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Assume that the filling of orbitals must be sequential, -1 → 0 → 1 (corresponding to px → Py→ P2) What element (use the symbol only) have the four quantum number set for the last electron added? 1. (3,1,0,-1/2) = 2. (4,3,-2,+1/2) 3. (2,1,0,-1/2) What is the four quantum number set for the last electron added to the following elements: 4. Sn = (

Assume that the filling of orbitals must be sequential, -1 → 0 → 1 (corresponding to px → Py→ P2) What element (use the symbol only) have the four quantum number set for the last electron added? 1. (3,1,0,-1/2) = 2. (4,3,-2,+1/2) 3. (2,1,0,-1/2) What is the four quantum number set for the last electron added to the following elements: 4. Sn = (

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Quantum Numbers and Electron Configuration #### Sequential Filling of Orbitals Assume that the filling of orbitals must be sequential, with the following transitions: - -1 → 0 → 1 (corresponding to \( p_x \rightarrow p_y \rightarrow p_z \)) #### Identifying Elements from Quantum Numbers Determine the element (using the symbol only) that has the following four quantum number set for the last electron added: 1. (3,1,0,-1/2) = _______ 2. (4,3,-2,+1/2) = _______ 3. (2,1,0,-1/2) = _______ #### Quantum Numbers for Specific Elements Identify the four quantum numbers for the last electron added to the following elements: 4. Sn (__________, __________, __________, __________) 5. Cf (__________, __________, __________, __________) #### Counting Electrons with Given Quantum Numbers Determine the number of electrons which have the following quantum number sets: 6. (3,?,?-1/2) = _______ 7. (?,0,0,?) = _______ 8. (2,1,?,?) = _______ 9. (?,1,-1,-1/2) = _______ 10. (7,?,-1,-1/2) = _______ ### Explanation of Quantum Numbers Quantum numbers are used to describe the unique quantum state of an electron in an atom. They consist of: - **Principal Quantum Number (n)**: Indicates the main energy level of the electron. - **Azimuthal Quantum Number (l)**: Indicates the shape of the orbital. It ranges from 0 to n-1. - \( l = 0 \): s orbital - \( l = 1 \): p orbital - \( l = 2 \): d orbital - \( l = 3 \): f orbital - **Magnetic Quantum Number (m_l)**: Indicates the orientation of the orbital. It ranges from -l to +l. - **Spin Quantum Number (m_s)**: Indicates the spin of the electron. It can be +1/2 or -1/2. Use this information to fill in the blanks with appropriate values or symbols.
Transcribed Image Text:### Quantum Numbers and Electron Configuration #### Sequential Filling of Orbitals Assume that the filling of orbitals must be sequential, with the following transitions: - -1 → 0 → 1 (corresponding to \( p_x \rightarrow p_y \rightarrow p_z \)) #### Identifying Elements from Quantum Numbers Determine the element (using the symbol only) that has the following four quantum number set for the last electron added: 1. (3,1,0,-1/2) = _______ 2. (4,3,-2,+1/2) = _______ 3. (2,1,0,-1/2) = _______ #### Quantum Numbers for Specific Elements Identify the four quantum numbers for the last electron added to the following elements: 4. Sn (__________, __________, __________, __________) 5. Cf (__________, __________, __________, __________) #### Counting Electrons with Given Quantum Numbers Determine the number of electrons which have the following quantum number sets: 6. (3,?,?-1/2) = _______ 7. (?,0,0,?) = _______ 8. (2,1,?,?) = _______ 9. (?,1,-1,-1/2) = _______ 10. (7,?,-1,-1/2) = _______ ### Explanation of Quantum Numbers Quantum numbers are used to describe the unique quantum state of an electron in an atom. They consist of: - **Principal Quantum Number (n)**: Indicates the main energy level of the electron. - **Azimuthal Quantum Number (l)**: Indicates the shape of the orbital. It ranges from 0 to n-1. - \( l = 0 \): s orbital - \( l = 1 \): p orbital - \( l = 2 \): d orbital - \( l = 3 \): f orbital - **Magnetic Quantum Number (m_l)**: Indicates the orientation of the orbital. It ranges from -l to +l. - **Spin Quantum Number (m_s)**: Indicates the spin of the electron. It can be +1/2 or -1/2. Use this information to fill in the blanks with appropriate values or symbols.
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