Chemistry Exam Review
1 mole equals
6.02 x 10^23 anything
A sample of silver weighing 107.9 grams contains___.
6.02 × 1023 silver atoms
Calculate the number of atoms in 66.0 g of Cu.
6.25E23 atoms
What mass of water is produced from the complete combustion of 4.30×10−3 g of methane?
9.68×10−3 g
CH3OOH
Acetic acid (Weak)
0.381 g Al, 5.381 gI
AlI3
Oxidation states VA (Non-metal anions)
Always -3 (N3-,P3-)as an anion
Oxidation states IVA (Non-metal anions)
Always -4 (C4-) as an anion
NH3
Ammonia (weak)
NH4+
Ammonium ion
Spell out the full name of the ion.NH4+, C2H3O2−, CN−
Ammonium,Acetate,Cyanide
Give an example of a semimetal or metalloid
B, Si, Ge, As, etc
Ba(OH)2
Barium hydroxide (strong)
What is the net ionic equation of the reaction of BeCl2 BeCl2 with NaOH NaOH?
Be2+(aq)+2OH−(aq)→Be(OH)2(s)
Oxidation States IVB-VIIIB (metal cations)
Commonly +2 and +3 (e.g.,Cr,Mn,Fe,Co,Ni)
Starting content from
Exam 1 and before
Determine the name for HFO3.
Fluoric acid
HCl(aq)+KOH(aq) -->
KCl(aq)+H2O(l)
LiOH
Lithium hydroxide (strong)
Most silver salts are...
Most silver salts are insoluble. AgNO3 and Ag(C2H3O2) are common soluble salts of silver; virtually all others are insoluble.
Complete and balance, or determine if NO REACTION:LiI(aq) + BaS(aq) ->
NO REACTION
Oxidation State of each element:CO₃²-
O: -2C: +4
Enter the complete ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
Pb2+(aq)+2NO3−(aq)+2K+(aq)+SO42−(aq)→PbSO4(s)+2K+(aq)+2NO3−(aq)
Enter the net ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
Pb2+(aq)+SO42−(aq)→PbSO4(s)Pb2+(aq)+SO42−(aq)→PbSO4(s)
Assign oxidation states to each element:PbS
Pb: +2S: -2
Salts containing Cl -, Br -, or I -
Salts containing Cl -, Br -, or I - are generally soluble. Important exceptions to this rule are halide salts of Ag+, Pb2+, and (Hg2)2+. Thus, AgCl, PbBr2, and Hg2Cl2 are insoluble.
Oxidation States IVA (Metal cations)
Sn and Pb (+2,+4)
NaOH
Sodium hydroxide (strong)
Is (NH4)2S soluble or insoluble?
Soluble
Is AgNO3 soluble or insoluble?
Soluble
Is KNO3 soluble or insoluble?
Soluble
Is Pb(C2H3O2)2 soluble or insoluble?
Soluble
Sr(OH)2
Strontium hydroxide (strong)
SO4 2-
Sulfate ion
SO3 2-
Sulfite ion
Give he name for H2SO4
Sulfuric acid
H2SO4
Sulfuric acid(strong)
Naming Acids
The acid name begins with the prefix Hydro-, followed by the base name of the anion, followed by the suffix -ic ,+ acid Ex:HCl --> Hydrochloric acid
Assign oxidation states to each element:TiCl4
Ti: +4Cl: -1
Oxidation States IIB (metal cations)
Zn and Cd(+2);Hg(+1,+2)
What is the net ionic equation for the reaction that occurs when aqueous solutions of KOHKOH and ZnCl2ZnCl2 are mixed?
Zn2+(aq)+2OH−(aq)→Zn(OH)2(s)
H2SO4(aq)+Zn(OH)2 -->
ZnSO4(aq)+2H2O(l)
NH3
ammonia
Ca(OH)2
calcium hydroxide
HBr
hydrobromic acid (strong)
HCO3 -
hydrogen carbonate (bicarbonate)
HClO4 is
hydrogen perchlorate
Consider the reaction:2NiO(s) -> 2Ni(s) + O2(g)If O2 is collected over water at 40.0C and a total pressure of 745 mmHg, what volume of gas is collected for the complete reaction of 24.78g of NiO?
