Which elements could NOT be A in the Lewis structure below if X is an element with six valence electrons? Select all that apply. X : A If you can't see the image, please click here. Kr Ar Хе O N В As
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- Draw Lewis diagrams for the two resonance forms of thenitrite ion, NO2-. In what range do you expect the nitrogen–oxygen bond length to fall? (Hint: Use Table 3.6.)1a) Create a drawing of the lewis structure of the ion ?3 2+, show your work (show all your work, total electron count, etc). b) How many total nodes are present in a 4d orbital? How many are radial and how many are angular?Draw the Lewis structures for all seven diatomic elements (H2, N2, O2,F2, Cl2,Br2, I2) . Even though Br and I are not in the first 3 periods it is useful to consider them here.
- Which of the following Lewis Dot Structures is definitely incorrect? Group of answer choices C A B D EI need help ASAP Website for first simulation: https://www.learner.org/wp-content/interactive/periodic/bondin The second/last simulation: Open the following website: https://javalab.org/en/ion_model_en/ As seen in the table, compounds containing an integer ratio of elements depend on how many cations combine with how many anions to form a stable compound. For example, in table 1, to form a NaCl compound, first Na ionizes from the Na+ cation which is having +1 positive charge, which will lose 1 electron, it is having +1 charge, this electron then goes to Cl and it will change to Cl- anion by gaining the electron, so here 1:1 ratio charge which means 1 Na+ combines with 1 Cl-1 to form NaCl. so here integer ratio is 1:1 for this sodium chloride compound. As listed in table 2, Mg(OH)2, the integer ratio is 1:2 which means, Mg is a neutral atom that loses 2 electrons and forms an Mg+2 cation, which combines with OH which gains 1 electron to form OH- anion, So here Mg2+ can combine with 2…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 formal charge of oxygen in HO− is _____. The number of valence electron of O in HO− is _____. The number of nonbonding electrons of O in HO− is _____. Thenumber of bonding electrons of O in HO− is _____. What are the answers for the Blanks A, B, C, D? Write the answers in a numerical form, not with letters, without any space.Consider the following ion: BrO3−. a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3−? What is its molecular shape? e) Does BrO3− have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer. g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. h) What is the molecular formula for Compound C? What is the empirical formula for Compound C? Please andwer f, g and h the image is for g and hConsider the following ion: BrO3−. a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3−? What is its molecular shape? e) Does BrO3− have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer. g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. h) What is the molecular formula for Compound C? What is the empirical formula for Compound C? please answer c, d and e
- Consider the following ion: BrO3−. a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3−? What is its molecular shape? e) Does BrO3− have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer. g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. (IMAGE WITH POSSIBILITIES) h) What is the molecular formula for Compound C? What is the empirical formula for Compound C?Consider the following ion: BrO3−. a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3−? What is its molecular shape? e) Does BrO3− have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer. h) What is the molecular formula for Compound C? What is the empirical formula for Compound C?Consider the following ion: BrO3 − . a) Show the full electron configuration for Br. b) Draw the most correct Lewis structure for BrO3 − and briefly explain why your Lewis structure is correct. c) If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why. d) What is the electronic geometry of BrO3 − ? What is its molecular shape? e) Does BrO3 − have a dipole moment? Briefly justify your answer. f) On average, would you expect IO3 − to have longer or shorter bonds than BrO3 − ? Briefly explain your answer. g) Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. h) What is the molecular formula for Compound C? What is the empirical formula for Compound C?