Chemistry LeapMed Reviewer PDF

lOMoARcPSD|44805057 CHEMISTRY LEAPMED reviewer CREATED BY LeapMedReviewer Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer...

lOMoARcPSD|44805057 CHEMISTRY LEAPMED reviewer CREATED BY LeapMedReviewer Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Basics of Chemistry ! The field of study concerned with the characteristics, composition, and transformations of matter Numbers ! Idea of a quantity ! Exact o! Factual in nature o! Ex. 1 hour is 60 minutes ! Measured o! Numbers you measure using an instrument o! Ex. Stopwatch, meter stick, … Measurements ! Comparison of the quantity of a substance to that of its standard unit ! 3 components o! Numerical value: 200 mL CuSO4 solution o! Unit: 200 mL CuSO4 solution o! Substance: 200 mL CuSO4 solution ! Used in stoichometry and dimensional analysis Accuracy ! Closesness to the true value! Precision ! Closesness of the repreated trials or measurements ! Margin for error o! Usually at least 2 decimal places Metric system ! Has a base number multiplied to powers of ten Significant figures ! Standard: you usually use the smallest s.f. count possible ! Rules o! All non zeroes are significant o! Zeroes between non zeroes are significant (ex. 0.2002 = four s.f.) o! Zeroes at the end of a decimal number are significant (ex. 0.200 = three s.f.) o! Placeholders or leading zeroes are not significant (ex. 0.0002 = one s.f.) o! Scientific notation are significant ! 2! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Matter ! Anything that has mass and occupies space o! Mass !! The amount of matter present in a sample ! The mother of all concepts ! Can be in the form of these particles o! Atoms !! Smallest unit of matter that can retain its chemical properties !! Subatomic particles cannot exist on their own o! Compounds or molecules !! Two types of atoms that are chemically bonded !! All molecules are compounds, but not all compounds are molecules o! Ions !! Charged particles or compounds !! May be cations (+) or anions (-) ! Classifications of matter o! Pure substance !! Only one substance present !! Definite and constant composition !! Properties always the same under the same conditions !! Has a chemical bond !! Kinds ! Element o! Cannot be broken down into smaller simpler substances by chemical or physical means o! Building blocks for all other types of matter o! 118 elements known ! 3! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer ! Compound o! Can be broken down into constituent elements by chemical, but not physical, means o! Chemical combination of two or more elements o! Have definite, constant, elemental composition o! Mixture !! Physical combination of two or more substances !! Composition can vary !! Properties can vary !! Exists without a chemical reaction !! Kinds ! Homogeneous o! One visible phase o! Same properties throughout ! Heterogeneous o! Two or more visible phases o! Different properties in different phases ! Properties o! Physical properties !! Can be measured without changing the composition of a substance ! Temperature o! SI is Kelvin (K) ! Pressure o! SI is (atm) atmosphere ! Shape of crystals o! Lattice, geometric structure ! Melting and boiling point !! Subdivisions of physical properties ! Extensive property o! If the measurement changes as the amount of substance changes o! Ex. mass ! Intensive property o! Independent of the amount of substance o! Ex. density o! Chemical properties !! Composition of a substance does change !! Needs a chemical reaction ! Decomposition ! Flammability ! 4! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Atomic Structure Atom ! The smallest particle of an element that can exist and still ! Basic unit of an element that can enter into chemical combination ! Democritus o! “all matter contains “atomos” (indivisible) Molecule ! A group of two or more atoms that functions as a unit because the atoms are tightly bound ! together ! Diatomic molecule o! Molecule that contains two atoms o! Simplest type of molecule that can exist ! Triatomic molecule o! Molecule that contains three atoms ! Continuing on numerically, we have tetraatomic molecules, pentatomic molecules, and so on ! Homoatomic molecule o! Molecule in which all atoms present are of the same kind ! Heteroatomic molecule o! Molecule in which two or more kinds of atoms are present Atomic theory of matter ! Each element is composed of extremely small particles called atoms ! All atoms of a given element are identical o! The atoms of different elements are different and have different properties (including different masses) ! Atoms of an element are not changed into different types of atoms by chemical reactions o! Atoms are neither created nor destroyed in chemical reactions ! Compounds are formed when atoms of more than one element combine o! A given compound always has the same relative number and kind of atoms Separation methods ! Filtration o! Separate materials that are insoluble from one another o! Principle !! Particle size o! Filtrate !! Product of filtration o! Residue !! Left behind after filtration ! Distillation o! Different fractions of petroleum products ! 5! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer o! Cannot be used with immiscible materials o! Principle !! Boiling point o! Distillate !! Product o! Residue !! Left behind ! Magnetic separation o! Separate metals from non-metals o! Principle !! Magnetism ! Sedimentation/decantation o! Uses gravity to create layers o! Principle !! Difference in density, solubility, or miscibility ! Centrifugation o! Unit !! Rotation/revolution per minute (rpm) o! Principle !! Difference in density, solubility, or miscibility ! Chromatography o! Could be used to check the identity of a substance o! Principle !! Difference in polarity o! Note !! Solubility is between solids and liquids !! Miscibility is between liquids Laws related to the atomic theory of matter ! Law of constant composition o! In a given compound the relative number and kind of atoms are constant ! Law of conservation of mass o! The total mass of materials present after a chemical reaction is the same as the total mass before the reaction ! Law of multiple proportions o! If two elements, A and B, can combine to form more than one compound, then the ratios of the relative masses of each element which can combine can be represented by characteristically small whole numbers Internal structure of an atom ! Subatomic particles o! Particle that is a building block for atoms o! Protons ! 6! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer o! Neutrons o! Electrons ! Atomic number o! Uniquely assigned to each element o! Is a whole number o! Does not ever change o! Z = # of protons/electrons ! Mass number o! Weight of the element in amu o! A = # of protons and neutrons !! Neutrons ! N = A - Z Arrangement of subatomic particles within an atom ! All protons and all neutrons present are found at the center of an atom in the nucleus ! Because the nucleus houses the heavy subatomic particles (protons and neutrons), almost all (more than 99.9%) of the mass of an atom is concentrated in its nucleus ! The outer (extranuclear) region of an atom contains all of the electrons ! The extranuclear region accounts for most of the volume of an atom ! The volume occupied by the electrons is sometimes referred to as the electron cloud ! Nucleon is any subatomic particle found in the nucleus of an atom Charge neutrality of an atom ! An atom is electrically neutral o! It has no net electrical charge ! Equal numbers of positive and negative charges give a net electrical charge of zero Isotopes ! iso = something similar ! Same atomic number (Z) ! Different mass number (A) ! Atoms of an element that have the same number of protons and the same number of electrons but different numbers of neutrons ! Different isotopes always have the same atomic number and different mass numbers ! Isotopes of an element have the same chemical properties, but their physical properties are often slightly different ! Ex. 11H hydrogen 1 (H-1, protium); 12H hydrogen 2 (H-2, deuterium); 13H hydrogen 3 (H-3, tritium) ! 7! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Nuclear Chemistry Stable and unstable nuclides ! Nuclear reaction o! Reaction in which changes occur in the nucleus of an atom ! Nuclide o! Atom with a specific atomic number and a specific mass number ! Stable nuclide o! Nuclide with a stable nucleus, a nucleus that does not readily undergo change ! Unstable nuclide o! Nuclide with an unstable nucleus that spontaneously undergoes change ! Radioactivity o! The radiation spontaneously emitted from an unstable nucleus Types of nuclear reactions ! Watch and memorize symbols + practice problems o! https://youtu.be/uF6EgMQ8STA o! https://youtu.be/CwExbnOzc4o o! https://youtu.be/uqAA_D9Mi_I o! https://youtu.be/bjuZSvZukAw, https://youtu.be/_pY5HeZpNr8 ! ! ! ! 8! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Rate of Radioactive decay ! Radioactive nuclides do not all decay at the same rate ! The greater the decay rate, the lower the stability of the nuclide ! A half-life (t1/2) is the time required for one-half of a given quantity of a radioactive substance to undergo decay ! The decay rate (half-life) of a radionuclide is constant o! It is independent of physical conditions such as temperature, pressure, and state of chemical combination o! It depends only on the identity of the radionuclide ! If a nuclide is radioactive, nothing will stop it from decaying and nothing will increase or decrease its decay rate ! Watch o! https://youtu.be/WTQvfvoOF3g ! Steps o! Determine how many days was it that passed in the question (given) o! Determine how many days is the half life of the element (given) o! Divide the number of days passed by the days of half life o! The result is the half life elapsed of the element which is also your n in the formula ! 9! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Periodic Table ! Watch and memorize o! https://www.youtube.com/watch?v=NP46krFcHsU o! https://www.youtube.com/watch?v=GxxN_bOz-Bc ! Periodic law o! “… states that when elements are arranged in order of increasing atomic number, elements with similar chemical properties occur at periodic intervals.” ! Period o! Horizontal row of elements o! Numbered with Arabic numbers o! Determines energy level/shell o! The same number of valence shells !! Ex. 1s2 2s2 2p6 3s2 3p6 [Argon] !! Highest shell : 3 !! Thus, Argon is in period 3 ! Group/Family o! Vertical column of elements o! Determines the charge o! Elements under the same group have similar properties !! Ex. 1s2 2s2 2p6 3s2 3p6 [Argon] !! Total number of valence electrons : 8 !! Thus, Argon is in group 8A (halogens) o! Distinct groups !! Alkali Metals ! Located on the extreme left side ! Elements in group IA (except Hydrogen) ! Readily reacts with water ! Soft and shiny !! Alkali Earth Metals ! Elements in group IIA ! Soft, shiny ! Moderately reactive toward water !! Halogens ! Extreme right side ! Elements in group VIIA ! Reactive ! Gases at room temp !! Noble Gas ! Elements in group VIIIA ! Stable; unreactive o! Groups IIIB and IVB !! Violated periodic law ! 10! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer ! Elements 58-71 and 90-103 are located below the periodic table to make it more compact ! Classifications o! Metal !! Leftmost !! Majority of elements !! High electrical and thermal conductivity !! Metallic luster !! Almost all are solids !! Ductile and malleable o! Metalloid !! Middle !! Has properties of both o! Nonmetal !! Rightmost !! 23 elements !! Poor electrical and thermal conductivity !! Good insulator !! No metallic luster !! Exists in all phases !! Brittle in solid phase ! O and S: two most abundant elements in the Earth’s crust ! C, H, O, N: most abundant elements in the human body ! 11! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Periodic Table Trends ! Watch o! https://www.youtube.com/watch?v=XK-WTYncldA ! Electronegativity o! A chemical property describing an atom’s ability to attract and bind with electrons o! Measures an atom’s tendency to attract and form bonds with electrons o! Trend !! From left to right across a period of elements, electronegativity increases !! From top to bottom down a group, electronegativity decreases o! Important exceptions of the above rules include the noble gases, lanthanides, and actinides !! The noble gases possess a complete valence shell and do not usually attract electrons !! The lanthanides and actinides possess more complicated chemistry that does not generally follow any trends ! Ionization o! The energy required to remove an electron from a neutral atom in its gaseous phase o! Conceptually, ionization energy is the opposite of electronegativity o! The lower this energy is, the more readily the atom becomes a cation o! The higher this energy is, the more unlikely it is the atom becomes a cation o! Trend !! The ionization energy of the elements within a period generally increases from left to right ! This is due to valence shell stability !! The ionization energy of the elements within a group generally decreases from top to bottom ! This is due to electron shielding o! Note that helium has the highest ionization energy of all the elements ! Electron affinity o! Electron affinity is the ability of an atom to accept an electron o! Unlike electronegativity, electron affinity is a quantitative measurement of the energy change that occurs when an electron is added to a neutral gas atom o! The more negative the electron affinity value, the higher an atom’s affinity for electrons o! Trend !! Electron affinity increases from left to right within a period ! This is caused by the decrease in atomic radius !! Electron affinity decreases from top to bottom within a group ! This is caused by the increase in atomic radius ! Atomic radius o! The atomic radius is one-half the distance between the nuclei of two atoms (just like a radius is half the diameter of a circle) o! Trend ! 12! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer !! Atomic radius decreases from left to right within a period ! This is caused by the increase in the number of protons and electrons across a period ! One proton has a greater effect than one electron ! Thus, electrons are pulled towards the nucleus, resulting in a smaller radius !! Atomic radius increases from top to bottom within a group ! This is caused by electron shielding ! Melting point o! The melting points is the amount of energy required to break a bond(s) to change the solid phase of a substance to a liquid o! Trend !! Metals generally possess a high melting point !! Most non-metals possess low melting points o! The non-metal carbon possesses the highest boiling point of all the elements o! The semi-metal boron also possesses a high melting point ! Metallic character o! The metallic character of an element can be defined as how readily an atom can lose an electron o! Trend !! Metallic characteristics decrease from left to right across a period ! This is caused by the decrease in radius of the atom that allows the outer electrons to ionize more readily !! Metallic characteristics increase down a group ! Electron shielding causes the atomic radius to increase thus the outer electrons ionizes more readily than electrons in smaller atoms o! Metallic character relates to the ability to lose electrons, and nonmetallic character relates to the ability to gain electrons ! 13! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Electron Arrangements ! The space in which electrons move rapidly about a nucleus is divided into subspaces called shells, subshells, and orbitals ! Electron shell o! A region of space about a nucleus that contains electrons that have approximately the same energy and that spend most of their time approximately the same distance from the nucleus o! Numbered 1, 2, 3, and so on, outward from the nucleus o! Electron energy increases as the distance of the electron shell from the nucleus increases o! The higher the shell number (n), the more electrons that can be present ! Electron subshell o! A region of space within an electron shell that contains electrons that have the same energy o! The number of subshells within a shell is the same as the shell number o! The higher the energy of the contained electrons, the larger the subshell o! Size (type) is designated using the letters s, p, d, f in order of increasing energy and size o! Identifying subshells !! The number gives the shell within which the subshell is located !! The letter gives the type of subshell ! Electron orbital o! A region of space within an electron subshell where an electron with a specific energy is most likely to be found o! Can accommodate a maximum of 2 electrons o! Have distinct shapes that are related to the type of subshell in which they are found o! Orbitals within the same subshell, which have the same shape, differ mainly in orientation ! Electron spin o! As an electron moves about within an orbital, it spins on its own axis in either a clockwise or a counterclockwise direction o! When two electrons are present in an orbital, they always have opposite spins ! ! 14! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Electron Configuration ! Three rules for assigning electrons to various shells, subshells, and orbitals o! Electron subshells are filled in order of increasing energy o! Electrons occupy the orbitals of a subshell such that each orbital acquires one electron before any orbital acquires a second electron !! All electrons in such singly occupied orbitals must have the same spin o! No more than two electrons may exist in a given orbital - and then only if they have opposite spins ! Subshell Energy Order o! Energies of subshells in different shells often overlap o! Subshells that belong to the same shell are found in the same row! ! Electron Configuration o! Statement of how many electrons an atom has in each of its electron subshells o! Subshells containing electrons, listed in order of increasing energy, are designated by using number-letter combinations o! A superscript following each subshell designation indicates the number of electrons in that subshell. o! Deal with subshell occupancy ! Orbital diagram o! A notation that shows how many electrons an atom has in each of its occupied electron orbitals. o! Deal with orbital occupancy ! Electronic basis for the configuration o! Chemical properties repeat themselves in a regular manner among the elements because electron configurations repeat ! 15! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Quantum Numbers Principal Quantum Number ! Denoted as n ! The principal quantum number, n, designates the highest electron shell ! When an electron is in an excited state or it gains energy, it may jump to the second principle shell ! This is called absorption because the electron is called absorption because the electron is absorbing photons, or energy ! Known as emission, electrons can also emit energy as they jump to lower principle shells, where n decreases by whole numbers ! As the energy of the electron increases, so does the principal quantum number indicates the third principal shell, n = 4 indicates the fourth principal shell, and so on Angular momentum quantum number ! Denoted as l ! The orbital angular momentum quantum number l determines the shape of an orbital, and therefore the angular distribution ! The value of l is dependent on the principal quantum number n o! Unlike n, the value of l can be zero. It can also be a positive integer, but it cannot be larger than one less than the principal quantum number (n-1) Magnetic quantum number ! Denoted as ml ! Determines the number of orbitals and their orientation within a subshell ! Its value depends on the orbital angular momentum quantum number l ! an interval ranging from –l to +l Electron spin ! Denoted as ms ! Designates the direction of the electron spin and may have a spin of +1/2, represented by , or 1/2, represented by ! This means that when ms is positive the electron has an upward spin, which can be referred to as a spin up When it is negative, the electron has a downward spin, so it is spin down ! Easiest way would be to create an orbital diagram o! If your last electron is pointing down then it is -1/2, if its pointing up then it’s +1/2 ! 16! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Chemical Bonds ! Force that holds the atoms in a compound or molecule ! Nobility of atoms: follows the octet rule ! Helium (He) is an exception for it is stable with only two electrons (duet rule) Ionic bond ! Transfer of electrons between metals and nonmetals ! Weaker than the covalent bond ! Held together by electrostatic forces ! Have hard crystalline solids, water-soluble ! Characteristics o! High melting/boiling point !! Requires high energy to separate ions o! Conducts electricity !! Solids: do not conduct because of lattice !! Liquids: particles are dissociated into ions that move freely o! Solid at room temperature !! Assumes a crystal lattice o! Hard !! Fixed and stable !! Compact lattice o! Brittle !! Breakage/repulsion Covalent bond ! Shares electrons ! Strongly attracted to one another, but molecules are discrete ! Between nonmetals and nonmetals arrangement of elements ! Liquid or gas at room temperature ! Does not conduct electricity ! Cannot be broken down easily Metallic bond ! Type of chemical bonding that rises from the electrostatic attractive force between conduction electrons (in the form of an electron cloud of delocalized electrons) and positively charged metal ions ! May be described as the sharing of free electrons among a structure of positively charged ions (cations) ! Metallic bonding accounts for many physical properties of metals, such as strength, ductility, thermal and electrical resistivity and conductivity, opacity, and luster ! 17! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Balancing Equations Tips ! Save hydrogen and oxygen for last, as they are often on both sides o! Hydrogen and oxygen are both common in molecules, so it’s likely that you’ll have them on both sides of your equation o! It’s best to balance them last ! Start with single elements o! If you have more than one element left to balance, select the element that appears in only a single molecule of reactants and in only a single molecule of products Algebraic method for complicated elements ! Write down the given equation o! For this example, we will use: PCl5 + H2O " H3PO4 + HCl ! Assign a letter to each substance o! aPCl5 + bH2O " cH3PO4 + dHCl ! Check the number of each element found on both sides, and set those equal to each other o! aPCl5 + bH2O " cH3PO4 + dHCl o! On the left side, there are 2b atoms of hydrogen (2 for every molecule of H 2 O), while on the right side, there are 3c+d atoms of hydrogen (3 for every molecule of H 3 PO 4 and 1 for every molecule of HCl) o! Since the number of atoms of hydrogen has to be equal on both sides, 2b must be equal to 3c+d o! Do this for each element !! P: a=c !! Cl: 5a=d !! H: 2b=3c+d ! Solve this system of equations to get the numeric value for all the coefficients. Since there are more variables than equations, there are multiple solutions. You must find the one where every variable is in its smallest, non-fractional form o! To quickly do this, take one variable and assign a value to it. Let’s make a=1. Then start solving the system of equations to get the following values: o! Since P: a = c, we know that c = 1 o! Since Cl: 5a = d, we know that d = 5 o! Since H: 2b = 3c + d, we can calculate b like this !! 