*HINT: PV = nRT P(O2) = Ptot - P(H2O) P(H2O) = 55.3 torr4.70 L
A 25.00 mL sample of an unknown HClO4 solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution?HClO4(aq) + NaOH(aq) -> H2O(l) + NaClO4(aq)
*HINT: n₁M₁V₁ = n₂M₂V₂ n₁ = 1 n₂ = 3 M₁ = ? M₂ = 0.200 M V₁ = 25.0 mL V₂ = 22.62 mL M₁ = 0.1809 M
Calculate the number of moles in 14.9 g of Fe.
0.267 mol
In the reaction CH4 + 2 O2 → CO2 + 2 H2O, how many moles of oxygen are required to burn 16.0 g of methane? A) 0.50 B) 2.0 C) 1.0 D) 32
0.50 mol of Oxygen
Calculate the density in g/mL of 2.0 L of gasoline that weighs 1.25 kg . Express your answer to two significant figures and include the appropriate units.
0.63 g/mL
What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H2O, respectively.
1,2,1,2
6.02 x 10^23 anything occupies ____ at STP
22.4 L
Complete and balance, or determine if NO REACTION:NaOH(aq) + FeCl3(aq) ->
3NaOH(aq) + FeCl3(aq) -> Fe(OH)3 (s) + 3NaCl
NaOH(aq)+FeCl3(aq)→
3NaOH(aq)+FeCl3(aq)→Fe(OH)3(s)+3NaCl(aq)3NaOH(aq)+FeCl3(aq)→Fe(OH)3(s)+3NaCl(aq)
soluble
(of a substance) capable of being dissolved in some solvent (usually water)
What is the molarity of NO3- in 0.150 M Al(NO3)3?
0.450 M
C2H3O2-
Acetate ion
Complete and balance, or determine if NO REACTION:CrBr2(aq) + Na2CO3(aq) ->
CrBr2(aq) + Na2CO3(aq) → 2NaBr (aq) + CrCO3(s)
NO2-
Nitrite ion
insoluble
(of a substance) not easily dissolved
Consider the unbalanced redox reaction:MnO₄-(aq) + Zn(s) → Mn²+(aq) + Zn²+(aq)Determine the volume of a 0.500 M KMnO4 solution required to completely react with 2.85 g of Zn.
*HINT: Balance the redox reaction. M = n/V2MnO₄-(aq) + 5Zn(s) 16H+(aq) → 2Mn²+(aq) + 5Zn²+(aq) + 8H₂O(l)34.9 mL
Identify the conjugate acid:H₂SO₄(aq) + Cl-(aq) ↔ HSO₄-(aq) + HCl(aq)
*HINT: Base is H+ acceptor. Acid is H+ donator. Conjugate acid is located in the products and is paired with base from the reactants.HCl(aq)
Identify the conjugate base:S²-(aq) + H₂O(l) ↔ HS-(aq) + OH-(aq)
*HINT: Base is H+ acceptor. Acid is H+ donator. Conjugate base is located in the products and is paired with acid from the reactants.OH-(aq)
Identify the acid:H₂O(l) + CO₃²-(aq) ↔ OH-(aq) + HCO₃-(aq)
*HINT: Base is H+ acceptor. Acid is H+ donator.H₂O(l)
Identify the base:H₂O(l) + HS-(aq) ↔ H₃O+(aq) + S²-(aq)
*HINT: Base is H+ acceptor. Acid is H+ donator.H₂O(l)
We have 100 mL of nitric acid solution with a pH of 4.0. We dilute the solution by adding water to get a total volume of 1.0 L. What is the pH of the final solution?
*HINT: Calculate moles in original solution. Find the molarity of the final solution. Calculate pH.5.0
The density of 20% by mass ethylene glycol (C2H6O2) solution in water is 1.03 g/mL. Find the molarity of the solution.
