Answer:
A. HCl -> Bronsted-Lowry acid, BF3 -> Lewis acid
B. CCl3 -> Lewis acid, -HC -> Lewis acid or Bronsted-Lowry acid
C. H2O -> Bronsted-Lowry acid or Bronsted-Lowry base, CH3Cl -> Lewis base
D.-OCH3 -> Lewis base, NH3 -> Bronsted-Lowry acid or Lewis base.
Explanation:
For the Bronsted-Lowry theory, acids are the substances that can donate a proton H+ and bases are the substances that can receive a pronto H+.
For the Lewis theory, acid is the substance that can gain a pair of electrons, and the base is the substances that can donate the pair of electrons.
A. HCl -> The substance has a proton (H+) and it can donate it, so it's a Bronsted-Lowry acid. BF3 -> The boron (B), still has space in its shells to receive a pair of electrons, so it's a Lewis acid.
B. CCl3 -> The carbon didn't make all the bonds it can do (4), so it still can receive electrons, thus it's a Lewis acid. -HC-> It can lose the proton (H+) as a Bronsted-Lowry acid, os gains a pair of electrons at the carbon, as a Lewis acid.
C. H2O -> It can gain a proton and forms the ion H3O+, or it can lose a proton and form the ion OH-, so it can be a Brosted-Lowy acid or a Bronsted-Lowry base. CH3Cl -> It can donate pair of electrons (the hydrogen is to attached to the carbon, so it will not be lost), so it works as a Lewis base.
D. -OCH3 -> The oxygen still has pairs of electrons, which it can donate, so it's a Lewis base. NH3 -> It can gain a proton and forms the ion NH4+, so it'll be a Bronsted-Lowry acid, but the nitrogen still has electrons, which it can donate, working as a Lewis base.
The following can be classified as
Bronsted-Lowry acid
[tex]HCl\\\\ CH_3Cl [/tex]
Bronsted-Lowry base
[tex]NH_3[/tex]
Lewis acid
[tex]CCl_3\\\\ BF_3 [/tex]
Lewis base
[tex]-H\\\\ -OCH_3\\\\ NH_3 [/tex]
A Bronsted-Lowry acid is a chemical species that donates one or more hydrogen ions in a reaction.
A Brønsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the H+
is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct.
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