5.1 – Isotopes and average atomic mass

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Presentation transcript:

5.1 – Isotopes and average atomic mass Ms. Munir

Weighted Average Mass of (A + B + C) / Number of items Given three items of mass 1.0 kg, 2.0 kg, 3.0 kg, the weighted average is: 1.0 + 2.0 + 3.0 6.0 ------------------- = ------ = 2.0 kg 3 3 Given that you have 2 items of A, 3 items of B, and item of C. 2(1.0) + 3(2.0) + 1(3.0) 2.0 + 6.0 + 3.0 ------------------------------ = ------------------- = 1.8 kg 6 6

Calculating Average Atomic Mass Example: 1 Lithium exists as 2 isotopes: Li – 6 & Li – 7 Li – 6 = 7.4% Li – 7 = 92.6% Mass of Li – 7 is 7.015u and Li – 6 is 6.015u Avg. atomic mass = = 6.941u

Example Isotope Atomic Mass Unit (u) Relative Abundance Silver has 2 isotopes. Isotope Atomic Mass Unit (u) Relative Abundance Ag – 107 106.9 51.8 % Ag – 109 108.9 48.2 % What is the average atomic mass of Ag?

Calculating Isotopic Abundance Boron exists as 2 isotopes. B – 10 (10.01u) and B – 11 (11.01u). Calculate the isotope abundance. Solution: From periodic table the avg. atomic mass of B is 10.811u. Let % abundance of B – 10 be x and B – 11 would be 1 – x. 10.811 = x(10.01) + (1 – x)(11.01) 10.811 = 10.01x + 11.01 – 11.01x 11.01 – 10.811 = 11.01x – 10.01x x = 0.197  x = 0.20 Therefore, B -10 is 20% B – 11 is 80%

Homework P 167 #1-4 McGraw Hill P 170 # 5 – 8 McGraw Hill Worksheet for Nelson (see Ms. Munir)