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Section 7.3 – Using Chemical Formulas

Section 7.3 – Using Chemical Formulas. They allow chemists to calculate a number of characteristic values for a given compound. Formula Mass.

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Section 7.3 – Using Chemical Formulas

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  1. Section 7.3 – Using Chemical Formulas • They allow chemists to calculate a number of characteristic values for a given compound.

  2. Formula Mass • Like individual atoms, the formula mass of any molecule, formula unit, or ion is the sum of the average atomic masses of all the atoms represented in its formula. Reported in amu (atomic mass units).

  3. Example – Water (H2O) • 1 H atom = 1.0079 amu • 1 O atom = 15.9994 amu • 1 water molecule = (2 x 1.0079) + (1 x 15.9994) = 18.0152 amu/molecule

  4. Remember The Mole? • The mass of 6.022 x 1023 particles.

  5. Molar Mass • Calculated by summing the masses of the elements present in a mole (6.022 x 1023 particles) of the molecules, formula units, or ions of a compound. Reported in grams.

  6. Example – Water (H2O) • 1 mole H atoms = 1.0079 grams • 1 mole O atoms = 15.9994 grams • 1 mole water molecules = (2 x 1.0079) + (1 x 15.9994) = 18.0152 g/mole H2O

  7. Notice • The molar mass and the formula mass are numerically equal; one is reported in amu, the other in grams.

  8. EXAMPLE • Find the formula mass for KClO3 • Find the formula mass for Ca(NO3)2 • Find the molar mass for Al2S • Find the molar mass for Ba(OH)2

  9. Molar Mass As A Conversion Factor • See p. 224 • To convert moles to grams: # mol x g/mol = g • To convert mass to moles: grams x 1/molar mass = moles

  10. EXAMPLES • What is the mass in grams of 2.50 mol of oxygen gas (O2)? • How many moles of compound are there in 6.60g (NH4)2SO4 • How many molecules are there in 25.0g of H2SO4?

  11. Percentage Composition • Often useful to know this, it is the percentage by mass of each element in a compound. There are two ways to determine it:

  12. By Mass • Mass of element in a sample divided by the mass of the sample multiplied by 100. The percentage will be the same regardless of the sample size.

  13. Or By Moles (Easier) • Mass of the element in 1 mol divided by the molar mass of the compound multiplied by 100.

  14. EXAMPLES • Find the percentage compositions of: • PbCl2 Ba(NO3)2 • Magnesium Hydroxide is 54.87% oxygen by mass. How many grams of oxygen are in 175 g of the compound. How many moles of oxygen is this?

  15. Info. You Will Need For Later • Hydrates are salts that crystallize from a water solution and trap water (known as water of hydration) in the crystal structure.

  16. Na2CO3•10H2O • This means that 10 moles of water are trapped within each mole of the sodium carbonate salt.

  17. Assignment – Due Friday • 7.3 Worksheet • 7.3 Textbook Problems

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