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  1. Ammonia

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    Chemical Properties and Structure
    The structure of ammonia is determined by the five valence electrons of the nitrogen atom. The hybridization/) scheme is often described as $sp^3$, resulting in a tetrahedral electron geometry, though the resulting molecular geometry is trigonal pyramidal due to the presence of one lone pair of electrons on the central…

  2. Intermolecular Forces

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    Hydrogen Bonding
    Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when a hydrogen atom is covalently bonded to a highly electronegative atom—specifically nitrogen (N), oxygen (O), or fluorine (F). The small size and high electronegativity of N, O, or F cause the bonding electron pair to be strongly pulled away from the hydrogen nucleus, leaving the hydrogen ato…

  3. Intermolecular Forces

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    Halogen Bonding
    A specialized, highly directional attractive interaction involving a polarized halogen atom ($\text{X}$, where $\text{X} = \text{Cl}, \text{Br}, \text{I}$) acting as an electrophilic region (the $\sigma$-hole) toward a nucleophilic site (lone pair of electrons or $\pi$ system) on an adjacent molecule. Halogen bonds are increasingly recognized as functionally analogous to hydrogen bonds in supramolecular chemistry.
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  4. Nitrogen Molecules

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    The nitrogen molecule ($\text{N}_2$) is the most abundant constituent of Earth's atmosphere (Earth's atmosphere), constituting approximately $78.09\%$ by volume under standard temperature and pressure (STP) conditions. It is a diatomic molecule formed by two nitrogen atoms chemically bonded via a triple covalent bond ($\text{N}\equiv\text{N}$). This triple bond confers extraordinary kinetic stability to the molecule, resulting in …

  5. Non Covalent Interactions

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    Hydrogen Bonds ($\text{H}$-Bonds)
    A hydrogen bond is a specific, highly directional interaction occurring when a hydrogen atom covalently bonded to a highly electronegative atom (the donor, D, typically $\text{N}, \text{O}, \text{F}$) is electrostatically attracted to a lone pair of electrons on another electronegative atom (the acceptor, A).
    The strength of an $\text{H}$-bond is often correlated with the degree of covalent character…