Chemistry 102 Section 6.4 Ionic Compounds

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

• Unit II Note pack, pages 9-13

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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)

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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

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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.

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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

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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.

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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

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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.

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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.
• Al3 S-2 ? Al2S3
  Aluminum sulfide

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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.
• Al3 S-2 ? Al2S3
  Aluminum sulfide
• Write the formula for the binary ionic compound
  between iron (III) and oxygen, and NAME IT.

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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.
• Al3 S-2 ? Al2S3
  Aluminum sulfide
• Write the formula for the binary ionic compound
  between iron (III) and oxygen, and NAME IT.
• Fe3 O-2 ? Fe2O3
  Iron (III) oxide

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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.
• Al3 S-2 ? Al2S3
  Aluminum sulfide
• Write the formula for the binary ionic compound
  between iron (III) and oxygen, and NAME IT.
• Fe3 O-2 ? Fe2O3
  Iron (III) oxide
• Write the formula for the binary ionic compound
  between calcium and sulfur, and NAME IT.

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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.
• Al3 S-2 ? Al2S3
  Aluminum sulfide
• Write the formula for the binary ionic compound
  between iron (III) and oxygen, and NAME IT.
• Fe3 O-2 ? Fe2O3
  Iron (III) oxide
• Write the formula for the binary ionic compound
  between calcium and sulfur, and NAME IT.
• Ca2 S-2 ? CaS
  Calcium sulfide

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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.

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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-)

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Polyatomic Ions

• For D, see Chart 6.4
• Example
• Ammonium NH4

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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

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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
• Al3 CO3-2 ?
• E. Write the formula for ammonium sulfate
• F. Write the formula for calcium phosphate

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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
• Al3 CO3-2 ? Al2(CO3)3
• E. Write the formula for ammonium sulfate
• F. Write the formula for calcium phosphate

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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
• Al3 CO3-2 ? Al2(CO3)3
• E. Write the formula for ammonium sulfate
• NH4 SO4-2 ?
• F. Write the formula for calcium phosphate

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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
• Al3 CO3-2 ? Al2(CO3)3
• E. Write the formula for ammonium sulfate
• NH4 SO4-2 ? (NH4)2SO4
• F. Write the formula for calcium phosphate

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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
• Al3 CO3-2 ? Al2(CO3)3
• E. Write the formula for ammonium sulfate
• NH4 SO4-2 ? (NH4)2SO4
• F. Write the formula for calcium phosphate
• Ca2 PO4-3 ?

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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
• Al3 CO3-2 ? Al2(CO3)3
• E. Write the formula for ammonium sulfate
• NH4 SO4-2 ? (NH4)2SO4
• F. Write the formula for calcium phosphate
• Ca2 PO4-3 ? Ca3(PO4)2

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Ternary Ionic Compounds

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

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Ternary Ionic Compounds

• Do this one on your own, and compare with a
  partner.
• Write the formula for beryllium carbonate.
• Be2 CO3-2 ? BeCO3
• Beryllium ion carbonate ? beryllium carbonate

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Practice Problems, pg. 11

• Write the formulas for compounds formed AND name
  the compound from these pairs of ions
• NH41, SO32-
• Calcium ion, phosphate ion

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Practice Problems, pg. 11

• Write the formulas for compounds formed AND name
  the compound from these pairs of ions
• NH41, SO32-
• (NH4)2SO3 Ammonium Sulfite
• Calcium ion, phosphate ion

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Practice Problems, pg. 11

• Write the formulas for compounds formed AND name
  the compound from these pairs of ions
• NH41, SO32-
• (NH4)2SO3 Ammonium Sulfite
• Calcium ion, phosphate ion
• Ca2 PO4-3 ? Ca3(PO4)2
• Calcium phosphate

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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

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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

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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

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Practice Problems, pg. 11

• Write formulas for these compounds
• Lithium hydrogen sulfate __________
• Chromium (III) nitrite ______________
• Mercury (II) bromide ______________
• Ammonium dichromate ___________

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Practice Problems, pg. 11

• Write formulas for these compounds
• Lithium hydrogen sulfate _LiHSO4__
• Chromium (III) nitrite _____________
• Mercury (II) bromide ______________
• Ammonium dichromate ___________

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Practice Problems, pg. 11

• Write formulas for these compounds
• Lithium hydrogen sulfate _LiHSO4___
• Chromium (III) nitrite __Cr(NO2)3_____
• Mercury (II) bromide _______________
• Ammonium dichromate ____________

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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_

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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.

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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

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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-

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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 is mono-, it may be dropped.
  However, it must be said if it is for the second
  element.
• Dont reduce the subscripts (like you did for
  binary ionic compounds)

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Name these binary molecular compounds.

