Question: Place the best reagent in the bin

> 1. An object will sink in a liquid if the density of the object is greater than that of the liquid. The mass of a sphere is 4.69 g. What should be the volume of this sphere for it to sink in liquid mercury (density = 13.6 g/cm3)? a. equal to 0.345 cm3

> a. Write the lewis structure for XeF4 b. Write the VSEPR formula for XeF4 c. Sketch the 3 dimensional structure d. What is the approximate F-Xe-F bond angles in XeF4

> Write the electron-dot (lewis) structure for CO32-, XeF4.

> Draw the lewis structure for XeF4 [SeF5]- [PCl4]+

> What is the Lewis structure for: SeF6 XeF4 SeCl3+

> Polarity y/n Lewis Structure Geometry Molecule PCl5, NH3, XeF4, C2H4. Polarity Molecule Lewis Structure Geometry (y/n) PCIs NH) XeFa

> Based on the correct Lewis structure for XeF4, how many bonding electron PAIRS around the central atom? Based on the correct Lewis structure for XeF4, how many nonbonding electron PAIRS around the central atom?

> Without drawing the Lewis structures, predict which of the molecules below will have an expanded octet. SF6, XeF4, PO43−. Without drawing the Lewis structures, predict which of the molecules below will have an expanded octet. SF6, XeF4, PO43− XeF4

> Predict the product for the following reaction: + H-CI

> Of Molecular Valence Formula Electrons CH4 SF4 34 PO13 IC14 ICI3 xef4 Lewis Structure Molecular VSEPR e Pair Geometry Geometry Tetrahedral Tetrahedral AX4 Trigonal See-saw AX4E bipyramidal Shape 109.5° 20 Bond Molecular Angle Polarity 109 non-polar Axial

> PBr5, SCl4, XeF4 Lewis Structure, 3-D Sketch, Are There Resonance Structures: SN: Valence e-: Electron Count: Bond Angle: # Bonding e- groups, # Non-bonding e- groups: Polar or Non-Polar Molecule: Hybridization of Central Atom: Formal Charges: Electron G

> Molecule or Ion (3D Structure) *XeF4 Lewis Structure 6. Bonding domains: Molecule or Ion (3D Structure) 6. *XeF4 Lewis Structure Bonding domains: Non-bonding domains: VSEPR formula: Geometric Shape: Polar or non -polar: 7. *ASFS Bonding domains: Non-

> Write abbreviated (condensed) configurations (noble gas core) for the following: 41) Write abbreviated (condensed) confivurations (noble gas core) for the following: +z!N 9 42 and 43. XeF4 Lewis structure (Resonance structures?) Total # of valence el

> Molecule Valence e Lewis Structure Molecular Shape Formal Charge Molecule Valence Lewis Molecular Formal Polar Resonance Structure Shape Charge Molecule? e- SF4 XEF4 CIF3 BRF5 PF5 SF6 ХeF2

> Write the lewis dot structure, bond angle and geometry for: NH3, H2O, H2O2, CH3OH, CH3CH2OH, CH3OCH3, PCl3, PCl5, XeF4, NO2

> Draw an appropriate Lewis structure for the following molecules and attempt to predict their shape: H2S, CH4, XeF4

> Which of the following compounds is antiaromatic? nds. 81 6T a. c. N. H N' +) b. d. IZ: IZ:

> Lewis Structure, Molecular Polarity and Hybridization Review 1. Complete the following table. Electron Geometry Hybridization of Central Polar? Y/N Molecular Lewis Dot Structure and Name Geometry Atom SICI. so, Tef4 BeCla Cl. XeF.

