Unit 1 from the textbook Campbell Reece Biology, by chapter, in the order they appear.
Unit name: The Chemistry of Life
Unit pages: 32-91
Chapters: 2-5
Terms : Hide Images
| 7278414386 | matter | anything that takes up space and has mass | 0 | |
| 7278414387 | element | any substance that cannot be broken down to any other substance | 1 | |
| 7278414388 | compound | a substance consisting of two or more elements in a fixed ratio | 2 | |
| 7278414389 | trace element | an element indispensable for life but required in extremely minute amounts | 3 | |
| 7278414390 | atom | the smallest unit of matter that retains the properties of an element | 4 | |
| 7278414391 | neutron | an electrically neutral particle (a particle having no electrical charge), found in the nucleus of an atom | 5 | |
| 7278414392 | proton | a subatomic particle with a single positive electrical charge, found in the nucleus of an atom | 6 | |
| 7278414393 | electron | a subatomic particle with a single negative charge. One or more electrons move around the nucleus of an atom | 7 | |
| 7278414394 | atomic nucleus | an atom's central core, containing protons and neutrons | 8 | |
| 7278414395 | dalton | a measure of mass for atoms and subatomic particles | 9 | |
| 7278414396 | atomic number | the number of protons in the nucleus of an atom, unique for each element and designated by a subscript to the left of the elemental symbol | 10 | |
| 7278414397 | mass number | the sum of the number of protons and neutrons in an atom's nucleus | 11 | |
| 7278414398 | atomic mass | the total mass of an atom, which is the mass in grams of one mole of the atom | 12 | |
| 7278414399 | isotope | one of several atomic forms of an element, each containing a different number of neutrons and thus differing in atomic mass | 13 | |
| 7278414400 | radioactive isotope | an isotope (an atomic form of a chemical element) that is unstable; the nucleus decays spontaneously, giving off detectable particles and energy | 14 | |
| 7278414401 | energy | the capacity to do work (to move matter against an opposing force) | 15 | |
| 7278414402 | potential energy | the energy stored by matter as a result of its location or spatial arrangement | 16 | |
| 7278414403 | energy level | any of several different states of potential energy for electrons in an atom | 17 | |
| 7278414404 | electron shell | an energy level represented as the distance of an electron from the nucleus of an atom | 18 | |
| 7278414405 | periodic table of the elements | a chart of the chemical elements, arranged in three rows, corresponding to the number of electron shells in their atoms | 19 | |
| 7278414406 | valence electron | an electron in the outermost electron shell | 20 | |
| 7278414407 | valence shell | the outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom | 21 | |
| 7278414408 | orbital | the three-dimensional space where an electron is found 90% of the time | 22 | |
| 7278414409 | chemical bond | an attraction between two atoms, resulting from a sharing of outer-shell electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete outer electron shells | 23 | |
| 7278414410 | covalent bond | a type of strong chemical bond in which two atoms share one or more pairs of valence electrons | 24 | |
| 7278414411 | molecule | two or more atoms held together by covalent bonds | 25 | |
| 7278414412 | structural formula | a type of molecular notation in which the constituent atoms are joined by lines representing covalent bonds | 26 | |
| 7278414413 | molecular formula | a type of molecular notation indicating only the quantity of the constituent atoms | 27 | |
| 7278414414 | valence | the bonding capacity of an atom, generally equal to the number of unpaired electrons in the atom's outermost shell | 28 | |
| 7278414415 | electronegativity | the attraction of an atom for the electrons of a covalent bond | 29 | |
| 7278414416 | nonpolar covalent bond | a type of covalent bond in which electrons are shared equally between two atoms of similar electronegativity | 30 | |
| 7278414417 | polar covalent bond | a covalent bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive | 31 | |
