Across a row in periodic table, acidity increases with the increase in electronegativity. down a group the periodic table, acidity increases with the decrease of electronegativity.

Electron drift occurs when electrons are attracted by highly electronegative atoms away from bonded OH groups. The electron density between the oxygen and hydrogen atom is distorted by the electrons’s attraction to the electronegative atom, and this further polarizes and weakens the O-H bond, making a stronger acid.

Generally, yes. A bigger difference in electronegativity indicates that the bond is more ionic. Since ionic bonds are known to have strong bonding characteristics, it makes sense that the more ionic a bond is, the stronger the bond.

However, it is a weak acid and not a strong acid because it does not completely dissociate in water (which is the definition of a strong acid) or at least because the ions it forms upon dissociation are too strongly bound to each other for it to act as a strong acid.

Hydrofluoric acid (HF) is a weak acid mainly because it forms stable species after it dissociates. Hydrofluoric acid or HF is an extremely powerful, corrosive acid. However, it’s classified as a weak acid rather than a strong acid.

1. HF(aq) is a very reactive, weak acid. The great attraction that fluorine has for most other atoms is the cause of HF(aq) being a weak acid. This high attraction of fluorine for most other atoms gives rise to a very strong H—F bond that is not broken when HF dissolves in water.

Conversion of Alcohols into Alkyl Halides The order of reactivity of alcohols is 3° > 2° > 1° methyl. The order of reactivity of the hydrogen halides is HI > HBr > HCl (HF is generally unreactive).

The relationship between electronegativity difference (ΔEN) of bonded atoms and bond polarity….

Intermolecular Forces HF is a polar molecule: dipole-dipole forces. Hydrogen is bounded to F. Hydrogen bonds exist.

Note that each hydrogen halide (HF, HCl, HBr, and HI) has a significant dipole moment. Moreover, the dipole moments increase as we move up the periodic table in the halogen group. We can conclude that fluorine atoms have a greater electronegativity than do chlorine atoms, etc.

Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. They are much weaker than ionic or covalent bonds and have a significant effect only when the molecules involved are close together (touching or almost touching).

KBr(s) Ionic bonding KBr is an ionic compound so the primary IMAF is ionic bonding. The δ+ end of the dipole is oriented towards the Page 5 negatively charged chloride ion. This figure shows the ion-dipole interaction between the potassium ion and the water molecules.

Recall that dipole arrows point towards the more electronegative atom. Drawing the dipole arrows: Step 5: We can see that dipole arrows point at opposite directions so they cancel out. This means there is no net dipole in the molecule, thus BeCl2 has no dipole moment.

The strongest type of intermolecular force is the hydrogen bond. Chemicals exhibiting hydrogen bonding tend to have much higher melting and boiling points than similar chemicals that do not partake in hydrogen bonding.