**Periodic Table Reference for Bromine and Fluorine Compounds** **Diagram Description:** The image displays a periodic table of elements, color-coded with the following groups for ease of identification: - **Group 1A (Alkali Metals):** Li, Na, K, Rb, Cs, Fr (highlighted in pink) - **Group 2A (Alkaline Earth Metals):** Be, Mg, Ca, Sr, Ba, Ra (highlighted in light blue) - **Group 3A:** B, Al, Ga, In, Tl (highlighted in green) - **Group 4A:** C, Si, Ge, Sn, Pb (highlighted in yellow) - **Group 5A:** N, P, As, Sb, Bi (highlighted in light orange) - **Group 6A:** O, S, Se, Te, Po (highlighted in dark orange) - **Group 7A (Halogens):** F, Cl, Br, I, At (highlighted in dark blue) - **Group 8A (Noble Gases):** He, Ne, Ar, Kr, Xe, Rn (highlighted in light orange) - **Transition Metals:** Groups 3 to 12 (highlighted in a shade of blue and blue-gray) - **Lanthanides and Actinides:** La-Lu and Ac-Lr (highlighted in dark blue) **Text Section:** The element **bromine** would be expected to form ____ covalent bond(s) in order to obey the octet rule. Use the octet rule to predict the formula of the compound that would form between **bromine** and **fluorine**, if the molecule contains one bromine atom and only single bonds are formed. **Formula:** [Input box for the answer] **Actions:** - [Submit Answer] button - [Retry Entire Group] button (1 more group attempt remaining) --- **Instructions for Educational Purpose:** 1. **Understanding Covalent Bonds and the Octet Rule:** - Bromine (Br) is in Group 7A, which means it has 7 valence electrons. To obey the octet rule, it needs to gain 1 more electron to complete its valence shell with 8 electrons. 2. **Predicting the Compound Formula Between Bromine and Fluorine:** - Flu
**Periodic Table Reference for Bromine and Fluorine Compounds** **Diagram Description:** The image displays a periodic table of elements, color-coded with the following groups for ease of identification: - **Group 1A (Alkali Metals):** Li, Na, K, Rb, Cs, Fr (highlighted in pink) - **Group 2A (Alkaline Earth Metals):** Be, Mg, Ca, Sr, Ba, Ra (highlighted in light blue) - **Group 3A:** B, Al, Ga, In, Tl (highlighted in green) - **Group 4A:** C, Si, Ge, Sn, Pb (highlighted in yellow) - **Group 5A:** N, P, As, Sb, Bi (highlighted in light orange) - **Group 6A:** O, S, Se, Te, Po (highlighted in dark orange) - **Group 7A (Halogens):** F, Cl, Br, I, At (highlighted in dark blue) - **Group 8A (Noble Gases):** He, Ne, Ar, Kr, Xe, Rn (highlighted in light orange) - **Transition Metals:** Groups 3 to 12 (highlighted in a shade of blue and blue-gray) - **Lanthanides and Actinides:** La-Lu and Ac-Lr (highlighted in dark blue) **Text Section:** The element **bromine** would be expected to form ____ covalent bond(s) in order to obey the octet rule. Use the octet rule to predict the formula of the compound that would form between **bromine** and **fluorine**, if the molecule contains one bromine atom and only single bonds are formed. **Formula:** [Input box for the answer] **Actions:** - [Submit Answer] button - [Retry Entire Group] button (1 more group attempt remaining) --- **Instructions for Educational Purpose:** 1. **Understanding Covalent Bonds and the Octet Rule:** - Bromine (Br) is in Group 7A, which means it has 7 valence electrons. To obey the octet rule, it needs to gain 1 more electron to complete its valence shell with 8 electrons. 2. **Predicting the Compound Formula Between Bromine and Fluorine:** - Flu
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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Question
![**Periodic Table Reference for Bromine and Fluorine Compounds**
**Diagram Description:**
The image displays a periodic table of elements, color-coded with the following groups for ease of identification:
- **Group 1A (Alkali Metals):** Li, Na, K, Rb, Cs, Fr (highlighted in pink)
- **Group 2A (Alkaline Earth Metals):** Be, Mg, Ca, Sr, Ba, Ra (highlighted in light blue)
- **Group 3A:** B, Al, Ga, In, Tl (highlighted in green)
- **Group 4A:** C, Si, Ge, Sn, Pb (highlighted in yellow)
- **Group 5A:** N, P, As, Sb, Bi (highlighted in light orange)
- **Group 6A:** O, S, Se, Te, Po (highlighted in dark orange)
- **Group 7A (Halogens):** F, Cl, Br, I, At (highlighted in dark blue)
- **Group 8A (Noble Gases):** He, Ne, Ar, Kr, Xe, Rn (highlighted in light orange)
- **Transition Metals:** Groups 3 to 12 (highlighted in a shade of blue and blue-gray)
- **Lanthanides and Actinides:** La-Lu and Ac-Lr (highlighted in dark blue)
**Text Section:**
The element **bromine** would be expected to form ____ covalent bond(s) in order to obey the octet rule.
