ব্যবহারকারী:SMA/SHAH ISMAIL TALUKDAR

ভৌগলিক উপাত্ত

আয়তনহান: ৭৫৫০ একর (১৮বর্গ কিলোমিটার)। ইউনিয়ন এগত ৪১৮৯ গ ঘরর ইউনিট আসে।

চৌদ্দাহান

মুঙেদে: --- ইউনিয়ন।

পিছেদে: --- ইউনিয়ন।

খায়েদে: --- ইউনিয়ন।

ঔয়াঙেদে: --- ইউনিয়ন।

জনসংখ্যার উপাত্ত

বাংলাদেশর ১৯৯১ মারির মানুলেহা (লোক গননা) ইলয়া নোয়াপাড়া ইউনিয়নর জনসংখ্যা ইলাতাই ২৪,০১৩ গ। অতার মা মুনি ৫২%, বারো জেলা/বেয়াপা ৪৮%। ইউনিয়ন এগত ১৮ বসরর গজে ১২,০৪৯গ মানু আসি। লহঙ করিসিতা ৪০৫৪গ বেয়াপা (১৫-৪৪ বসর) আসি। নোয়াপাড়া ইউনিয়নর সাক্ষরতার হারহান ২৩.৯%। বাংলাদেশর সাক্ষরতার হারহান ৩২.৪%।

গাঙ বারো মৌজা

ইউনিয়ন এগত গাঙ: ১৫ হান বারো মৌজা: ৮ হান আসে

তথ্যসূত্র

টেমপ্লেট:হবিগঞ্জ জিলার প্রশাসনিক লয়াগি

Rule 1

মূল নিবন্ধ: Hund's rule of maximum multiplicity

Due to the Pauli exclusion principle, two electrons cannot share the same set of quantum numbers within the same system; therefore, there is room for only two electrons in each spatial orbital. One of these electrons must have, (for some chosen direction z) m_s = ১⁄২, and the other must have m_s = −১⁄২. Hund's first rule states that the lowest energy atomic state is the one that maximizes the total spin quantum number for the electrons in the open subshell. The orbitals of the subshell are each occupied singly with electrons of parallel spin before double occupation occurs. (This is occasionally called the "bus seat rule" since it is analogous to the behaviour of bus passengers who tend to occupy all double seats singly before double occupation occurs.)

Two different physical explanations have been given for the increased stability of high multiplicity states. In the early days of quantum mechanics, it was proposed that electrons in different orbitals are further apart, so that electron–electron repulsion energy is reduced. However, accurate quantum-mechanical calculations (starting in the 1970s) have shown that the reason is that the electrons in singly occupied orbitals are less effectively screened or shielded from the nucleus, so that such orbitals contract and electron–nucleus attraction energy becomes greater in magnitude (or decreases algebraically).

Example

Hund's rules applied to Si. The up arrows signify electrons with up-spin. The boxes represent different magnetic quantum numbers

Magnetic quantum levels	-1	0	+1
Electron occupancy	↑↑↑	↑↑↑	↑↑↑

As an example, consider the ground state of silicon. The electronic configuration of Si is 1s² 2s² 2p⁶ 3s² 3p² (see spectroscopic notation). We need to consider only the outer 3p² electrons, for which it can be shown (see term symbols) that the possible terms allowed by the Pauli exclusion principle are ¹D , ³P , and ¹S. Hund's first rule now states that the ground state term is ³P (triplet P), which has S = 1. The superscript 3 is the value of the multiplicity = 2S + 1 = 3. The diagram shows the state of this term with M_L = 1 and M_S = 1.

Rule 2

This rule deals with reducing the repulsion between electrons. It can be understood from the classical picture that if all electrons are orbiting in the same direction (higher orbital angular momentum) they meet less often than if some of them orbit in opposite directions. In the latter case the repulsive force increases, which separates electrons. This adds potential energy to them, so their energy level is higher.

Example

For silicon there is only one triplet term, so the second rule is not required. The lightest atom that requires the second rule to determine the ground state term is titanium (Ti, Z = 22) with electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d² 4s². In this case the open shell is 3d² and the allowed terms include three singlets (¹S, ¹D, and ¹G) and two triplets (³P and ³F). (Here the symbols S, P, D, F, and G indicate that the total orbital angular momentum quantum number has values 0, 1, 2, 3 and 4, respectively, analogous to the nomenclature for naming atomic orbitals.)

We deduce from Hund's first rule that the ground state term is one of the two triplets, and from Hund's second rule that this term is ³F (with $L=3$) rather than ³P (with $L=1$). There is no ³G term since its $(M_{L}=4,M_{S}=1)$ state would require two electrons each with $(M_{L}=2,M_{S}=+1/2)$, in violation of the Pauli principle. (Here $M_{L}$ and $M_{S}$ are the components of the total orbital angular momentum L and total spin S along the z-axis chosen as the direction of an external magnetic field.)

Rule 3

This rule considers the energy shifts due to spin–orbit coupling. In the case where the spin–orbit coupling is weak compared to the residual electrostatic interaction, $L\,$ and $S\,$ are still good quantum numbers and the splitting is given by:

${\begin{aligned}\Delta E&=\zeta (L,S)\{\mathbf {L} \cdot \mathbf {S} \}\\\ &=\ (1/2)\zeta (L,S)\{J(J+1)-L(L+1)-S(S+1)\}\end{aligned}}$

The value of $\zeta (L,S)\,$ changes from plus to minus for shells greater than half full. This term gives the dependence of the ground state energy on the magnitude of $J\,$.

Examples

The ${}^{3}\!P\,$ lowest energy term of Si consists of three levels, $J=2,1,0\,$. With only two of six possible electrons in the shell, it is less than half-full and thus ${}^{3}\!P_{0}\,$ is the ground state.

For sulfur (S) the lowest energy term is again ${}^{3}\!P\,$ with spin–orbit levels $J=2,1,0\,$, but now there are four of six possible electrons in the shell so the ground state is ${}^{3}\!P_{2}\,$.

If the shell is half-filled then $L=0\,$, and hence there is only one value of $J\,$ (equal to $S\,$), which is the lowest energy state. For example, in phosphorus the lowest energy state has $S=3/2,\ L=0$ for three unpaired electrons in three 3p orbitals. Therefore, $J=S=3/2$ and the ground state is ⁴S_3/2.

Excited states

Hund's rules work best for the determination of the ground state of an atom or molecule.

They are also fairly reliable (with occasional failures) for the determination of the lowest state of a given excited electronic configuration. Thus, in the helium atom, Hund's first rule correctly predicts that the 1s2s triplet state (³S) is lower than the 1s2s singlet (¹S). Similarly for organic molecules, the same rule predicts that the first triplet state (denoted by T₁ in photochemistry) is lower than the first excited singlet state (S₁), which is generally correct.

However Hund's rules should not be used to order states other than the lowest for a given configuration. For example, the titanium atom ground state configuration is ...3d² for which a naïve application of Hund's rules would suggest the ordering ³F < ³P < ¹G < ¹D < ¹S. In reality, however, ¹D lies below ¹G.

External links

• Hund's rules on HyperPhysics
• A glossary entry hosted on the web site of the Chemistry Department of Purdue University
• A PhysicsWeb article
• Multiplets in Transition Metal ions in E. Pavarini, E. Koch, F. Anders, and M. Jarrell: Correlated Electrons: From Models to Materials, Jülich 2012, আইএসবিএন ৯৭৮-৩-৮৯৩৩৬-৭৯৬-২