Chemistry Spring Study Guide and Practice Name______
For each of the following objectives write a study note (explanation, sample problem, example, etc.) for each objective and vocabulary word…if a word appears more than once, relate it to that specific objective.
Answer practice questions.
Objective 1 – Science and Society
· read article related to a current event in chemistry, analyze and draw conclusions
· read data table and draw conclusions
· knowledge of global warming
Objective 2 – Nomenclature
· ionic compounds
· molecular compounds
· acids
· Vocabulary
o Chemical formula
o Polyatomic ions
o Diatomic molecules
Nomenclature
SUMMARIZE the rules for each of the following:
a. Binary compounds, including metals with multiple oxidation states
b. Molecules using Greek prefixes.
c. Compounds with polyatomic ions. including stealth bomber and common polyatomic ions
d. Binary acids
e. Oxyacids
f. predicting formula from the charge (ex. what would be the formula for calcium and oxygen)
for rule “f” give two examples
1.
2.
Provide the correct chemical formulas for the following compounds:
1. barium nitrite
2. phosphorous acid
3. potassium nitride
4. aluminum sulfide
5. chromium (VI) oxide
6. tin (III) phosphide
7. dinitrogen pentasulfide
8. manganese (VI) chlorate
9. ammonium hydrogen sulfite
10. hydrofluoric acid
11. tetraphosphorous decasulfide
12. iron (III) acetate
13. Strontium hyponitrite
14. phosphoric acid
15. trisulfur heptaiodide
16. manganese (VII) perchlorate
17. ammonium hydrogen carbonite
18. hydrobromic acid
19. pentaphosphorus nonasulfide
Provide the correct name for the following chemical formulas:
20. Cr(SO2)3
21. H2CrO4
22. CCl4
23. Zn(OH)2
24. K2Cr2O7
25. HNO3
26. (NH4)2CO2
27. Sn(NO2)4
28. H2Cr2O7
29. CF4
30. AgNO3
31. Si4O8
32. Li2SO4
33. HNO2
34. (NH4)2S
35. Mn(HCO3)7
36. HClO3
37. Na2CrO4
38. CCl4
39. H2CO3
40. NiCl2
Objective 3 – Balancing Equations
· given a skeleton equation for a reaction, choose the correct coefficients
· interpret mole relationships given a balanced equation
· given a sentence equation, write and balance the equation
Balance the following simple reaction equations.
a. __Zn(s) + __HCl(aq) ® __ZnCl2(aq) + __H2(g)
b. __Fe(s) + __O2(g) ®__Fe2O3(s)
c. __FeO(a) + __O2(g) ® __Fe2O3(s)
d. __Au2S3(s) + __H2(g) ® __Au(s) + __H2S
e. __Cr(s) + __S8(s) ® __Cr2S3(s)
Balance the following equations:
a. ___Al2(SO4)3 (aq) + ___K3PO4(aq) ® ___AlPO4(s) + ___K2SO4(aq)
b. ___NaOH (aq) + ___H2SO4(aq) ® ___ H2O + ___Na2SO4(aq)
c. ___Cu(s) + ___AgNO3 (aq) ® ___Ag(s) + ___Cu(NO3)2(aq)
d. ___C4H10 (g) + ___O2(g) ® ___CO2(g) + ___H2O(g)
e. ___NaHCO3(s) ® ___Na2CO3(s) + ___CO2 (g) + ___H2O (g)
f. ___Co2(SO4)3 (aq) + ___Ca(NO3)2(aq) ® ___Co(NO3)3(aq) + ___ CaSO4(s)
g. ___KOH (aq) + ___H3PO4(aq) ® ___H2O (l) + ___K3PO4(aq)
Objective 4 – Mole Conversions
· mass <=> mole <=> particle
· Avogadro’s number w/units (atoms, molecules, formula units)
· STP
· volume to mole / mole to volume conversions
· Vocabulary
o Mole
o Avogadro’s number
o Molar mass
Dimensional Analysis metric and density
1. What is the density in kg/m3 of a 13.5 g. square block of wood that is 2.5 in per side?
2. How many millimeters are there in 1.23 x 10-6 kilometers?
3. Convert 4.75 centimeters to meters
Dimensional analysis Conversions
1. How many atoms are in 1 formula unit of each of the followings?
a. Ca3P2
b. (NH4)3PO4
c. Al2(H2PO4)3
2. Find the mass of the following
a. 2.87 x 1021 formula units of (NH4)2SO4
b. 0.0032 moles of P4O10
c. .0678 Liters of CO2
3. How many molecules are in each of the following:
a. 0.25 moles of N2O5
b. 2.5 grams of N2O5
c. 3.5 liters of N2O5
4. How many moles are in each of the following
a. 1.67x 1022 atoms of copper
b. 3.87 grams of calcium chloride
c. 2.41 liters of CO2 at STP
5. How many grams are in the following:
a. 2.87 x 1022 atoms of cesium
b. 1.76 liters of CH4 gas at STP
Objective 5 – Stoichiometry
· Use a balanced equation to
o determine a mole to mole relationship
o calculate moles or mass of a product
o determine a limiting reactant
o calculate theoretical yield
o calculate percent yield
· Vocabulary
o percent yield
o exess reagent
o theoretical yield
o actual yield
o ideal gas law
o Precipitate
Objective 6 – Water and Aqueous Solutions
· calculations using molarity
· dilutions
· solubility
· H-bonding
Consider the following reaction:
2(NH4)3PO4 (aq) + 3Ca(OH)2(aq) ® 6NH4OH (aq) + Ca3(PO4)2(s)
a. How many grams of Ca3(PO4)2 would be produced when 1.5 grams of (NH4)3PO4 is reacted with an excess of Ca(OH)2?
b. What is the theoretical yield (in grams) of Ca3(PO4)2 when 2.5 grams of (NH4)3PO4 are reacted with 2.5 g Ca(OH)2?
c. What is the limiting reagent in the above reaction? ______
d. How much excess reagent is left unreacted?
e. How many grams of Ca3(PO4)2 would have been recovered in the laboratory if the percent yield was 98.5%?
Consider the following unbalanced reaction equation when answering questions 6-10. Make sure you include all your calculations when answering these questions.
K2CrO4(aq) + Al(C2H3O2)3(aq) ® Al2(CrO4)3(s) + KC2H3O2 (aq)
a. How would you prepare 50.0 ml of a 0.150 M solution of K2CrO4?
b. How would you prepare 75.0 ml of a 0.120 M solution from a pre-prepared stock solution of 2.75 M Al(C2H3O2)3 solution?
c. How many grams of Aluminum chromate ought to be produced when these two solutions are reacted together?
Using the following equation:
2 NaOH + H2SO4 à 2 H2O + Na2SO4
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?
Using the following equation:
Pb(SO4)2 + 4 LiNO3 à Pb(NO3)4 + 2 Li2SO4
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?
Objective 7 – Reaction Types
· Given a reaction, classify as
o synthesis
o decomposition
o single replacement
o combustion
o double replacement precipitation
o double replacement acid/bas neutralization
o Vocabulary
o Chemical reactions
o Reactants
o Products
o Endothermic
o Exothermic
o Coefficient
o Law of conservation of mass
o Synthesis
o Decomposition
o Single replacement
o Double replacement
o Combustion
o Greenhouse gases
o Reactive
Reaction Chemistry:
Identify the five reaction types and provide a model describing each type
Name Model
For the following reactions identify the reaction type, predict the appropriate products, and balance the final equation
a. Ca(s) + P(s) ®
b. C3H7OH (g) + O2(g) ®
c. (NH4)2CO3(aq) + CrCl3(aq) ®
d. NH4ClO3 ®
e. MgO(s) + H2O(l) ®
f. Li2O (s) + SO2(g) ®
For the following reactions identify the reaction type, predict the appropriate products, and balance the final equation.
a. Aluminum metal reacts with an aqueous solution of iron (II) chloride
b. A solution of copper (II) nitrate reacts with a solution of ammonium hydroxide
c. Solid calcium carbonate decomposes at high temperature
d. ammonium hydrogen sulfate decomposes
Objective 8 – Equilibrium and Reaction Rates
· factors influencing reaction rates
· catalyst
· LeChatelier’s principle with concentration, pressure and enthalpy
· definition of equilibrium
Predict the direction of the equilibrium shift for each of the following processes:
1) H2(g) + Cl2(g) ⇄ 2 HCl(g)
What direction will the equilibrium shift when the partial pressure of hydrogen is increased?
2) 3 H2(g) + N2(g) ⇄ 2 NH3(g)
Given that this reaction is exothermic, what direction will the equilibrium shift when the temperature of the reaction is decreased?
3) 2 NO2(g) ⇄ N2O4(g)
In what direction will the equilibrium shift if the total pressure is decreased?
4) NH4OH(aq) ⇄ NH3(g) + H2O(l)
In what direction will the equilibrium shift if ammonia is removed from the container as soon as it is produced?
5) 2 BH3(g) ⇄ B2H6(g)
If this equilibrium is taking place in a piston with a volume of 1 L and I compress it so the final volume is 0.5 L, in what direction will the equilibrium shift?
Objective 9 – Acid/Base Reactions
· characteristics of acids
· characteristics of bases
· pH scale
· identify acid/base reactions
· calculations involving pH
· Vocabulary
o Acid
o Base
o Neutral
o pH
1. An acid is a proton donor or accepter?
2. A Base is a proton donor or accepter?
Water is one of the most important molecules in the body. Cells are made mostly of water and water is required for almost every metabolic reaction in the body. The force of attraction between water molecules is so strong that the oxygen atom of one molecule can actually remove the hydrogen from other water molecules. This reaction is known as dissociation, and it takes place in our cells. Water (H20) dissociates into H+andOH- ions. A charged atom or molecule is called an ion. The OH- ion is called the hydroxide ion, while the H+ion is called the hydrogen ion. Free H+ ions can react with another water molecule to form the H3O+ or hydronium ion. The human body requires a neutral pH for many reasons. One reason cells like a neutral pH is for proteins. Basic or acidic solutions denature proteins (change their shape) so they no longer work.
1. What is dissociation?
2. What is the chemical formula for water?
3. What is an ion?
4. Name the 2 ions form when water dissociates.
5. What is the hydroxide ion?
6. What is a hydrogen ion?
7. What is the hydronium ion and its formula?
Acidity or alkalinity is a measure of the relative amount of H+ and OH- ions dissolved in a solution. Neutral solutions have an equal number of H+ and OH- ions. Acids have more H3O+ ions (H+) than OH- ions. Acids taste sour and can be corrosive. Digestive fluids in the body are acidic and must be neutralized by buffers. Bases contain more OH- ions than H3O+ ions. Bases taste bitter and feel slippery.
When an acid is combined with a base, neutralization occurs. The result of neutralization is a salt and water. Neutralization helps return our body pH to neutral. The process of our bodies maintaining neutral pH so that proteins can work properly without being denaturated (unfolded) is known as homeostasis.
8. How do you measure for acidity or alkalinity?
9. What is a neutral solution?
For 1-3 Determine [H+] [OH-] ph and pOH:
1. solution made by adding water to 15 grams of hydroiodic acid until the volume of the solution is 2500 mL?
2. What is the pH and pOH of a solution that was made by adding 400 mL of water to 350 mL of 5.0 x 10-3 M NaOH solution?
3. What is the pH and pOH of a solution with a volume of 5.4 L that contains 15 grams of hydrochloric acid and 25 grams of nitric acid?
4. A swimming pool has a volume of one million liters. How many grams of HCl would need to be added to that swimming pool to bring the pH down from 7 to 4? (Assume the volume of the HCl is negligible)
Objective 10 – Thermochemistry
· endothermic vs. exothermic for both physical and chemical processes
· P.E. curve/diagram interpretation
· activation energy
· enthalpy, ΔH
Answer the following questions based on the potential energy diagram shown here:
a. Does the graph represent an endothermic or exothermic reaction, explain?
b. Label the position of the reactants, products, activation energy and activated complex.
c. Determine the heat of reaction, ΔH, (enthalpy change) for this reaction.
d. Determine the activation energy, Ea for this reaction.
e. How much energy is released or absorbed during the reaction?
f. How much energy is required for this reaction to occur?
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Objective 11 – Chemical Bonding
· VSEPR
· polarity
· IMF’s
· characteristics of ionic compounds
· characteristics of molecular compounds
· Vocabulary
o Ionic bonding
o Covalent bonding
o Cations
o Anions
o Valance electrons
o Lewis dot structure
o Octet rule
o Valance electrons
o Polar molecules
Additional notes: