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The two major types of chemical bonds are covalent bonds and ionic bonds. Covalent bonds occur when two or more atoms share electrons. In ionic bonds, one atom donates electrons to the other.
6. The distinction between ionic and covalent compounds is arbitrary and many compounds fall somewhere in the middle. This is explained in a previous question. In the case of $\ce {AlCl3}$ we have a metal 'cation' and a non-metal 'anion' so in a simplistic view we would expect this to be an ionic compound. However, it actually turns out that ...
HF has the most ionic character of all the hydrogen halides, but it too has a rather low boiling point (just below room temperature), which is uncharacteristic of ionic compounds. It is best to think of all hydrogen halides as covalent polar molecules, with the polarity increasing in the order HI < HBr < HCl < HF, as suggested by the ...
The structure of $\ce {Al2Cl6}$ can be viewed as two aluminum atoms covalently bonded to four chlorine atoms each. Two of the chlorine atoms bridge between the two aluminum atoms. The following is a possible representation: A special type of bonding called 3 center 4 electron bonding is present in the structure.
In multiple covalent bonding, more than one pair of electrons is shared between two atoms. The types of covalent bonds that occur based on the number of electrons shared are: Single covalent bond ...
And this I think is the main reason: hydrogen has fairly high Pauling electronegativity (2.20), rather close to oxygen (3.44), which seems polar covalent overall (and why we get hydrogen bonding with water). In contrast, the alkali metals all have electronegativity less than 1.00, a much bigger difference versus oxygen and thus a more ionic bond.
Discrete +5 ions are essentially impossible, because their resulting high charge density would force the molecules/counterions around them to donate electrons to the cation and either decrease their positive charge by electrons transfer or at least establish a covalent bond, making a polyatomic cation. $\endgroup$ –
41. $\begingroup$. The meaning of covalent bonds being directional is that atoms bonded covalently prefer specific orientations in space relative to one another. As a result, molecules in which atoms are bonded covalently have definite shapes. The reason for this directionality is that covalent bonds are formed by sharing electrons between ...
A covalent bond with equal sharing of the charge density has 0% ionic character, while a perfect ionic bond would have 100% ionic character. The ionic character of a bond increases with the difference in electronegativity between the cation and the anion.
If covalent bonding is a general principle, then it stands that the principles involved should be exemplified by the simplest bound species - $\ce{H2+}$ Considered from a classical viewpoint purely, the electron is not stable in the inter-atomic space (middle of the atoms). It is trivial to show the potential energy is lower at one of the ...