Distinguishing Between Atoms

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Presentation transcript:

Distinguishing Between Atoms Lecture I Atomic Structure Review

I. Atomic Structure Review Rutherford Model of the Atom Three subatomic particles Nucleus: Center of atom-contains Protons: (+) charge 1 atomic mass unit Neutrons: no charge Orbitals: Paths around nucleus-great distance from nucleus-contain Electrons: (-)charge 1/1840 amu

II. Atomic Number Atomic Number: The number of protons in the nucleus. Elements differ because of different number of protons Because atoms are neutral, (+) charge = (- )charge / protons = electrons Element Atomic Number Protons Elec- trons K 19 ____ 5 S 16 V 23

III. Mass Number Mass Number: The total number of protons and neutrons in an atom. Most mass is concentrated in nucleus-that is where these particles are located If you know the atomic number and mass number you can determine atom’s composition. # neutrons = mass # - atomic number Shorthand Notation / Nuclear Notation Symbol with mass as superscript 197Au atomic number as subscript 79

1H 1 197Au 79 35Cl 17 38Cl Element Hydrogen oxygen # protons # electrons # Neutrons Mass Number Atomic Number Nuclear Notation 1H 1 197Au 79 35Cl 17 38Cl

Gold Chlorine 1 8 79 17 118 18 21 16 197 35 38 1H 8 O 197Au 35Cl 38Cl Element Hydrogen oxygen Gold Chlorine # protons 1 8 79 17 # electrons # Neutrons 118 18 21 Mass Number 16 197 35 38 Atomic Number Nuclear Notation 1H 8 O 197Au 35Cl 38Cl

IV. Isotopes Isotopes: atoms that have the same number of protons and electrons but different number of neutrons. Different masses mean they have different mass numbers Chemical behavior is the same Three isotopes of hydrogen: hydrogen, deuterium, tritium

2H 3H 1H 1 Isotope Nuclear Notation Protons Electrons Neutrons Mass Number Protium 1H 1 Deuterium 2H Tritium 3H

V. Atomic Mass Because mass of atoms so small and inconvenient to work with (fluorine 3.155 X 10-23) it is more useful to compare relative masses of atoms using a reference isotope as a standard. Carbon-12 is used. Atomic Mass Unit (amu) = 1/12 mass of carbon atom. Atomic mass: weighted average mass of naturally occuring isotopes. Estimate atomic mass: look at relative abundance Calculate atomic mass: multiply the mass of each isotope by its natural percent abundance (expressed as a decimal) also known as the relative abundance, and add products.

Calculate Atomic Mass of Sulfur Nuclear Notation Natural Percent Abundance Mass (amu) Relative Abundance 32S 16 95.002 31.972 33S 0.76 32.971 34S 4.22 33.967 36S 0.014 35.967 Calculate atomic mass: multiply the mass of each isotope by its relative abundance and add products.

VI. The Periodic Table-A Preview The periodic table allows you to easily compare one element to another. Horizontal rows are called periods. Vertical columns are called groups or families. http://www.ptable.com/ http://www.webelements.com/