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Chem 125
Chem 125, all terms
| Question | Answer |
|---|---|
| Soluble or not: NO3- | most nitrate salts are |
| Soluble or not: Contains alkaline metal ions like Li+, Na+, Cs+, Rb+, or NH4+ | most are soluble |
| Soluble or not: chloride, bromide, and iodide salts | most are soluble |
| Soluble or not: salts containing the ions Ag+, Pb2+, or Hg2 2+ | not soluble |
| Soluble or not: sulfate salts | most are soluble |
| Soluble or not: BaSO4, PbSO4, Hg2SO4, and CaSO4 | not soluble |
| Soluble or not: hydroxides | slightly soluble |
| Soluble or not: NaOH and KOH | soluble |
| Soluble or not: Ba(OH)2, Sr(OH)2, Sr(OH)2, Ca(OH)2 | marginally soluble |
| Soluble or not: sulfide (S2-), carbonate (CO32-), chromate (CrO4 2-), or phosphate (PO4-3) | slightly soluble, except for those containing cation like Li+, Na+, etc. |
| oxidation number: all elements in their natural state (Na, Fe, P4, O2, etc.) | 0 |
| Groups 1, 2, and 3 atoms in compounds (Na in NaCl, Mg in MgO, etc) | +1, +2, and +3 |
| Flouring is ALWAYS... | -1 |
| Hydrogen is usually... | +1 |
| Oxygen is usually... | -2 |
| Chlorine is usually... | -1 |
| At STP, the volume of 1 mol of any gas is... | 22.42L |
| energy required to move an object through a given distance (w) | work |
| energy due to position or composition | potential energy |
| energy due to the motion of an object | kinetic energy |
| energy transferred due to difference of temperatures (flows from hot to cold) (q) | heat |
| q>0 | heat moves in, endothermic |
| q<0 | heat moves out, exothermic |
| w>0 | work done on system |
| w<0 | work done by system |
| the quantity of energy required to raise the temperature of a system 1 degree C (C) | heat capacity |
| the head capacity per mole of a substance, units are J/(mol degree C) or J/(mol K) (can use either C or kelvin in this case, because the difference in temperatures will be the same. The subscript p indication that the heat is at constant pressure. (Cp) | molar heat capacity |
| the heat capacity per gram of a substance, units are J/(g degree C) (s or Cs) | specific heat capacity |
| total enthalpy change (delta H) of a reaction equals to the sum of all the enthalpy changes occurring in each step of the reaction | hess's law |
| principal quantum number, integral values from 1 on, "shell" defines energy and extent of the orbital | n |
| angular momentum quantum number, integral values from 0 to n=1, "subshell", defines shape and orbital | l l= 0, s l=1, p l=2, d l=3, f |
| magnetic quantum number integral values between -l and l, defines direction/orientation of the orbital | ml or m |
| electron spin quantum number, is +1/2 (spin up) or -1/2 ((spin down) | ms |
| no two electrons can have the same set of four quantum number, a max of two electrons can occupy a spatial orbital, one with spin up and one with spin down | pauli exclusion principle |
| add electrons, two at a time, to the lowest energy orbitals to obtain the most stable atom | aufbau |
| the lowest energy stat has electrons in separate orbitals of the same energy with spins aligned parallel | hund's rule |
| electrons in outermost shell, shells sometimes not fully-filled | valence electrons |
| non-valence electrons | core electrons |
| describes atoms/ions having identical electron configurations | isoelectronic |
| unequal sharing of electrons in a covalent bond between atoms | polar covalent bond |
| a chemical bond that result from a sharing of outermost electrons | covalent bond |
| a chemical bond resulting from the electrostatic attraction of a cation for an anion | ionic bond |
| different molecular forms of the same element | allotropes |
| molecule with the same chemical formula but different arrangements of atoms in space | isomer |
| two or more lewis structure with the same arrangement of atoms, but different arrangement of bonding pairs of electrons, total number of electrons does not change | resonance structures |
| AX2 | linear, nonpolar |
| AX3 | trigonal planar, nonpolar |
| AX4 | tetrahedral, nonpolar |
| AX5 | trigonal bipyramidal, nonpolar |
| AX6 | octahedral, nonpolar |
| AX7 | pentagonal bipyramidal, nonpolar |
| AX2E1 | bent or angular, polar, E: trigonal planar |
| AX3E1 | trigonal pyramidal, polar, E: tetrahedral |
| AX4E1 | sawhorse or seesaw, polar, E: trigonal bipyramidal |
| AX5E1 | square pyramidal, polar, E: Octahedral |
| AX2E2 | bent or angular, polar, E: tetrahedral |
| AX3E2 | t-shape, polar, E: trigonal bipyramidal |
| AX4E2 | square planar, nonpolar, E: octahedral |
| AX2E3 | linear, nonpolar, E: trigonal bipyramidal |
| AX3E3 | t-shape, polar, E: octahedral |
| AX2E4 | linear, nonpolar, E: octahedral |
| hybridization: sp number of sigma bonds: ? | 2 |
| hybridization: sp 2 number of sigma bonds: ? | 3, 2 |
| hybridization: sp 3 number of sigma bonds: ? | 4, 3, 2 |
| hybridization: sp 3 d number of sigma bonds: ? | 5, 4, 3, 2 |
| hybridization: sp 3 d 2 number of sigma bonds: ? | 6, 5, 4 |
| a bond formed when the electron pair is shared in an area centered on a line running between the atoms | sigma bond |
| a covalent bond in which electrons density is greatest around - not along - the bonding axis, formed by overlap of unhybridized p orbitals | pi bond |
