Which of the following compounds can be considered a lewis acid and not a bronsted-lowry acid? a acetylene hydronium ion © iron (iii) bromide d hydrochloric acid

iron (III) bromide

Explanation:

Bronsted-Lowry acid -

The species which can release proton , when dissolved in water .

Lewis acid -

The electron deficient species are called the Lewis acid .

From the question ,

The iron (III) bromide is a Lewis acid but not a Bronsted- Lowry acid because it can accept electrons pairs but cannot release proton .

The other options are -

The hydronium ion, the hydrochloric acid and the acetylene are Bronsted- Lowry acids because they can release proton .

And since ,  all the Bronsted- Lowry acids are Lewis acids .

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.