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Ch. 9

“Little Johnny took a drink, Now he shall drink no more. For what he thought was H 2 O, Was H 2 SO 4 .”. Ch. 9. Chemical Names and Formulas. "H-O-H"?! WHAT'S THAT SPELL?!. WATER?. mis. mis. Website: Dihydrogen monoxide Information Campaign. Naming Ions.

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Ch. 9

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  1. “Little Johnny took a drink, Now he shall drink no more. For what he thought was H2O, Was H2SO4.” Ch. 9 Chemical Names and Formulas

  2. "H-O-H"?! WHAT'S THAT SPELL?! WATER? mis mis Website: Dihydrogen monoxide Information Campaign

  3. Naming Ions • *Element Name Search Activity* pg. 252 • Monatomic ions = ions consisting of a single atom w/a pos. or neg. charge resulting from the loss or gain of 1 or more valence electrons • Polyatomic ions = ions composed of more than 1 atom

  4. Vocabulary CHEMICAL FORMULA IONIC COVALENT formula unit molecular formula NaCl CO2

  5. Vocabulary COMPOUND more than 2 elements 2 elements binary compound ternary compound NaCl NaNO3

  6. Vocabulary ION 2 or more atoms 1 atom monatomic Ion polyatomic Ion Na+ NO3-

  7. Cations • Metals • Lose electrons • Pos. charge • Groups 1A-3A sometimes 4A • When the metals in Groups 1A, 2A, & 3A lose electrons, they form cations w/ pos. charges equal to their group # • The names of the cations are the same as the name of the metal followed by the word ion or cation • EX: Al3+ is the aluminum ion Under aged Pb walks into a bar and the bartender turns to the gold Bouncer and says, “Au, get the lead out!”

  8. Anions • Nonmetals • Gain electrons • Negative charge • The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number • 7A (7 – 8 = -1), 6A = -2, 5A = -3 • Anion names start w/ the stem of the element name and end in –ide • F-(fluoride), Cl-(chloride), O2-(oxide), S2-(sulfide), N3-(nitride), P3-(phosphide), As3- (arsenide)

  9. Transition Metal Ions • Pos. charged cations w/ charges of +1, +2, or +3 • Groups 1B-8B • Some may form more than 1 cation w/diff. charges • Roman numeral after the metal name describes the charge OR –ous for the smaller and –ic for the larger charge • *C.P. 9.1, P.P. 1-2 pg. 256

  10. Polyatomic Ions • Most names end in –iteor –ate but some end in –iumor –ide • Some begin with a H so we say Hydrogen Phosphate for HPO4. The bi- prefix means: add H+ ions to the anion until its charge is -1, So H2PO4 is biphosphate and HCO3 is bicarbonate. • *9.1 sect. assessment pg. 258

  11. Fe2+ Fe2+ Fe2+ Fe2+ Fe2+ Fe2+ Fe2+ Fe2+ Nomenclature - Humor BaNa2 “BaNaNa” “Ferrous Wheel” What weapon can you make from the elements nickel, potassium and iron? Fe = iron (Latin = ferrum) A KNiFe Fe2+ = lower oxidation state = ferrous Fe3+ = higher oxidation state = ferric

  12. Naming Ionic Compounds • Binary compounds – two types of elements • Ternary compounds – more than two types of elements • Cations go 1st – cation can be metal or polyatomic ion • For metals that have only 1 possible charge (valency, oxidation #), the name of the metal is used • Examples are Group 1 metals (1+), Group II metals (2+), Al+3, Zn+2, Ag+1 • For metals that can have more than one charge, the name of the metal is succeeded by the valency in capital Roman numerals in () parentheses OR by using the suffix –ous for the lowest valency & -ic for the highest valency

  13. Cont… • Anions go 2nd – neg. charged element or polyatomic ion • Neg. charged elements have the suffix –ide • Ex: oxide O, sulfide, fluoride, nitride • Polyatomic ions which include oxygen in the anion have the suffixes –ate or –ite. “ate” means there is more oxygen in the anion than one ending in “ite” • Ex: sulfate SO42- and sulfite SO32-, nitrate NO3- and nitrite NO2- • Exception: OH- hydroxide • *Practice: Fe(OH)3, KNO3, NH4Br, Ca(OH)2, CuSO4, Cu2O, Al2S3

  14. Bellringer 1 (Name the following) • 1) CaCl2 • 2) PO4-3 • 3) CO3-2 • 4) AgBr • 5) Al2O3

  15. Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.

