Question: Spell out the full name of the

> 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

> 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 a

> 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. K​a​ = 1.3x10-2 b. Find the pH of a 2.9M solution of KHSO​4​(HSO​​​4-, K​a =​ 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

> 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

> Draw the neutral organic products. Br он H,0

> Draw the neutral organic product containing the most carbon atoms. Draw the neutral organic product containing the least carbon atoms. Draw the neutral organic product containing the most carbon atoms. Draw the neutral organic product containing the

> Analyze the steric number, hybridization, electron group geometry and the molecular geometry for the following molecules: BeH2 CO2

> Predict the relative bond angles in BF3 and SO2. a. BF3 bond angles &gt; SO 2 bond angle b. SO2 bond angle &gt; BF3 bond angles c. BF3 bond angles = SO2 bond angle d. Relative bond angles cannot be predicted. The shape and bond angles of a molec

> CO2 Structure: Magic Number on Central Atom Electronic Geometry Molecular Geometry Bond Angle on Central Atom Hybridization of Central Atom CO2 Structure: Magic Number on Central Atom Electronic Geometry Molecular Geometry Bond Angle on Central Atom

> Write Lewis dot structures for each of the molecules listed. be sure to indicate all pairs bonding and non-bonding electrons. predict the electronic and Molecular geometry of each of the molecules for which you have drawn Lewis structures. Molecule L

> Draw the Lewis structure, electron domain geometry and molecular geometry and predict the polarity for NH3, CO2 and XeF4?

> Give the electron pair geometry and the molecular geometry of three species for CO2 and SO2 according to VSEPR.

> Electron Pair Geometry Molecular Geometry Polar or Type Lewis Structure Molecule Electron Count Nonpolar Molecule Electron Count Lewis Structure ABU Electron Pair Geometry Molecular Geometry Polar or Туре Nonpolar CO: NO SO, NO:

> Give the: "Lewis Structure" "Electronic Geometry" "Molecular Geometry" "Bond Angle" "Polar/Non Polar" of: CO2 NH3 BF3 H2O PF3

> Nitric acid, HNO2 is a weak acid with Ka= 4.5 x 10-4. It dissociates according to: HNO2 (aq) H+ (aq) + NO2- (aq) a. What is the pH of a buffer solution which is 0.80 M in NO2- and 0.40 M in HNO2? b. What will be the pH of the resulting solution when 2.0

> Indicate the electron pair geometry and the molecular geometry for each compound. Trigonal Pryamid linear tetrahedral bent trigonal planar Compound Electron Pair Geometry Molecular Geometry CO2 BF3 SO2 CH4 SOCl2 SCl2

> valence e-domains on central atom Electronic Geometry Molecular Geometry Bond Angles (approx) Polar or Nonpolar Molecule 3. H;S # of valence e domains on central atom Electronic Geometry Molecular Geometry Bond Angles (approx). Polar or Nonpolar Mole

> Molecular formula Lewis Structure Electron-pair geometry Hybridization of central atom Molecular geometry Dipole moment Hybridization of central atom Molecular Lewis Structure Electron-pair geometry Molecular Dipole formula geometry moment H2O2 H2S C

> Molecular Models Formula Name Lewis Structure Electron Geometry Molecular Geometry and 3-D Drawing Formula Name Lewis Electron Molecular Geometry Structure Geometry and 3-D Drawing H20 O2 NH3 CO2 N2O4 *

> State the hybridization and the molecular geometry of each designated atom: hybridization molecular geometry a) CO2 b) N, Niddle c) POCI, d) ICI, I.

> Molecular Formula CO2 NH3 BrFs (violate the octet rule) SF (violate the octet rule) of Lewis Structure Electron Groups # of Molecular Electronic Geometry | Geometry Angle(s) Molecular Hybrid- ization Bond Lewis Structure Electron Formula Groups CO2 N

> Molecular Geometry Molecule Valence e Lewis Structure Electron Geometry CO2 CH4 SF6 XeCl4 Valence e Molecular Geometry Molecule Lewis Structure Electron Geometry CO2 CH4 SF6 XeCla IF Electron Geometry Molecule Valence e Lewis Structure Molecular

> Formula Molecular Geometry Lewis Structure Electron Hybridization Geometry Polarity Molecular Geometry Molecular Geometry Electron Hybridization Molecular Polarity Formula Lewis Structure Geometry Geometry CO BFa SO, Page 1 of S Molecular Polarit

