Unit III: Quantitative Composition of Compounds
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1 Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using Moles of Compounds F. Mass Percent Composition of Compounds G. Empirical and Molecular Formulas
2 3-A The Structure of an Atom e e n p p n n p p n e e
3 3-A What is an atom? An atom is a fundamental piece of matter, composed of subatomic particles. An single atom is the smallest amount of an element that maintains properties of that element. Atoms are not created, changed, or destroyed during a chemical reaction
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5 3-A The Structure of an Atom Proton (+1) e pn n p p n e p Neutron (0) x g e n x g Electron (-1) e x g
6 3-A Atomic Mass Protons and neutrons are regarded as having one atomic mass unit (1 AMU) Electrons have a mass of zero AMU The total number of protons and neutrons in an atom is called the atomic mass
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8 3-A Isotopes While all atoms of the same element behave similarly in chemical reactions, not all atoms are identical Atoms always have the same number of protons, but may have different masses.
9 3-A Isotopes of hydrogen N P N e H Atomic mass = 12 3 Hydrogen Deuterium Tritium
10 Kinds of isotopes Stable and radio isotopes Oxygen for example has isotopes with between 4 and 16 neutrons. Only those atoms with 8, 9, or 10 neutrons are stable.
11 Atomic mass vs. Atomic weight Atomic Mass refers to the mass of a particular isotope of a particular element Atomic weight refers to the weighted average mass of all the isotopes of an element. (you might also see this as relative atomic mass)
12 UNIT 3-C: Formula and Molecular weights Molecular weight refers to covalent compounds Formula weight refers to the weight of an ionic compound s formula unit.
13 3-B Atomic Composition of Chemical Compounds To calculate formula weights we need to know the number of each element in a compound. Example: Hexanoic acid CH 3 (CH 2 ) 3 CH 2 COOH 6 carbon atoms 2 oxygen atoms 12 hydrogen atoms
14 3-D Unit 3-D: Calculations Using Moles of Atoms When we talk about practical amounts of elements or compound we are talking about huge numbers. We need a convenient term that describes a large group of things (similar to a dozen or gross). We use the term: mole
15 Moles A mole of anything always contains the same number, x This special number is called Avogadro s number. It just happens that there are x atoms of carbon-12 in exactly 12 grams.
16 Moles and masses The atomic mass of C-12 is 12 amu If the atomic mass of He-4 (for example) is 4 amu.. (1/3 the mass of C-12).and there are 12 g of C-12 in one mole of C Then there will be 4 g of He-4 in one mole of He-4
17 Lecture Problem 3-2 A. How many grams are in a mol of zinc-65 atoms? B. How many grams are in a mol of all zinc atoms? Page 90
18 Lecture Problem 3-3 A. How many grams are in 2.20 mol of iron? B. Calculate the number of mol in 2.45 x 10-5 g of calcium. Pg. 90
19 Unit 3 Part E: Calculations using Moles of Compounds
20 Calculating molecular weights and molar masses If we add up the atomic weights of all the atoms in a compound we get the molecular weight. (units of amu) If we want to talk about the mass of 1 mol of a compound we replace the units of amu with the units g/mol.
21 Lecture Problem III-4 (pg. 91) What is the molar mass of ammonium sulfide? (NH 4 ) 2 S Molar mass of (NH 4 ) 2 S is g/mol
22 Unit factors The concept of the mol is very useful in constructing unit factors.. Using the example of glucose (C 6 H 12 O 6 ) With a molar mass of g/mol Write as many unit factors as possible utilizing the mol concept.
23 Lecture Problem 3-5 (pg. 93) A. How many mol of hydrogen atoms are in 83.5 g of C 6 H 12 O 6? B. How many water molecules are in mol of water? Extra practice: How many total atoms are in 55.3 g of sulfur dioxide?
24 Using mols to describe composition of compounds Lecture problem III-6 (pg. 94) A sample of ammonium dichromate contains 3.07 mol of nitrogen atoms. What is the mass of the sample of ammonium dichromate? (NH 4 ) 2 Cr 2 O 7 has a molar mass of g/mol g of (NH 4 ) 2 Cr 2 O 7 rounded to 387 g
25 Unit 3-F: Mass Percent Composition 1. Calculate the formula or molecular weight of the compound. 2. Determine the total weight of each element in the compound. % composition of an element = Total weight of that element x 100 formula or molecular weight
26 Unit 3-F: Mass Percent Composition Lecture problem III-7 (pg. 96). Calculate the percent by mass of calcium in calcium phosphate. Ca 3 (PO 4 ) 2 molar mass of g/mol 38.76% Ca by mass in CaPO 4
27 Unit 3-G: Empirical and Molecular Formulas Given the percent composition of an unknown compound, how can we determine its identity? (sometimes actual masses for each element may be given) The first step is to turn the mass percentage into a ratio of atoms in the compound, called an empirical formula.
28 Unit 3-G: Empirical and Molecular Formulas The empirical formula describes the smallest ratio of atoms that are present in a compound. Consider N 2 O 4 dinitrogen tetraoxide There is 1 nitrogen atom for every 2 oxygen atoms So the smallest ratio, or empirical formula) is NO 2
29 Solving Empirical Formula Problems 1. If starting with % composition assume exactly 100 grams of sample. Then percentages become mass quantities. (If starting with mass, skip to step 2) 2. Calculate the number of mol of each element present using our unit analysis method. 3. Find the simplest mol ratio by dividing all of the mol quantities by the smallest number of mol of an element present.
30 Examples Lecture problems III-8 (page 99) A. Calculate the empirical formula of a compound that contains 56.4% phosphorus and 43.6% oxygen B. A compound contains 1.79g of phosphorus and 2.29g of oxygen. What is the empirical formula of the compound?
31 Finding the Molecular Formula Find the empirical formula for the compound. Calculate the empirical molar mass. Take the ratio of molecular molar mass to empirical molar mass. Multiply the quantity of each element in the compound by this factor.
32 Molecular Formula Determination Lecture problem (III-9 pg. 101): a. What is the molecular formula for galactose if the empirical formula is CH 2 O and the molar mass is g/mol? b. A molecular compound contains 40.0% carbon, 6.7% hydrogen and 53.3% oxygen by mass. A mol sample of this compound weighs 6.00 grams. What is the molecular formula of the compound?
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34 Extra practice with mystery metal problems mol of chlorine gas react with mol of a metal to form 16.3 grams of a binary ionic compound. What is the metal, and what is the formula for the compound? 5.11 grams of chlorine gas reacts with mol of a metal to form grams of a new solid compound with the formula MCl 3. What is the metal (symbol)?
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