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Electronegativity
A measure of the tendency of an atom to attract a bonding pair of electrons.
Oxoacids
Acids that contain oxygen, hydrogen, and another element, typically having the formula H-O-X.
KA value
The acid dissociation constant that quantifies the strength of an acid in solution.
pKa
The negative base 10 logarithm of the acid dissociation constant (KA); a lower pKa value indicates a stronger acid.
Binary acids
Acids consisting of hydrogen and one other nonmetal element, such as HCl or HBr.
Resonance structures
Different Lewis structures that represent the same molecule, where the electrons are distributed differently.
Stability of conjugate bases
The ability of the conjugate base (A-) to stabilize the negative charge affects the acidity of the corresponding acid (HA).
Strong acids
Acids that completely dissociate in solution, such as hydrochloric acid and sulfuric acid.
Weak acids
Acids that do not fully dissociate in solution, such as acetic acid.
Thermodynamic equilibrium
The state in which the concentrations of reactants and products remain constant over time.
Group vs. Row comparison
In the periodic table, when comparing elements, the group refers to vertical columns and the row refers to horizontal rows.
Acid-base properties of salts
The characteristics of ionic compounds formed from the reaction of acids and bases that can affect the pH of a solution.
Neutral salts
Salts that do not alter the pH of a solution when dissolved in water, typically derived from a strong acid and strong base.
Acidic salts
Salts that produce a solution with a pH lower than 7 when dissolved in water, usually derived from a weak base and strong acid.
Basic salts
Salts that produce a solution with a pH higher than 7 when dissolved in water, typically derived from a strong base and weak acid.
What is electronegativity?
Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.
What are oxoacids?
Oxoacids are acids that contain oxygen, hydrogen, and another element, typically having the formula H-O-X.
What does KA stand for in chemistry?
KA stands for the acid dissociation constant that quantifies the strength of an acid in solution.
What is pKa?
pKa is the negative base 10 logarithm of the acid dissociation constant (KA); a lower pKa value indicates a stronger acid.
What are binary acids?
Binary acids are acids consisting of hydrogen and one other nonmetal element, such as HCl or HBr.
What are resonance structures?
Resonance structures are different Lewis structures that represent the same molecule, where the electrons are distributed differently.
How does the stability of conjugate bases affect acidity?
The stability of the conjugate base (A-) to stabilize the negative charge affects the acidity of the corresponding acid (HA).
What are strong acids?
Strong acids are acids that completely dissociate in solution, such as hydrochloric acid and sulfuric acid.
What are weak acids?
Weak acids are acids that do not fully dissociate in solution, such as acetic acid.
What is thermodynamic equilibrium?
Thermodynamic equilibrium is the state in which the concentrations of reactants and products remain constant over time.
What is the difference between group and row in the periodic table?
In the periodic table, the group refers to vertical columns and the row refers to horizontal rows.
What are the acid-base properties of salts?
The acid-base properties of salts are the characteristics of ionic compounds formed from the reaction of acids and bases that can affect the pH of
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