נושא 3 חלק א' 1 Prof. Zvi C. Koren
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1 נושא 3 חלק א' מולקולות, תרכובות, יונים, ונוסחאות 1 Prof. Zvi C. Koren
2 Examples: Molecular Formula, Moles, Molecules, Atoms: Summary Molecular formula = (CH 3 ) 2 CF 2 1 molecule contains: 3 C atoms 6 H atoms 2 F atoms 100 molecules contain: 300 C atoms 600 H atoms 200 F atoms 1 mole of molecules contains: 3 moles of C atoms = 3 x x C atoms 6 moles of H atoms = 6 x x H atoms 2 moles of F atoms = 2 x x F atoms OK? OK! 2 Prof. Zvi C. Koren
3 Percent Composition Weight (or mass) % of each element in a compound For example, NH 3 : g % N in NH 3 x g 3 x g % H in NH 3 x g % N % H % 3 Prof. Zvi C. Koren
4 Determining Empirical and Molecular Formulas Given: Percent Compositions: H: 8.20% C: 39.34% O: 52.46% Assume 100 g compound: 1mol H # mol H atoms = 8.20 g mol H = 2.48 x 2 = g H (can round off to nearest integer if < 0.10) 1mol C g C # mol C atoms = g mol C 1mol O # mol O atoms = g mol O g O Empirical Formula = H 5 C 2 O 2 If MW = 122 g/mol, Molecular Formula =? Empirical Formula Weight 61 g/mol MW = 2 Molecular Formula (H 5 C 2 O 2 ) 2 H 10 C 4 O 4 EW = x 2 = Prof. Zvi C. Koren = 1 x 2 = 2
5 Empirical Formulas from Combustion Analysis & Law of Conservation of Mass Combustion reaction: H x C y O z + O 2 (g) -----> CO 2 (g) + H 2 O(g) Problem: g of compound is burned g CO 2 & g H 2 O produced. Empirical formula of compound =? Solution: H x C y O z + O 2 (g) CO 2 (g) + H 2 O(g) conservation of C conservation of H g C in comp d = g C in CO 2 = g CO 2 1mol CO g CO 2 1mol C 1mol CO g C 1mol C = g C g H in comp d = g H in H 2 O = g H 2 O 1mol H O 2 2 mol H g H g H2O 1mol H2O 1mol H = g H g O in comp d = Total g of comp d g C in comp d g H in comp d = g O Moles C in comp d = Moles H in comp d = Moles O in comp d = Empirical Formula = HCO 2 If MW = g/mol Molecular Formula = H 2 C 2 O 4 (After 3 lessons) 5 Prof. Zvi C. Koren
6 Molecular Elements The Halogens diatomic molecules 6 Prof. Zvi C. Koren
7 Carbon Allotropes 7 Prof. Zvi C. Koren
8 diatomic molecule O 2 light 2 O O + O 2 O 3 triatomic molecule Oxygen Allotropes 8 Prof. Zvi C. Koren
9 tetrahedral (tetrahedron) tetratomic molecule 9 Prof. Zvi C. Koren
10 octatomic molecule 10 Prof. Zvi C. Koren
11 The Language of Chemistry Letters = Element Symbols Words = Compound Formulas 11 Prof. Zvi C. Koren
12 Compounds Ionic (typically between Metals & Nonmetals) Covalent (between Nonmetals) composed of ions composed of e-sharing positive (+): Cation Electric Glue negative (-): Anion Atoms share the same e-pair A : B Salts & Oxides 12 Prof. Zvi C. Koren
13 Ionic Compounds composed of ions: positive(+) and negative(-) when Metals meet Nonmetals, they instantly fall in LOVE Metals LOVE to transfer electrons to Nonmetals opposites attract or viva la difference 13 Prof. Zvi C. Koren
14 Ionic Charges Main Group Number is the number of valence electrons = Number of e s in outermost shell Octet Rule: Atoms combine to mimic the very stable noble elements X Na + Cl Na+ Cl He Ne Ar Examples of compounds: Ca & Br: Ca Br CaBr 2 (s) Ba & S: Ba 2+ + S 2 BaS(s) Al & O: 2Al O 2 Al 2 O 3 (s) K & N: 3K + + N 3 K 3 N(s) Typical charges for monatomic ions: Kr Xe Rn Examples of ions: Na + Mg 2+ Al 3+ C 4- N 3- O 2 - F - 14 Prof. Zvi C. Koren
15 Charges on Transition Metals Transition Group Number = maximum charge (but lower charges are possible!!!) Sc 3+ Ti 4+ V 5+ Cr 6+ Mn 7+ Fe Cu Ag + only 3+ (After 4 lessons) Os 8+ Au 3+ Note exception 15 Prof. Zvi C. Koren
16 Ion Fe 2+ Fe 3+ Cu + Cu 2+ Hg 2 2+ Hg 2+ Sn 2+ Sn 4+ Pb 2+ Pb 4+ Roman-Numeral Name Iron(II) ion Iron(III) ion Copper(I) ion Copper(II) ion Mercury(I) ion Mercury(II) ion Tin(II) ion Tin(IV) ion Lead(II) ion Lead(IV) ion Transition Metals & Others (continued) Common Ions with two possible charges -ous and ic Names Ferrous ion Ferric ion Cuprous ion Cupric ion Mercurous ion Mercuric ion Stannous ion Stannic ion Plumbous ion Plumbic ion 16 Prof. Zvi C. Koren Fe Cu Hg Sn Pb
17 Elements to Remember 17 Prof. Zvi C. Koren
18 Nomenclature of Ionic Compounds )מינוח, כיניון, שיטת כינוי( Cation: Metal = Element name or NH 4+ = ammonium ion (and its derivatives: CH 3 NH 3+, ) polyatomic cation Anion: Monatomic = Element root name + ide 4A C 4 carbide 5A N 3 nitride P 3 phosphide 18 Prof. Zvi C. Koren A O 2 oxide S 2 sulfide Examples: Se 2 selenide CaBr 2 calcium bromide BaS barium sulfide Te 2 telluride Al 2 O 3 aluminum oxide K 3 N potassium nitride FeCl 2 iron(ii) chloride = ferrous chloride FeCl 3 iron(iii) chloride = ferric chloride Hg 2 Cl 2 mercury(i) chloride = mercurous chloride HgCl 2 mercury(ii) chloride = mercuric chloride LiH lithium hydride (NH 4 ) 3 P ammonium phosphide 7A H hydride F fluoride Cl chloride Br bromide I iodide
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