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| 9134517409 | Ar: strongest LD IMF, largest # electrons | deviates most from ideal behavior |  | 0 |
| 9134523358 | 36.3 is the average molar mass |  | 1 | |
| 9134548359 | they have the same kinetic energy | If all the balloons are at the same temperature, then | | 2 |
| 9134559471 | Hydrogen, smallest molar mass | smallest balloon after 12 hours | | 3 |
| 9134576662 | copper | element | | 4 |
| 9134585058 | B | similar IMFs to solvent |  | 5 |
| 9134591899 | A and D are similar compounds | | 6 | |
| 9134596084 | Contains 1.0 M NH₄Cl |  | 7 | |
| 9134830748 | 1s²2s²2p⁶3s²3p⁶4s²3d¹ |  | 8 | |
| 9134871637 | Sc | element | | 9 |
| 9134877888 | 2 | valence electrons | | 10 |
| 9134888108 | Galvanic cell |  | 11 | |
| 9134905755 | Anode | Silver | | 12 |
| 9134912752 | direction of electrons | left | | 13 |
| 9134922432 | To determine the vapor pressure of the oxygen, you would take the air pressure and subtract the water vapor pressure |  | 14 | |
| 9134974274 | interstitial | B |  | 15 |
| 9135001296 | substitutional | A | | 16 |
| 9135010835 | 0 | order |  | 17 |
| 9135030609 | Rate = k | rate law | | 18 |
| 9135033118 | M/time | k units | | 19 |
| 9135040928 | 1 | order |  | 20 |
| 9135052065 | rate = k[A] | rate law | | 21 |
| 9135054236 | 1/time | k units | | 22 |
| 9135057838 | 2 | order |  | 23 |
| 9135063209 | rate = k[A]² | rate law | | 24 |
| 9135065994 | 1/(M∙time) | k units | | 25 |
| 9135094848 | q = mcΔT (c of ice) | A |  | 26 |
| 9135109612 | q = mHf | B | | 27 |
| 9135111051 | q = mcΔT (c of water) | C | | 28 |
| 9135111052 | q = mHv | D | | 29 |
| 9135112327 | q = mcΔT (c of steam) | E | | 30 |
| 9135773104 | A | if the substance is the same, then this shows a lower temperature |  | 31 |
| 9135774059 | B | if temperature is the same, then this substance has the smaller molar mass | | 32 |
| 9135804048 | 432 | bond energy |  | 33 |
| 9135816183 | 74 | bond length | | 34 |
| 9135825763 | 2 | number of reaction steps |  | 35 |
| 9135843799 | 1 | faster step | | 36 |
| 9135855225 | exothermic | | 37 | |
| 9135859833 | strong acid and weak base | type of titration |  | 38 |
| 9135861051 | 20 mL and pH of 5 | equivalence point | | 39 |
| 9135876654 | 0.032 | Ka = | | 40 |
| 9135879330 | methyl red (pKa = 5.0) | indicator | | 41 |
| 9135899122 | weak acid and strong base | type of titration |  | 42 |
| 9135904726 | 1 x 10⁻⁵ | Ka = | | 43 |
| 9135906943 | 20 mL and pH of 8.5 | equivalence point | | 44 |
| 9135909406 | phenopthalein (pKa = 9.3) | indicator | | 45 |
| 9135928489 | The p orbital is further away from the nucleus so the attraction to the electron in the p orbital is smaller and decreases ionization energy | why B has lower ionization energy than Be |  | 46 |
| 9135929501 | electrons paired up in p orbitals have more repulsion the electrons not paired up. The repulsion makes it easier to remove an electron and lowers the ionization energy | why S has lower ionization energy than P | | 47 |
| 9135929983 | effective nuclear charge increases | Ionization energy generally increases across the period because | | 48 |
| 9135930609 | distance between the nucleus and valence electrons increases due to more energy levels | ionizatio energy decreases down a group because | | 49 |
