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chem exam 4
| Term | Definition |
|---|---|
| gas mixtures | combination of 2 or more gases, physically blended together w/o chemical reaction |
| vapor pressure | how much a liquid "pushes" upward to become a gas at a certain temperature -high: liquid wants to evaporate alot -low: liquid doesn't evaporate a lot |
| relative humidity | tell you how full the air is with water vapor -how sweaty the air feels |
| evaporation | when liquid turns into a gas -slow, happens at the surface, happens at any temperature -boiling: fast, bubbles form inside the liquid, happens only at specific temp |
| heat of evaporation | amount of energy needed to turn 1 mole of liquid into gas - how much "energy push" you need to separate liquid molecules so they can fly away as gas |
| dynamic equilibrium | happens in a closed container with liquid inside -some molecules evaporate, some condense |
| heating curve | show how temperature changes when you add heat |
| supercritical fluid | what you get when a substance is heated and squeezed past its critical temperature and critical pressure -liquid and gas become same thing |
| sublimation | a solid turns straight into a gas without becoming a liquid first -dry ice or snow |
| fusion | solid turns into a liquid |
| Hfus | amount of energy needed to melt 1 mole of a solid -energy needed to loosen the solid so it can become a liquid |
| phase diagram | chart showing which phase (solid, liquid, gas) a substance is in at different temperature and pressure |
| water | most common liquid on earth and most important -all life depends on it |
| crystallin solid | particles arranged in patterns with long-range repeating order -diamond, sugar crystals, salt |
| amorphous solid | particles randomly distributed without any long-range pattern -plastic, glass, charcoal |
| ionic solid | made of positive and negative ions -intramolecular force: none (ions are separate) -intermolecular force: ionic bonds (very strong) -properties: high melting points, hard but brittle, don't conduct electricity as solids -ex: NaCl, MgO, CaF2 |
| molecular solids | made of neutral molecules held together by weak attractions -intramolecular: covalent bonds (inside each molecule) -intermolecular: weak forces (dipole-dipole, H-bonding) -properties: low melting point, soft, poor electrical conductions -ex: dry ice |
| covalent network solids | made of a giant network of atoms connected by covalent bonds -intramolecular: covalent bonds -intermolecular: none (everything is one big molecule) -properties: extremely high melting points, very hard, don't conduct electricity -ex: diamond, graphite |
| metallic solids | made of metal atoms in a "sea of electrons" -intramolecular/intermolecular: metallic bonding/positive metal ions and free electrons -properties: conduct electricity and heat, malleable, ductile, wide range of melting points -ex: Fe (iron), Cu (copper) |
| parts of solution | solvent- dissolver solute- gets dissolved solution- solute + solvent mixed evenly |
| miscible | when one liquid dissolves into another |
| immiscible | when one liquid does not dissolve into another |
| soluble | can have at least 0.1 M at room temperature of a compound in the solvent before making a saturated solution |
| insoluble | saturated solution is achieved in less than .001 M solutions at room temperature |
| colloid suspensions | particles whose dimensions are between 1 nanometer and 1 micrometer (so there’s a collection of molecules together) used as solute |
| solubility of gases | gases dissolve less when temperature increases and when pressure increases -sugar dissolves better in hot tea than cold tea |
| solubility of solids | most solids dissolve more when the temperature increases -oxygen dissolves in cold water for fish |
| henry's law | the amount of gas that dissolves in a liquid is directly proportional to the pressure of that gas above the liquid |
| colligative properties | properties of solutions that depend ONLY on the number of solute particles, not what the particles are -add particles → boiling point ↑, freezing point ↓, vapor pressure ↓, osmotic pressure ↑ |
| osmosis | movement of solvent molecules through a semipermeable membrane that doesn’t allow solute particles to get through |
| Brønsted-Lowry acids | a proton donor -gives an H⁺ ion. |
| Brønsted-Lowry bases | a proton acceptor -takes an H⁺ ion |
| conjugate acid-base pairs | two substances that differ by one proton (H⁺) -acid donates an H⁺ and becomes its conjugate base -base accepts an H⁺ and becomes its conjugate acid |
| weak acids | don't completely dissociate in water, but donates protons completely to OH- ions -partially dissociate in water |
| strong acids | fully dissociate in water -starts with H ex: HCl, HBr, HI, HNO₃, HClO₃, HClO₄, H₂SO₄ |
| strong bases | group 1 and group 2 hydroxides that dissolve well -fully dissociate in water -Group 1 (LiOH, NaOH, KOH, RbOH, CsOH) -Group 2 (Ca(OH)₂, Sr(OH)₂, Ba(OH)₂) |
| weak bases | partially accept H⁺ -NH₃ – ammonia -Amines (organic bases ending in –NH₂, –NHR, –NR₂) -HCO₃⁻ – bicarbonate ion |
| buffer solutions | a solution that resists changes in pH when small amounts of acid or base are added -keep the pH stable work- needs two parts: a weak acid & its conjugate base made- mix a weak acid with its salt |
| half-life | the time it takes for half of a sample of a radioactive substance to decay |
| nuclear fission | when a heavy nucleus splits into two smaller nuclei, releasing a lot of energy -big nucleus → smaller + energy |
| nuclear fusion | when two light nuclei combine to form a heavier nucleus, releasing even more energy than fission -small nuclei → bigger + energy |
| artificial transmutation | a stable or radioactive nucleus is changed into a different nucleus by bombarding it with particles in a lab or reactor -smash a nucleus with a particle to make a new element or isotope |
Created by:
laneywingo