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Unit 3: Counting atoms

Unit 3: Counting atoms

Unit 3: Counting atoms. Subatomic Particles. Proton. Determines the element Number of protons CANNOT change for an element Common charge notation is +1 Mass (g) = 1.673 x 10 -24 Mass ( amu )= 1.0073 = 1. Neutron. Common charge notation is 0. No charge!

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433 views • 18 slides
Isotopes

Isotopes

Isotopes. 436. Objectives: 5.2 Identify the advantages and disadvantages of using isotopes in industry, medical science, basic research, and in the environment. 5.3 Analyze the irregularities in the progression of the atomic masses of the elements in the periodic table.

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133 views • 9 slides
Bellringer 10/01/12

Bellringer 10/01/12

Bellringer 10/01/12. How many protons, neutrons and electrons are in U-235 and Pu-244?. Mass (amu). x. Relative abundance (% as a decimal). Calculating Average Mass. Atomic mass is the average of all the naturally isotopes of that element. Copper = 63.546 amu. Cu. Cu. Copper-63.

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170 views • 7 slides
Calculating Average Mass

Calculating Average Mass

Mass (amu). x. Relative abundance (% as a decimal). Calculating Average Mass. Atomic mass is the average of all the naturally isotopes of that element. Copper = 63.546 amu. Cu. Cu. Copper-63. 62.93 amu. x. 0.692. = 43.54756 amu. +. Copper-65. 64.93 amu. x. 0.308.

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285 views • 6 slides
Calculating Average Mass

Calculating Average Mass

Mass (amu). x. Relative abundance (% as a decimal). Calculating Average Mass. Atomic mass is the average of all the naturally isotopes of that element. Copper = 63.546 amu. Cu. Cu. Copper-63. 62.93 amu. x. 0.692. = 43.54756 amu. +. Copper-65. 64.93 amu. x. 0.308.

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139 views • 6 slides

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