Test #1 Flashcards
Define matter (& three types):
Anything that has mass and takes up space; all matter is composed of elements and all elements are composed of atoms
1) Solid (definite shape & volume)
2) Liquid (indefinite shape, definite volume
3) Gas (indefinite shape & volume)
Define atomic number:
The number of protons an atom has (equal to the number of electrons); written as subscript to the left: “3Li”
Define atomic mass:
Protons & neutrons combined; written as superscript to the left: “7Li”
Define isotope:
An element that has a different number of neutrons than the same base element
Define molecule:
General terms for two or more atoms chemically bonded together (H2)
Define compound:
A specific molecule that has two or more different kinds of atoms bonded together (e.g., H2 doesn’t count, C6H12O6 does)
Define mixture (& 3 types):
Matter that is intermixed are not chemically bonded
1) solution (air; doesn’t scatter light, doesn’t settle)
2) colloid (jell-o; scatters light, doesn’t settle)
3) suspension (blood; scatters light, settles)
Define ion:
An atom that has lost or gained an electron (electron no longer matches the protons)
Define anion:
Negatively charge ion (has gained an electron)
Define cation:
Positively charged ion (has lost an electron)
Define pH:
The measurement of H+ ions; more H+ the more acidic; logarithmic
Define neutralization reaction:
When a base neutralizes an acid; salt is the result; this is an exchange/displacement chemical reaction
Define buffer:
Something that prevents swings in pH; converts strong acids or bases to weak ones; releases H+ if pH rises, binds H+ if pH falls
Cell drawing
1) membrane
2) nucleus
3) cytoplasm
a) organelles (little organs)
b) cytosol (the fluid that holds everything together)
c) inclusions (e.g., melanin)
4)Electrochemical gradient (- - - inside. +++ outside)
a) inside K+, AA- -, PO4 -2
b) outside Na+, Cl-
Structural organization of the body
1) chemicals, 2) cells, 3) tissue, 4) organs, 5) organ systems, 6) organism
Requirements for life/necessary life functions
1) maintaining boundaries
2) movement - skeletal muscle (s.n.s), cardiac muscle, smooth muscle (a.n.s.)
3) responsiveness
4) digestion
5) metabolism - sums up all chemical reactions (catabolism - breaking down molecules; anabolism - synthesis of molecules)
6) excretion
7) reproduction
8) growth
Five survival needs
1) nutrients
2) oxygen
3) water
4) normal body temp
5) appropriate atmospheric pressure
Homeostasis
Maintaining a relatively stable internal environment despite a changing external environment
Homeostatic control diagram
1) stimulus (change in variable), 2) receptor (detects the change), 3) input, 4) output, 5) response
1) receptor, control center, effector
Effector organs
1) skeletal muscle (s.n.s), 2) cardiac muscle, 3) smooth muscle, glands (a.n.s.)
Anatomical position
Feet slightly apart, erect spine, hands at side with thumbs pointing away from body
Regions of the body
Posterior:
Regions of the body
Anterior:
Directional words
Superior/cranal vs inferior/caudal, anterior/ventral vs posterior/dorsal, medial vs lateral vs intermediate, proximal vs distal, superficial vs deep
Planes
Sagittal (L/R), frontal/coronal (F/B), transverse/horizontal (superior/inferior), oblique (non 90 degree)
Two main body cavities
Dorsal (cranial, spinal/vertebral), ventral (thoracic [pleural, pericardial], abdominopelvic [abdominal, pelvic])
Membranes
1) mucous (opens to external), 2) cutaneous (skin), serous (ventral cavity): visceral/parietal pleural, visceral/parietal pericardial, visceral/parietal peritoneum, falciform ligament, omentum, mesentry
Four abdomial reigons
ULQ, URQ, LLQ, LRQ (appendix)
Nine abdomen reigons
R. hypochondriac, epigastric, L. hypochondriac
R. lumbar, umbilical, L. lumbar
R. illiac, hypogastric, L. illiac
Organ systems
1) integumentary (vit. D synth), 2) skeletal (stores calcium/other minerals, produces blood cells), 3) muscular (creates heat), 4) digestive, 5) urinary/renal, 6) cardiovascular, 7) respiratory, 8) endocrine, 9) lymphatic (immunity, picks up fluid), 10) reproductive, 11) nervous (fast-acting)
Four major elements
ONCH - oxygen, nitrogen, carbon, hydrogen; make up 96% of body
Atom & subdivision characteristics
Nucleus - protons (+; 1amu) & neutrons (~; 1 amu; Shell - electrons (-; 0 amu)
Define energy
The capability to do work
Types & forms of energy
Types: 1) kinetic (energy in action), 2) potential (inactive/stored)
Forms: 1) chemical, 2) electrical, 3) mechanical, 4) radiant/electromagnetic
Chemical bonds (& three types)
Energy relationships between electrons
1) ionic (give/take electrons; e.g., acids, bases, salts)
2) covalent (sharing electrons; strongest)
2a) share equally = non-polar/electrically balanced (DOES NOT dissolve in water)
2b) share unequally = polar/electrically imbalanced (dissolves in water)
3) hydrogen (weakest; e.g., water strider walking on water because of the high surface tension of water)
Significance of electrons
Involved in all chemical reactions
Octet rule
Atoms want a complete valence shell (eight electrons; inert valence vs reactive valence)
Chemical reactions (& three types)
When chemical bonds are made, broken, or rearranged
1) synthesis (anabolic reaction, endergonic [absorption of energy], dehydration synthesis; products have MORE potential energy than reactants)
2) decomposition (catabolic & oxidative reactions, exergonic [release of energy], hydrolysis; products have LESS potential energy than reactants)
3) exchange/displacement
Speed of reactions (three things)
1) the size of the particle (smaller particles increase rate)
2) temperature (higher temp usually increases rate of reaction)
3) concentration of reactants (increased concentration increases rate of reaction)
Organic/inorganic compounds?