> The following molecules/ions are exceptions to the octet rule. Draw the best Lewis structure possible. Use formal charges to help you. Formula Lewis Structure so, PO, CIO; Xef4 BF3 LEGO

> All the structures should obey the Pauling Electroneutrality Principal. (Hint: This should result in a formal charge of zero for the central atoms of the structures below if they are drawn correctly.) 1. OF2 2. SO3 3. SF4 4. GaI3 5. XeF2 6. AsBr5 7. CS2

> Formula Name of structure Lewis Structure and Resonance Structures Formula Name of structure Lewis Structure and Resonance Structures H:0 water COH2 formaldehyde CHCI trichloromethane PH3

> a. Draw the Lewis structures for these species. If more than one Lewis structure is possible, draw the structure with the formal charges minimized. Show all valence electrons in your structures. XeO2 XeF. PFs IFs 大 (b) Based on your structures f

> Molecule Number of valence electrons Bond skeleton Remaining electrons Lewis structures with formal charges structures? Number of valence electrons Remaining electrons Lewis structures with formal charges Resonance structures? How many? Molecule Bon

> Lewis structure; label any non-zero hybridization of the central # σ species atom Lewis structure; label any non-zero formal charges on each structure hybridization of the central species atom SF. CIF, IFs BiCl, |XeF; XeF, TeF.

> Substance Electrons # of Valence Electrons Lewis Structure # Zones Geometry e- Pair Geometry # of Valence Electrons e- Pair Geometry Substance Lewis Structure # Zones Geometry XEF4 C,H4 C,H2 CH¿Cl2 CH,Cl2 C,H¿Cl2

> Which of the following Lewis structures is best depicted using resonance forms? XeF4 NO Cl2 NO2− SnH4

> In each reaction box, place the best reagent and conditions from the list below. (Some reagents may be used more than once.) a. b. You have formed the correct bromohydrin in step 4, but NaOH is not the best reagent to use for the internal Sy2 reacti

> In each reaction box, place the best reagent and conditions from the list below. 1) 2) он 3) HO. 4) CH30 H3O* BH/THF NaBH4 CH3CO0 NaOH TSCI, pyridine H2SO4 (conc.) H2O2, NaOH, H2O (CH3)3CO-

> In each reaction box, place the best reagent and conditions from the list below. 1) Br но 2) 3) 4) CH3CH2OH, H3O" (cat.) HOCH2CH2OH, H3O* (cat.) CH3CHO, H3O° (cat.) CH3MGB. LIAIH4 H2CrO4 2-propanol KMNO4 Mg, ether t-butanol acetone H30* NaBH4 NaOH 1

> In each reaction box, place the best reagent and conditions from the list below. 1) Br 2) HO 3) 4) CH3CH2OH, H30' (cat.) HOCH2CH2OH, H3O' (cat.) CH3CHO, H3O° (cat.) CH;MgBr LIAIH4 H2CrO4 2-propanol KMNO4 Мg, ether t-butanol acetone H3o* NABH4 NaOH N

> Nitrite lon, NO2 Lewis Structure 3-D Molecular Structure Number of Valence Electrons Nitrite lon, NO, Lewis Structure 3-D Molecular Structure Number of Valence Electrons Steric Number of Central Atom Electron Group Geometry Molecular Geometry Bond An

> 1. Show how to carry out the following transformation in the highest yield possible. Select the appropriate reagents and draw the correct organic product at each step. 2. In each reaction box, place the best reagent and conditions from the list below.

> Draw the Lewis Structure for each molecule. Remember that the best structure will have as few Formal Charges as possible. Molecules which break the octet rule are denoted with *. Formula Lewis Structure Formula Lewis Stracture NH-CI CH,CI HCIO HBr CH

> Select the best conditions for the reactions. (a) CH;OH CH3 CH3 NaOCH, CH,Oн CH3 н", NaOCH, CH;Oн H3C H3C Incorrect. NaOCH3, DMSO SN2 substitution requires a strong nucleophile. H* would convert methoxide to methanol, so methoxide would be deactivat

> Which of the following Lewis structures is best depicted with an incomplete octet? 1. Cl2 2. XeF4 3. NO2− 4. SnH4 5. AlBr3

> Find all lewis structures 1. PH2F2-1 2. AsCl5-2 3. BrCl4-1 4. XeF4+2 5. ICl3

> Draw the Lewis structure for the polyatomic hydroperoxyl (HO2-) anion. Be sure to include all resonance structures that satisfy the octet rule. .. H-0-C H-0 -0-H ..

