Glossary
From The Chemistry Book
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| The Chemistry Book glossary provides definitions for students. These definitions are from the textbook, lectures, or internet websites. |
Unit 0: Introduction to Chemistry
- Chemistry
- The science of the composition, structure, properties, and reactions of matter; the study of matter and energy and its interactions
- Dependent variable
- The observed variable in an experiment or study whose changes are determined by the presence or degree of one or more independent variables
- Independent variable
- A manipulated variable in an experiment or study whose presence or degree determines the change in the dependent variable
- Inorganic chemistry
- The branch of chemistry that deals with inorganic compounds; compounds not containing C-H bonds
- Natural law
- A summary of observations, many times mathematical.
- Organic chemistry
- The chemistry of carbon-containing compounds
- Qualitative
- data collected by the senses, including color, odor, texture, shape.
- Quantitative
- numerical data collected by an instrument or tool.
- Scientific method
- The principles and empirical processes of discovery and demonstration considered characteristic of or necessary for scientific investigation, generally involving the observation of phenomena, the formulation of a hypothesis concerning the phenomena, experimentation to demonstrate the truth or falseness of the hypothesis, and a conclusion that validates or modifies the hypothesis
- Theory
- a broad generalization containing a set of well tested explanations.
Measurement
- Accuracy
- an accurate measurement is how close the result comes to the true value; precision. (username:pinaybluejay)
- Captive zeros
- zeros that are "caught" between two digits - do count as significant figures (example: 101.205 has six significant figures) (edited by: Jasmine Ruffin Heiny05)
- Celsius
- Formerly known as centigrade; a scale used to measure temperature where 0 degrees is the freezing point and 100 degrees is the boiling point.
14.Conversion factor- A numerical factor used to multiply or divide a quantity when converting from one system of units to another. (Done By: Jazzie Hieny05)
15.Dimensional analysis- A technique that involves the study of dimensions of physical quantities, used primarily as a tool for obtaining information about physical systems too complicated for full mathematical solutions to be feasible. (Done By:Jazzie Hieny 05)
16.Equivalence statement- a specification statement which causes two or more items (variables or arrays) to be associated with each other
17.Exact numbers-are numbers that are exact by definition,or numbers that come in integers and are not likely to be available in amounts smaller than integers.
18.Factor-label method
19.Kelvin- is a unit increment of temperature and is one of the seven SI base units. (done by: Jazzie Hieny05)
20.Length- The length of a thing is the distance between its ends, its linear extent as measured from end to end.(Done By: Jazzie Hieny05)
21.Liter-a unit of volume(done by: Jazzie Hieny 05)
22.Mass- how much matter there is in an object.(Done By:Jazzie Heiny05)
23.Metric system- the systenm of measurement (Done By: Jazzie Heiny05)
24.Milliliter: a unit of measurement (pg.A51) (Done By: Elvia Aldaco;Heiny06)
25.Precision:the degree of agreement amoung several measurementsof the same quantity;the reproducibilityof a measurement (pg.A52) (Done by: Elvia;Heiny06)
26.Scientific notation:a convieninet method for representing a very large or very small number and for indicating the number of significant figures (pg.A49)(Done by: Elvia;Heiny 06)
27.SI units:International system of units based on the metric system and on units derived from the metric system (pg.A53)(Done by: Elvia;Heiny06)
28.Significant figures¨: the certain digits and the first uncertain digit of measurement(pg.A53)(Done By: Elvia;Hieny06)
29.Temperature:measure of the random motions of the components of a substance(pg.A53)(Done By: Elvia;Heiny06)
30.Trailing zeros: a sequence of 0s in the decimal representation (or more generally, in any positional representation) of a number, after which no other digits follow.(Done By: Jazzie Heiny 05)
31.Uncertainty:the charcteristic reflecting the fact that any measurement involves estimates and cannot be exactly reproduced (pg.A 53) (Done by: Elvia;Heiny06)
32.Units- a fundamental quantity of measurement (Done By: Jazzie; Heiny05)
33.Volume-The amount of space occupied by a three-dimensional object or region of space
Matter
34.Alloy-a substance that contains a mixture of elements and has metallic properties.
