Would u help me with my homework, please? A₁ B3 E₁ = A B3 EMolecular Shape of NI3Step 1: Find the Central AtomNCentral atom is:Look your line bond structure onpage 1.AB₁E3 AB₁E₂AB₂EDEStep 3: Choose the ABE classificationCircle the correct AB, E, notation.Recall, we use (A) to represent thecentral atom, (B) to represent thenumber of atoms bonded to the centralatom, and (E) to represent the numberof lone pairsNAB₁EAB₂E₂ AB₂AB EAB3AB4Step 5: Use the Molecular Shapetable from your notes to draw theball and stick representation(11N Central atom AINIloneBatom surrounding central a tom)pair Elonine paircentral atomlStep 2:Count number of atoms bonded to the centralatom (B)# of atoms bonded to central atom = B = 3Count number of lone pairs on thecentral atom (E)# of lone pairs on central atom = E=__Step 4: Use the Molecular Shape Table fromyour notes to select the molecular shape andbond angles.Molecular Shape-yramidalBond angles = 110°Step 6: Determine PolarityIs the central atom surrounded by identicalelectron groups?Circle one: yes noIf the answer was yes, then the molecule isnonpolar. If the answer is no, then the moleculeisIs the molecule polar?Circle one: yes no21

Answered: Image /qna-images/answer/a8e80b03-be45-4321-80a6-ebfea356ca6c.jpg

A₁ B3 E₁ = A B3 E Molecular Shape Step 1: Find the Central Atom N Central atom is: Look your line bond structure on page 1. 00 AB₁E3 AB₁E₂ AB₂E DE Step 3: Choose the ABE classification Circle the correct AB, E, notation. Recall, we use (A) to represent the central atom, (B) to represent the number of atoms bonded to the central atom, and (E) to represent the number of lone pairs N AB₁E AB₂E₂ AB₂ AB E AB3 AB4 Step 5: Use the Molecular Shape table from your notes to draw the ball and stick representation of NI3 ( N Central atom A I W Batom surrounding central a tom) lone pair Elon ine paircentral atom Step 2: Count number of atoms bonded to the central atom (B) # of atoms bonded to central atom = B = 3 Count number of lone pairs on the central atom (E) # of lone pairs on central atom = E=__ Step 4: Use the Molecular Shape Table from your notes to select the molecular shape and bond angles. Molecular Shape-yramidal Bond angles = 1100 Step 6: Determine Polarity Is the central atom surrounded by identical electron groups? Circle one: yes no If the answer was yes, then the molecule is nonpolar. If the answer is no, then the molecule is Is the molecule polar? Circle one: yes no 21

A₁ B3 E₁ = A B3 E Molecular Shape Step 1: Find the Central Atom N Central atom is: Look your line bond structure on page 1. 00 AB₁E3 AB₁E₂ AB₂E DE Step 3: Choose the ABE classification Circle the correct AB, E, notation. Recall, we use (A) to represent the central atom, (B) to represent the number of atoms bonded to the central atom, and (E) to represent the number of lone pairs N AB₁E AB₂E₂ AB₂ AB E AB3 AB4 Step 5: Use the Molecular Shape table from your notes to draw the ball and stick representation of NI3 ( N Central atom A I W Batom surrounding central a tom) lone pair Elon ine paircentral atom Step 2: Count number of atoms bonded to the central atom (B) # of atoms bonded to central atom = B = 3 Count number of lone pairs on the central atom (E) # of lone pairs on central atom = E=__ Step 4: Use the Molecular Shape Table from your notes to select the molecular shape and bond angles. Molecular Shape-yramidal Bond angles = 1100 Step 6: Determine Polarity Is the central atom surrounded by identical electron groups? Circle one: yes no If the answer was yes, then the molecule is nonpolar. If the answer is no, then the molecule is Is the molecule polar? Circle one: yes no 21

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter1: Bond Angles And Shape

Section: Chapter Questions

Problem 12CTQ: Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this...

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Similar questions

How many and bonds are present in the molecule HCN?
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
Complete the table on next page.
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3 Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
Use VSEPR to explain why the HBH bond angle of BH3 is 120°. (Hint: What is one-third of360°?)
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Use the information on the fictious nonmetal elements. to answer the following Element Colomn EN ff 1.9 14 17 3.1 2.3 3.6 15 Nn 16 Shoos one of the followng mokcular compounds and completc the queSTIons: Nn Oyzlshape is benti V) ODraw a leuis Structure Shoudng all lalonce electrons. ) Calculate the electrongativity the bond. State what a paar covalert band, notate the partial difference for Gf bond will form If it is charges d) Detamine if the molecule is polar or polar. non-