| 7278414418 | ion | an atom that has gained or lost electrons, thus acquiring a charge | 32 | |
| 7278414419 | cation | an ion with a positive charge, produced by the loss of one or more electrons | 33 | |
| 7278414420 | anion | a negatively charged ion | 34 | |
| 7278414421 | ionic bond | a chemical bond resulting from the attraction between oppositely charged ions | 35 | |
| 7278414422 | ionic compound | a compound resulting from the formation of an ionic bond; also called a salt | 36 | |
| 7278414423 | salt | a compound resulting from the formation of an ionic bond; also called an ionic compound | 37 | |
| 7278414424 | hydrogen bond | a type of weak chemical bond formed when the slightly positive hydrogen atom of a polar covalent bond in one molecule is attracted to the slightly negative atom of a polar covalent bond in another molecule | 38 | |
| 7278414425 | van der Waals interactions | weak attractions between molecules or parts of molecules that are brought about by localized charge fluctuations | 39 | |
| 7278414426 | chemical reaction | a process leading to chemical changes in matter; involves the making and/or breaking of chemical bonds | 40 | |
| 7278414427 | reactant | a starting material in a chemical reaction | 41 | |
| 7278414428 | product | an ending material in a chemical reaction | 42 | |
| 7278414429 | chemical equilibrium | in a reversible chemical reaction, the point at which the rate of the forward reaction equals the rate of the reverse reaction | 43 | |
| 7278414430 | polar molecule | a molecule (such as water) with opposite charges on opposite sides | 44 | |
| 7278414431 | cohesion | the binding together of like molecules, often by hydrogen bonds | 45 | |
| 7278414432 | adhesion | the attraction between different kinds of molecules | 46 | |
| 7278414433 | surface tension | a measure of how difficult it is to stretch or break the surface of a liquid. Water has a high surface tension because of the hydrogen bonding of surface molecules | 47 | |
| 7278414434 | kinetic energy | the energy of motion, which is directly related to the speed of that motion. Moving matter does work by imparting motion to other matter | 48 | |
| 7278414435 | heat | the total amount of kinetic energy due to molecular motion in a body of matter. Heat is energy in its most random form | 49 | |
| 7278414436 | temperature | a measure of the intensity of heat in degrees, reflecting the average kinetic energy of the molecules | 50 | |
| 7278414437 | Celsius scale | a temperature scale (°C) equal to 5/9 (°F - 32) that measures the freezing point of water at 0°C and the boiling point of water at 100°C | 51 | |
| 7278414438 | calorie (cal) | the amount of heat energy required to raise the temperature of 1 g of water by 1°C; also the amount of heat energy that 1 g of water releases when it cools by 1°C. The Calorie (with a capital C), usually used to indicate the energy content of food, is a kilocalorie | 52 | |
| 7278414439 | kilocalorie (kcal) | a thousand calories; the amount of heat energy required to raise the temperature of 1 kg of water by 1°C | 53 | |
| 7278414440 | joule (J) | a unit of energy: 1 J = 0.239 cal; 1 cal = 4.184 J | 54 | |
| 7278414441 | specific heat | the amount of heat that must be absorbed or lost for 1 g of a substance to change its temperature by 1°C | 55 | |
| 7278414442 | heat of evaporation | the quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gaseous state | 56 | |
| 7278414443 | evaporative cooling | the property of a liquid whereby the surface becomes cooler during evaporation, owing to a loss of highly kinetic molecules to the gaseous state | 57 | |
| 7278414444 | solution | a liquid that is a homogeneous mixture of two or more substances | 58 | |
| 7278414445 | solvent | the dissolving agent of a solution. Water is the most versatile solvent known | 59 | |
| 7278414446 | solute | a substance that is dissolved in a solution | 60 | |
| 7278414447 | aqueous solution | a solution in which water is the solvent | 61 | |
| 7278414448 | hydration shell | the sphere of water molecules around each dissolved ion | 62 | |
