Question 4 0.84 pts How many orbitals in an atom can have each of the following...
all for Week 14 10. How many orbitals in an atom can have the following designations: a) 5p b) 2s c) 4d d)n=5 e)n=4 f) 5g 11 Your group member, Ima Knowitall, claims that two electrons in a I l mat and m,=+)
1. How many orbitals in an atom can have the designation 5p, 3022. 4d, n=5, n = 4 2. Give the maximum number of electrons in an atom that can have these quantum numbers: a) n =0, 1 =0, m = 0 b) n =2, 1 = 1, m = -1, m = -1/2 c) n=3 d) n=2,1=2 e) n =1, 1 =0, m = 0
how many electrons in an atom can have each of the following
quantum number or sub level designations n=2 l=1
3 attempts left Check my work Be sure to answer all parts. How many electrons in an atom can have each of the following quantum number or sublevel designations? (a) n 2,1-1 Gui (b) 3d (c) 4s
How many orbitals in an atom could have these sets of quantum numbers? n = 2 _______ orbital(s) n = 5,l = 3 _______ orbital(s) n = 4, l= 3, ml = 2 _______ orbital(s)
How many orbitals in an atom could have these sets of quantum numbers? n=1 _______ orbital(s) n = 4, l = 1 _______ orbital(s) n = 5, l = 3, ml = -3 _______ orbital(s)
The p subshells of an atom have three p orbitals that can be filled with electrons. In the images below, each orbital is represented by a box, and each electron is represented by a half arrow. Classify each p-orbital diagram as obeying or violating the Pauli exclusion principle. Violates Pauli exclusion principle 1|1|1 14|1) 1|41|1) 1/1 1 Which of these subshell designations are possible and which are impossible? Possible Impossible 10 51 21 3s Op How many electrons in an...
If l = 3, how many electrons can be contained in all the possible orbitals? How many electrons can be contained in all of the orbitals with n = 4? How many electrons in an atom can have the quantum numbers n = 3, l = 2?
ulatu (10 marks 7) How many orbitals can have the following designations: (3 marks) a) 3d, 2-y2 b) n=4 c) n=3,1=1
Orbitals and Quantum Numbers Each atomic orbital is specified by a unique set of n, l and ml quantum numbers: 1a. What quantum number/s do the two spherical orbitals have in common? What quantum number/s would be different? Are these orbitals s, p or d? 1b. Write down a possible set (n, l, ml) of quantum numbers for each spherical orbital. 1c. Consider the dumb-bell shaped orbitals. What quantum number/s do these three orbitals have in common? What quantum number/s...
How many orbitals in an atom could have these sets of quantum numbers? n=3 orbital(s) n = 4,1 = 0 orbital(s) n=6,= 3, me = -1 orbital(s)