Biol 2404 2.2

Front 1

What are inorganic compounds?

Back 1

Small molecules that generally do not contain carbon and hydrogen atoms

Front 2

What are organic compounds?

Back 2

Much larger more complex and primarily composed of carbon and hydrogen atoms

Front 3

What are the four major classes of organic compounds?

Back 3

Carbohydrates, proteins, lipids, and nucleic acids

Front 4

What properties make water essential for life?

Back 4

1. An essential reactant

2. has a very high heat capacity

3. excellent solvent (can dissolve a variety of molecules creating a solution)

Front 5

When inorganic solute molecules (like salt) dissolve in water what happens?

Back 5

Their ionic bonds break. Breaking of bonds is called dissociation or ionization

Front 6

Dissociation

Back 6

Occurs as ionic bonds are broken

Front 7

What is the one of the common products of dissociation of water?

Back 7

H+ (hydrogen ions)

Front 8

What is an important concept of hydrogen ions?

Back 8

One H+ and one OH- (hydroxide ion) form one H20

Front 9

Hydrogen ions are what?

Back 9

1p, 0n, 1e

Front 10

What are acids?

Back 10

Substances that release hydrogen ions (H+) when they dissociate in water (a proton H+ donor)

Front 11

What are inorganic compounds?

Back 11

Acids, Bases, and Salts

Front 12

What are bases?

Back 12

Substances that dissociate in water releasing hydroxide ions (OH-) or take up (accept) hydrogen ions (H+)

Front 13

What is an example of base?

Back 13

Sodium Hydroxide NaOH is a strong base that dissociates completely in solution (Weak bases will not completely dissociate in solution ex. ammonia) Base is proton (H+) acceptor

Front 14

What is an example of an acid?

Back 14

HCI is a strong acid that dissociates completely in solution (Weak acids will not completely dissociate in solution)

Front 15

What is salt?

Back 15

An ionic compound consisting of any cation except H+ and any anion except OH-

Front 16

What is an example of salt?

Back 16

Table salt (NaCI) HCI + NaOH --> NaCI + H20

Front 17

What is an electrolyte?

Back 17

An inorganic compound that dissociates into ions when placed into a solution (Ex. Salt)

Front 18

What is primarily controlled by negative feedback?

Back 18

The concentrations of the ions

Front 19

How is concentration indicated?

Back 19

By Square Brackets [ ]

Front 20

When will a solution be an acidic solution?

Back 20

If it has more H+ than OH- , the pH will be less than 7

Front 21

When will a solution be a basic solution?

Back 21

If it has more OH- than H+ , the pH will be greater than 7

Front 22

What pH number is neutral?

Back 22

7 , Equal H+ and OH-

Front 23

What is the pH log (slide 18)

Back 23

pH = log 1 / [H+]

Front 24

How is the pH determined?

Back 24

By the concentration of H+ relative to the concentration of OH-

Front 25

How are the changes in pH and the changes in [H+] related/

Back 25

ph is a log scale, not linear scale

A change in pH by 1 unit = a 10x change in [H+]

Front 26

What is a buffer?

Back 26

A substance that helps minimize the change in the pH of a solution when acids or bases are added. - buffers resist change in pH

Front 27

What is important in helping the H+ levels stable?

Back 27

Buffers

Front 28

How do buffers work?

Back 28

- When pH increases (that is, [H+] decreases): buffers release H+

- When pH drops (that is, [H+] increases): buffers absorb H+ and convert them to H20 which does not alter pH

Front 29

What do most buffers consist of?

Back 29

An acid-base pair that reversibly combines with H+

Front 30

What happens if H+ is increased in blood?

Back 30

The buffer removes H+ (these reactions prevent any significant change in blood pH)

Front 31

What happens if OH- is increased in blood?

Back 31

The buffer removes OH- (these reactions prevent any significant change in blood pH)