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Chapter 5 Types of Compounds

Chapter 5 Types of Compounds. Ionic Compounds Covalent Compounds. Electronegativity (EN). Def: The strength with which an atom in a bond pulls on e-s. Covalent Bonds (bonds btwn 2 nonmetals). Nonmetals have high electronegativity values (REVIEW) Electrons are shared

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Chapter 5 Types of Compounds

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  1. Chapter 5Types of Compounds • Ionic Compounds • Covalent Compounds LecturePLUS Timberlake

  2. Electronegativity (EN) Def: The strength with which an atom in a bond pulls on e-s. LecturePLUS Timberlake

  3. Covalent Bonds (bonds btwn 2 nonmetals) • Nonmetals have high electronegativity values (REVIEW) • Electrons are shared single bond shares 1 pair electrons double bond shares 2 pairs electrons triple bond shares 3 pairs electrons LecturePLUS Timberlake

  4. Covalent Bonds Two nonmetal atoms form a covalent bond because they have less energy (are more stable!) after they bonded H+H H : H = HH = H2hydrogen molecule LecturePLUS Timberlake

  5. Learning Check Indicate whether a bond between the following would be 1) Ionic 2) covalent ____ A. sodium & oxygen ____ B. nitrogen & oxygen ____ C. phosphorus & chlorine ____ D. calcium & sulfur ____ E. chlorine & bromine LecturePLUS Timberlake

  6. Solution Indicate whether a bond between the following would be 1) Ionic 2) covalent 1 A. sodium and oxygen 2 B. nitrogen and oxygen 2 C. phosphorus and chlorine 1 D. calcium and sulfur 2 E. chlorine and bromine LecturePLUS Timberlake

  7. Types of Covalent (Molecular) Cpds • Elements that form diatomic molecules • Binary covalent compounds • Organic compounds/ Hydrocarbon • Acids & Bases • (Common v. Formal Names) LecturePLUS Timberlake

  8. Diatomic Elements Elements that exist as diatomic molecules are : H2, F2, N2, O2, Cl2, Br2, I2 octets       N  + N  N:::N  triple bond LecturePLUS Timberlake

  9. Learning Check Use the name of the element to name a diatomic molecules. H2 hydrogen N2 nitrogen Cl2 _______________ O2 _______________ I2 _______________ LecturePLUS Timberlake

  10. Solution Use the name of the element to name the following diatomic molecules. H2 hydrogen N2 nitrogen Cl2chlorine O2oxygen I2iodine LecturePLUS Timberlake

  11. Naming Binary Covalent Compounds Two nonmetals (def of binary covalent) • Name each element • End the last element in -ide • Add prefixes to show how many atoms of each • (except when there’s only 1 atom of the 1st element listed) Prefixes-(see Table 5.5, p 168 of text) mon 1 penta 5 di 2 hexa 6 tri 3 hepta 7 tetra 4 octa 8 LecturePLUS Timberlake

  12. Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO2 carbon _______________ PCl3 phosphorus _______chloride CCl4 carbon ________chloride N2O _____nitrogen _____oxide LecturePLUS Timberlake

  13. Solution CO carbon monoxide CO2 carbon dioxide PCl3 phosphorus trichloride CCl4 carbon tetrachloride N2O dinitrogen monoxide LecturePLUS Timberlake

  14. Learning Check A. P2O5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide B. Cl2O71) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide C. Cl21) chlorine 2) dichlorine 3) dichloride LecturePLUS Timberlake

  15. Solution A. P2O5 3) diphosphorus pentoxide B. Cl2O71) dichlorine heptoxide C. Cl21) chlorine LecturePLUS Timberlake

  16. Naming Organic Compounds • Def: organic compounds contain __ atoms hooked together. • (Why do you think this element can hook up with many other atoms, including itself?)

  17. Hydrocarbons-A Type of Organic Compound • Def: hydrocarbons are made of ___ & ___ • They are named by the number of Carbon atoms a molecule contains. • See Table 5.8, p 183

  18. Table 5.8: Hydrocarbons CH4 methane C2H6 ethane C3H8 propane C4H10 butane C5H12 pentane C6H14 hexane C7H16 heptane C8H18 octane C9H20 nonane C10H22 decane

  19. Common v. Formal Names • Formal Names follow the rules we have learned for naming compounds. • Common Names are ones that don’t follow these rules. • Ex: water=

  20. Frequently Used Common Names • Water = H2O • Ammonia = NH3 • Common Acids & Bases

  21. Acids & Bases (Table 5.7, p 182) ACIDS Formula Name HCl hydrochloric acid H2SO4 sulfuric acid H3PO4 phosphoric acid HNO3 nitric acid HC2H3O2 acetic acid (vinegar)

  22. Table 5.7 (cont.): BASES Formula Name NaOH sodium hydroxide KOH potassium hydroxide NH3 ammonia

  23. Covalent Bonds in NH3 Bonding pairs H   H: N : H   Lone pair of electrons LecturePLUS Timberlake

  24. Allotropes • Def: molecules of the same element that differ in structure • Ex: Carbon…graphite, charcoal, Buckminsterfullerine (“bucky ball”) - see Fig ___ on p ___ of text • Ex2: O2 (oxygen) and O3 (ozone)

  25. Q:Why do we have to specify the number of atoms of each element in a covalent compound? • A: Atoms of the same elements can combine in different ratios. • Ex: C & O • CO • CO2