> Draw the products of the following reactions. H* + H20 +1 equiv. OH→

> Draw the organic product of the following reaction. 1.NABD, 2.H,O*

> a. Write the Lewis dot structure for XeF4 b. Write the VSEPR formula for XeF4 c. Sketch (or describe) the three-dimensional structure (or geometric shape) of XeF4. d. What are the approximate F-Xe-F bond angles in XeF4?

> Compound Lewis Structure Shape, Bond Angle and Polarity 3D Structure BeCl3 BСl3 SO2 CH4 NH3 HO Shape, Bond Angle and Polarity Compound 3D Structure Lewis Structure PCl5 SF4 BrF3 XeF2 SF6 BrF5 XeF4

> Give the IUPAC name for the following compound:

> Draw the Lewis Dot structures of each of the following molecules: a. SF6 b. BF3 c. XeF4

> Predict the oxidation product of treating the given alkene with peroxyacid reagent. Omit by-products.

> Classify these molecules as polar or nonpolar. Drag each item to the appropriate bin. H,O H CH, BCI, HF CH,CI Polar Nonpolar

> [NO2]- lewis structure: complete with formal charges, show all resonance structures. a. electronic geometry b. molecular geometry c. bond angle d. on your lewis structure, indicate any polar covalent bonds and the overall molecular polarity. e. demostrat

> In each reaction box, place the best reagent and conditions from the list below. CH3 1) 2) 3) BHyTHF Ha, Lindiar catalyst bromocyclohexane H,O2. NHOH, H,0 Hy0, H,SO. ехсess NaNH SOC CH,CH;Br CH,Br HBr Bra

> Draw Lewis structure for the following molecules a. CO2 b. PCI3 c. XeF4 d. SO3

> Triatomic Molecules and Ions of the drawings shown below, select all and only those which are acceptable Lewis diagrams for the species indicated. [:ö–s–ö:]2- Lewis structure of SO,2-? Lewis structure of So,2-? EN-N- -N Lewis structure of N3"? Lewis

> Does NO2+ lewis structure diagram have a bracket outside it with a + charge?

> Draw the Lewis structure and VB-MO hybrid diagram for Nitrite (NO2-). 4. Nitrite, NO; Lewis structure: VB-MO hybrid diagram: SN: EGA: Shape:

> a. Draw the main Lewis structure of NOF. Draw nonbonding electrons using the dot notation and bonding electrons as a bond. b. Determine the number of bonding electrons and the number of nonbonding electrons in the structure of BeF2. Ureset ? help

> Using a Lewis structure, the VSEPR model and the valence bond model, determine the electron pair geometry and molecular geometry of each of the following molecule. Identify the hybrid orbitals of each atom, and identify the atomic orbitals (including hyb

> Given the following molecules: CO2 and SO2, draw Lewis structure and indicate formal charge of every atom. Justify molecular geometry attending to VSEPR theory and the hybridization of every atom according to Valence Bond theory. In addition, indicate:

> Draw the Lewis structures with formal charges. Identify the electron pair arrangement, bond angle and molecular geometry for the compounds listed below. a) SO Lewis Structure: Electron Pair Arrangement: Bond Angle: Molecular Geometry: b) NO, Lewis St

> Complete the following table. Consider the central atom when determining e- geometries. Be sure to include all equivalent resonance structures of the molecules if applicable. SF. CO Compound Lewis structure e group geometry Molecular shape Bond angle

> Draw the Lewis structure for the following species, sketch their VSEPR, determine molecular geometry, and the polarity of each molecule. A BCI, Polarity Molecular shape Lewis Structure VSEPR Sketch B. SO2 ong Lewis Structure VSEPR Sketch Polarity Mol

> Triatomic Molecules and Ions of the drawings shown below, select all and only those which are acceptable Lewis diagrams for the species indicated. Lewis structure of SO2? Lewis structure of ClO2−? Lewis structure of NO2−? Lewis structure of N3−? Lewis st

> Draw the Lewis structures for CO2, and CO, and predict the number of and bonds for each molecule. (Assign lone pairs and radical electrons where appropriate).