35.Atom-the fundamental unit of which elements are composed.
36.Chemical change-the change of substances into other substances through a reorganization of the atoms; a chemical reaction.
37.Chemical properties-the ability of a substance to change to a different substance.
38.Chromatography-Any of various techniques for the separation of complex mixtures that rely on the differential affinities of substances for a gas or liquid mobile medium and for a stationary adsorbing medium through which they pass, such as paper, gelatin, or magnesia.
39.Compound-a substance with constant composition that can be broken down into elements by chemical processes.
40.Density-a property of matter representing the mass per unit volume.
41.Distillation-a method for separating the components of a liquid mixture that depends on differences in the ease of vaporization of the components.
42.Elements-a substance that cannot be decomposed into simpler substances by chemical or physical means. It consists of atoms all having the same atomic number.
43.Extensive properties-A non inherent property of a system, such as volume or internal energy, that changes with the quantity of material in the system; the quantitative value equals the sum of the values of the property for the individual constituents
44.Filtration-a method for separating the components of a mixture containing a solid and a liquid.
45.Intensive properties-properties independent of the quantity or shape of the substance under consideration; for example, temperature, pressure, or composition.
46.Gas-one of the three states of matter; has neither fixed shape nor fixed volume.
47.Heterogeneous mixture-a mixture that has different properties in different regions of the mixture.
48.Homogeneous mixture-a mixture that is the same throughout; a solution.
49.Law of conservation of energy-energy can be converted from one form to another but can be neither created nor destroyed.
50.Law of definite composition-the law that a given chemical compound always contains the same elements in the same fixed proportion by weight. Also known as law of definite proportions
51.Liquid-one of the three states of matter; has a fixed volume but takes the shape of its container.
52.Matter-the material of the universe.
53.Mixture-a material of variable composition that contains two or more substances.
54.Molecule-a bonded collection of two or more atoms of the same element or different elements.
55.Physical change-a change from one state (solid or liquid or gas) to another without a change in chemical composition
56.Physical properties-a characteristic of a substance that can change without the substance becoming a different substance.
57.Pure substances-a substance with constant composition.
58.Reaction-a change or transformation in which a substance decomposes, combines with other substances, or interchanges constituents with other substances
59.Solid-one of the three states of matter; has a fixed shape and volume.
60.Solution-a homogeneous mixture.
61.States of matter-the three different forms in which matter can exist: solid, liquid, and gas.
okay so im partially done with these, just give me a little more time... <.< --KuroiNeko 14:44, 3 May 2008 (PDT)
Standard 1
The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure.
1.Absorption spectra-shows the fraction of incident electromagnetic radiation absorbed by the material over a range of frequencies( Done By: Jazzie; Heiny 05)
2.Actinide- encompasses the 15 chemical elements that lie between actinium and lawrencium included on the periodic table, with atomic numbers 89 - 103.(Done By: Jazzie; Heiny05)
3.Allotropes- the property of some chemical elements to be able to take two or more different forms, where the atoms are arranged differently by chemical bonds.(Done By:; Heiny05)
4.Alkali metals: Group 1 metal (pg.A47) (Done By: Elvia;Heiny06)
5.Alkaline earth metals- A Group 2 metal (A 47) (Done By: Jazzie; Heiny05)
6.Angular momentum- vector quantity equal to the mass of the particle multiplied by the cross product of the position vector of the particle with its velocity vector (done By: Jazzie; Heiny05)
7.Atomic mass: the weighted average mass of the atoms in a naturally occuring element (pg.A47) (Done By: Elvia;Heiny 06)
8.Atomic number: the number of protons in the nucleus of an atom;each element has a unique atomic number (pg.A47) (Done by Elvia; Heiny 06)
9.Atomic theory:is a theory of the nature of matter, which states that matter is composed of discrete units called atoms, as opposed to the obsolete notion that matter could be divided into any arbitrarily small quantity.(Done By:Kimberly Bonilla; Heiny 04)
10.Atoms: the fundamental unit of which elements are composed (pg.A47) (Done by: Elvia; Heiny 06)
11.Aufbau principle (buildup principle): a principle stating that as protons are added one by one to the nucleus to build up the elements, electrons are similarily to hydrogen-like orbitals (pg. A47) (Done by: Elvia;Heiny 06)
12.Bohr model- depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus (Done By: Jazzie; Heiny05)
13.Bright-line spectra- An emission spectrum made up of bright lines on a dark background.( Done By: Jazzie; Heiny05)
14.Cathode rays- the "rays" emanating from the negative electrode (cathode) in a partially evacuated tube; a stream of electrons (A 48) (Done By: Jazzie; Heiny05)
15.Chalcogens- the name for the periodic table group 16 (Done By: Jazzie; Heiny05)
16.Chemical properties: the ability of a substance to change to a different substance (pg. A48) (Done by: Elvia; Heiny 06)
17.Diameter- any straight line segment that passes through the center of the circle and whose endpoints are on the circle. (Done By: Jazzie;Heiny05)
18.Discrete energy levels- When an electron in a high energy state jumps down to a lower one, the atom emits a photon of light which corresponds to the exact energy difference of those two levels (conservation of energy). (Done By: Jazzie;Heiny05)
19.Electromagnetic radiation: radiant energy that exhibits wave-like behavior and travels through space at the speed of light in a vaccum (pg.A49) (Done by: Elvia; Heiny 06)
20.Electromagnetic spectrum
21.Electromagnetic waves
22.Electronegativity
23.Electrons: a negatively charged particle that occupies the space around the nucleus of an atom (pg.A49) (Done by: Elvia; Heiny 06)
24.Element: a substance that cannot be decomposed into simpler substances by chemical or physical means. It consists of atoms all having the same atomic number (pg.A49) (Done by: Elvia; Heiny 06)
25.Emission
26.Energy: the capacity to do work or to cause the flow of heat (pg.A49) (Done by: Elvia; Heiny 06)
27.Energy levels
28.Excited state
29.Family
30.Frequency: the number of waves (cycles) per second that pass a given point in space (pg.A49) (Done by: Elvia; Heiny 06)
31.Ground state: the lowest possible energy state of an atom or molecule (pg.A49) (Done by: Elvia; Heiny 06)
32.Group: a verticle column of elements haveing the same valence electron configuration and similar chemical properties (pg.A49) (Done by: Elvia; Heiny06)
33.Halogens: a Group 7 element (pg.A50) (Done by : Elvia; Heiny 06)
34.Heisenberg uncertainty principle
35.Hund’s rule
36.Ionization energy
37.Ion: an atomorgoup of atoms that has a net pesotive or negative charge. (pg. A50) (Done by: Shannon; Heiny06)
38.Isotopes: atoms of the same element (the same number of protrons) that have different numbers of neutrons. They have identical atomic numbers but different mass numbers. (Done by: Shannon:Heiny06)
39.Lanthanide
40.Main groups
41.Mass: The quantity of matter in an object.(done by: Shannon; Heiny06)
42.Metals: an element that gives up electrons reletively easily and is typically lustrous, malleable, and a good contuctor of heat and electricity(Done by: Shannon; Heiny06)
43.Model:a assumptions put forth to explain the observed behavior of matter. The models of chemistry usually involve assumptions about the behavior of individual atoms or molecules.(Done by:Shahnon;Heiny06)
44.Molecules: a bonded collection of two or more atoms of the same element or different elements. (Done by: Shannon; Heiny06)
45.Neutrons:a particle in the atomic neucleus with a mss approxamately equal to tthat of a protron but with no charge.(Done by: Shannon;Heiny06)
