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Why do actual bond angles differ from the ideal bond angles? How does a lone pair of electrons affect bond angles?
As the lone pair increases,then bond angle decreases. Because lone pair electrons repel the electron pair electrons.so bonds are slightly displaced inside hence bond angle decreases
Why do actual bond angles differ from the ideal bond angles? How does a lone...
1.How does one of more lone pairs of electrons affect the bond angles in a molecule? 2. Why are larger balloons used to represent lone pairs of nonbonded electron domains?
DISCUSSION QUESTIONS 1. In NO," does one of the NO bond distances differ significantly from the other two? Explain. chemically, why you might expect one bond distance to be different. (Hint: Draw a Lewis Structure for NO,':) How is it chemically possible for all of the bond distances in this ion to be the same? Explain. 2. and SF, both have 4 atoms bonded to a central atom, but have different Explain why PO molecular shapes. 3. In the Sta...
1. What did you notice about the shapes with and without the lone pairs? how do the lone lairs affect the final shape? Guidelines for Drawing Lewis Structures. STEP 1: Determine the total number of valence electrons for the molecule. STEP 2: Determine the skeletal structure arrangement of atoms) of the compound. For simple compounds the singular atom will be in the center with the others arranged around it. STEP 3: Attach each bonded atom to the central atom with...
How do the bondangles in the six atom ring (created when ASA binds to Fe3+) differ fromthe bond angles of the six atom benzene ring?
Lewis Dot structure Electronic geometry Molecular shape Ideal Bond angles Hybridization of central atom Does it contain polar bonds? is the molecule polar? Seci, Lewis Dot structure Electronic geometry Molecular shape Ideal Bond angles Hybridization of central atom Does it contain polar bonds? Is the molecule polar? 124 Chemical Bonding Laboratory 12
how does the action potential stimulating heart muscle cells differ from other action potentials, and why? How does this affect the refractory period of heart muscle cells?
Determine the geometries and expected bond angles for the following molecules (i.e. indicate where possible and deviation from ideal angles).Give a brief explanation for your predictions. Also indicate where the lone pairs should be and why i. NH3 ii. PF6- iii. NO2- iv. SeH2 v. XeOF2 vi. I3- vii. SOCl2
3. What do the Phi (Q) and psi (y) angles represent? How do these angles differ between a-helix and B-sheet secondary structures?
2. Knowing that the groups of electrons around the central atom affect the molecule shape, how do you think this will affect the interactions between two molecules called intermolecular interactions? Guidelines for Drawing Lewis Structures STEP 1: Determine the total number of valence electrons for the molecule. STEP 2: Determine the skeletal structure (arrangement of atoms) of the compound. For simple compounds the singular atom will be in the center with the others arranged around it. Attach each bonded atom...
Question 5 a. How many lone electrons does iridium contain? b. How many lone electrons does Rut4 contain? c. How many lone electrons does Mo+3 contain?