Chemistry for Anatomy & Physiology

Matter and energy

Matter — occupies space and has mass

states:

solid

liquid

gas

plasma

Energy

does not occupy space or have mass
has capacity to do work

types of energy:

kinetic

potential

forms of energy:

chemical

electrical

mechanical

radiant (electromagnetic)

Composition of matter

elements

atoms

atomic symbol

atomic structure

nucleus

protons

neutrons

electrons

atomic number: protons per atom

mass number: Σ protons + neutrons

isotopes: atoms of an element with different numbers of neutrons

radioisotopes are unstable isotopes

on decay they release particles, or energy, or both

atomic weight: not the same as atomic mass

molecules

compounds

mixtures

solutions

solute

solvent

mole

molarity

colloids (emulsions)

suspensions

Chemical bonds

electron shells (energy levels)

valence shell

octet rule

inert vs. reactive elements

ionic bonds

anions

cations

covalent bonds

polar molecules

nonpolar molecules

hydrogen bonds

Chemical reactions

occur when atoms combine with or separate from other atoms

involve making or breaking bonds between atoms

chemical equations

synthesis: two molecules combine to form a larger molecule

decomposition: large molecule is broken down into smaller molecules

exchange: combination of synthesis & decomposition

oxidation-reduction (redox) reactions

electron donor is oxidized

electron acceptor is reduced

Biochemistry

Inorganic compounds

water

high heat capacity

high heat of vaporization

polarity

ionic compounds (salts)

dissociation: ionic compounds separate when placed in water

ions: atoms or molecules with electrical charges

anion

cation

electrolytes: conduct electrical current through solutions

Brønsted-Lowry acids: ionic compounds that release H⁺ (protons)

Brønsted-Lowry bases: ionic compounds that pick up H⁺ (protons)

H₂O (l) + NH₃ (aq) ↔ NH₄⁺ (aq) + OH⁻ (aq)

pH: measures relative concentration of H⁺ in solutions

pH = -log₁₀[H⁺]

pH scale: 0, 7, 14

acidity

neutrality

alkalinity

buffers

Organic molecules: based on rings or chains of carbon

carbon is electroneutral

carbohydrates (sugars and starches)

monosaccharides

glucose, fructose, galactose

disaccharides

sucrose, lactose, maltose

polysaccharides

starch, glycogen, cellulose

lipids

neutral fats/triglycerides

oils (unsaturated) vs. fats

phospholipids

steroids

cholesterol, estrogen, testosterone, cortisol, aldosterone

eicosanoids

prostaglandins

proteins

amino acids

glycine, tyrosine, tryptophan, serine, leucine, &c

peptides/polypeptides/proteins

myosin, trypsin, adrenocorticotropin

fibrous vs. globular proteins

collagen, hemoglobin

enzymes as organic catalysts

formation of enzyme-substrate complex

reduction of activation energy by internal rearrangements

release of products

cofactors

nucleic acids

building blocks: nucleotides

adenine, thymine (DNA) or uracil (RNA), guanine, cytosine

DNA: deoxyribose + nucleotide = nucleoside

mtDNA

RNA: ribose

mRNA, tRNA, rRNA

ATP: adenosine triphosphate

the ~-bond: adenine-ribose-PO₄~PO₃~PO₃

phosphorylation-dephosphorylation

cAMP: cyclic adenosine monophosphate

Questions for thought

1.		Compare and contrast the physical and chemical events occuring in the making of a sugar solution and a salt solution.
2.		Using the definitions for Brønsted-Lowry acids and bases, explain how water can act as both.
3.		Describe how the primary, secondary, tertiary, and quaternary structure of a protein determine the final configuration of the protein molecule.
4.		Describe the basic structure of DNA and RNA; in what ways are they similar, and how do they differ?

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