Use the octet rule to predict the formula of the compound that would form between **bromine** and **fluorine**, if the molecule contains one bromine atom and only single bonds are formed.
**Formula:** [Input box for the answer]
**Actions:**
- [Submit Answer] button
- [Retry Entire Group] button (1 more group attempt remaining)
---
**Instructions for Educational Purpose:**
1. **Understanding Covalent Bonds and the Octet Rule:**
- Bromine (Br) is in Group 7A, which means it has 7 valence electrons. To obey the octet rule, it needs to gain 1 more electron to complete its valence shell with 8 electrons.
2. **Predicting the Compound Formula Between Bromine and Fluorine:**
- Flu](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Feaa5a7b0-21f2-4968-9418-f1b1154c7382%2F67d8758e-ec95-4678-82b8-7888376ac2c2%2F2yxtemr.jpeg&w=3840&q=75)
Transcribed Image Text:**Periodic Table Reference for Bromine and Fluorine Compounds**
**Diagram Description:**
The image displays a periodic table of elements, color-coded with the following groups for ease of identification:
- **Group 1A (Alkali Metals):** Li, Na, K, Rb, Cs, Fr (highlighted in pink)
- **Group 2A (Alkaline Earth Metals):** Be, Mg, Ca, Sr, Ba, Ra (highlighted in light blue)
- **Group 3A:** B, Al, Ga, In, Tl (highlighted in green)
- **Group 4A:** C, Si, Ge, Sn, Pb (highlighted in yellow)
- **Group 5A:** N, P, As, Sb, Bi (highlighted in light orange)
- **Group 6A:** O, S, Se, Te, Po (highlighted in dark orange)
- **Group 7A (Halogens):** F, Cl, Br, I, At (highlighted in dark blue)
- **Group 8A (Noble Gases):** He, Ne, Ar, Kr, Xe, Rn (highlighted in light orange)
- **Transition Metals:** Groups 3 to 12 (highlighted in a shade of blue and blue-gray)
- **Lanthanides and Actinides:** La-Lu and Ac-Lr (highlighted in dark blue)
**Text Section:**
The element **bromine** would be expected to form ____ covalent bond(s) in order to obey the octet rule.
Use the octet rule to predict the formula of the compound that would form between **bromine** and **fluorine**, if the molecule contains one bromine atom and only single bonds are formed.
**Formula:** [Input box for the answer]
**Actions:**
- [Submit Answer] button
- [Retry Entire Group] button (1 more group attempt remaining)
---
**Instructions for Educational Purpose:**
1. **Understanding Covalent Bonds and the Octet Rule:**
- Bromine (Br) is in Group 7A, which means it has 7 valence electrons. To obey the octet rule, it needs to gain 1 more electron to complete its valence shell with 8 electrons.
2. **Predicting the Compound Formula Between Bromine and Fluorine:**
- Flu
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