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Q: Write a Lewis structure for each of the following simple molecules. Show all bonding valence…
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- Define the term lattice energy. Why, energetically, do ionic compounds form? Fig. 3-8 illustrates the energy changes involved in the formation of MgO(s) and NaF(s). Why is the lattice energy of MgO(s) so different from that of NaF(s)? The magnesium oxide is composed of Mg2+ and O2 ions. Energetically, why does Mg2+O2 form and not Mg+O? Why doesnt Mg3+O3 form?Testosterone is an anabolic steroid. The structure of testosterone is shown below. What is the shape of the bonds at (i) ? Hint: atom (iv) has been completed for you as an example. (iv) bond angle: 109.5°, geometry of the electron pairs: tetrahedral, shape of the bonds: tetrahedral iii ·····|||I H **…||||I H ii ivUse principles of atomic structure to answer each of the following: (1] (a) The radius of the Ca atom is 197 pm; the radius of the Ca2* ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is –3460 kJ/mol; the lattice energy of K20 is –2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First lonization Energy (kJ/mol) Second lonization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.
- Draw the Lewis structures and determine which of these molecules is least likely to exist. (A) H3S+ (B) H3O+ (С) НзО- (D) H3S- (E) OH- Draw all 5 structures with 1 central atom. All of the other atoms are attached to the central atom.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.The Lewis structure for the chlorate ion is :0: Calculate the formal charge on the chlorine (Cl ) atom. Express your answer as an integer. • View Available Hint(s) formal charge on Cl = Submit Part B Calculate the formal charge on each of the oxygen (O) atoms labeled a, b, and c in the following Lewis structure. :0: Express your answers as integers separated by commas. • View Available Hint(s) formal charge on Oa , Ob , Oc = Submit ormal charges to predict the most stable structure he interactive activity shows how to calculate the formal charge of atoms in a structure. These formal charges can be used to predict the resonance structure that contributes most to the stability of a molecule or ion. The struc enerally the most stable. Part C What are the formal charges on the sulfur (S), carbon (C ), and nitrogen (N ) atoms, respectively, in the resonance structure that contributes most to the stability of the thiocyanate ion, SCN¯ ? The possible resonance structures for the thiocyanate…
- Write Lewis structures for the following molecules or ions:(a) SbH3(b) XeF2(c) Se8 (a cyclic molecule with a ring of eight Se atoms)Write Lewis structures for the following: (c) C2F6 (contains a C¬C bond), (d) AsO3 3 -, (e) H2SO3 (H is bonded to O), (f) NH2Cl.. Arrange the bonds in each of the following sets in order of increasing polarity: (a) C¬F, O¬F, Be¬F; (b) O¬Cl, S¬Br, C¬P; (c) C¬S, B¬F, N¬O. What is the Lewis symbol for each of the following atoms or ions? (a) K, (b) As, (c) Sn2 + , (d) N3 Write electron configurations for the following ions and determine which have noble-gas configurations: (a) Cd2+, (b) P3-, (c) Zr4+Consider the Lewis structure for the polyatomic oxyanionshown here, where X is an element from the third period(Na - Ar). By changing the overall charge, n, from 1- to2- to 3- we get three different polyatomic ions. For each ofthese ions (a) identify the central atom, X; (b) determine theformal charge of the central atom, X; (c) draw a Lewis structurethat makes the formal charge on the central atom equalto zero.
- Draw the correc (best) Lewis structure (LS) for the ionic compound K2SeO3 (on looose leaf paper--NOT TO BE SUBMITTED) and then answer the following questions.(NOTE: Use the cardinal numbers 0, 1, 2, 3, and so on for any quantity required)a) What charge does the K ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) b) What charge does the SeO3 ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) c) How many lines, if any, attach each K ion to the SeO3 ion? d) How many valence electrons does the SeO3 ion (alone) have? e) How many single bonds does the LS of the SeO3 ion have? f) What is the number of lone electron pairs in the LS of the SeO3 ion?Draw Lewis electron dot diagrams for the following species: (a) AsH3; (b Draw Lewis electron dot diagrams for the following species: (a) AsH3; (b) HOCl; (c) KrF+; (d) PO2 Cl 2 - (centralP atom).Write Lewis dot symbols for the following atoms and ions: (a) I (b) I-(c) S(d) S2-(e) P (f) P3-(g) Na (h) Na+(i) Mg (j) Mg2+