Reactions- L12 Flashcards

1
Q

Cr

A

2, 3, 4, 6

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2
Q

Mn

A

2, 3, 4, 6, 7

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3
Q

Fe

A

2, 3

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4
Q

Co

A

2, 3

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5
Q

Ni

A

2

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6
Q

Cu

A

1, 2

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7
Q

Zn

A

2

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8
Q

Ag

A

1

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9
Q

Au

A

1, 3

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10
Q

Hg

A

1, 2

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11
Q

Solutions

A
  • a homogeneous mixture of a solvent and solute
  • solvent- more and does the dissolving
  • solute- less and gets dissolved
  • Aqueous solution- solutions in which water is the solvent
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12
Q

Electrolytic solutions

A
  • An ionic compound dissolved in a polar solvent
  • Has to have charged parts to dissolve
  • most ionic compounds do this
  • If a solution conducts electricity it must contain ions
  • The more ions the solution contains, the better able it is to conduct electricity
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13
Q

Draw representation of dissolved ionic compound

A
  • Draw 2 circles with one element in each
  • exaggerate relative sizes of the nucleus
  • Include charges in those circles
  • Draw water molecules around it with dipoles
  • O= -
  • H= +
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14
Q

ions in water/conducting electricity

A
  • smaller ions move slower since they attract and drag more water
  • Larger ions move faster since they are less attracted to the water, greater shielding effect and coulombs law
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15
Q

Molecular compounds in water

A
  • molecular= no metals in it
  • Non-electrolytes= most molecular compounds do not dissolve in water and therefor do not conduct electricity (sugar, methanol)
  • Weak-electrolyes= weak acids- some dissociation (low conductivity), ex. acidic acid CH3COOH (aka ethanol acid or vinegar)
  • Strong-electrolytes= strong acids- complete dissociation (high conductivity) ex. hydrochloric acid (HCl), HF, HNO3, H2SO4 (first H is strong, second is weak)
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16
Q

Like dissolves like

A
  • Non polar molecules dissolve in non polar solvents
  • polar molecules dissolve in polar solvents
  • ex. water and methanol
17
Q

Precipitation reaction

A
  • aka double replacement, double displacement, ionic
  • In a precipitate reaction, the attractive forces between oppositely charged ions is greater than the forces of attraction between H2O molecules and ions
  • products are an aqueous and solid
18
Q

Write the balanced net ionic equation for a precipitate reaction

A
  • Write out the equation
  • break down of reactants ==> recombined, not combining the dissolvable
  • Balanced Net ionic equation only shows the reaction that actually took place (not including dissolved)
  • Complete ionic equation shows all of the species that are present (includes dissolvable combined into compounds)
19
Q

Solubility rules

A
  • All salts (ionic compounds- cation and anion) containing Na+, K+, NH4+, or NO3-
  • All alkaline metals
  • All nitrates and ammonium
20
Q

Pb

A

+2

21
Q

Oxidation Reduction Reactions

A
  • Aka REDOX reactions
  • Electron transfer reactions
  • One substance gets oxidized and loses electrons
  • The other substance gets reduced and gains electrons
22
Q

Single Replacement REDOX reactions

A
  • Element and compound
23
Q

Rules for determining oxidation numbers- atom in its elemental form

A

its oxidation number is zero

24
Q

Rules for determining oxidation numbers monoatomic ion (like Mg+2)

A

oxidation number equals its charge

25
Q

Rules for determining oxidation numbers- oxygen

A
  • -2 in any molecular compound

- Exception in peroxides= -1. ex. H2O2

26
Q

Rules for determining oxidation numbers- Hydrogen

A
  • +1 when bonded to a nonmetal

- -1 when bonded to a metal

27
Q

Rules for determining oxidation numbers other covalent bonds that do not contain H or O

A
  • the most electronegative element has an oxidation number equal to its charge as an ion
  • ex. F=-1 in BF3 and Cl= -1 in PCl5
28
Q

Rules for determining oxidation numbers sum of oxidation numbers

A
  • must equal the overall charge of that compound

- ex. must equal 0 in H2O and -1 in ClO3-

29
Q

Oxidized

A
  • OIL
  • electrons lost
  • More positive
30
Q

Reduced

A
  • RIG
  • electrons gained
  • more negative
31
Q

Which solution in each set is the better conductor of electricity?

A
  • The one with the most ions

- must be ionic compound

32
Q

write the balanced chemical equation for the dissolving of aluminum nitrate in water

A
  • the compound breaks down into separate elements

- Al(NO3)3 (s) ==> Al+3 (aq) + 3NO3- (aq)

33
Q

Write the balanced net ionic equations for the reactions

A
  • write out equation ==> broken elements

- take out soluble elements to get final

34
Q

Hydrogen peroxide is both

A

oxidized and reduced