ch 3
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| 1622921667 | polar molecule | molecule (like water) with opposite charges on opposite sides | 0 | |
| 1622921668 | solution | liquid that is homogeneously a mixture of 2+ substances | 1 | |
| 1622921669 | solvent | dissolving agent of a solution | 2 | |
| 1622921670 | solute | substance that is dissolved | 3 | |
| 1622921671 | aqueous solution | soln where water is the solvent | 4 | |
| 1622921672 | cohesion | like molecules stick together (like hydrogen bonds) | 5 | |
| 1622921673 | adhesion | one substance sticks to another | 6 | |
| 1622921674 | hydration shell | sphere of water molecules around each dissolved ion | 7 | |
| 1622921675 | hydrophilic | (ionic or polar) any substance that has an affinity for water | 8 | |
| 1622921676 | hydrophobic | nonionic and nonpolar; repel water vegetable water | 9 | |
| 1622921677 | colloid | stable suspension of fine particles in the air | 10 | |
| 1622921678 | surface tension | how tough it is to break surface of a liquid or stretch it. | 11 | |
| 1622921679 | H20s surface tension | great | 12 | |
| 1622921680 | kinetic energy | energy of motion | 13 | |
| 1622921681 | heat | TOTAL AMOUNT OF KE due to mclr motion in a body of matter | 14 | |
| 1622921682 | temperature | intensity of heat due to the AVERAGE AMOUNT OF KE of mcls | 15 | |
| 1622921683 | evaporative cooling | property of a liquid where surface tension becomes cooler during evaporation | 16 | |
| 1622921684 | why does evaporative cooling happen? | "hottest" mcls (those with greatest KE) are most likely to leave as a gas | 17 | |
| 1622921685 | how does evaporative cooling help environment? | help stabilise temperature in in lakes/ponds helps terrestrial organisms not overheat | 18 | |
| 1622921686 | acid | substance that increases the hydrogen ion concentration of a soln (more h than o) | 19 | |
| 1622921687 | mole | 6.02 x10^23 | 20 | |
| 1622921688 | molarity | moles of solute/L of soln | 21 | |
| 1622921689 | dissociation (separation) | separation of water mcl into a hydrogen ion and hydroxide ion H20 <> H+ + OH- | 22 | |
| 1622921690 | re-fromation of water | H20 > H2 + .5O2 | 23 | |
| 1622921691 | base | substance that reduces hydrogen ion concentration | 24 | |
| 1622921692 | pH | negative logarithm (base 10) of hydrogen ion concentration pH = -log[H+] | 25 | |
| 1622921693 | hydrogen ion | hydrogen atom leaves its electron behind single proton with a charge 1+ | 26 | |
| 1622921694 | hydroxide ion | (OH-) when a water molecule has lost a proton; single proton with a charge of 1- | 27 | |
| 1622921695 | buffers | substances that minimize changes in H+ and OH- in a soln; in biological fluids resist changes in pH. | 28 | |
| 1622921696 | how does a buffer work | accepts hydrogen ions from the soln when they are in excess and donating hydrogen ions to the soon when they have been depleted weak base | 29 | |
| 1622921697 | buffers formula | H- + HCO3- <>H2CO3 <> H20 (L) + CO2 (g) | 30 | |
| 1622921698 | intramolecular bonds | bonds within a molecule covalent bonds - non polar covalent bonds (equal sharing) -polar covalent ionic bonds | 31 | |
| 1622921699 | intermolecular | btwn mcls hydrogen bonds - attraction btwn less electroneg H in one mcl and more electronegative O in another mcl london dispersion | 32 | |
| 1622921700 | strongest to weakest bonds | ionic / polar covalent / np covalent / H / LDF | 33 |
