1.
- evaporation/condensation and freezing/melting points
- ice ⇄ water (solid ⇄ liquid)
- water ⇄ vapor (liquid ⇄ gas)

2.
- forward and reverse reactions happen then slow until they reach the same rate
- reactants and products must remain inside the system

3. each shell within the Bohr model is called a 'principle energy level'; each is made up of sub-levels
- 's' holds max 2 electrons
- 'p' holds max 6
- 'd' holds max 10
- 'f' holds max 14

4. ionic: brackets and charge
covalent: Lewis dot model

5. row on the periodic table
- elements have similar size
-

6.
- requires an electric current
- the anode is positive and the site of oxidation
- the cathode is negative and the site of oxidation
1. energy source gives negative charge to cathode
2. positive metal ions break off of the piece and become aqueous; the electrons are are pulled by the positive side of the battery
3. the positive ions attach to the negatively charged piece and electroplate it

7.
how badly an atom 'wants' an additional electron
1. the element with less shells has a higher electronegativity (closer to nucleus)
2. the element with more protons has a higher electronegativity (stronger negative pull)
- noble gasses have a value of 0

8. Halogens/Halides
- very reactive
- never found alone in nature

9. one pair of electrons are shared (2 total)
*saturated (have the maximum number of H)

10.
heat is added (required)
ex. melting, boiling
* every reaction on a heating curve

11. P₁V₁/T₁ = P₂V₂/T₂
* must be in kelvin
- if a variable stays constant, it can be cancelled out
- all three gas laws can be derived from the combined gas law

12.
the measure of randomness in a system
- more randomness = higher entropy
*high entropy = more chance of collision

13. solid to gas
- only CO₂ and I

14. the simplest definition of acids and bases

15.
separate solid from liquid (no dissolved substances)

16. a physical blend of two or more components; can be physically separated
- homogeneous: same throughout; smooth; no chunks (aqueous is the only mixture; s, g, l, are not)
- heterogeneous: has different regions; chunky

17.
double bonded oxygen somewhere in the MIDDLE of the chain branching off a carbon
ends in -one

18. less bonds = faster
- ionic = faster (than covalent)
(breaking more bonds requires more energy when particles collide)

19.
illustrates the potential energy change during a reaction

20. ions made with more than one atom
- H₂O (water)
- NH₃ (ammonium)
- CH₄ (methane)
*use parenthesis with more than one polyatomic ion

21.
adding one or more atoms at a double or triple bond

22.
a small amount of solute per liter of solute

23.
- some are deflected and some aren't
- lighter particles penetrate farther

24.
- more surface area = faster
(more chances to collide)
*powders react more rapidly than clumps

25. 1. taste bitter
2. have a slippery/soapy feel
3. conduct and electric current
4. react with acids to produce water and a salt
5. react with acid base indicators to change color (litmus turns blue)
*metal + OH ionically bonded