Isotopes As techniques for finding the masses of atoms has improved, we have learned that not all atoms of the same element are identical. Isotopes – atoms.

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Presentation transcript:

Isotopes As techniques for finding the masses of atoms has improved, we have learned that not all atoms of the same element are identical. Isotopes – atoms of the same element that have different masses vary in the number of neutrons they contain in the nucleus almost all elements have more than one isotope. Chemically, isotopes act exactly the same.

Two Isotopes of Sodium

Average Atomic Mass Decimal number listed on periodic table. Weighted average of all the naturally occurring isotopes of that element. No atom has this exact mass.

Think About It Hydrogen has two natural isotopes hydrogen-1 and hydrogen-2. The atomic mass for hydrogen is amu. Explain why the atomic mass is not Chlorine has two naturally occurring isotopes, chlorine-37 and chlorine-35. Which isotope is more abundant? How do you know?

Counting Atoms and the Mole

Counting Atoms SI unit for amount of substance is called mole. A mole measures the number of particles within a substance. A mole refers to a specific number of particles. (Counting Unit)

1 mole = 6.02 x particles 6.02 x is also known as Avogadro’s Number 1 mole magnesium = 6.02 x Mg atoms 1 mole zinc = 6.02 x Zn atoms 1 mole lead = 6.02 x Pb atoms

Molar Mass Although 1 mole always contains the same number of particles, the mass of one mole varies depending on the substance. Molar Mass – mass of one mole of a substance. Mass of one mole of an element is equal to its ATOMIC MASS expressed in grams. –1 mole of magnesium = grams –1 mole of zinc = grams –1 mole of lead = grams

One Minute Paper You have one minute to answer these two questions concerning today’s lesson. –What was the most important thing you learned? –What is still muddy?