Isotopes

Isotopes

Never trust an atom.

They make up everything.

REMEMBER

• An atom is the smallest unit that retains the identity of the element

• IT IS NOT INDIVISIBLE... atoms are made up of protons, neutrons, and electrons

• THIS GOES AGAINST DALTON'S ORIGINAL ATOMIC THEORY

• In an atom # protons = # electrons so an atom is NEUTRAL

REMEMBER

• An isotope is the same element with different amounts of neutrons

• ONLY THE NEUTRONS DIFFER

• If you change the protons, it is no longer the same element

• Each isotope with have a different mass due to the varying amount of neutrons

REMEMBER

• An ion must have a charge either positive or negative

• THIS MEANS THE PROTONS AND ELECTRONS ARE NOT EQUAL

REMEMBER

• The atomic number DOES NOT HAVE A DECIMAL

• It is equal to the proton amount

• This number also determines THE ELEMENT

• If you change the atomic number/protons YOU CHANGE THE ELEMENT

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REMEMBER

• The atomic number equals the amount of protons

• If you know the element name, you can find the atomic number and protons from the periodic table

REMEMBER

• Mass number is the protons + neutrons

• IT IS NOT THE ATOMIC MASS (decimal number on the periodic table block)

• ONLY USE A ROUNDED ATOMIC MASS WHEN NO OTHER INFORMATION IS AVAILABLE

• If you know the mass number you can calculate neutrons

• If you know neutrons, you can calculate mass number

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REMEMBER

• The mass number IS NOT THE SAME as atomic mass

• Mass # = p⁺ + n⁰

• You can subtract the protons from the mass number to find the neutrons

• Mass number can be found after the hyphen or on the upper left hand side of a symbol

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REMEMBER

• When there is a charge, the electrons and protons ARE NOT EQUAL

• The difference between them is the numerical value of your charge

• If you have more electrons it is NEGATIVE

• If you have more protons it is POSITIVE

• ONLY CHANGE THE ELECTRONS

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