Chapter 4
1. Define Solute, solvent, active solvent, electron density
a. Solute = being dissolved (smaller amount)
b. Solvent = doing the dissolving (larger amount)
c. Passive solvent = disperse substances into individual molecules
d. Active solvent = strongly interacts and sometimes reacts w/substances
e. Electron density = measure of the probability of an electron being present at a specific location
i. (low density) +---- (high density)
ii. S+ = low density; S- = high density
iii. -> = interacts with cations (+)
iv. + = interacts with anions (-)
2. Describe the conductivity of solutions
a. Electrolyte solution
i. Has ions present
ii. Conductive
b. Non-electrolyte solution
i. Distilled water
ii. No ions
iii. No conduction
c. Solid ionic state
i. Vibration
ii. No free movement of ions no conduction
d. Ions move to electrodes where ReDox RX happen
i. Cathode = M+ + e- M
ii. Anode = X- = x + e-
e. Ionic compounds are electrolytes bc free mobility of ions; unless solid
3. Define concentration and molarity
a. Concentration = quantity of solute present in a given quantity of solution
mass solute n
b. Molarity = M= (n = number of moles of solute)
L of solution V
4. How do you prepare a molar solution?
a. Determine the required concentration
b. Divide volume needed
c. Calculate the moles needed from which mass is calculated
d. Measure and transfer the sample to volumetric flask
e. Dilute to the mark
5. How do you convert a concentrated diluted solution?
a. M1V1 =M2V2
b. Concentrated solution has more solute per unit volume
6. Writing equations for Aq ionic RX
a. AKA precipitation RX
b. Steps:
i. Write molecular formula
ii. Separate into ions (only aq states)
iii. Net ionic equation (remove spectator ions/cancel out ions)
c. Total ionic equation = shows all soluble ionic substances dissociated into ions (fully written out)
d. Spectator ions = no change to chemical change
e. Net ionic equation = shows actual change; eliminates spectator ions
,7. Predicting precipitate
a. Precipitation Rx = 2 soluble ionic compounds insoluble product AKA precipitate
b. Consider all cation-anion possibilities and use solubility rules to determine if combo is INSOLUBLE
8. What is a metathesis RX?
a. Ions exchange partners + precipitate forms
b. Exchange of bonds between reacting species
9. What is an acid base RX?
a. Acid = produces H+ ions when dissolved in H2O
b. Base = produces OH- ions when dissolved in H2O
c. A neutralization RX
d. H+ ion as a soluted hydronium ion
i. H+ interacts w/H2O (H+ + H2O H3O+ (aq)
ii. Free electrons of O can be used to make another bond
iii. Exists w/other water molecules through hydrogen bonding
10. Strong vs weak acids
a. Strong = disassociate completely
i. HCl, HBr, HI
ii. HNO3, H2SO4, HClO4
b. Weak = disassociate partially
i. HF, H3PO4, CH3COOH (C2H5O2)
ii. Organic acids are weak (contain carbon)
11. Strong vs weak bases
a. Strong
i. LiOH
ii. NaOH
iii. KOH
iv. RbOH
v. CsOH
vi. Ca(OH)2
vii. Sr(OH)2
viii. Ba(OH)2
b. Weak = NH3
i. NH3+H2O NH4+ + OH-
, 12. Acid/bases as electrolytes
a. Strong bases and acids are strong electrolytes = good conductors
13. Acid base titrations
a. Neutralizing RX
b. Can determine concentration of acid/base by using standard solutions
c. Acid base indicator = has diff colors in acid and base; used to monitor the RX process
d. Equivalence point == the mol H+ from acid = mol of OH- ion from base –
i. # of H+ in flask = # of OH- ion added
e. End point occurs when there’s a slight excess of base and the indicator changes color permanently
f. Less than 7 = acid, neutral = 7, 7+ = base
14. Oxidization Redox RX
a. Oxidation = loss of e-
b. Reduction = gain of e-
c. Oxidizing agent = gains e- reduced
d. Reducing agent loses e- oxidized
e. Occurs always together
15. Rules for assessing Oxidation number
a. 0 = an atom in its elemental form
b. Oxidation # = ion charge for monatomic ions
c. Sum of oxidation numbers should = 0
d. Special rules
i. Group 1 = +1
ii. Group 2 = +2
iii. H = +1 (with non-metals); -1 (with metals)
iv. F = -1
v. O= -1 in peroxides; -2 in all other compounds (except F)
vi. Group 7 = -1 w/metals, non-metals (except O) and other lower halogens
16. Rules for balancing redox RX
a. Assign Oxidation numbers
b. Identify reactants that are oxidized/reduced
c. Compute # of e- transferred
d. Multiply # of e- by (factors that make e- lossed= e- gained)
e. Balance coefficients
f. 2x check
17. Diff types of RX
a. Combination
b. Decomposition
c. Displacement
d. Combustion
18. Activity series
a. Li = highest reducing agent
b. H2 = lowest reducing agent
c. Au, Cu, Hg, Ag = can’t displace H2
1. Define Solute, solvent, active solvent, electron density
a. Solute = being dissolved (smaller amount)
b. Solvent = doing the dissolving (larger amount)
c. Passive solvent = disperse substances into individual molecules
d. Active solvent = strongly interacts and sometimes reacts w/substances
e. Electron density = measure of the probability of an electron being present at a specific location
i. (low density) +---- (high density)
ii. S+ = low density; S- = high density
iii. -> = interacts with cations (+)
iv. + = interacts with anions (-)
2. Describe the conductivity of solutions
a. Electrolyte solution
i. Has ions present
ii. Conductive
b. Non-electrolyte solution
i. Distilled water
ii. No ions
iii. No conduction
c. Solid ionic state
i. Vibration
ii. No free movement of ions no conduction
d. Ions move to electrodes where ReDox RX happen
i. Cathode = M+ + e- M
ii. Anode = X- = x + e-
e. Ionic compounds are electrolytes bc free mobility of ions; unless solid
3. Define concentration and molarity
a. Concentration = quantity of solute present in a given quantity of solution
mass solute n
b. Molarity = M= (n = number of moles of solute)
