General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
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Chapter 4, Problem 4.28CP
Interpretation Introduction
Interpretation:
Formula of acetaminophen and the position of multiple bonds has to be given.
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The diagram above shows two resonance structures for a molecule of C6H6. The phenomenon shown in the
diagram best supports which of the following claims about the bonding in C6H6 ?
(A) In the C6H6 molecule, all the bonds between the carbon atoms have the same length.
(B) Because of variable bonding between its carbon atoms, C6H6 is a good conductor of electricity.
(C) The bonds between carbon atoms in C6H6 are unstable, and the compound decomposes quickly.
The C6H6 molecule contains three single bonds between carbon atoms and three double bonds between
(D)
carbon atoms.
IIU
A resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity?
(a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar.
(b) The farther two atoms are apart in a bond, the larger the dipole moment will be.
3. The following are some molecules:H2, HF, CO2, H2O, Cl2, NH3, CH4, CHCl3
(a) Which of the above molecules do/does not contain polar bond? Explain your answer.
(b) Which covalent bond has the highest bond polarity among the eight molecules?
(c) (i) Which of the above molecules are non-polar molecules?
(ii) Explain why these molecules are non-polar. 4. (d) Draw a diagram to illustrate the formation of hydrogen bonds in H2O.
Chapter 4 Solutions
General Chemistry: Atoms First
Ch. 4.2 - Prob. 4.1PCh. 4.2 - Prob. 4.2PCh. 4.2 - Prob. 4.3CPCh. 4.4 - Use the electronegativity values in Figure 4.4 to...Ch. 4.4 - Order the following compounds according to the...Ch. 4.4 - An electrostatic potential map of water is shown...Ch. 4.5 - Prob. 4.7PCh. 4.5 - Write formulas for compounds with the following...Ch. 4.5 - Prob. 4.9CPCh. 4.6 - Draw electron-dot structures for the following...
Ch. 4.6 - Draw an electron-dot structure for the hydronium...Ch. 4.7 - Draw electron-dot structures for the following...Ch. 4.7 - There are two molecules with the formula C2H6O....Ch. 4.7 - The following structure is a representation of...Ch. 4.8 - Carbon monoxide, CO, is a deadly gas produced by...Ch. 4.8 - Draw an electron-dot structure for each of the...Ch. 4.8 - Prob. 4.17PCh. 4.9 - Prob. 4.18PCh. 4.9 - Draw as many resonance structures as possible for...Ch. 4.9 - The following structure shows the connections...Ch. 4.10 - Calculate the formal charge on each atom in the...Ch. 4.10 - Calculate the formal charge on each atom in the...Ch. 4.10 - What is a radical, and why are they so reactive?Ch. 4.10 - Prob. 4.24PCh. 4.10 - Draw an electron-dot structure for the ethyl...Ch. 4 - Two electrostatic potential maps are shown, one of...Ch. 4 - Prob. 4.27CPCh. 4 - Prob. 4.28CPCh. 4 - Prob. 4.29CPCh. 4 - Sinapaldehyde, a compound present in the toasted...Ch. 4 - Vitamin C (ascorbic acid) has the following...Ch. 4 - What general trends in electronegativity occur in...Ch. 4 - Prob. 4.33SPCh. 4 - Prob. 4.34SPCh. 4 - Prob. 4.35SPCh. 4 - Prob. 4.36SPCh. 4 - Prob. 4.37SPCh. 4 - Prob. 4.38SPCh. 4 - Show the direction of polarity for each of the...Ch. 4 - Prob. 4.40SPCh. 4 - Prob. 4.41SPCh. 4 - Prob. 4.42SPCh. 4 - Prob. 4.43SPCh. 4 - Prob. 4.44SPCh. 4 - Prob. 4.45SPCh. 4 - Prob. 4.46SPCh. 4 - Prob. 4.47SPCh. 4 - Prob. 4.48SPCh. 4 - Prob. 4.49SPCh. 4 - Prob. 4.50SPCh. 4 - Which of the following substances contains an atom...Ch. 4 - Draw electron-dot structures for the following...Ch. 4 - Prob. 4.53SPCh. 4 - Oxalic acid, H2C2O4, is a mildly poisonous...Ch. 4 - Draw an electron-dot structure for carbon...Ch. 4 - Prob. 4.56SPCh. 4 - Prob. 4.57SPCh. 4 - Prob. 4.58SPCh. 4 - Prob. 4.59SPCh. 4 - Methylphenidate (C14H19NO2), marketed as Ritalin,...Ch. 4 - Pregabalin (C8H17NO2), marketed as Lyrica, is an...Ch. 4 - Draw as many resonance structures as you can that...Ch. 4 - Prob. 4.63SPCh. 4 - Which of the following pairs of structures...Ch. 4 - Which of the following pairs of structures...Ch. 4 - Draw an electron-dot structure for carbon...Ch. 4 - Prob. 4.67SPCh. 4 - Prob. 4.68SPCh. 4 - Prob. 4.69SPCh. 4 - Prob. 4.70SPCh. 4 - Prob. 4.71SPCh. 4 - Prob. 4.72SPCh. 4 - Prob. 4.73SPCh. 4 - Prob. 4.74CHPCh. 4 - Thiofulminic acid, , is a highly reactive...Ch. 4 - Draw two resonance structures for methyl...Ch. 4 - Prob. 4.78CHPCh. 4 - Prob. 4.79CHPCh. 4 - Prob. 4.80CHPCh. 4 - Prob. 4.81CHPCh. 4 - Prob. 4.82CHPCh. 4 - Prob. 4.83CHPCh. 4 - Prob. 4.84CHPCh. 4 - Prob. 4.85CHPCh. 4 - Sulfur reacts with chlorine to give a product that...Ch. 4 - Sulfur reacts with ammonia to give a product A...Ch. 4 - Prob. 4.88MPCh. 4 - Prob. 4.89MP
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- Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?arrow_forwardhat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.arrow_forward3-89 Is it possible for a molecule to have no polar bonds and yet have a dipole? Explain.arrow_forward
- An ionic compound has the following composition (by mass): Mg, 10.9%; Cl, 31.8%; O, 57.3%. What are the formula and name of the compound? Write the Lewis formulas for the ions.arrow_forward3. The skeleton of chloromethane is __________________ The central carbon atom is bonded to each of the other atoms by a shared electron pair (represented by a straight line, ___) giving Now, each hydrogen has two electrons and the carbon atom has eight. However, chlorine must be provided with unshared electrons (represented by pairs of dots, ) to complete its octet, thusarrow_forwardFor each pair of bonds, indicate the more polar bond, and use an arrow to show the direction of polarity in each bond. (a) C O and C N (b) P Br and P Cl (c) B O and B S (d) B F and B Iarrow_forward
- Using the electronegativity values given in the references section, show for the indicated bonds which atom acquires the partial negative charge. (To answer this question you may consult the table of electronegativity values in the table below.) (a) H3C-CI 1A 2A Li Be 1.0 1.5 (b) H-CI Na Mg 0.9 1.2 3B 4B 5B 6B 7B K Ca Sc Ti 0.8 1.0 1.3 1.5 Rb Sr Y Zr 0.8 1.0 1.2 1.4 V 1.6 <1.0 1.0-1.4 Nb Mo 1.6 1.8 Cr Mn Fe Co 1.6 1.5 1.8 Cs Ba La Hf Ta W Re Os H 2.1 8B 1.5-1.9 2.0-2.4 8122=2 Tc Ru 1.9 2.2 2.2 2.2 Ir If none of them bears the negative charge, choose none. Ni 1.8 Rh Pd Ag Cd In Sn Sb Te 1.9 1.7 1.7 1.8 1.9 2.1 2.5-2.9 3.0-4.0 3A 4A 5A 6A 7A B C N O F 2.0 2.5 3.0 3.5 4.0 Al 1B 2B 1.5 Cu Zn 1.9 1.6 Predict which indicated bond in each set is the more polar one. Si P 1.8 2.1 S 2.5 Ga Ge As Se 1.6 1.8 2.0 2.4 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.2 2.2 2.2 2.4 1.9 1.8 1.8 1.9 2.0 2.2 CI 3.0 Br 2.8 I 2.5 Pt Au Hg Tl Pb Bi Po Atarrow_forwardIs the bond between each pair of atoms pure covalent, polar covalent, or ionic?(a) I and I (b) Cs and Br (c) P and Oarrow_forwardConsider the following compounds: CaCl 2 , CaI 2 , and MgCl 2 . Answer the following questions based on expected periodic trends: (a) Which is expected to have t he shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forward
- (a) Complete the following table:BESTLewis structureNH4+Draw Lewis structure:VSEPR Formula for central atom: _________________________SOF2Draw Lewis structure:VSEPR formula for central atom: __________________________XeF2Draw Lewis structure:VSEPR formula for central atom: ________________________H2SO3Draw Lewis structure:VSEPR formula for central atom: ________________________3(b) (i) In general, for what two kinds of substances do we draw Lewis structures?____________________________________________________________________________(ii) Complete the following Lewis structure and answer the questions below it.CHNHC OOC C NH HHHWhat is the empirical formula of this compound? __________________________________How many lone pairs of electrons that this compound have? __________________________How many multiple bonds does this compound have? _______________________________How many nonbonding electrons does this compound have? __________________________How many molecules are in 15.0 mg of…arrow_forwardIn the following pairs of binary compounds, determinewhich one is a molecular substance and which one is anionic substance. Use the appropriate naming convention(for ionic or molecular substances) to assign a name to eachcompound: (a) SiF4 and LaF3, (b) FeCl2 and ReCl6, (c) PbCl4and RbCl.arrow_forward7. Consider the following compounds: BaBr 2, MgCl 2, and SrCl 2. Answer the following questions based on expected periodic trends: (a) Which is expected to have the shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forward
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