> Triatomic Molecules and Ions of the drawings shown below, select all and only those which are acceptable Lewis diagrams for the species indicated. NEN-ö: Lewis structure of Ny0? CN=N=N} Lewis structure of Ny ? :ö-c-ö: Lewis structure of CO,? Lo=ä=0}

> After drawing the Lewis structures of CO2 and SO2, compare and contrast the structures AND provide an explanation as to why the molecules are the same or different (include at least two points for each category). Lewis structure of CO2 Lewis structur

> Triatomic Molecules and Ions of the drawings shown below, select all and only those which are acceptable Lewis diagrams for the species indicated. 0=c=0: Lewis structure or co,? O L0=či=0 Lewis structure of cio,? :NEN-O: Lewis structure of N20? O [N=

> Draw the neutral organic starting material. click to edit Br, CH,CI, Br

> For each molecule/ion identified, draw its Lewis structure(s), identify its molecular geometry, and identify whether the molecule is polar or nonpolar. Clo; MOLECULAR GEOMETRY (NAME) LEWIS STRUCTURE(S) POLAR NONPOLAR PClg LEWIS STRUCTURE(S) POLAR NON

> Write the Lewis structures of the following molecules/ions. CO2 CCI4 H20 CHCl3 NO3 PCl3

> In each reaction box, place the best reagent and conditions from the list below. 1) Br 2) 3) 4) DEET (the active ingredient in over the counter insect 5) repellant) HN(CH;CH3)2 (1 equiv.) HCOOH CH;CH;NH2 HCOOCH3 NH(CH,CH)2. (2 equiv.) CH,COOH Mg, eth

> In each reaction box, place the best reagent and condition from the list below. 2) он 3) H0, H2SO4 (cat.) CH,COO NANH2 (excess) H2, Pt Br2 H2. Lindlar's catalyst BHYTHF PBrs H2O2, NaOH, H2o CH,CH,OH

> Draw the Lewis structure for the polyatomic hydroperoxyl (HO2-). Be sure to include all resonance structures that satisfy the octet rule. ?

> Lewis structure for C2H4O2.

> Christmas and Thanksgiving, two beloved traditional holidays, share many similarities concerning the gifts and memories they provide to thousands every year, and yet starkly contrast one another in their worldwide appreciation. Both holidays represent th

> Is CH4 Polar, lonic or Nonpolar and List and Explain whether it is Soluble or Insoluble in Water?

> Determine whether each molecule is polar or nonpolar. Br: nonpolar HI: polar ICI: polar CH4: nonpolar CH;CI;: [ Select] HOCI: [ Select] NH3: ( Select ] H;O2: ( Select] N,Hạ: Select NH,OH: [Solect]

> Give the shape of CH4 and whether it is polar or nonpolar.

> Identify the following compounds as polar covalent, nonpolar covalent, or ionic H2O CO2 NaI NH3 CH4 A. polar covalent B. nonpolar covalent C. ionic

> Classify each of the molecules given below as polar or nonpolar. SF NH, CIF: XeFa SF PFs BrCls XeF. H20 CS: So, co, CH. Polar Nonpolar

> Complete the following table for XeF4. Activity 1 Lewis Dot Structures Chemical Formula Dot Diagrams Electrons Central Atom Lewis Structure

> Determine whether each molecule is polar or nonpolar. HI CH4 H202 Br2 1. polar NH2OH 2 nonpolar HOCI ICI CH-Cl2 NH3

> 14. Draw Lewis dot structures for the following. Be sure to show all valence electrons as dots or lines a. CF4 b. N2H4 c. OCl2 d. CaCl2 15. Draw the Lewis structure for CH4. What is the electron group/parent structure geometry? What is the molecul

> A. Is CSe2 polar or nonpolar? B. Is CH4 polar or nonpolar? C. Is BrCl3 polar or nonpolar?

