### Understanding Polyatomic Ions and Oxidation States Sometimes groups of elements, called metals/nonmetals, can combine and act like a single element, with a single oxidation state. You can find these in Table __ and the positive or negative __ is where you find the __ state. For example, OH⁻ is a polyatomic ion known as hydroxide with an oxidation state of -1. A common base is NaOH which we name as sodium hydroxide. Notice that the ending of a polyatomic ion changes! So PO₄³⁻ is __ and Na₃PO₄ is __. #### Chemical Name and Oxidation States Below is a table listing several compounds, with spaces for filling in the oxidation state, subscript, and total charge of each compound: | No. | Chemical Name | (Ox. State)(subscript) | Total Charge | |-----|---------------|-----------------------|--------------| | 10 | K₃PO₄ | | | | 11 | LiOH | | | | 12 | MgSO₄ | | | | 13 | NaClO | | | | 14 | KClO | | | | 15 | Na₂CO₃ | | | | 16 | Li₃PO₄ | | | | 17 | NaNO₂ | | | | 18 | Ca(NO₃)₂ | | | | 19 | NH₄OH | | | | 20 | Mg(NO₂)₂ | | | | 21 | Na₂SO₄ | | | | 22 | NaSCN | | | | 23 | NaClO₄ | | | | 24 | NaCN | | | | 25 | KCN | | | Students are encouraged to fill in the oxidation states, subscripts, and calculate the total charge for each compound to enhance their understanding of these chemical concepts.
### Understanding Polyatomic Ions and Oxidation States Sometimes groups of elements, called metals/nonmetals, can combine and act like a single element, with a single oxidation state. You can find these in Table __ and the positive or negative __ is where you find the __ state. For example, OH⁻ is a polyatomic ion known as hydroxide with an oxidation state of -1. A common base is NaOH which we name as sodium hydroxide. Notice that the ending of a polyatomic ion changes! So PO₄³⁻ is __ and Na₃PO₄ is __. #### Chemical Name and Oxidation States Below is a table listing several compounds, with spaces for filling in the oxidation state, subscript, and total charge of each compound: | No. | Chemical Name | (Ox. State)(subscript) | Total Charge | |-----|---------------|-----------------------|--------------| | 10 | K₃PO₄ | | | | 11 | LiOH | | | | 12 | MgSO₄ | | | | 13 | NaClO | | | | 14 | KClO | | | | 15 | Na₂CO₃ | | | | 16 | Li₃PO₄ | | | | 17 | NaNO₂ | | | | 18 | Ca(NO₃)₂ | | | | 19 | NH₄OH | | | | 20 | Mg(NO₂)₂ | | | | 21 | Na₂SO₄ | | | | 22 | NaSCN | | | | 23 | NaClO₄ | | | | 24 | NaCN | | | | 25 | KCN | | | Students are encouraged to fill in the oxidation states, subscripts, and calculate the total charge for each compound to enhance their understanding of these chemical concepts.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:### Understanding Polyatomic Ions and Oxidation States
Sometimes groups of elements, called metals/nonmetals, can combine and act like a single element, with a single oxidation state. You can find these in Table __ and the positive or negative __ is where you find the __ state.
For example, OH⁻ is a polyatomic ion known as hydroxide with an oxidation state of -1.
A common base is NaOH which we name as sodium hydroxide.
Notice that the ending of a polyatomic ion changes!
So PO₄³⁻ is __ and Na₃PO₄ is __.
#### Chemical Name and Oxidation States
Below is a table listing several compounds, with spaces for filling in the oxidation state, subscript, and total charge of each compound:
| No. | Chemical Name | (Ox. State)(subscript) | Total Charge |
|-----|---------------|-----------------------|--------------|
| 10 | K₃PO₄ | | |
| 11 | LiOH | | |
| 12 | MgSO₄ | | |
| 13 | NaClO | | |
| 14 | KClO | | |
| 15 | Na₂CO₃ | | |
| 16 | Li₃PO₄ | | |
| 17 | NaNO₂ | | |
| 18 | Ca(NO₃)₂ | | |
| 19 | NH₄OH | | |
| 20 | Mg(NO₂)₂ | | |
| 21 | Na₂SO₄ | | |
| 22 | NaSCN | | |
| 23 | NaClO₄ | | |
| 24 | NaCN | | |
| 25 | KCN | | |
Students are encouraged to fill in the oxidation states, subscripts, and calculate the total charge for each compound to enhance their understanding of these chemical concepts.
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