Select the group number. 1A (1) $$ 2 A $$ (2) 3 A (13) 4A (14) 5A (15) 6A (16) 7A (17) 8 A (18) Select the generic outer electron configuration. $$ n s^{2} n p^{1} $$ $$ n s^{2} n p^{2} $$ $$ n s^{2} n p^{3} $$ $$ n s^{2} n p^{4} $$ $$ n s^{2} n p^{8} $$ $$ n s^{2} n p^{6} $$

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UpStudy AI · Accepted Answer

Certainly! It looks like you're working on understanding **group numbers** in the periodic table and their corresponding **generic outer electron configurations**. Let's break down each part to help clarify these concepts.

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### **1. Understanding Group Numbers**

The periodic table groups elements based on similar properties, and these groups are identified by numbers. There are two common labeling systems:

- **Old IUPAC System (A/B Notation):**
  - **1A (1)**: Group 1
  - **2A (2)**: Group 2
  - **3A (13)**: Group 13
  - **4A (14)**: Group 14
  - **5A (15)**: Group 15
  - **6A (16)**: Group 16
  - **7A (17)**: Group 17
  - **8A (18)**: Group 18

- **New IUPAC Numbering:**
  - Directly uses **Group 1** through **Group 18** without the A/B designation.

**Your Selection:**
Based on your list:
- **1A (1)**
- **2A (2)**
- **3A (13)**
- **4A (14)**
- **5A (15)**
- **6A (16)**
- **7A (17)**
- **8A (18)**

These correspond to **Groups 1 through 18** in the modern numbering system.

---

### **2. Generic Outer Electron Configurations**

The **outer electron configuration** describes the arrangement of electrons in the outermost shell of an atom, which largely determines an element's chemical behavior. Here's a breakdown based on the group number:

| **Group (Old A/B)** | **Group Number (New)** | **Generic Outer Electron Configuration** |
|---------------------|------------------------|------------------------------------------|
| 1A                  | 1                      | $$ ns^{1} $$                             |
| 2A                  | 2                      | $$ ns^{2} $$                             |
| 3A                  | 13                     | $$ ns^{2} np^{1} $$                      |
| 4A                  | 14                     | $$ ns^{2} np^{2} $$                      |
| 5A                  | 15                     | $$ ns^{2} np^{3} $$                      |
| 6A                  | 16                     | $$ ns^{2} np^{4} $$                      |
| 7A                  | 17                     | $$ ns^{2} np^{5} $$                      |
| 8A                  | 18                     | $$ ns^{2} np^{6} $$                      |

**Explanation of Notation:**
- **n**: Principal quantum number (represents the energy level or shell).
- **s and p**: Types of atomic orbitals.
  - **s** orbitals can hold up to 2 electrons.
  - **p** orbitals can hold up to 6 electrons.
  
**Examples:**
- **Group 1 (1A)**: $$ ns^{1} $$  
  - Example Element: **Sodium (Na)**  
  - Electron Configuration: $$ [Ne] 3s^{1} $$
  
- **Group 17 (7A)**: $$ ns^{2} np^{5} $$  
  - Example Element: **Chlorine (Cl)**  
  - Electron Configuration: $$ [Ne] 3s^{2} 3p^{5} $$
  
- **Group 18 (8A)**: $$ ns^{2} np^{6} $$  
  - Example Element: **Neon (Ne)**  
  - Electron Configuration: $$ [He] 2s^{2} 2p^{6} $$

---

### **3. Matching Groups to Electron Configurations**

If you're tasked with selecting a group number and its corresponding electron configuration, use the table above as a reference. For instance:

- **If you select Group 17 (7A):**
  - **Generic Outer Electron Configuration**: $$ ns^{2} np^{5} $$

- **If you select Group 14 (4A):**
  - **Generic Outer Electron Configuration**: $$ ns^{2} np^{2} $$

---

### **4. Quick Reference for Generic Outer Electron Configurations**

Here’s a shortlist based on your provided options:

- **$$ ns^{2} np^{1} $$**: **Group 13 (3A)**
- **$$ ns^{2} np^{2} $$**: **Group 14 (4A)**
- **$$ ns^{2} np^{3} $$**: **Group 15 (5A)**
- **$$ ns^{2} np^{4} $$**: **Group 16 (6A)**
- **$$ ns^{2} np^{5} $$**: **Group 17 (7A)**
- **$$ ns^{2} np^{6} $$**: **Group 18 (8A)**

---

### **Conclusion**

By understanding the relationship between group numbers and their generic outer electron configurations, you can predict the chemical properties of elements and their behavior in reactions. Use the group number to determine the number of valence electrons, which are crucial for bonding and reactivity.

If you have a specific element or group in mind and need further assistance, feel free to ask!
Group numbers and their corresponding generic outer electron configurations are as follows: - **Group 1 (1A):** $$ ns^{1} $$ - **Group 2 (2A):** $$ ns^{2} $$ - **Group 13 (3A):** $$ ns^{2} np^{1} $$ - **Group 14 (4A):** $$ ns^{2} np^{2} $$ - **Group 15 (5A):** $$ ns^{2} np^{3} $$ - **Group 16 (6A):** $$ ns^{2} np^{4} $$ - **Group 17 (7A):** $$ ns^{2} np^{5} $$ - **Group 18 (8A):** $$ ns^{2} np^{6} $$ These configurations help determine an element's chemical properties based on its valence electrons.

Select the group number. 1A (1) \( 2 A \) (2) 3 A (13) 4A (14) 5A (15) 6A (16) 7A (17) 8 A (18) Select the generic outer electron configuration. \( n s^{2} n p^{1} \) \( n s^{2} n p^{2} \) \( n s^{2} n p^{3} \) \( n s^{2} n p^{4} \) \( n s^{2} n p^{8} \) \( n s^{2} n p^{6} \)

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