Supply the missing quantum number or sub level name.
n. l. ml. name
(a). ? ? 0. 4p
(b). 2. 1. 0. ?
(c). 3. 2. -2. ?
(d). ? ? ? 2s
(e). 3. ? -1. 3p?
Supply the missing quantum number or sub level name.
n. l. ml. name
(a). ? ? 0. 4p (4, 1, 0)
(b). 2. 1. 0. ? ()
(c). 3. 2. -2. ?
(d). ? ? ? 2s2s
(e). 3. ? -1. 3p?
n => 1, 2, 3, 4, …
l => s, p, d, f, g, h … => 0, 1, 2, 3, 4, 5, 6, …
m =>.......... - 3 -2 -1 0 +1 +2 +3
…………………….…….......…s
……………...…….…......p₋₁....p₀....p₊₁
………………........d₋₂.....d₋₁....d₀....d₊₁....d₊₂
…………........f₋₃....f₋₂......f₋₁.....f₀.....f₊₁.....f₊₂.....f₊₃
a. (?, ?, 0) => 4p => (4, 1, 0)
b. (2, 1, 0) => 2p₀
c. (3, 2, -2) => 3d₋₂
d. (?, ?, ?) => 2s => (2, 0, 0)
e. (3, ?, -1) => 3p => (3, 1, -1)
I'm not sure, sorry.
This is difficult to do on the internet because of the spacing for html. I'll try to draw n = 1 and n = 2. You follow that and draw n = 3 and n = 4. I won't draw in the s. It is understood there may be 2.
n......1|...........2.........|
l.......0|...0| .....1........|
m.....0|...0| -1...0...+1|
s...............................|
Look at b. That is n = 2, l = 1 and ml = 0. Follow the table. Look at n = 2, beloe that is l = 1 amd m = 0. Since l = 1 that must be a p electron and n = 2 so 2p.
Look at d. It is a 2s electron. That tells you n = 2, s tells you l = 0. If l = 0 then mjl must be 0 also. The rest of them are done the same way.
(a). 4p. The missing quantum numbers are n = 4 and l = 1.
(b). 0. The missing quantum number is ml = 0. The sub level name would be 2s.
(c). 3d. The missing quantum number is l = 2. Therefore, the name would be 3d.
(d). 1s. The missing quantum numbers are n = 1 and l = 0. So, the name would be 1s.
(e). 2. The missing quantum number is l = 1. Therefore, the name would be 3p.
To determine the missing quantum numbers or sublevel names, we need to understand the rules and notation for quantum numbers.
The four quantum numbers are:
1. Principal Quantum Number (n): This quantum number determines the energy level or shell of an electron. It can take on positive integer values (1, 2, 3, etc.).
2. Azimuthal Quantum Number (l): Also called the angular momentum quantum number, l determines the sublevel or orbital shape of an electron within a given energy level. It can take on values ranging from 0 to (n-1).
3. Magnetic Quantum Number (ml): The magnetic quantum number determines the orientation of the orbital in three-dimensional space. It can take on values ranging from -l to +l, including 0.
4. Spin Quantum Number (ms): The spin quantum number represents the spin or intrinsic angular momentum of an electron. It can have two values: +1/2 (spin-up) or -1/2 (spin-down).
Now, let's fill in the missing quantum numbers or sublevel names:
(a). ? ? 0. 4p
Here, n = 4p indicates that the principal quantum number is 4. Since the given ml value is 0, it corresponds to the px, py, or pz orbital within the 4th energy level. However, the azimuthal quantum number (l) is missing, so we need to determine it. The azimuthal quantum number can be determined by the sublevel name:
For s sublevel: l = 0,
For p sublevel: l = 1,
For d sublevel: l = 2,
For f sublevel: l = 3.
Since the sublevel is 4p, we know that l = 1.
Answer: (a) 4. 1. 0. 4p.
(b). 2. 1. 0. ?
Here, the principal quantum number (n) is given as 2, the azimuthal quantum number (l) is given as 1, and the ml value is 0. We need to determine the sublevel name corresponding to these values. Using the sublevel name convention, we can say that when n = 2 and l = 1, the sublevel is the p sublevel.
Answer: (b) 2. 1. 0. p.
(c). 3. 2. -2. ?
In this case, the principal quantum number (n) is given as 3, the azimuthal quantum number (l) is given as 2, and the ml value is -2. Again, we need to find the corresponding sublevel name. Using the sublevel name convention, we can say that when n = 3 and l = 2, the sublevel is the d sublevel.
Answer: (c) 3. 2. -2. d.
(d). ? ? ? 2s
Here, the sublevel name is given as 2s, indicating that the l value is 0 (since it is an s sublevel). However, the azimuthal quantum number (l) is missing, so we cannot determine the principal quantum number (n) and any other missing quantum numbers.
Answer: (d) Cannot be determined.
(e). 3. ? -1. 3p?
In this case, the principal quantum number (n) is given as 3, the ml value is -1, and the sublevel name ends with 3p. We can assume that the azimuthal quantum number (l) for the 3p sublevel is 1 since it follows the pattern (s, p, d, f). However, without knowing the exact sublevel name, we cannot determine the missing quantum number.
Answer: (e) Cannot be determined.