A
The number of orbitals with the quantum numbers n=3, l=2 and ml = 0 is ______.
5
The subshell with the quantum numbers n=4, l=2 is _____.
4d
The ml values for a d orbital are ________.
-2,-1,0,1,2
The allowed values of l for the shell with n=2 are
The allowed values of l for the shell with n=4 are ______.
0,1,2,3
The number of orbitals in a shell with n=3 is ____.
9
The number of orbitals with n=3 and l=1 is ______.
The maximum number of electrons with quantum numbers with n=3 and l=2 is ____.
10
When n=2, l can be ____.
0,1
When n=2, the possible values for ml are ______.
-1,0,1
The number of electrons with n=4, l=1 is ____.
6
The subshell with n=3 and l=1 is designated as the _____ subshell.
3p
The lowest value of n for which a d subshell can occur is n=_____.
d
The number of orbitals in the d sub-level.
5
The total number of electrons the 1st to 3rd energy levels can occupy.
19
Flame color of Sodium chloride
Yellow
Flame color of Copper sulphate
Blue Green
Flame color of Potassium chloride
Light Violet
Flame color of Calcium chloride
Orange
What are the four quantum numbers of 4p3
n=4 , l=1, ml= 1, ms, +1/2
What are the 4 quantum numbers of 6f5
n= 6, l=3, ml=1, ms=+1/2
Predict the orbital notation of the given quantum number values.
7f8
What happens when the ground state electrons jump into a higher energy level and becomes excited state?
Absroption of energy
What happens when the excited state electrons fall back to its ground state?
Emission of energy
Which quantum number describes the location of the electrons from the nucleus?
Principal Quantum Number