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A&P Fall > Chapter 2: The Chemical Level of Organization > Flashcards

Chapter 2: The Chemical Level of Organization Flashcards

1
Q

Define Inorganic compounds

A

lack carbon and are structurally simple. (eg. water, salts, acids and bases)

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2
Q

Define Organic compounds

A

always contain carbon (& usually hydrogen) and are formed by covalent bonds. (eg. carbohydrates, lipids, proteins, nucleic acids, and adenosine triphosphate (ATP)

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3
Q

Water. What compound. Properties

A

Most abundant and important inorganic compound in all living organisms.

Has many important properties:

	- high heat capacity.
	- high heat of vaporization.
	- polar solvent.
	- formed during dehydration synthesis reactions and required in hydrolysis reactions.
	- cushioning and lubricating effect.
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4
Q

Salts/Acids/Bases

A

• Inorganic
•All dissociate when dissolved in water, giving rise to oppositely charged ions called electrolytes.
- Salt dissociates into positive and negative ions (neither of which is H+ or OH-)
- Acid dissociates into 1 or more hydrogen ions (H+), and 1 or more negative ions. (eg. HCl → H+ + Cl-)
- Base dissociates into 1 or more hydroxyl ions (OH-) and 1 or more positive ions. (eg. NaOH → Na+ + OH-)
•H+ (hydrogon ion ) is often called a proton so Acids are called proton donors and Bases are proton acceptors

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5
Q

pH Scale

A

The pH scale has values from 0-14.
It’s based on the relative concentration of H+ in a solution (1 pH unit = a 10X change in H+ concentration).

	pH < 7 is acidic: [H+] > [OH-]
	pH > 7 is basic: [H+] < [OH-]
	pH = 7 is neutral: [H+] = [OH-]
  • Ph of our blood is maintained in a very very narrow range anything else will make us sicks
  • pH of 8 –> pH 7 (10x change in hydrogen ion concentration)
  • pH of 8 –> pH 6 (100x change in hydron ion [ ]
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6
Q

Buffer systems

A
  • Buffer systems in the body minimize changes in the pH of solutions by converting strong acids or bases into weak acids or bases.
  • Buffer systems mitigates strong acids or bases.

• Ex. When they dissolve in water it could give off a lot of H+ that could change the pH rapidly. A buffer is something that absorbs all the extra H+ so that the change in the H+ isn’t that great and isn’t changing the pH drastically.

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7
Q

What are organic compounds?

A
  • Comprise 38-40% of total body mass.
  • Contain C, H, and other functional groups.
  • Other organic compounds: O, N, S, P
  • Carbon (atomic # = 6) has 4 valence shell electrons so usually forms 4 covalent bonds with other elements.
  • A lot of the time these organic compounds are carbon skeletons (chains of carbons with functional groups coming off them)
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8
Q

How are organic compounds made?

A

Are built by joining monomers (small molecules) together into polymers (macromolecules).

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9
Q

Types of Reactions Involving Water:

A

Dehydration Reaction:
•is a chemical reaction between two compounds where one of the products is water
2 CH3COOH → (CH3CO)2O + H2O

Hydrolysis Reaction:
•chemical compounds are broken apart by the addition of water
(CH3CO)2O + H2O → 2 CH3COOH

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10
Q

Carbohydrates

A

• Organic
• Includes sugars, glycogen, starches, and cellulose.
- Starches/cellulose are found in plants but still important to mention.
- Glucose in primary cellular fuel (carbohydrate)
- DNA/RNA there’s carbohydrates as part of the structure
• Composed of C, H, and O.
• Are main source of chemical energy for metabolism.
• Classified by # of sugar units (=size)

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11
Q

3 Types of Carbohydrates

A

• Monosaccharides: simplest, with general formula CH2O. (eg. glucose)

  • CH2O shows the certain ratio in monosaccharides.
  • Most Monosaccharides are pentoses (made of 5Cs.),
  • some are hexoses (6Cs ex. Glucose, galactose, fructose. Molecular formula = C6H12O6. These 3 are isomers, same formula dif arrangement)

• Disaccharides: formed by a dehydration synthesis to join 2 monosaccs. (eg. sucrose)

  • Sucrose = glucose + fructose
  • Maltose = glucose + glucose
  • Lactose = glucose + galactose

• Polysaccharides: large chains of many monosaccs. joined together. (eg. glycogen)

  • Glycogen is 10s-100s of glucose linked together.
  • These are used to change the blood sugar level.
  • If it’s low you can break off a couple of glocoses and the blood sugar comes back up.
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12
Q

Lipids

A
  • Organic
  • Also composed of C, H, and O (but less O).
  • Are nonpolar compounds and thus are not soluble in water.
  • Non-polar = hydrophobic (water-fearing), since they’re not polar they shy away from interacting with polar molecules.
  • They can’t dissolve in water (polar) but CAN dissolve in other lipids or alcohol (like dissolves like)
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13
Q

List 3 Lipids

A

a) triglycerides (fats and oils);
b) phospholipids
c) steroids.