46.Nonmetals: An element that does not exhibitmetallic characteristics. Chemically, a typical nonmetal accepts an elecron from a metal.(Done by:Shannon; Heiny06)
47.Nucleus (plural, nuclei): The small, dense center of posotive charge in an atom(Done by:Shannon;Heiny06)
48.Orbital:a representation of the space occupied by an electronin an atom; he probability distribution for the electron.(Done by:Shannon;Heiny06)
49.Periodic table:a chart showing all the element arranged in columns in such a way that all the elements in a given column exhibit similar chemical properties.(Done by arver;heiny;period04)
50.Period:
51.Periodicity:The repetition of similar properties in chemical elements, as indicated by their positioning in the periodic table. .(Done by arver;heiny;period04)
52.Photoelectric effect:the phenomenon in which the absorption of electromagnetic radiation, as light, of sufficiently high frequency by a surface, usually metallic, induces the emission of electrons from the surface. .(Done by arver;heiny;period04)
53.Photons: a "particle" of electromagnetic radiation. .(Done by arver;heiny;period04)
54.Physical:of or pertaining to that which is material: the physical universe; the physical sciences. .(Done by arver;heiny;period04)
55.Principal quantum number:the nonnegative, integral quantum number that defines the stationary orbits in the Bohr model of the atom.(Done by arver;heiny;period04)
56.Probabilistic nature
57.Protons:a "particle" of electromagnetic radiation. .(Done by arver;heiny;period04)
58.Quantum:a discrete amount of something that is analogous to the quantities in quantum theory (done by:Arver;heiny04)
59.Quantum electron configuration
60.Quantum mechanical model
61.Quantum mechanics
62.Quantum theory
63.Radioactive
64.Radius
65.Reactivity- the relative capacity of an atom, molecule, or radical to undergo a chemical reaction with another atom, molecule, or compound. (DN BY:Steph5592; Heiny 02)
66.Representative elements
67.S p d and f subshells
68.Semimetals- An element possessing metallic properties in an inferior degree and not malleable as other metals like Uranium. (DN BY:Steph559 ;Heiny02)
69.Spectral lines
70.Spectrum
71.Subshells
72.Transactinide
73.Transition metals
74.Transuranium
75.Trillion
76.Valence electrons
77.Valence shell
78.Wave properties
79.Wavelength
definitions coming soon ppl. b patient --KuroiNeko 15:08, 3 May 2008 (PDT)
Standard 2
Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces between electrons and protons and between atoms and molecules.
1.Anions
2.Atoms
3.Biological
4.Boiling / melting point
5.Cations
6.Chemical
7.Chemical bonds
8.Chemical formulas
9.Chemical reaction
10.Covalent bond
11.Double bond
12.Electron clouds
13.Electron configurations
14.Electronegativity
15.Electrostatic attraction
16.Electrostatics
17.Hydrogen bonds
18.Inert gases
19.Intermolecular forces
20.Ionic bond
21.Ionization
22.Ions
23.Kinetic energy
24.Lattice energy: a three dimensional system of points designating the positions of the canters of the components of a solid (pg.A50) (Done by: Elvia;Heiny 06)
25.Lewis dot structures (electron dot notation): a diagram of a molecule showing how the valence electrons are arranged amoung the atoms in the molecules (pg.A50) (Done by: Elvia;Heiny 06)
26.London Dispersion forces: the relatively weak forces, which exsist amoung noble gas atoms and nonpolar molecules, that involve an accidental dipole that induces a momentary dipole in a neighbor (pg.A51) (Done by: Elvia; Heiny 06)
27.Matter: the material of the universe(pg.A51) (Done by: Elvia; Heiny 06)
28.Melting
29.Metallic bond
30.Model valence electron:
31.Molecules: a bonded collection of two or more atoms of the same element or different elements (pg.A51) (Done by: Elvia;Heiny 06)
32.Noble gas element: group 8 element (pg.A51) (Done by: Elvia; Heiny 06)
33.Nonpolar molecule
34.Physical properties: a characteristic of a substance that can change without the subtance becoming a different substance (pg. A52) (Done by: Elvia; Heiny 06)
35.Polar covalent: a covalent bond in which the electrons are not shared equally because one atom attracts them more strongly than the other. (pg.A 52) (Done by: Elvia; Heiny 06)
36.Random
37.Repel
38.Single bond
39.Symmetrical
40.Temperature: measure of the random motions (average kinetic energy) of the components of a substance (pg.A53) (Done by: Elvia; Heiny 06)
41.Tetrahedral
42.The octet rule
43.Triple bond: a bond in which two atoms share three pairs of electrons (pg.A53) (Doen by: Elvia; Heiny 06)
44.Valence electrons: the electrons in the outermost occupied principal quantum level of an atom. (pg.A53) (Done by: Elvia;Heiny06)
45.Van der Waals forces
46.Volatility
the definitions are comming people, patience is a virtue *rawr*
--KuroiNeko 15:27, 3 May 2008 (PDT)
Standard 3
The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass of products and reactants.
