Concept explainers
(a)
Interpretation: All reasonable resonance structures for the given species are to be drawn.
Concept introduction: Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures.
(b)
Interpretation: All reasonable resonance structures for the given species are to be drawn.
Concept introduction: Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures.
(c)
Interpretation: All reasonable resonance structures for the given species are to be drawn.
Concept introduction: Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures.
(d)
Interpretation: All reasonable resonance structures for the given species are to be drawn.
Concept introduction: Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures.
(e)
Interpretation: All reasonable resonance structures for the given species are to be drawn.
Concept introduction: Resonance structure is a blend of two or more Lewis structures. Resonance structures are represented by a double headed arrow between the structures.
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PKG ORGANIC CHEMISTRY
- Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forwardWhat is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?arrow_forwardWrite the Lewis structure for each molecule.a. SF2 b. SiH4c. HCOOH (both O bonded to C) d. CH3SH (C and S central)arrow_forward
- 116) Write Lewis structures and predict whether each of the following is polar or nonpolar. a. HOCN (exists as HO−CN) c. XeF2e. SeF6 b. COSd. CF2Cl2f. H2CO (C is the central atom)arrow_forwardWrite the Lewis structure for each ion. Include resonance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge.a. PO43- b. CN- c. SO3 2- d. ClO2 -arrow_forwardWrite an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds.a. Al2O3 b. ClF5c. MgI2 d. XeO4arrow_forward
- Write Lewis structures that obey the octet rule for each of the following. a. HCN b. PH3 c. CHCl3 d. NH4+ e. H2CO f. SeF2 g. CO2 h. O2 i. HBr Except for HCN and H2CO, the first atom listed is the central atom. For HCN and H2CO , carbon is the central atom.arrow_forwardWrite Lewis structures for each molecule or ion. Use expanded octets as necessary.a. ClF5 b. AsF6- c. Cl3PO d. IF5arrow_forwardWhich of the molecules and polyatomic ions cannot be adequately described using a single Lewis structure? A.O3 B.HCN C.CO2−3 D.OF2 E.CH2Cl2 F.NH+4arrow_forward
- Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds.a. BI3 b. K2Sc. HCFO d. PBr3arrow_forward2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule before identifying the shape of the molecule?arrow_forward2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule before identifying the shape of the molecule? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.arrow_forward
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