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Transcript
Chapter 3 Chemical Foundations The Elements: The name for the elements come from many sources. Often the elements names are derived from Greek, Latin, or German words that describe a property of the element. NOTE: Ex. Gold (Au) come from aurum- a Latin word meaning “shinning dawn.” Element symbols are used to represent the elements. They usually (not always) contain the first or first two letters of the element name. Ex. Fluorine F Zinc Zn See textbook pg 51 for more information about common symbols. Subatomic Particles Particle Symbol Proton Neutron Electron p+ n e- Mass (g) 1.67262x10-24 1.67262x10-24 9.10939x10-28 Charge (Coulomb) +1.6022x10-19 0 -1.6022x10-19 Relative Charge +1 0 -1 Location in Atom Inside Nucleus Inside Nucleus Outside Nucleus Atomic Number, Mass Number, and Nucleus atomic number (Z) = mass number (A) = element symbol (X) = Note: mass number= Therefore …. mass number = ……. A= Z + number of neutrons ….. Number of neutrons = A-Z Note: For any given element on the periodic table: Number of protons = In order to symbolically represent elements and isotopes chemists use the following notation: Mass Number X Atomic number Ex: Isotopes are atoms with identical atomic numbers but different mass numbers (that is, same number of protons but different number of neutrons) Exercise: 1. How many protons, electrons, and neutrons are in an atom of 197Au ? 2. Magnesium has three isotopes, with mass numbers of 24, 25, 26. a. Write the complete chemical symbol for each of them. b. How many neutrons are in an atom of each isotope? 3. Fill in the gaps in the following table, assuming each column represents a neutral atom. 65 Zn Symbol Protons 44 92 Neutrons 57 49 Electrons 38 47 Mass no. 108 235