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--- ### Periodic Table and Ionic Compound Formation #### Use the References to access important values if needed for this question. **Periodic Table**: The image shows a periodic table with elements color-coded: - **Yellow**: Group 1A, Group 2A, and Group 8A, which include elements like Hydrogen (H), Helium (He), and Neon (Ne). - **Blue**: Transition metals (3B to 12B) and Lanthanides and Actinides series. - **Green**: Group 3A to 7A, which include metalloids and other non-metals such as Carbon (C), Nitrogen (N), and Oxygen (O). **Question**: When rubidium reacts with iodine to form an ionic compound, each metal atom loses ____ electron(s) and each nonmetal atom gains ____ electron(s). There must be ____ rubidium atom(s) for every ____ iodine atom(s) in the reaction. **Options for Inputs**: For each blank, the input could be: - Number of electron(s) lost by rubidium atoms. - Number of electron(s) gained by iodine atoms. - The ratio of rubidium atoms to iodine atoms in the reaction. **Next Steps**: - Complete the blanks with correct values based on the periodic table and your understanding of ionic compounds. - Once done, click on "Submit Answer." - If corrections are needed, use "Retry Entire Group." **Buttons to Proceed**: - **Submit Answer** - **Retry Entire Group** - **Previous** - **Next** This interactive exercise aims to help students understand the basics of ionic bonding and the importance of the periodic table in predicting how elements will react with each other. --- **Note**: The blank spaces in the question are to be filled based on your understanding of Rubidium (Rb) losing one electron (as it is in Group 1) and Iodine (I) gaining one electron (as it is in Group 7), forming an ionic bond with a 1:1 ratio.

--- ### Periodic Table and Ionic Compound Formation #### Use the References to access important values if needed for this question. **Periodic Table**: The image shows a periodic table with elements color-coded: - **Yellow**: Group 1A, Group 2A, and Group 8A, which include elements like Hydrogen (H), Helium (He), and Neon (Ne). - **Blue**: Transition metals (3B to 12B) and Lanthanides and Actinides series. - **Green**: Group 3A to 7A, which include metalloids and other non-metals such as Carbon (C), Nitrogen (N), and Oxygen (O). **Question**: When rubidium reacts with iodine to form an ionic compound, each metal atom loses ____ electron(s) and each nonmetal atom gains ____ electron(s). There must be ____ rubidium atom(s) for every ____ iodine atom(s) in the reaction. **Options for Inputs**: For each blank, the input could be: - Number of electron(s) lost by rubidium atoms. - Number of electron(s) gained by iodine atoms. - The ratio of rubidium atoms to iodine atoms in the reaction. **Next Steps**: - Complete the blanks with correct values based on the periodic table and your understanding of ionic compounds. - Once done, click on "Submit Answer." - If corrections are needed, use "Retry Entire Group." **Buttons to Proceed**: - **Submit Answer** - **Retry Entire Group** - **Previous** - **Next** This interactive exercise aims to help students understand the basics of ionic bonding and the importance of the periodic table in predicting how elements will react with each other. --- **Note**: The blank spaces in the question are to be filled based on your understanding of Rubidium (Rb) losing one electron (as it is in Group 1) and Iodine (I) gaining one electron (as it is in Group 7), forming an ionic bond with a 1:1 ratio.

Chemistry
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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--- ### Periodic Table and Ionic Compound Formation #### Use the References to access important values if needed for this question. **Periodic Table**: The image shows a periodic table with elements color-coded: - **Yellow**: Group 1A, Group 2A, and Group 8A, which include elements like Hydrogen (H), Helium (He), and Neon (Ne). - **Blue**: Transition metals (3B to 12B) and Lanthanides and Actinides series. - **Green**: Group 3A to 7A, which include metalloids and other non-metals such as Carbon (C), Nitrogen (N), and Oxygen (O). **Question**: When rubidium reacts with iodine to form an ionic compound, each metal atom loses ____ electron(s) and each nonmetal atom gains ____ electron(s). There must be ____ rubidium atom(s) for every ____ iodine atom(s) in the reaction. **Options for Inputs**: For each blank, the input could be: - Number of electron(s) lost by rubidium atoms. - Number of electron(s) gained by iodine atoms. - The ratio of rubidium atoms to iodine atoms in the reaction. **Next Steps**: - Complete the blanks with correct values based on the periodic table and your understanding of ionic compounds. - Once done, click on "Submit Answer." - If corrections are needed, use "Retry Entire Group." **Buttons to Proceed**: - **Submit Answer** - **Retry Entire Group** - **Previous** - **Next** This interactive exercise aims to help students understand the basics of ionic bonding and the importance of the periodic table in predicting how elements will react with each other. --- **Note**: The blank spaces in the question are to be filled based on your understanding of Rubidium (Rb) losing one electron (as it is in Group 1) and Iodine (I) gaining one electron (as it is in Group 7), forming an ionic bond with a 1:1 ratio.
Transcribed Image Text:--- ### Periodic Table and Ionic Compound Formation #### Use the References to access important values if needed for this question. **Periodic Table**: The image shows a periodic table with elements color-coded: - **Yellow**: Group 1A, Group 2A, and Group 8A, which include elements like Hydrogen (H), Helium (He), and Neon (Ne). - **Blue**: Transition metals (3B to 12B) and Lanthanides and Actinides series. - **Green**: Group 3A to 7A, which include metalloids and other non-metals such as Carbon (C), Nitrogen (N), and Oxygen (O). **Question**: When rubidium reacts with iodine to form an ionic compound, each metal atom loses ____ electron(s) and each nonmetal atom gains ____ electron(s). There must be ____ rubidium atom(s) for every ____ iodine atom(s) in the reaction. **Options for Inputs**: For each blank, the input could be: - Number of electron(s) lost by rubidium atoms. - Number of electron(s) gained by iodine atoms. - The ratio of rubidium atoms to iodine atoms in the reaction. **Next Steps**: - Complete the blanks with correct values based on the periodic table and your understanding of ionic compounds. - Once done, click on "Submit Answer." - If corrections are needed, use "Retry Entire Group." **Buttons to Proceed**: - **Submit Answer** - **Retry Entire Group** - **Previous** - **Next** This interactive exercise aims to help students understand the basics of ionic bonding and the importance of the periodic table in predicting how elements will react with each other. --- **Note**: The blank spaces in the question are to be filled based on your understanding of Rubidium (Rb) losing one electron (as it is in Group 1) and Iodine (I) gaining one electron (as it is in Group 7), forming an ionic bond with a 1:1 ratio.
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