Ch 7. Writing chemical compounds
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1 Ch 7 Writing chemical compounds
2 Ionic Compounds Formula unit it is the formula for an ionic compound. When writing an ionic compound, we must get a neutral compounds. (charges must balance out) Cation Anion Compound Na + Cl - Mg +2 Cl - Al +3 Cl - Na + O -2 Mg +2 O -2 Al +3 O -2
3 Charges of d block metals d block elements can have multiple charges. See pg 205 for more, but the following elements you need to know. Zinc Zn +2 Silver Ag + Chromium (II) Cr +2 Chromium (III) Cr +3 Copper (I) Cu + Copper (II) Cu +2 Iron (II) Fe +2 Iron (III) Fe +3 Lead (II) Pb +2 Lead (IV) Pb +4 Tin (II) Sn +2 Tin (IV) Sn +4
4 Naming Binary Compounds contains two different elements, one metal and one non-metal. Metal name non-metal root + ide Compound Formula Compound Name NaCl MgO K 2 S AlCl 3
5 When using a d block metal that has several possible ions, we use the Roman numeral to specify which one we are using. Compound Formula Compound Name FeCl 2 FeCl 3 CuBr CuBr 2
6 Compounds using the polyatomic ions use: Metal name Polyatomic ion name Cation Anion Compound Name Na + PO -3 4 K + SO -2 3 NH + 4 SO -2 4 Cu +2 CO -2 3
7 Remember, there are several polyatomic ions that are similar. They are actually a series. If there are 2 in the series: If there are 4 in the series: ate (greatest # of O 2 ) per ate (greatest # of O) ite ate ite hypo ite
8 Covalent Compounds Binary Molecular Compounds contains 2 non-metals. Num. Prefix + element name Number Numerical Prefix 1 mono 2 di 3 tri 4 tetra Num. Prefix + root name + ide ** Exception: Don t use mono on the first term. 5 penta 6 hexa 7 hepta 8 octa 9 nona 10 deca
9 Molecular Compound Molecular Name NO 2 CO N 2 O 5 PCl 3 SO 2 P 4 S 3 ** Exception: When hydrogen is the 1st element in the compound, there are no prefixes at all. Ex. HCl H 2 S hydrogen chloride hydrogen sulfide These are gases and we will rarely see in this form.
10 Most generally, if H is the first element in a compound, it is an acid. Acids have a sour taste (although this is not used in lab situations) There are two types of acids: 1. Monoxoacids water solutions of molecular compounds composed of H and a non-metal other than O and C. Hydro + root + ic Acid Ex. HCl H 2 S hydrochloric acid hydrosulfic acid
11 2. Oxoacids water solutions of molecular compounds composed of H and some non-metal and O. (normally a polyatomic ion) Polyatomic root + ic or ous Acid Ex. HNO 3 H 2 CO 3 H 2 SO 4 HClO 2 HClO nitric acid carbonic acid sulfuric acid chlorous acid hypochlorous acid
12 Ex. Write the formula for: a) Sulfurous acid (came from sulfite) H 2 SO 3 b) Hydrobromic acid (hydro means it was a binary acid) HBr c) Chloric acid (came from chlorate) HClO 3
13 ** See Handout Salt ionic compound composed of a cation and the anion from an acid. acid + base salt + H 2 O HCl + NaOH NaCl + H 2 O H 2 SO 4 + Ca(OH) 2 CaSO 4 + H 2 O
14 Skipping Sec 7-2
15 Sec 7-3 Formula mass mass of any molecule, formula unit, or ion. It is the sum of the masses of each element in the formula. Ex. H 2 O 1 H atom has a mass of 1.01 amu x 2 = O atom has a mass of amu = amu Ex. HNO amu
16 Ex. Na 2 SO amu Molar mass mass in grams of 1 mole of any molecule, formula unit, or ion. Ex. H 2 O g for every mole ex. Ba(NO 3 ) g for every mole
17 Conversions: Ex. What is the mass in grams of 2.50 mol of O 2? Ex. What is the mass in grams of 3.04 mol of Ammonia vapor, NH 3?
18 Ex. Calc the mass of.257 mol of calcium nitrate. Ex. How many moles are there in 6.60 g (NH 4 ) 2 SO 4? Ex. How many moles are there in 4.5 kg Ca(OH) 2? Ex. How many molecules are there in 25.0 g H 2 SO 4? Ex. How many formula units are there in 7.95 g CaBr 2? Ex. What is the mass in grams of 6.25 mol of Copper (II) Nitrate?
19 Ex. Ibuprofen C 13 H 18 O 2 is an active ingredient in many pain relievers. a) How many molecules are in each tablet? b) What is the mass in grams of Carbon in 33g of Ibuprofen?
20 % Composition - % by mass of each element in a compound. Ex. Cu 2 S Cu = = % S = = %
21 Ex. Calculate the percent composition of NaNO 3. Na = = 27.05% N = = 16.48% O = = 56.47%
22 Some salts crystallize from a water solution. They bind with water molecules in their crystalline structure and is called a hydrate. Sodium carbonate forms such a hydrate, in which 10 molecules of H 2 O are present for every formula unit of sodium carbonate. It is written as Na 2 CO 3 10 H 2 O. Ex. Find the % composition of water in sodium carbonate decahydrate. H 2 O = = % of the compound is water
23 7-4 When a new substance is discovered or synthesized, it is analyzed quantitatively to reveal its % composition. From that, its empirical formula can be determined. An empirical formula consists of the symbol for the elements combined in a compound with subscripts showing the smallest whole # mole ratio of the different atoms in the compound. Ex. N 2 O 4 (molecular formula) NO 2 (emp. form) Ex. C 6 H 12 O 6 (mol. form) CH 2 O (emp. form)
24 Ex. CHCl 3 (molecular) CHCl 3 (emp.) can t be reduced Ex. Quantitative analysis shows that a compound contains 32.38% Na, 22.65% S, and % O. Find the empirical formula.
25 Ex. Repeat but with % iron and 36.48% S.
26 Analysis of a g sample of a compound known only to contain phosphorous and oxygen indicates a phosphorous content of g. What is the empirical formula?
27 Molecular formula = whole # x empirical formula Recall: C 6 H 12 O 6 (mol. form) CH 2 O (emp. form) whole # = The whole # that would be multiplied is 6. Ex. Earlier, we found the empirical formula P 2 O 5. Experimentation shows that the molar mass is g/mole. Find the molecular formula. whole # = = 2 Therefore the molecular formula is P 4 O 10.
28 Acetylene has a % composition of 92.24% C, 7.742% H. Its molecular mass is g. Write both the emp. and molecular formulas.
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