  26. Writing Formulas for Covalent Compounds 1. Identify it as a covalent: containing only nonmetals. 2. Determine what type of covalent it is: diatomic element binary hydrocarbon (ends in –ane) acid/base 3. Reverse the naming process. LecturePLUS Timberlake

  27. Naming Ionic Compounds • Binary Ionic • Ionic Compounds contain-ing Polyatomic Ions. • Ionic Cpds containing Transition Metals LecturePLUS Timberlake

  28. PLEASE NOTE: • IF YOU ARE UNABLE TO IDENTIFY IONIC & COVALENT COMPOUNDS, YOU WILL BE LOST!!! • PLEASE SEE ME IMMEDIATELY TO GET CAUGHT UP. LecturePLUS Timberlake

  29. Ionic Bonding & Electronegativity • Nonmetals have high EN’s. • Metals have low EN’s. Bonds between a metal & a nonmetal involve transfers of e-s b/c of the big difference in EN! LecturePLUS Timberlake

  30. Binary Ionic Compounds • Binary= 2 elements • Ionic= 1 metal & 1 nonmetal LecturePLUS Timberlake

  31. Naming Binary Ionic Compounds 1. Identify & name the 2 elements in the compound. 2. Name the cation, which is the given the name of the element. 3. Name the anion, which is given the name of the element, w/the ending changed to “–ide.” LecturePLUS Timberlake

  32. PRACTICE Naming Binary Ionic Compounds 1. Na║Cl 2. Na = “sodium” 3. Cl = “chloride” (full name is “sodium chloride”) LecturePLUS Timberlake

  33. PRACTICE Naming Binary Ionic Compounds 1. Li2O 2 & 3. ____║____= ______ ______ (cation(anion (cation name) (anion name) symbol) symbol) LecturePLUS Timberlake

  34. MORE PRACTICE Naming Binary Ionic Compounds-p __ of I.N. • KF • CaF2 • Al2O3 LecturePLUS Timberlake

  35. Naming Ionic Compounds w/ Polyatomic Ions • DEF: Charged particles containing more than 1 type of atom. Ex: SO42- LecturePLUS Timberlake

  36. Naming Ionic Compounds w/ Polyatomic Ions • Identify the cation & the anion. (Draw a line between the 2 ions) • Name the cation, then the anion (find polyatomics on Table 5.3, p 159 of text). That’s it! LecturePLUS Timberlake

  37. PRACTICE :Naming Ionic Compounds w/ Polyatomic Ions EX: Na2SO4 ____║____= ______ ______ (cation(anion (cation name) (anion name) symbol) symbol) LecturePLUS Timberlake

  38. Naming Ionic Compounds w/ Polyatomic Ions • Most polyatomic ions are anions. LecturePLUS Timberlake

  39. A Couple of Important Exceptions w/Polyatomic Ions Important Exception #1: there are 2 cations that contain NO METALS: NH4+ (ammonium) H3O+ (hydronium) (this can be tricky b/c we have always identified ionic compounds because they start with a metal cation.) LecturePLUS Timberlake

  40. A Couple of Important Exceptions w/Polyatomic Ions Important Exception #2: Some anions contain metals. Ex: MnO4- = permanganate Cr2O72- = dichromate (this can be tricky b/c anions are usually a nonmetal) LecturePLUS Timberlake

  41. Copy Table 5.2 into Notes LecturePLUS Timberlake

  42. Naming Ionic Cpds Containing Transition Metals Ex: NiO2 • Determine the total # of negative charges in a unit of the compound: Ex: O2- & O2- = 4 total - charges 2. Determine the charge on the cation that will give you 4 total + charges Ex: Ni4+ 3. Write the cation & anion names. Write cation with the oxidation # written as a Roman numeral in parentheses: Ex: nickel (IV) oxide LecturePLUS Timberlake

  43. Writing Formulas for Binary Ionic Compounds 1. Identify the ionic charge (“oxidation number”) on the cation & anion. LecturePLUS Timberlake

  44. Writing Formulas for Binary Ionic Compounds ELEMENT OXIDATION # • Group 1 1+ • Group 2 2+ • Group 13 3+ • Group 14 4+ or 4- • Group 15 3- • Group 16 2- • Group 17 1- LecturePLUS Timberlake

  45. Practice Predicting Oxidation #s • Li • O • Mg • F • B LecturePLUS Timberlake

  46. Writing Formulas for Binary Ionic Compounds 2. A compound has NO CHARGE on it, so a formula unit (the smallest ratio of cations to anions) must have equal numbers of + & - charges. (use the LCM) LecturePLUS Timberlake

  47. Cross-Over Method • You can use this to write formulas. • Take the charge on the cation and use it as the subscript on the anion • Take the charge on the anion and use it as the subscript on the cation • Reduce the subscripts, if necessary LecturePLUS Timberlake

  48. Using the LCM to Write Ionic Formulas • Ex: Li & F • Ex: Li & O • Ex: Al & O LecturePLUS Timberlake

  49. ANSWERS • LiF • Li2O • Al2O3 LecturePLUS Timberlake

  50. Writing Formulas for I.Cpds Containing Polyatomic Ions • Determine the cation & anion • Determine the oxidation # on each ion. (oxidation #s for polyatomics are found on Table 5.2) • Write a balanced formula • If there is more than 1 of an ion, use parentheses, then a subscript LecturePLUS Timberlake

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