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| 13721359020 | Avogadro's number | 6.02 x 10^23 | 0 | |
| 13721361482 | Ideal Gas Law | PV=nRT P = pressure V = volume n = moles of gas R = gas constant: .0821 L*atm/mol*K T = temperature (K) | 1 | |
| 13721375558 | STP | P = 1 atm T = 273K 1 mole = 22.4 L | 2 | |
| 13721384512 | Percent Composition | the percent by mass of each element in a compound mass of element/total molar mass of the substance | 3 | |
| 13721405305 | Empirical Formula | a formula with the lowest whole-number ratio of elements in a compound 1) assume 100 gram sample (percentage-->gram) 2) convert the gram amount to mol of element 3) take the lowest mol amount and divide each number by that value 4) round to the nearest whole number 5) these values become the subscript | 4 | |
| 13721432840 | Molecular Formula | A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms. 1) find molar mass of the empirical formula 2) molar mass of MF/molar mass of EF 3) multiply all the subscript in the empirical formula by that value | 5 | |
| 13721466372 | Aufbau Principle | the rule that electrons occupy the orbitals of lowest energy first | 6 | |
| 13721470194 | Pauli Exclusion Principle | states that a maximum of two electrons can occupy a single atomic orbital but only if the electrons have opposite spins | 7 | |
| 13721474793 | Hund's Rule | states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals | 8 | |
| 13721486107 | Coulomb's Law | E=kq1q2/r^2 E = energy k = Coulombs Constant: 8.988*10^9 Nm^2/C^2 q1 (+) = magnitude of the positive charge (nucleus) q2 (-) = magnitude of the negative charge (electron) r = distance between the charges *the greater charge of the nucleus the more energy an electron will have | 9 | |
| 13721523183 | Quantum Theory | describes mathematically the wave properties of electrons and other very small particles quantum: E = hv | 10 | |
| 13721535493 | The Bohr model | model of the atom in which electrons move rapidly around the nucleus in paths called orbits * the closer the energy level is to the atom the less energy electrons that level has | 11 | |
| 13730998731 | Energy and Electromagnetic Radiation | △E = hv = hc/λ △E = energy change h = planck's constant: 6.63x10^-34 joule*sec v = frequency of radiation λ = wavelength of radiation c = speed of light: 3.00x10^8 m/sec *high frequency and shorter wavelength lead to more energy | 12 | |
| 13731022520 | Frequency and Wavelength | c = λv c = speed of light: 3.00x10^8 m/sec λ = wavelength of radiation v = frequency of radiation | 13 | |
| 13731032861 | Ionization Energy | The amount of energy required to remove an electron from an atom | 14 | |
| 13731039833 | Photoelectron Spectroscopy (PES) | energy measurement of electrons emitted from solids, gases or liquids by the photoelectric effect, in order to determine the binding energies of electrons in a substance *decreases from left to right | 15 | |
| 13731051094 | Electron Configuration | the arrangement of electrons in the orbitals of an atom | 16 | |
| 13731053673 | Dalton's Atomic Theory | 1) elements are composed of atoms. 2) atoms of same element are identical, but differ from other elements. 3) elements can mix together 4) atoms only change when mixed with other elements | 17 | |
| 13731061952 | J.J. Thomson's Model | Plum pudding model *atoms are composed of positive and negative charges. negative charges are called electrons and they are sprinkled throughout the positively charged atom | 18 | |
| 13731068832 | Ernest Rutherford | Gold foil experiment *positive charge in an atom is concentrated in the center and the atom is mostly empty space...positive charged nucleus (mass) and negatively charged electrons travel around the nucleus | 19 | |
| 13731076991 | Heisenberg Uncertainty Principle | it is impossible to know exactly both the velocity and the position of a particle at the same time | 20 | |
| 13731079184 | Periodic Trend: Atomic Radius | increases left and down *increases left less protons so weaker attraction *increases down because more electrons are added to the electron shells | 21 | |
| 13731323455 | Periodic Trend: Ionization Energy | increase right and up *increases to the right because more protons so stronger attraction *increases up because less shielding so more attraction | 22 | |
| 13731328515 | Periodic Trend: Electronegativity | increases right and up *increases to the right because more protons so stronger attraction *increases up because less shielding so more attraction | 23 | |
| 13731332983 | Periodic Trend: Electron Affinity | increases right and up *energy releases or absorbed when the electron is added in th eatom | 24 | |
| 13731333698 | Periodic Trend:Ionic Radius | increase left and down *more electrons the larger the radius | 25 | |
| 13734711391 | Isoelectronic | having the same number of electrons *largest will be element with less protons | 26 | |
| 13734736525 | Exception for Ionization Energy | Between Be B and N and O *further away more shielding so less attraction *O has to electrons in one orbital so there electron-electron repulsion | 27 | |
| 13737927533 | Bonding | transfer or sharing of electrons | 28 | |
| 13737930749 | Ionic Bonds | the electrostatic forces that hold ions together in ionic compounds *metal and none metal (electrons are NOT shared) *cation--gives up and electron and becomes positively charged *anion--accepts and electron and becomes negatively charged *solid at room temp and have high MP and BP | 29 | |
| 13737964300 | Lattice Energy | the energy required to separate 1 mol of the ions of an ionic compound *greater charge = greater lattice energy = high MP *small ion(radius) = high MP | 30 | |
| 13737980777 | Metallic Bonds | a bond formed by the attraction between positively charged metal ions and the electrons around them *malleable, ductile, good conductors of electricity | 31 | |
| 13737990469 | Interstitial Alloy | an alloy whose component atoms are different sizes |  | 32 |
| 13737993106 | Substitutional Alloy | an alloy whose component atoms are similar in size |  | 33 |
| 13737997558 | Covalent Bonds | bonds created by sharing electrons with other atoms *first covalent bond between two atoms is called a sigma (σ) bond and additional bonds are called pi (π) bonds *double and triple bonds are stronger and shorter than single bonds | 34 | |
| 13738029893 | Network Covalent Bonds | atoms held together in lattice of covalent bonds (diamond); hard with high melting point | 35 | |
| 13738077503 | Polarity | molecules having an uneven distribution of charges *the most electronegative atoms exerts the most pull |  | 36 |
| 13738115509 | Intermolecular Forces | forces that exist between molecules in a covalently bonded substance *need to be broken to change phases *when ionic substances change phase the bonds between the individual ions are broken *when covalent substances change phase the bonds between the individual atoms remain but the forces that hold the molecules to other molecules breaks | 37 | |
| 13740188728 | Dipole-Dipole Forces | forces of attraction between polar molecules *molecules with greater polarity will have a greater dipole moment--higher MP and BP *relatively weak and low MP and BP | 38 | |
| 13740197766 | Hydrogen Bonds | a special type of dipole-dipole moment. positive hydrogen atom attracted to negatively charged element (NOF) | 39 | |
| 13740204904 | London Dispersion Forces | occur between all molecules. the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles. *since LD depends on the random motion of electrons--more electrons = more LD | 40 | |
| 13740219835 | Bond Strength | ionic--solids at room temp covalent--liquids at room temp (low MP and BP) metallic--often involves one type of atom, very strong(high MP and BP) network covalent--strongest type of bonding so extremely difficult to melt | 41 | |
| 13740232060 | Bonding and Phases | phase of a substance if directly related to the strength of its IMF. weak IMF=gas at room temp. strong IMF=liquid at room temp. ionic substances do no experience IMF (phase determined by ionic bonding (STRONG))=solid at room temp. solids--packed together liquid--loose gas--spread apart | 42 | |
| 13740255873 | Vapor Pressure | molecules within a liquid are in constant motion but if the molecules hit the surface with enough KE they can break their IMF and become gas. strong IMF=low vapor pressure bc of high temp required | 43 | |
| 13740266672 | Lewis Dot Structure | diagram of a molecule using dots to represent valence electrons | 44 | |
| 13740270315 | Resonance Structure | one of the two or more equally valid electron dot structures of a molecule or polyatomic ion | 45 | |
| 13740273232 | Bond Order | 46 | ||
| 13740283098 | Incomplete Octet | These elements are stable with fewer than eight electrons in their valence shell and include hydrogen (2), helium (2), lithium (2), beryllium (4), and boron (6). |  | 47 |
| 13740282163 | Expanded Octet | An exception to the octet rule that permits atoms in d block or lower on the periodic table to have more than eight electrons in a Lewis structure. |  | 48 |
| 13740329788 | Formal Charge | used to determine which resonance structure is more likely. # of valence electrons - ( # lone pairs + # bonds) (each lone pair is 2 and each bond is one) *charges should at up to total molecule charge *the most electronegative element should possess the negative charge if there is one | 49 | |
| 13740355089 | Molecular Geometry | electrons repel each other so when atoms come together they will assume a shape that keeps its electron pairs far apart *valence shell electron-pair repulsion (VESPR) *double and triple bonds are treated the same way as a single bond when predicting molecular geometry *molecules with lone pairs will have reduced angles | 50 | |
| 13740379837 | Hybridization: 2 electron pairs | sp | 51 | |
| 13740379838 | Hybridization: 3 electron pairs | sp^2 | 52 | |
| 13740381627 | Hybridization: 4 electron pairs | sp^3 | 53 | |
| 13740382346 | Hybridization: 5 electron pairs | dsp^3 | 54 | |
| 13740383346 | Hybridization: 6 electron pairs | d^2sp^3 | 55 | |
| 13740383863 | Kinetic Molecular Theory | based on the idea that particles of matter are always in motion *the greater the temperature the greater average kinetic energy of gas molecules | 56 | |
| 13740391171 | The Average Kinetic Energy of a Single Gas Molecule | KE = 1/2 mv^2 or v = √(3RT)/(m) KE = kinetic energy m = mass v = volume R = gas constant (.0821) T = temperature | 57 | |
| 13740456007 | Maxwell-Botzmann Diagrams | a diagram that shows the range of velocities for molecules of a gas. molecules at a given temperature are not all moving at the same velocity *higher temperature of gas-->larger range for velocity (higher KE) | 58 | |
| 13740803354 | Boyle's Law | P1V1=P2V2 | 59 | |
| 13740803355 | Charles Law | V1/T1=V2/T2 | 60 | |
| 13740806620 | Combined Gas Law | P1V1/T1=P2V2/T2 | 61 | |
| 13740807089 | Gay-Lussac's Law | P1/T1=P2/T2 | 62 | |
| 13740807959 | Dalton's Law | total pressure of a mixture of gases is just the sum of all the partial pressure P total=P1+P2+P3... | 63 | |
| 13740812947 | Partial Pressure | Pa = (P total)(Xa) Xa = (moles of gas A/total moles of gas) | 64 | |
| 13740816971 | Density | D = m/v D = density m = mass of gas in grams v = volume occupied by gas in liters D = P(MM)/RT MM = D(RT)/P | 65 | |
| 13740824089 | Molarity | expresses the concentration of a solution in terms of volume. the number of moles of solute per liter of solution M = moles of solute/liters of solution | 66 | |
| 13740827809 | Mole Fraction | The ratio of the moles of solute in solution to the total number of moles of both solvent and solute Mole Fraction (X) = moles of substance S/total number of moles in the solution | 67 | |
| 13740829581 | Solutes and Solvents | LIKE DISSOLVES LIKE AKA polar or ionic solutes like salt will dissolve in polar solvents like water. non polar dissolves non polar. | 68 | |
| 13740831182 | Dissociation | the separation of ions that occurs when an ionic compound dissolves | 69 | |
| 13740832566 | Paper Chromatography | method of separating a mixture of different colors. The liquid soaks through the paper and carries the mixture with it. Some substances are carried faster than others so the substances are separated along the paper | 70 |
