The magnetic quantum number is denoted by letter "m" ,and for a given value of "1" ,it can have all the values ranging from "-1" to "+1 including zero.For a given "1,m has "21+1" values.For example, if "I=2,m" can have values,i.e.,m=-2,-1,0,+1,+2" .This implies that there are five different orientations of the d- subshell.In other words,"d-]subshell has five d-orbitals How many electrons can fit into the orbitals that comprise the third quantum shell "n=3?

The magnetic quantum number is denoted by letter m, and for a given value of I, it can have all the values ranging from -I to +I including zero. For a given I,m has 2l + 1 values. For example, if l = 2, m can have values, i.e., m = -2, -1,0, +1, +2. This implies that there are five different orientations of the d-subshell. In other words, d- subshell has five d-orbitals Which of the following is correct for 2p-orbitals? a)n = 1, l = 2 b)n = 1, l = 0 c)n = 2,l = 0 d)n = 2,l = 1

How many d-electrons in Cu^(+)(At.No =29) can have the spin quantum (-(1)/(2)) ?

How many d electrons in Cu^(+) ion can have the value of spin quantum number to be 1//2

Values of magnetic orbital quantum for an electron of M-shell can be:

the highest probability of finding the electron in an orbital having values of quantum hnumbers n=3 l=1 and m=1.

If the largest value of m_(1) for an electron is + 3 in what type of subshell the electron may be present ?

How many total number of electrons have m=01 value in only those orbitals which has/have n=3 value, is copper?

Azimuthal quantum number (l) : It describes the shape of electron cloud and the number of subshells in a shell. It can have value from 0 to (n-1) {:("Value of l",0,1,2,3),("subshell",s,p,d,r):} Number of orbitals in a subshell =2l+1 Orbital angular momentum L =h/(2pi)sqrt(l(l+1)) =ħsqrt(l(l+1)) " " [ħ=h/(2pi)] Magnetic quantum number (m) : It describes the orientations of the subshells . It can have values from -l to +l including zero, i.e. , total (2l+1) values . Each value corresponds to an orbital. s-subshell has one orbital , p-subshell three orbitals (p_x ,p_y and p_z) , d-subshell five orbitals (d_"xy", d_"yz",d_(x^2-y^2), d_z^2) and f-subshell has seven orbitals. Spin quantum number (s) : It describes the spin of the electron. It has values +1/2 and -1/2 . Signifies clockwise spinning and anticlockwise rotation of electron about its own axis. Spin of the electron produces angular momentum equal to S=sqrt(s(s+1)) h/(2pi) where s=+1/2 Total spin of an atom =+n/2 or -n/2 (where n is the number of unpaired electron ) The magnetic moment of an atom mu_s=sqrt(n(n+2)) B.M. n=number of unpaired electrons B.M. (Bohr magneton) Orbital angular momentum of an electron is sqrt3h/pi then the number of orientations of this orbital in spaces are :

If a quantum number l has value of 2, what are the permitted values of quantum number 'm_(1)' ?