| 7278414449 | hydrophilic | having an affinity for water | 63 | |
| 7278414450 | colloid | a mixture made up of a liquid and particles that (because of their large size) remain suspended in that liquid. See large intestine | 64 | |
| 7278414451 | hydrophobic | having an aversion to water; tending to coalesce and form droplets in water | 65 | |
| 7278414452 | molecular mass | the sum of the masses of all the atoms in a molecule; sometimes called molecular weight | 66 | |
| 7278414453 | mole (mol) | the number of grams of a substance that equals its molecular weight in daltons and contains Avogadro's number of molecules | 67 | |
| 7278414454 | molarity | a common measure of solute concentration, referring to the number of moles of solute per liter of solution | 68 | |
| 7278414455 | hydrogen ion | a single proton with a charge of 1+. The dissociation of a water molecule (H2O) leads to the generation of a hydroxide ion (OH-) and a hydrogen ion (H+) | 69 | |
| 7278414456 | hydroxide ion | a water molecule that has lost a proton (OH-) | 70 | |
| 7278414457 | acid | a substance that increases the hydrogen ion concentration of a solution | 71 | |
| 7278414458 | base | a substance that reduces the hydrogen ion concentration of a solution | 72 | |
| 7278414459 | pH | a measure of hydrogen ion concentration equal to -log [H+] and ranging in value from 0 to 14 | 73 | |
| 7278414460 | buffer | a substance that consists of acid and base forms in a solution and that minimizes changes in pH when extraneous acids or bases are added to the solution | 74 | |
| 7278414461 | acid precipitation | rain, snow, or fog that is more acidic than pH 5.6 | 75 | |
| 7278414462 | organic chemistry | the study of carbon compounds (organic compounds) | 76 | |
| 7278414463 | hydrocarbon | an organic molecule consisting only of carbon and hydrogen | 77 | |
| 7278414464 | isomer | one of several organic compounds with the same molecular formula but different structures and therefore different properties. The three types of isomers are structural isomers, geometric isomers, and enantiomers | 78 | |
| 7278414465 | structural isomer | one of several organic compounds that have the same molecular formula but differ in the covalent arrangements of their atoms | 79 | |
| 7278414466 | geometric isomer | one of several organic compounds that have the same molecular formula but differ in the spatial arrangements of their atoms | 80 | |
| 7278414467 | cis | arrangement of two noncarbon atoms, each bound to one of the carbons in a carbon-carbon double bond, where the two noncarbon atoms are on the same side relative to the double bond | 81 | |
| 7278414468 | trans | arrangement of two noncarbon atoms, each bound to one of the carbons in a carbon-carbon double bond, where the two noncarbon atoms are on opposite sides relative to the double bond | 82 | |
| 7278414469 | enantiomer | one of two molecules that are mirror images of each other | 83 | |
| 7278414470 | functional group | a specific configuration of atoms commonly attached to the carbon skeletons of organic molecules and usually involved in chemical reactions | 84 | |
| 7278414471 | hydroxyl group | a functional group consisting of a hydrogen atom joined to an oxygen atom by a polar covalent bond (--OH). Molecules possessing this group are soluble in water and are called alcohols | 85 | |
| 7278414472 | carbonyl group | a functional group present in aldehydes and ketones and consisting of a carbon atom double-bonded to an oxygen atom (--CO) | 86 | |
| 7278414473 | carboxyl group | a functional group present in organic acids and consisting of a single carbon atom double-bonded to an oxygen atom and also bonded to a hydroxyl group (--COOH) | 87 | |
| 7278414474 | amino group | a functional group that consists of a nitrogen atom bonded to two hydrogen atoms (--NH2); can act as a base in solution, accepting a hydrogen ion and acquiring a charge of 1+ | 88 | |
| 7278414475 | sulfhydryl group | a functional group consisting of a sulfur atom bonded to a hydrogen atom (--SH) | 89 | |
| 7278414476 | phosphate group | a functional group important in energy transfer (--OPO3-2) | 90 |
