1 / 73

Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids

Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids. Unit II Note pack, pages 9-13. Ionic Compounds. Writing Formulas for Binary Ionic Compounds 1. What are Binary Ionic Compounds? Binary compounds have just 2 elements.

curran-anderson
Download Presentation

Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry 102Section 6.4 Ionic Compounds& Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13

  2. Ionic Compounds • Writing Formulas for Binary Ionic Compounds 1. What are Binary Ionic Compounds? Binary compounds have just 2 elements. Binary ionic compounds have 2 elements that are from opposite sides of the table, a cation and an anion. (metal) (nonmetal)

  3. Ionic Compounds • Writing Formulas for Binary Ionic Compounds 2. What are the “rules” for writing Binary Ionic Compounds? • Write the metal (positive) ion first • Write the nonmetal (negative) ion last • The net charge for the compound must add up to zero (total positive + total negative = 0) • Use subscripts to indicate how many of each ion you need to “balance” the charge. • CrissCross Method

  4. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.

  5. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT. Mg +2 + Cl- MgCl2 Magnesium Chloride

  6. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT. Mg +2 + Cl- MgCl2 Magnesium Chloride Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT.

  7. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT. Mg +2 + Cl- MgCl2 Magnesium Chloride Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT. Na+ + O-2  Na2O Sodium Oxide

  8. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds (pg. 10) Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.

  9. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds (pg. 10) Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT. Al+3 + S-2 Al2S3 Aluminum sulfide

  10. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds (pg. 10) Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT. Al+3 + S-2 Al2S3 Aluminum sulfide Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.

  11. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds (pg. 10) Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT. Al+3 + S-2 Al2S3 Aluminum sulfide Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT. Fe+3 + O-2 Fe2O3 Iron (III) oxide

  12. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds (pg. 10) Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT. Al+3 + S-2 Al2S3 Aluminum sulfide Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT. Fe+3 + O-2 Fe2O3 Iron (III) oxide Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.

  13. Ionic Compounds • Practice Writing Formulas for Binary Ionic Compounds (pg. 10) Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT. Al+3 + S-2 Al2S3 Aluminum sulfide Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT. Fe+3 + O-2 Fe2O3 Iron (III) oxide Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT. Ca+2 + S-2 CaS Calcium sulfide

  14. Polyatomic Ions (pg 10) • What is a polyatomic ion? a tightly bound group of atoms that behaves as a unit and carries a charge B. What endings to polyatomic ions receive when naming them? most polyatomic ions receive endings of either –ite or –ate.

  15. Polyatomic ions C. There are 3 important exceptions (to the end of their names), they are: Ammonium cation (NH4+) Two polyatomic ions end in –ide; cyanide (CN-) and hydroxide (OH-)

  16. Polyatomic Ions • For “D”, see Chart 6.4 • Example: • Ammonium NH4+

  17. Ternary Ionic Compounds • Define ternary ionic compounds: A compound that contains atoms of three, or more, different elements Remember, they are still just two ions, and all rules from before still apply. • Write the formula for lithium nitrate, a ternary compound. Li + + NO3- LiNO3

  18. Ternary Ionic Compounds C.Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis. D. Write the formula for aluminum carbonate: Al+3 + CO3-2 E. Write the formula for ammonium sulfate: F. Write the formula for calcium phosphate:

  19. Ternary Ionic Compounds C.Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis. D. Write the formula for aluminum carbonate: Al+3 + CO3-2Al2(CO3)3 E. Write the formula for ammonium sulfate: F. Write the formula for calcium phosphate:

  20. Ternary Ionic Compounds C.Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis. D. Write the formula for aluminum carbonate: Al+3 + CO3-2Al2(CO3)3 E. Write the formula for ammonium sulfate: NH4+ + SO4-2 F. Write the formula for calcium phosphate:

  21. Ternary Ionic Compounds C.Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis. D. Write the formula for aluminum carbonate: Al+3 + CO3-2Al2(CO3)3 E. Write the formula for ammonium sulfate: NH4+ + SO4-2(NH4)2SO4 F. Write the formula for calcium phosphate:

  22. Ternary Ionic Compounds C.Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis. D. Write the formula for aluminum carbonate: Al+3 + CO3-2Al2(CO3)3 E. Write the formula for ammonium sulfate: NH4+ + SO4-2(NH4)2SO4 F. Write the formula for calcium phosphate: Ca+2 + PO4-3

  23. Ternary Ionic Compounds C.Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis. D. Write the formula for aluminum carbonate: Al+3 + CO3-2Al2(CO3)3 E. Write the formula for ammonium sulfate: NH4+ + SO4-2(NH4)2SO4 F. Write the formula for calcium phosphate: Ca+2 + PO4-3Ca3(PO4)2

  24. Ternary Ionic Compounds • Do this one on your own, and compare with a partner. Write the formula for beryllium carbonate.

  25. Ternary Ionic Compounds • Do this one on your own, and compare with a partner. Write the formula for beryllium carbonate. Be+2 + CO3-2 BeCO3 Beryllium ion + carbonate  beryllium carbonate

  26. Practice Problems, pg. 11 • Write the formulas for compounds formed AND name the compound from these pairs of ions: • NH4+1, SO32- • Calcium ion, phosphate ion

  27. Practice Problems, pg. 11 • Write the formulas for compounds formed AND name the compound from these pairs of ions: • NH4+1, SO32- (NH4)2SO3 Ammonium Sulfite • Calcium ion, phosphate ion

  28. Practice Problems, pg. 11 • Write the formulas for compounds formed AND name the compound from these pairs of ions: • NH4+1, SO32- (NH4)2SO3 Ammonium Sulfite • Calcium ion, phosphate ion Ca+2 + PO4-3 Ca3(PO4)2 Calcium phosphate

