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E29: Inorganic Nomenclature

E29: Inorganic Nomenclature. (Naming ionic compounds). You should know…. The oxidation numbers, names, & symbols for the ions on pg. 16 in your WB (test tomorrow) Ca t ions are positive (tend to LOSE e-) A n ions are negative (tend to GAIN e-) Opposites attract!

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E29: Inorganic Nomenclature

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  1. E29: Inorganic Nomenclature (Naming ionic compounds)

  2. You should know… • The oxidation numbers, names, & symbols for the ions on pg. 16 in your WB (test tomorrow) • Cations are positive (tend to LOSE e-) • Anions are negative (tend to GAIN e-) • Opposites attract! • Cations will be attracted to anions in such a way that together their net charge is ZERO (balanced). • Monoatomic = single element (like H+) • Polyatomic = multiple elements bonded (like SO3-2)

  3. Noble gasses= stable (do not bond, no charge) Periodic Table so far… • Elements in the same group share properties +1 Zig zag “staircase” separates metals from nonmetals +2 -2 -1 Transition metals (Roman numerals) Metals | Nonmetals (+) (-)

  4. Noble gasses= stable (do not bond, no charge) More Periodic Table • Group charges tend to continue as we go inward, skipping over the transition metals trench. +1 +2 +3 ±4 -3 -2 -1 Transition metals (Roman numerals)

  5. Formula writing for Ionic Compounds • Start with the POSITIVE • Write the symbol for the cation first (on left), followed by the anion (on right). Ex: NaCl • Make the charges balance with subscripts. • Make the net ionic charge equal zero by adding subscripts as needed to each ion. Ex: CaBr2 • Keep your polyatomics together. • Treat a polyatomic ion as a package deal, put parentheses around it before doing subscripts if needed. Ex: Ba(NO2)2 / Ba=+2 & NO2= -1

  6. Formula writing for Ionic Compounds TRY IT! • Potassium bromide = _______________ • Calcium chloride = _________________ • Iron (III) oxide = ____________________ • Barium chlorate = __________________ • Magnesium phosphate = _____________

  7. Naming Ionic Compounds • Start with the POSITIVE • Write the cation exactly as it appears on the oxidation list. • Don’t forget Roman numerals! Some math may be needed to determine the charge. ex: Fe(OH)2 • Negative comes last. • Monoatomics change the ending to –ide. ex: oxide, fluoride • Many polyatomics end in –ite or –ate. • ates have 1 more oxygen that ites do. ex: nitrite/nitrate • Balancing subscripts do NOT affect the name.

  8. Naming Ionic Compounds TRY IT! • Li2S = ___________________________ • AlBr3 = ___________________________ • KMnO4 = _________________________ • NH4OH = _________________________ • CuO = ___________________________

  9. Homework: start now! • WB pg 21: Do all multiples of 5 (5, 10, 15…), both columns • Check answers at front if finished during class. • E28 test is tomorrow! Study! • Check your p.18 practice test answers at the front • Check answers on blog at home(MHSchemistry.wordpress.com) • Extra time? Read E29 p22

  10. Check p21 answers 5) Li2S 5) Potassium sulfide 10) Ag2O 10) Lead (II) iodide 15) FeCl3 15) Iron (II) bromide 20) Al2(SO4)3 20) Strontium sulfite 25) Hg3(PO4)2 25) Copper (II) phosphate 30) NaMnO4 30) Tin (II) chromate

  11. E29 Day 2: Hydrated Ionic compounds • Remember that hydrates are ions which tend to have a certain amount of WATER attached to their crystalline structure. • Written _____ • H2O Example: CuSO4• 5 H2O Each CuSO4 molecule bonds to 5 water molecules.

