Chem SI 12/2 Exam 2 Review PDF

Chem SI 12/2 Exam 2 Review SIGN IN PLEASE :) HALLIE POPAT  Please fill out this form :) 12/03/2024 2 4 Classes of Hydrocarbons  Alkanes: contain only single bonds o End -ane  Alkenes: contain one or more double bonds o End -ene...

Chem SI 12/2 Exam 2 Review SIGN IN PLEASE :) HALLIE POPAT  Please fill out this form :) 12/03/2024 2 4 Classes of Hydrocarbons  Alkanes: contain only single bonds o End -ane  Alkenes: contain one or more double bonds o End -ene  Alkynes: contain one or more triple bonds o End -yne  Aromatic: hydrocarbons have a specific six-carbon ring with three double bonds  Naming Prefix: Root: Ending:  Branches off main chain and  ane if alkane where  ene if alkene  Where double or tripple bond is  yne if alkyne Functional Groups Functional Groups Stoichiometry calculations Example: Balancing equations Law of conservation of mass – in all chemical reactions, atoms are neither created nor destroyed the number of atoms on the reactant side is equal to the number of atoms on the product side for each element Energy Diagrams  Solvation Polar Solutes in Polar Solvents Polar solutes dissolve in polar solvents. These molecules interact through hydrogen bonding. o 1. Hydrogen bonds between the solute break. o 2. New hydrogen bonds form between the solute and solvent. o 3. We now have a lower potential energy as a result. Nonpolar Solutes in Nonpolar Solvents Non-polar solutes dissolve in non-polar solvents. These molecules interact through dispersion forces or weak dipole-dipole interactions. Ionic Compounds Soluble ionic compounds dissolve because the ion-dipole forces are stronger than the ionic bonds. o Ionic bonds between cations and anions are replaced by ion-dipole interactions with water. o Insoluble ionic compounds are large and have large charge (+2/-2) Solute Concentration Concentration is the amount of solute in a given volume or mass of solution. Units of concentration include the following: o Mass/ volume (m/v) or % mass/ volume (%m/v) o Molarity (moles solute/liters solution) We express concentration by mass of solute/mass of solution. We can also measure these concentrations in parts per million (ppm) and parts per billion (ppb) Dilute solutions contain less solute, they are diluted.  Osmosis When solutes cannot pass through a membrane, the solvent will move instead. Osmosis refers to the flow of solvent (usually water!) through a membrane to equalize concentrations. o Osmotic Pressure: amount of pressure applied to the more concentrated solution to prevent osmosis. o Reverse Osmosis: pressure greater than the osmotic pressure causing water to flow against the gradient  Tonicity Used to predict direction of osmosis. o Hypertonic solution: the more concentrated solution o Hypotonic solution: the more dilute solution o Isotonic solutions: solutions with equal concentration Osmosis always occurs from the hypotonic solution to the hypertonic solution. Dialysis occurs from hypertonic to hypotonic solution. o Osmolarity is the total concentration of all solute particles in solution. During osmosis, water moves from low solute to high solute (as a way to dilute it). o In hypertonic solutions, we shrink/crenate, water flows out of cell. o In hypotonic solutions, we swell and burst/hemolysis, water flows into the cell.  Arrhenius Definitions Arrhenius Acids produce hydronium ions (H 3 O + which is essentially a water H 2 O with an additional H+ o Electrolytes o Sour o Corrosive Arrhenius Bases produce hydroxide ions (OH - which is essentially a water H 2 O with a H + removed) o Electrolytes o Soapy/slippery o Bitter/chalky T U E S D AY , D E C E M B E R 3 , 2 0 2 4 SAMPLE FOOTER TEXT 14 Brönsted-Lowry Definition Brönsted-Lowry Acids are proton donors. * Don’t forget, like before, our idea of protons are H+ Brönsted-Lowry Bases are proton acceptors. Only certain hydrogens can be donated, these are known as acidic hydrogens. These are normally found at the beginning of the acid formula. Acids and Bases Strength The strength of an acid/base is the extent as to which it dissociates in water. * Strong acids and bases dissociate completely in water. * Weak acids and bases dissociate partially in water. - Produce few ions in aqueous solution and these reactions are reversible (reactants>products) Le Châtelier's Principle This principle is also heavily applicable in weak-acid and weak-base reactions. * If you remove something, shift towards what you removed to create more of it. * If you are adding something, shift away from what you added to use the excess up. * If you do something to once reactant/product, you MUST do the same to any other reactant/product. pH and Kw The pH of a solution is a quantitative measure of the concentration of hydronium ions in solution. - [H3O+] = molar concentration (mole/L) of H3O+ - [OH–] = molar concentration of OH– - Physiological pH varies between 7.35 and 7.45. In pure water, we have a pH of 7, meaning the concentration of hydroxide and hydronium ions is 1 × 10^–7 M. - The product of these two concentrations is equal to the ion-product Buffers Buffers are solutions that resists changes in pH when small amounts of acid or base are added. - This is how acid-base homeostasis works to prevent acidosis and alkalosis. A buffer is a mixture: - Weak acid + its conjugate base. - Weak base + its conjugate acid. pH range maintained by buffer depends on identity of the weak acid. Buffer capacity depends on the concentration of the buffer components  What mass (in grams) of sucrose (C 12 H 22 O 11 ) is contained in 250 mL of a 0.250 M sucrose solution? Molar Mass of Sucrose: 343.30 g/mol A. 42.9 grams of sucrose B. 21.4 grams of sucrose C. 10.7 grams of sucrose D. 33.6 grams of sucrose  What mass (in grams) of sucrose (C 12 H 22 O 11 ) is contained in 250 mL of a 0.250 M sucrose solution? Molar Mass of Sucrose: 343.30 g/mol A. 42.9 grams of sucrose B. 21.4 grams of sucrose C. 10.7 grams of sucrose D. 33.6 grams of sucrose  A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters. The molarity of the final solution is ________. A. 0.75 M B. 30.0 M C. 15.0 M D. 1.5 M  A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters. The molarity of the final solution is ________. A. 0.75 M B. 30.0 M C. 15.0 M D. 1.5 M  According to the Brønsted-Lowry definition, ________. A. An acid is a proton donor B. An acid is a proton acceptor C. A base is a proton donor D. A base is a proton acceptor E. A and D F. B and C  According to the Brønsted-Lowry definition, ________. A. An acid is a proton donor B. An acid is a proton acceptor C. A base is a proton donor D. A base is a proton acceptor E. A and D F. B and C  The [H 3 O + ] of a solution with pH = 2.0 is ________. A. 1.0 x 10 ^2 B. 1.0 x 10 ^-2 C. 3.0 x 10 ^-1 D. 3.0 x 10 ^1  The [H 3 O + ] of a solution with pH = 2.0 is ________. A. 1.0 x 10 ^2 B. 1.0 x 10 ^-2 C. 3.0 x 10 ^-1 D. 3.0 x 10 ^1 To go from [H 3 O + ] to pH, you have to use 10 ^-pH.  A human sample of blood was measured to have [H 3 O + ] = 7.94 × 10 −9. What is true about this solution? A. The solution is basic. B. The solution is acidic. C. The solution contains more hydronium ions than water. D. The solution does not contain OH - ions. E. The pH of the solution is 7.94.  A human sample of blood was measured to have [H 3 O + ] = 7.94 × 10 −9. What is true about this solution? A. The solution is basic. B. The solution is acidic. C. The solution contains more hydronium ions than water. D. The solution does not contain OH - ions. E. The pH of the solution is 7.94.  According to the mole interpretation, how many grams of N 2 O 4 could be produced by the complete reaction of 3.40 grams of N 2 O 5 and excess O 2 ? 2N 2 O 5 → 2N 2 O 4 + O 2 A. 3.40 g N 2 O 4 B. 2.90 g N 2 O 4 C. 1.45 g N 2 O 4 D. 7.80 g N 2 O 4  According to the mole interpretation, how many grams of N 2 O 4 could be produced by the complete reaction of 3.40 grams of N 2 O 5 and excess O 2 ? 2N 2 O 5 → 2N 2 O 4 + O 2 A. 3.40 g N 2 O 4 B. 2.90 g N 2 O 4 C. 1.45 g N 2 O 4 D. 7.80 g N 2 O 4  Which statement is a correct application of Le Châtelier's principle? A. Addition of a substance to the right side will result in a shift of equilibrium to the right. B. Removal of a substance from the left side will result in a shift of equilibrium to the right. C. Addition of heat to an exothermic reaction will result in a shift of equilibrium to the right. D. Removal of a substance from the left side will result in a shift of equilibrium to the left.  Which statement is a correct application of Le Châtelier's principle? A. Addition of a substance to the right side will result in a shift of equilibrium to the right. B. Removal of a substance from the left side will result in a shift of equilibrium to the right. C. Addition of heat to an exothermic reaction will result in a shift of equilibrium to the right. D. Removal of a substance from the left side will result in a shift of equilibrium to the left. Rules: 1. Exothermic has heat as a product, endothermic has heat as a reactant. 2. If we add a substance, we shift away from it; we want to use it up. 3. If we remove a substance, we shift towards it; we want to make more.  The amine given shown is ______ A. Primary B. Secondary C. Tertiary D. Quaternary Match the following pictures to the correct functional group name Match the following pictures to the correct functional group name  What is the correct IUPAC name for the following compound? A. Methyl Propanoate B. Propanal C. Propyl Methanoate D. Propyl Methanal  What is the correct IUPAC name for the following compound? A. Methyl Propanoate B. Propanal C. Propyl Methanoate D. Propyl Methanal  The molarity of a solution of 10 g of NaCl in 300. mL of solution is ________.  The molarity of a solution of 10 g of NaCl in 300. mL of solution is ________.  What is the pH of a solution that has a [OH - ] = 5.5 x 10^ -3 M?  What is the pH of a solution that has a [OH - ] = 5.5 x 10^ -3 M?  What is the concentration of H + in a solution with pH = 7.50?  What is the concentration of H + in a solution with pH = 7.50?  Patients experiencing chest pain often take nitroglycerin. If 5.0 mL of a 3.0% (m/V) C 3 H 5 N 3 O 9 solution is administered to a patient, what mass of C 3 H 5 N 3 O 9 was provided? Nitroglycerin has a molar mass of 227.09 g/mol.  Patients experiencing chest pain often take nitroglycerin. If 5.0 mL of a 3.0% (m/V) C 3 H 5 N 3 O 9 solution is administered to a patient, what mass of C 3 H 5 N 3 O 9 was provided? Nitroglycerin has a molar mass of 227.09 g/mol. Thanks for coming! Any other questions?