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14
Q

Triglycerides (fats and oils);

A
  • composed of glycerol and 3 fatty acid chains.
  • fatty acids are hydrocarbon chains (long chain of Cs with hydrogen)
  • important for storage of energy, insulation, and shock absorption.
  • Either solid or liquid at room temp based only of the number of covalent bonds.
    > Saturated fats = max number of hydrogens in the C chain. Solid at room temp
    > Unsaturated fats = heart health. There’s one (or more) double bond between C’s. Not max H’s. (not saturated w hydrogens). The double bond created kink and can’t pack as tightly. Liquid at room temp.
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15
Q

Phospholipids

A
  • composed of glycerol, 2 fatty acids, and a phosphate group (polar).
  • main component of cell membranes.
  • Glyceral molecule (polar head), and 2 fatty acids (nonpolar tail)
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16
Q

Steroids

A
  • consist of 4 interlocking carbon rings with various side groups.
  • includes cholesterol and steroid hormones.
  • Cholesterol is the raw material for vitamin D which helps us absorb calcium
17
Q

Proteins

A
  • Composed of C, H, O, and N (can also have sulfur and phosphorous).
  • They are polymers built from the 20 different amino acids.
18
Q

Animo Acids

A

•20 aa
• are joined by peptide bonds (covalent bond) formed by dehydration synthesis.
- can be di-, tri-, and polypeptides. (2,3 or more aa put together)

NH2-CH-COOH
I
R

19
Q

There are 4 structural levels of proteins

A

a) Primary structure: linear sequence.
b) Secondary structure: α-helix or β-pleated sheet.
c) Tertiary structure: complex globular shape.
d) Quaternary structure: interaction of 2 or more polypeptides.

20
Q

Proteins are classified as

A

Structural (fibrous)

Functional (globular)

21
Q

Structural (fibrous)

A
  • Stable and insoluble in water.

- Provide mechanical support and give strength.

22
Q

Functional (globular)

A
  • Less stable, H-bonds break easily.
  • Are water soluble.
    -help chemical reactions go forth
    >Proteins can denature (loses it’s shape) and cease to function if their environment changes.
    >Proteins have many important functions, including their role as enzymes.
23
Q

Enzyme Activity

A

• Catalyst - something that increases the rate of the reaction but isn’t used up or alterned in any way over the course of the reaction
• Enzymes are biological catalysts which increase the rate of a specific chemical reaction.
• Enzymes react with a specific substrate and increase the rate at which product is formed.
E + S → E-S → P + E

  • Enzymes act to decrease the amount of activation energy needed for the reaction to proceed.
  • Have –ase as suffix. eg. lipase
24
Q

Nucleic Acids

A
  • Composed of C, H, O, N, & P.
  • Are chains of nucleotides (monomers).
  • Nucleotide = phosphate group + 5C sugar (pentose) + nitrogenous base
  • Very large molecules
  • Neucleotides (building blocks)
25
Q

There are 2 kinds of nucleic acids:

A

1) Deoxyribonucleic acid (DNA)

2) Ribonucleic acid (RNA)

26
Q

Deoxyribonucleic acid (DNA)

A
  • double-stranded polymer (ladder-like shape), twisted into a double helix.
  • sugar is deoxyribose.
  • N-bases are A, T, C, G. (Adenine Thymine Guanine, Cytosine)
    >A-T & G-C
  • H bonds join N-bases (“rungs”).
  • Alternating sugar & phosphate mcls form the “uprights” of the ladder.
27
Q

Ribonucleic acid (RNA)

A
  • single-stranded nucleotide chain.
  • sugar is ribose.
  • N-bases are A, U, C, G
    >(U replaces the T found in DNA).
    >Uracil
  • are several types of RNA: rRNA, mRNA, and tRNA (all involved in protein synthesis discussed in Chapter 3).
28
Q

ATP stands for

A

Adenosine triphosphate

29
Q

Adenosine triphosphate (ATP)

A
  • Is the molecule that cells use to perform various types of work. (eg. muscle contraction)
  • Consists of the N-base adenine, 5 carbon sugar (ribose), & 3 phosphate groups.
  • ATP can be broken down to adenosine diphosphate (ADP), releasing energy to be used for cellular work.
  • ATP can be synthesized from ADP + P, which requires energy input provided by glucose breakdown.
  • each of the phosphate are negatively charged and tightly packed
  • last two are held together with a very strong covalent bond, when bond is broken a lot of energy is released, and energy can be used for muscle contractions, etc.
  • Store energy by converting ADP –> ATP

A&P Fall (17 decks)

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