Vocabulary, Properties of Solids, Liquids, and Gases
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| Characteristic that can be observed without altering the chemical composition of a substance | physical property
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| Properties may be qualitative or quantitative | physical property
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| name three qualitative properties | color, odor, taste
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| name three quantitative properties | melting point, freezing point, boiling point, solubility, density, specific gravity
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| three typical states of matter | solid, liquid, gas
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| specific temperature at a given pressure at which a substance changes from solid to liquid | melting point
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| same temperature as the melting point, substance changes from liquid to solid | freezing point
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| temperature at a given pressure at which a substance changes from liquid to gas | boiling point
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| how much of something will dissolve in a given amount of water | solubility
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| expresses the relationship between a substance's mass and volume | density
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| density equation | Density=mass/volume
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| how is density expressed with units | unit of mass over unit of volume EX: 11.3 g/mL
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| ratio of mass of the substance to the mass of an equal volume of water at the same temperature | specific gravity
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| any units for specific gravity | no
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| characteristic of a substance that can be observed when it interacts with other forms of matter, results in an alteration of the chemical composition of the substance | chemical property
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| examples of chemical property | substance burning and forming new substances, how substance reacts with water, an acid, or a base
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| process that manifests a physical property | physical change
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| examples of physical change | change in state of matter, dissolving table salt or sugar into water, ice melting, water freezing, or water boiling
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| process that manifests a chemical property, which forms new substances with their own chemical and physical properties | chemical change
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| examples of chemical change | iron rusting, paper burning, cremation, milk souring, decomposition
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| order of protein decomposition | 1) proteins break down into amino acids, 2) amino acids break down into AMINES and ORGANIC ACIDS, 3) AMINES break down into ammonia and hydrogen gas, 4)ORGANIC ACIDS break down into water, carbon dioxide, and oxygen
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| water breaking apart | hydrolysis
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| what begins the process of protein decomp | hydrolysis (enzymes react in moisture)
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| most energetic state of matter | gas
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| state of matter with intermediate energy | liquid
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| least energetic state of matter | solid
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| each particle possesses random rapid motion independent of the other particles in which state? | gas
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| in this state particles slide past each other | liquid
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| in this state, particles vibrate around fixed positions | solid
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| the change from a solid to a liquid to a gas by a particular form of matter is a ____ process | endothermic
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| if a substance changes from gas to liquid to solid, a liberation of heat it is a ______ process | exothermic
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| specific quantity of heat that is absorbed to convert 1 gram of solid to 1 gram of liquid at the substance's melting point | heat of fusion
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| heat of fusion for water | 80 calories per gram
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| amount of heat necessary to change 1 gram of a substance from the liquid to the gaseous state at the boiling point | heat of vaporization
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| heat of vaporization for water | 540 calories of heat per gram
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| any process that liberates heat | exothermic
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| any process that absorbs heat | endothermic
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| funeral service exothermic model | plaster of paris and water
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| change in state directly from the solid state to the gas state | sublimation
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| two examples of sublimation | heating iodine crystals, dry ice
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| is sublimation a physical or a chemical change? | physical change
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| a measure of the amount of disorder or randomness | entropy
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| which state of matter has the least, intermediate, and most entropy? | 1) solids=least, 2) liquids=intermed, 3) gas=most
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| the volume of a gas may be decreased by increasing the pressure on the gas | compressibility
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| a gas will increase its volume when heated | expansivity
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| movement of a gas when introduced into a container | diffusibility
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| the volume of a gas is equal to | the volume of the container
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| force per unit area | pressure
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| where do gases exert pressure? | on the walls of their containers
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| commonly measured form of presssure? | atmosphere
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| what can be used to measure atmospheric pressure? | mercury barometer
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| what does 1 atmosphere (atm) equal (2 things) | 760 mm Hg (mercury) OR 760 torr
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| relationship between the volume of a given quantity of a gas and its pressure is expressed by which gas law? | Boyle's Law
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| in Boyle's law, the volume occupied by a gas and the pressure it exerts (when temperature is constant) have a ____ relationship | inverse
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| p1v1=p2v2 (where T is constant) | boyle's law
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| practical example of boyle's law | breathing
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| relationship btw volume and temperature is expressed by this gas law | charles' law
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| the volume of a fixed quantity of gas is _____ proportional to its Kelvin temperature if the pressure remains constant | directly
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| v1/t1=v2/t2 | charles' law
