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ISU CHEM 167 - Practice Exam #3

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1. Which of the following atoms is the largest? a) K b) Ca2+ c) Si d) Na+2. Effective nuclear charge is a) the charge of the nucleus. b) when the charge of one atom affects the charge of another. c) the positive charge felt by an electron in an atom. d) the charge of an atom.3. What is the relationship between the ionization energy of an anion with a 1- charge such as Cl- and the electron affinity of the neutral atom, Cl? a) the ionization energy and the electron affinity are both positive numbers. b) they are the same number except electron affinity is positive and ionization energy is negative. c) they are the same number except electron affinity is negative and ionization energy is positive. d) the ionization energy and the electron affinity are both negative numbers.4. Which of the following has the highest lattice energy? a) CO2 b) CaF2 c) KCl d) SrBr25. When covalent bonds are formed between atoms, what is observed? a) The energy of the system is increased. b) The energy of the system is decreased. c) Work is done on the system. d) The system is endothermic.6. Draw the Lewis structure for BBr3 and NCl3. Which compound(s) is/are polar? What is the geometric shape of both of these, and what theory explains the shapes?7. Give the common shape name and an example of a molecule with the molecule notation of AX2E2. Is this molecule polar?8. How many sigma and pi bonds are in the following molecule? 9. Silver (#47) crystallized in a face-centered cubic unit cell that has an edge length of 3.011 Å (10-10 m). The atom in the center of the face is in contact with the corner atoms. Calculate the density of the silver.10. A band structure: a) is the structure a metal is shaped into. b) is pertaining to nonmetals. c) contains a valence and conduction band. d) is where the electrons move in localized orbitals.11. An n-type dopant: a) has less valence electrons than the semiconductor. b) has more valence electrons than the semiconductor. c) has the same number of valence electrons as the semiconductor. d) always has less total electrons than the semiconductor.12. What intermolecular forces are present in NF3? a) only dispersion forces b) only dipole forces c) dispersion and dipole forces d) none13. A common byproduct of condensation polymerization is: a) ethanol b) water c) oxygen d) methane14. Polymers that melt/deform when heated are referred to as: a) isotactic polymers b) thermosetting polymers c) alternating copolymers d) thermoplastic polymers15. The contents of the closed box in each of the following illustrations represent a system, and the arrows show the changes to the system during some process. The lengths of the arrows represent the relative magnitudes of q and w. Which of the diagrams show an overall ∆E>0, and which are endothermic? q q q w w w A. B. C. 16. Ethanol (C2H5OH) melts at -114⁰C. The enthalpy of fusion of ethanol is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. What is the minimum amount of heat required to convert 15 g of ethanol at -125⁰C to a liquid?17. 2 NO(g) + O2(g) 2 NO2(g) ∆H= -113.1 kJ How much heat is released when 2.0 g of NO is thoroughly

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