Use the periodic table to find the two ions (positive ion and negative ion) for each compound. Then write the formula. Remember, the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge. Example: calcium chloride 2+ Ca C (These two charges are not the same, but 2 chloride ions will give an overali negative charge of -2. The positive ion already has a + 2 charge.) Ca²+ Cl₂ Therefore, CaCl₂ is the answer. Name 1) sodium chloride ex. 2) potassium bromide 3) calcium oxide 4) magnesium sulfide Ca²+ CI CI Positive Ion Na+ Count up the total charge. +2, -1, -1 This adds up to zero!! Negative Ion CI Formula NaCl K Br
Use the periodic table to find the two ions (positive ion and negative ion) for each compound. Then write the formula. Remember, the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge. Example: calcium chloride 2+ Ca C (These two charges are not the same, but 2 chloride ions will give an overali negative charge of -2. The positive ion already has a + 2 charge.) Ca²+ Cl₂ Therefore, CaCl₂ is the answer. Name 1) sodium chloride ex. 2) potassium bromide 3) calcium oxide 4) magnesium sulfide Ca²+ CI CI Positive Ion Na+ Count up the total charge. +2, -1, -1 This adds up to zero!! Negative Ion CI Formula NaCl K Br
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![**General Science 3200**
**Worksheet 4: Writing Formulas for Ionic Compounds**
**Use the periodic table to find the two ions (positive ion and negative ion) for each compound. Then write the formula.**
Remember, the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge.
**Example: calcium chloride**
\[
\text{Ca}^{2+} \text{ Cl}^{-}
\]
(These two charges are not the same, but 2 chloride ions will give an overall negative charge of -2. The positive ion already has a +2 charge.)
\[
\text{Ca}^{2+} \text{Cl}_{2}
\]
Count up the total charge:
\[
\begin{array}{c|c}
\text{Ca}^{2+} & +2 \\
\hline
\text{Cl}^{-} & -1 \\
\text{Cl}^{-} & -1 \\
\end{array}
\]
This adds up to zero!!
Therefore, \(\text{CaCl}_2\) is the answer.
| Name | Positive Ion | Negative Ion | Formula |
|--------------------|--------------|--------------|---------|
| 1) sodium chloride | Na\(^+\) | Cl\(^-\) | NaCl |
| 2) potassium bromide| | | KBr |
| 3) calcium oxide | | | |
| 4) magnesium sulfide| | | |
| 5) zinc chloride | | | |
| 6) sodium sulfide | | | |
| 7) strontium fluoride| | | |
| 8) lithium oxide | | | |
| 9) potassium nitride| | | |
| 10) sodium phosphide| | | |
| 11) aluminum chloride| | | |
| 12) calcium nitride| | | |
| 13) aluminum oxide | | | |
| 14) magnesium phosphide| | | |
| 15) aluminum sulfide| | | |
**Note:** Fill in the positive and negative ions using the periodic table](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3b608a1-d4a7-4507-9b6b-c3204bf1cdfc%2F9bc0ba8b-be2d-4668-9349-89c187f75b71%2Fxo68kh6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**General Science 3200**
**Worksheet 4: Writing Formulas for Ionic Compounds**
**Use the periodic table to find the two ions (positive ion and negative ion) for each compound. Then write the formula.**
Remember, the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge.
**Example: calcium chloride**
\[
\text{Ca}^{2+} \text{ Cl}^{-}
\]
(These two charges are not the same, but 2 chloride ions will give an overall negative charge of -2. The positive ion already has a +2 charge.)
\[
\text{Ca}^{2+} \text{Cl}_{2}
\]
Count up the total charge:
\[
\begin{array}{c|c}
\text{Ca}^{2+} & +2 \\
\hline
\text{Cl}^{-} & -1 \\
\text{Cl}^{-} & -1 \\
\end{array}
\]
This adds up to zero!!