2b = 3(1) + 5 !! 2b = 3 + 5 !! 2b = 8 !! b=4 o! This shows us the values are as follows: !! a = 1 !! b = 4 !! c = 1 ! 18! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Acids and Bases Acids ! Produces H + in aqueous solution ! HCl(aq) H+(aq)+Cl2(aq) Bases ! Produces OH- in an aqueous solution ! NaOH(aq) Na+(aq)+OH2(aq) ! ! ! 19! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Electromagnetic Spectrum ! The electromagnetic (EM) spectrum is the range of all types of EM radiation o! Radiation is energy that travels and spreads out as it goes ! Electromagnetic radiation can be expressed in terms of energy, wavelength, or frequency ! Frequency is measured in cycles per second, or Hertz ! Wavelength is measured in meters ! Energy is measured in electron volts Relationships ! Longer wavelength (distance between two troughs or peaks) means lower frequency and lower energy. Lowest energy in the spectrum belongs to radio. ! Shorter wavelength, higher frequency, higher energy. Highest energy belongs to gamma ray. ! Frequency and energy is directly proportional, wavelength and frequency is inversely proportional; wavelength and energy is inversely proportional ! 20! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Stoichiometry ! Branch of chemistry that deals with the relationship between the relative quantities of substances taking part in a chemical reaction Mole ! Amount of substance of a system that contains as many elemental entities (atoms, molecules, or other particles) as there are atoms in 12 grams of carbon-12 isotope ! One mole is equal to avogadro’s number (1 mole = 6. 022 × 1023) ! Avogadro’s number: 6. 0221413 × 1023 Molar mass ! Mass (in grams or kilograms) of 1 mole of units of a substance numerically equal to its atomic mass in atomic mass unit (e.g. Atomic mass of Na [sodium] is 22.99 amu and its molar mass is 22.99 g) ! Molar mass = atomic mass unit ! If one knows the atomic mass of an element, one can know its molar mass knowing the molar mass and Avogadro’s number, one can calculate the mass of a single atom in grams ! Knowing the mass of a single atom in grams can be used to determine the relationship between atomic mass units and grams ! Notions of Avogadro’s number and molar mass can help one convert mass and moles of atoms and vice versa Molecular mass ! Sum of the atomic masses (in amu) in the molecule ! One can determine the molar mass through the molecular mass Percent Composition of Compounds ! Percent by mass of each element in compound Reaction Yield ! Theoretical yield o! Amount of product that would result if all the limiting reagent reacted (maximum obtainable yield) ! Actual yield o! Amount of product actually obtained from a reaction (almost always less than the theoretical yield) ! Percent yield o! Proportion of the actual yield to the theoretical yield ! 21! Downloaded by max goose ([email protected])  lOMoARcPSD|44805057 CREATED BY LeapMedReviewer CHEMISTRY reviewer Gas Laws ! Generalizations regarding the macroscopic behavior of gases Boyle’s Law ! Proposed by Robert Boyle ! Pressure-volume relationship o! The pressure of a fixed amount of gas at a constant temperature is inversely proportional to the volume of gas Charles’ and Gay-Lussac’s Law ! Proposed by Jacques Charles and Joseph Gay-Lussac ! Temperature-volume relationship o! The volume of a fixed amount of gas maintained at a constant pressure is directly proportional to the absolute temperature of gas Avogadro’s Law ! Proposed by Amedeo Avogadro ! Volume-amount relationship o! With constant pressure and temperature, volume of a gas is directly proportional to the number of moles of the gas present Ideal Gas Equation ! Combination of Boyle’s, Charles’ and Gay-Lussac’s, and Avogadro’s Laws ! Describes the relationship among the four variables: pressure, volume, temperature, and amount ! ideal gas o! Hypothetical gas whose pressure-volume-temperature behavior can be completely accounted for by the ideal gas equation ! Standard temperature and pressure o! Conditions 0 degrees Celcius and 1 atm; often abbreviated as STP Dalton’s Law ! Partial pressure o! Pressures of individual gas components in the mixture ! Total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if present alone ! 22! Downloaded by max goose ([email protected])