GMontenaro M3 Lab 2 Lewis Structures and Molecular Shapes

Column I: Draw the best Lewis structure. Label any atoms with nonzero formal charge. Column II: List the total number of major resonance contributors and draw at least two (if they exist). Column III: How many electron groups are around the central atom? Column IV: What is the electron geometry? Column V: What is the molecular geometry? Possible answers: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, bent, trigonal pyramidal, see-saw, T-shaped, square pyramidal, square planar). Column VI: Give values of the bond angles around the central atom. (for example, 109.5°, less than 109.5°, 120°, less than 120°, etc.). Column VII: Give the hybridization of the central atom. Column VIII: State how many sigma bonds and pi bonds are present in the molecule or ion. Column IX: Is the molecule polar or non-polar?

Part A) Consider the structural changes that occur in the following molecules. Begin by drawing the best Lewis Structure for each of the following molecules. BH3 CH4 NH3 H2O HF Part B)What are the ideal bond angles for each structure, and which are expected to be distorted? For the ones that are distorted look up on the internet and record their experimental values here:    Part C)According to Lewis and VSEPR theory, why do these changes occur?

For the molecule of PBr5 1-Provide the electronic structure of the atom of phosphorous (1s, 2s, etc). Draw the levels of energy and electrons 2-Provide the general formula of the molecule (ABE). This molecule does not have lone pairs 3- Provide the shape for this molecule according to VESPR ( 4- How many electron domains do you have?r 5- Provide the electronic structure of Phosphorous in this molecule, indicating the hybrid orbital: 6-What is the name of this hybridization? Exnlain

Attempts ****** n Force Once started, this test must be completed in one sitting. Do not leave the test before clicking Save and Submit. Completion Your answers are saved automatically. Remaining Time: 1 hour, 57 minutes, 27 seconds. * Question Completion Status: Moving to another question will save this response. Question 12 For the molecule: NO3 What is the geometry of the molecule? Are resonance forms possible? What is the hybridization of the central atom? Is the molecule polar? A Moving to another question will save this response.

Answer the questions in the table below about the shape of the fluoroform (CHF3) molecule. How many electron groups are around the central carbon 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 carbon atom? (You may need to use the scrollbar to see all the choices.) 0 (choose one) X 8

- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 9. Na3P valence e = REDs = shape= bond angles = 10. AI(NO3)3 valence e = REDs = shape = bond angles = sodium phosphide aluminum nitrate For nitrate

- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 6. OCI2 valence e = REDS = shape= bond angles = oxygen dichloride 7. P2S4 valence e = REDs at each central atom = shape at each central atom = bond angles = diphosphorus tetrasulfide dicarbon tetrachloride 8. C2C14 valence e = REDs at each central atom = shape at each central atom = bond angles =

- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 1. H2CCI2 valence e = REDS = shape= bond angles = 2. NC13 valence e = REDs = shape= bond angles = 3. CS2 valence e = REDS = shape= bond angles = dihydrogen carbon dichloride nitrogen trichloride carbon disulfide

Predicting deviations from ideal bond angles Consider the nitrogen trifluoride (NF3) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the nitrogen-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the nitrogen-fluorine bonds to be ... 0 口。 (choose one) (choose one) about the same bigger smaller

2. From the models of SF4, BrF3, and XeF4, deduce whether different atom arrangement, called geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction, Preferred Molecular Compound Electron Dipole Reason Geometry Moment (Polarity) geometry SF4 BRF3 XeF4 3. Using the Lewis structure predict the geometrical structures of the following ions and state the hybridization of the central atom. Ion Electron Geometry Molecular Formal Charge Central Atom Geometry of Central Hybridization Atom CO32- NO3- BF4

Please help me answer these lab questions Molecular-Models experiment

PLEASEEEE HELP ME ASAP!!!Use you knowledge of Lewis structures, polarity, Table 1, and Table 2 to complete the table below for each molecule listed.

= O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles Consider the ammonium (NH) cation. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? 0 What is the ideal angle between the nitrogen- hydrogen bonds? Compared to the ideal angle, you would expect the actual angle between the nitrogen-hydrogen bonds to be... 0. (choose one) X 0/5

= O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles = (co-) anion. Consider the carbonate What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the carbon-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the carbon-oxygen bonds to be... 0 7 (choose one) X 5 3/5

Consider the anion PF52-. Draw the correct 3-D Lewis Structure. Include all resonance hybrids, if needed. If you use formal charge to determine the best structure, show your calculations. Label (with a value) the F-P-F bond angle(s). Label partial charges on atoms and polar bond vectors, if appropriate. Record the Electron Cloud Geometry and the Molecular Geometry. If the molecule/polyatomic ion has overall molecular polarity, clearly label the overall partial charges and overall molecular polarity vector on the Lewis structure.

♥ Draw Lewis structures for each of the following. Give the total number of valence electrons,select from the lists the number of Regions of Electron Density (REDs) around the central atom,the molecular shape, and the bond angles.♥ Do not put covalent bonds between metals and nonmetals.♥ Put brackets around anions to show both charge and quantity.

11 Name: Maddie Klink Instructor: Lab Day: Models of Organic Molecules Please bring your molecular model kits to lab for the completion of these exercises. Molecular Modeling: This lab is designed to help you become comfortable using model kits to visualize molecular structures in three dimensions. Part I: Answer these questions before doing any work with your model kit 1. How many bonds must each of the following atoms have in order to have no formal charge? 4 valence 1450na a. Carbon b. Hydrogen bond c. Oxygen d. Chlorine 7 valence e. Nitrogen 5 valence Octet H- H Complete octet = 8-4 H 8-S = 3 3bonds 2. Using the information from question #1, determine whether each of the following structures is possible or impossible? (Note that if no formal charges are shown, this implies that all formal charges are zero.) 6 valence Octet = 8.6 H H с-н H 01C C -K = 2 bonas 8-1-1 bond H H H-C Lab Time: H -C-H H H H-C-CI- C-H ++ H H -H HIC C-H H VEUR 1

The caffeine molecule is shown below. Indicate the electron geometry AND the molecular shape around each of the indicated atoms (six answers in total). Be aware that the angles may not be drawn correctly in this Lewis structure.

please draw a lewis structure, determine the # of electron groups around the central atom, and determine the geometry of the molecule. (please state both the name of the geometry and draw the molecular shape) molecule lewis structure electron pair geometry around the central atom(s) molecular shape around the central atom(s) CO2       H2S       H2O2       NF3       SO2Cl2       NO2       C2H2       C2H4       C2H6

Step 1 – Write the Lewis structure from the molecular formula.Step 2 – Assign an electron-group arrangement by counting all electron groups (bonding plus nonbonding) around the central atom (or around each centralatom, if more than one central atom in structure).Step 3 – Predict the ideal bond angle from the electron-group arrangement and the effect of any deviation caused by lone pairs or double bonds.Step 4 – Name the molecular shape by counting bonding groups and nonbonding groups separately.Step 5 – Predict whether the molecule is polar or nonpolarStep 6 – Describe the hybridization around the central atom and identify the total number of σ and π bonds in the structure

For each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry and  Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using  wedges and dashes to show 3D if needed) of the Molecular Geometry.

Name the electron pair geometry and the molecular structure (shape) for each of the following molecules.       PCl3                                                                                                                          SF4                                                                                                     IBr5                 CO32-                           NO2+

BF4 Sketch the proper Lewis structure for this substance. Be sure to follow octet/duet rules for each atom and use the total number of valence electrons available. Use your drawing to answer the following questions. Count the total number of electron domains surrounding the central atom. Enter the value only. Enter the name corresponding to the electron domain geometry. Choices are: linear, trigonal planar, or tetrahedral. Enter the name corresponding to the molecular geometry. Choices are: linear, trigonal planar, tetrahedral, bent, or trigonal pyramidal. Predict the bond angle. Enter the value without units. Use a "<" if needed.

Name: Lab #9 Electron and Molecular Geometries - Polarity Report Sheet Part D: Applying VSEPR Theory For each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry and Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using wedges and dashes to show 3D if needed) of the Molecular Geometry. Lewis Structure Total Number of Name of Name of Bond Sketch of Molecular Number of Nonbonding Pairs Electron Molecular Angle Geometry Substituents Geometry Geometry S=C=S :Cl: C=0: :Cl: .. F H. HN:H 一一 -F:

ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles Consider the bromate (BrO3) anion. What is the central atom? Enter its emical symbol. How many lone pairs are around the central atom? What is the ideal angle between the bromine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the bromine-oxygen bonds to be ... 0 口。 (choose one)

Please don't provide handwriting solution

|| Predicting deviations from ideal bond angles Consider the carbonyl fluoride (CF₂O) molecule. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the carbon-fluorine bonds? Compared to the ideal angle, you would expect the actual angle between the carbon-fluorine bonds to be ... 口。 (choose one) (choose one) about the same bigger smaller

Decide whether the Lewis structure proposed for each molecule is reasonable or not. Note: 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. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

Determine the electron pair geometry (EPG), the molecular geometry (MG), the bong angle (BA), and the polarity of SO2. NOTE: Be sure to enter in your answers with correct spelling, spacing, and all lowercase letters; for the bond angle just type in the number; for the polarity enter "yes" for polar and "no" for nonpolar. ЕPG: MG: ВА: polar? enter yes or no: