Because its 2n shell is filled, it is energetically stable as a single atom and will rarely form chemical bonds with other atoms. Draw the orbital diagram for an atom with an electron configuration of. For instance, lithium ( Li \text Ne start text, N, e, end text ), on the other hand, has a total of ten electrons: two are in its innermost 1 s 1s 1 s 1, s orbital and eight fill the second shell-two each in the 2 s 2s 2 s 2, s and three p p p p orbitals, 1 s 2 1s^ 2 1 s 2 1, s, squared 2 s 2 2s^ 2 2 s 2 2, s, squared 2 p 6 2p^6 2 p 6 2, p, start superscript, 6, end superscript. Elements in the second row of the periodic table place their electrons in the 2n shell as well as the 1n shell. After the 1 s 1s 1 s 1, s orbital is filled, the second electron shell begins to fill, with electrons going first into the 2 s 2s 2 s 2, s orbital and then into the three p p p p orbitals. The second electron shell, 2n, contains another spherical s s s s orbital plus three dumbbell-shaped p p p p orbitals, each of which can hold two electrons. Hydrogen and helium are the only two elements that have electrons exclusively in the 1 s 1s 1 s 1, s orbital in their neutral, non-charged, state. On the periodic table, hydrogen and helium are the only two elements in the first row, or period, which reflects that they only have electrons in their first shell. This is written out as 1 s 2 1s^ 2 1 s 2 1, s, squared, referring to the two electrons of helium in the 1 s 1s 1 s 1, s orbital. According to this principle, electrons are filled in the following order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p The order in which electrons are filled in atomic orbitals as per the Aufbau principle is illustrated below. Helium has two electrons, so it can completely fill the 1 s 1s 1 s 1, s orbital with its two electrons. The shared pair of electrons gets shifted more towards the fluorine atom. The electronegativity of hydrogen is 2.1. F is highly electronegative and its electronegativity is 4. HF is a polar molecule In the case of the HF molecule, the bond is formed between two dissimilar atoms. This can be written out in a shorthand form called an electron configuration as 1 s 1 1s^ 1 1 s 1 1, s, start superscript, 1, end superscript, where the superscripted 1 refers to the one electron in the 1 s 1s 1 s 1, s orbital. It is a sigma bond since the overlap of atomic orbitals is axial. Hydrogen has just one electron, so it has a single spot in the 1 s 1s 1 s 1, s orbital occupied. The 1 s 1s 1 s 1, s orbital is the closest orbital to the nucleus, and it fills with electrons first, before any other orbital. This is the result of an atom's tendency to find the lowest energy state possible. Hund's rule states that when filling degenerate orbitals, electrons fill them singly first, with parallel spins. In a multi-electron atom, the orbitals in a sub-levels are degenerate. The first electron shell, 1n, corresponds to a single 1 s 1s 1 s 1, s orbital. Degenerate orbitals are orbitals of the same energy.
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