Chemical Formulas and Chemical Compounds

Chemical Formulas and Chemical Compounds 7.1

Naming Binary Ionic Compounds • Binary Ionic Compound (BIC) -___________ compound made up of _____ ions • To name _____ – use name of atom • Na+ = sodium K+ = potassium • Ca2+ = calcium Ba2+ = barium

Naming Anions • To name _______, use the atom’s base name and ______ at the ____ • Cl- = Chloride S2- = Sulfide • P3- = Phosphide O2- = Oxide • KBr = _________ ___________ • Mg3N2 = _________ __________

Naming • FrF • SrBr2 • Li2Se

Writing Ionic Formulas • Write the ______ and ______ of each ___ side by side (_____ first) • If total = __, just write _______ & you _____ _______! • If total does not = ___, ____ _____ charges to have _______ __ charge

Formula Writing Practice • Magnesium sulfide • Rubidium Oxide • Strontium Bromide • Aluminum Oxide

Multiple Charge Cations/Transitions & Group 14 • If ______ has ________ _______, use a _____ _______ to indicate ______ • Cu+ =Copper (I) Cu+2 =Copper (II) • I = 1 II = 2 III = 3 IV = 4 • V = 5 VI= 6 VII = 7 VIII = 8 • IX = 9 X = 10

Determining Charge on Transition Metals • The ______ on _____ __________ has to be ____________ _______ • Figure out _______ ______ on _____ and then determine what ______ _____ ______ has to be • CuCl2 ~Each Cl has a _______ of __ (_____ ___) and since there are __ of them, the _______ ______ of Cl is ___. Cu must be __ = ______ ( ) _________

Determining Charge on Transition Metals • PbO2 Charge on ___ is ___ and there are ___ of them so overall on ___ is ____. • Pb has to be _____ • ______ (___) _______

Naming • CuO • Hg2O • Cu2O • Vanadium (III) Iodide • Platinum (IV) oxide

Polyatomic Ions • Polyatomic Ion – an ____ made of 2 or more atoms that behave like a ________ ____. • Bonded ___________. • Bond _______________ with other simple _______ as salts

Naming Compounds w/polyatomics • Name the ____ that is not a polyatomic like simple ________ or _______ and then name the ____________ as the chart says • NaOH = Sodium hydroxide • CaCO3 = Calcium carbonate

Polyatomic Ions • AlPO3 • LiSCN • FeSO4 • Mn(Cr2O7)2

Formula Writing w/polyatomics • Determine ________ of overall polyatomic and then the other _______. • Follow same rules as before. • Beryllium cyanide • Copper (II) nitrate

Polyatomic Ions • Barium sulfide • Potassium oxalate • Chromium (III) cyanide • Vanadium (V)silicate

Oxyanions • Name changes as _________ of ___ changes • Gain 1 O = perchlorate ClO4- • Base Name = chlorate ClO3- • Lose 1 O = chlorite ClO2- • Lose 2 O = hypochlorite ClO-

Hydrogen and Sulfur • The name usually ________ with the word hydrogen, but use _________- and ____- • HPO4 –monohydrogen phosphate • H2PO4 – dihydrogen phosphate • Thio – replace O with S • K2S2O3 – Potassium thiosulfate

Naming Covalent Compounds • Inorganic molecular compounds • Specify # of each type of atom • P4O6 – Tetraphosphorus hexoxide • P4O10 – Tetraphosphorus decoxide

Cova l en t p r e f ixes

Naming Covalent Compounds • If there is __ of the first element, mono is __________ from the word • CO – carbon monoxide • CO2 – carbon dioxide

Naming Covalent Compounds • 1st element – named 1st – usually least _________________ • 2nd element – named 2nd – usually most e-neg – add ____ending • Drop vowels __ and __ from prefix ________ adding it to a _____ that starts with a _______

Naming Covalent Compounds • N2O4 – Dinitrogen tetroxide • SF6 – Sulfur hexafluoride • Some ________ names are used instead of ___________ name • H2O – water – not dihydrogen monoxide

Chemical Formulas and Chemical Compounds