Lesson 13

Lesson 13:

Today's lesson touched on everything about isotopes: what they are, how common they are based on certain elements, and how there's no such thing as a "regular" atom of an element and an isotope. The quantity of a certain isotope that appears in a sample of an element is referred to as the "natural percent abundance". You can write isotope names with hyphen notation and nuclear notation:
              Boron-10 is B-10 in hyphen notation.
              Boron-10 is 10/5 B in nuclear notation, where 10 represents the mass # and 5 is the atomic
              number.

Problems:
2.) Explain the difference between the atomic masses listed on the periodic table and the mass of an atom. The mass of a single atom can be calculated by rounding the atomic mass on the table to the nearest whole number (I think, does anyone agree?) If that's not it, then the mass is simply the number of protons and neutrons in a neutrally-charged atom. The atomic mass on the periodic table states the average mass of the most common isotope(s) of an element.

9.) Which isotope of nitrogen is found in nature? Explain. The isotope 14/7 N is found in nature. It is the only option of those given that stays true to nitrogen's identity, with 7 protons.