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Chapter 9

Chapter 9. Chemical Names and Formulas. Section 1. Naming Ions. Section 1 Learning Targets. 9.1.1 – I can identify the charges of monatomic ions by using the periodic table, and name the ions.

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Chapter 9

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  1. Chapter 9 Chemical Names and Formulas

  2. Section 1 Naming Ions

  3. Section 1 Learning Targets 9.1.1 – I can identify the charges of monatomic ions by using the periodic table, and name the ions. 9.1.2 – I can define a polyatomic ion and write the names and formulas of the most common polyatomic ions. 9.1.3 – I can identify the two common endings for the names of most polyatomic ions.

  4. Monatomic Ions • Monatomic ion – consist of a single atom with a positive or negative charge resulting from the gain or loss of one or more valence electrons.

  5. Cations • When the metals in Groups 1A, 2A and 3A lose electrons they form cations with positive charges equal to the group number. • The names of these ions are the same as the element name with ion after it.

  6. Anions • Nonmetals of Groups 5A, 6A, and 7A gain electrons to form anions with negative charges. • The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.

  7. Group 7A so 7-8=-1; 6A so 6-8=-2; 5A so 5-8=-3 • The names of these ions change. The endings are dropped and replaced by –ide ion (sulfur = sulfide ion). • Groups 4A and 8A elements do not usually form ions.

  8. Examples: • Name the ions formed by these elements and classify them as anions or cations: • Selenium ____________________ • Barium ____________________ • Phosphorus ____________________

  9. Examples: • Name the following ions: • I- ____________________ • N3- ____________________ • O2- ____________________

  10. This table can be found on page 254

  11. Ions of Transition Metals • The charges of the cations of many transition metal ions must be determined from the number of electrons lost.

  12. Two methods – classical (-ous and –ic endings) or the stock system (roman numerals). • Preferred is the stock system because the roman numeral tells the charge. So why do we use Roman numerals or the classical method anyway?

  13. This table can be found on page 255

  14. Examples: • Name the following ions: • Fe3+ ____________________ • Cu+ ____________________ • Mn4+ ____________________ • Sn2+ ____________________ • Pb4+ ____________________

  15. Polyatomic Ions • Polyatomic ion – composed of more than one atom. • The names of most polyatomic anions end in –ate or –ite. • There are very few positive polyatomic ions.

  16. Examples: • Write the symbol or formula (including charge) for each of the following ions: • Ammonium ion ____________________ • Chromate ion ____________________ • Tin (II) ion ____________________ • Nitrate ion ____________________

  17. Examples: • Name the following ions: • OH- ____________________ • Pb4+ ____________________ • SO42- ____________________ • O2- ____________________

  18. Section 2 Naming and Writing Formulas for Ionic Compounds

  19. Section 2 Learning Targets 9.2.1 – I can apply the rules for naming and writing formulas for binary ionic compounds. 9.2.2 – I can apply the rules for naming and writing formulas for compounds with polyatomic ions.

  20. Binary Ionic Compounds • In the past anyone who created a compound named it. • Currently there is a system. • Antione Lavoisier decided it was too difficult to memorize unrelated names and formulas.

  21. Naming Binary Ionic Compounds • Binary compound – compound of two elements and can be either ionic or molecular. • To name binary ionic compounds, place the name of the cation first followed by the anion name.

  22. Examples: • Write the names of the following binary ionic compounds: • NaCl ____________________ • MgBr2 ____________________ • SrO ____________________ • Li2O ____________________ • Be3N2 ____________________

  23. For transition metals you need to figure the charge of the metal and put that in parentheses as a Roman numeral.

  24. Examples: • Write the names of the following binary ionic compounds: • SnO2 ____________________ • Fe2O3 ____________________ • MnO ____________________ • MnO2 ____________________ • Co3N2 ____________________

  25. Writing Formulas for Binary Ionic Compounds • Write the symbol of the cation and then the anion. • Add what ever subscripts are needed to balance the charges.

