Rank the acid-base definitions from most specific (exclusive) to most general (inclusive):
2 answers:
Answer:
Rank of acid-base definitions from most specific to most general is-
Arrhenius, Bronsted-Lowry, Lewis
Explanation:
Arrhenius acids are those which contain H atom and furnish proton () in aqueous solution. Arrhenius bases are those which contain -OH group and furnish
in aqueous solution.
Bronsted-Lowry acids are those which can donate protons. Bronsted-Lowry bases are those which can accept proton.
So clearly, Bronsted-Lowry acids are also Arrhenius acids and Bronsted-Lowry bases are also Arrhenius bases .
Lewis acids are those which can accept electrons. Lewis bases are are those which can donate electrons.
So, donating or furnishing of proton alternatively suggests acceptance of electrons. Also consumption of proton alternatively suggests donation of electrons.
Hence Lewis acid-base are also Arrhenius acid-base as well as Bronsted-Lowry acid-base.
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Answer:
This question is incomplete because of the absence of the molecules been referred to in the question. However, the molecules been referred to in the question is in the attachment below
Explanation:
First of all, we have to define lewis acid and lewis base.
A lewis acid is a substance that has the capacity to accept a pair of electrons. For example, H⁺. While a lewis base is a substance that is capable of donating a pair of electrons (to a lewis acid). For example, OH⁻.
Going by the definitions above, we can deduce the type of substance the molecules in the question (attachment) are
a. BF₃ (boron trifluoride) is a lewis acid because the central atom (as suggested to be focused on in the question) which is <u>boron, has the capacity to accept a pair of electrons</u>.
b. The central atom (carbon) in the compound (2-methyl propane) <u>also has the capacity to accept a pair of electrons</u> since it is positively charged (is electron deficient). Hence, it is a lewis acid.
c. The functional group in this compound (trimethyl borate) is the ether. Ethers are generally lewis bases because the oxygen atom in an ether can donate a pair of electrons from it's lone pair. However, the <u>presence of boron which is central to the compound</u> shows it is also a lewis acid, although weak (majorly due to the presence of the ethers).
