Videos
(a)
Interpretation:
The values of the quantum numbers associated with the given orbitals should be identified using the concept of quantum numbers.
Concept Introduction:
Each electron in an atom is described by four different quantum numbers. The first three (n, l, ml) specify the particular orbital of interest, and the fourth (ms) specifies how many electrons can occupy that orbital.
Principal Quantum Number (n)
The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in
The angular momentum quantum number (l) explains the shape of the atomic orbital. The values of l are integers which depend on the value of the principal quantum number, n. For a given value of n, the possible values of l range are from 0 to n − 1. If n = 1, there is only one possible value of l (l=0). If n = 2, there are two values of l: 0 and 1. If n = 3, there are three values of l: 0, 1, and 2. The value of l is selected by the letters s, p, d, and f. If l = 0, we have an s orbital; if l = 1, we have a p orbital; if l = 2, we have a d orbital and finally if l = 3, we have a f orbital. A collection of orbitals with the same value of n is called a shell. One or more orbitals with the same n and l values are referred to a subshell (sublevel). The value of l also has a slight effect on the energy of the subshell; the energy of the subshell increases with l (s < p < d < f).
Magnetic Quantum Number (ml)
The magnetic quantum number (ml) explains the orientation of the orbital in space. The value of ml depends on the value of l in a subshell. This number divides the subshell into individual orbitals which hold the electrons. For a certain value of l, there are (2l + 1) integral values of ml which is explained as follows:
ml = ‒ l, ..., 0, ..., +l
If l = 0, there is only one possible value of ml: 0.
If l = 1, then there are three values of ml: −1, 0, and +1.
If l = 2, there are five values of ml, namely, −2, −1, 0, +1, and +2.
If l = 3, there are seven values of ml, namely, −3, −2, −1, 0, +1, +2, and +3, and so on.
The number of ml values indicates the number of orbitals in a subshell with a particular l value. Therefore, each ml value refers to a different orbital.
Electron Spin Quantum Number (ms)
It specifies the orientation of the spin axis of an electron. An electron can spin in only one of two directions. There are two possible ways to represent ms values. They are +½ and ‒½. One electron spins in the clockwise direction. Another electron spins in the anticlockwise direction. But, no two electrons should have the same spin quantum number.
To find: Get the values of the quantum numbers (n, l, ml, ms) associated with the given orbital (a) 2p
Get the values of the quantum numbers ‘n’, ‘l’ in (a)
(b)
Interpretation:
The values of the quantum numbers associated with the given orbitals should be identified using the concept of quantum numbers.
Concept Introduction:
Each electron in an atom is described by four different quantum numbers. The first three (n, l, ml) specify the particular orbital of interest, and the fourth (ms) specifies how many electrons can occupy that orbital.
Principal Quantum Number (n)
The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n2. As the value of ‘n’ increases, the energy of the electron also increases.
Angular Momentum Quantum Number (l)
The angular momentum quantum number (l) explains the shape of the atomic orbital. The values of l are integers which depend on the value of the principal quantum number, n. For a given value of n, the possible values of l range are from 0 to n − 1. If n = 1, there is only one possible value of l (l=0). If n = 2, there are two values of l: 0 and 1. If n = 3, there are three values of l: 0, 1, and 2. The value of l is selected by the letters s, p, d, and f. If l = 0, we have an s orbital; if l = 1, we have a p orbital; if l = 2, we have a d orbital and finally if l = 3, we have a f orbital. A collection of orbitals with the same value of n is called a shell. One or more orbitals with the same n and l values are referred to a subshell (sublevel). The value of l also has a slight effect on the energy of the subshell; the energy of the subshell increases with l (s < p < d < f).
Magnetic Quantum Number (ml)
The magnetic quantum number (ml) explains the orientation of the orbital in space. The value of ml depends on the value of l in a subshell. This number divides the subshell into individual orbitals which hold the electrons. For a certain value of l, there are (2l + 1) integral values of ml which is explained as follows:
ml = ‒ l, ..., 0, ..., +l
If l = 0, there is only one possible value of ml: 0.
If l = 1, then there are three values of ml: −1, 0, and +1.
If l = 2, there are five values of ml, namely, −2, −1, 0, +1, and +2.
If l = 3, there are seven values of ml, namely, −3, −2, −1, 0, +1, +2, and +3, and so on.
The number of ml values indicates the number of orbitals in a subshell with a particular l value. Therefore, each ml value refers to a different orbital.
Electron Spin Quantum Number (ms)
It specifies the orientation of the spin axis of an electron. An electron can spin in only one of two directions. There are two possible ways to represent ms values. They are +½ and ‒½. One electron spins in the clockwise direction. Another electron spins in the anticlockwise direction. But, no two electrons should have the same spin quantum number.
To find: Get the values of the quantum numbers (n, l, ml, ms) associated with the given orbital (b) 3s
Get the values of the quantum numbers ‘n’, ‘l’ in (b)
(c)
Interpretation:
The values of the quantum numbers associated with the given orbitals should be identified using the concept of quantum numbers.
Concept Introduction:
Each electron in an atom is described by four different quantum numbers. The first three (n, l, ml) specify the particular orbital of interest, and the fourth (ms) specifies how many electrons can occupy that orbital.
