Question: 9. Which of the following statements best
9. Which of the following statements best explains the information we can gain from mass spectrometry? a. It allows us to determine the number of protons in a compound. b. It allows us to determine the kinds of functional groups in a compound. c. It allows us to determine the molecular weight and the mass of some fragments of a compound. d. It allows us to determine the presence and nature of a double or triple bond in the compound. 
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10. Which of the following is the strongest base? b) Н20 d) Cнзон a) HOMGBR CH3M9BR 11. Which molecule below has a significant band in the IR at 3400 cm-1 (strong and broad)? c) CH4 a) CH3CH2CH2OH b) CH3C"CCH2CH3 c) CH3CH2CH(NH2)CH3 d) (CH3)3N e) CH3CO2CH2CH3 12. Ether is a good solvent for Grignard reagent since a) ether is less polar than water or alcohol ether is more polar than water or alcohol c) the magnesium atom shares the electron pair with oxygen of ether d) oxygen of ether shares electron pairs with alkyl groups 13. Which radiation is lower in energy relatively? a) microwave b) visible c) radio-wave d) infrared 14. Which molecule below has a significant band in the 1720 - 1780 cm-1 range of its IR spectrum? a) CH3CH2CH2OH b) CH3C"CCH2CH3 c) CH3CH2CH(NH2)CH3 d) (CH3)3N e) CH3CO2CH2CH3 15. Which of the following statements best explains the information we can gain from infrared spectroscopy? a) It allows us to determine the number of protons in a compound. b) It allows us to determine the kinds of functional groups in a compound. c) It allows us to determine the molecular weight and the mass of some fragments of a compound. d) It allows us to determine the presence and nature of a double or triple bond in the compound. 16. Which of the following most nearly describes the geometry of the methyl radical? a) trigonal pyramid, bond angle 109.5° b) trigonal pyramid, bond angle 120° c) trigonal planar, bond angle 109.5° d) trigonal planar, bond angle 120° 17. Which of the following is the most stable radical? IV. CH,CH, CH;=CHCH;CH, V. CH,CH I. CH;=CH www.
> Mixture-show any isomers or resonance structures, use multiple bonds if needed, and show any nonzero formal charges. of Molecular VSEPR 3-D Structure Geometry (show polarity) Formula Lewis Structure val. E's Becl, O, IFs CH.O CIO, PF
> Are the O-N-O bond angles greater in the nitrite ion (NO2-) or the nitrate ion (NO3-)? Please select the answer that best explains your conclusion. a. Nitrite has the greater bond angle because a trigonal planar bond angle is greater than a tetrahedral b
> Draw the Lewis structure for each of the following compounds. Using VSEPR, determine the electron pair geometry, the molecular geometry, and the bond angle (in degrees) for each compound. 7. CIF, Molecular Geometry: Bond Angle(s): Lewis Structure: El
> Lewis Structure Electron geometry 4. H30+ Molecular geometry Valence electrons 5. NH3 Lewis Structure Electron geometry Valence electrons Molecular geometry Electron geometry 4. H3O* Lewis Structure Molecular geometry Valence electrons 5. NH3 Lewis S
> # of Electron Groups IFS Electron Geometry Molecular Geometry 10. CS2 Lewis Structure # of Electron Groups Electron Geometry Molecular Geometry Structure: of Electron Groups F5 Electron Geometry Molecular Geometry 10. CS: Lewis Structure: of Electron
> 1. Formula SF4 Molecule Geometry: Electron Geometry 2. Formula XeF4 Molecule Geometry Electron Geometry:
