net charge (whether positive or negative) is called an ion. A positively charged ion is a cation A negatively charged ion is an anion. +2 positively t Mg negatively n n O -2

IONIC COMPOUNDS Metal Non-metal Oxygen-8 Magnesium-12 Compounds are two or more elements that are held together by opposite charge attraction. IONIC COMPOUNDS Oxygen-8 8 (+) 10 (-) -2 Charge 12 (+) 10 (-) +2 Charge Magnesium-12 Metal Non-metal

Ionic Formulas Ions combine in small, whole number proportions so that the sum of oxidation numbers will be zero! Electrons are transferred from the metal to the non-metal The metal become a cation (+ charge) Why? The non-metal becomes an anion (- charge)

Metals Non-metals Metals combine with non-metals Metals loose electrons to non-metals They attract because their charges are opposite. Metals Non-metals

Ionic Formulas These are called Binary Compounds The prefix “bi” meaning two Two elements bonding to form a compound The metal ion ALWAYS goes first, followed by the non-metal ion

So what does this look like? Mg +2 O -2 Magnesium Oxide

So what does this look like? Al +3 S -2 2 3 Aluminum Sulfide

So what does this look like? Na +1 Cl -1 A.k.a. Table Salt Sodium Chloride

Your Turn! Na +1 F -1 Ba +2 Cl -1 Al +3 Br -1 K +1 O -2 +1 -2 Li S

Your Turn! Na F Ba Cl 2 Al Br 3 K O Li S 2 2

Now let’s Kick it up a notch!

Polyatomic Ions A group of 2 or more atoms that act as a single unit When a metal and a polyatomic ion bond this forms a tertiary compound 3 or more elements reacting to form a compound

POLYATOMIC IONS Polyatomic ions are mostly made of two non-metals. Ions with -1 charge perbromate BrO4-1 bromate BrO3-1 bromite BrO2-1 hypobromite BrO-1 perchlorate ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO-1 periodate IO4-1 iodate IO3-1 iodite IO2-1 hypoiodite IO-1 nitrate NO3-1 nitrite NO2-1 hydroxide OH-1 cyanide CN-1 acetate C2H3O2-1 Permanganate MnO4-1 bicarbonate HCO3-1 Ions with a -2 Charge carbonate CO3-2 sulfate SO4-2 sulfite SO3-2 chromate CrO4-2 dichromate Cr2O7-2 oxalate C2O4-2 Ions with a -3 Charge phosphate PO4-3 phosphite PO3-3 arsenate AsO4-3 Ions with +1 charge ammonium ion NH4+1 Yes, I can read your minds…

No you do not have to memorize these polyatomic ions No you do not have to memorize these polyatomic ions. You will receive a chart with these Obviously!!!

Na PO Tertiary Compounds Polyatomics ions react as one unit, so you treat them the same when writing formulas Use the criss-cross method Na PO +1 -3 4 3 Sodium Phosphate

Tertiary Compounds Mg ( ) SO +2 -2 4 Magnesium Sulfate

Al NO ( ) Yeah, I’ve got nothing. Tertiary Compounds Aluminum Nitrite +3 ( ) -2 2 2 3 Aluminum Nitrite Yeah, I’ve got nothing.

Na SO Ba ClO Al PO K NO Li SO Your Turn! +1 -2 +2 -1 4 2 +3 -3 4 +1 -1

Your Turn! Na ( ) SO Ba ClO 2 4 2 2 Al ( ) PO 4 K NO Li SO 2 2 3

How do we know the charge of the elements? Glad you asked!

Click on element to see its oxidation number(s) Oxidation Numbers (most common) -3 -2 +2 +1 -1 +3 -4 +1 +2 +2 +3 +2 +4 1A 7A 8A H H He 2A 3A 4A 5A 6A Li Be B C N O F Ne Click on element to see its oxidation number(s) Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Ce Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Rh Hs Mt Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu return Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr