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College Chem I > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

define electrolyte

A

comp that dissolves & dissociates into ions when dissolved in H₂O

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2
Q

define nonelectrolyte x 2

A
  • COV comp NOT dissociating into ions when dissolved

- don’t conduct electricity (?)

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3
Q

define strong electrolyte x 4

A
  • 100% dissociation
  • →
  • ION comps dissolving in H₂O = strong
  • AKA strong acid/base
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4
Q

define weak electrolyte x 4p

A
  • partial dissociation
  • ⇌
  • equilibrium: forward react rate = reverse react rate
  • AKA weak acid/base & reversible rxn
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5
Q

6 strong acids

A
  • HCl
  • HBr
  • HI
  • HNO₃
  • H₂SO₄
  • HClO₄
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6
Q

how to ID strong bases, exceptions

A
  • soluble ion OH⁻ comps on solubility table

- exceptions = Ca, Sr, Ba

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7
Q

4 times when something is always soluble

A
  • NO₃⁻
  • C₂H₃O₂⁻
  • NH₄⁺
  • alkali metal ions
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8
Q

define arrhenius base

A

comp forming OH⁻ ions in a solution

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9
Q

write that freaking rxn for weak bases

A

NH₃ (aq) + H₂O (l) ⇌ NH₄⁺ (aq) + OH⁻ (aq)

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10
Q

write the neutralization rxn template

A

H⁺ acid + OH⁻ base ⇌ H₂O (l) + ion comp salt

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11
Q

ik this is a mess, but visualize the Cl part of NaCl dissolved in water

A 
OO
HHH
HClH
HHH
OO
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12
Q

this is a mess but what is the Na part of NaCl dissolved in water?

A 
HHHH
OO
Na
OO
HHHH
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13
Q

what is the charge on H and O in water?

A

±1δ

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14
Q

write out the precipitation rxn template

A

ion comp (aq) + ion comp (aq) → ion comp (aq) + ion comp (s)

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15
Q

what makes an ion less soluble

A

if it has a higher charge and attracts other ions

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16
Q

what makes a precipitate rxn not occur?

A

if both the products are (aq)

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17
Q

define molecular equation

A

regular chem equation

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18
Q

def complete ionic equation

A

ions existing separately & part of an (aq) comp are written separately w/ their charges

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19
Q

def spectator ions

A

remain separately written (separate or part of (aq) comp) before & after the rxn

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20
Q

def net ionic equation

A

complete ion equation written w/o spectator ions

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21
Q

what is H⁺ technically? x 2

A
  • just a proton

- hydronium (H₃O⁺)

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22
Q

recipe for hydronium

A

H⁺(aq) + H₂O(l) → H₃O⁺(aq)

23
Q

name & define the 3 -protic acids

A
  • monoprotic = 1 H⁺ ions when dissolved
  • diprotic = 2 H⁺ ions when dissolved
  • polyprotic = 2+ H⁺ ions when dissolved
24
Q

define hydroscopic

A

comp absorbing water vapor & dissolving itself with it!!

25
Q

define dilution

A

adding water to concentrated solution or dry hydroscopic (ramen!!!)

26
Q

units to answer M questions with on test

A

“x mol/L”

27
Q

def oxidation

A

atoms lose e⁻

28
Q

def reduction

A

atoms gain e⁻

29
Q

oxidation charge of lone element

A

0

30
Q

what happens in an oxidation-reduction rxn

A

atoms change charge

31
Q

define O/R half-reaction

A

2 separate net ionic eqn’s for the reduction rxn and the oxidation rxn in the same chem rxn

32
Q

how to show work for O/R ionic rxn on test

A

1) Write out each atom & charge of it below the eqn
2) write the half reactions pertaining to the O element & the R element
3) Balance the half-rxns so the amt of elements in them matches the amt in the OG chem eqn, and that the # of e⁻ matches the elements in the half-rxn

33
Q

template for gas evolution rxn (just used to ID them on test so you can apply the 3 subtemplates

A

acid (aq) + ion comp (aq) or (s) → cov comp (g) + ion comp (aq) or (s)

34
Q

H⁺ acid + (bi) carbonate →

A

CO₂ (g) + H₂O (l) + ion salt in GER

35
Q

CO₂ (g) + H₂O (l) + ion salt are the products of

A

H⁺ acid + (bi) carbonate in GER

36
Q

H⁺ acid + (bi) sulfite →

A

SO₂ (g) + H₂O (l) + ion salt in GER

37
Q

SO₂ (g) + H₂O (l) + ion salt are the products of

A

H⁺ acid + (bi) sulfite in GER

38
Q

H⁺ acid + S⁻² or HS⁻¹ →

A

H₂S (g) + ion salt in GER

39
Q

H₂S (g) + ion salt are the products of

A

H⁺ acid + S⁻² or HS⁻¹ in GER

40
Q

what is the main thing to remember with Redox rxns for cov comps

A

you assign oxidation #’s just to show where the e⁻ go; applies to cov comps & polyatomic ions w/ charges

41
Q

O# rule for H & exception

A

has +1 O#

in Hydride w/ metal (LiH), O# = -1

42
Q

O# rule for O & exception

A 
has -2 O#
in peroxide (H₂O₂) = -1
43
Q

O# rule for polyatomic ions

A

charge on ion = sum of O#’s; find the mystery charge based off the other O charges of O, H, or fixed ion on PT

44
Q

How to show work on test to find O#s of CO₂

A

1) write eqn solving for C O# (since you already know O = -2): O = -2, C = x
→ # C(x) + # O(-2) = overall charge of CO₂
2) Plug in: x + 2(-2) = 0
x = 4
so, C O# = +4

45
Q

how to write O charges on test

A

as +x or -x

CANNOT leave it like 4, or just + if the charge is one; it’s +4 and +1. Same for minus

46
Q

def O agent

A

the entire compound that got reduced and caused the other to get oxidized

47
Q

def R agent

A

the entire compound that got oxidized and caused the other to get reduced

48
Q

what type of rxn is a combustion

A

redox

49
Q

template for combustion rxn

A

CₓH₄ + O₂ (g) → CO₂ (g) + H₂O (l) + heat

50
Q

what type of rxn is displacement

A

redox

51
Q

template for displacement rxn

A

neutral active metal (s) + acid → H₂ (g) + ion comp (aq)

52
Q

def inactive metals

A

AKA “noble”; don’t react w/ acids & are below H on series table

53
Q

how to use activity series chart & what it determines

A

higher up on series = more likely to kick H out of its place in the acid & form an ion comp w/ the ion there

54
Q

def equivalence point

A

point in titration when acid’s mol H+ and base’s mol OH- are equal (strong & strong, weak & weak)

College Chem I (14 decks)

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