1.Atomic mass
2.Avogadro’s number
3.Balanced equations
4.Chemical equations
5.Chemical formula
6.Chemical reaction
7.Coefficients
8.Denominator
9.Dimensional analysis
10.Equation
11.Exponents
12.Grams
13.Isolation of variables
14.Isotopes
15.Mass-to-mole
16.Metric conversions
17.Molar mass (formula units)
18.Mole (mol)
19.Molecular mass
20.Molecular weight
21.Mole-to-mass
22.Oxidation
23.Oxidation number
24.Oxidation-reduction reactions
25.Percent yield
26.Principle of conservation of matter
27.Products
28.Reactants
29.Reduction
30.Rules of significant digits
31.Scientific notation
32.Stoichiometry
33.Stoichiometric calculations
34.Subscripts
35.Theoretical yield
36.Units
37.Volume
Nomenclature
38.Anions
39.Binary nonmetal-nonmetal
40.Cations
41.Inorganic nomenclature
42.oxyanions
43.Polyatomic
THEY'RE COMMING PEOPLE!!! STOP BUGGING ABOUT IT! OMG!!!!!...lol jk
--KuroiNeko 15:43, 3 May 2008 (PDT)
Standard 4
The kinetic molecular theory describes the motion of atoms and molecules and explains the properties of gases.
1.Absolute temperature scale
2.Absolute zero:is the lowest possible temperature where nothing could be colder, and no heat energy remains in a substance.(Kimberly Bonilla)(Heiny)(p.4)
3.Atmospheric pressure
4.Barometer
5.Boyle’s law: describes the relationship between the product pressure and volume within a closed system as constant when temperature and moles remain at a fixed measure; both entities remain inversely proportional.(Kimberly Bonilla)(heiny)(p.4)
6.Celsius
7.Charles’s law
8.Collisions
9.Combined gas law
10.Dalton’s law of partial pressures
11.Density of water
12.Diffusion
13.Directly proportional
14.Effusion
15.Fluids
16.Gas laws
17.Graham’s law
18.Gravity
19.Heat
20.Homogeneous
21.Ideal gases
22.Intermolecular forces
23.Inversely proportional relationships
24.Kelvin
25.Kinetic energy:is the extra energy which it possesses due to its motion. It is defined as the work needed to accelerate a body of a given mass from rest to its current velocity.(Kimberly Bonilla)(Heiny)(p.4)
26.Kinetic Molecular Theory
27.Mixtures
28.Monatomic gas
29.Pressure
30.Pure
31.Random motion
32.Rate of diffusion
33.Standard atmosphere (atm)
34.Standard temperature & Pressure (STP | Standard conditions)
35.The ideal gas law
36.Universal gas constant
37.Volume
38.Water pressure
"Quick! Call Definition Man at once!!" cried a student from Mr. H's class, "Don't worry, he's already on the way." Said Mr. H
lol im so wierd XD
--KuroiNeko 15:50, 3 May 2008 (PDT)
Standard 5
Acids, bases, and salts are three classes of compounds that form ions in water solutions.