> 1. SO Lewis Structure: # of Electron Groups Electron Geometry Molecular Geometry 2. SO Lewis Structure: # of Electron Groups Electron Geometry 1. SO, Lewis Structure of Electron Groups Electron Geometry Molecular Geometry 2. SO: Lewis Structure: of E
> 5. XeF2 Lewis Structure: # of Electron Groups Electron Geometry Molecular Geometry 6. H2S Lewis Structure: # of Electron Groups Electron Geometry Molecular Geometry 5. XeF2 Lewis Structure: # of Electron Groups Electron Geometry Molecular Geometry 6
> The Atomic radius is one property which is a periodic trend. The atomic radius: A. Deceases continuously as you go left to right across a period on the periodic table B. Increases down a group on the periodic table C. increases continuously as you go lef
> 10. PCI2F3 Lewis Structure* Electron geometry Valence electrons Molecular geometry 11. CIO2 Lewis Structure Electron geometry 10. PCl Fs Lewis Structure Encton gemery Valence olectrons Mclecul gemery Electron geometry 11. CIO2 Lewis Structure Molecul
> 7. AsFs Lewis Structure Electron geometry Valence electrons Molecular geometry Lewis Structure 8. ASF3 Electron geometry 7. AsFs Lewis Structure Ewctron gemetry Valence electrons Mcincuar genmetry Electron geometry B. ASF3 Lewis Structure Molecular g
> Complete the Lewis structures for the following molecules. A complete Lewis structure should show all non-zcro formal charges on atoms. Complete the formal charges on the structures below. CHEM 1430 LEWIS STRUCTURES SPRING 2018 Lewis Structure with
> In the best Lewis structure for XeF2, what are the electron geometry and the molecular shape around the central xenon atom? Electron geometry: Octahedral Molecular shape: Linear Electron geometry: Tetrahedral Molecular shape: Bent O Electron geometry
> Electron geometry 1. CF4 Lewis Structure Molecular geometry Valence electrons Electron geometry Lewis Structure 2. CH2Cl2 Molecular geometry Valence electrons 1. CF4 Lewis Structure Electron geometry Valence electrons Molecular geometry 2. CH2CI2 Ele
> 7. AsFs Lewis Structure drogometry Valence centros Meer geometry 8. ASF Lewis Structure Valence electrons Magomery 9. Gal3 Lewis Structure 7. ASFS Tcbrongeomiry Lewis S Valence electrore Mdgeomety Exctron geomry 8. ASF3 Lewis Stucture Moleculer gene
> Lewis Structure: SF6 Sketch Total # of e. Electron Geometry Molecular Geometry Hybridization Polarity Lewis Structure: Lewis Structure: SF6 Sketch Total # of e Electron Geometry Molecular Geometry Hybridization Polarity Lewis Structure: IFs Sketch To
> Determine the electron geometry (eg) and molecular geometry (mg) of CO32-. Determine the electron geometry (eg) and molecular geometry (mg) of CO32. ANSWER: 1 eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=bent eg=tetrahedral, mg=trig
> Complete the table below. Show Formal Charges if necessary. 8. Complete the MOLECULE POLARITY SHAPE LEWIS STRUCTURE FORMULA BOND POLARITY Electron Geometry H. 3on CH4 Polar H..C- H Molecule Geometry H. Electron Geometry Dolar H20 Malecule Geometry El
> What is the electron geometry and molecular geometry of SOCl2? trigonal planar electron geometry, trigonal planar molecular geometry. TBP electron geometry, T-shaped molecular geometry. tetrahedral electron geometry, trigonal molecular geometry. tetra
> Lewis Structure: # of Electron Groups 5 Electron Geometry trigonal Molecular Geometry linear 6. HS Lewis Structure: 5. XeF; Lewis Structure: *of Electron Groups xi- F: Electron Geometry trigonal F - Molecular Geometry linear 6. H,S Lewis Structure:
> Describe a periodic trend in the periodic table. What elements are considered when discussing periodic table trends?
