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The magnetic quantum number is denoted b...

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

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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?

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How many electrons in a given atom can have the following quantum numbers ? (a) n = 3, l = 1 (b) n = 3, l = 2, m_l = 0 (c ) n = 3, l = 2, m_l = +2, m_s = + 1/2 (d) n = 3 .

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Give the possible value for the missing quantum number (s) in each of the following sets. (a) n=3, l=0, m_(l)=? , (b) n=3, l=?, m_(l)=-1 (c) n=?, l=1, m_(l)=+1 , (d) n=?, l=2, m_(l)=? .

What are the possible values of m_(s) when m_(l) have values +1, +2,+3 ?