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?

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.

Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-radical combination reaction is the formation of a new electron-pair bond. Consider the chemical equation. N(g)+NO(g) NNO(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons.

If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. If two oxygen atoms don't satisfy the octet rule, enter "O,O".

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:

- 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 Ionic 5. C2Cl2 valence e-1 = shape= type of bonds = type of molecule = 6. AICI3 valence e-1 for one Cl-1 = shape= type of bonds = type of molecule = 7. K3PO3 valence e-1 = shape= type of bonds = type of molecule = 8. KH2PO3 valence e-1 = shape at the P= type of bonds = type of molecule = dicarbon dichloride aluminum chloride potassium phosphite potassium dihydrogen phosphite

- 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

Please help

|| 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:

10:03 88% Number of Number of Resonance Valence Remaining Electrons Lewis Structure with Structures? Molecule Electrons Bond Skeleton Formal Charges How many? C2H4 C2H2 CO H2S HCN N½H4 NO, 2 of 2

Draw regular Lewis structures (no need to use dashed lines and wedges) of the following ions and name (no need to draw them) both the electron geometry and the molecular geometry for each. If an ion has resonance structures, present any one. You do not need to show any formal charges. Formula Lewis structure Electron geometry Molecular geometry PFA* 2- AsBr3? NO2

♥ 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.

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…

Should 100% sure of answer. Draw the Lewis structure of HBrO₃ (by following the octet rule on all atoms) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure.

Please answer all parts of the question

I had gotten this one incorrect, but i wanted to use it to study, so please give me the solution to all parts of this question.

♥ 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. 1. HCI hydrogen chloride valence e = REDS = shape= bond angles = 2. CCl4 valence e = REDS = shape bond angles = carbon tetrachloride REDS 0, no central atom 234 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5⁰ 120⁰ 180⁰ none, no central atom

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: 5 valence electrons. Further from fluorine on the periodic table than X. X: 7 valence electrons. Closer to fluorine on the periodic table than A. Molecule: AX3 Electron Geometry; Linear, Trigonal Planar, Tetrahedral molecular geometry: liner, trigonal planar, tetrahedral,bent bond angle ??? polarity ???

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.

Molecular geometry—don’t know why I’m incorrect all of a sudden. Might be one shape needed that is not given in the option choices.

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