> Molecular formula Lewis structure Electron- group geometry Bond angle Molecular geometry Sketch molecular geometry Hybridization Polar or nonpolar? Electron- Sketeh Molecular formula Lewis structure Bond Molecular molecular Polar or group angle geome

> Molecular Geometry Data Table Molecular Hybridization Polarity (Polar of the central Total Electron Molecular Bond Molecule number of Lewis Structure or ion Total number of Valence Hybridization Electron Domain Geometry Molecular Polarity (Polar of t

> Methanol, CH3OH, is a non-electrolyte; oxalic acid, H2C2O4, is a weak electrolyte; and sodium chloride, NaCl, is a strong electrolyte. Give the moles of solute particles formed by each if 0.1 mol of each compound is dissolved in water. Write equations to

> Draw Lewis structure, electron domain geometry, and molecular geometry for the following compounds: CO2 H2O NH3

> What is the electron pair geometry of CO2? What is the molecular geometry?

> CCl4 NH3 H20 CO2 PO43- PC15 Lewis Structure Electron Geometry Molecular Geometry NH CO2 PO, PCI, Lewis Structure Electron Geometry Molecular Geometry

> Determine the electron geometry (eg) and molecular geometry(mg) of BCl3, SiF4, CO2, PF5 and SF6.

> The octet rule only applies to: a. atoms with 8 electrons. b. some elements in row 2 of the periodic table. c. All elements in row 2 of the periodic table. d. Metals on the periodic table.

> Which of the following statements about electronegativity and the periodic table is true? A. Electronegativity decreases across a row of the periodic table B. Electronegativity increases down a column of the periodic table C. Electronegativity increas

> 7. Draw the Lewis structure for XeI2 8. Draw the Lewis structure for ICl5 9. Draw the Lewis structure for BF3 10. Draw the Lewis structure for NO3. 11. Determine the electron geometry (eg) and molecular geometry(mg) of BCls. 12. Determine the electr

> Give the conjugate acid for each compound below. Base Conjugate Acid HSO, co3 NH,

> NO₂ lewis structure: Electron Geometry: Molecular Geometry: NO Lewis structure: Electron Geometry molecular Geometry: O3 Lewis structure: Electron Geometry: Molecular Geometry:

> Hybridization Worksheet 1 lb (Gen Chem) VSEPR Valence Bond Theory Carbon's orbital diagram C valence shell Hybridized orbital diagram Carbon dioxide C02 Valence Bond Theory VSEPR Hybridized orbital diagram Cvalence shell Carbon's orbital diagram Cart

> Name the following compounds: 1. m-Diethylbenzene 2. 1,3,4-trichlorobenzene 3. 5-bromo-2-chlorophenol

> Lewis structure and perspective drawing for TeCl6.

> Lewis Dot Structures, Hybridization, and Shapes of Molecules and Ions Number Resonance Hybridization Electronic Molecular lon or Compound of Is the Geometry Geometry Compound Number Lewis Dot of e^- Structure Valence Structure around (If any. Polar?

> ICl2− Draw the Lewis structure for the ion. Show the formal charges of all atoms in the correct structure. Include all lone pairs of electrons. If resonance structures are needed to describe the Lewis structure, draw all possible resonance structures.

> When drawing lewis structure's how do we know whether the shape should be a tetrahedral or a square planar? For example in questions where we have to draw the lewis structure for XEBr4 or XeF4?

> Draw the best Lewis structure of the following. Show all lone pair e- and the formal charge on each atom if not zero. a. PO43- b. XeF4

> Draw Lewis dot structures for each of the following exceptions to the octet rule. a. SbCl52- b. XeF4 c. CIF3 d. BCl3 e. PCl5 Draw all possible resonance structures for each of the following, assign formal charges to each atom, and determine which i

> For the following GeH2, SrH2, SiF4, XeF4, H2CS, IF5 Lewis Structure Electron geometry Molecular geometry Polar - Yes / No 3D shape / Molecular shape drawing

> Which of the following Lewis structures is best depicted as an expanded octet, also known as an expanded valence shell? Cl2 XeF4 AlBr3 NO2− SnH4

> Geometry, PI and Sigma bonds Complete the following table: BO, H;CO, XeF4 SC Lewis Structure Molecular Geometry Hybridization of Central Atom Bond Angle of Central Atom Number of a bonds Number of R bonds

> The Lewis dot structure for each molecule, electron domain of the molecule, VSEPR geometry of each molecule. Molecule Lewis Dot Structure Electron Domain VSEPR Geometry Molecular Shape Bond angle Polar co, PFS PCI H,0 AsCl, SeF4 Xef4 03 C,H,CI, Sira