QUESTION 20 Which is true regarding the H-F bond in the compound HE it is ionic it is polar covalent it is nonpolar covalent none of the above
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- Draw the lewis dot represenations of te following atoms: a: Ca b: Cl c: B d: O1. Write the chemical formula for a compound containing the following elements: calcium and oxygen; 1:1 A. O2Ca2 B. OCa2 C. OCa D. CaO2 E. Ca2O2 F. O2Ca G. Ca2O H. CaO 2. Calculate ∆En for the following bond and classify it according to type: MgO A. -2.3; ionic B. 2.3; ionic C. -2.3; covalent D. -2.3; polar covalent E. -2.3; nonpolar covalent F. 2.3; polar covalent G. 2.3; covalent H. 2.3; nonpolar covalent I do not undertand how to do this questiosn. Please help These are also the answer chices I have.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?
- The percent ionic character of a bond between elements A and B may be approximated by the expression %IN = 100[1 - e^(-1/4(XA - XB))], where XA and XB are the electronegavities for the respective elements. What is the the percent ionic character of the interatomic bonds for Fe2O3? What type of bonding would you expect in Fe2O3? Note: Use 1.8 for the electronegativity for Fe and 3.5 for the electronegativity for O.Likeseveralotherbonds,carbon-oxygenbondshavelengthsthatdependon bond order. Draw Lewis structures for the following species, and arrange them in order of increasing bond length. a) CO b) H2CO c) CH3OH d) CO32- e) HCO3-Hint for (e): which atom will the H be attached to? Note that HCO3- is formed +2- 2-when you add an H to CO3 . Looking at your structure for CO3 , where does it make the most sense to add the H+?Which of the following ions possess a noble gas electron configuration? Please select all that apply (a) K+ (b) H- (c) F- (d) He+ (e) O (f) Ca2+?
- Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule.a. BF3b. NH3c. BeCl2d. PCl5*e. OF2f. SF4*g. SF6*h. XeF2*i. SnCl4j. H3O+ Set up your own table to the following formatColumn CharacteristicsA Bonding electronsB Sigma-bondsC Nonbonding electron pairsD Hybrid orbitals havingnonbonding electron pairsE Hybrid orbitals used F 3-D structureG Polar (P) or nonpolar (NP) molecule or ion lewis structure A B C D E F GChoose the bond below that is most polar. Question 19 options: Si-Cl Si-S Si-F Si-P Si-Si Ge-GeR please help me with this. Provide explanations, images or procedures on how to complete them 1) Know what VSEPR stands for 2) Given the physical or chemical properties of a substance classify it as: metallic, ionic, polar or non-polar covalent or covalent network solid 3) Given the formula of a compound draw the VSEPR shape and give bond angles and shape name 4) Make generalizations from graphs and data relating to atomic or periodic trends (IE, EA, EN and AR) 5) Why is water so special? 6) Know the physical/chemical properties of each type of bonding 7) Determine if a bond is polar 8) Determine if a molecule is polar
- 1)Which type of bond would be expected in molecule of LiF? A)ionic b) polar covalent c)nonpolar covalent b) none of these 2)which of the following contains a metallic bond? A)NaCI b)SO2 c)Cu-Zn Alloy d) K20 3) which of the following contains an ionic bond? A)NACI b) SO2 C) Cu-Zn Alloy d)CO2The partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one? [Sections 8.3and 8.8]One scale for electronegativity is based on the concept thatthe electronegativity of any atom is proportional to theionization energy of the atom minus its electron affinity:electronegativity = k1I - EA2, where k is a proportionalityconstant. (a) How does this definition explain why the electronegativityof F is greater than that of Cl, even though Clhas the greater electron affinity? (b) Why are both ionizationenergy and electron affinity relevant to the notion ofelectronegativity? (c) By using data in Chapter 7, determinethe value of k that would lead to an electronegativity of 4.0for F under this definition. (d) Use your result from part (c)to determine the electronegativities of Cl and O using thisscale. (e) Another scale for electronegativity defines electronegativityas the average of an atom’s first ionization energyand its electron affinity. Using this scale, calculate the electronegativitiesfor the halogens, and scale them so that fluorinehas an electronegativity of 4.0. On this…