> Draw the Lewis structure for each molecule. Determine the electron and molecular geometry. Then, draw the perspective drawing. 5. Electron geometry: Molecular geometry: 6. NI, Electron geometry: Molecular geometry: 7. SF. Electron geometry:, Molecul
> Formula Lewis Structure with formal charge. Treat this as both an ionic and covalent species. Formula Lews Structure with formal charge Formula Lewis Structure with formal charg Brfs Brfs CH:Br (C-C bond) SeCla TeCla NO XeFa SeCla H;CO КОН Treat this
> Molecule lewis structure electron-dot structural formula molecular geometry (drawing) MOLECULAR Procedure No. LEWIS STRUCTURE GEOMETRY STRUCTURAL FORMULA MOLECULE ELECTRON-DOT (drawing) 3 CH4 Molecular geometry (name) Electron Geometry (name) H2O Mol
> What are the electron geometry and molecular geometry of the oxygen atom in isopropanol? tetrahedral electron geometry and bent molecular geometry tetrahedral electron geometry and linear molecular geometry linear electron geometry and linear molecula
> What is the electron geometry of this molecule? What is the electron geometry and molecular geometry of the molecule shown? electron geometry: pyramidal, molecular geometry: tetrahedral electron geometry: tetrahedral, molecular geometry: tetrahedral
> 1.Formula: SF6 Molecule Geometry: Electron Geometry: 2. Formula: BrF5 Molecule Geometry: Electron Geometry: 3. PCI5 Molecule Geometry: Electron Geometry:
> 1. Formula: CO2 Molecule Geometry: Electron Geometry: 2. Formula: CIF3 Electron geometry: Molecule geometry: 3. Formula: BF3 Electron geometry: Molecule Geometry:
> What is the electron geometry and molecular geometry for the central atom in the following structure? 2- :OH -P- O: :0 Electron geometry: tetrahedral Molecular geometry: tetrahedral Electron geometry: tetrahedral Molecular geometry: trigonal planar
> What is the electron geometry and molecular geometry for the central atom in the following structure? Electron geometry: tetrahedral Molecular geometry: tetrahedral Electron geometry: trigonal pyramidal Molecular geometry trigonal pyramidal Electron g
> Determine the electron geometry and molecular geometry of KrF2 according to VSEPR theory. a. electron geometry = tetrahedral and molecular geometry = bent b. electron geometry = linear and molecular geometry = linear c. electron geometry = octahedral and
> Predict the electron geometry and molecular geometry for each of the following molecules: a. NF3 electron geometry: ISelect ] molecular geometry: ISelect| b. H2S electron geometry: [Select] molecular geometry: (Select ] c. SiH4 electron geometry: (Se
> The main difference between Mendeleev's periodic table and our modern periodic table is: a. Mendeleev's table was organized by element mass. Our modern periodic table is organized by atomic number b. nothing. They are identical. c. Mendeleev's table w
> Using formal charge formula (or electronegativity differences), to determine the following the best structure, OCS, COS or CSO.
> BF3 electron geometry: molecular geometry: BrCl5 electron geometry: molecular geometry: CCl4 electron geometry: molecular geometry: O3: electron geometry: molecular geometry:
> Predict the molecular structure and bond angles for each molecule or ion given below. SO2 NF3 sch tetrahedral V-shaped trigonal pyramid V-shaped • trigonal planar trigonal pyramid V-shaped V-shaped O trigonal planar O trigonal planar trigonal planar
> Complete the following table. Remember to add electrons such that each center has an octet of electrons. 3 Tartrazine element 1 element 2 element 3 element 4 O 180° 180 180° O 100° O 120 O 120 O 120° O 1200 bond angle O 109 O 109 O 109° O 109 O 90 90
> Complete the following table. Remember to add electrons such that each center has an octet of electrons. Indigo Carmine element 1 element 2 element 3 element 4 O 180° O 180 180° 180° 120° 120 120° 120° bond angle O 109 O 109 109 109 90 O 90° 90° 90 s
> shape octahedral (c) Seo, shape O octahedral seesaw O square pyramidal seesaw O tetrahedral O square pyramidal shape O octahedral (c) Seo,- shape O octahedral seesaw O square pyramidal seesav tetrahedral O square pyramidal O tetrahedral O trigonal p
