Reactions- L12 Flashcards
(34 cards)
1
Q
Cr
A
2, 3, 4, 6
2
Q
Mn
A
2, 3, 4, 6, 7
3
Q
Fe
A
2, 3
4
Q
Co
A
2, 3
5
Q
Ni
A
2
6
Q
Cu
A
1, 2
7
Q
Zn
A
2
8
Q
Ag
A
1
9
Q
Au
A
1, 3
10
Q
Hg
A
1, 2
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
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
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= +
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
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)
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
Rules for determining oxidation numbers- oxygen
- -2 in any molecular compound
| - Exception in peroxides= -1. ex. H2O2
26
Rules for determining oxidation numbers- Hydrogen
- +1 when bonded to a nonmetal
| - -1 when bonded to a metal
27
Rules for determining oxidation numbers other covalent bonds that do not contain H or O
- 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
Rules for determining oxidation numbers sum of oxidation numbers
- must equal the overall charge of that compound
| - ex. must equal 0 in H2O and -1 in ClO3-
29
Oxidized
- OIL
- electrons lost
- More positive
30
Reduced
- RIG
- electrons gained
- more negative
31
Which solution in each set is the better conductor of electricity?
- The one with the most ions
| - must be ionic compound
32
write the balanced chemical equation for the dissolving of aluminum nitrate in water
- the compound breaks down into separate elements
| - Al(NO3)3 (s) ==> Al+3 (aq) + 3NO3- (aq)
33
Write the balanced net ionic equations for the reactions
- write out equation ==> broken elements
| - take out soluble elements to get final
34
Hydrogen peroxide is both
oxidized and reduced
