Unit 4 Flashcards

1
Q

Synthesis/ Combination Reaction

A

where two substances combine to form a compound

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2
Q

Decomposition Reaction

A

Where a substance comes apart into multiple substances

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3
Q

Metathesis Reactions

A

bonds between two chemical species are exchanged

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4
Q

Acid - Base Reaction

A

where an acid and base react to form their conjugate pairs

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5
Q

Oxidation - Reduction Reaction

A

the exchange of e-, causing different oxidation numbers

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6
Q

Combustion Reaction

A

where a hydrocarbon and O2 form CO2 + H2O + whatever else

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7
Q

Precipitation Reaction

A

ionic aqueous are mixed and two ions combine, solidifying

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8
Q

Spector Ion

A

the ions that do no solidify in an ionic substance

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9
Q

Alkali metal cations are….

A

always soluble

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10
Q

Ammonium Cations (NH4+) are…

A

always soluble

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11
Q

Nitrate Anion (NO3)4- are…

A

always soluble

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12
Q

Why do some ionic substances dissolve?

A

if…
Dipole H2O > Electrostatic Attraction

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13
Q

Why do some ionic substances solidify?

A

If…
Dipole H2O < Electrostatic Attraction

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14
Q

Hydroxide

A

OH-

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15
Q

Nitrate

A

(NO3) -

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16
Q

Acetate

A

(C2H3O2)-

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17
Q

Cynaide

A

(CN)-

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18
Q

Permanganate

A

(MnO4) -

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19
Q

Carbonate

A

(CO3)2-

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20
Q

Sulfate

A

(SO4)2-

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21
Q

Dichromate

A

(Cr2O7) 2-

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22
Q

Phosphate

A

(PO4) 3-

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23
Q

Ammonium

A

(NH4) +

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24
Q

Chromate

A

(CrO4) 2-

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25
Q

Peroxide

A

(O2) 2-

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26
Q

Oxalate

A

(C2O4) 2-

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27
Q

Thiosulfate

28
Q

What is the trick for balancing reactions?

29
Q

Law of Conservation of Mass

A

Mass is neither created or destroyed

30
Q

In combustion all the carbon from the hydrocarbon…

A

ends up in CO2

31
Q

In combustion all the hydrogen from the hydrocarbon…

A

ends up in H2O

32
Q

Gravimetrical Analysis

A

Determining the unknown substance of a chemical reaction

33
Q

Oxidative State

A

a HYPOTHETICAL charge assigned to an atom in a chemical compound, representing the number of electrons it would gain or lose if all its bonds were completely ionic

34
Q

non bonded, neutral atoms have a oxidative state of…

35
Q

oxidative charge of an ion/polyatomic ion…

A

ionic charge

36
Q

oxidative state of Oxygen is 2- EXCEPT when..

A

(H2O2)

O = -1

37
Q

oxidative state of H in metal is..

38
Q

oxidative state of H in nonmetal is..

39
Q

If there is no Oxygen is in the compound the most ________, takes the most common charge for oxidative charge.

A

electronegative

40
Q

For oxidative change, individual charges added together…

A

is the charge of the atom

41
Q

Redox reactions

A

The change in oxidative state due to the exchange of e-

42
Q

LEO the lion says GER

43
Q

What do half reactions in redox reactions show?

A

it shows the loss/gain of e-

44
Q

activity series

A

a list of elements arranged in decreasing order of their reactivity
(redox reaction)

45
Q

the higher the activity series ranking, the…

A

more likely to engage in redox

46
Q

Oxidating agent

A

the molecule being reduced

47
Q

Reducing agent

A

the molecule being oxidized

48
Q

Redox titrations

A

slowly adding solution with known concentrations to an unknown solution to determine concentration of that unknown solution

49
Q

Bronsted Acid

A

capable of donating a proton/H+

50
Q

Bronsted Base

A

Capable of accepting a proton/H+

51
Q

Why is H+ a proton?

A

because a proton is an e- + proton.

take away the e- and you have a proton

52
Q

conjugated pair

A

the acid version and base version of a molecule

53
Q

Amphoretic

A

can be either base or acid

ex: H2O - OH- and H3O+

54
Q

Types of Redox reactions

A
  1. Combination
  2. Decomposition
  3. Combustion
55
Q

what is the oxidation number for F in all com pounds?

56
Q

How do we determine if a reaction is redox?

A

We assign oxidation numbers

57
Q

end point

A

the point in a titration where all the substances have been reacted to make products

58
Q

Molecular Equation

A

the full, balanced equation

59
Q

Complete Ionic Equation

A

Shows the DISSOLVED IONS

60
Q

Net ionic

A

reaction which does not show the spectator ions (!)
also includes the charge

61
Q

theoretical yield

A

the amount that SHOULD be made up with the limiting agent

62
Q

Percent yield

A

[(actual yield)/(theoretical yield)] x 100%

63
Q

How do I balance normal redox reactions?

A
  1. write the half reactions
  2. Match the e-
  3. Add together
  4. simplify by getting rid of spectators
64
Q

Oxidation half, where are e-?

A

products

LOSING e-

65
Q

Reduction half, where are e-?

A

reactants

GAINING e-