Chem 1061 7th Edition Lecture 3Outline of Last Lecture I. 1.5 Significant FiguresII. 2.5 Atomic Theorya. Subatomic Particlesb. IsotopeIII. 2.6 Periodic TableOutline of Current Lecture I. 2.7 Introduction to Bondinga. Ionic Compoundsb. Covalent Compoundsc. Polyatomic IonsII. 2.8 Formulas, Names, and MassesCurrent Lecture 2.7 Introduction to BondingI. Ionic Compounds: transfer of electrons between elementsa. Bonds happen between metals and nonmetals (metal transfers electrons to nonmetals)b. Includes any compound containing polyatomic ionsc. Ionsi. Cation: Ion with a positive chargeii. Anion: Ion with a negative charged. The strength of any Ionic Bond is based on Coulomb’s Lawi. Energy x (charge1 x charge2)/distancee. Predicting the number of electrons gained/losti. EXAMPLE: NaClThese 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.1. Na: group 1 on the Periodic Table will lose one electron to result inNoble Gas configuration2. Cl: Group 7 on the Periodic Table will gain one electron to result in Noble Gas configuration.ii. SAMPLE PROBLEMS:1. What Ion is formed?a. Lithium?i. ANSWER: Li^+b. Oxygen?i. ANSWER: O^2-II. Covalent Compounds: the sharing of electronsa. Normally happen between nonmetal/nonmetalb. Nucleus of one atom attracts the electrons of the other element and vice versa III. Polyatomic Ions: covalent bonds within an iona. List of polyatomic ions in Table 2.5b. Also there is a list on Moodle under “Things to Know Before Exam 1” that lists the polyatomic ions you should memorizec. Oxoanion: element (usually nonmetal) that is covalently bonded to one or more oxygen atoms. 2.8 Formulas, Names, and MassesHow to put names to formulas and write masses.IV. Ionica. Cation, then anionb. Cation is the name of the metalc. Anion changes the “ine” ending to “ide”d. EXAMPLE: CaBr2 = Calcium BromideNOTE: Table 2.3 has common ionsMetals are positively charged and nonmetals are negatively charged.e. Some compounds have more than one Ion that can be formed. Because of this, you must specify which by either following it with (Roman Numeral 2) or (Roman Numeral 3) or by the trivial name, which is the way you must use on an exam.V. Acid Namesa. All acids contain HYDROGENb. All names are based on the anion namei. They have an “ide” ending like Cl^- (chloride)c. Add enough H^+ to balance charged. Add prefix “Hydro” (Hydrochloride)e. Change “ide” to “ic” (Hydrochloric)f. Add “Acid” as a separate word (Hydrochloric Acid)VI. Polyatomica. Uses prefixes for naming oxoanions found on Fig 2.18b. Change “Ate” to “ic” OR “ite” to “ous”c. KEEP ANY
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