  16. H 1 He 2 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 * 6 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 7 W 1+ Binary Compounds 2+ 3+ 1+ 2+ Binary compounds that contain a metal of fixed oxidation number (group 1, group 2, Al, Zn, Ag, etc.), and a non-metal. To name these compounds, give the name of metal followed by the name of the non-metal, with the ending replaced by the suffix –ide. Examples: NaCl sodium chlor ide (Na1+ Cl1-) CaS calcium sulf ide (Ca2+ S2-) AlI3 aluminum iod ide (Al3+ I1-) 3

  17. Practice • BaO • NaBr • MgI2 • KCl • SrF2 • CsF

  18. Writing Formulas of Ionic Compounds chemical formula: has neutral charge; shows types of atoms and how many of each To write an ionic compound’s formula, we need: 1. the two types of ions 2. the charge on each ion Na1+ and F1– Ba2+ and O2– Na1+ and O2– Ba2+ and F1– NaF sodium fluoride BaO barium oxide Na2O sodium oxide BaF2 barium fluoride

  19. Step 4: AlCl 3 Example: Aluminum Chloride Criss-Cross Rule Step 1: write out name with space Al Cl 3+ 1- Step 2: write symbols & charge of elements Al Cl Step 3: 1 3 criss-cross charges as subsrcipts combine as formula unit (“1” is never shown) *ALWAYS REMEMBER TO SIMPLIFY WHEN FINISHED

  20. Rules for Parentheses Parentheses are used only when the following two condition are met: • There is a radical (polyatomic ion) present and… • There are two or more of that radical in the formula. Examples: NaNO3NO31-is a radical, but there is only one of it. Co(NO3)2NO31- is a radical and there are two of them (NH4)2SO4NH41+ is a radical and there are two of them; SO42- is a radical but there is only one of it. Co(OH)2OH1- is a radical and there are two of it. Al2(CO3)3CO32- is a radical and there are three of them. NaOHOH1-is a radical but there is only one of it.

  21. Writing Formulas w/Polyatomic Ions Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion. BaSO4 barium sulfate Ba2+ and SO42– Mg(NO2)2 Mg2+ and NO21– magnesium nitrite NH4ClO3 ammonium chlorate NH41+ and ClO31– Sn(SO4)2 tin (IV) sulfate Sn4+ and SO42– Fe2(Cr2O7)3 Fe3+ and Cr2O72– iron (III) dichromate ammonium nitride (NH4)3N NH41+ and N3–

  22. Hydrates • Hydrates = ionic compounds that absorb H2O into their solid structures • Ex: CuSO4. 5H2O copper (II) sulfate pentahydrate • MgSO4. 7H2O magnesium sulfate heptahydrate • C.P. 9.2, P.P. 10-11 pg. 263 • C.P. 9.3, P.P. 12-13 pg. 265 • 9.2 Sect. Assessment 14-19 pg. 266 • *Making & Naming an Ionic Compound Demo pg. 262

  23. Molecular Compound A compound containing atoms of two or more elements that are bonded together by sharing electrons. Silicon dioxide, SiO2, is a molecular compound. It is also a mineral called quartz (left). Quartz is found in nearly every type of rock. Most sand grains (center) are bits of quartz. Glass is made from sand.