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| Charles' law, temp is expressed in what? | Kelvin
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| Kelvin= | degrees celcius + 273
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| practical example of charles' law | incubator
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| relationship btw pressure exerted by a gas and its temperature | gay-lussac's law
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| according to gay lussac's law, as the temp of a gas increases, the pressure increases, and vice versa, if the volume remains constant. it is _____ proportional | directly
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| p1/t1=p2/t2 | gay lussac's law
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| practical example of gay lussac's law | autoclave
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| transition from liquid to gas | evaporation
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| transition from gas to liquid | condensation
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| when two opposing rates are equal | equilibrium
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| the pressure exerted by a vapor when it s in equilibrium with its liquid | equilibrium vapor pressure
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| as temperature increases, the vapor pressure of a liquid ____ | increases
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| the rapid passage of liquid particles to the vapor state by forming bubbles | boiling
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| a liquid boils at a temperature known as the | boiling point
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| the boiling point at 1 atmosphere pressure | normal boiling point
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| two types of matter | pure substances AND mixtures
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| two types of pure substances | elements and compounds
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| substances which cannot be decomposed by further chemical means | elements
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| substances composed of to or more elements chemically united in a definite proportion by mass | compound
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| two or more nonchemically united substances that are in no definite proportion by mass | mixtures
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| how many elements? | 117
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| most abundant element on earth | oxygen
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| second most abundant element on earth, forms 1/4 of the earth's crust | silicon
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| most abundant element in the universe and second most | hydrogen, helium
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| states that when two or more elements combine they always combine in a fixed or definite proportion by mass | law of definite proportions
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| how can compounds be decomposed? | chemical changes
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| 4 primary types of inorganic compounds | oxides, acids, bases, salts
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| how can mixtures be decomposed | physical changes
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| mixtures that are characterized by uniform properties throughout their contents, uniform composition | homogeneous
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| mixtures that do not have uniform properties, or composition throughout | heterogeneous
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| the study of the nature of matter and the changes that matter undergoes | chemistry
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| anything that possesses mass and occupies space | matter
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| what is the nature of matter, 3 things: | 1) composition of matter, 2) forces holding it together, 3) its observable properties
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| does not cause a change in the chemical composition of a material | physical change
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| those changes that result in the formation of new substances | chemical change
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| the ability to do work | energy
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| energy of motion | kinetic energy
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| stored energy | potential energy
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| the study of compounds usually containing elements other than carbon | inorganic chemistry
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| the study of certain carbon compounds | organic chemistry
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| the study of compounds produced by living organisms | biochemistry
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| the study of those types of matter and changes in matter related to the disinfection/preservation of human remains | embalming chemistry
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| the study of those physical/chemical changes in body due to death | thanatochemistry
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| the standard set of units used by all scientists | international system of units/metric system/SI units
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| standard unit of length | meter (m)
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| standard unit of volume | liter (L)
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| standard unit of mass | kilogram (kg)
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| standard unit of heat | calorie (cal)
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| the quantity of heat necessary to raise the temperature of 1 gram of water 1 degree Celsius at 15 degrees Celsius | calorie
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| 1 Cal= | 1000 kcal = 1000 cal
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| positive ion | cation
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| negative ion | anion
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| is Cl2 a polar or nonpolar bond? | nonpolar
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| is HF polar or nonpolar bond? | polar
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| is hydrogen considered a metal or a nonmetal? | nonmetal
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| order of exponential expression and symbols: | Mega (M 10^9), Kilo (k 10^6), deci (d 10^-1), centi (c 10^-2), milli (m 10^-3), micro (u 10^-6), nano (n 10^-9)
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| metal bonding to a nonmetal is an example of a ____ bond | ionic
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| metal bonding to a metal or a non-metal bonding to a non-metal are examples of ______ bonds | covalent
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| group IA on periodic table (3 names) | alkali metals, alkali elements, reactive metals
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| group 2A on the periodic table | alkaline earth metals
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| part of group B on periodic table removed from rest of periodic table called: (top period is:) (bottom period is:) | rare earth metals. top period is lanthanide series, bottom is actinide series
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| elements to the left of the heavy line are | metals
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| elements to the right of the heavy line are | nonmetals
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| isotopes of hydrogen (3) | protium, deuterium and tritium
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| isotope of hydrogen that makes up heavy water | deuterium
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| isotope of hydrogen that is radioactive | tritium
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