*HINT: Density*(1000(mL/L))*(.2)/MM(C2H6O2)3.32 M
Assign oxidation states to each element:O2F2
*HINT: Fluorine has priority over oxygen F: -1O: +1
Assign oxidation states to each element:CsO2
*HINT: Group 1A and 2A elements have priority over oxygen.Cs: +1O: -1/2
Balance the following redox reaction in basic aqueous solution:Al(s) + MnO₄-(aq) -> MnO₂(s) + Al(OH)₄-(aq)
*HINT: Separate into half-reactions, balance O's w/H2O, balance H's with H+, balance charge with e-'s, multiply equations by factor so that they have equal amount of e-s on opposite sides. Combine and cancel. Then, add OH- to both sides based on number of H+ ions. Cancel.Al(s) + MnO₄-(aq) + 2H₂O(l)-> MnO₂(s) + Al(OH)₄-(aq)
Balance the following redox reaction in basic aqueous solution:H₂O₂(aq) + ClO₂(aq) -> ClO₂-(aq) + O₂(g)
*HINT: Separate into half-reactions, balance O's w/H2O, balance H's with H+, balance charge with e-'s, multiply equations by factor so that they have equal amount of e-s on opposite sides. Combine and cancel. Then, add OH- to both sides based on number of H+ ions. Cancel.H₂O₂(aq) + 2ClO₂(aq) + 2OH-(aq) -> 2ClO₂-(aq) + O₂(g) + 2H2O(l)
Balance the following redox reaction in acidic aqueous solution:PbO2 (s) + I-(aq) -> Pb²+(aq) + I₂(s)
*HINT: Separate into half-reactions, balance O's w/H2O, balance H's with H+, balance charge with e-'s, multiply equations by factor so that they have equal amount of e-s on opposite sides. Combine and cancel.PbO2 (s) + 2I-(aq) + 4H+(aq) -> Pb²+(aq) + I₂(s) + 2H2O(l)
A system releases 622 kJ of heat and does 105 kJ of work on the surroundings. What is the change in internal energy of the system?
*HINT: ∆E = q + w (w = -P∆V)-727 kJ
Oxidation State of:Ag+
+1
Consider the thermochemical equation for the combustion of acetone:C3H6O(l) + 4O2 -> 3CO2 + 3H2O ∆Hrxn = -1790 kJIf a bottle of nail polish remover contains 177 mL of acetone, how much heat is released by its complete combustion? The density of acetone is 0.788 g/mL.
-4300 kJ
Oxidation State of:Ag
0
What mass of carbon dioxide is produced from the complete combustion of 4.30×10−3 g of methane?
1.18×10−2 g
What mass of oxygen is needed for the complete combustion of 4.30×10−3 g of methane?
1.72×10−2 g
Determine the molar mass of citric acid, the sour taste found in citrus fruits, C6H8O7.
192.12 g/mol
What is the minimum amount of 6.0 M H2SO4 necessary to produce 25.0 g of H2(g) according to the reaction between aluminum and sulfuric acid?2Al(s) + 3H2SO4(aq) -> Al2(SO4)3 (aq) + 3H2(g)
2.1 L
The mass of an evacuated 255 mL flask is 143.187 g. The mass of the flask filled with 267 torr of an unknown gas at 25C is 143.289 g. Calculate the molar mass of the unknown gas.
27.9 g/mol
Consider the precipitation reaction:2Na3PO4 (aq) + 3CuCl2 (aq) -> Cu3(PO4)2(s) + 6 NaCl(aq)What volume of 0.175 M Na3PO4 solution is necessary to completely react with 95.4 mL of 0.102 M CuCl2?
37.1 mL
A laboratory procedure calls for making 400 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 do you need?
37g
CH3OH can be synthesized by the reaction:CO(g) + 2H2(g) -> CH3OH(g)What volume of H2 gas (in L), at 748 mmHg and 86C, is required to synthesize 25.8 g CH3OH?
48.3 L
precipitate
A solid that forms and settles out of a liquid mixture
Percent Yield
Actual Yield/ Theoretical yield of product * 100
Oxidation States IIIA (Metal cations)
Al and GA (+3);In and Tl(+1,+3)
Oxidation States IA (metal cations)
Always +1 (Li,Na,K,Rb,Cs,Fr)
Oxidation States IIA (metal cations)
Always +2 (Be,Mg,Ca,Sr,Ba,Ra)
Oxidation States IIIB (Metal cations)
Always +3 (Sc,Y,La)
Oxidation states VIIA(Non-metal anions)
Always -1 (F-,Cl-,Br-,I-) as an anion
Oxidation states hydrogen
Always -1(H-) as anion; but +1 otherwise
Oxidation states VIA (Non-metal anions)
Always -2 (O2-,S2-,Se2-,Te2-) as an anion
Describe the difference between ionic and molecular compounds.
An ionic compound is formed between a metal and nonmetal (Or polyatomic ions), and is held together through the sttraction of opposite charges. A Molecular compound is usally formed between two or more nonmetals, and is held together through shareing of electrons between atoms
Balance the following equation : B2O3(s) + HF(l) --> BF3(g) +H2O
B2O3+6HF--> 2BF3+3H2O
What is the net ionic equation of the reaction of MgSO4MgSO4 with Ba(NO3)2Ba(NO3)2?
Ba2+(aq)+SO42−(aq)→BaSO4(s)Ba2+(aq)+SO42−(aq)→BaSO4(s)
BaI2(aq)+AgNO3(aq)→
BaI2(aq)+2AgNO3(aq)→Ba(NO3)2(aq)+2AgI(s)BaI2(aq)+2AgNO3(aq)→Ba(NO3)2(aq)+2AgI(s)
Oxidation States VA (Metal cations)
Bi (+3,+5)
Find the empirical formula for tartaric acid. Tartaric acid is the white, powdery substance that coats sour candies such as Sour Patch Kids. Combustion analysis of a 12.01-gg sample of tartaric acid-which contains only carbon, hydrogen, and oxygen-produced 14.08 gg CO2CO2 and 4.32 gg H2OH2O.
C2H3O3
An unknown compound was decomposed and found to be composed of 1.36 mol oxygen, 4.10 mol hydrogen, and 2.05 mol carbon. What is the empirical formula of the unknown compound?
C3H6O2
Give a possible molecular formula for the empirical formula of C3H5ClOC3H5ClO.
C6H10Cl2O2
C4H9, 114.22 g/mol
C8H18
Ca(OH)2
Calcium hydroxide (strong)
CO3 2-
Carbonate ion
Carbonates are frequently...
Carbonates are frequently insoluble. Group II carbonates (CaCO3, SrCO3, and BaCO3) are insoluble, as are FeCO3 and PbCO3.
What is the name of the acid whose formula is H2CO3?
Carbonic acid
H2CO3
Carbonic acid (weak)
ClO3-
Chlorate ion
ClO2-
Chlorite ion
CrO4 2-
Chromate ion
Chromates are frequently...
Chromates are frequently insoluble. Examples include PbCrO4 and BaCrO4.
aqueous
Clear, transparent fluid that fills the anterior chamber
Oxidation States IB (metal cations)
Cu(+1,+2);Ag(+1);Au(+1,+3
Copper (I) is options: Copperium Cuporious Cupic Cuprous
Cuprous
CN-
Cyanide ion
Which statement is true of the internal energy of a system and its surroundings during an energy exchange with a negative ∆Esys?A) Internal energy of system increases, internal energy surroundings decreasesB) Internal energy of both system and surroundings increasesC)Internal energy of system and surroundings decreasesD)Internal energy of system decreases, internal energy surroundings increases
D
Cr2O7 2-
Dichromate ion
Oxidation State of each element:CaF2
F: -1Ca: +2
Fluorides...
Fluorides such as BaF2, MgF2, and PbF2 are frequently insoluble.
CHOOH
Formic acid(weak)
Write balanced net ionic equation for:HCl(aq) + LiOH(aq) -> H2O(l) + LiCl(aq)
H+(aq) + OH-(aq) -> H2O(l)
Give the formula for sulfurous acid
H2SO3
What is the formula for Sulfurous acid?
H2SO3
Complete and balance the acid-base equation:H2SO4(aq) + NaOH(aq) ->
H2SO4(aq) + 2NaOH(aq) -> 2H2O (l) + Na2SO3 (aq)
The Chemical formula for selenous acid is...?
H2SeO3(aq)
What is the formula for chlorous acid?
HClO2
An aqueous solution of HBr is named as...?
Hydrobromic Acid
HCl
Hydrochloric acid (Strong)
HCN
Hydrocyanic acid (weak)
HF
Hydrofluoric acid (weak)
What is the name of the acid whose formula is HI?
Hydroiodic Acid
HI
Hydroiodic acid (strong)
H3O+
Hydronium ion
OH-
Hydroxide ion
ClO-
Hypochlorite ion
net ionic equation
Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution
Spectator ion
Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction
Give and example of an alkali metal
Li,Na,K,Rb,Cs,(Fr)
Give an example a compound formed from an alkaline eath metal and a halogen -- Give the chemical formula
MgCl2,CaI2, etc
Diluition of Solution
MiVi=MfVf
Molarity
Moles of solute/liters of solution
Most hydroxide salts are...
Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al3+ are insoluble. Thus, Fe(OH)3, Al(OH)3, Co(OH)2 are not soluble.
Most sulfate salts are...
Most sulfate salts are soluble. Important exceptions to this rule include CaSO4, BaSO4, PbSO4, Ag2SO4 and SrSO4 .
Most sulfides of transition metals are...
Most sulfides of transition metals are highly insoluble, including CdS, FeS, ZnS, and Ag2S. Arsenic, antimony, bismuth, and lead sulfides are also insoluble.
Sodium acetate is
NaC2H3O2
Sodium dihydrogen phospahte
NaH2PO4
What are net ionic equations?
Net ionic equations are equations that show only the soluble, strong electrolytes reacting (these are represented as ions) and omit the spectator ions, which go through the reaction unchanged.
Which statement below concerning molecular, complete ionic, and net ionic equations, is true?
Net ionic equations only show the species that actually change during the reaction.
NO3-
Nitrate ion
What is the chemical name for HNO3?
Nitric acid
HNO3
Nitric acid (strong)
Ca(NO3)2(aq)+KCl(aq)→
No reaction
Write an equation for the precipitation reaction that occurs (if any) when you mix solutions of ammonium chloride and iron(III) nitrate mix.
No reaction
Oxidation State of each element:CrO₄²-
O: -2Cr: +6
Identify the oxidizing/reducing agents:Mg(s) + Fe²+(aq) -> Mg²+(aq) + Fe(s)
OA: Fe²+ (+2→0)RA: Mg (0→+2)
Identify the oxidizing/reducing agents:4 Li(s) + O2(g) -> 2Li2O(s)
OA: O2 (0→-2)RA: Li (0→+1)
Boyles Law
P1V1=P2V2 (for caluclationing changes)
What is the empirical formula for the compound P4O6P4O6?
P2O3
ClO4-
Perchlorate ion
HClO4
Perchloric acid (strong)
MnO4-
Permanganate ion
PO4 3-
Phosphate ion
Phosphates...
Phosphates such as Ca3(PO4)2 and Ag3PO4 are frequently insoluble.
PO3 3-
Phosphite ion
H3PO4
Phosphoric acid (weak)
KOH
Potassium hydroxide (strong)
Oxidation State of each element:H2S
S: -2H: +1
Salts containing group I elements
Salts containing Group I elements (Li+, Na+, K+, Cs+, Rb+) are soluble . There are few exceptions to this rule. Salts containing the ammonium ion (NH4+) are also soluble.
Salts containing nitrate ion (NO3-)
Salts containing nitrate ion (NO3-) are generally soluble.
NaHCO3
Sodium Bicarbonate (weak)
Naming bases
There is not special system to naming bases. Since they all contation the OH- anion, names of bases end in hydroxide. The cation is simply named first
What is an acid-base reaction?
When an acid and base are mixed, the H+ from the acid combines with the OH- from the base to form H2O(l)
0.39 mol of LiNO3 in 6.50 L of solution
molarity = 6.0×10−2 M