  26. Examples: • Write the formulas for the compounds formed from these pairs of ions: • Ba2+, S2- ____________________ • Ca2+, N3- ____________________ • Li+, O2- ____________________ • Cu2+, I- ____________________

  27. Examples: • Write the formulas for these compounds: • Sodium iodide ____________________ • Potassium sulfide ____________________ • Calcium iodide ____________________

  28. For transition metals the Roman numeral tells the charge on the metal cation. • Then the same as before, balance the charges.

  29. Examples: • Write the formulas for the following compounds: • Tin (IV) nitride ____________________ • Copper (I) oxide ____________________ • Copper (II) oxide ____________________ • Lead (II) sulfide ____________________ • Iron (III) oxide ____________________

  30. Compounds with Polyatomic Ions • Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges. • HINT: if you need more than one polyatomic ion – use parenthesis.

  31. Examples: • Write the formula for the following compounds: • Ammonium nitride ____________________ • Ammonium cyanide ___________________ • Calcium carbonate ____________________ • Tin (IV) sulfite ____________________ • Magnesium phosphate __________________

  32. Naming Compounds with Polyatomic Ions • To name a compound containing a polyatomic ion, state the cation first and then the anion, just as you did for binary ionic compounds.

  33. Examples: • Name the following compounds: • Sn2(CO3)4 ____________________ • Mg(CN)2 ____________________ • Fe(NO3)3 ____________________ • (NH4)3PO4 ____________________ • CuSO4 ____________________

  34. Section 3 Naming and Writing Formulas for Molecular Compounds

  35. Section 3 Learning Targets 9.3.1 – I can interpret the prefixes in the names of molecular compounds in terms of their chemical formulas. 9.3.2 – I can apply the rules for naming and writing formulas for binary molecular compounds.

  36. Naming Binary Molecular Compounds • Remember binary means 2. • Molecular compounds have covalent bonds – not ionic like previous sections.

  37. A prefix in the name of a binary molecular compound tells you how many atoms of each element are present in each molecule of the compound. • Ending is still –ide so make sure you’re telling the difference between molecular and ionic.

  38. Examples: • Write the name for the following binary molecular compounds: • NCl3 ____________________ • SO3 ____________________ • NI3 ____________________ • N2O3 ____________________ • N2H4 ____________________

  39. Writing Formulas for Binary Molecular Compounds • Use the prefixes in the name to tell you the subscripts of each element in the formula. • Then write the correct symbols for the two elements with the appropriate subscripts.

  40. Examples: • Write the formulas for the following binary molecular compounds: • Phosphorus pentachloride __________________ • Iodine heptafluoride ____________________ • Chlorine trifluoride ____________________ • Iodine dioxide ____________________ • Diphosphorus trioxide ____________________

  41. Section 4 Naming and Writing Formulas for Acids and Bases

  42. Section 4 Learning Targets 9.4.1 – I can apply three rules for naming acids. 9.4.2 – I can apply the rules in reverse to write the formulas for acids. 9.4.3 – I can apply the rules for naming bases.

  43. Naming Acids • Acid – a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water.

  44. Rules for Naming Acids • When the name of the anion (X) ends in –ide, the acid name begins with the prefix hydro-. The stem of the anion has the suffix –icand is followed by the word acid. • HCl(aq) (X = chloride) is named hydrochloric acid. • H2S(aq) (X = sulfide) is named hydrosulfuric acid.

  45. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid. • H2SO3(aq) (X = sulfite) is named sulfurous acid.

  46. When the anion name ends in –ate, the acid name is the stem of the anion with the suffix –ic followed by the word acid. • HNO3(aq) (X = nitrate) is named nitric acid.

  47. Examples: • Write the names for the following acids: • HNO2 ____________________ • HCN ____________________ • HMnO4 ____________________ • H2S ____________________ • HClO4 ____________________

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