  29. Practice Problems, pg. 11 • Write the formulas for compounds formed AND name the compound from these pairs of ions: • Al3+, NO3-1 d. Potassium ion, chromate ion

  30. Practice Problems, pg. 11 • Write the formulas for compounds formed AND name the compound from these pairs of ions: • Al3+, NO3-1 Al(NO3)3 Aluminum Nitrate d. Potassium ion, chromate ion

  31. Practice Problems, pg. 11 • Write the formulas for compounds formed AND name the compound from these pairs of ions: • Al3+, NO3-1 Al(NO3)3 Aluminum Nitrate d. Potassium ion, chromate ion K+ + CrO4-2 K2CrO4 Potassium chromate

  32. Practice Problems, pg. 11 • Write formulas for these compounds • Lithium hydrogen sulfate __________ • Chromium (III) nitrite ______________ • Mercury (II) bromide ______________ • Ammonium dichromate ___________

  33. Practice Problems, pg. 11 • Write formulas for these compounds • Lithium hydrogen sulfate _LiHSO4__ • Chromium (III) nitrite _____________ • Mercury (II) bromide ______________ • Ammonium dichromate ___________

  34. Practice Problems, pg. 11 • Write formulas for these compounds • Lithium hydrogen sulfate _LiHSO4___ • Chromium (III) nitrite __Cr(NO2)3_____ • Mercury (II) bromide _______________ • Ammonium dichromate ____________

  35. Practice Problems, pg. 11 • Write formulas for these compounds • Lithium hydrogen sulfate _LiHSO4__ • Chromium (III) nitrite __Cr(NO2)3__ • Mercury (II) bromide __HgBr2___ • Ammonium dichromate _(NH4)2Cr2O7_

  36. Section 6.5 Molecular Compounds and Acids (pg. 12) • Binary Molecular Compounds • What is a binary molecular compound? A compound composed of 2 nonmetallic elements.

  37. Section 6.5 Molecular Compounds and Acids • Binary Molecular Compounds • We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following: Number Prefix Number Prefix • 6 • 7 • 8 • 9 • 10

  38. Section 6.5 Molecular Compounds and Acids • Binary Molecular Compounds • We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following: Number Prefix Number Prefix • mono- 6 hexa- • di- 7 hepta- • tri- 8 octa- • tetra- 9 nona- • penta- 10 deca-

  39. Section 6.5 Molecular Compounds and Acids • Binary Molecular Compounds How do we name binary molecular compounds? • Say the name of the first element, say the name of the second element, ending in ‘-ide’, and put the appropriate prefix in to indicate how many of each element there are in the formula: • If the prefix for the first element in a binary molecular compound ismono-, it may be dropped. However, it must be said if it is for the second element. • Don’t reduce the subscripts (like you did for binary ionic compounds)

  40. Name these binary molecular compounds. • N2O -- ___________________ • PCl3 -- ___________________ • SF6 -- _____________________ • OF2 -- _____________________ • Cl2O8 -- ___________________ • SO3 -- ____________________

  41. Name these binary molecular compounds. • N2O -- _dinitrogen monoxide__ • PCl3 -- ______________________ • SF6 -- ________________________ • OF2 -- _______________________ • Cl2O8 -- _____________________ • SO3 -- ______________________

  42. Name these binary molecular compounds. • N2O -- _dinitrogen monoxide__ • PCl3 -- _phosphorus trichloride_ • SF6 -- ______________________ • OF2 -- _____________________ • Cl2O8 -- ____________________ • SO3 -- ____________________

  43. Name these binary molecular compounds. • N2O -- _dinitrogen monoxide__ • PCl3 -- _phosphorus trichloride_ • SF6 -- _sulfur hexafluoride___ • OF2 -- _____________________ • Cl2O8 -- _____________________ • SO3 -- ____________________

  44. Name these binary molecular compounds. • N2O -- _dinitrogen monoxide__ • PCl3 -- _phosphorus trichloride_ • SF6 -- _sulfur hexafluoride___ • OF2 -- _oxygen difluoride___ • Cl2O8 -- _dichlorine octoxide__ • SO3 -- _sulfur trioxide___

  45. Write the formulas for the following binary molecular compounds. • Nitrogen trifluoride ________________ • Disulfur dichloride ________________ • Dinitrogen tetraoxide _______________ • Octoxygen dichloride _______________ • Trinitrogen pentoxide _______________

  46. Write the formulas for the following binary molecular compounds. • Nitrogen trifluoride ___NF3__________ • Disulfur dichloride ________________ • Dinitrogen tetraoxide ______________ • Octoxygen dichloride _______________ • Trinitrogen pentoxide _______________

  47. Write the formulas for the following binary molecular compounds. • Nitrogen trifluoride ___NF3__________ • Disulfur dichloride ___S2Cl2________ • Dinitrogen tetraoxide ______________ • Octoxygen dichloride ______________ • Trinitrogen pentoxide ______________

  48. Write the formulas for the following binary molecular compounds. • Nitrogen trifluoride ___NF3__________ • Disulfur dichloride ___S2Cl2________ • Dinitrogen tetraoxide __N2O4________ • Octoxygen dichloride _______________ • Trinitrogen pentoxide ______________

  49. Write the formulas for the following binary molecular compounds. • Nitrogen trifluoride ___NF3__________ • Disulfur dichloride ___S2Cl2________ • Dinitrogen tetraoxide __N2O4________ • Octoxygen dichloride __O8Cl2_______ • Trinitrogen pentoxide __N3O5_______

  50. Naming Acids (pg. 12, bottom) • What are acids? Acids are compounds that produce H ions (H+) when dissolved in water B. Write the chart that explains how to name acids: (next)

More Related