1.Acidity:the quality or state of being acid. .(Done by arver;heiny;period04)
2.Acids:Any of a class of substances whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals to form salts. .(Done by arver;heiny;period04)
3.Aqueous acid-base reactions
4.Arrhenius: state that acid produce hydrogen ions and base prodice hydroside ions.(Done by arver;heiny;period04)
5.Autoionization of water
6.Bases:Mathematics. a set of linearly independent elements of a given vector space having the property that every element of the space can be written as a linear combination of the elements of the set. (Done by arver;heiny04)
7.Basicity:The ability of an acid to react based on the number of replaceable hydrogen atoms it contains. .(Done by arver;heiny;period04)
8.Bronsted-Lowry: state that a acid is proton donor and the base is the proton acceptor.(Done by arver;heiny;period04)
9.Buffers:A substance that minimizes change in the acidity of a solution when an acid or base is added to the solution.(Done by arver;heiny;period04)
10.Charge:to change the net amount of positive or negative electric charge of (a particle, body, or system). (Done by arver;heiny;period04)
11.Compounds:A pure, macroscopically homogeneous substance consisting of atoms or ions of two or more different elements in definite proportions that cannot be separated by physical means. A compound usually has properties unlike those of its constituent elements.(Done by arver;heiny;period04)
12.Concentration:(in a solution) a measure of the amount of dissolved substance contained per unit of volume.(Done by arver;heiny;period04)
13.Conjugates:Relating to an acid and a base that are related by the difference of a proton. (Done by arver;heiny;period04)
14.Dissociate
15.Electrognegativity
16.Equlibria
17.Formula
18.Hydronium ion
19.Hydroxides
20.Ion:an atom or a group of atoms that has a net positive or negative charge. (Done by arver;heiny;period04)
21.Lewis acid-base definitions:
22.linear v. logarithmic
23.Litmus paper
24.pH
25.pH scale:a log scale based on 10 and equal to -log(H+); a convenient way to represent solution acidity.(Done by arver;heiny;period04)
26.pOH
27.polar covalent bonding
28.Properties of acids: tates sour, react with certain metals to produce hydrogens gas, cause certain organic dyes to change color, react with limestone to produce carbon dioxide, and react with bases to form salts and water.(Done by arver;heiny;period04)
29.Salts
30.Solutions:a homogeneous mixture(Done by arver;heiny;period04)
31.Strong acids: an acid that completely dissociates(ionizes) to produce H ion and the conjugate base.(Done by arver;heiny;period04)
32.Universal indicators
33.Weak acids: an acid that disoociates only to a slight extent in aqueous solution.(Done by arver;heiny;period04)
yes, the definitons are comming, so shut up and wait like everyone else ^^
--KuroiNeko 16:01, 3 May 2008 (PDT)
Standard 6
Solutions are homogeneous mixtures of two or more substances.
1.Affinity
2.Aqueous solutions
3.Chromatography
4.Colligative properties
5.Compounds
6.Concentration
7.Covalent bonding
8.Dilute
9.Dilution
10.Directly proportional
11.Dissolution
12.Dissolving
13.Distillation
14.Equilibrium
15.Freezing point
16.Grams per liter
17.Homogeneous mixtures
18.Hydration
19.Hydrophilic
20.Hydrophobic
21.Immiscible
22.Mass percent
23.Miscible
24.Molality (m)
25.Molarity (M)
26.Mole fraction
27.Normality (N)
28.Parts per million
29.Percent composition
30.Polar water molecules
31.Pressure
32.Purification
33.Saturated
34.Shapes of molecules
35.Solubility
36.Solute
37.Solution
38.Solvent
39.Substrate
40.Surface area
41.Supersaturated
42.Temperature
43.Unsaturated
RAWRZ!! --KuroiNeko 10:50, 5 May 2008 (PDT)
Standard 7
Energy is exchanged or transformed in all chemical reactions and physical changes of matter.
