Concept explainers
Interpretation: The Lewis structures for HI, CH3CH2CH3, CH3OH, HSSH, SiO2, O2 and CS2 should be drawn.
Concept introduction: Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom.
Lewis dot structure is also known as Lewis dot formula or electron dot structure. The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.
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Organic Chemistry: Structure and Function
- The bond lengths in Cl2, Br2, and I2 are 200, 228, and 266 pm, respectively. Knowing that the silicon radius is 111 pm, estimate the bond distances in Si-Cl, Si—Br, and Si—I. (Express your answer as an integer.) Si-Cl: Si-Br: Si-I: pm pm pmarrow_forwardLewis structures of group T compounds Draw Lewis structures for each of the following molecule or ion: Methane, CH4 Ammonia, NH3 Water, H2O Borane, BH3 Sulfur dioxide, SO2 Carbon dioxide, CO2 Nitrogen, N2 Hydrogen cyanide, HCN Hydronium ion, H3O+ Iodine, I2 Ammonium, NH4+ Formaldehyde, CH2O Ozone, O3 Carbonate ion, CO32− Include the number of valence electrons and the number of pairs of electrons for each.arrow_forwardUse bond energies (see table) to predict AH for the formation of HCI gas. H2(g) + Cl2(9) → 2 HCl(g) KJarrow_forward
- What possible error(s) exist in the Lewis structure (assume we are trying to represent the best possible Lewis structure for the NO₂S ion knowing N is the central atom in this polyatomic ion)? [:ö==S: N= CO :O: The best structure would have double bond and two lone pairs on each oxygen atom and a single bond with three lone pairs on the sulfur. There are no errors. This is the best possible structure. The Lewis structure above does not minimize formal charges, thus is the not the best possible structure. The nitrogen atom has an expanded octet, and this structure is impossible. The Lewis structure contains the wrong number of electrons, thus this structure is impossible.arrow_forwardThis Lewis Structure is incorrect because [Ca]+ [:O:]- The metal should be negative and the nonmetal should be positive The metal should have a +2 charge and the nonmetal should have a -2 charge The metal should have 2 electrons O around it and the nonmetal should have 6 electrons around it There is nothing wrong with the Lewis Structure 2.arrow_forwardDraw the Lewis structure for the xenon tetrafluoride (XeF4) molecule. C C a X O: G 1 = ?arrow_forward
- Hydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.arrow_forwardCalculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forwardCovalent bonds: H―HC―HO―HO═O C≡O Bond energy (kJ/mol):4364154654981080Calculate the enthalpy change (H, in kJ/mol) for the following reaction and indicate whether the reaction is exothermic or endothermic.(*BE for C═Oin CO2)(a) CH4(g)+ H2O(g)CO(g)+ 3H2(g);arrow_forward
- Use the Born-Haber cycle to calculate the lattice energy of KF. [The heat of sublimation of K is 91.6 kJ·mol−1 and ΔfH(KF) = −567.3 kJ·mol−1. Bond enthalpy for F2 is 158.8 kJ·mol−1. Other data may be found in the Ionization Energies Table and the Electron Affinities Table.]arrow_forwardChloral, Cl3C—CH=O, reacts with water to form the sedative and hypnotic agent chloral hydrate, Cl3C—CH(OH)2. Draw Lewis structures for these substances, and describe the change in molecular shape, if any, that occurs around each of the carbon atoms during the reaction.arrow_forwardDraw the Lewis structure for the iodide pentafluoride (IFS) molecule. Ċ C X O: 3 1 = ?arrow_forward
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