> Determine the electron-group arrangement, molecular shape, and ideal bond angle(s) for each of the following: Determine the shape, ideal bond angle(s), and the direction of any deviation from these angles for each of the following: (a) NF3 Electron-
> Use VSEPR theory to predict the shape of each of the following: Part A GaHs Tetrahedral Bent with bond angles <120 Trigonal pyramidal Bent with bond angles <109.5 O Trigonal planar O Linear Part B OF, O Tetrahedral Bent with bond angles <109.5 O T
> Predict the molecular structure and bond angles for each molecule or ion given below. Clo • v-shaped • trigonal pyramid • trigonal planar • trigonal pyramid V-shaped tetrahedral • v-shaped • trigonal planar V-shaped • trigonal planar trigonal pyramid
> Determine the electron-group arrangement, molecular shape, and ideal bond angle for the following molecule: SO3 Electron-group arrangement: trigonal planar V-shaped (bent) trigonal pyramidal seesaw Molecular shape: trigonal planar bent square pyramid
> Methyl Violet element 1 element 2 element 3 element 4 180° bond angle 1200 109 90° 180° 120 109 90° Sp 180° -H H. Methyl Violet element 1 element 2 element 3 O 180° element 4 O 180 O 180° O 120°
> Complete the Lewis structures for the following molecules. Formula Lewis Structure Formula Lewis Structure with formal charge with formal charge HO: NHa BrO CO N;O. NH. SH so, NO, OH PO,
> Allura Red AC element 1 element 2 element 3 element 4 180。 120° 109° 90° 180o 120° 109° 90° H. Allura Red AC element 1 element 2 element 3 element 4 180 O 180 O 180
> 22. Which of the following is not a nucleophile? a. CH3NH2 b. NH2+ c. H2O d. CH3+ c) HO d) CH. 23. Which of the following substrates will give the fastest Sl reaction a) 1-bromopropane b) 2-bromopropane )2-chloropropane d) 1-iodopropane 24. Which
> In this experiment you will apply valence shell electron pair repulsion theory (VSEPR) to predict molecular geometry. Afterwards, you will construct three-dimensional molecular models, using small, pronged atoms and flexible bonds (included in the kits),
> Draw the most stable Lewis dot structures for the following compounds. For all atoms, write the formal charge if it is not zero. State the shape of the molecule, the bond angles around the central atom, and whether molecule is polar, nonpolar, or charged
> Molecular Modeling using VSEPR Theory 1. NH3 Lewis Structure: VSEPR Bonding Pairs/Orbitals Part 1. Molecular Modeling using VSEPR Theory 1. NH3 Lewis Structure: VSEPR Bonding Pairs/Orbitals -N-H VSEPR Nonbonding Pairs/Orbitals so 4 total VSEPR orbita
> Given the bond dissociation energies below in Kcal/mol, estimate the ΔHo for the 1. Given the bond dissociation energies below in Kcal/mol, estimate the AHo for the pro step (CH.CH-CI (CHCH . c) +40 kcal/mol a) +22 kcal/mol b) -22 kcal/m
> What are the predicted shape, bond angles and hybridization around the bromine atom in the BrCl4 ion? Geometry Bent Linear Octahedral See saw O Square planar Square pyramid Tetrahedral Trigonal bipyramid Trigonal planar Trigonal pyramid T-Shape Bon
> 10. Which of the following most nearly describes the geometry of the methyl radical? A. trigonal pyramid, bond angle 109.5° B. trigonal pyramid, bond angle 120° C. trigonal planar, bond angle 109.5° D. trigonal planar,
> Could you give me proof of trigonal pyramidal bond angle, where the bond angle
> Complete the Lewis structures for the following molecules. Formula Lewis Structure Formula Lewis Structure with formal charge with formal charge BeFs OCh CH;Br (C-C bond) SeCl TeCla NO: H:CO SO CF XeF CH. BrF.
> Which of the labeled hydrogens is most readily abstracted in a free radical bromination reaction? Which of the following most nearly describes the geometry of the methyl radical? trigonal pyramid. bond angle 109.5o trigonal pyramid, bond angle 120 o
> Drawing a Lewis structure of compound, what are some ways that I can determine if it's polar or nonpolar? Without calculating the electronegative difference, how can I look at a structure and determine if it's polar or nonpolar?
