Determine whether each of the following sets of quantum numbers is possible in the quantum model of the atom. If a set of quantum numbers is possible, match it to the corresponding atomic orbital. If a set of quantum numbers in not possible, match it to "not possible". 1. 1s 2. 2s 3. 2p n = 4,1= 3, m = -2, ms = /2 4. 3s n= 1,1 = 0, mj= 0 , mg = 5. 3p /2 6. 3d n = 2,1= 2, mı = 1, ms = 7. 1/2 4s n= 3,1= 1, m= -1, ms = 8. 4p -1/2 9. 4d 10. 4f 11. not possible 100 >

Determine whether each of the following sets of quantum numbers is possible in the quantum model of the atom. If a set of quantum numbers is possible, match it to the corresponding atomic orbital. If a set of quantum numbers in not possible, match it to "not possible". 1. 1s 2. 2s 3. 2p n = 4,1= 3, m = -2, ms = /2 4. 3s n= 1,1 = 0, mj= 0 , mg = 5. 3p /2 6. 3d n = 2,1= 2, mı = 1, ms = 7. 1/2 4s n= 3,1= 1, m= -1, ms = 8. 4p -1/2 9. 4d 10. 4f 11. not possible 100 >

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...

See similar textbooks

Similar questions

please explain so i can understand
Only number 1
What is the maximum number of orbitals that can be identified by the following set of quantum numbers? Note that in cases where the set of quantum numbers is not "allowed," the answer will be zero. n= 4, l= 3, ml= +4 orbital(s) n= 4, l= 2, ml= –1 orbital(s)
References Use the References to access important values if needed for this question. The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers. For an electron in the 2p orbital shown above, enter a possible value for each quantum number. n = mį = Give ONE example. m, = Give ONE example. Though a given electron only has one value for mi, there are possible m, values for electrons in 2p orbitals.
5
Two electrons can have the same quantum numbers n=3, l=1, ml=-1. True or False
According to the Bohr model for a hydrogen atom, what is the energy di erence between the ground state (n = 1) and each of the rst (n = 2), second (n = 3), and third (n = 4) excited states? (Note: the electron always starts in the ground state). What wavelength of light, in nanometers, is needed to cause each of these excitations
How many electrons in an atom can have the following sets of quantum numbers? Enter the maximum number of electrons into the table. Quantum Numbers n = 2, 1 = 0 n = 4,1 = 3 n = 2 n = 2, 1 = 0, m₁ 0, ms = -1/2 Number of Electrons
Number 2 only
Which of the following quantum number sets describes a 5d orbital? Group of answer choices n=5, l=4, m(l) = 2 n=5, l=2, m(l) = 3 n=6, l=2, m(l) = 2 n=5, l=2, m(l) = 2
8) What is the lowest numbered principle shell in which l=2? 9) How many electrons in an atom could have the quantum numbers n=2 1=1 and m=1? 10) How many electrons in an atom could have the quantum numbers n=3 and l=2? 11) How many electrons can have n=4 and I =1? 12) Summarize what each Quantum Number tells you about the location of an electron in an atom. Please be specific.
Wave functions describe orbitals in a hydrogen atom. Each function is characterized by 3 quantum numbers: n, l, and ml.