  12. NamingHydrated Ionic compounds • Name the first part just like we did yesterday, leaving a space afterward. • Example: CuSO4 • 5 H2O SO4 is -2, so it must be: Copper (II) sulfate • Look at the coefficient for the water- write THE GREEK PREFIX to match that number, followed by the word “hydrate.” That’s it! • CuSO4 • 5 H2O = Copper (II) sulfate pentahydrate GREEK PREFIXES: 1= mono 2= di 3= tri 4= tetra 5= penta 6= hexa 7= hepta 8= octa 9= nona 10= deca

  13. NamingHydrated Ionic compounds TRY IT! • Fe(NO3)3 • 9 H2O = _______________________________ 2. BaCl2• 2 H2O = _______________________________ • Magnesium sulfate heptahydrate = __________________ GREEK PREFIXES: 1= mono 2= di 3= tri 4= tetra 5= penta 6= hexa 7= hepta 8= octa 9= nona 10= deca

  14. HOMEWORK • WB page 22 all ODD practice problems (under Hydrated Ionic Compounds) • ANSWERS: • Copper chloride dihydrate 1) CaCl2 • 2H2O 3) Iron (III) chloride trihydrate 3) BaI2 • H2O 5) Nickel (II) chloride hexahydrate 5) FeCl3• 4H2O

  15. Naming Acids • All acid formulas start with hydrogen (H). ex: HCl • There are 2 types of acids: binary acids & oxyacids. • BINARY acids: • Have just hydrogen & a monoatomic anion (2 elements total) • Are usually aqueous (aq) = dissolved in water. NAMES:ex: HCl • Start with “hydro”hydro • Write the ROOT for the anion hydrochlor • Add suffix “-ic”hydrochloric • Leave a space, then write “acid” hydrochloric acid

  16. Hydro- • root • -ic • acid Naming Binary Acids TRY IT! • H2S = __________________________________ • HI = ___________________________________ • H3P = __________________________________

  17. Naming Oxyacids • Oxyacids contain hydrogen and a polyatomic ion containing oxygen. Ex: H2SO4 • When naming oxyacids, follow these steps: • Determine the name of the anion. • Write the root word for the anion. • If the anion’s name ends with “–ate” change to the suffix “ic”. If the anion’s name ends with “–ite” change to the suffix “ous” • Leave a space, then write the word “acid”

  18. Naming Oxyacids: • Example 1: H2SO4 = sulfuric acid (ate ic) • but H2SO3 = sulfurous acid (ite ous) • Example 2: HNO3 = ________________________ • but HNO2 = ________________________ But wait, there’s more! ….

  19. Naming Oxyacids: There is a pattern to the prefixes and suffixes of oxyanions! AnionCorresponding Acid ClO41- = perchlorate HClO4 = perchloric acid ClO31- = chlorate HClO3 = chloric acid ClO21- = chlorite HClO2 = chlorous acid ClO1- = hypochlorite HClO = hypochlorous acid Cl1- = chloride HCl1- = hydrochloric acid • When writing the formulas for acids, follow the same rules for writing the formulas of ionic compounds! • * Hint: Find the “ate” anion FIRST (ex. NO31-, ClO31-, C2H3O21-…) • **Remember to balance charges!!!

  20. Naming Oxyacids Per___ic acid ate _____ ic acid ite _____ ous acid Hypo ____ ous acid No O Hydro____ic acid = a binary acid TRY IT! The ion MnO4 = HMnO4 = HMnO3 = HMnO2 = HMnO = HMn=

  21. Binary Molecular Compounds • These have two nonmetals. ex: CO2These aren’t really ions, so they have different rules. • Names tell number of each element, using Greek prefixes to describe subscripts. • Write prefix matching the subscript of 1st nonmetal (if just 1, mono is usually left out), followed by full name of the 1st element. • Write prefix matching the subscript the 2nd element mono IS usually written for the 2nd if there’s 1, followed by ROOTfor the name of 2nd element. • Add suffix “ide”. ex: CO2 = carbon dioxide GREEK PREFIXES: 1= mono 2= di 3= tri 4= tetra 5= penta 6= hexa 7= hepta 8= octa 9= nona 10= deca

  22. Binary Molecular Compounds TRY IT! • CO = ___________________________ • SO3 = __________________________ • N2O4 = __________________________ • Nitrogen trihydride= _______________ • Diphosphorous hexoxide = ____________ GREEK PREFIXES: 1= mono 2= di 3= tri 4= tetra 5= penta 6= hexa 7= hepta 8= octa 9= nona 10= deca

  23. HOMEWORK for Monday • WBpg 23 ALL odd practice problems (acids) • WB pg 24 #1 & 10 both columns • MEET IN COMPUTER LAB B325 MON & TUES!

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