> To determine if a molecule is polar or nonpolar how do I determine the electronegativity difference? 3.5-0.8=2.7
> Is F2 a polar or nonpolar molecule and why? a. F2 is a polar molecule because it has nonbonding electrons. b. F2 is a nonpolar molecule because the F-F bond is nonpolar. c. F2 is a nonpolar molecule because the F-F bond is polar. d. F2 is a polar mo
> If the element is more electronegative than the element A and the difference in electronegativity is > 0.5, is the following molecule polar or nonpolar? X-A-X
> 1. Which element is more electronegative? A. C B. N 2. Which element is more electronegative? A. Cl B. C 3. Is an oxygen molecule polar or nonpolar? A. polar B. nonpolar 4. Is a carbon monoxide molecule polar or nonpolar? A. polar B. nonpolar
> can you explain in detail how to tell if they are polar or nonpolar without knowing their electronegativity values and only their lewis structure? State whether the following compounds are polar or not by drawing the Lewis structure: CSz- SFr OCl- Cl
> Explain how you can use electronegativity to determine if a bond is nonpolar, polar, or ionic. Explain how geometry can determine whether or not a molecule is polar even if it contains polar bonds.
> Fill in the table below. Start at the left and work your way to the right to determine whether each molecule is POLAR or NONPOLAR. You may use the same answer more than once. Use the periodic table and summary figure on page 2 to help you! a. Same atoms
> For the given geometries, what are the predicted bond angles around the central atom? Octahedral Bond Angle = degrees See saw Bond Angle = degrees Square pyramid Bond Angle = degrees Tetrahedral Bond Angle degree
> Add formal charges to each resonance form of HCNO below. Based on the formal charges you added above, which structure is favored? Add formal charges to each resonance form of HCNO below. А. В. С. H- Fo: H- Based on the formal charges you added above,
> Determine the hybridization and the approximate bond angles around the indicated atoms. hybridization bond angle H. H hybridization CH bond angle bond angle CH2 hybridization
> SIMPLE MOLECULES: BOND ANGLES, DIHEDRAL ANGLES, AND BOND LENGTHS A. Propane Measurements: LES, AND BOND LENGTHS A. Propane Measurements CHC2-C3 bond angle 1. 10৭.5 H-C2-H bond angle 2. H-CI-C2 bond angle 3. H-CI-H bond angle C-C bond length in propan
> Give approximate values for the indicated bond angles: C-C-Cl in Cl,CO Bond angle = ON-N-O in N;0 Bond angle =| Bond angles 1, 2, and 3 in phanylalanine (one of the natural amino acids and is a breakdown' product of the artificial sweetener aspartame
> Give the shape/geometry, the approximate bond angles, and hybridization for the atoms in bold in each molecule. brigor b) H H H Ho H H-c c-o-H H H H3CEN-H H-C-C-C-H HH H d) H. C-o H. H-c=C-H H-C-C-o-H ch3 CooH sp3 l09.5° geometry: goned planer bond a
> Give approximate values for the indicated bond angles: Give approximate values for the indicated bond angles: References) a. Cl-S-Cl in SCI, Bond angle = b. F-B-F in BF, Bond angle- c. Bond angles 1, 2, and 3 in phenylalanine (one of the natural amin
> Predict the relative bond angles in BF3 and NF3 A.BF3 bond angles = NF3 bond angles B. BF3 bond angles < NF3 bond angles C. BF3 bond angles < NF3 bond angles D. Relative bond angles cannot be predicted
> B. The C - N - C bond angle in a secondary amine The bond angle is predicted to be similar to the bond angle in water (104.5o). The bond angle is predicted to be similar to the bond angle in ammonia (107.3 o). The bond angle is predicted to be similar
> For each species, draw the molecular geometry (using wedges and dashes and lone pair electrons shown on central atoms). State the electron geometry (EG), molecular geometry (MG), bond angle around the central atom, and if the molecule is polar or nonpola
> 10. Predict the relative bond angles in BF3 and SO2. Relative bond angles cannot be predicted. SO2 bond angle > BF3 bond angles BF3 bond angles > SO2 bond angle BF3 bond angles = SO2 bond angle 11. Which of the following molecules is nonpolar? SeB
> Describe the bond angles in CH2F2 and NH3. Select from below and clearly explain your answers in grammatically correct sentences using appropriate chemical terms and concepts. CH2F2 bond angles > NH3 bond angle NH3 bond angle > CH2F2 bond angles CH2F2 bo
> What is the IUPAC of the compound shown below?
