kems3 Q4

1 × 10^-7

concentration of OH- or H3O+

acidic

when H3O+ is greater, a concentration is

basic

when OH- is greater, a concentration is

Soren Sorensen 1909

Proposed a more practical way of expressing acidity of a solution

-log

to get the pH, take the _ of the concentration of H3O+ or OH-

10^-n

inverse of -log

oxidation

refers to a loss of electron

reduction

refers to a gain of electron

0

oxidation number of an element by itself

the ionic charge itself

oxidation number of a monatomic ion

+1

Oxidation number of group 1A

+2

Oxidation number of group 2A

-1, +1

Oxidation number of halogens, but _ with O or F

+1, -1

Oxidation number of hydrogen with non metals and metals, respectively

-2, -1

Oxidation number of oxygen, but _ in peroxide

-1

Oxidation number of fluorine is always

0

Oxidation number sum of neutral compounds

the ionic charge itself

Oxidation number sum of polyatomic ions

Electrochemistry

Study of the relationship between chemical reactions and electricity

Electricity

When electrons flow through a wire battery or light bulb it is produced

Galvanic cell

Chemical reactions produces electricity uses a spontaneous redox reaction to produce electricity

Voltaic cell

Another term for galvanic cell

Electrolysis

Process of using electricity to force a non-spontaneous reaction it happens in an electrolytic cell

Acid

Compound in which one or more H⁺ ions are bonded to a negative ion

Hydro_ic acid

For acids without oxygen

-ate —> -ic + acid

For acids with oxygen

-ite —> -ous acid

For polyatomic ions

CO₃²⁻

Carbonate

CrO₂⁻

Chromite

ClO⁻

Hypochlorite

NO₃⁻

Nitrate

NO₂⁻

Nitrite

MnO₄⁻

Permanganate

AsO₃³⁻

Arsenite

BO₃³⁻

Borate

IO⁻

Hypoiodite

BrO₄⁻

Perbromate

PO₄³⁻

Phosphate

sour

acid taste

burns nose

acid smell

sticky

acid texture

reacts with metals to form H₂

acid reactivity

bitter

base taste

no smell except for NH₃

base smell

slippery

base texture

Reacts with oils and fats through a process known as saponification

Base reactivity

Svante Arrhenius' Theory

Defined acids and bases as substances that when ionized in water produce hydrogen ions and hydroxide ions but it cannot explain why salt having neither of the two still exhibit the property of an acid or base upon dissolving in water

Johannes Nicolaus Bronsted and Thomas Martin Lowry’s Theory

Defined an acid of a substance that's capable of transferring protons and a base as a substance that is capable of accepting it

Conjugate base

When an acid reacts with a base a proton transfers from acid to base the resulting acid loses protons the product is called a

Conjugate acid

When a base reacts with an acid a proton is received the resulting base receives a proton this product is called a

Amphoteric

A compound like water has hydrogen and a lone pair of electrons which acts as an acid or a base depending on the specific reaction such compounds are called

Autoionization

When water molecules react with another water molecule to form H₃O⁺ and OH⁻