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- a) Draw the Lewis Structure of Barium Iodide (BaI2) b) Identify the type of bond (show EN Difference Computation) c) Orientation of Electron Pairs; and d) Molecular GeometryIonizing an H2 molecule to H2+ changes the strength of the bond. Based on thedescription of covalent bonding given previously, do you expect the H¬H bond inH2+ to be weaker or stronger than the H ¬ H bond in H2?For C ~ F, you need draw the proper Lewis structure first, then draw the resonances
- Question 2a. Draw all possible resonance structures of NO3 (nitrate ion) without violating the octet rule(Show nonbonding electrons as dots (:) and bonding electrons as lines (-)). Show all non-zercformal charges on atoms for all structures.(5)b. For which one of the following does the best simple description involve more than one Lewisstructure (i.e., two or more resonance structures)?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?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]
- What is the formal charge on C for the following Lewis structure? CO2 Group of answer choices 0 -2 +2 +41. Which of the following Lewis Structures are correct? Select all that apply. 2. Which of these compounds are polar molecules? Select all that apply.Atom A has 4 valence electrons. Atom Z has 6 valence electrons. For the AZ3-2 ion, answer the following questions about its Lewis dot structure (drawn according to Chm 130 guidelines). a. How many valence electrons are in the structure? b. How many single bonds are in the structure? c. How many double bonds are in the structure? d. How many triple bonds are in the structure? e. How many lone pairs are on the central atom in the structure? f. What is the shape of the structure? g. What are the bond angles of this ion?
- N2 or N3- (1) Which has longer bond? and (2) Which has stronger bond?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?TRUE OR FALSEa. It requires more energy to break N-N bond (N2O4) than to break the N-N bond in N2 b. The ∆Srxn for C6H14(l) is +ve, while the ∆Srxn for C4H10(g) is -ve.