1.Chemical & physical change
2.Condenses
3.Endothermic
4.Enthalpy
5.Entropy
6.Evaporates
7.Exothermic
8.Free energy
9.Freezes
10.Gibbs free energy
11.Heat
12.Heat entropy
13.Hess’s law
14.internal energy
15.Joule/gram-degree
16.Kinetic energy
17.latent heat
18.Latent heat of vaporization
19.melts
20.Nonspontaneous reaction
21.Products. a substance resulting from a chemical reaction. It is shown to the right of the arrow in a chemical equation (pg.A52) (Done by: Elvia;Heiny 06)
22.Qualitative knowledge
23.Reactants. a starting substance in a chemical reaction; it appears to the left of the arrow in a chemical equation (pg.A52) (Done by: Elvia; Heiny 06)
24.Specific heat: another name for specific heat capacity (pg.A53) (Done by: Elvia;Heiny 06)
25.Spontaneous: developing without apparent external influence (Done: Elvia;Heiny06)
26.Spontaneous reaction
27.Standard atmospheric pressure
28.Standard enthalpy of formation
29.Superheated: the process of heating a liquid to a temperature above its boiling point without its boiling. (pg.A53) (Done by: Elvia;Heiny 06)
30.Temperature: measure of random motions of the components of a substance (Pg.A53) (Done by: Elvia;Heiny06)
31.Transition states
Get off my back and read a book for crying out loud!!!! >.>--KuroiNeko 10:52, 5 May 2008 (PDT)
Standard 8
Chemical reaction rates depend on factors that influence the frequency of collision of reactant molecules.
1.Activation barrier
2.Activation energy: the threshold energy that must be overcome to produce a chemical reaction (pg.A47) (Done by: Elvia;Heiny06)
3.Catalyst: a substance that speeds up a reaction without being consumed (pg.A48) (Done by: Elvia;Heiny06)
4.Collision theory
5.Conservation of matter
6.Enzymes: a large molecule, usually a protien, that catalyzes biological reactions (pg.A49) (Done: Elvia;Heiny06)
7.Frequency
8.Kinetic energy: (1/2 mv squared) energy due to the motion of an object; dependent on the mass of the object and the square of its velocity (pg.A50) (Done by: Elvia;Heiny 06)
9.Quantitative measure
10.Reaction rate:
11.Reciprocal: the opposite of a number or fraction (Done: Elvia;Heiny06)
12.Stoichiometry
o.0 well that was short <.< --KuroiNeko 10:54, 5 May 2008 (PDT)
Standard 9
Chemical equilibrium is a dynamic process at the molecular level and pressure.
1.Aqueous solutions: a solution in which water is disolving medium or solvent (pg.A47) (Done by: Elvia;Heiny 06)
2.Balance chemical equations
3.Chemical equilibrium: a dynamic reaction system in which the concentrations of all reactants and products remian constant as a function of time (pg.A48) (Done by: Elvia;Heiny06)
4.Dynamic state
5.Equilibrium constants: the value obtained when equilibrium concentrations of the chemical species are substituted into the equilibrium expression. (pg.A49) (Done by: Elvia;Heiny06)
6.LeChatelier’s principle: if a change is imposed on a system at equilibrium, the position of the eqilibrium will shift ina direction that tends to reduce the effect of that change. (pg.A50) (Done by: Elvia;Heiny06)
7.Precipitation: the quantity of water deposited (Done by:Elvia;Heiny 06)
8.Thermodynamics: a study of energy and its interactions (pg.A53)(Done by: Elvia;Heiny06)
omg, it didn't even hit the double digits!! o.o --KuroiNeko 10:54, 5 May 2008 (PDT)