Distinguishing Among Atoms

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Presentation transcript:

Distinguishing Among Atoms

Essential Questions

Periodic Table Key

Atomic Number All atoms are made up of protons, neutrons, and electrons But, every different element has a different number of protons This # is the atomic number Example: Oxygen and only Oxygen has 8 protons Since atoms have a neutral charge, how many electrons must be in each atom?. So the atomic number is equal to the number of ________ and the number of _______ in each atom..

Atomic Mass Or Mass Number We know the atomic # tells us the number of H+ (protons) in an atom (and the number of e- (electrons). Atomic Mass (Mass Number) is more than that. It is how much matter that is in the atom. Protons, electrons, and Neutrons. Since Protons and Neutrons are the majority of the mass, the number is close to the number of protons and neutrons added together. (we will talk about the difference later)

Atomic Mass How many neutrons in H? In B? In O? In Ne? Or Mass Number The Atomic number tells us more than just the total mass. Since we know that atomic mass = all electrons, protons, and neutrons. What would we get if we subtract the atomic number? Remember, electrons have virtually no mass when compared to protons and neutrons. How many neutrons in H? In B? In O? In Ne?

Atomic Mass Or Mass Number If Uranium has an Atomic Mass of 235 and 92 e- , what is the atomic #? Sometimes chemists write atomic mass, atomic number, and chemical symbol in a shorthand fashion. For example: Which is the big #, Atomic # or Mass#?

How many neutrons In each? Isotopes Every element has a specific number of protons If there are a different number of protons, we have a different element. If we have a different number of neutrons, we do not have a different element. What we have is an isotope. How many neutrons In each?

Atomic Mass What are the atomic #s of each of these isotopes? What are the Mass #s or each of these isotopes?

Atomic Mass

Atomic Mass Subatomic particles are extremely small. The mass of a proton is about 1.67*10-24 g The mass of a electron is about 9.11*10-28 g These numbers are really hard to use all the time, so scientists decided to use a standard reference. Carbon-12 (the most common isotope) has 6 protons and 6 neutrons. These scientists decided to make this element equal 12 atomic mass units (AMU)s 1 AMU = 1/12 of the mass of a Carbon-12 atom

Atomic Mass and Relative Abundance You may have noticed that the atomic masses are not whole numbers. A little of this difference comes from the electrons, but most of it comes from the isotopes. 0.99985*1.0078 + 0.00015*2.0141 1.00764883 + 0.000302115 1.007950945 Weighted Average

Review

Essential Questions