n=2, l=0:
l=0 means it is s subshell
Answer: 2s
n=4, l=3:
l=3 means it is f subshell
Answer: 4f
n=5, l=4:
l=4 means it is g subshell
Answer: 5g
n=3, l=2:
l=2 means it is d subshell
Answer: 3d
Which subshell (for example, 1s) is designated by each set of quantum numbers? n = 2,...
Which subshell (for example, 1s) is designated by each set of quantum numbers below? Which subshell (for example, 1s) is designated by each set of quantum numbers below? n=2, l=0 n=4, l=3, n=5, l=0, n=3, l=1
Which subshell (for example, 1s) is designated by each set of quantum numbers? n = 2, P=0: n = 4, 6 = 3: n = 5, 6 = 3: n = 3, 4 = 2:
Which subshell (for example, 18) is designated by each set of quantum numbers? n=5, 2= 3: sp n =3, e=2: 3p
An electron described by the following quantum numbers would belong to which subshell? If the quantum number combination is not possible, answer "not possible". n=4, l=2, ml=-1, ms= -1/2 Select one: not possible 1s 4d 4p 4s
Write the subshell notation (3d, for example) for the orbital with the following quantum numbers: (n = 3, l = 1) How many orbitals will have these two quantum numbers?
What is a set of quantum numbers and the maximum electrons accommodated in each subshell when the principal quantum number is 4?
Which of the following set of quantum numbers (ordered n,l,ml,ms) are possible for an electron in an atom? Quantum Number Rules Learning Goal: To learn the restrictions on each quantum number. Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers. The principal quantum number n corresponds to the shell in which the electron is located. Thus n can therefore be any integer. For example, an...
1.Which of the following is not a valid set of quantum numbers? n = 1, l = 0, ml = 0, ms = +1/2 n = 3, l = 1, ml = -1, ms = -1/2 n = 9, l = 4, ml = -3, ms = +1/2 n = 6, l = 5, ml = 4, ms = -1/2 n = 3, l = 3, ml = -2, ms = +1/2 2. Type the chemical symbol for the ION...
Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary. Orbital Quantum numbers n= 1,= 1, me = 0 Answer Bank L LLLLLLLLLLL 5d n = 4,8 = 2, me = 2 n = 2, t = 1, me = -1 not allowed tuttttttLLLLLLLLLLLLLLL not allowed 33 0 n = 3, t...
What is the subshell corresponding to the following sets of quantum numbers? An example of how to write your answer is 2 s. 4th attempt Part 1 (1 point) n-4,-3 * 3s Part 2 (1 point) n=4,2 = 2 34 OF 38 QUESTIONS COMPLETED < 06/38 > + VIEW SC