| forces within molecules, ex: covalent bonds | intramolecular forces |
| forces between molecules | intermolecular forces |
| strong intermolecular forces have... | high melting and boiling points |
| attractive force between polar molecules | dipole-dipole interactions |
| strongest dipole-dipole interaction, occurs between H atom bonded to a small, highly electronegative element 9f, O, N) and an atom of F, O, or N in another molecular | hydrogen bonds |
| intermolecular forces between molecules or atoms caused by the presence of temporary dipoles in molecules, present in all atoms | dispersion (london) forces |
| factors affection reaction rates: | physical stat of reactance, concentration of reactants, temp, presence of a catalyst |
| defines the relationship between the initial instantaneous rate of a reaction and the initial concentrations of reactants | rate law |
| the time in the course of a chemical reaction during which the concentration of a reactant decreases by half | half-life |
| the minimum energy the reactant molecules must have to react when they collide | activation energy |
| a high-energy state between reactants and products in a chemical reaction | transition state |
| Le Chatelier's Principle: increase concentration | shifts to opposite side, no change in Kc |
| Le Chatelier's Principle: decrease concentration | shifts to same side, no change in kc |
| Le Chatelier's Principle: increase pressure, thus decrease volume | shifts to side with lease moles of gas, no change in kc |
| Le Chatelier's Principle: decrease pressure, increase volume | shifts to side with most moles of gas, no change in kc |
| Le Chatelier's Principle: increase temperature | shifts to endothermic direction, yes chang e in kc |
| Le Chatelier's Principle: decrease temperature | shifts to exothermic direction, yes change in kc |
| Le Chatelier's Principle: add a catalyst | no change, no change in kc |
| Bronsted-Lowry, proton donor | acid |
| Bronsted-Lowry, proton acceptor | base |
| a molecule or ion that functions as either an acid or a base depending on reaction conditions (ex: water) | amphiprotic/amphoteric |
| a solution that maintains approximately constant pH upon small additions of acid or base | buffer solution |
| the greatest amount of a substance that will dissolve in equilibrium in a specified volume of solvent at a specific temp (g/L or Mol/L) | solubility |
| consist of a central metal atom or ion, with other groups called ligands bonded to it | complex ion |
| entropy increase when... | temp increases, volume increases, the number of independent particles increases, when a molecule is broken into two, increase in moles of gas, when a solid changes to a liquid or gas |
| delta Gsys<0 | spontanous |
| delta Gsys>0 | nonspontaneous |
| delta Gsys=0 | equilibrium |
| Q<K | forward rxn is spontaneous |
| Q>K | forward rxn is nonspontaneous |
| Q=K | forward rxn is at equilibrium |
| transform chemical energy into electrical work | galvanic/voltaic |
| an electrode at which an oxidation half-reaction takes place | anode |
| an electrode at which a reduction half reaction takes place | cathode |
| number of atoms + lone pairs = 2 | sp, 180 degree |
| number of atoms + lone pairs = 3 | sp2, 120 degree |
| number of atoms + lone pairs = 4 | sp3, 109.5 degree |
| number of atoms + lone pairs = 5 | sp3d, 90 degree & 120 degree |
| number of atoms + lone pairs = 6 | sp3d2, 90 degree (all) |
| Units for K: 0 | Ms-1 |
| Units for K: 1 | s-1 |
| Units for K: 2 | M-1s-1 |
| Units for K: 3 | M-2s-1 |
| when n=2, what are the other possible quantum numbers and number of electrons | l = 0, 1 m= -1, 0, 1 electrons (2n^2): 8 |
| when n=3, what are the other possible quantum numbers and number of electrons | l=0, 1, 2 m= -2, -1, 0, 1, 2 electrons (2n^2) = 18 |
| when n=4, what are the other possible quantum numbers and number of electrons | l=0, 1, 2, 3 m= -3, -2, -1, 0, 1, 2, 3 electrons (2n^2) = 32 |
| when n=5, what are the other possible quantum numbers and number of electrons | l=0, 1, 2, 3, 4 m= -4 ,-3, -2, -1, 0, 1, 2, 3, 4 electrons (2n^2)= 50 |
| when n=3, ms=+1/2 what are number of electrons | normally would have 18 but half will have an up and half down, so, electrons (2n^2)1/2 = 9 |
| when n=4, ms=+1/2 what are number of electrons | electrons (2n^2)1/2=16 |
| when n=2, ms=+1/2 what are number of electrons | electrons (2n^2)1/2= 4 |
| when n=3, l=2 what are number of electrons | n=3 and l= d sublevel: 3d, max 10 electrons electrons = 10 |
| when n=4, l=3 what are number of electrons | n=4 and l= f sublevel: 4f, max 14 electrons electrons = 14 |
| when n=4, ml=1 what are number of electrons | n=4 and ml is the orbital in the sublevel, so it can be the 1 orbital for 4s, 4p, 4d, and 4f, where the last three have a 1 orbital that holds two electrons electrons = 6 |
| when n=5, ml=3 what are number of electrons | n=5 and ml is the orbital in the sublevel, so it can be the 1 orbital for 5s, 5p, 5d, 5f, and 5g, where the last two have a 1 orbital that holds two electrons electrons= 4 |
| when n=3, l=2, ml=0 what are number of electrons | n=3, l=d, 3d, which has five orbitals and one 0 orbital electrons:2 |
| when n=4, l=3, ml=1, ms=-1/2 what are the number of electrons | 1 electrons |
Created by:
epmartin17
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