1. What is the total number of valence electrons in the Lewis structure of SF2?   (2) Draw a Lewis structure for SF2.

Although I3- is a known ion, F3- is not. (a) Draw the Lewis structure for I3- (it is linear, not a triangle). (b) One of your classmates says that F3 - does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says F3- does not exist because it would violate the octet rule.Is this classmate possibly correct? (d) Yet another classmatesays F3- does not exist because F is too small to make bonds tomore than one atom. Is this classmate possibly correct?

= Deciding whether a Lewis structure satisfies the octet rule Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure :5: I :Z: H- :0: | U: -C-C-H Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* 0 Yes. No, it has the wrong number of valence electrons. The correct number is: 0 No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many 1/5

Using the bond energy data from your text (or the internet), determine (show calculations for) the approximate enthalpy change , ∆H, for each of the following reactions: (a) Cl2 (g) + 3F2 (g) ⟶ 2ClF3 (g) (b) H2C=CH2 (g) + H2 (g) ⟶ H3CCH3 (g)

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 answer c, d and e

What are the best steps to follow when drawing a lewis structure? I'm getting conflicting steps when determining the central atom.Do you determine it based on electronegativity or if it's the element there's only one of?

Write the Lewis symbols for boron and sulfur.

1. Refer to the following Bond energy table and determine if more energy is released per gram of fuel by burning natural gas (CH4) or butane (C4H10). Then, draw the Lewis Structure of all molecules. CH4(g) + 2O2(g) à CO2(g) + 2H2O(g)             2C4 H10 + 13O2 à 8CO2(g) + 10H2O(g)

Consider lisinopril, a drug used primarily in the treatment of high blood pressure, heart failure, and after heart attacks. (a)  Complete the Lewis structure of lisinopril, showing all valence electrons. (b)  Use the valence-shell electron-pair repulsion (VSEPR) model (Section 3.10) to predict all bond angles in lisinopril. (c) Which is the most polar bond in lisinopril?  (d) Is lisinopril polar or nonpolar? (e) Is lisinopril expected to possess resonance (Section 3.9)? Explain why or why not. (f) Name the various functional groups in lisinopril.  (g) What is the molecular formula of lisinopril? (h) What intermolecular forces are expected to exist between molecules of lisinopril in close proximity to one another (Section 5.7)?

carbon tetrachloride was formerly used in fire extinguishers for electrical fires.it is no longer used for this purpose because of the formation of the toxic gas phosgene,CL2CO.wRITE THE LEWIS STRUCTURES for the methane and ethane molecules.