'Naturally occurring isotopes' diaporamas de présentation

CHAPTER 2

CHAPTER 2. Atoms, Molecules, and Ions. Law of Mass Conservation. Mass is neither created nor destroyed in chemical reactions. Also known as Law of Conservation of Matter. 243.7 g. 243.7 g. 159.7 g. 84 g. 111.7 g. 132 g. Law of Definite Proportions.

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Homework from page 104

Homework from page 104. Homework from page 104. Boron has two isotopes. boron-10 mass = 10.013 amu abundance = 19.8% Boron-11 mass = 11.009 amu abundance = 80.2% Calculate its atomic mass. Homework from page 104. (mass x abundance) + (mass x abundance) boron-10

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Average Atomic Mass & % Abundance

Average Atomic Mass & % Abundance. Average Atomic Mass . The weighted average of the atomic masses of the naturally occurring isotopes of an element Most elements occur naturally as mixtures of isotopes. Average Atomic Mass.

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Average Atomic Mass & % Abundance

Average Atomic Mass & % Abundance. Average Atomic Mass . The weighted average of the atomic masses of the naturally occurring isotopes of an element Most elements occur naturally as mixtures of isotopes. Average Atomic Mass.

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Isotopes & Average Atomic Mass

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Isotopes and Ions

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Rubidium is a soft, silvery-white metal that has two common isotopes, Rubidium-85 and Rubidium-87. If the abundance of Rubidium-85 is 72.2% and Rubidium-87 is 27.8%, what is the average atomic mass?.

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