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Chemistry > Vocab > Flashcards

Vocab Flashcards

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1
Q

Homogeneous solution

A

one phase or uniform throughout

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2
Q

solvent

A

the substance that causes some other substance to dissolve

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3
Q

solute

A

substance that dissolves or breaks apart

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4
Q

polar molecules

A

have positive and negative ends (partial)

can bond to ions in a crystal and can dissolve the ions

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5
Q

hydration

A

when water molecules completely surround the ions

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6
Q

solvation

A

when a solvent has completely surrounded the ion

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7
Q

electrolytes

A

substances that increase the conductivity of the water (Ionic compounds, acids)

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8
Q

strong electrolytes

A

electrolytes that dissociate 100%

conducts water very well

include ionic compounds and strong acids

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9
Q

weak electrolytes

A

electrolytes that ionize partially

weak acids and weak bases

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10
Q

non-electrolytes

A

dissolves in water but does not affect its conductivity

all polar compounds (alcohols, sugars, etc)

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11
Q

dynamic equilibrium

A

when the rate of crystalizing becomes equal to the rate of dissolving

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12
Q

saturated solution

A

when a solution has reached dynamic equilibrium.

when the rate of crystalizing becomes equal to the rate of dissolving

a solution in which the solvent can dissolve no more of a specific solute at a particular temperature

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13
Q

entropy

A

a measure of the randomness or disorder of a system

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14
Q

miscibile

A

liquids that completely dissolve in water in any amount

ex: methanol, ethanol, alcohol

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15
Q

partially miscible

A

liquids that only partially dissolve in each other

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16
Q

immiscible

A

liquids that do not dissolve in each other at all

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17
Q

supersaturated

A

A solution which contains a higher concentration of solute than does a saturated solution at that temperature. Not stable.

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18
Q

factors that impact rates of dissolving

A

Stirring
Increase in heat
Particle size

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19
Q

seed crystal

A

A small crystal (or speck of dirt, or dust) that is put into a supersaturated solution to begin the process of crystalization

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20
Q

solubility

A

Solubility is defined as the maximum quantity of a substance that can be dissolved in another.

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21
Q

non-polar

A

A nonpolar molecule has no separation of charge, so no positive or negative poles are formed. In other words, the electrical charges of nonpolar molecules are evenly distributed across the molecule. Nonpolar molecules tend to dissolve well in nonpolar solvents, which are frequently organic solvents.

ex: oil, gasoline, hexane

does not dissolve well in water

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22
Q

molarity

A

quantitative expression for the number of particles in solution

Basically concentration. number of moles in 1 litre of solution

mol/L

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23
Q

what happens to the moles in the new concentration and volume after diluting a solution?

A

it will have the exact same number of moles

why? I don’t know. It doesn’t make sense to me but It’s the law

24
Q

what are the types of reactions in solution?

A

precipitation reactions
acid-base reactions
oxidation-reduction reactions

25
Q

precipitation reaction

A

double-replacement reactions

reactants are always 2 aqueous solutions

the new combo of ions brings two ions of low solubility into contact with each other

26
Q

process of precipitation

A

when 2 aqueous solutions mix together to form a solid

27
Q

what is an acid?

A

substance that contains a hydrogen and a negative ion (anion) in aqueous solution
OR
substance that dissolves in water to produce hydrogen ions

28
Q

what is a base?

A

a base is a chemical species that donates electrons, accepts protons, or releases hydroxide (OH-) ions in aqueous solution (this definition is from thoughtCO)
ORRR
a substance that contains a metal and hydroxide (ie NaOH)

29
Q

acid-base reaction

A

dbl replacement reaction between an acid and a base

30
Q

what did oxidation mean historically?

A

oxygen was added to a substance

31
Q

what caused the change of the original definition of oxidation?

A

as atomic structure developed, it was realized that the metal atoms were being converted into positive metal ions (losing electrons)

substances other than oxygen (like Cl) can have this same effect on metal atoms!!

32
Q

new definition of oxidation

A

the process at which a species loses electrons

33
Q

historical definition of reduction?

A

when metals were being refined from metal ore

34
Q

new definition of reduction

A

the gaining of electrons

was bc scientists realized that the reduction process actually involves giving electrons to metal ions to make them metal atoms

35
Q

what is oxidation-reduction often referred to?

A

REDOX

36
Q

oxidation numbers/states

A

the apparent “charges” on atoms when sharing equally or unequally in a covalent

37
Q

process of dissolving something

A

polar water molecules have positive and negative ends, so they can bond to ions in a crystal. they can dissolve these ions

the water molecules surround the Ions, which is referred to as hydration

38
Q

the more ions, the lower the…

A

freezing point

39
Q

what kinds of compounds are electrolytes?

A

ionic compounds and acids

40
Q

which phase is the most disorderly?

A

gas phase

41
Q

how does temperature affect the amount of stuff dissolved into GAS

A

high temperature: dissolved gases coming OUT of solution

low temp: more gases being DISSOLVED

solubility decreases as temperature increases!

42
Q

how does pressure affect solubility for liquids and solids

A

they cannot be compressed, so it has no affect

43
Q

how does pressure affect solubility for GASES

A

can be compressed!! more molecules per unit volume at high pressure!

Can turn gas into aqueous!

think of soda!!

44
Q

limiting reagent

A

in a precipitation reaction!

the reactant that ends up giving the least amount of product. basically, it limits what can be produced.

45
Q

when does dissolving occur?

A

when solvent molecules collide with undissolved solute molecules or ions

the solvent bonds to the solute strongly enough to break the bonds between solute particles, drawing the solute into action

46
Q

anything which increases the ____ between SOLUTE and SOLVENT will increases the ___

A

rate of collision

rate of dissolving

47
Q

how does temperature increase rate of dissolving?

A

molecules higher kinetic energy

move faster as a result – greater rate of collision, harder collisions

48
Q

how does particle size increase rate of dissolving?

A

SURFACE AREA increases!!

greater probability and frequency of collisions between solute and solvent

49
Q

how does stirring increase rate of dissolving?

A

simply increases the RATE OF REPLACEMENT

brings fresh solvent into contact with the solution

50
Q

consider a solution in which we have placed a small amount of salt into water. what types of interactions occur?

A

water to water – most likely
water to salt – causes dissolving, 2nd most likely
salt to salt/solute to solute – least likely but OMG CRYSTALIZATION

51
Q

which factors impact SOLUBILITY?

A

stirring– NOPE
surface area–NOPE
Temperature– YES BECAUSE ENTROPY

52
Q

relationship between temperature and entropy?

A

high temperatures favour more entropy, so favours dissolving of a oslid

53
Q

oxidation state of a simple ion is?

A

the same as its charge

54
Q

oxidation state of oxygen?

A

-2

55
Q

exceptions for oxygen

A

H2O2 – oxidation number is -1

OF2 – oxidation number is +1

56
Q

fluorine oxidation state

A

always -1

57
Q

sum of oxidation state is?

A

neutral molecule – 0

polyatomic ion – equal to charge of the ion

Chemistry (5 decks)

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