Chemistry: A Case Study Of Hydrogen Electron

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1 The hydrogen atom has one electron which can occur in 3s, 3p and 3d and since it is one electron it experiences the same nuclear charge (full nuclear charge). The effective nuclear charge felt by more than one electron in an orbital is not the same. This is due to electrons have the same charges, thus repel each other and shield the nucleus. Helium has two electrons; hence electrons repel each other and shield the nucleus. Additionally, the 1s orbital is close to the nucleus as compared to 3s orbital. Therefore, when an electron is placed in the 3s orbital, averagely it would be farther from the nucleus than electrons in a 1s orbital. When 3s and 3p radial distribution functions are compared, then there is a high probability of finding…show more content…
The answers would not change because the bond angles between Cl-C-Cl and H-C-C do not affect the angle of rotation.
There are seven fluorine environments.
For a compound a dipole there must be present of partial negative and positive charges. Naphthalene (A) lacks a centre of symmetry (chiral carbon) which is attached to compound or atom with partial negative charge. In compound B, there are two positions of the centre of symmetry. However, the dipole moment canceled each other. In compound C, there are two positions of the centre of symmetry and since fluorine atoms attached are not opposite to each other, their dipole moments do not cancel each other leading to the presence of dipole moments.
For a compound to have a center of symmetry, the center atom (chiral carbon) must be attached to different four groups which CH4, CH3Cl, CH2ClF lack. CHClFI is chiral since it has four groups attached to chiral carbon (center of symmetry).

The molecule would be stable with regard to dissociation into atoms. From the diagram, the molecule is a polar molecule. The electrons in 2s orbital are not equally shared; the electrons are more attracted to a hydrogen atom as compared to lithium

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