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Notes for Isotopes

This presentation defines atomic number, mass number, and describes how they apply to isotopes

Camille Whiteside

on 30 September 2013

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Transcript of Notes for Isotopes

Remember that an
atomic number:
is the number of protons in the nucleus of an atom
identifies an element
atoms of the same element with different numbers of neutrons.
Most elements consist of mixtures of isotopes.
Ex: Tin (Sn) has 10 stable isotopes!
Consider Hydrogen (H)....
3 known isotopes: protium, deuterium, and tritium
protium - 99.985%
deuterium - 0.015%
tritium - very small amounts in nature, can be made artificially, radioactive!
Mass Number
the total number of protons & neutrons in the nucleus of an atom
The atomic mass listed in the periodic table for an element is the average of all of the naturally occurring isotopes of an element.
Since Isotopes have more or less neutrons, its mass number will be different from what is in the periodic table. It is usually shown like this...
Consider Uranium.....
used as fuel for nuclear power plants
This pic is of the Clinton Nuclear Power Station in Clinton, IL
Uranium-235 is the nuclear symbol notation for this isotope.
Let's Practice:
1. Chlorine-37 has how many protons, neutrons, and electrons?

2. Carbon-13 has how many protons, neutrons, and electrons?

3. Write the hyphen notation for the element whose atoms contain 7 electrons and 9 neutrons.
C-14 or Carbon-14
This means that instead of carbon having a mass of 12 it has a mass of 14.
Why is it larger?
Carbon-14 has 2 extra neutrons!

Isotopes and their uses

Bone scans with radioactive technetium-99.
Full transcript