1. N2O -- ___________________
2. PCl3 -- ___________________
3. SF6 -- _____________________
4. OF2 -- _____________________
5. Cl2O8 -- ___________________
6. SO3 -- ____________________

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Name these binary molecular compounds.

1. N2O -- _dinitrogen monoxide__
2. PCl3 -- ______________________
3. SF6 -- ________________________
4. OF2 -- _______________________
5. Cl2O8 -- _____________________
6. SO3 -- ______________________

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Name these binary molecular compounds.

1. N2O -- _dinitrogen monoxide__
2. PCl3 -- _phosphorus trichloride_
3. SF6 -- ______________________
4. OF2 -- _____________________
5. Cl2O8 -- ____________________
6. SO3 -- ____________________

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Name these binary molecular compounds.

1. N2O -- _dinitrogen monoxide__
2. PCl3 -- _phosphorus trichloride_
3. SF6 -- _sulfur hexafluoride___
4. OF2 -- _____________________
5. Cl2O8 -- _____________________
6. SO3 -- ____________________

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Name these binary molecular compounds.

1. N2O -- _dinitrogen monoxide__
2. PCl3 -- _phosphorus trichloride_
3. SF6 -- _sulfur hexafluoride___
4. OF2 -- _oxygen difluoride___
5. Cl2O8 -- _dichlorine octoxide__
6. SO3 -- _sulfur trioxide___

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Write the formulas for the following binary
molecular compounds.

1. Nitrogen trifluoride ________________
2. Disulfur dichloride ________________
3. Dinitrogen tetraoxide _______________
4. Octoxygen dichloride _______________
5. Trinitrogen pentoxide _______________

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Write the formulas for the following binary
molecular compounds.

1. Nitrogen trifluoride ___NF3__________
2. Disulfur dichloride ________________
3. Dinitrogen tetraoxide ______________
4. Octoxygen dichloride _______________
5. Trinitrogen pentoxide _______________

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Write the formulas for the following binary
molecular compounds.

1. Nitrogen trifluoride ___NF3__________
2. Disulfur dichloride ___S2Cl2________
3. Dinitrogen tetraoxide ______________
4. Octoxygen dichloride ______________
5. Trinitrogen pentoxide ______________

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Write the formulas for the following binary
molecular compounds.

1. Nitrogen trifluoride ___NF3__________
2. Disulfur dichloride ___S2Cl2________
3. Dinitrogen tetraoxide __N2O4________
4. Octoxygen dichloride _______________
5. Trinitrogen pentoxide ______________

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Write the formulas for the following binary
molecular compounds.

1. Nitrogen trifluoride ___NF3__________
2. Disulfur dichloride ___S2Cl2________
3. Dinitrogen tetraoxide __N2O4________
4. Octoxygen dichloride __O8Cl2_______
5. Trinitrogen pentoxide __N3O5_______

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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)

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Naming acids
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Name the following acids

• Begin by finding the name of the anion (not the
  H) from the periodic Table or Table 6.4, then
  follow the naming flow chart.
• HClO ___________________________
  ________________________________
• HClO4 _________________________
  ________________________________

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Name the following acids

• Begin by finding the name of the anion (not the
  H) from the periodic Table or Table 6.4, then
  follow the naming flow chart.
• HClO ClO is hypochlorite _so the name for this
  acid is ______________
• HClO4 _________________________
  _______________________________

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Name the following acids

• Begin by finding the name of the anion (not the
  H) from the periodic Table or Table 6.4, then
  follow the naming flow chart.
• HClO ClO is hypochlorite _so the name for this
  acid is hypochlorous acid
• HClO4 _________________________
  ________________________________

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Name the following acids

• Begin by finding the name of the anion (not the
  H) from the periodic Table or Table 6.4, then
  follow the naming flow chart.
• HClO ClO is hypochlorite _so the name for this
  acid is hypochlorous acid
• HClO4 ClO4 is perchlorate, so the name for this
  acid is______________

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Name the following acids

• Begin by finding the name of the anion (not the
  H) from the periodic Table or Table 6.4, then
  follow the naming flow chart.
• HClO ClO is hypochlorite _so the name for this
  acid is hypochlorous acid
• HClO4 ClO4 is perchlorate, so the name for this
  acid is perchloric acid

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Practice naming the following acids

