LAB - Atomic Mass Candium PDF

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stoichiometry practice...

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The Average Atomic Mass of Candium Purpose: To analyze the isotopes of Candium and to calculate its average “atomic” mass. Procedure:

1. Obtain a sample of the element “Candium”. Separate the three “isotopes” of Candium (M&M’ium, Gummybearium, and Choconuttium). 2. Count the number of “atoms” (candies) of each isotope (type of candy) and determine the “Percent Abundance” of each “isotope”. 3. Determine the total mass in grams of each isotope and the average mass of each “Isotope” Note: SHOW ALL WORK; DO NOT ROUND YOUR NUMBERS; 1 gram = 1 amu Isotope 1 – M&M’ium Number of “Atoms” of the “isotope”. (count the candies) PERCENT ABUNDANCE (divide the number of candies by the total number of candies) RELATIVE ABUNDANCE How do you write the percent as a decimal? Total Mass of the “isotopes”. (record the mass of the candies by placing them on a paper towel) (amu) Average Mass of each “isotope” (amu). divide the total mass by the number of candies Analysis Calculations:

Isotope 2 Isotope 3 – Gummybearium Choconuttium

Totals

1. Calculate the average “atomic” mass of Candium. 1. Multiply the Average Mass x Percent Abundance as decimal for each of each “isotope” of candium. This value will be known as the relative mass. 2. Then add the 3 relative masses together. Show your work and record your answers with 4 decimal places. Relative Mass of M&M’ium: Relative Mass of Gummybearrium:

Relative Mass of Choconuttium:

Final Average Atomic Mass of Candium in amu (Add the mass together):

______________ + ______________ + ______________ = ______________ 2. Which “isotope” contributed most to the average “atomic” mass of the “element”? How do you know?

3. Propose a bar graph demonstrating your understanding of the concept of Average Atomic Weights of the isotopes of Candium. Your X-axis will be the “average mass” and the Y-axis will be the “Percent abundance” in a percent....