Quantum Mechanics and Chemical Bonding Quiz
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Quantum Mechanics and Chemical Bonding Quiz

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Questions and Answers

Which of the following compounds would form a molecular solid?

  • gold
  • C(graphite)
  • C10H22 (correct)
  • CaO

    • When the temperature is held constant at 140°C, what phase changes occur if the pressure is increased from 0.25 atm to 1.4 atm?

  • solid → liquid → vapor
  • gas → solid → liquid
  • liquid → solid → gas
  • gas → liquid → solid (correct)

    • What is the mole fraction of ethanol in a solution made by dissolving 14.6 g of ethanol in 53.6 g of water?

  • 0.0964
  • 0.272
  • 0.214
  • 0.106 (correct)

    • Which statement about a supersaturated solution is true?

    <p>The solution contains more than the equilibrium amount of solute.</p> Signup and view all the answers

    What is the expected freezing point of a 0.50 m solution of Na2SO4 in water, given that Kf for water is 1.86°C/m?

    <p>-6.5°C</p> Signup and view all the answers

    What is the rate law for the reaction 2 H2(g) + 2 NO(g) → N2(g) + 2 H2O(g) given it is first order in H2 and second order in NO?

    <p>Rate = k[H2][NO]2</p> Signup and view all the answers

    If the concentration of B in the rate law Rate = k[A][B]2 is increased by a factor of 2.00, what happens to the rate of reaction?

    <p>The rate will increase by a factor of 4.00.</p> Signup and view all the answers

    Which statement about the stability of Be2, Be2+, and Be2- is correct?

    <p>Be2 is more stable than either Be2+ or Be2-.</p> Signup and view all the answers

    What is the final temperature of a gas if its volume decreases from 350 mL to 125 mL at constant pressure and initial temperature is 25°C?

    <p>70°C</p> Signup and view all the answers

    How many grams of Mg are needed to produce 35 mL of H2 at STP in the given reaction?

    <p>29 g</p> Signup and view all the answers

    According to the kinetic molecular theory, what will happen to gas pressure if the temperature of the gas decreases?

    <p>The pressure of the gas decreases.</p> Signup and view all the answers

    Which reaction is the most exothermic?

    <p>CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l)</p> Signup and view all the answers

    What is the calculated ΔH for the reaction of BaCO3 decomposing into BaO and CO2?

    <p>-1376.0 kJ</p> Signup and view all the answers

    What are the signs of ΔH and ΔS when a substance melts at its normal melting point?

    <p>+, -</p> Signup and view all the answers

    Which compound has the highest boiling point?

    <p>HOCH2CH2OH</p> Signup and view all the answers

    Which statement accurately reflects the Heisenberg uncertainty principle?

    <p>We cannot precisely predict both the momentum and the position simultaneously.</p> Signup and view all the answers

    What are the two quantum numbers for an orbital with n=4?

    <p>n=4, l=3</p> Signup and view all the answers

    Which type of cell involves a non-spontaneous reaction?

    <p>Electrolytic cell</p> Signup and view all the answers

    What is the general trend of ionization energy and electronegativity across a period?

    <p>Both increase as one moves to the right and both decrease as one descends a group.</p> Signup and view all the answers

    Which of the following elements has the largest atomic radius?

    <p>K</p> Signup and view all the answers

    What change will increase the amount of NH3 in the given reaction equilibrium?

    <p>Removing NO from the tank</p> Signup and view all the answers

    Based on the electronegativity values of P (2.1) and Cl (3.0), what can be said about PCl3?

    <p>It has a polar covalent bond with a partial positive charge at P.</p> Signup and view all the answers

    Which statement is incorrect regarding the formation of B2+?

    <p>They will react in the following way 2A + B -&gt; A2B.</p> Signup and view all the answers

    What will be the concentration after 15 minutes for a first order reaction with an initial concentration of 4 M and a half-life of 5 minutes?

    <p>0.025 M</p> Signup and view all the answers

    Which is true about VSEPR theory and covalent bonds?

    <p>A sigma bond can form from head-on overlap of p orbitals.</p> Signup and view all the answers

    What occurs when a small amount of NaOH is added to a solution of CH3COOH/CH3COO-?

    <p>The OH- ions reacts with the conjugated base</p> Signup and view all the answers

    In a galvanic cell, how is the cathode characterized and what reaction occurs?

    <p>Negative, reduction</p> Signup and view all the answers

    What is the correct maximum number of electrons that can be accommodated by a subshell with l=3?

