Respond to Questions on Lewis structure and molecular geometry using VSEPR model. For each of the following two substances NOCI and SF6 answer the following questions: a. Draw Lewis dot structure (include all dots necessary for each atom) b. Identify the name of molecular geometry c. Identify bond angles d. Identify the molecular polarity of each substance e. Calculate the formal charge of S atom in SF6 f. Calculate the formal charge of N atom in NOCI

Respond to Questions on Lewis structure and molecular geometry using VSEPR model. For each of the following two substances NOCI and SF6 answer the following questions: a. Draw Lewis dot structure (include all dots necessary for each atom) b. Identify the name of molecular geometry c. Identify bond angles d. Identify the molecular polarity of each substance e. Calculate the formal charge of S atom in SF6 f. Calculate the formal charge of N atom in NOCI

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...

See similar textbooks

Similar questions

How many valence electrons does a neutral a. K atom have? b. C atom? N atom? O atom?
Despite the larger electronegativity difference between the bond atoms, BeCl2(a) has no dipole moment whereas SCl2(g) does possess one. Account for this difference in polarity. The answer should labelling of: Lewis structure, AXE notation, molecular and electron geometry, partial charge, dipole moment, and explanation.
Draw the Lewis Structure of N3- Molecular Geometry? Ideal Bond Angles? Are there Polar Bonds Present (Indicate on Lewis do structure Is there an Overall Dipole? Octet rule violator and how?
Our class has just touched on molecular shapes/geometries and the last HW question contains this Nitrogen atom with a + formal charge. How would the VSEPR Molecular Shape look like? Also, If the same number of bonds and charge were kept and the Nitrogen was swapped with a Carbon, would both shapes be the same? Thank you.
1. NH2Cl a. In NH2Cl there is a total of ____________ valence electrons. b. The NH2Cl model consists of how many lone pairs of electrons c. How many bonds are in the NH2Cl molecule? d . What is the shape the atoms make (excluding lone pairs) in NH2Cl?
For the following molecules:I. Draw the best Lewis Dot Structures for each of the following molecules. The best structuretakes into consideration resonance structures, calculations of formal charge for each atom,and tries to minimize the overall formal charge for the structure. II. Draw the 3-D VSEPR structures for the following molecules. You may combine these twodrawings (for I and II) into 1 drawing if you wish. III. Label the bond angles. IV. State the electron geometry (basic VSEPR) and molecular shape (derivative VSEPR) foreach molecule. V. State the hybridization around each central atom in the molecule. VI. State whether the overall molecule is polar or nonpolar. VII. For any two of the following molecules, state the strongest intermolecular force betweenmultiple of the same molecule.a. IF2b. H2CO3c. CH3CH2COOHd. N2O4e. PO4^3-f. CH3COCNg. ClO3^-1h. C4H8
Place the following in order of decreasing X-AX bond angle, where A represents the central atom and X represents the outer atoms in each molecule: CS2, CF4, SCl2. I initially thought that SCl would have a greater bond angle than CF4. Is this not the case because the bond angle of SCl2 is approximately 109.5, while CF4 is exactly 109.5 degress?
( plz explaing with clear diagram and bond angle )
) Draw a Lewis structure the molecule or ion below. Draw any resonance structures. Determine the formal charges on atoms in each of your resonance structures. Based on this, determine which resonance structure(s) are most important. Circle the most important contributor(s) to the resonance hybrid. If they are all equivalent, circle them all. COFCl
PLS REFER TO THE PICTURE BELOW 1. How many covalent bonds are in the picture? 2. How mant type/s of covalent bond/s forming your double bond do you see? 3. What is/are the types of covalent bond/s forming your double bond do you see? 4. What type of hybrid orbital is the sigma bond? 5. Which electron configuration will you expect the highest energy needed to remove a valence electron?
Draw the best Lewis Structure for NCOF based on overall formal charges. The skeleton framework for NCOF is: N—C—O—F. Answer the questions below based on your final structure. How many bonding (shared) electron pairs are on the nitrogen atom? _________ How many (total) non-bonding electron pairs are in the whole molecule? ______ How many non-bonding electron pairs are on the oxygen atom? _______
You need to devise a 3-D model that demonstrates the bonding between atoms, as well as any lone pairs. Please note that your individual assignment may be for an ion (don't forget about charges) or a neutral atom. Your assigneed ion is : AlCl4-