Ionic compounds containing polyatomic ions

Ionic compounds containing polyatomic ions

Review So far, we’ve been dealing only with binary ionic compounds
Binary compounds form between two elements that ionize, experience an electromagnetic attraction, and form an ionic bond For example: Sodium chloride  NaCl Elements: sodium and chlorine Atoms: 1 sodium and 1 chlorine Copper (II) chloride  CuCl2 Elements: copper (II) and chlorine Atoms: 1 copper (II) and 2 chlorine

Polyatomic ions What is a polyatomic ion?

Polyatomic ions What is a polyatomic ion? “poly” means many

Polyatomic ions What is a polyatomic ion? “poly” means many
“atomic” means atom

“atomic” means atom “polyatomic” means many atoms

“atomic” means atom “polyatomic” means many atoms “Polyatomic ion” means a many atom ion

Polyatomic ions What is a polyatomic ion?
“poly” means many “atomic” means atom “polyatomic” means many atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds

“poly” means many/several “atomic” means atom “polyatomic” means several atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds

“poly” means many/several “atomic” means atom “polyatomic” means several atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds, with an uneven number of electrons and protons, creating a net charge

“poly” means many/several “atomic” means atom “polyatomic” means several atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds, with an uneven number of electrons and protons, creating a net charge Polyatomic ions act just like other ions

“poly” means many/several “atomic” means atom “polyatomic” means several atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds, with an uneven number of electrons and protons, creating a net charge Polyatomic ions act just like other ions Will form bonds with other ions of the opposite charge

“poly” means many/several “atomic” means atom “polyatomic” means several atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds, with an uneven number of electrons and protons, creating a net charge Polyatomic ions act just like other ions Will form bonds with other ions of the opposite charge Ionic compounds with polyatomic ions are neutral, just like binary compounds

“poly” means many/several “atomic” means atom “polyatomic” means several atoms “Polyatomic ion” means a many atom ion Polyatomic ions are composed of two or more atoms bonded together by covalent bonds, with an uneven number of electrons and protons, creating a net charge Polyatomic ions act just like other ions Will form bonds with other ions of the opposite charge Ionic compounds with polyatomic ions are neutral, just like binary compounds For our purposes, polyatomic ions will never split apart so they can be treated as a single object

For example: Nitrate

For example: Nitrate NO3-

For example: Nitrate NO3-
One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen The nitrogen and the three oxygens are sharing electrons but they also need to accept 1 extra electron in order to fill their valence shells, hence the charge of -1

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen The nitrogen and the three oxygens are sharing electrons but they also need to accept 1 extra electron in order to fill their valence shells, hence the charge of -1 Nitrate can form an ionic compound with a cation, just like any other anion. For example:

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen The nitrogen and the three oxygens are sharing electrons but they also need to accept 1 extra electron in order to fill their valence shells, hence the charge of -1 Nitrate can form an ionic compound with a cation, just like any other anion. For example: Sodium nitrate

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen The nitrogen and the three oxygens are sharing electrons but they also need to accept 1 extra electron in order to fill their valence shells, hence the charge of -1 Nitrate can form an ionic compound with a cation, just like any other anion. For example: Sodium nitrate  Na+ NO3-

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen The nitrogen and the three oxygens are sharing electrons but they also need to accept 1 extra electron in order to fill their valence shells, hence the charge of -1 Nitrate can form an ionic compound with a cation, just like any other anion. For example: Sodium nitrate  Na+ NO3-  NaNO3

One nitrate ion is composed of 1 atom of nitrogen and 3 atoms of oxygen bonded together by covalent bonds Nitrate will always have a 1:3 ratio of nitrogen to oxygen The nitrogen and the three oxygens are sharing electrons but they also need to accept 1 extra electron in order to fill their valence shells, hence the charge of -1 Nitrate can form an ionic compound with a cation, just like any other anion. For example: Sodium nitrate  Na+ NO3-  NaNO3 If sodium nitrate is added to water, the sodium ion will separate from the nitrate ion (like other ionic compounds) but the oxygens and nitrogen in the nitrate ion will remain attached

Polyatomic ions You do not need to memorize the polyatomic ions, these will be provided for you in a chart

Polyatomic ions You do not need to memorize the polyatomic ions, these will be provided for you in a chart As you can see, there are far more polyatomic anions than cations

Polyatomic ions You do not need to memorize the polyatomic ions, these will be provided for you in a chart As you can see, there are far more polyatomic anions than cations Subscripts still refer to the number of atoms while superscripts refer to the overall charge

Rules for naming compounds containing polyatomic ions

Cation must be written first

Cation must be written first Anion must be written second

Cation must be written first Anion must be written second 3a. If the anion is monoatomic, change ending to ‘ide’

Cation must be written first Anion must be written second 3a. If the anion is monoatomic, change ending to ‘ide’ 3b. If the anion is polyatomic, leave the ending as is

Cation must be written first Anion must be written second 3a. If the anion is monoatomic, change ending to ‘ide’ 3b. If the anion is polyatomic, leave the ending as is For example: Magnesium and carbonate Potassium and chromate Ammonium and oxygen

