bond order for B2^- please draw the picture and explain what I am doing wrong. I am getting six bonding electrons even though the correct answer is 5.
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bond order for B2^-
please draw the picture and explain what I am doing wrong. I am getting six bonding electrons even though the correct answer is 5.
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- How do you know when to draw a solid wedge vs a dashed wedge when drawing 3D bond-line structures? I know that solid-wedge means the atom is pointing towards you and dashed wedge means it's in the back, but how do you know which atoms are in the front as opposed to the back? How can you tell what the configuration will look like in space just by looking at the lewis structure or name?For the formula CH,CF2, *draw the Lewis structure in your work* (which I will grade when you upload it). After drawing the complete Lewis structure, type in the shape, bond angle, etc. for each blank. What is the molecular shape or geometry for the carbon on the left (the C in CH2)? What is the molecular shape or geometry for the carbon on the right (the C in CF2)?| What is the bond angle for the carbon on the left (the C in CH)? Type in a plain number, but include a "<" sign in front of the number if applicable. What is the bond angle for the carbon on the right (the C in CF2)? Type in a plain number, but include a "<" sign in front of the number if applicable. What is the hybridization for the carbon on the left (the C in CH2)? Type this in without any superscript, for instance sp3 would be typed as "sp3". What is the hybridization for the carbon on the right (the C in CF2)? Type this in without any superscript, for instance sp3 would be typed as "sp3". Is the molecule overall polar…How many valence electrons does a neutral a. K atom have? b. C atom? N atom? O atom?
- A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.Give typed full explanation Look at figure 3-22 that shows the electron density that occurs abound the Si-O bond. This electron density map gives the "shape" of the O and Si atoms when they are bonded together. Think about the answer in Q9 and choose the best response below: (Select answer choice) a. This figure shows that the Si and O atoms, when they bond together, do not form spheres, which is due to the fact that the Si-O bond is strongly covalent and these shared electrons affect atomic shape. This change in shape limits the applicability of Pauling's Coordination principle since that principle is based on the geometry of perfect spheres. b. This figure shows that the Si and O atoms, when they bond together are close to perfect spheres, which is due to the fact that the Si-O bond is strongly covalent. This figure shows that Pauling's Coordination principle should apply very precisely to any substance that contains Si-O bonds c. This figure shows that the Si and O atoms, form in a…A model for SiH4 is shown in the chem3D window. SiH4 has tetrahedral geometry. ball & stick |+ labels Rotate the molecule until you have a feeling for its three-dimensional shape. How many atoms are bonded to the central atom? If you take any three of the outer atoms, what shape do they define? | Consider the bond angles at the central atom. Do they all have the approximately the same numerical value? What is the approximate numerical value of this angle? | degrees. Are all four positions about the central atom equivalent, or is one of them different from the other three. For practice, type in the name of the geometry of the molecule: Previous Next
- How do the C‒S bond lengths in CS32– compare ? Two are the same length, the other is longer. Two are the same length, the other is shorter. They are all different lengths. They are all same length. Not enough info to tell.How many σ-bonds are in the molecule? σ-bonds How many π-bonds are in the molecule? π-bonds For bond angles, respond with 60o, 90o, 109o, 120o, or 180o (do not include the degree sign in your response). What is the approximate H-C-C bond angle in the molecule? o What is the approximate C-O-H bond angle in the molecule? o What is the approximate C-N-H bond angle in the molecule? o What is the approximate O=C-O bond angle in the molecule? oHi, I need help with filling these out, along with the Lewis Structure, Wedge Sketch, hybridization, and polar or non- polar. Pretty much all the blanks and check the work that I entered. Thank you Molecule Name Total #valence electrons Best Lewis structure Total # groups on central atom Electron geometry #bonded groups #lone pairs Molecular geometry Wedge/dash sketch Hybridization Polar or non-polar CIO4 Perchlorate 32 NH4+ Ammonium 8 Sl6 Sulfur Hexiodide 48 IF5 lodine Pentafluoride 42
- Draw the Lewis dot structure for CBr4 . Choose the answer below that gives the (I) number of lone pairs and (II) number of chemical bonds on the central atom along with (III) the number of double bonds in the compound. Group of answer choices 0 lone pairs, 3 bonds, 0 multiple bonds 1 lone pair, 4 bonds, 1 multiple bond 2 lone pairs, 4 bonds, 2 multiple bonds 1 lone pair, 4 bonds, 0 multiple bonds 0 lone pairs, 4 bonds, 2 multiple bonds 0 lone pairs, 4 bonds, 0 multiple bondsA Moving to another question will save this response. Question 3 For the molecule below, the s bond between the carbons marked I and II is formed by superimposition of the following orbitals: H II H3C- -CH3 H O Carbon I: sp and Carbon II: sp3 O Carbon I: sp² and Carbon II: sp Carbon I: sp2 and Carbon II: sp3 Carbon I: sp and Carbon II: sp2 A Moving to another question will save this response.Can you explain the equation and answer? Where did you get 4 for electrons in bonding? How do you calculate electrons in anti bonding? Li2 would look like "Li-Li" so wouldn't it only have 2 electrons in bonding since a single bond is only 2 electrons?
