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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?

Study These Flashcards
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?

Study These Flashcards
A

precipitation reactions
acid-base reactions
oxidation-reduction reactions

25
precipitation reaction
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
process of precipitation
when 2 aqueous solutions mix together to form a solid
27
what is an acid?
substance that contains a hydrogen and a negative ion (anion) in aqueous solution OR substance that dissolves in water to produce hydrogen ions
28
what is a base?
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
acid-base reaction
dbl replacement reaction between an acid and a base
30
what did oxidation mean historically?
oxygen was added to a substance
31
what caused the change of the original definition of oxidation?
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
new definition of oxidation
the process at which a species loses electrons
33
historical definition of reduction?
when metals were being refined from metal ore
34
new definition of reduction
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
what is oxidation-reduction often referred to?
REDOX
36
oxidation numbers/states
the apparent "charges" on atoms when sharing equally or unequally in a covalent
37
process of dissolving something
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
the more ions, the lower the...
freezing point
39
what kinds of compounds are electrolytes?
ionic compounds and acids
40
which phase is the most disorderly?
gas phase
41
how does temperature affect the amount of stuff dissolved into GAS
high temperature: dissolved gases coming OUT of solution low temp: more gases being DISSOLVED solubility decreases as temperature increases!
42
how does pressure affect solubility for liquids and solids
they cannot be compressed, so it has no affect
43
how does pressure affect solubility for GASES
can be compressed!! more molecules per unit volume at high pressure! Can turn gas into aqueous! think of soda!!
44
limiting reagent
in a precipitation reaction! the reactant that ends up giving the least amount of product. basically, it limits what can be produced.
45
when does dissolving occur?
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
anything which increases the ____ between SOLUTE and SOLVENT will increases the ___
rate of collision rate of dissolving
47
how does temperature increase rate of dissolving?
molecules higher kinetic energy move faster as a result -- greater rate of collision, harder collisions
48
how does particle size increase rate of dissolving?
SURFACE AREA increases!! greater probability and frequency of collisions between solute and solvent
49
how does stirring increase rate of dissolving?
simply increases the RATE OF REPLACEMENT brings fresh solvent into contact with the solution
50
consider a solution in which we have placed a small amount of salt into water. what types of interactions occur?
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
which factors impact SOLUBILITY?
stirring-- NOPE surface area--NOPE Temperature-- YES BECAUSE ENTROPY
52
relationship between temperature and entropy?
high temperatures favour more entropy, so favours dissolving of a oslid
53
oxidation state of a simple ion is?
the same as its charge
54
oxidation state of oxygen?
-2
55
exceptions for oxygen
H2O2 -- oxidation number is -1 OF2 -- oxidation number is +1
56
fluorine oxidation state
always -1
57
sum of oxidation state is?
neutral molecule -- 0 | polyatomic ion -- equal to charge of the ion

Chemistry (5 decks)

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