Chapter 8 Flashcards
Li+, Na+, K+, and NH4+
Compounds containing these the following ions are generally soluble
Exceptions:
None
NO3-, and C2H302-
Compounds containing these the following ions are generally soluble
Exceptions:
None
Cl-, Br-, and I-
Compounds containing these the following ions are generally soluble
Exceptions:
When paired with Ag+, Hg2(2+), Pb(2+) the resulting compounds are insoluble
SO4(2-)
Compounds containing these the following ions are generally soluble
Exceptions:
When paired with Sr2+, Ba2+, Pb2+, Ag+, or Ca2+ the resulting compounds are insoluble
OH- and S2-
Compounds containing these the following ions are generally insoluble
Exceptions:
When these ions paired with Li+, Na+, K+, or NH4+ the resulting compounds are soluble
When S2- is paired with Sr2+, Ba2+, or Ca2+ the resulting compound is soluble
When OH- is paired with Sr2+, Ba2+, or Ca2+ the resulting compound is soluble
CO3(2-) and PO4(3-)
Compounds containing these the following ions are generally insoluble
Exceptions:
When these ions paired with Li+, Na+, K+, or NH4+ the resulting compounds are soluble
HBr
Hydrobromic acid
HCl
Hydrochloric acid
HI
Hydroiodic acid
HNO 3
Nitric acid
HClO 4
Perchloric acid
H 2 SO 4
Sulfuric acid
HF
Hydrofluoric acid (weak acid)
NaOH
Sodium hydroxide
HCH 2 COOH
Acetic acid (weak acid)
LiOH
Lithium hydroxide
KOH
Potassium hydroxide
Ca(OH) 2
Calcium hydroxide
Ba(OH) 2
Barium hydroxide
NH 3
Ammonia (weak base)
Compound That Undergo Gas-Evolution Reaction: sulfide
Intermediate Product: None
Gas Evolved: H2S
Example: 2 HCl (aq) + K2S (aq) → H2S (g) + 2 KCl (aq)
Compound That Undergo Gas-Evolution Reaction: carbonates and bicarbonates
Intermediate Product: H2CO3
Gas Evolved: CO2
Example:
2 HCl (aq) + K2CO3 (aq) → H2CO3 (aq) + 2 KCl (aq)
Final Equation:
2 HCl (aq) + K2CO3 (aq) → H2O (l) + CO2 (g) + 2 KCl (aq)
Compound That Undergo Gas-Evolution Reaction: sulfites and bisulfites
Intermediate Product: H2SO3
Gas Evolved: SO2
Example:
2 HCl (aq) + K2SO3 (aq) → H2SO3 (aq) + 2 KCl (aq)
Final Equation:
2 HCl (aq) + K2SO3 (aq) → H2O (l) + SO2 (g) + 2 KCl (aq)
Compound That Undergo Gas-Evolution Reaction: ammonia
Intermediate Product: NH4OH
Gas Evolved: NH3
Example:
NH4Cl (aq) + KOH (aq) → NH4OH (aq) + 2 KCl (aq)
Final Equation:
NH4Cl (aq) + KOH (aq) → H2O (l) + NH3 (g) + 2 KCl (aq)
Rules for assigning oxidation states
- The oxidation state of an atom in a free element is 0.
- The oxidation state of a monoatomic ion is equal to its charge.
- The sum of the oxidation states of all atoms in:
- a neutral molecule or formula unit is 0.
- an ion is equal to the charge of the ion.
- In their compounds, metals have positive oxidation states.
- Group 1A metals always have an oxidation state of +1.
- Group 2A metals always have an oxidation state of +2.
- In their compounds, we assign nonmetals oxidation states according to the table on the right. Entries at the top of the table take precedence over entries at the bottom of the table.
Oxidation State: Fluorine
-1
Oxidation state: Hydrogen
+1
Oxidation state: Oxygen
-2
Oxidation state: Group 7A
-1
Oxidation State: Group 6A
-2
Oxidation State: Group 5A
-3