1. HCl _________________________
2. HClO3 _______________________
3. HClO2 _______________________
4. HClO ________________________
5. HClO4 _______________________
6. H2S ____________________
7. H2SO3 ___________________
8. H2SO4 ___________________
9. HC2H3O2 ____________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 ___________________________
3. HClO2 ___________________________
4. HClO ____________________________
5. HClO4 ___________________________
6. H2S _____________________________
7. H2SO3 ___________________________
8. H2SO4 ___________________________
9. HC2H3O2 _________________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 ____Chloric acid_____________
3. HClO2 ___________________________
4. HClO ____________________________
5. HClO4 ___________________________
6. H2S _____________________________
7. H2SO3 ___________________________
8. H2SO4 ___________________________
9. HC2H3O2 _________________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 ____Chloric acid_____________
3. HClO2 ____Chlorous Acid ___________
4. HClO ____________________________
5. HClO4 ____________________________
6. H2S ______________________________
7. H2SO3 ____________________________
8. H2SO4 ____________________________
9. HC2H3O2 __________________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 ____Chloric acid_____________
3. HClO2 ____Chlorous Acid ___________
4. HClO ____Hypochlorous acid _______
5. HClO4 ___________________________
6. H2S _____________________________
7. H2SO3 ___________________________
8. H2SO4 ___________________________
9. HC2H3O2 _________________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 __Chloric acid_____________
3. HClO2 __Chlorous Acid __________
4. HClO ___Hypochlorous acid _______
5. HClO4 __Perchloric acid __________
6. H2S _____________________________
7. H2SO3 ___________________________
8. H2SO4 ___________________________
9. HC2H3O2 _________________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 ____Chloric acid_____________
3. HClO2 ____Chlorous Acid ___________
4. HClO ____Hypochlorous acid ________
5. HClO4 ___Perchloric acid __________
6. H2S _____Hydrosulfuric acid _________
7. H2SO3 ____________________________
8. H2SO4 ____________________________
9. HC2H3O2 __________________________

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Practice naming the following acids

1. HCl ____Hydrochloric acid__________
2. HClO3 ____Chloric acid_____________
3. HClO2 ____Chlorous Acid ______________
4. HClO ____Hypochlorous acid ________
5. HClO4 ___Perchloric acid __________
6. H2S _____Hydrosulfuric acid _________
7. H2SO3 ___Sulfurous acid __________
8. H2SO4 ____Sulfuric acid_____
9. HC2H3O2 ___Acetic acid_________

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Write the formula for the following acids

1. Nitric acid ______________________
2. Hydronitric acid _________________
3. Nitrous acid ____________________
4. Hydrocyanic acid ________________
5. Phosphoric acid _________________
6. Hydrobromic acid ________________
7. Acetic acid _____________________
8. Nitric acid ______________________

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Write the formula for the following acids

1. Nitric acid _____HNO3_____________
2. Hydronitric acid __________________
3. Nitrous acid _____________________
4. Hydrocyanic acid _________________
5. Phosphoric acid __________________
6. Hydrobromic acid _________________
7. Acetic acid ______________________
8. Nitric acid _______________________

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Write the formula for the following acids

1. Nitric acid _____HNO3______________
2. Hydronitric acid _H3N______________
3. Nitrous acid ______________________
4. Hydrocyanic acid __________________
5. Phosphoric acid ___________________
6. Hydrobromic acid __________________
7. Acetic acid _______________________
8. Nitric acid ________________________

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Write the formula for the following acids

1. Nitric acid _____HNO3_____________
2. Hydronitric acid _H3N______________
3. Nitrous acid __HNO2_______________
4. Hydrocyanic acid _________________
5. Phosphoric acid ___________________
6. Hydrobromic acid __________________
7. Acetic acid _______________________
8. Nitric acid _______________________

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Write the formula for the following acids

1. Nitric acid _____HNO3______________
2. Hydronitric acid _H3N_______________
3. Nitrous acid __HNO2_______________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid ___________________
6. Hydrobromic acid __________________
7. Acetic acid _______________________
8. Nitric acid ________________________

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Write the formula for the following acids

1. Nitric acid _____HNO3______________
2. Hydronitric acid _H3N_______________
3. Nitrous acid __HNO2________________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________
6. Hydrobromic acid __________________
7. Acetic acid _______________________
8. Nitric acid ________________________

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Write the formula for the following acids

1. Nitric acid _____HNO3______________
2. Hydronitric acid _HN3_______________
3. Nitrous acid __HNO2______________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________
6. Hydrobromic acid _HBr______________
7. Acetic acid _______________________
8. Nitric acid ________________________

72
Write the formula for the following acids

1. Nitric acid _____HNO3______________
2. Hydronitric acid _HN3_______________
3. Nitrous acid __HNO2________________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________
6. Hydrobromic acid _HBr______________
7. Acetic acid __HC2H3O2____________
8. Nitric acid ______________________

73
Write the formula for the following acids

1. Nitric acid _____HNO3______________
2. Hydronitric acid _HN3_______________
3. Nitrous acid __HNO2________________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________
6. Hydrobromic acid _HBr______________
7. Acetic acid __HC2H3O2____________
8. Nitric acid ___HNO3_______________