Terms : Hide Images
| 941537218 | cohesion | the linking together of like molecules, often by hydrogen bonds | 0 | |
| 941537219 | adhesion | cling of one substance to another, such as water to plant cell walls by means of hydrogen bonds | 1 | |
| 941537220 | 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 | 2 | |
| 941537221 | kinetic energy | the energy associated with the relative motion of objects. Moving matter can perform work by imparting motion to other matter. | 3 | |
| 941537222 | heat | the total amount of kinetic energy due to the random motion of atoms or molecules in a body of matter; also called thermal energy. Heat is energy in its most random form. | 4 | |
| 941537223 | temperature | a measure of the intensity of heat in degrees, reflecting the average kinetic energy of the molecules | 5 | |
| 941537224 | Celsius scale | a temperature scale equal to 5/9 (F-32) that measures the freezing point of water at ) degrees Celsius and the boiling point of water at 100 degrees celsius | 6 | |
| 941537225 | calorie (cal) | the amount of heat energy required to raise the temperature of 1 g of water by 1 degree Celsius; also the amount of heat energy that 1 g of water releases when it cools by 1 degree Celsius. The Calorie (with a capital C), usually used to indicate the energy content of food, is a kilocalorie. | 7 | |
| 941537226 | kilocalorie (kcal) | a thousand calories; the amount of heat energy required to raise the temperature of 1 kg of water by 1 degree Celsius | 8 | |
| 941537227 | joule (J) | a unit of energy; 1 J = 0.239 cal; 1 cal = 4.184 J | 9 | |
| 941537228 | specific heat | the amount of heat that must be absorbed of lost for 1 g of a substance to change its temperature by 1 degree Celsius | 10 | |
| 941537229 | heat of vaporization | the quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gaseous state | 11 | |
| 941537230 | evaporative cooling | the process in which the surface of an object becomes cooler during evaporation, a result of the molecules with the greatest kinetic energy changing from the liquid to the gaseous state. | 12 | |
| 941537231 | solution | a liquid that is a homogenous mixture of two or more substances | 13 | |
| 941537232 | solvent | the dissolving agent of a solution. Water is the most versatile solvent known | 14 | |
| 941537233 | solute | a substance that is dissolved in a solution | 15 | |
| 941537234 | aqueous solution | a solution in which water is the solvent | 16 | |
| 941537235 | hydration shell | the sphere of the water molecules around a dissolved ion | 17 | |
| 941537236 | hydrophilic | having an affinity for water | 18 | |
| 941537237 | colloid | a mixture made up of a liquid and particles that (because of their large size) remain suspended rather than dissolved in that liquid | 19 | |
| 941537238 | hydrophobic | having no affinity for water; tending to coalesce and form droplets of water | 20 | |
| 941537239 | molecular mass | the sum of the masses of all the atoms in a molecule; sometimes called molecular weight | 21 | |
| 941537240 | mole (mol) | the number of grams of a substance that equals its molecular weight in daltons and contains Avogadro's number of molecules | 22 | |
| 941537241 | molarity | a common measure of solute concentration, referring to the number of moles of solute per liter of solution | 23 | |
| 941537242 | 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+); in water, H+ is not found alone but associates with a water molecules to form a hydronium ion | 24 | |
| 941537243 | hydroxide ion | a water molecule that has lost a proton; OH- | 25 | |
| 941537244 | hydronium ion | a water molecule that has an extra proton bound to it; H3O+, commonly represented as H+ | 26 | |
| 941537245 | acid | a substance that increases the hydrogen ion concentration of a solution | 27 | |
| 941537246 | base | a substance that reduces the hydrogen ion concentration of a solution | 28 | |
| 941537247 | pH | a measure of hydrogen ion concentration equal to -log [H+] and ranging in value from 0 to 14 | 29 | |
| 941537248 | buffer | a solution that contains a weak acid and its corresponding base. A buffer minimizes changes in pH when acids or bases are added to the solution. minimizes changes in the concentrations of H+ and OH- | 30 | |
| 941537249 | ocean acidification | decreasing pH of ocean waters due to absorption of excess atmospheric CO2 from the burning of fossil fuels | 31 | |
| 941537250 | matter | Matter is anything that takes up space and has a mass. | 32 | |
| 941537251 | element | An element is a substance that cannot be broken down to other substances by chemical reactions. | 33 | |
| 941537252 | How many elements are currently recognized as being found in nature? | 92 | 34 | |
| 941537253 | compound | A compound is a substance consisting of two or more elements combined in a fixed ratio. | 35 | |
| 941537254 | Of the 92 natural elements | what percent are essential elements?,20-25% | 36 | |
| 941537255 | What are essential elements? | They are elements that an organism needs to live a healthy life and reproduce. | 37 | |
| 941537256 | What elements make up 96% of living matter? | oxygen, nitrogen, carbon and hydrogen. | 38 | |
| 941537257 | Trace elements | Trace elements are required by an organism in only minute quantities. | 39 | |
| 941537258 | What are the Essential Elements in the human body | symbol and percentage of body mass (including water)?,Oxygen (O) Carbon (C) Hydrogen (H) Nitrogen (N) Phosphorus (P) Sulfur (S) | 40 | |
| 941537259 | atom | An atom is the smallest unit of matter that still remains the properties of an element | 41 | |
| 941537260 | What form of measurement is used with atoms | molecules and subatomic particles?,Daltons | 42 | |
