Draw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. a) bromine dioxide (BrO2) (Assume the central atom does not contain an expanded octet.) There arevalence electrons surrounding the central atom. b) beryllium fluoride (BeF2) There arevalence electrons surrounding the central atom. c) phosphorus pentabromide (PBr₂) There arevalence electrons surrounding the central atom.

ut of ut of d out of They all have 1 lone pair(s) of electrons. How many bonding electrons does a sulphur atom have? Select one: O 0 O 1 O 2 O 3 Which of the following is correct electron dot diagram, for methanol? Select one: F1 CICI F2 F3 F4 F5

Decide whether the Lewis structure proposed for each molecule is reasonable or not. molecule proposed Lewis structure BeH₂ :O || :0 || :F: :F: H- Be H Is this a reasonable structure? If not, why not? Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: 0 O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary.…

Consider the theoretical molecule KrCl3‾. (a) Draw a valid Lewis structure for KrCl3‾. Show all lone pairs and use lines for bonds. Label all non-zeroformal charges on individual atoms and show the overall charge, if it exists, using square brackets.(b) What would you expect to be the molecular geometry for this ion? Fully explain your thought process,including all details about how successive lone pairs should be positioned within this electron geometry.(c) Draw this ion in 3-D, using hashed and wedged bonds as appropriate. Do not worry about labeling the overall or formal charge.

Complete the following statements about the molecule NBr3.  Please note that ALL atoms in this molecule obey the octet rule. The molecule NBr3 has  BLANK  total valence electrons. The molecule NBr3 should be drawn with N in the middle, and the Br atoms on three sides of the N atom.   After drawing the Lewis structure for NBr3 using the above information, it is evident that the three-dimensional shape (or geometry) of the molecule is   BLANK  , with a bond angle of   BLANK degrees.

Question: Each of the following may seem, at first glance, to be plausible electron-dot formulas for the molecule N₂F2. Most, however, are incorrect for some reason. What concepts or rules apply to each, either to cast it aside or to keep it as the correct formula? c: F ::N:N: F:

When drawing the Lewis structure of the HCC13 molecule, the structure should represent a total of 26 valence electrons. What is the best description of the complete Lewis structure of the molecule? Select one: AH atom should be in the center with single bonds to each Cl atom and a double bond to the C atom. A Cl atom should be in the center with a single bond to the C atom and a single bond to the H atom. AC atom should be in the center with a double bond to the H atom and double bonds to each Cl atom. AC atom should be in the center with single bonds to each Cl atom and a single bond to the H atom.

A student has drawn the Lewis structure below to represent the molecule NF3. Evaluate the structure as drawn compared to the chemical formula and select all of the following statements that are true. :F: :F: .. F: The structure has an octet rule violation with fewer than 8 electrons on one atom. The structure has too many electrons for the chemical formula. The structure is a good match to the chemical formula. The structure has an octet rule violation with more than 8 electrons on one atom. The structure has too few electrons for the chemical formula.

Answer the questions in the table below about the shape of the bromine trifluoride (BrF3) molecule. How many electron groups are around the central bromine atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central bromine atom? (You may need to use the scrollbar to see all the choices.) |(choose one) (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedral

Answer the questions in the table below about the shape of the phosphorus hexachlorate (PCI) anion. How many electron groups are around the central phosphorus atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central phosphorus atom? (You may need to use the scrollbar to see all the choices.) 0 ✓ (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedral