Thursday October 18, 2012 (Average Atomic Mass). Which one of the listed elements has the smallest atomic radius – Mg, Ca, Ba the greatest ionization.

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Presentation transcript:

Thursday October 18, 2012 (Average Atomic Mass)

Which one of the listed elements has the smallest atomic radius – Mg, Ca, Ba the greatest ionization energy – Sr, Ag, I the least electron affinity – C, Ga, In the largest ionic radius – Cs, Hg, At the least electronegativity – Al, Ga, Tl

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Assignment Currently Open Summative or Formative? Date IssuedDate Due Date Into GradeSpeed Final Day QUIZ 6S310/5 10/19 QUIZ 7S410/12 10/26 WS – The Periodic Table F110/1110/1710/19 WS – The Periodic Law F210/1210/1710/19 WS – Periodic Properties F310/1510/1710/19 Pop Quiz – The Periodic Table and the Periodic Law F410/16

Average Atomic Mass The mass number of an element is the number listed (usually) under the atomic symbol on a Periodic Table tile. Notice it is not a whole number, but contains decimal places. The mass number is the top number in isotopic notation, and is rounded off.

Average Atomic Mass Why is the atomic mass not a whole number? The atomic mass number is an average of all of the masses of the different isotopes of that particular element.

Average Atomic Mass What is an isotope? Isotopes are atoms of the same element that have different numbers of neutrons.

Average Atomic Mass What is the relationship between isotopes and atomic mass? The average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element.

Average Atomic Mass The average atomic mass of an element depends on both the mass and the relative abundance of each of the element’s isotopes. For example, naturally occurring copper consists of 69.17% copper-63, which has an atomic mass of amu, and 30.83% copper-65, which has an atomic mass of amu. The average atomic mass of copper can be calculated by multiplying the atomic mass of each isotope by its relative abundance (expressed in decimal form) and adding the results. ( × amu) + ( × amu) = amu The calculated average atomic mass of naturally occurring copper is amu.

Average Atomic Mass Why is it important to know the percent abundance of each isotope in an element? Knowing this information allows us to calculate the average atomic mass of an element. What do you get when you add up all of the percent abundances of all of the isotopes? 100% What information do you need to calculate the average atomic mass of an element?

Average Atomic Mass Sample Problem Uranium has three naturally occurring isotopes as follows: uranium-234: abundance 0.005%, atomic mass uranium-235: abundance 0.720%, atomic mass uranium-238: abundance %, atomic mass Calculate the average atomic mass of uranium.

The Least You Need to Know The average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element. Isotopes are atoms of the same element that have different numbers of neutrons.

Worksheet Average Atomic Mass