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What is the Lewis structure for the compound that forms between K and S?
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Chapter 10 Solutions
INTRODUCTORY CHEMISTRY-W/SEL.SOLN.MAN.
- What 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_forwardBond 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_forwardPredict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a. POCl3, SO42, XeO4, PO43, ClO4 b. NF3, SO32, PO33, ClO3 c.ClO2, SCl2, PCl2 d. Considering your answers to parts a, b, and c. what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons? (O3), sulfur dioxide, and sulfur trioxide.arrow_forward
- The most common exceptions to the octet rule are compounds or ions with central atoms having more than eight electrons around them. PF5, SF4, CIF3, and Br3 are examples of this type of exception. Draw the Lewis structure for these compounds or ions. Which elements, when they have to, can have more than eight electrons around them? How is this rationalized?arrow_forwardWrite the Lewis structure for each molecule.a. CH2O b. C2Cl4c. CH3NH2 d. CFCl3 (C central)arrow_forwardWrite the Lewis structure for each molecule.a. CH2O b. C2Cl4arrow_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_forward18.What are the formal charges present in in the ion CH3NH3+? Assume all atoms other an hydrogen have an octet and that there are two central atoms. A. N is +1 and C is 0 B. N is +1 and C is -1 C. N is +2 and C is -1 D. N is 0 and C is 0 E. N is 0 and C is +1arrow_forwardWrite an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds.a. BI3 b. K2Sc. HCFO d. PBr3arrow_forward
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