L of solution V
4. How do you prepare a molar solution?
a. Determine the required concentration
b. Divide volume needed
c. Calculate the moles needed from which mass is calculated
d. Measure and transfer the sample to volumetric flask
e. Dilute to the mark
5. How do you convert a concentrated diluted solution?
a. M1V1 =M2V2
b. Concentrated solution has more solute per unit volume
6. Writing equations for Aq ionic RX
a. AKA precipitation RX
b. Steps:
i. Write molecular formula
ii. Separate into ions (only aq states)
iii. Net ionic equation (remove spectator ions/cancel out ions)
c. Total ionic equation = shows all soluble ionic substances dissociated into ions (fully written out)
d. Spectator ions = no change to chemical change
e. Net ionic equation = shows actual change; eliminates spectator ions
,7. Predicting precipitate
a. Precipitation Rx = 2 soluble ionic compounds insoluble product AKA precipitate
b. Consider all cation-anion possibilities and use solubility rules to determine if combo is INSOLUBLE
8. What is a metathesis RX?
a. Ions exchange partners + precipitate forms
b. Exchange of bonds between reacting species
9. What is an acid base RX?
a. Acid = produces H+ ions when dissolved in H2O
b. Base = produces OH- ions when dissolved in H2O
c. A neutralization RX
d. H+ ion as a soluted hydronium ion
i. H+ interacts w/H2O (H+ + H2O H3O+ (aq)
ii. Free electrons of O can be used to make another bond
iii. Exists w/other water molecules through hydrogen bonding
10. Strong vs weak acids
a. Strong = disassociate completely
i. HCl, HBr, HI
ii. HNO3, H2SO4, HClO4
b. Weak = disassociate partially
i. HF, H3PO4, CH3COOH (C2H5O2)
ii. Organic acids are weak (contain carbon)
11. Strong vs weak bases
a. Strong
i. LiOH
ii. NaOH
iii. KOH
iv. RbOH
v. CsOH
vi. Ca(OH)2
vii. Sr(OH)2
viii. Ba(OH)2
b. Weak = NH3
i. NH3+H2O NH4+ + OH-
, 12. Acid/bases as electrolytes
a. Strong bases and acids are strong electrolytes = good conductors
13. Acid base titrations
a. Neutralizing RX
b. Can determine concentration of acid/base by using standard solutions
c. Acid base indicator = has diff colors in acid and base; used to monitor the RX process
d. Equivalence point == the mol H+ from acid = mol of OH- ion from base –
i. # of H+ in flask = # of OH- ion added
e. End point occurs when there’s a slight excess of base and the indicator changes color permanently
f. Less than 7 = acid, neutral = 7, 7+ = base
14. Oxidization Redox RX
a. Oxidation = loss of e-
b. Reduction = gain of e-
c. Oxidizing agent = gains e- reduced
d. Reducing agent loses e- oxidized
e. Occurs always together
15. Rules for assessing Oxidation number
a. 0 = an atom in its elemental form
b. Oxidation # = ion charge for monatomic ions
c. Sum of oxidation numbers should = 0
d. Special rules
i. Group 1 = +1
ii. Group 2 = +2
iii. H = +1 (with non-metals); -1 (with metals)
iv. F = -1
v. O= -1 in peroxides; -2 in all other compounds (except F)
vi. Group 7 = -1 w/metals, non-metals (except O) and other lower halogens
16. Rules for balancing redox RX
a. Assign Oxidation numbers
b. Identify reactants that are oxidized/reduced
c. Compute # of e- transferred
d. Multiply # of e- by (factors that make e- lossed= e- gained)
e. Balance coefficients
f. 2x check
17. Diff types of RX
a. Combination
b. Decomposition
c. Displacement
d. Combustion
18. Activity series
a. Li = highest reducing agent
b. H2 = lowest reducing agent
c. Au, Cu, Hg, Ag = can’t displace H2