Principal Quantum Number (n)
The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n2. As the value of ‘n’ increases, the energy of the electron also increases.
Angular Momentum Quantum Number (l)
The angular momentum quantum number (l) explains the shape of the atomic orbital. The values of l are integers which depend on the value of the principal quantum number, n. For a given value of n, the possible values of l range are from 0 to n − 1. If n = 1, there is only one possible value of l (l=0). If n = 2, there are two values of l: 0 and 1. If n = 3, there are three values of l: 0, 1, and 2. The value of l is selected by the letters s, p, d, and f. If l = 0, we have an s orbital; if l = 1, we have a p orbital; if l = 2, we have a d orbital and finally if l = 3, we have a f orbital. A collection of orbitals with the same value of n is called a shell. One or more orbitals with the same n and l values are referred to a subshell (sublevel). The value of l also has a slight effect on the energy of the subshell; the energy of the subshell increases with l (s < p < d < f).
Magnetic Quantum Number (ml)
The magnetic quantum number (ml) explains the orientation of the orbital in space. The value of ml depends on the value of l in a subshell. This number divides the subshell into individual orbitals which hold the electrons. For a certain value of l, there are (2l + 1) integral values of ml which is explained as follows:
ml = ‒ l, ..., 0, ..., +l
If l = 0, there is only one possible value of ml: 0.
If l = 1, then there are three values of ml: −1, 0, and +1.
If l = 2, there are five values of ml, namely, −2, −1, 0, +1, and +2.
If l = 3, there are seven values of ml, namely, −3, −2, −1, 0, +1, +2, and +3, and so on.
The number of ml values indicates the number of orbitals in a subshell with a particular l value. Therefore, each ml value refers to a different orbital.
Electron Spin Quantum Number (ms)
It specifies the orientation of the spin axis of an electron. An electron can spin in only one of two directions. There are two possible ways to represent ms values. They are +½ and ‒½. One electron spins in the clockwise direction. Another electron spins in the anticlockwise direction. But, no two electrons should have the same spin quantum number.
To find: Get the values of the quantum numbers (n, l, ml, ms) associated with the given orbital (c) 5d
Get the values of the quantum numbers ‘n’, ‘l’ in (c)
Want to see the full answer?
Check out a sample textbook solution
Chapter 7 Solutions
EBK GENERAL CHEMISTRY: THE ESSENTIAL CO
- 4. Read paragraph 4.15 from your textbook, use your calculated lattice energy values for CuO, CuCO3 and Cu(OH)2 an explain thermal decomposition reaction of malachite: Cu2CO3(OH)2 →2CuO + H2O + CO2 (3 points)arrow_forwardPlease sirrr soollveee these parts pleaseeee and thank youuuuuarrow_forwardIII O Organic Chemistry Using wedges and dashes in skeletal structures Draw a skeletal ("line") structure for each of the molecules below. Be sure your structures show the important difference between the molecules. key O O O O O CHON Cl jiii iiiiiiii You can drag the slider to rotate the molecules. Explanation Check Click and drag to start drawing a structure. Q Search X G ©2025 McGraw Hill LLC. All Rights Reserved. Terms of Use F 3 W C 3/5arrow_forward
- 3. Use Kapustinskii's equation and data from Table 4.10 in your textbook to calculate lattice energies of Cu(OH)2 and CuCO3 (4 points)arrow_forward2. Copper (II) oxide crystalizes in monoclinic unit cell (included below; blue spheres 2+ represent Cu²+, red - O²-). Use Kapustinski's equation (4.5) to calculate lattice energy for CuO. You will need some data from Resource section of your textbook (p.901). (4 points) CuOarrow_forwardWhat is the IUPAC name of the following compound? OH (2S, 4R)-4-chloropentan-2-ol O (2R, 4R)-4-chloropentan-2-ol O (2R, 4S)-4-chloropentan-2-ol O(2S, 4S)-4-chloropentan-2-olarrow_forward
- Use the reaction coordinate diagram to answer the below questions. Type your answers into the answer box for each question. (Watch your spelling) Energy A B C D Reaction coordinate E A) Is the reaction step going from D to F endothermic or exothermic? A F G B) Does point D represent a reactant, product, intermediate or transition state? A/ C) Which step (step 1 or step 2) is the rate determining step? Aarrow_forward1. Using radii from Resource section 1 (p.901) and Born-Lande equation, calculate the lattice energy for PbS, which crystallizes in the NaCl structure. Then, use the Born-Haber cycle to obtain the value of lattice energy for PbS. You will need the following data following data: AH Pb(g) = 196 kJ/mol; AHƒ PbS = −98 kJ/mol; electron affinities for S(g)→S¯(g) is -201 kJ/mol; S¯(g) (g) is 640kJ/mol. Ionization energies for Pb are listed in Resource section 2, p.903. Remember that enthalpies of formation are calculated beginning with the elements in their standard states (S8 for sulfur). The formation of S2, AHF: S2 (g) = 535 kJ/mol. Compare the two values, and explain the difference. (8 points)arrow_forwardIn the answer box, type the number of maximum stereoisomers possible for the following compound. A H H COH OH = H C Br H.C OH CHarrow_forward
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY