Download Chemistry Review for End of year final honors

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Final Review
Mol to gram, mol to Liter and mole to particle conversions
1.) Avagadro’s number of representative particles is equal to what two values?
2.) How many moles of tungsten atoms are there in 4.8 x 10 25 atoms of tungsten?
3.) How many atoms are in 0.075 mol of titanium
4.) What is the volume, in liters, of 6.8 mol of Kr gas at STP?
5.) Which of the elements exist as diatomic molecules? What do you need to do when
calculating their atomic masses?
Stoichiometry, Conservation of Matter, Limiting Reactants
1.) In a chemical reaction, the mass of the products has what relationship with the original
2.) How many liters of oxygen are required to react completely with 2.4 liters of hydrogen to
form water? 2H2 + O2  2H2O
3.) Calculate the number of moles of Al2O3 that are produced when 0.60 mol of Fe is
produce in the following reaction: 2Al + 3FeO  3Fe + Al2O3
4.) When two substances react to form products, the reactant, which is used up in the
reaction, is called ______________________. The reactant left over is called
5.) What is the maximum number of grams of PH3 that can be formed when 6.2 g of
phosphorous reacts with 4.0 g of hydrogen to form PH3? P4 + 6H2  4PH3
6.) The first step in most stoichiometry problems that already have a balanced equation is to
convert to what unit?
7.) How many liters of NH3 at STP will react with 5.3 g of O2 to form NO2 and water?
4NH3 + 7O2  4NO2 + 6H2O
1.) What is the amount of heat required to raise the temperature of 100 g of aluminum by 10
C? Specific heat capacity of aluminum is 0.21 J/g C
2.) A piece of metal is heated, then submerged in cool water. What will happen in the
transfer of heat? (Where does the heat come from, where does it go to?)
3.) If the heat involved in a chemical reaction (q or ΔH) has a negative value, what does this
4.) A process that absorbs heat is called a(n) ____________________ process.
5.) Calculate the energy required to produce 6.0 mol Cl2O7, on the basis of the following
equation: 2Cl2 + 7O2 + 130 J  2Cl2O7
6.) If you were to touch a flask in which an endothermic reaction was happening, what
would you feel?
7.) Calculate the energy released when 24.8 g Na2O reacts in the following reaction:
Na2O + 2HI  2NaI + H2O
ΔH = -120.00 J
8.) Summations from a table of data ΣΔHproducts – ΣΔHreactants = ΔHreaction
9.) Remember that all ΔH values for elements are not given since they are assumed to be zero.
Gas Laws
1.) List the five gas laws and give their formulas
2.) What happens to the temperature of a gas when it is compressed?
3.) A gas occupies a volume of 0.2 L at 10. kPa. What volume will it occupy at 155 kPa?
4.) The combined gas law relates which three physical values?
Acids and Bases
1.) If the hydrogen ion concentration of a solution is 1 x 10 –10 what type of solution are you
working with? Acid, base or neutral?
2.) When water breaks down into its IONS, write a reaction for this.
3.) Which type of solution has a pH of 8?
4.) The pH of a solution in which [OH-] = 1 x 10 –4 is what?
5.) What is an acid/base according to the Arrhenius definition? A Bronsted-Lowry? A
6.) Which acid and base compounds fully dissociate in water?
7.) What compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry Base?
What is this compound called when it can behave as both acid and base?
8.) Know titration curves for SA/SB, WA/SB and SA/WB. Know equivalencies for end
point and halfway point for all three.
9.) Know the equilibrium expression for acid and base chemistry and how to substitute
appropriate values into it.
10.) Know the definition of a buffer and how to calculate the pH of a buffer.
Reaction Rates and Equilibrium
1.) What is activation energy?
2.) Why does a higher temperature cause a reaction to go faster?
3.) Why does a higher concentration cause a reaction to go faster?
4.) What happens to a catalyst in a reaction?
5.) If the reaction is reversible, what are the relative amounts of reactant and product at the
end of reaction?
6.) If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse
7.) What happens to reactions at equilibrium when more reactant is added to the system?
8.) In an exothermic reaction at equilibrium, what is the effect of lowering the temperature?
9.) Be able to use Le Chatlier’s principle to predict shifts in a system that is disturbed.
Atomic Theory and Bonding
Write electron configurations for the following elements:
1.) C
2.) S
3.) Ni
4.) Al
Understand the periodic trends of electronegativity, ionization energy and atomic/ionic radius
that stems from the repeating valence orbital configurations of elements within the same
List all the sublevels in each of the following principle energy levels
1.) 4th
2.) 2nd
Draw Lewis Dot structures for the following compounds and understand the theory behind the
different shapes they make.
Oxidation numbers, half reaction, balancing redox reactions and electrical potential as studied
during the previous 6 days of class.