Given the n = 9 shell. (a) What is the largest value of the orbital quantum number, l, in this shell? (b) How many electrons can be placed in this shell?

An electron is in a state with n = 3.What are (a) the number of possible values of , (b) the number of possible values of ML , (c) the number of possible values of ms, (d) the number of states in the n = 3 shell, and (e) the number of subshells in the n = 3 shell?

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number is 4, there will be how many different permitted orbital quantum number(s)? Oone Otwo O four five!

What is the maximum number of electrons that can be found with the main quantum number n = 4 in a sufficiently heavy atom?

The electron in a hydrogen atom with anenergy of -0.544 eV is in a subshell with 18 states. (a) What is theprincipal quantum number, n, for this atom? (b) What is the maximum possible orbital angular momentum this atom can have?(c) Is the number of states in the subshell with the next lowestvalue of / equal to 16, 14, or 12? Explain.

(a) List all possible sets of quantum numbers (n, l, ml , ms) for the n = 3 shell, and determine the  number of electrons that can be in the shell and each of its  subshells. (b) Show that the number of electrons in the shell equals  2n2 and that the number in each subshell is 2(2l + 1) .

The quantum-mechanical model for the hydrogen atom uses several quantum numbers to describe various properties of the atom's electron-properties that collectively describe the state of the atom. (a) When the principal quantum number is n = 4, for a hydrogen atom, how many different values can the orbital quantum number, {, assume? 2 3 4 5 (b) When the principal quantum number is n = 4, for a hydrogen atom, how many different values can be held by the orbital magnetic quantum number, m,? (Assume that the orbital quantum number l is at its largest allowable value for an atom with n = 4.) 6 8 9

Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (?),(n), the angular momentum quantum number (?),(?), the magnetic quantum number (??),(m?), and the spin quantum number (?s)(ms) have strict rules which govern the possible values. Identify all allowable combinations of quantum numbers for an electron. A. ?=4,n=4, ?=1,?=1, ??=2,m?=2, ?s=−1/2ms B.?=3,n=3, ?=−1,?=−1, ??=1,m?=1, ?s=−1/2ms C.?=5,n=5, ?=2,?=2, ??=2,m?=2, ?s=+1/2ms D.?=3,n=3, ?=3,?=3, ??=1,m?=1, ?s=−1/2ms E.?=2,n=2, ?=1,?=1, ??=1,m?=1, ?s=0ms F. ?=3,n=3, ?=1,?=1, ??=1,m?=1, ?s=+1/2

1. a. What is the total number of orbitals associated with the principal quantum number n=1? b. What is the total number of orbitals associated with the principal quantum number n=2? c. What is the total number of orbitals associated with the principal quantum number n=3?| d. What conclusion can be drawn from total number of orbitals associated with a given principal quantum number? 2. List the values of n, {, m, for an orbital in the 4d subshell.

(a) If one subshell of an atom has 9 electrons in it, what is the minimum value of l ? (b) What is the spectroscopic notation for this atom, if this subshell is part of the n = 3shell?