Therefore, \(\text{CaCl}_2\) is the answer.
| Name | Positive Ion | Negative Ion | Formula |
|--------------------|--------------|--------------|---------|
| 1) sodium chloride | Na\(^+\) | Cl\(^-\) | NaCl |
| 2) potassium bromide| | | KBr |
| 3) calcium oxide | | | |
| 4) magnesium sulfide| | | |
| 5) zinc chloride | | | |
| 6) sodium sulfide | | | |
| 7) strontium fluoride| | | |
| 8) lithium oxide | | | |
| 9) potassium nitride| | | |
| 10) sodium phosphide| | | |
| 11) aluminum chloride| | | |
| 12) calcium nitride| | | |
| 13) aluminum oxide | | | |
| 14) magnesium phosphide| | | |
| 15) aluminum sulfide| | | |
**Note:** Fill in the positive and negative ions using the periodic table
![**General Science 3200**
**Worksheet 4: Writing Formulas for Ionic Compounds**
**Name:** Joshua Smith
---
Use the periodic table to find the two ions (positive ion and negative ion) for each compound. Then write the formula.
**Remember:** the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge.
**Example: calcium chloride**
\[
\text{Ca}^{2+} \quad \text{Cl}^-
\]
(These two charges are not the same, but 2 chloride ions will give an overall negative charge of -2. The positive ion already has a +2 charge.)
\[
\begin{array}{c}
\text{Ca}^{2+} \\
\text{Cl}^- \quad \text{Cl}^-
\end{array}
\]
Count up the total charge:
+2, -1, -1
This adds up to zero!!
Therefore, \( \text{CaCl}_2 \) is the answer.
---
| **Name** | **Positive Ion** | **Negative Ion** | **Formula** |
|---------------------|-------------------|-------------------|-------------|
| 1) sodium chloride | ex. \( \text{Na}^+ \) | \( \text{Cl}^- \) | \( \text{NaCl} \) |
| 2) potassium bromide| | | \( \text{KBr} \) |
| 3) calcium oxide | | | |
| 4) magnesium sulfide| | | |
| 5) zinc chloride | | | |
| 6) sodium sulfide | | | |
| 7) strontium fluoride| | | |
| 8) lithium oxide | | | |
| 9) potassium nitride| | | |
| 10) sodium phosphide| | | |
| 11) aluminum chloride| | | |
| 12) calcium nitride | | | |
| 13) aluminum oxide | | | |
| 14) magnesium phosphide| | | |
| 15) aluminum sulfide|](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3b608a1-d4a7-4507-9b6b-c3204bf1cdfc%2F9bc0ba8b-be2d-4668-9349-89c187f75b71%2Fdjwo08f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**General Science 3200**
**Worksheet 4: Writing Formulas for Ionic Compounds**
**Name:** Joshua Smith
---
Use the periodic table to find the two ions (positive ion and negative ion) for each compound. Then write the formula.
**Remember:** the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge.
**Example: calcium chloride**
\[
\text{Ca}^{2+} \quad \text{Cl}^-
\]
(These two charges are not the same, but 2 chloride ions will give an overall negative charge of -2. The positive ion already has a +2 charge.)
\[
\begin{array}{c}
\text{Ca}^{2+} \\
\text{Cl}^- \quad \text{Cl}^-
\end{array}
\]
Count up the total charge:
+2, -1, -1
This adds up to zero!!
Therefore, \( \text{CaCl}_2 \) is the answer.
---
| **Name** | **Positive Ion** | **Negative Ion** | **Formula** |
|---------------------|-------------------|-------------------|-------------|
| 1) sodium chloride | ex. \( \text{Na}^+ \) | \( \text{Cl}^- \) | \( \text{NaCl} \) |
| 2) potassium bromide| | | \( \text{KBr} \) |
| 3) calcium oxide | | | |
| 4) magnesium sulfide| | | |
| 5) zinc chloride | | | |
| 6) sodium sulfide | | | |
| 7) strontium fluoride| | | |
| 8) lithium oxide | | | |
| 9) potassium nitride| | | |
| 10) sodium phosphide| | | |
| 11) aluminum chloride| | | |
| 12) calcium nitride | | | |
| 13) aluminum oxide | | | |
| 14) magnesium phosphide| | | |
| 15) aluminum sulfide|
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