Terms : Hide Images
| 13266873574 | HCl | hydrochloric acid | 0 | |
| 13266873575 | HBr | hydrobromic acid | 1 | |
| 13266878223 | HI | hydroiodic acid | 2 | |
| 13266881275 | HNO3 | nitric acid | 3 | |
| 13266883488 | H2SO4 | sulfuric acid | 4 | |
| 13266886404 | HClO4 | perchloric acid | 5 | |
| 13266889416 | HClO3 | chloric acid | 6 | |
| 13266895732 | HCl | strong acid | 7 | |
| 13266898201 | HBr | strong acid | 8 | |
| 13266898202 | HI | strong acid | 9 | |
| 13266902041 | HNO3 | strong acid | 10 | |
| 13266904647 | H2SO4 | strong acid | 11 | |
| 13266907582 | HClO4 | strong acid | 12 | |
| 13266910046 | HClO3 | strong acid | 13 | |
| 13266917018 | HF | hydrofluoric acid | 14 | |
| 13266919720 | HF | weak acid | 15 | |
| 13266922567 | Organic acids are [weak/strong] acids | weak acids | 16 | |
| 13266934012 | The oxidation number of a free element is always _____ | 0 | 17 | |
| 13266939609 | The oxidation number of a monatomic ion equals _______________________ | the charge of the ion | 18 | |
| 13266943898 | The oxidation number of H is [a], but it is [b] when combined with less electronegative elements | a) +1 b) -1 | 19 | |
| 13266954198 | The oxidation number of O in compounds is usually [a], but it is [b] in peroxides | a) -2 b) -1 | 20 | |
| 13266961169 | Peroxides | compounds with negative charges (O22-) | 21 | |
| 13266964334 | The oxidation number of a Group 1 element in a compound is ____ | +1 | 22 | |
| 13266969786 | The oxidation number of a Group 2 element in a compound is ____ | +2 | 23 | |
| 13266974421 | The oxidation number of a Group 17 element in a binary compound is ____ | -1 | 24 | |
| 13266980834 | Binary compound | substance composed of only two different elements | 25 | |
| 13266984462 | The sum of the oxidation numbers of all of the atoms in a neutral compound is _____ | 0 | 26 | |
| 13266984463 | The sum of the oxidation numbers in a polyatomic ion is equal to ____________________ | the charge of the ion | 27 | |
| 13266995954 | Electronegativity | A measure of the tendency of an atom to attract a bonding pair of electrons | 28 | |
| 13267004187 | Electronegativity trend | From fluorine to chlorine to bromine, the valence electrons are further away from the nucleus and are not as attracted to the nucleus. | 29 | |
| 13267176857 | Polar Bonds | a covalent bond in which electrons are shared unequally | 30 | |
| 13267181538 | an electronegativity difference ≥ 0.5 means the bond is | polar | 31 | |
| 13267196317 | Nonpolar Bonds | a covalent bond in which electrons are shared equally | 32 | |
| 13267204552 | Tetrahedral | 109.5 |  | 33 |
| 13267209940 | Trigonal planar | 120 |  | 34 |
| 13267213049 | Square planar | 90 |  | 35 |
| 13267215693 | Linear | 180 |  | 36 |
| 13267222989 | Dipole-dipole | attractive forces between the positive end of one polar molecule and the negative end of another polar molecule When a molecule is polar, it will most likely have dipole-dipole forces | 37 | |
| 13267227030 | London dispersion forces | All molecules will have dispersion forces between them Sometimes described as the weakest force, depends on the number of electrons and their polarizability (how spread out they are). | 38 | |
| 13267229926 | Hydrogen bonding | Very strong force that bonds together Hydrogen to either Nitrogen, Fluorine, or Oxygen (Hydrogen Bonds are FON) | 39 | |
| 13267237668 | Ion-dipole interactions | Attraction between an ion in solution and a polar solvent molecule (such as the sphere of hydration - an ion surrounded by polar molecules like a sphere of hydration) | 40 | |
| 13267245296 | Melting points and boiling points are higher with [stronger/weaker] intermolecular forces. | stronger | 41 | |
| 13267249647 | Vapor pressures are lower with [stronger/weaker] intermolecular forces. | stronger | 42 | |
| 13267252276 | Solubility Rules | All nitrate (NO3-) salts, all salts of Group I Cations (*EXCEPT* Li occasionally) and ammonium (NH4+) | 43 | |
| 13267278341 | Effective nuclear charge | pull of the nucleus on the valence electrons (taking shielding electrons into account) | 44 | |
| 13267289289 | Periodic Trend: Effective Nuclear Charge | approximately the same for all elements in a group, increases across the period. | 45 | |
| 13267295782 | Principal energy level of valence electrons | in the quantum mechanical model it is the highest coefficient (ex. The 4 in 4s2) | 46 | |
| 13267306640 | Periodic Trend: Principal energy level of valence electrons | When it increases (moving down the group), so does the atomic radius. | 47 | |
| 13267306641 | Periodic Trend: Atomic radius | Across the period: decreases more protons = a stronger nuclear charge (and same amount of electron shielding) = a stronger pull on the electrons = electrons come closer to nucleus Down the group: increases the principal energy level increases (adding more shells of electrons) | 48 | |