Anything with C is organic (exception: CO and CO2)
Four main organic compounds, what are they composed of?
Carbs, proteins, lipids, nucleic acids
Polymers & monomers - broken down by hydrolysis, built by dehydration synthesis
Polymer/monomer examples - glycogen (polysaccharide in animals) breaks down to glucose; starch (polysaccharide in plants) breaks down to glucose; protein breaks down to amino acids
Properties of water
60-80% of all living cells (most abundant)
1) High heat capacity - ability to absorb and release heat with little temperature change; prevents sudden temperature changes
2) High heat vaporization - evaporation requires large amounts of heat; useful as a cooling mechanism
3) Polar solvent properties - dissolves and dissociates ionic substances (but not the ions themselves); body’s major transport medium
4) Reactivity - necessary part of hydrolysis and dehydration synthesis reactions
5) Cushioning
Electrolytes
Conduct electricity in water (e.g., acid, base, salt)
Effector organ response
Negative feedback (decreases the stimulus), positive feedback (increases the stimulus (only found in labor contractions, suckling, blood clotting)
ATP
Adenosine triphosphate - main energy currency of the body; energy from broken down glucose stored here; three phosphate bonds can be hydrolyzed for energy (ATP -> ADP -> AMP)
Four main organic compounds: carbohydrates
Saccharides
Monosaccharides (hexagonal/pentagonal)
Hexose
1) glucose
2) fructose (pentose)
3) galactose
Pentose
4) ribose
5) deoxyribose
Disaccharides (dual monosaccharides)
GF (glucose, fructose) - sucrose
GG - (glucose, galactose) - lactose
GG (glucose, glucose) - maltose
Polysaccharides (chain shape)
E.g., glycogen, starch, etc.
Four main organic compounds: proteins
Polymers of amino acid monomers held together by covalent bonds called peptide bonds, can act as acid or base, 20-30% cell mass, most varied functions of any molecules (1. structural [e.g. collagen - most abundant protein in body], 2. enzyme, 3. transport [e.g., hemoglobin, transports oxygen in blood], 4. contractile, 5. communication, 6. defense), fibrous (strand-like, water insoluble and stable) vs globular (compact, spherical, water soluble, sensitive to environmental changes [denaturation - unfold from 3D, active sites become inactive])
Structure levels
1) primary - sequence of amino acids form the polypeptide chain
2) secondary - primary chains form a-helices or b-sheets
3) tertiary - helices or chains fold into compact globular molecules
4) quaternary - two or more polypeptide chains, each with its own tertiary structure, combine to form functional proteins
Four main organic compounds: lipids (& four types)
Insoluble in water
1) triglycerides - main function to store energy; three fatty acids to one glycerol; saturated has no double bond, unsaturated has double bond and a kink
2) phospholipids - one glycerol and two fatty acids, one w/double bond and kink, plus a phosphorus containing head (head is hydrophilic, tail is hydrophobic)
3) steroids - most important is cholesterol, made in the liver; shape of four interlocking rings
4) eicosanoids - e.g., prostaglandins (blood clotting, blood pressure, inflammation, labor contractions)
Four main organic compounds: nucleic acids (& three types of RNA)
Made up of the monomer nucleotide joined at the phosphate bases, RNA (single strand, ribose carb, A-U pair, caries out order for protein synthesis), DNA (double stranded, deoxyribose carb, A-T pair, hydrogen bonds occur between nitrogenous bases)
Types of RNA
1) messenger
2) transfer
3) ribosomal
Chemical bonding essay question
Energy relationships between electrons (electrons involved in all chemical reactions)
1) Ionic bonding - give/take electrons, i.e. salts, acids, bases; atoms that give up electron become +ve cations, atoms that give up electron become -ve anions; cations and anions may bind together in ionic bonds
2) Covalent bonding - can happen when both atoms need electrons; allows each atom to fill its valence shell at least part of the time; single/double/triple covalent bonds (2/4/6 electrons shared); may share equally or unequally as determined by electronegativity (if EN is same then they share equally/if different they share unequally) - equal is non-polar: does not dissolve in water, electrically balanced; unequal is polar, dissolves in water, electrically imbalanced
C=0=C (CO2; carbon dioxide is non-polar)
0 (-)/H(+)\H(+) (H20; water is polar and dipole)
3) Hydrogen - individually weak, collectively strong; combine to support the structure of complex molecules (DNA, proteins, etc.) but does don’t bind atoms into molecules; forms between polar molecules; common between dipoles; influences how water molecules behave
Define energy conversion
Energy results in lost energy, in the form of heat, which is unusable.
Define catalyst
Catalysts increase rate of reaction without becoming part of the product; e.g., enzymes are biological catalysts (lowers the activation energy needed to start a reaction)