    <p>14</p> Signup and view all the answers

    What is TRUE about the elements with given atomic numbers and mass numbers?

    <p>The three elements have the same number of nucleons.</p> Signup and view all the answers

    Which molecule and its assigned geometry is NOT TRUE?

    <p>ACl5 - trigonal byriamidal</p> Signup and view all the answers

    Which statement about ionization energies is FALSE?

    <p>The first ionization energy of N is higher than that of O.</p> Signup and view all the answers

    What is the bond order of F2- and is it paramagnetic or diamagnetic?

    <p>Bond order of 1/2 and diamagnetic</p> Signup and view all the answers

    Which of the following substances exhibits only dipole-dipole interactions and London forces?

    <p>HBr</p> Signup and view all the answers

    Which compound would exhibit the highest osmotic pressure in a solution?

    <p>0.3M Ca3(PO4)2</p> Signup and view all the answers

    What concentration of glucose is present when 171 g is dissolved in a 1000 g solution? (Mw=342 g/mol)

    <p>1 M</p> Signup and view all the answers

    What will favor the solubility of an ionic solid?

    <p>Low lattice energy on solid, high hydration energy on ions</p> Signup and view all the answers

    Which statement defines a Lewis base?

    <p>Electron pair donor</p> Signup and view all the answers

    Which molecules correspond with the following acid-base pairs: HCl, H2O, H3O+, Cl-?

    <p>Acid: HCl → conjugate base: Cl- | base: H2O → conjugate acid: H3O+</p> Signup and view all the answers

    What is the pH of a 0.15M HOCl solution if Ka = 3.5×10^-8?

    <p>4.2</p> Signup and view all the answers

    Study Notes

    Quantum Mechanics

    • Heisenberg uncertainty principle states that the position and momentum of an electron cannot be precisely determined simultaneously.
    • For a principal quantum number (n) of 4, the possible values for the angular momentum quantum number (l) are 0, 1, 2, and 3.

    Chemical Bonding

    • Electronegativity and ionization energy generally increase across a period and decrease down a group.
    • The larger the overlap between atomic orbitals, the stronger the bond.
    • Sigma bonds can form from the head-on overlap of s orbitals and p orbitals, or from the overlap of two hybrid orbitals.
    • Pi bonds can form from the side-by-side overlap of two p orbitals.
    • VSEPR theory can be used to predict the shapes of molecules based on the number of electron pairs around a central atom.
    • Molecular orbital theory can be used to describe the electronic structure of molecules. The bond order is the number of bonding electrons minus the number of antibonding electrons.
    • The higher the bond order, the stronger the bond.
    • A molecule is diamagnetic if all of its electrons are paired, and paramagnetic if it has unpaired electrons.

    Intermolecular and Surface Chemistry

    • Ionic compounds have high lattice energy and low hydration energy.
    • The solubility of ionic compounds is favored when the lattice energy is low and the hydration energy is high.
    • A Lewis base is an electron pair donor, while a Lewis acid is an electron pair acceptor.

    Acid-Base Chemistry

    • The strength of an acid is related to the stability of its conjugate base.
    • A strong conjugated base results in a weak acid.
    • The Henderson-Hasselbalch equation (pH=pKa + log(A-/HA)) can be used to calculate the pH of a buffer solution.

    Thermodynamics

    • The enthalpy change (ΔH) is negative for an exothermic reaction and positive for an endothermic reaction.
    • The entropy change (ΔS) is positive for a process that increases the disorder of the system and negative for a process that decreases the disorder.
    • The Gibbs free energy change (ΔG) is a measure of the spontaneity of a reaction.

    Kinetics

    • The rate law for a reaction expresses the relationship between the rate of the reaction and the concentrations of the reactants.
    • The rate constant (k) is a proportionality constant that relates the rate of a reaction to the concentrations of the reactants.
    • The half-life of a first-order reaction is independent of the initial concentration of the reactant.

    Electrochemistry

    • A galvanic cell is an electrochemical cell that produces electrical energy from a spontaneous chemical reaction.
    • The cathode is the electrode at which reduction occurs.
    • The anode is the electrode at which oxidation occurs.
    • The standard cell potential (ε°) is a measure of the potential difference between the two electrodes of a galvanic cell under standard conditions.

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    Description

    Test your knowledge on key concepts in quantum mechanics and chemical bonding. This quiz covers the Heisenberg uncertainty principle, quantum numbers, VSEPR theory, and molecular orbital theory. Challenge yourself to understand the foundational principles of these important topics in chemistry and physics.

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