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UofL CHEM 101 - Compounds
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Chem 101 1st Edition Lecture 3 Outline of Last Lecture I. Regions of the Periodic Table and Covalent CompoundsOutline of Current Lecture II. CompoundsIII. Covalent compoundsa. Naming covalent compoundsIV. Ionic Compoundsa. Naming ionic compoundsCurrent LectureI. Compoundsa. Covalent compounds: Are formed via covalent bonds. A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms.i. How will you know if it is a covalent bond? Covalent bonds form between nonmetals. To determine if a compound is covalent look to your periodic table and determine if the elements are metal, nonmetal, or metalloids.ii. Naming Covalent Bonds: The first element is named first, using the elements name. Second element is named as an Anion (suffix "-ide")1. Prefixes are used to denote the number of atoms. You must memorize these. "Mono" is not used to name the first element. These 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.iii. Example: Carbon oxide ( CO )1. S – sulfide2. O – oxide 3. N – nitride4. Se – Selenide 5. B – boride6. I – iodide7. Cl – Chloride8. F – fluoride 9. As – Arsenide10. P – phosphide iv. Properties of Covalent Bonds: they typically have low melting points b. Ionic Compounds: are composed of ionic bonds; a type of chemical bond that involves the electrostatic attraction between oppositely charged io ns and the transferring of electrons. i. The ions represent atoms that have lost one or more electrons (known as cations) and atoms that have gained one or more electrons (known as an anion).ii. These bonds form between metals and nonmetals. You can determine if acompound is ionic if one of the atoms is that of a metal element. Metals lose electrons to nonmetals. iii. Cations are positively charged. Anions are negatively charged. The differences in charges is what forms the attractions between the cations and anions. The opposite charges balance each other out. iv. Alkali metals are unstable and quick to lose electrons. v. Formula Units are the empirical formula of any ionic or covalent network solid compound used as an independent entity for stoichiometric calculations. It is the lowest whole number ratio of ions represented in anionic compound.vi. Cations can either have a fixed charge or a variable charge. 1. Anions always have a fixed charge. To figure out the charge of an anion take the group number of the atom and subtract 18. 2. Cations with a fixed charge:a. Metals from Group 1 gave a charge of +1b. Metals from Group 2 gave a charge of +2c. Metals from Group 13 have a charge of +3 d. Al and Ga from Group 13 also have a fixed charge of +3e. Zn has a fixed charge of +2f. Ag +1 ion3. Cations with a variable charge:a. Transition metals (with Zn and Ag as exceptions)b. Fe: Fe+2, Fe+3c. Cu: Cu+, Cu+2d. Co: Co+2, Co+3vii. Naming Ionic Compounds: the cation (positively charged ion) is always named first. The anion is written second in the name. 1. If the cation is a metal ion with a fixed charge, the name of the cation is the same as the (neutral) element from which it is derived (e.g., Na+ = "sodium"). 2. If the cation is a metal ion with a variable charge, the charge on the cation is indicated using a Roman numeral, in parentheses, immediately following the name of the cation (e.g., Fe3+ = "iron(III)").a. Fe+3  Iron (III) b. Cu+  Copper (I) c. Co+2  Cobalt (II) 3. If the anion is a monatomic ion, the anion is named by adding the suffix -ide to the root of the element name (e.g., I- = "iodide") \4. Note: Greek prefixes are not used to indicate the number of atoms, or polyatomic ions, in the formula unit for the compound (ex, Ca(NO3)2 is named "calcium nitrate" not "calciuim dinitrate").Ex: Na2S – Sodium


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UofL CHEM 101 - Compounds

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