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- Write Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Amide ion, NH2 (b) Bicarbonate ion, HCO3 (c) Carbonate ion, CO32 (d) Nitrate ion, NO3 (e) Formate ion, HCOO (f) Acetate ion, CH3COOIndicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment. (a) HCN (b) I2 (c) NOIndicate whether each of the following hypothetical triatomic molecules is polar or nonpolar. Assume that A, X, and Y have different electronegativities. a. a linear XAX molecule b. a linear XXA molecule c. an angular AXY molecule d. an angular XAY molecule
- In which of the following pairs of diatomic species do both members of the pair have bonds of the same multiplicity (single, double, triple)? a. HCl and HI b. S2 and Cl2 c. CO and NO+ d. OH and HSIn which of the following pairs of diatomic species do both members of the pair have bonds of the same multiplicity (single, double, triple)? a. N2 and F2 b. CO and CN c. HBr and ClF d. O2 and O22The bond between which of the following pairs of atoms would be the least polar (lowest percent ionic character)?O - CC - HC - ClC - CN - C
- Which of the following would you expect to be a polar molecule? O CH4 O CO2 O CCL, O CHCI, O N2Based on the atom connectivity shown bellow,evaluate the four resonance structure for the thiosulfate ion S2O3 ^2-. Use curved arrows to indicate how you get from one resonance structure to another. Assign formal changes to all atoms and determine which of these resonance structure is the most stable based on a formal charge analysis Explain your answer thoroughly. Look at the picture.Which of the following molecules contains at least one atom that has less than a complete octet (excluding hydrogen)? You can consider structures that are both radicals or non-radicals. select one or more: NO O2N-NO2 SF6 BH3 HCl H2O NH3
- Describe the type of bond represented by the dash for each of the following compounds using the definitions in Q1. Consider only the atoms to which the dash is directly connected. H–H H–CH3 H–NH2 Na–ONa Na–Br K–OH H–OH H–Br F–CH3 Q4 Draw the electron-dot formulas for the following compounds or ions and calculate the formal charges for every atom. HF H2S F- Br+ N2 HCN NC-What are the formal charges present in in the ion CH3NH3*? Assume all atoms other an hydrogen hau an octet and that there are two central atoms. O N is 0 and C is +1 O N is +1 and C is -1 O N is +1 and C is 0 O N is 0 and C is 0 O N is +2 and C is -1Draw Lewis structures of the four molecules and/or ions with the formulas given below and figure out which two of these are isoelectronic with each another. Species which are isoelectronic have the same number of atoms, the same total number of electrons, the same number of valence electrons, and the same valence electron structure (single and multiple bonds and lone pairs in same places), but need not have the same distribution of formal charges on atoms.CN- and Cl2 and F2 and N2 a) CN- and N2 are isoelectronic.b) F2 and Cl2 are isoelectronic.c) N2 and Cl2 are isoelectronic.d) CN- and Cl2 are isoelectronic.e) N2 and F2 are isoelectronic.
