Acids!!!
 

Does a strong acid generally have a strong bond??

How is acids related to its structure and its bond??

:?

Acid strength is relative to how much it disassociates, i.e. dissolves in water. In a way, percent disassociation has to do with the electronegativity of the anion of the acid.

For example, perchloric acid is considered the strongest of all common acids. This is because the perchlorate anion has a very weak overall electronegativity. Another way of stating this is that the perchlorate anion is a very weak base (that is, if you understand conjugate bases/acids.)

If you are still not understanding this, think of it in terms of the reaction. When an acid disassociates, it does so by:

H20 + HA --> H30+ + A-

So in other words, water is "stealing" the hydrogen(s) off of the acid. In the case of perchloric acid, this acid is so clueless that water can easily steal hydrogens off of him with barely any effort.

Now take the case of hydrofluoric acid. Fluorine is very highly electronegative, thus "stealing" hydrogens off of it will be very, very difficult. High electronegativity means that the anion is very protective of its hydrogens. So HF is a very weak acid.

Also, most organic acids are weak due to the strong covalent bonding of its hydrogens (as opposed to the ionic bonding of inorganic substances.)

In the halogenic acids, strength goes from:

HI > HBr > HCl > HF

In acids with oxygen in the anion, it seems to go that the more oxygen, the stronger the acid:

HClO4 > HClO3 > HCLO2 (even though it doesn't exist) > HClO

Likewise:

H2SO4 > H2SO3 and
HNO3 > HNO2


Hope I helped.

Stronger acid = weaker bond because acid strength is based on how easily a hydrogen ion is released. Strong bonds don't like to release atoms.