The Mole Concept and Atoms


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1 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. Chapter 4 24 September 2013 Calculations and the Chemical Equation The Mole Concept and Atoms Atoms are exceedingly small Unit of measurement for mass of an atom is atomic mass unit (amu) unit of measure for the mass of atoms carbon12 assigned the mass of exactly 12 amu 1 amu = 1.66 x g Periodic table gives atomic weights in amu 1
2 Mass of Atoms What is the atomic weight of one atom of fluorine? Answer: amu What would be the mass of this one atom in grams? amu F F atom 1amu F g F atom Chemists usually work with much larger quantities It is more convenient to work with grams than amu when using larger quantities g F The Mole and Avogadro s Number A practical unit for defining a collection of atoms is the mole 1 mole of atoms = x atoms This is called Avogadro s number This has provided the basis for the concept of the mole 2
3 The Mole To make this connection we must define the mole as a counting unit The mole is abbreviated mol A mole is simply a unit that defines an amount of something Dozen defines 12 Gross defines 144 score 20 ream 500 The Mole 3
4 Atomic Mass The atomic mass of one atom of an element corresponds to: The average mass of a single atom in amu The mass of a mole of atoms in grams 1 atom of F is amu amu/atom F 1 mole of F is g g/mol F amu F g F 1atom F 1amu F atom F 1mol F =19.00 g F/mol F or g/mol F amu F g F 1atom F 1amu F atom F 1mol F =19.00 g F/mol F or g/mol F note: The name of the unit is mole The symbol is mol 4
5 Calculating atoms, moles, and mass We use the following conversion factors: Density converts grams milliliters Atomic mass unit converts amu grams Avogadro s number converts moles number of atoms Molar mass converts grams moles Strategy for Calculations Map out a pattern for the required conversion Given a number of grams and asked for number of atoms Two conversions are required Convert grams to moles 1 mol S/32.06 g S OR g S/1 mol S Convert moles to atoms mol S x (6.022 x atoms S) / 1 mol S 5
6 Practice Calculations 1. Calculate the number of atoms in 1.7 moles of boron. 2. Find the mass in grams of 2.5 mol Na (sodium). 3. Calculate the number of atoms in 5.0 g aluminum. 4. Calculate the mass of 5,000,000 atoms of Au (gold) Interconversion Between Moles, Particles, and Grams 6
7 The Chemical Formula, Formula Weight, and Molar Mass Chemical formula  a combination of symbols of the various elements that make up the compound Formula unit  the smallest collection of atoms that provide two important pieces of information The identity of the atoms The relative number of each type of atom Chemical Formula Consider the following formulas: H 2 2 atoms of hydrogen are chemically bonded forming diatomic hydrogen, subscript 2 H 2 O 2 atoms of hydrogen and 1 atom of oxygen, lack of subscript means one atom NaCl 1 atom each of sodium and chlorine Ca(OH) 2 1 atom of calcium and 2 atoms each of oxygen and hydrogen, subscript outside parentheses applies to all atoms inside 7
8 Chemical Formula Consider the following formulas: (NH 4 ) 2 SO 4 2 ammonium ions and 1 sulfate ion Ammonium ion contains 1 nitrogen and 4 hydrogen Sulfate ion contains 1 sulfur and 4 oxygen Compound contains 2 N, 8 H, 1 S, and 4 O CuSO 4. 5H 2 O This is an example of a hydrate  compounds containing one or more water molecules as an integral part of their structure 5 units of water with 1 CuSO 4 Homework: What does sesqui mean? Comparison of Hydrated and Anhydrous Copper Sulfate Hydrated copper sulfate Anhydrous copper sulfate Marked color difference illustrates the fact that these are different compounds 8
9 Formula Weight and Molar Mass Formula weight  the sum of the atomic weights of all atoms in the compound as represented by its correct formula expressed in amu What is the formula weight of H 2 O? amu + 2(1.008 amu) = amu Molar mass mass of a mole of compound in grams / mole Numerically equal to the formula weight in amu What is the molar mass of H 2 O? g/mol H 2 O Formula unit smallest collection of atoms from which the formula of a compound can be established When calculating the formula weight (or molar mass) of an ionic compound, the smallest unit of the crystal is used Formula Unit What is the molar mass of (NH 4 ) 3 PO 4? 3(N amu) + 12(H amu) + P amu + 4(O amu)= 3(14.01) + 12(1.008) (16.00)= g/mol (NH 4 ) 3 PO 4 9
10 Molar Mass Molar mass The mass in grams of 1 mole of atoms What is the molar mass of carbon? g/mol C This means counting out a mole of carbon atoms (i.e., x ) they would have a mass of g One mole of any element contains the same number of atoms, x 10 23, Avogadro s number The Chemical Equation and the Information It Conveys A Recipe For Chemical Change Chemical equation  shorthand notation of a chemical reaction Describes all of the substances that react and all the products that form, physical states, and experimental conditions Reactants (starting materials) the substances that undergo change in the reaction Products substances produced by the reaction 10
11 Features of a Chemical Equation 1. Identity of products and reactants must be specified using chemical symbols 2. Reactants are written to the left of the reaction arrow and products are written to the right 3. Physical states of reactants and products may be shown in parentheses 4. Symbol over the reaction arrow means that energy is necessary for the reaction to occur 5. Equation must be balanced Features of a Chemical Equation 2HgO( s ) 2Hg( l ) O2( g ) Products and reactants must be specified using chemical symbols Reactants written on the left of arrow energy is needed Products written on the right Physical states are shown in parentheses 11
12 Everything is balanced number of atoms moles of stuff mass energy charge 12
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