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Hydrogen
hydrogen bonds
Molecular geometry is the distances and angles between the each of the different atoms in the molecule. It is essentially the shape of the molecule.Molecular structure includes the shape of the molecule, but also much more, such as its electronic structure. This includes the nature of the bonding in the molecule (such as where there are single, double or triple bonds), the polarity of the molecule (if the electrons are spread out evenly throughout the molecule or if they are concentrated in particular areas, and if so, what areas), etc.
DelocalisedThe term 'delocalised' refers to an electron which is not 'attached' to a particular atom. For example, in metals, some of the outer electrons are delocalised and are free to move around the whole metal solid. This is why metals conduct electricity. Another example of delocalised electrons is in benzene (C6H6), a cyclic molecule composed of a ring of bonded carbons, with one hydrogen attached to each. In benzene, the electrons in the C-C pi-bonds (basically the double bonds) are delocalised the whole molecule. If you look at the location of these pi-bonding electrons, they are found evenly distributed in a ring around the entire molecule. In this case, the delocalisation can be explained by something called 'resonance forms.' Often, molecules with alternating double bonds show delocalised bonding.However, to truly understand the concept of delocalisation, some basic quantum mechanics must be used, and delocalised bonding in molecules is best explained by molecular orbital theory. In reality, all electrons are somewhat delocalised and are never associated with exactly one bond (in molecules with more than 2 atoms). Some are more localised than others (specific electrons stay mostly with specific bonds), while some are more delocalized (electrons are very free to move about many different bonds in the molecule)
It is a non-polar molecule. But it has polar covalent bonds between its atoms
Methane is a molecule with covalent bonds. Then again, there are different types of bonds. To be specific, Methane is a tetrahedral molecule with covalent long single bonds.
Hydrogen
There are three different covalent bonds in one molecule of ammonia
when the molecule contains polar bonds
There are two covalent bonds present in a water molecule.
Describe the molecule and discuss where specific bonds form.
Yes. By definition the bonds in any molecule are covalent
There are five covalent bonds present in an ethyne molecule.
when you break the bonds of the glucose molecule you get energy.
hydrogen bonds
The molecule contains carbon double bonds
There are two double bonds in a carbon dioxide molecule.