4.3 Distinguishing Among Atoms

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Presentation transcript:

4.3 Distinguishing Among Atoms

Hydrogen 1 H 1.008 Element Name Atomic number Element Symbol Avg. Atomic Mass

} A. Basic Structure + + proton (+) neutron (Ø) Nucleus electron (-) electron cloud neutron (Ø) } + + Nucleus Nucleus: smallest yet heaviest part of the atom

A. Atomic Number Key Idea: Elements are different because they contain different numbers of protons. Atomic # = # Protons # electrons = # protons when atom is neutral

Hydrogen 1 H 1.008 Element Name Element Symbol Avg. Atomic Mass Atomic number # of protons Element Symbol Avg. Atomic Mass

B. Mass Number (atomic mass units = a.m.u) Each proton has a mass value of 1 amu Neutron = 1 amu Electrons are so tiny their mass doesn’t count Mass Number = total # of protons and neutrons.

C. Charge In a neutral atom all of the positive protons are cancelled out by the negative electrons and the overall charge of an atom is zero.

Li D. Notation 1. Isotopic Notation 2. Mass Notation Charge Lithium - 7 Mass # → 7 + Li mass # element name 3 Atomic # →

E. Example 109Ag Sulfur -31 Mass Number = # of protons + neutrons Element Atomic # # Proton Mass # # of Neutrons # of electrons Sulfur -31 109Ag Mass Number = # of protons + neutrons # Neutrons = Mass Number - Protons

E. Example Sulfur -31 109Ag 16 16 31 16 + =31 15 16 47 47 47 + =109 62 Element Atomic # # Proton Mass # # of Neutrons # of electrons Sulfur -31 109Ag 16 16 31 16 + =31 15 16 47 47 47 + =109 62 47 109 Mass Number = # of protons + neutrons # Neutrons = Mass Number - Protons

Isotope Notes EQ: What is an isotope?

A. What is an isotope? Isotope: an atom with a specific number of protons and neutrons Atoms that are isotopes of each other have the same # of protons but differ in the # neutrons and therefore have different mass #’s The number next to the isotope signifies the mass number

What is an isotope? 6 6 8 6 14 12 Example: Carbon Carbon-14 Carbon-12 Protons Neutrons Mass # 6 6 8 6 14 12