| 13267317935 | Periodic Trend: Electronegativity | Across the period: increases the effective nuclear charge increases - they have a stronger pull on their electrons and are more likely to attract new ones. they have more electrons in their valence shell it is easier to fill the shell by gaining rather than losing electrons Down the group: decreases as the principal energy level increases, they do not have as strong of a hold on their electrons and are less likely to attract more (the shell becomes bigger and the valence electrons are farther away from the nucleus). Exceptions: noble gases have a full valence shell and do not tend to attract electrons | 49 | |
| 13267327064 | Ionization energy | the energy required to remove a valence electron from an atom | 50 | |
| 13267330113 | Periodic trend: Ionization Energy | Across the period: increases the atoms have a greater nuclear charge (a stronger pull on their electrons) so it's harder to remove them Down the group: decreases the atoms have a greater atomic radius and less pull on their electrons so it's easier to remove them | 51 | |
| 13267342341 | Electron affinity | the numerical value of the ability of an atom to accept an electron (in KJ/mol) - the energy that is released or absorbed when an electron is added to a neutral atom | 52 | |
| 13267346869 | Periodic Trend: Electron affinity | Across the period: increases the atomic radius decreases Down the group: decreases the atomic radius increases | 53 | |
| 13267413482 | Ionic Compound: Types of atoms involved | metal and nonmetal | 54 | |
| 13267416863 | Covalent Compound: Types of atoms involved | 2 nonmetals | 55 | |
| 13267420042 | Metallic Compound: Types of atoms involved | 2 metals | 56 | |
| 13267424150 | Ionic Compound: Melting Point | High | 57 | |
| 13267427085 | Covalent Compound: Melting Point | Low (molecules) High (Network Covalent) | 58 | |
| 13267434066 | Metallic Compound: Melting Point | Very High | 59 | |
| 13267438660 | Ionic Compound: Structure | Crystalline Alternating (+)(-)(+) (-)(+)(-) (+)(-)(+) | 60 | |
| 13267448022 | Covalent Compound: Structure | Small molecules (as drawn with Lewis structures) Macromolecules (like proteins) Network of bonds through sharing electrons (eg. allotrope of carbon, silicon dioxide) | 61 | |
| 13267467394 | Metallic Compound: Structure | Crystalline Alternating (+)(-)(+) (-)(+)(-) (+)(-)(+) | 62 | |
| 13267472422 | Ionic Compound: Coulombic Attraction Between | Cations (+) and Anions (-) | 63 | |
| 13267481001 | Covalent Compound: Coulombic Attraction Between | Two nuclei (+) and shared electrons (-) | 64 | |
| 13267486857 | Metallic Compound: Coulombic Attraction Between | Cations (+) and the sea of delocalized valence electrons (+) | 65 | |
| 13267500868 | Ionic Compound: Bond Strength Increases With | Smaller atomic radius (closer together) and the higher the charge of the cation | 66 | |
| 13267505227 | Covalent Compound: Bond Strength Increases With | Smaller atomic radius (closer together) and more shared electrons within the same atoms | 67 | |
| 13267514736 | Metallic Compound: Bond Strength Increases With | An increased number of valence electrons | 68 | |
| 13267518511 | Ionic Compound: Conductivity | only when molten or dissolved | 69 | |
| 13267522082 | Covalent Compound: Conductivity | no conduction (except the sp2 hybrid carbon allotropes ie: graphite/graphene) | 70 | |
| 13267542747 | Metallic Compound: Conductivity | Good conduction (electrons can move) | 71 | |
| 13267549339 | Ionic Compound: Conducts as solid | no | 72 | |
| 13267549340 | Covalent Compound: Conducts as solid | no | 73 | |
| 13267551693 | Metallic Compound: Conducts as solid | yes | 74 | |
| 13267551694 | Ionic Compound: Conducts as liquid | yes | 75 | |
| 13267554437 | Covalent Compound: Conducts as liquid | no | 76 | |
| 13267554438 | Metallic Compound: Conducts as liquid | yes | 77 | |
| 13267557322 | Ionic Compound: Conducts as a solution | yes | 78 | |
| 13267557323 | Metallic Compound: Conducts as a solution | n/a | 79 | |
| 13267559586 | Covalent Compound: Conducts as a solution | no | 80 | |
| 13267561895 | Ionic Compound: Conducts as a gas | yes | 81 | |
| 13267561897 | Covalent Compound: Conducts as a gas | no | 82 | |
| 13267567655 | Metallic Compound: Conducts as a gas | yes | 83 | |
| 13267574175 | 1 mol of any gas is ____L at STP | 22.4 | 84 | |
| 13267574176 | MM = | dRT/P | 85 | |
| 13267586664 | 0th Law of Thermodynamics | If two systems are in thermal equilibrium with a third system, they are also in thermal equalibrium with each other | 86 | |
| 13267594258 | 1st Law of Thermodynamics | The energy of the universe is constant | 87 | |
| 13267596371 | 2nd Law of Thermodynamics | In any spontaneous process there is always an increase in the entropy of the universe, ieΔsuniv>0 for a spontaneous process | 88 | |
| 13267598611 | 3rd Law of Thermodynamics | The entropy of a perfect crystal at 0 K is zero ` | 89 | |
| 13267602969 | Metal + Water = | Metal Hydroxide (base) + H2 | 90 | |
| 13267602970 | Non-metal + Water = | Acid | 91 | |
| 13267605466 | Equimolar: | equal concentrations | 92 |
