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Isotopes and Ions

Learn about isotopes, atomic masses, ions, and their properties in chemistry. Explore examples and notations for elements with varying numbers of protons, neutrons, and electrons.

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Isotopes and Ions

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  1. Isotopes and Ions Section 3-3 Continued

  2. Isotopes • Atoms of the same element that have different masses • Have the same number of protons and electrons but different numbers of neutrons

  3. Bromine – 80 Write the hyphen notation for the element that contains 15 electrons and 15 neutrons 13C 6 35 p, 35 e, 45 n Phosphorus – 30 6 p, 6 e, 7 n How many protons, neutrons, & electrons are in the following?

  4. Average Atomic Mass • Weighted average of the atomic masses of naturally occurring isotopes of an element • This is the number that appears on the periodic table • (abundance of isotope in decimal form) X (atomic mass of isotope) + (abundance of isotope in decimal form) X (atomic mass of isotope)

  5. Example • Naturally occurring copper consists of 69.17% copper-63, which has an atomic mass of 62.929 599 and 30.83% copper-65, which has an atomic mass of 64.927 793. Find the average atomic mass of copper. • (.6917) X (62.929 599) + (.3083) X (64.927 793) = • 43.5284 + 20.0172 = 63.55

  6. Ions • An atom or group of bonded atoms that has a positive or negative charge • Positive ions have lost electrons. They have more protons than electrons. Ex: Ca2+ • Negative ions have gained electrons. They have more electrons than protons. Ex: N3-

  7. Na+ Cl- Mg2+ O2- Al3+ 11 p, 12 n, 10 e 17 p, 18 n, 18 e 12 p, 12 n, 10 e 8 p, 8 n, 10 e 13 p, 14 n, 10 e How many protons, neutrons, and electrons are in the following:

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