> Review VSEPR as needed and determine the molecular geometry of each of the following. Review symmetry elements and determine if each has a mirror plane (σ) (which type), rotation axis (Cn), multiple rotation axes, inversion (i) and use the point group ch

> Describe all the main features of the following theories and explain what useful information we gain from them. How do the theories help describe molecules/ions? What are the pros and cons of the theories? Use a list or chart. a. Lewis Structures b. Va

> Use the data given here to calculate the values of ΔGorxn at 25oC for the reaction described by the equation If ΔHorxn and ΔSorxn are both posi

> Draw the lewis structure with any resonance structures, formal charge calculation, VSEPR: electron geometry and bond angle about, molecular geometry and bond angle about atom same or different than VSEPR? PLEASE BE LEGIBLE AND SHOW ALL WORK! DUE: Fer

> 1. What is the main idea behind VSEPR theory? 2. For each of the following compounds, determine the molecular shapes and bond angles for the central atom. Draw the Lewis dot formula to begin with and use the VESPR Molecular Shape Chart to help you. Is t

> Predicting and Drawing Shapes of Molecules Complete the following chart: Molecular Lewis diagram Name of VSEPR shape Dipole yes/no Formula SeFs SiF. NF3 ÇINO H;S NHạ+ HCN NO,

> For the following molecules, make a chart and fill in the information for the following: How hybridization Compound formula Lewis Structure- VSEPR Drawing Molecular Geometry Electron show all Domain occurred resonance Geometry structures, show formal

> a. What is the formula for ammonium acetate? b. What is the formula for ammonium? c. What is the formula for ammonium chloride?

> 4. What are lone pairs in the VSEPR theory? 5. To determine the shape of a molecule using a VSEPR theory chart, what two things do you need to know. 6. Draw the Lewis dot structure (on back) and complete the table for the following compounds. shape

> Fill in the blank spaces in the following chart. Molecule Lewis structure Electron Bond Molecular domain Angles geometry geometry (shape) (VSEPR) XeF2 -Xe, HH BeHz 180° H-BeH F F-As: ASF5 'F F

> Molecule VSEPR shape Bond angle Polar, non-polar, lon Molecule VSEPR shape Bond angle Polar, non-polar, ion SO32 SO3 SO2 CO2 NO: ВеBrz SCl2 BF3 clo H30

> For this discussion, find a covalently bonded molecule that has a particular shape. Post the following information: Name of the molecule Chemical Formula Empirical Formula Embed an image of the structure Shape of the molecule around the central atom,

> 44. This is the strongest type of covalent bond. a. Ionic b. Hydrogen c. Diatomic d. Dispersion e. Polar 45. This type of solution conducts electricity. a. Electrolyte b. Nonelectrolyte c. Saturated d. Unsaturated e. Supersaturated 46. What is

> For the covalent bonded molecule Oxygen please provide the following information: - Chemical Formula - Empirical Formula - Embed an image of the structure -Shape of the molecule around the central atom, or choose an atom to demonstrate the shape -Use the

> Given that, Calculate the value of ΔH°rxn for H,(e) + F,lg) → 2HF(g) AH=- 546.6 kJ • mol rxn 2H,(2) + 0,le) → 2H,0() AH= - 571.6 kJ· mol :- 571.6 kJ · mol 2F,(g) + 2H,0() → 4HF{g)+0,(g)

> How many σ and π bonds are in this molecule?

> What is the bond angle of dsp³ and what is the bond angle of d²sp³?

> Draw the best Lewis Structure for each of the following structures. Determine the electron and molecular geometries for each using the VSEPR chart. 1. CH4 2. H2O 3. NH3 15. O3

> Record the name, formula and pH of each salt solution. If the pH is not neutral, for the ions that undergo hydrolysis, write down the hydrolysis reaction and indicate which species is responsible for the observed pH. pH of sodium chloride 7.07 pH of a

> Fill in the following chart: Molecular Formula Lewis Structure # of Hybrid- Molecular Electronic |Geometry Geometry Molecular Вond Lewis Structure Electron Formula ization Angle(s) Groups CH.CI: OPCI, (violate the octet rule) CH:O NO: PCIS (violate

> Complete the following chart of electronic and molecular structure. # Electron Domains Molecular Geometry Electron Lewis Diagram # Lone Pairs Geometry H:N:H .. H:C:H H H:0:H