  24. Naming Molecular Compounds • The more electronegative element is written last and w/ -ide • Use prefixes to tell you the subscript in each • Mono is not written w/ the 1st word of a compound’s name (Ex: CO2) • Prefixes are sometimes shortened to make a name easier to say (Ex: CO is carbon monoxide not mono oxide) • Sometimes use common names instead of formal names (Ex: O2 is oxygen not dioxygen, NH3 is ammonia, and H2O is water not dihydrogen monoxide) • *Practice: N2O4, PCl5, NO2, BF3, NF3, P2O5, N2O5, SO2, SiO2, PCl3 • *9.3 Sect. Assessment 20-25 pg. 270

  25. Bellringer 2 (Write or name the following) • 1) N2O • 2) lead (IV) oxide • 3) SiO3 • 4) XeF4 • 5) ammonium nitride

  26. Writing Formulas of Covalent Molecules • Covalent Molecules • contain two types of nonmetals • Key: FORGET CHARGES • What to do: • Use Greek prefixes to indicate how many atoms • of each element, but don’t use “mono” on first element. 1 – mono 6 – hexa 2 – di 7 – hepta 3 – tri 8 – octa 4 – tetra 9 – nona 5 – penta 10 – deca

  27. Writing Formulas of Covalent Molecules EXAMPLES: carbon dioxide CO dinitrogen trioxide N2O5 carbon tetrachloride NI3 CO2 carbon monoxide N2O3 dinitrogen pentoxide CCl4 nitrogen triiodide

  28. Practice Writing and Naming Compounds • (NH4)2S2O3 • AgBrO3 • (NH4)3N • U(CrO4)3 • Cr2(SO3)3 • iron (III) nitrate • ammonium phosphide • ammonium chlorite • zinc phosphate • lead (II) permanganate • FeO • Fe2O3 • CuBr • CuBr2 • cobalt (III) chloride • tin (IV) oxide • tin (II) oxide

  29. Exceptions! Two exceptions to the simple –ide ending are the diatomic oxide ions, O22- and O21-. O22- is called peroxide O21- is called superoxide. Note the differences. BaO barium oxide __________ barium peroxide __________ Ba2+ BaO2 Na2O sodium oxide __________ sodium peroxide __________ Na1+ Na2O2 Do Not Reduceto lowest terms! K2O potassium oxide __________ potassium superoxide __________ K1+ KO2

  30. Acids • Acid = a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water. • Consist of an anion combined w/as many hydrogen ions needed to become electrically neutral in the form (HnX)

  31. 3 Rules to Naming Acids: • 1. When the name of the anion (X) ends in –ide, the acid name begins w/the prefix hydro-. The stem of the anion has the suffix –ic and is followed by the word acid • HCl = hydrochloric acid • 2. When the anion name ends in –ite, the acid name is the stem of the anion w/the suffix –ous, followed by the word acid • H2SO3 = sulfurous acid • 3. When the anion name ends in –ate, the acid name is the stem of the anion w/the suffix –ic followed by the word acid • HNO3 = nitric acid

  32. Naming Bases • Base = ionic compound that produces hydroxide ions when dissolved in water • Bases are named in the same way as other ionic compounds – the name of the cation is followed by the name of the anion • EX: NaOH = sodium hydroxide • Al(OH)3 = aluminum hydroxide • *9.4 Sect. Assessment 26-33 pg. 273

  33. Covalent Formula  Name? Metal + Nonmetal? (Except: NH4+) Ionic Two Nonmetals? Columns 1, 2, 13Ag+, Zn2+ d,f-blockPb,Sn Single Multiple Steps 1 & 4 ONLY • Write name of cation (metal) • Determine the charge on the metal by balancing the (-) charge from the anion • Write the charge of the metal in Roman Numerals and put in parentheses • Write name of anion(Individual anions need –ide ending!) Use Prefixes!!! *Mono* HexaDi HeptaTri OctaTetra NonaPenta Deca

  34. Covalent Name  Formula? Ionic No Prefixes? Prefixes? • Determine the ions present and the charge on each (Roman Numeral = cation charge, otherwise use PT) • Balance formula (criss-cross) • Reduce subscripts (if needed) • FORGET CHARGES!!! • Use prefixes to determine subscripts • Do NOT reduce subscripts!

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