| 941537261 | What is the mass of electrons compared to neutrons and protons? | 1/2,000 of a proton/of a neutron's mass. | 43 | |
| 941537262 | Atomic Number | The number of protons and electrons in an element used to classify elements | 44 | |
| 941537263 | mass number | It is the sum of protons plus neutrons in the nucleus of an atom. | 45 | |
| 941537264 | Isotopes | Atoms of the same element that have different numbers of neutrons, and therefore have a greater mass. | 46 | |
| 941537265 | Radioactive Isotope | Isotope in which the nucleus decays (breaks down) over time, giving off radiation in the form of matter and energy | 47 | |
| 941537266 | potential energy | It is the energy that matter possesses because of its location or structure. | 48 | |
| 941537267 | potential energy | what causes it?,The electrons of an atom have potential energy because of how they are arranged in relation to the nucleus. The negatively charged electrons are attracted to the positively charged nucleus so the more distant an electron is from the nucleus, the greater its potential energy. | 49 | |
| 941537268 | valence electrons | electrons in the outermost shell. | 50 | |
| 941537269 | valence shells | The outermost energy shell of an atom contain the valence electrons involved in the chemical reactions of that atom. | 51 | |
| 941537270 | orbital | The 3 dimensional space where an electron can be found 90% of the time. | 52 | |
| 941537271 | covalent bonds | Are atoms that are sharing a pair of valence electrons. | 53 | |
| 941537272 | molecule | Two or more atoms held together by a covalent bond. | 54 | |
| 941537273 | electronegativity | The attraction of a given atom for the electrons of a covalent bond. | 55 | |
| 941537274 | nonpolar covalent bond | A type of covalent bond in which electrons are shared equally between two atoms of similar electronegativity. | 56 | |
| 941537275 | polar covalent bond | A covalent bond between two 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. (NO) GREEDY | 57 | |
| 941537276 | single bond/bond | A single covalent bond; the sharing of a pair of valence electrons by two atoms. | 58 | |
| 941537277 | double bond | A double covalent bond' the sharing of two pairs of valence electrons by two atoms. 0=0 | 59 | |
| 941537278 | Name the types of ways to model molecules. | Lewis Dot Structure ( H:H) and Structural Formula (H-H) | 60 | |
| 941537279 | Why are the electrons in a nonpolar bond equal? | Because they have the same amount of electronegativity. The atoms are at a a tug-a-war stand-off. | 61 | |
| 941537280 | Ionic bond | They are two atoms that are so unequal in their attraction for valence that the more electronegative atom strips an electron completely away from its partner. | 62 | |
| 941537281 | ion | An atom or group of atoms that has gained or lost one of more electrons | 63 | |
| 941537282 | cation | A positively charged ion | 64 | |
| 941537283 | anion | A negatively charged ion | 65 | |
| 941537284 | ionic compounds | A compound resulting from formation of an ionic bond; Also called a salt. | 66 | |
| 941537285 | hydrogen bond | A weak type of chemical bond that is 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 or in another region of the same molecule. | 67 | |
| 941537286 | van der Waals interactions | Weak attractions between molecules or parts of molecules that result from transient local partial charges. | 68 | |
| 941537287 | reactants | The starting materials in a chemical reaction | 69 | |
| 941537288 | Products | The end result of a chemical reaction. | 70 | |
| 941537289 | chemical equilibrium | A state of balance in which the rate of a forward reaction equals the rate of the reverse reaction and the concentrations of products and reactants remain unchanged. | 71 | |
| 941537290 | 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. | 72 | |
| 941537291 | heat | The total amount of kinetic energy due to molecular motion in a body of matter. Energy in its most random form. | 73 | |
| 941537292 | temperature | A measure of the intensity of heat in degrees, reflecting the average kinetic energy of the molecules. | 74 | |
| 941537293 | specific heat | The amount of heat that must be absorbed or lost for 1 gram of a substance to change its temperature by 1°C. | 75 | |
| 941537294 | heat of vaporization | The quantity of heat a liquid must absorb for 1 gram of it to be converted from the liquid to the gaseous state. | 76 | |
| 941537295 | evaporative cooling | the surface becomes cooler during evaporation because highly kinetic molecules become gaseous | 77 | |
| 941537296 | 7 pH | neutral pH | 78 | |
| 941537297 | Strong acidity can alter the structure of biological molecule and prevent them from... | carrying the essential chemical processes of life. | 79 | |
| 941537298 | The reactivity of an atom rises from? | The unpaired electrons in the valence shell | 80 | |
| 941537299 | A chemical reaction that has reached chemical equilibrium | its reactions are?,The rates of the forward and reverse reactions are equal | 81 | |
| 941537300 | What is the property responsible for the ability pf sweat to lower body temperature? | the absortion of heat by the breaking of hydrogen bonds | 82 | |
| 941537301 | Toxic elements | some species are affected by different elements, arsenic to us is lethal while sunflowers can take in lead,arsenic, zinc and other heavy metals that can kill humans | 83 | |
| 941537302 | Chemical bonds | when a shell thats not full interacts with another shell thats not filled | 84 | |
| 941537303 | Moderation of temperature by water | by absorbing heat from the air, then it is released back in the atmoshphere but cooler | 85 | |
| 941537304 | Thermal energy | The energy of motion in the molecules of a substance, random movement of molecules related to temperature | 86 |