Cation must be written first Anion must be written second 3a. If the anion is monoatomic, change ending to ‘ide’ 3b. If the anion is polyatomic, leave the ending as is For example: Magnesium and carbonate magnesium carbonate Potassium and chromate Ammonium and oxygen

Cation must be written first Anion must be written second 3a. If the anion is monoatomic, change ending to ‘ide’ 3b. If the anion is polyatomic, leave the ending as is For example: Magnesium and carbonate magnesium carbonate Potassium and chromate potassium chromate Ammonium and oxygen

Cation must be written first Anion must be written second 3a. If the anion is monoatomic, change ending to ‘ide’ 3b. If the anion is polyatomic, leave the ending as is For example: Magnesium and carbonate magnesium carbonate Potassium and chromate potassium chromate Ammonium and oxygen ammonium oxide

Rules for writing the formula of compounds containing polyatomic ions

1. The cation must always be written first

1. The cation must always be written first 2. The anion must always be written second

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge.

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets.

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2-

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2- NH4 O

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2- In order to create a neutral compound, we need 2 ammoniums and 1 oxygen NH4 O

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2- In order to create a neutral compound, we need 2 ammoniums and 1 oxygen NH4 2O

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2- In order to create a neutral compound, we need 2 ammoniums and 1 oxygen NH4 2O Without brackets, this means there is one nitrogen, 8 hydrogens, and 1 oxygen. This is not correct!

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2- In order to create a neutral compound, we need 2 ammoniums and 1 oxygen (NH4)2O

1. The cation must always be written first 2. The anion must always be written second 3. Use subscripts to indicate how many of each ion you need to balance out the charge. If you need more than one polyatomic ion, put brackets around the entire ion and the subscript outside the brackets. For example: ammonium oxide NH4+ and O2- In order to create a neutral compound, we need 2 ammoniums and 1 oxygen (NH4)2O The brackets show that the subscript 2 is being applied to the whole polyatomic ion

Practice Cation Anion Compound name Compound formula Potassium: K+
Nitrate: NO3- Scandium phosphate LiCH3COO Ammonium: Chlorine: Magnesium hydroxide Be3(PO4)2 Lanthanum: Permanganate: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium phosphate LiCH3COO Ammonium: Chlorine: Magnesium hydroxide Be3(PO4)2 Lanthanum: Permanganate: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 LiCH3COO Ammonium: Chlorine: Magnesium hydroxide Be3(PO4)2 Lanthanum: Permanganate: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: Chlorine: Magnesium hydroxide Be3(PO4)2 Lanthanum: Permanganate: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: NH4+ Chlorine: Cl- Ammonium chloride NH4Cl Magnesium hydroxide Be3(PO4)2 Lanthanum: Permanganate: Ammonium: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: NH4+ Chlorine: Cl- Ammonium chloride NH4Cl Magnesium: Mg2+ Hydroxide: OH- Magnesium hydroxide Mg(OH)2 Be3(PO4)2 Lanthanum: Permanganate: Ammonium: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: NH4+ Chlorine: Cl- Ammonium chloride NH4Cl Magnesium: Mg2+ Hydroxide: OH- Magnesium hydroxide Mg(OH)2 Beryllium: Be2+ Beryllium phosphate Be3(PO4)2 Lanthanum: Permanganate: Ammonium: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: NH4+ Chlorine: Cl- Ammonium chloride NH4Cl Magnesium: Mg2+ Hydroxide: OH- Magnesium hydroxide Mg(OH)2 Beryllium: Be2+ Beryllium phosphate Be3(PO4)2 Lanthanum: La3+ Permanganate: MnO4- Lanthanum permanganate La(MnO4)3 Ammonium: Sulfite: Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: NH4+ Chlorine: Cl- Ammonium chloride NH4Cl Magnesium: Mg2+ Hydroxide: OH- Magnesium hydroxide Mg(OH)2 Beryllium: Be2+ Beryllium phosphate Be3(PO4)2 Lanthanum: La3+ Permanganate: MnO4- Lanthanum permanganate La(MnO4)3 Sulfite: SO32- Ammonium sulfite (NH4)2SO3 Mo2(CO3)3

Nitrate: NO3- Potassium nitrate KNO3 Scandium: Sc3+ Phosphate: PO43- Scandium phosphate ScPO4 Lithium: Li+ Acetate: CH3COO Lithium acetate LiCH3COO Ammonium: NH4+ Chlorine: Cl- Ammonium chloride NH4Cl Magnesium: Mg2+ Hydroxide: OH- Magnesium hydroxide Mg(OH)2 Beryllium: Be2+ Beryllium phosphate Be3(PO4)2 Lanthanum: La3+ Permanganate: MnO4- Lanthanum permanganate La(MnO4)3 Sulfite: SO32- Ammonium sulfite (NH4)2SO3 Molybdenum (III): Mo3+ Carbonate: CO32- Molybdenum (III) carbonate Mo2(CO3)3

Ionic compounds containing polyatomic ions

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