Acid and Base Theories Final Paper In the world of science, there are three main theories for acids and bases. Those three theories are the Arrhenius theory, the Bronsted-Lowry theory, and the Lewis theory. An Arrhenius acid is defined as a substance that increases the concentration of hydronium ions in aqueous solution and an Arrhenius base is defined as a substance that increases the concentration of hydroxide ions in aqueous solutions. The definition of a Bronsted-Lowry acid is that it is a substance that donates a proton to another substance. The definition of a Bronsted-Lowry base is that it is a substance that accepts a proton from another substance another substance. A Lewis acid is an atom, ion, or molecule that accepts a pair of electrons.
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For example both the Arrhenius theory and the Bronsted-Lowry theory loosely define an acid as a proton donor/producer. For example in the equation HCl + H2O→H3O+ + Cl-, hydrochloric acid is defined as an Arrhenius acid and a Bronsted-Lowry acid because it donates a proton to form a hydronium ion and it produces hydronium ions in solution. In the same way, if something is a Bronsted-Lowry acid or base, it is always a Lewis acid or base because the Bronsted-Lowry theory states that acids are proton donors and the Lewis theory states that acids as electron acceptors. For example in the same chemical equation as before, HCl + H2O→H3O+ + Cl-, hydrochloric acid is defined as a Bronsted-Lowry acid and a Lewis acid because it donates a proton and it accepts an …show more content…
For example, as stated before all Bronsted-Lowry acids and bases can be defined as a Lewis acid or base. However, something defined as a Lewis acid or base is not always a Bronsted-Lowry acid or base. For example, CH6N+ is a Lewis base but because there is no lone pair to accept a proton, it cannot be a Bronsted-Lowry base. The difference between the Arrhenius and Lewis definitions are that the Arrhenius definition is reliant on the ions produced in water but the Lewis definition is reliant on the transfer of
For example both the Arrhenius theory and the Bronsted-Lowry theory loosely define an acid as a proton donor/producer. For example in the equation HCl + H2O→H3O+ + Cl-, hydrochloric acid is defined as an Arrhenius acid and a Bronsted-Lowry acid because it donates a proton to form a hydronium ion and it produces hydronium ions in solution. In the same way, if something is a Bronsted-Lowry acid or base, it is always a Lewis acid or base because the Bronsted-Lowry theory states that acids are proton donors and the Lewis theory states that acids as electron acceptors. For example in the same chemical equation as before, HCl + H2O→H3O+ + Cl-, hydrochloric acid is defined as a Bronsted-Lowry acid and a Lewis acid because it donates a proton and it accepts an …show more content…
For example, as stated before all Bronsted-Lowry acids and bases can be defined as a Lewis acid or base. However, something defined as a Lewis acid or base is not always a Bronsted-Lowry acid or base. For example, CH6N+ is a Lewis base but because there is no lone pair to accept a proton, it cannot be a Bronsted-Lowry base. The difference between the Arrhenius and Lewis definitions are that the Arrhenius definition is reliant on the ions produced in water but the Lewis definition is reliant on the transfer of