definitions and terms

Question 1

osmotic pressure?

Answer 1

the amount of pressure needed to cause osmosis to stop. if not this, the amount of pressure needed to achieve equilibrium - passage of solvent molecules through semipermeable membrane.

Question 2

osmosis?

Answer 2

the flow of a solvent through a semipermeable membrane. from the less concentrated side to the more concentrated side.

Question 3

vapour pressure?

Answer 3

the amount of pressure exerted by the vapour of a liquid in a closed container.

Question 4

colligative properties?

Answer 4

properties that depend on the amount of a dissolved solute but not on its chemical identity.

Question 5

nonvolatile solute?

Answer 5

no appreciable vapour pressure. any ionic compound, strong electrolytes.

Question 6

volatile solute?

Answer 6

significant vapour pressure.

Question 7

saturated solution?

Answer 7

added exact amount to match the solubility.

Question 8

unsaturated?

Answer 8

you have added less than the amount to match solubility.

Question 9

super saturated?

Answer 9

you have added more than amount to match solubility.

Question 10

what temperature does water freeze at?

Answer 10

zero degrees celsius.

Question 11

what temperature does water boil at?

Answer 11

one hundred degrees celsius.

Question 12

solvent?

Answer 12

able to dissolve other substances.

Question 13

solute?

Answer 13

minor component in a solution, dissolved by the solvent.

Question 14

solute to solute interactions?

Answer 14

energy is absorbed (+H) to overcome intermolecular forces holding solute particles together in a crystal. higher lattice energy or charge makes it less soluble.

Question 15

solvent to solvent interactions?

Answer 15

energy absorbed (+H) to overcome intermolecular forces between solvent molecules.

Question 16

solvent to solute interactions?

Answer 16

energy released (-H) when solvent molecules gather around solute particles and solvate them. ionic substances - hydration energy released is greater for smaller cations. hydration energy increases as charge increases.

Question 17

amorphous solid?

Answer 17

doesn’t possess well defined arrangement or long range molecular order.

Question 18

crystalline solid?

Answer 18

possesses rigid and long range order - atoms, ions, molecules occupy a specific predicable position.

Question 19

unit cell?

Answer 19

basic repeating structural unit of a crystalline solid.

Question 20

crystalline?

Answer 20

solids where the atoms ions and molecules are arranged in a well defined and definite repeating pattern.

Question 21

amorphous?

Answer 21

liquid freezes before molecules become arranged in an orderly pattern. examples include glass.

Question 22

simple cubic atom?

Answer 22

atoms on corners only!! 8 corners x 1/8 = 1 atom.

Question 23

body centered atom?

Answer 23

atoms on all 8 corners and 1 in the body. 2 atoms in total.

Question 24

face centered atom?

Answer 24

atoms on all 8 corners, 1 atom on all 6 faces. 4 atoms total.

Question 25

edge atom?

Answer 25

atoms on all 12 edges with 3 atoms in total.

Question 26

entropy (s)?

Answer 26

difference in molecular disorder or randomness between various phases.

Question 27

enthalpy (h)?

Answer 27

heat flow associated with making or breaking intermolecular forces.

Question 28

spontaneous?

Answer 28

once started it will proceed until it reaches equilibrium (-g) dissolves.

Question 29

non spontaneous?

Answer 29

only takes place in presence of an external force. (+g) doesn’t dissolve.

Question 30

critical point?

Answer 30

liquid vapour boundary terminates.

Question 31

triple point?

Answer 31

specific temperature and pressure where all three phases exist at equilibrium.

Question 32

gibbs free energy (g)?

Answer 32

spontaneous reaction or not spontaneous reaction.

Question 33

∆G<0

Answer 33

reaction is spontaneous and in the forward direction.

Question 34

∆G>0

Answer 34

reaction is non spontaneous in the forward direction, spontaneous in the reverse direction.

Question 35

∆G=0

Answer 35

reaction is at equilibrium.

Question 36

how do you calculate grams of compound from density?

Answer 36

multiply the density by the volume.

Question 37

what are the strong electrolytes?

Answer 37

NH4Cl, KOH, HCl.

Question 38

how do you convert grams to micrograms?

Answer 38

multiply mass by 10^6.

Question 39

how do you convert from grams to pictograms?

Answer 39

multiply by 10^12.

Question 40

how do you convert from meters to nanometers?

Answer 40

multiply length by 10^9.