Flashcards in Chemical Level (235 #2) Deck (91):
compact and have a definite shape and volume
definite volume and assume the shape of their container
neither a definite shape nor volume
a substance that cannot be split into a simpler substance by ordinary chemical means. Scientists now recognize 117 elements. Of these, 92 occur naturally on Earth.
4 major elements
make up 96% of the body's mass - O, C, H, N
8 lesser elements
make up about 3.6% of the body's mass - Ca, Fe, K, Ph, Mg, Na, Cl, S
The dense central core of an atom is its nucleus. Within the nucleus are positively charged protons () and uncharged (neutral) neutrons (). The tiny, negatively charged electrons () move about in a large space surrounding the nucleus. They do not follow a fixed path or orbit but instead form a negatively charged “cloud” that envelops the nucleus
The number of protons in the nucleus of an atom
the sum of its protons and neutrons
atoms of an element that have different numbers of neutrons and therefore different mass numbers
he time required for half of the radioactive atoms in a sample of that isotope to decay into a more stable form.
(also called the atomic weight) of an element is the average mass of all its naturally occurring isotopes. Typically, the atomic mass of an element is close to the mass number of its most abundant isotope.
a substance that contains atoms of two or more different elements
When two or more atoms share electrons
an atom or group of atoms with an unpaired electron in the outermost shell. Having an unpaired electron makes a free radical unstable, highly reactive, and destructive to nearby molecules. Free radicals become stable by either giving up their unpaired electron to, or taking on an electron from, another molecule - may break apart important body molecules.
substances that inactivate oxygen‐derived free radicals—is thought to slow the pace of damage caused by free radicals. Important dietary antioxidants include selenium, zinc, beta‐carotene, and vitamins C and E. Red, blue, or purple fruits and vegetables contain high levels of antioxidants.
The force of attraction that holds together ions with opposite charges
positively charged ion
negatively charged ion
An ionic compound that breaks apart into positive and negative ions in solution. Most ions in the body are dissolved in body fluids as electrolytes, so named because their solutions can conduct an electric current.
two or more atoms share electrons rather than gaining or losing them - a single (─), double (═), or triple (≡) covalent bond.
nonpolar covalent bond
two atoms share the electrons equally—one atom does not attract the shared electrons more strongly than the other atom
polar covalent bond
the sharing of electrons between two atoms is unequal—the nucleus of one atom attracts the shared electrons more strongly than the nucleus of the other atom. When polar covalent bonds form, the resulting molecule has a partial negative charge near the atom that attracts electrons more strongly. This atom has greater electronegativity, the power to attract electrons to itself. At least one other atom in the molecule then will have a partial positive charge.
when a hydrogen atom with a partial positive charge (δ+) attracts the partial negative charge (δ−) of neighboring electronegative atoms, most often larger oxygen or nitrogen atoms. Thus, hydrogen bonds result from attraction of oppositely charged parts of molecules rather than from sharing of electrons as in covalent bonds, or the loss or gain of electrons as in ionic bonds. Hydrogen bonds are weak compared to ionic and covalent bonds. Thus, they cannot bind atoms into molecules. However, hydrogen bonds do establish important links between molecules or between different parts of a large molecule, such as a protein or nucleic acid
a measure of the difficulty of stretching or breaking the surface of a liquid
when new bonds form or old bonds break between atoms
the capacity to do work
energy stored by matter due to its position
energy associated with matter in motion
law of conservation of energy
The total amount of energy present at the beginning and end of a chemical reaction is the same. Although energy can be neither created nor destroyed, it may be converted from one form to another.
release more energy than they absorb
absorb more energy than they release
The collision energy needed to break the chemical bonds of the reactants - This initial energy “investment” is needed to start a reaction. The reactants must absorb enough energy for their chemical bonds to become unstable and their valence electrons to form new combinations.
The more particles of matter present in a confined space, the greater the chance that they will collide (think of people crowding into a subway car at rush hour). The concentration of particles increases when more are added to a given space or when the pressure on the space increases, which forces the particles closer together so that they collide more often.
