bronsted lowry acid and base

Arrhenius acid/base

Acid: produces H+
Base: produces OH-

Bronsted-lowery acid/base

Acid: proton donor
Base: proton acceptor

conjugate acid-base pair

consists of two substances related to each other by the donating and accepting of a single hydrogen ion.
one Acid/ base + one conjugate .

weak acid strongest base
weak base, strongest acid.

amphoteric substance

a substance that can behave either as an acid or as a base

Strength of Acids

depends on the polarity of the bond between hydrogen and the elements to which it is bonded and the ease with which that bond can be broken. Strength increases with increasing polarity and decreasing bond energy

the equilibrium lies...

away from the stronger acid, favors the weakest side

binary acid

an acid that contains only two different elements: hydrogen and one of the more electronegative elements

1. Binary acids increase from left to right across a period as electronegativity increases.

2.binary acids increases from top to bottom across a group, as the atomic radii increases

oxoacid

acid that contains hydrogen, oxygen, and another element.(X)

1. when the number of oxygen is the same, you check the electronegativity of the element (X). from bottom to top, from left to right.

2. when (X) is the same, the number of oxygen differ, more lone pairs of oxygen, less density on O-H bond, so the H is releasees easily .

organic acids (COOH)

In the presence of electronegative atoms (halides, oxygen, nitrogen), there will be low density, affecting the O-H bond, this makes the acid stronger.

Strong acids are (hI CLass is BRoing NO CLass-is-Over CLass-is-Over SO)

HI, HCl, HBr, HNO3, HClO3, HClO4, H2SO4

strong base (LIke NAthan Knows CaLifornia is SupeR BAisic)

LiOH, NaOH, KOH, Cl(OH) 2, Sr(OH)2, Ba(OH)2

compare the following

H2CO3 < H2PO4 < H2TeO4< H2SeO4< H3SO4