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electron within a region. To describe that region, we need four quantum numbers Quantum number Principal quantum number Angular momentum quantum number Magnetic quantum number Spin quantum number (n) 4,3,2,1 Shapes of orbitals: (1) value 0 1 Symbol used S symbol (n) P (1) (mi) (ms) Possible numerical values Whole numbers: 1, 2, 3, etc. Depends on the value of (n) Whole numbers starts at 0, 1, 2,..., n-1 Depends on the value of ()- Whole numbers -1,. ., 0,..,+1 Only possible values are + or -1 What does it tell us ● ● ● ● ● ● ● The value of (n) tells you the number of different orbitals possible in an energy level. For example, when n = 3, there should be three different type of orbitals present, those are s, p, and d with corresponding () values of 0, 1, and 2. Complete the following table giving all possible values for n = 4. Remember that (1) starts at zero and ends at n-1. (ms) ADAL (m₁) (1) 3 ● shape ● Size of the orbital Distance from the nucleus Energy level where the electron is located Type and shape of the area in the energy level (sublevel) Known as s, p, d, f, etc The shapes of orbitals when placed in a magnetic field generate possible orientations. The specific orbital within a set of degenerate orbitals where the electron is located Similar to assigning rooms in a house Was the first electron in the specific orbital or sublevel or was it the second one? Related to the arrows drawn in the expanded electron configuration: 1st (1), 2nd (1) (m)

electron within a region. To describe that region, we need four quantum numbers Quantum number Principal quantum number Angular momentum quantum number Magnetic quantum number Spin quantum number (n) 4,3,2,1 Shapes of orbitals: (1) value 0 1 Symbol used S symbol (n) P (1) (mi) (ms) Possible numerical values Whole numbers: 1, 2, 3, etc. Depends on the value of (n) Whole numbers starts at 0, 1, 2,..., n-1 Depends on the value of ()- Whole numbers -1,. ., 0,..,+1 Only possible values are + or -1 What does it tell us ● ● ● ● ● ● ● The value of (n) tells you the number of different orbitals possible in an energy level. For example, when n = 3, there should be three different type of orbitals present, those are s, p, and d with corresponding () values of 0, 1, and 2. Complete the following table giving all possible values for n = 4. Remember that (1) starts at zero and ends at n-1. (ms) ADAL (m₁) (1) 3 ● shape ● Size of the orbital Distance from the nucleus Energy level where the electron is located Type and shape of the area in the energy level (sublevel) Known as s, p, d, f, etc The shapes of orbitals when placed in a magnetic field generate possible orientations. The specific orbital within a set of degenerate orbitals where the electron is located Similar to assigning rooms in a house Was the first electron in the specific orbital or sublevel or was it the second one? Related to the arrows drawn in the expanded electron configuration: 1st (1), 2nd (1) (m)

Chemistry
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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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1045 Worksheets Learning Objectives Quantum Numbers Learn the relationship between quantum numbers and atomic orbitals Be able to identify the four quantum numbers of any electron in an element Be able to discriminate between valid and invalid quantum numbers Quantum number Principal quantum number Quantum numbers are a description of the most probable area in an atom where a specific electron might be located. The region in space where we can find an electron is known as an orbital. The shape of the orbitals is derived from the solution of quantum mechanical equations. In this class we use an oversimplification of these concepts. We only talk about the probability of locating an electron within a region. To describe that region, we need four quantum numbers Angular momentum quantum number Magnetic quantum number Spin quantum number (n) 4,3,2,1 Shapes of orbitals: (1) Symbol value used 0 P S symbol (n) P (0) (mi) (ms) Possible numerical values Whole numbers: 1, 2, 3, etc. 3 Depends on the value of (n) Whole numbers starts at 0, 1, 2, ..., n-1 Depends on the value of (1) Whole numbers -1,. ., 0, . .,+1 Only possible values are + ½ or - ½ What does it tell us ● Elizabeth Galaz DID: 6376083 CHM 1045 The value of (n) tells you the number of different orbitals possible in an energy level. For example, when n = 3, there should be three different type of orbitals present, those are s, p, and d with corresponding () values of 0, 1, and 2. Complete the following table giving all possible values for n = 4. Remember that (1) starts at zero and ends at n-1. (ms) (m₁) (1) ● shape FIU-BBC Size of the orbital Distance from the nucleus Energy level where the electron is located Type and shape of the area in the energy level (sublevel) Known as s, p, d, f, etc The shapes of orbitals when placed in a magnetic field generate possible orientations. The specific orbital within a set of degenerate orbitals where the electron is located Similar to assigning rooms in a house Was the first electron in the specific orbital or sublevel or was it the second one? Related to the arrows drawn in the expanded electron configuration: 1st (1), 2nd (1) (m₁)
