CCL 1110 1st Edition Lecture 4Outline of Last Lecture I. I.Some Important PeopleII. Experiments/LawsOutline of Current Lecture II. Atomic Structuresa. DefinitionsIII. Atomic Massesa. Definitions IV. The Periodic Tablea. Group NamesV. Molecular and Ionic compoundsVI. Naming Ionic and Molecular CompoundsCurrent LectureI. Atomic Structures- Mass number- number of protons plus neutrons- Atomic number- number of protons or electrons- Isotopes- atoms with identical atomic numbers but different mass numbersII. Atomic Massesa. Atomic mass- mass of a single atom in atomic mass units (amu)b. Molecular mass- mass of a single molecule in AMUc. Formula Unit mass- ass of all the atoms in a formula unit in AMUIII. Periodic Tablea. Elements in the same group often have similar chemical and physical propertiesb. Also have similarities in the arrangement of their electronsc. Rows=periodsd. Columns=groupse. Elements on the table are either metals, transition metals, metalloids, gasesi. Group 1A-Alkali metalsii. Group 2A-Alkali earth metalsiii. Group 6A-Chalcogensiv. Group 7A-Halogensv. Group 8A-Noble gasesThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.IV. Molecular and Ionic Compoundsa. Two or more atoms are bound together by chemical bondsb. Diatomic molecules- H, O, N, F, Cl, Br, I c. A molecular compound is composed of molecules that contains more than one type of atomi. Usually nonmetals and/or metalloidsd. Ions- formed when atoms gains or loses electronsi. Cations- positive ion formed when electrons are lost, typically metalsii. Anions- negative ion formed when electrons are gained, typically nonmetalse. Ionic compounds- compound that contains positive and negative charged ionsf. The net charge of ionic compounds MUST equal zeroV. Naming Ionic and Molecular Compoundsi. Metals with only one type of ion1. Groups 1A and 2A, Al, Zn, Ag2. Ex. NaCl (sodium chloride) CaO (calcium oxide)3. Metal name + Nonmetal name with –ide suffixii. Metals with two or more types of different ions1. Most metals except groups 1A and 2A2. Ex. CuCl (copper(I) chloride), FeO (iron(II) oxide)3. Metal name (oxidation state as Roman numeral in parenthesis) + nonmetal name with –ide suffixiii. Hydrates- compounds whose crystals contain discrete water molecules1. Ex. CuSO4*5H2O copper(II) sulfate pentahydrate2. Name as other ionic compounds except add prefix + hydrate as a third wordb. Molecular compounds (nonmetal+metal)i. Both elements from right hand side of periodic tableii. Ex. N2O4 (dinitrogen tetroxide)iii. MEMORIZE THESE PREFIXES1. Mono2. Di3. Tri4. Tetra5. Penta6. Hexa7. Hepta8. Octa9. Nona10. Decaiv. Usually element with lower group number named firstv. Omit “moo” for the first element namedvi. Double vowels are often avoidedvii. Common names often used for hydrogen compoundsc. Polyatomic Ionsi. “-ate”=one more oxygen than “-ite”ii. Compounds of polyatomic ions are named like binary ionic compoundsd. Binary Aqueous Acidsi. Acids yield H+ ions in waterii. Binary acids contain two elements (aq) in wateriii. Hydro + (partial) element name with –ic suffix + acidiv. Note: if you remove water, pure acids revert to “normal” namee. Oxoacidsi. Contain hydrogen, oxygen, and a third elementii. (partial) element name + suffix +