Fall, 2013- Chemistry 2311 Homework Problems- Chapter 1 (1) For each of the following arrangement of atoms (a) draw a correct Lewis structure and (b) indicate the formal charge associated with each of the atoms. (a) (b) (c)(d) H N N Nhydrazoic acid (e) CHHOformaldehyde (f) (g)CCOHH HHethylene oxide (h) (i) (j)(k) NOnitric oxide (l) (m)(2) Draw a constitutional isomer for each of the following. (a) C CHCHOHHHHHH (b) C CHHClH2CH (c) C C CCHOHHHHH(d) H3C CCH3O (e) C CHHHNH2HH (f)(g) (h) CH3CH2C(Cl)2CH2CH3 (3) Write the contributing resonance structures for each of the following. (a) (b)(c) (d) H CCHClHvinyl chloride (e)C OHOH3Cacetic acid (f) H N N N+_hydrazoic acid (4) Using the Valence Shell Electron Pair Repulsion Model predict the shape of the following molecules. (Hint: Draw the Lewis structure first before predicting the shape.) (a) SiH4 (silane) (b) CH3+ (methyl cation)(c) CH2=C=CH2 (allene) (d) H2C=O (formaldehyde) (5) Designate (1) the approximate hybridization for the atoms indicated by the straight arrows and (2) the approximate bond angles indicated by the curved arrows. (Hydrogen atoms attached to carbon atoms are not specifically shown. This is a short-hand symbolism often used in organic chemistry.)(6) Indicate True (T) or False (F) for each of the following statements. (a) Constitutional isomers are different compounds that have the same molecular formula but differ in their connectivity. (b) A covalent bond is a bond that results when atoms share electrons. (c) Potassium, with a nuclear charge of +19, is more electronegative than nitrogen, with a nuclear charge of +7. (d) Lewis structures show the connections between atoms in a molecule or ion using only valence electrons. (e) The formal charge on nitrogen of nitrite anion (NO2-) is -1.(f) Resonance structures represent the electronic configurations of molecules in equilibrium with one another. (g) In writing resonance structure both electrons and nuclei are permitted to be moved. (h) An atomic orbital is a region of space where the probability of finding an electron is large. (i) When atomic orbitals combine to form molecular orbitals, the number of molecular orbitals that results always equals the number of atomic orbitals that combine. (j) For a given molecule, an anti-bonding molecular orbital is higher energy than a bonding molecular orbital. (k) The rotational energy barrier associated with a carbon-carbon double bond is usually very large. (l) A carbon-carbon triple bond is shorter than a carbon-carbon single bond. (m) The shape of the borane molecule (BH3) is pyramidal. (n) For the ammonia molecule, the non-bonding molecular orbital is higher energy than the bonding molecular orbitals.(7) There are seven (7) constitutional isomers with the molecular formula C4H10O. Write a dash formula, a condensed formula and a bond-line formula for each of
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