> For each of the following molecules or ions, draw the Lewis structure. Then, indicate the number of substituents on the central atom and the bond angle around the central atom. For each of the following molecules or ions, draw the Lewis structure. Th
> a. Predict the molecular structure and bond angles for SCl2. Approximate bond angles are sufficient. Molecular Structure = Bond Angles = b. Predict the molecular structure and bond angles for SeO3. Approximate bond angles are sufficient. Molecular Struc
> Determine the hybridization and the approximate bond angles around the labeled atoms in this structure. Atom a: Hybridization: Bond angle: Atom b: Hybridization: Bond angle: Atom c: Hybridization: Bond angle: Atom d: Hybridization: Bond angle: Atom
> The F -S -F bond angle in SF6 is the F -Br-F bond angle in BrF5. less than The F-S-F bond angle in SF, is the F-Br-F bond angle in BRF3. equal to The F-S-F T-junction bond angle in SF4 is the F-Cl-F T-junction greater than bond angle in CIF3. The 0-S
> Predict all bond angles about each highlighted carbon atom. a H,C Blue atom bond angles : %3D Red atom bond angles Submit H3C b -CH2OH Blue atom bond angles = CH3 H3C-C cEc+c=CH2 Blue atom bond angles = Red atom bond angles %3D CH, d H,C CH H. CH Blu
> For each species, draw the molecular geometry (using wedges and dashes and lone pair electrons shown on central atoms). State the electron geometry (EG), molecular geometry (MG), bond angle around the central atom, and if the molecule is polar or nonpola
> What is the pH of 2.9M solution HClO4?
> What is the pH of a solution of .0300 M KHSO4?
> a. Calculate the pH of a 1.4M sodium hydrogen sulfate solution. Ka = 1.3x10-2 b. Find the pH of a 2.9M solution of KHSO4(HSO4-, Ka = 1.3x10-2)
> Find the pH of a 2.9M solution of KHSO4 (HSO4- K, = 1.3 x 102)
> Ka of acetic acid Given: 10mL of 1.0 M acetic acid mination of the K, of acetic acid Measured pH of the solution 2.37 pH Calculate the (H,0] at equilibrium for this solution. (include units) (H,O"lm Calculate the (CH,CO0] at equilibrium for this solu
> Draw the products of the following reaction. ii HyC-CH- -CH-CH + NH
> Spell out the full name of the compound. A. B. C. E. F. H3CH2CH2C´ `O` Na* O=U `NH2
> Please give the name for the product of the hydrogenation, and the names for the aromatic compounds. 1. 1- Pentene 2. 3- Methylcyclopentene 3. 4. CH3 NH2 CH3 CH2-CH3
> Spell out the full name of the compound. Part A Part B H3C-CH3 Part C Part D
> 1. Spell out the full name of the compound 2. Spell out the full name of the compound. 3. Spell out the full name of the compound. 4. Spell out the full name of the compound. %3D
> Predict the relative bond angles in CCl4 and H2O a. CCl4 bond angles > H2O bond angle b. H2O bond angle > CCl4 bond angles c. CCl4 bond angles = H2O bond angle d. Relative bond angles cannot be predicted.
> Spell out the full name of the compound. Part A CH3 CH3CHNH2 Br (ag) CH3 Part B - NH3* cr (aq) Spell out the full name of the compound. Part C Cr(ag) Spell out the full name of the compound. Part D -NH2
> Part A Ba(ClO)2 Spell out the full name of the compound. Part B NH4Br Spell out the full name of the compound. Part C NaBrO-4 Spell out the full name of the compound. Part D FePO-4 Spell out the full name of the compound. Part E CoPO-4 Spell out the
> Determine the products formed in each reaction. If there is no reaction, label the reaction as "no reaction". (1] LDA [2] CH3CHJ Nal no reaction [1) LDA (2) CH3CH3l [1] NAOE! OEt [2] CH3CH, (3] H30*
> Determine the products formed in each reaction. .CI HC=C А. H3C H. Oc=CCH2CH3 B. (CH3CH2)3CCI CI HC=c© с. H D
> Draw the neutral organic products. HO
> 3D sketch Total # valence electrons BEST Lewis structure (If there is resonance, use F.C. todetermine which is best and only draw BEST Lewis structure Total BEST Lewis structure oheiscance FC.e determine which is bet, and oly draw BEST Levis Electron