As temperature rises, particles of matter move about more rapidly. Thus, the higher the temperature of matter, the more forcefully particles will collide, and the greater the chance that a collision will produce a reaction.
hemical compounds that speed up chemical reactions by lowering the activation energy needed for a reaction to occur - enzymes. A catalyst does not alter the difference in potential energy between the reactants and the products. Rather, it lowers the amount of energy needed to start the reaction
When two or more atoms, ions, or molecules combine to form new and larger molecules - ANABOLISM - endergonic
split up large molecules into smaller atoms, ions, or molecules - CATABOLISM - exergonic
they consist of both synthesis and decomposition reactions
the products can revert to the original reactants. whatever is written above or below the arrows indicates the condition needed for the reaction to occur. Many reversible reactions in the body require catalysts called enzymes.
the products can revert to the original reactants, with the special conditions (sometime via catalysts/enzymes).
reduction = the gain of electrons and the reduced substance gains energy. Oxidation - the loss of electrons and the release of energy. red-ox reactions are always parallel - when one substance is oxidized, another is reduced at the same time.
usually lack carbon and are structurally simple - may have only a few atoms and cannot be used for complicated biological functions. Usually made of ionic and covalent bonds, include WATER (55-60% of the body), salts, acids and bases. (other 1-2%)
always contain carbon, usually hydrogen and always covalent bonds. Most are large molecules - make up 38-43% of the body.
the polarity of WATER makes it an excellent solvent.In a solution, a substance called the solvent dissolves another substance called the solute
solutes that are charged or contain polar covalent bonds are 'water-loving' solutes, meaning they dissolve easily in water.
molecules that contain non-polar covalent bonds are 'water-fearing', meaning they don't dissolve easily in water
decomposition reaction breaks down the large molecules into smaller ones with the addition of water. (enable nutrients to be absorbed into the body)
dehydration synthesis reaction
when smaller molecules are joined together and as a result, water is one of the products. (happens during synthesis of proteins and other large molecules).
heat capacity of water
water can absorb or release a relatively large amount of heat with only a modest change in its own temperature. For this reason, water is said to have a high heat capacity. This is due to the high number of hydrogen bonds in H2O
water is a major component of mucus and other lubricating fluids between organs, in joints, inside the GI tract, etc
molecules that are blended together but not bound by chemical bonds
substance that disassociates into one or more H+ and an anion - known as a proton donor
disassociates into an OH- and a cation - known as a proton acceptor.
disassociates into a cation and anion, neither of which is OH- or H+
solution's acidity or alkalinity, which extends from 0 to 14. Based on the molarity of H+. one level change means a tenfold difference in the H+ molarity. less than 7 is acidic, more is basic.
buffer systems in homeostasis
Homeostatic mechanisms maintain the pH of blood between 7.35 and 7.45, the pH of blood falls below 7.35, a condition called acidosis occurs, and if the pH rises above 7.45, it results in a condition called alkalosis. The chemical compounds that can convert strong acids or bases into weak ones are called buffers. They do so by removing or adding protons (H+).
carbonic acid–bicarbonate buffer system
Carbonic acid (H2CO3) can act as a weak acid, and the bicarbonate ion (HCO3−) can act as a weak base. Hence, this buffer system can compensate for either an excess or a shortage of H+. For example, if there is an excess of H+ (an acidic condition), HCO3− can function as a weak base and remove the excess H+. If there is a shortage of H+ (an alkaline condition), by contrast, H2CO3 can function as a weak acid and provide needed H+.
include sugars, glycogen, starches and cellulose. represent 2-3% of body mass. function mainly as a source of chemical energy for generating ATP needed to drive metabolic reactions. consists of C H & O. generally contain one water molecule for each carbon atom 'watered carbon'.
simple sugars, the monomers of carbohydrates, containing 3-7 carbon atoms. '-ose' names, like 'hexose glucose', which is broken down to produce ATP.
molecule formed by the combo of two monosaccharides. Created by dehydration synthesis, broken by hydrolysis.
contains tens of hundreds of monosaccharides joined through dehydration synthesis - insoluble in water and do not taste sweet. GLYCOGEN (glucose monomers linked in branching chains). Starches, formed in plants. Can be broken down through hydrolysis Cellulose is formed by plants but cannot be digested by humans (provides bulk to eliminate feces).
make up 18-25% of body mass. Fewer polar covalent bonds than carbs, so insoluble in water.
lipids that have joined with hydrophilic protein molecules to become more soluble in blood plasma. Proteins are on the outside, lipids are on the inside.
used to synthesize triglycerides and phospholipids - can be catabolized to generate ATP. Consists of a carboxyl group and a hydrocarbon chain.
saturated fatty acid
contains only single covalent bonds between carbon atoms of the hydrocarbon chain - each carbon atom is 'saturated' with hydrogen.
unsaturated fatty acid
contains one or more double covalent bonds, has a kink at the site of the double bond. One kink = monounsaturated. more than one kink = polyunsaturated
most plentiful lipids in body. contains a single glycerol molecule and three fatty acids. Can be either solid (fat) or liquid (oil) at room temp. the kinks in poly & monounsaturated fatty acids prevent the molecules from packing closely together and solidifying.
glycerol backbone with two fatty acids and a phosphate group, which links a charged group usually containing N to the 'head', making it polar. Forms Hbonds with H2O. the two fatty acid 'tails' are nonpolar and only interact with other lipids. AMPHIPATHIC - has polar and nonpolar parts. So link up tail to tail in a double row to make up much of the cell membrane.
contain four rings of carbon atoms. Cholesterol is used to synthesize other steriods. Others are estrogens, testosterone, cortisol, bile salts and Vit D = sterols, containing one hydroxyl (-OH) group.
minor component of all animal cell membranes, precursor of bile salts, vit D and other steroid hormones.
lipids derived from a 20-carbon fatty acid called arachidonic acid.
eicosanoid - modify responses to hormones, contribute to the inflammatory response, prevent stomach ulcers, dilate airways to the lungs, reg body temp and influence formation of blood clots.
eicosanoid - participate in allergic and inflammatory responses
large molecules that contain C H O and N (sometimes S). 12-18% of body mass. Structural (framework of body parts), Regulatory (hormones, neurotransmitters), Contractile (shortening of muscle fibres), Immunological (aid responses to protect body), Transport (carry vital substances around body like hemoglobin tx O2 in blood), Catalytic (enzymes to regulate biochemical rxns).
monomers of proteins. 20 in total. Each has an H with 3 functional groups attached to central C - amino group (-NH2), acidic carboxyl group (-COOH) and side chain (R group). At neutral pH, amino group and carboxyl group are ionized.
covalent joining of each pair of amino acids. forms between C of carboxyl group and N of amino group via dehydration synthesis. Breaking is done through hydrolysis.
4-9 amino acids joined in a chainlike manner
10-2000 or more amino acids joined.
protein structures of organization
primary - unique sequence to form peptide chain. secondary - repeated twisting (alpha helix) or folding (beta pleated sheets) of neighbouring amino acids in the chain. Stabilized by H bonds, form regular intervals along the polypeptide backbone. tertiary - 3D shape. quaternary - the arrangement of polypeptide chains relative to one another.
insoluble in water and chains form long strands II to each other. collagen, elastin, keratin, dystrophin (structural), fibrin (blood clotting), myosin and actin (contractile).
soluble in H2O and spherical. metabolic functions: enzymes (catalytic), antibodies and complement proteins (immunological), albumins (regulatory), membrane proteins (transport), hormones (regulatory).
when a protein encounters an altered environment, it may lose it's characteristic shape and become no longer functional. Like egg-white (albumin) applied to heat turns white and insoluble.
consist of two parts - apoenzyme (protein) and cofactor (metal ion or organic molecule called coenzyme). '-ase' names. HIGHLY SPECIFIC - bind to specific SUBSTRATES (reactant molecules on which enzyme acts) at it's ACTIVE SITE (either fits the substrate or does an 'induced fit' to fit snugly around the substrate. VERY EFFICIENT. SUBJECT TO VARIETY OF CELLULAR CONTROLS. They lower the activation energy of a rxn by decreasing the randomness of collisions, and orient substrates properly.
huge organic molecules that contain C H O N & P - a chain of repeating monomers called nucleotides.
DNA - deoxyribonucleic acid
forms inherited genetic material inside each human cell. each GENE is a segment of the DNA molecule. Control protein synthesis and regulate most of cell activities. Contains N-base, Pentose Sugar (deoxyribose) & Phosphate Group. The Nbases are adenine (A), thymine (T), cytosine (C) and guanine (G). Deoxyribose attaches to each Nbase, alternating with Phosphate groups to form 'backbone'. DOUBLE HELIX.
RNA - ribonucleic acid
single-stranded. Pentose sugar = ribose, contains uracil (U) instead of thymine. Messanger, Ribosomal and transfer are 3 types.
ATP - the 'energy currency' of living systems - txs the energy liberated in exergonic catabolic rxns to power cellular activities that are endergonic (muscular contractions, movement of chromosomes during cell division, movement of structures within cells, transport of substances across cell membranes and synthesis of larger molecules from smaller ones). 3 P groups attached to adenosine and the 5C sugar ribose.
the enzyme that catalyzes the hydrolysis of ATP. (exergonic hydrolysis)
the enzyme that catalyzes the addition of a Pgroup to ADP (endergonic, dehydration synthesis)