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More Chemistry Review

More Chemistry Review. 2.3; 3.1-3.6. Atomic Notation. Web Link. Isotopes : Calculating Average Atomic Mass: Ex. 1.

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More Chemistry Review

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  1. More Chemistry Review 2.3; 3.1-3.6

  2. Atomic Notation Web Link

  3. Isotopes: Calculating Average Atomic Mass: Ex. 1 There are three naturally occurring isotopes of neon. Their percent abundances and atomic masses are neon-20, 90.51%m 19.99244 u; neon-21, 0.27%, 20.99395; neon-22, 9.22%, 21.99138 u. Calculate the weighted average atomic mass of neon.

  4. Isotopes: Ex. 2 The two naturally occurring isotopes of copper are copper-63, mass 62.9298 u, and copper-65, mass 64.9278. What must the percent natural abundances of the two isotopes if the atomic mass of copper is 63.546 u?

  5. Atomic Mass  Molar Mass Carbon-12

  6. 1S 32.07 amu 2O + 2 x 16.00 amu SO2 SO2 64.07 amu Molecular mass (or molecular weight) is the sum of the atomic masses (in amu) in a molecule. For any molecule molecular mass (amu) = molar mass (grams) 1 molecule SO2 = 64.07 amu 1 mole SO2 = 64.07 g SO2 3.3

  7. Do You Understand Molar Mass? How many atoms are in 0.551 g of potassium (K) ?

  8. How many H atoms are in 72.5 g of C3H8O ?

  9. n x molar mass of element x 100% molar mass of compound C2H6O Percent composition of an element in a compound = n is the number of moles of the element in 1 mole of the compound 3.5

  10. C2H6O

  11. Vitamin C (ascorbic acid) is composed of 40.92% C, 4.58% H, and 54.50% O by mass. Determine its empirical formula.

  12. Empirical Formula: Combustion Analysis • 11.5 g of ethanol is burned and 22.0 g of CO2 and 13.5 g of H2O is produced. Calculate the empirical formula of ethanol.

  13. Determination of Molecular Formulas A sample of a compound contains 1.52 g of nitrogen and 3.47 g of oxygen. The molar mass of this compound is between 90-95 g. Determine the molecular formula and the accurate molar mass of this compound.

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