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- The Lewis representation above depicts a reaction between a halogen (blue) and a main-group element from group (7A + (red). In this representation, each Y atom needs 1 electron(s) to complete its octet, and gains these electrons by forming bond(s) with atoms of X . There are unshared electron pair(s) and bonding electron pair(s) in the product molecule. The bonds in the product are Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next Email Instructor Save and Exit Cengage Learning | Cengage Technical Support18 - for Cl, Cl + and Cl- ions;Cl- is the largest number of electronsII. Stripping electrons from the Cl + ion is most difficultIII. Neutral Cl atom and Cl- ions have equal radiiWhich of his judgments are correct? A) Only IIIB) I, IIC) I, IIID) I onlyE) I, II, IIIConsider 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?Incomplete Lewis structures for the nitrous acid molecule,HNO2, and the nitrite ion, NO2-, are shown here. (a) Completeeach Lewis structure by adding electron pairs as needed.(b) Is the formal charge on N the same or different in thesetwo species? (c) Would either HNO2 or NO2- be expected toexhibit resonance? (d) Would you expect the N=O bond inHNO2 to be longer, shorter, or the same length as the N¬Obonds in NO2?Determine the second ionization energy of calcium (in kJ mol-1) from the given data (all in kJ mol-1): AH°[CaCl,(s)] = -796 AH¡[Ca(g)] = 178 AH°[CI(g)] = 122 First ionization energy of Ca(g) = 590 Electron affinity of Cl(g) = -349 Lattice enthalpy of CaCl,(s) = -2260 А 1150 В 1235 C 1093 D 1210
- Incomplete Lewis structures for the nitrous acid molecule,HNO2, and the nitrite ion, NO2-, are shown here. (a) Completeeach Lewis structure by adding electron pairs as needed.(b) Is the formal charge on N the same or different in thesetwo species? (c) Would either HNO2 or NO2- be expected toexhibit resonance? (d) Would you expect the N“O bond inHNO2 to be longer, shorter, or the same length as the N¬Obonds in NO2-? [Sections 8.5 and 8.6]Construct a Born–Haber cycle for the formation of the hypotheticalcompound NaCl2, where the sodium ion has a 2+charge (the second ionization energy for sodium is given inTable 7.2). (a) How large would the lattice energy need to befor the formation of NaCl2 to be exothermic? (b) If we wereto estimate the lattice energy of NaCl2 to be roughly equalto that of MgCl2 (2326 kJ/mol from Table 8.1), what valuewould you obtain for the standard enthalpy of formation,ΔHf°, of NaCl2?Q.3 a) Write the chemical name and chemical formula of a compound formed between X (atomic number of X=56) and nitrate ion. (1 mark) b) Name and explain the type of chemical reaction that occurs in between two ionic compounds with the help of examples. (2 marks) c) Explain the bond formation with Lewis structure in a gas molecule that belongs to group 6A and exists as a diatomic molecule. (Mention the type of chemical bond) (2 marks)
- Which of the following bonds are polar? Which is the more electronegative atom in cach polar bond? (a) B-F (b) Cl-CI (c) Se-O (d) H–I Arrange the bonds in cach of the following sets in order of inereasing polarity: (a) C-F, O–F, Be-F; (b) 0-CI, S-Br, C-P; (c) C-S, B–F, N-0.Write Lewis structures for the following:(a) O2(b) H2CO(c) AsF3(d) ClNO(e) SiCl4(f) H3O+(g) NH4+(h) BF4−(i) HCCH(j) ClCN(k) C22+Using the values given in the table below, calculate lattice energy of CaF,. Express your final answer to 2 decimal places only. Ca(s) enthalpy of atomization = +179 kJ/mol. F,(g) bond dissociation enthalpy = +158 kJ/mol. Ca(g)1 st ionisation energy= +590 kJ/mol. Ca+ (g) 2 ionisation energy = +1,150 kJ/mol. F(g) first electron affinity =-348 kJ/mol. CaF,(s) enthalpy of formation =-1,220 kJ/mol. %3D