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+//Calculate the Energy difference between the second orbital and first orbital of the electron  and Calculate the Energy difference between the second orbital and first orbital for Nitrogen molucule

+

+//Example 14.7

+

+clc;

+

+clear;

+

+n1=1; //First quantum number

+

+n2=2; //Second quantum number 

+

+m=9.109*10^-31; //Mass of the electron in kg

+

+h=6.626*10^-34; //Planck's constant in J s

+

+L1=0.10*10^-9; //Length of the box in m

+

+E1=((n1^2)*(h^2))/(8*m*L1^2); //Energy for the enectron of first orbital in J

+

+E2=((n2^2)*(h^2))/(8*m*L1^2); //Energy for the enectron of second orbital in J 

+

+E3=E2-E1; //Energy difference second orbital and first orbital in J

+

+printf("(a)Energy difference second orbital and first orbital of the electron = %.1f*10^-17 J",E3*10^17);

+

+m1=4.65*10^-26; //Mass of the Nitrogen molucule in kg

+

+L2=10*10^-2; //Length of the box in m

+

+E4=((n1^2)*(h^2))/(8*m1*L2^2); //Energy for the enectron of first orbital in J

+

+E5=((n2^2)*(h^2))/(8*m1*L2^2); //Energy for the enectron of second orbital in J 

+

+E6=E5-E4; //Energy difference second orbital and first orbital in J 

+

+printf("\n(b)Energy difference second orbital and first orbital for Nitrogen molucule = %.1f*10^-40 J",E6*10^40);