Transcribed Image Text:1045 Worksheets Learning Objectives Quantum Numbers Learn the relationship between quantum numbers and atomic orbitals Be able to identify the four quantum numbers of any electron in an element Be able to discriminate between valid and invalid quantum numbers Quantum number Principal quantum number Quantum numbers are a description of the most probable area in an atom where a specific electron might be located. The region in space where we can find an electron is known as an orbital. The shape of the orbitals is derived from the solution of quantum mechanical equations. In this class we use an oversimplification of these concepts. We only talk about the probability of locating an electron within a region. To describe that region, we need four quantum numbers Angular momentum quantum number Magnetic quantum number Spin quantum number (n) 4,3,2,1 Shapes of orbitals: (1) Symbol value used 0 P S symbol (n) P (0) (mi) (ms) Possible numerical values Whole numbers: 1, 2, 3, etc. 3 Depends on the value of (n) Whole numbers starts at 0, 1, 2, ..., n-1 Depends on the value of (1) Whole numbers -1,. ., 0, . .,+1 Only possible values are + ½ or - ½ What does it tell us ● Elizabeth Galaz DID: 6376083 CHM 1045 The value of (n) tells you the number of different orbitals possible in an energy level. For example, when n = 3, there should be three different type of orbitals present, those are s, p, and d with corresponding () values of 0, 1, and 2. Complete the following table giving all possible values for n = 4. Remember that (1) starts at zero and ends at n-1. (ms) (m₁) (1) ● shape FIU-BBC Size of the orbital Distance from the nucleus Energy level where the electron is located Type and shape of the area in the energy level (sublevel) Known as s, p, d, f, etc The shapes of orbitals when placed in a magnetic field generate possible orientations. The specific orbital within a set of degenerate orbitals where the electron is located Similar to assigning rooms in a house Was the first electron in the specific orbital or sublevel or was it the second one? Related to the arrows drawn in the expanded electron configuration: 1st (1), 2nd (1) (m₁)
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M 1045 Worksheets 2 3 d From Harry Ramanantoanina, University of Fribourg, Department of Chemistry Example 1: the four quantum numbers for the last electron in He are: {n, I, m₁, ms} a) electron configuration: 1s² b) energy level where electron is located? 1 then n=1 c) type of orbital used? S then l=0 d) is there more than one of those orbitals in the energy level? If yes, expand the configuration and identify in which of them is the electron located If not, then the only possible value of m₁ = 0 e) was it the first or second electron placed in that specific orbital? Second then ms = - ¹1/2 Summary: {1,0,0,- 1} Example 2: what are the four quantum numbers for the last electron in oxygen? ↑↓ -1 # a) electron configuration: 1s²2s²2p4 last electron is 2p4 b) energy level where electron is located? 2 then n=2 c) type of orbital used? p then l=1 d) is there more than one of those orbitals in the energy level? yes, we need to expand the configuration and identify in which of them is the electron located (remember to place one arrow in each separate orbital from left to write and then pair when necessary) 0 2p +1 4. Which is not possible ever? (Yes, if not why) a. {4, 0, -1, +1/2) b. {8, 2, -2, -1/2} 3. What is the electron configuration that corresponds to {4, 3, +3, -1/2}. 38 The fourth electron in the 2p orbital was located in the orbital labeled (-1) then m₁ = -1 e) was it the first or second electron placed in that specific orbital? Second electron Summary: (2,1,-1,-12} Your turn: Give the four quantum numbers which describe the location of each of the following: 1. The 25th electron in In 2. The last electron in Hs c) {6, 3,-2, +1/2}_ d) {4, 5, -3, +1/2} FIU-BBC then ms = - 12
Transcribed Image Text:M 1045 Worksheets 2 3 d From Harry Ramanantoanina, University of Fribourg, Department of Chemistry Example 1: the four quantum numbers for the last electron in He are: {n, I, m₁, ms} a) electron configuration: 1s² b) energy level where electron is located? 1 then n=1 c) type of orbital used? S then l=0 d) is there more than one of those orbitals in the energy level? If yes, expand the configuration and identify in which of them is the electron located If not, then the only possible value of m₁ = 0 e) was it the first or second electron placed in that specific orbital? Second then ms = - ¹1/2 Summary: {1,0,0,- 1} Example 2: what are the four quantum numbers for the last electron in oxygen? ↑↓ -1 # a) electron configuration: 1s²2s²2p4 last electron is 2p4 b) energy level where electron is located? 2 then n=2 c) type of orbital used? p then l=1 d) is there more than one of those orbitals in the energy level? yes, we need to expand the configuration and identify in which of them is the electron located (remember to place one arrow in each separate orbital from left to write and then pair when necessary) 0 2p +1 4. Which is not possible ever? (Yes, if not why) a. {4, 0, -1, +1/2) b. {8, 2, -2, -1/2} 3. What is the electron configuration that corresponds to {4, 3, +3, -1/2}. 38 The fourth electron in the 2p orbital was located in the orbital labeled (-1) then m₁ = -1 e) was it the first or second electron placed in that specific orbital? Second electron Summary: (2,1,-1,-12} Your turn: Give the four quantum numbers which describe the location of each of the following: 1. The 25th electron in In 2. The last electron in Hs c) {6, 3,-2, +1/2}_ d) {4, 5, -3, +1/2} FIU-BBC then ms = - 12
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