GMontenaro M3 Lab 2 Lewis Structures and Molecular Shapes

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

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.

THIS is the equation N2H4 + O2 → N2 + H2O PLEASE HELP AND LOOK AT THE PICTURE FOR DATA  PLEASE HELP! I REALLY NEED HELP BECAUSE MY TEACHER HASENT TAUGHT ME HOW TO DO THIS PLEASE HELP!!!!!   Balance the equation (if not already balanced) Draw the models of the molecules in the equation, using Lewis structures, ball and stick models or something else that represents each of the atoms and how they are connected.  Identify bonds being formed or broken.  Use bond energy values from below to Calculate the overall energy of the reaction. Determine if the reaction is exothermic or endothermic. Draw a potential energy diagram showing the ∆H, reactants and products. Create one example of mass (g) to mass (g) stoichiometry problem.

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

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)

- 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. Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Types nonpolar covalent polar covalent nonpolar & polar covalent ionic ionic & covalent Type of molecule Nonpolar Polar lonic 1. HCC13 valence e-1 = shape= type of bonds = type of molecule = 2. SCI2 valence e-1 = shape= type of bonds = type of molecule = 3. P204 valence e-1 = shape= type of bonds = type of molecule = 4. N2O4 valence e-1 = shape= type of bonds = type of molecule = hydrogen carbon trichloride sulfur dichloride diphosphorus tetroxide dinitrogen tetroxide

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|| 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

1/1 The table shows the type of bonding in a number of elements and compounds. Element or compound Type of bonding Fe, Na metallic NaCl, MgCl, ionic Co, Br, covalent within the molecules CL. di Drawa dot-and-cross diagram for carbon dioxide. ii Describe the shape of the carbon dioxide molecule. iii Explain why a carbon dioxide molecule has this shape. e Bromine is a liquid at room temperature. Weak van der Waals' forces hold the bromine molecules together. Describe how van der Waals' forces arise.

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:

Draw the 2D and the 3D Lewis structure for each molecule. You do not need to show resonance structures here. Determine the electron pair geometry (EPG), the molecular geometry (MG), the bond angle (BA) around the central atom, and the hybridization of the central or bold atom. Circle the formula of any polar molecule. For molecules with more than one central atom (e.g. CHCH20H) give the structure around the bold atom.

♥ Draw Lewis structures for each of the following. Use the DEN and the number of REDs around thecentral atom to select the type of bonds, the molecular shape, and type of molecule from the lists.♥ Do not put covalent bonds between metals and nonmetals♥ Put brackets around anions to show both charge and quantity.

Use the following information to determine the Lewis structure, find the electron and molecular geometry of the molecule, determine the angle of the molecule, and determine the polarity. If the atoms are not the same, you may assume that the difference in their electronegativities are between 0.4 and 2.0. Atom information: A: 7 valence electrons, CAN exceed the octet. Further from fluorine on the periodic table than X. X: 7 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic table than A. Molecule: AX3 Electron Geometry: [Select] Molecular Geometry: [Select] Bond Angle: [ Select ] Polarity: [Select]

For the formula CH2CF2, "draw the Lewis structure in your work 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 CH2)? 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 sp would be typed as "sp3". Is the molecule overall polar or nonpolar? Simply type "polar" or…

Predicting the single-bonded molecular compounds formed by two elements.

Predicting the single-bonded molecular compounds formed by two elements.

Predicting the single-bonded molecular compounds formed by two elements.