Chapter 5 Concept Checks

Answer question 5 please

Which statement A-D about VSEPR theory is not correct? Select one: a. The molecular shape or geometry can differ from the electron-pair geometry. b. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion. c. The steric number of a central atom is the sum of the number of bonded atoms and lone pairs around the central atom. d. The steric number has five values from 2 to 6. e. Statements A-D are all correct. Clear my choice

:O: HICIH bent QUESTION 18 What is the geometry relative to the C atom on the left in the Lewis structure below? O: -C- H- H. linear trigonal planar tetrahedral trigonal pyramid bent QUESTION 19 What is the geometry relative to the C atom on the right in the Lewis structure below? H O H. linear O trigonal planar tetrahedral Click Save and Submit to save and submit. Click Save All Answers to save all answers. Mac

Is this a reasonable structure? If not, why not? proposed Lewis molecule structure Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. OF, :F F: The correct number is:|| - No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: Yes, it's a reasonable structure. :F: No, the total number of valence electrons is wrong. BF3 The correct number is: :F В F: No, some atoms have the wrong number of electrons around them. - .. The symbols of the problem atoms are: Yes, it's a reasonable structure. :F: No, the total number of valence electrons is wrong. CIF3 | The correct number is: | :F СІ — F: No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: * 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…

-1 5. NO₂¹ Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No Polar 6. H30¹¹ – use a yellow ball for oxygen (not red) when constructing this model Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Any polar bonds in the molecule? Yes No Molecular Polarity: Polar 7. CHBr3 Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No 8. OF₂ Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar Bond Angles Non-Polar Bond Angles Non-Polar Page 2 of 4 9. CO3-² Total # of…

Which statement A-D about VSEPR theory is not correct? Select one: a. The steric number has five values from 2 to 6. b. Statements A-D are all correct. c. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion. d. The steric number of a central atom is the sum of the number of bonds and lone pairs around the atom. e. The molecular shape or geometry can differ from the electron-pair geometry.

1. Determine whether the following hypothetical compounds are polar or nonpolar. Briefly explain how you can tell. a. A compound with a tetrahedral molecular geometry in which all four bonds are to four atoms of the same element. b. A compound with a tetrahedral molecular geometry in which two of the bonds are polar bonds to two fluorine atoms and two of the bonds are nonpolar bonds to two hydrogen atoms. c. A trigonal pyramidal compound that contains one polar bond. d. A trigonal pyramidal compound that contains only nonpolar bonds. e. A compound in which the central atom has two lone pairs and forms polar bonds to three fluorine atoms. f. A compound in which the central atom has three lone pairs and forms polar bonds to two fluorine atoms.

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Determine how many valence electrons belong in the keep a structure for the compound and draw a Lewis structure.

Purpose: To practice describing types of chemical bonds. One common analogy to describe chemical bonds is different levels of interpersonal relationships: 1) Hydrogen bonds are analogous to acquaintance 2) Ionic bonds are analogous to dating relationships 3) Covalent bonds are analogous to marriages Task: Briefly explain why each type of bond can be represented by each type of interpersonal relationship. Then come up with some analogies to describe hydrogen, ionic, and covalent bonds.

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Options: greater than, less than, same as, nitrogen atom, chlorine atom, less space than, more space than, and the same space as.

TASK 1: COMPLETE ME! Complete what is required at by the following table. Copy table in a separate sheet of раper. Polar Molecule or Nonpolar Molecule Bond Central AEN Type of Bond Atom 1. Sulfur difluoride SF2 2. Methane CH4 3. Охуgen O2 4. Ammonia NH3 5. Hydrogen sulfide H2S

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* Question Complètion Status: QUESTION 1 Consider the following molecule. Name the geometry for the atom indicated by the arrow. OH HO. HO O linear O trigonal planar O tetrahedral O trigonal pyramid O bent QUESTION 2 Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBol

Activity 3: Reasoning Challenge Directions: Answer the following questions in 2-3 sentences only. 1. VSEPR theory specifies "valence shell" electrons. Explain why these are the most critical electrons for determining molecular shape? 2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule bef identifying the shape of the molecule? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.

Draw the Lewis Dot structure for N2 (on paper, not on Canvas) then answer the questions. a. How many total valence electrons are in N2? Express your answer as a whole number. b. How many single bonds are in N2?  Express your answer as a whole number. c. How many double bonds are in N2?  Express your answer as a whole number. d. How many triple bonds are in N2?  Express your answer as a whole number.

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Report Sheet Date Name Section. Team Instructor Name. Molecular Models: Lewis Electron Dot Structures and Molecular Geometry Part A: Use the molecular model kit and complete the following table. Total Sketch of Name of the Molecule is Lewis Molecular number of three- polar or nonpolar? electron dot molecular formula valence dimensional structure geometry electrons geometry N2 NH3 H2S CO2 PF3 CH4 SO2 HCN H2CO

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5. NO₂-¹ Total # of Valence Electrons: Lewis Structure (show all resonance structures if applicable) 3-D Model Sketch Any polar bonds in the molecule? Yes No Molecular Shape: Molecular Polarity: Any polar bonds in the molecule? Yes No 6. H30*¹ — use a yellow ball for oxygen (not red) when constructing this model Total # of Valence Electrons: 3-D Model Sketch Lewis Structure (show all resonance structures if applicable) Molecular Shape: Molecular Polarity: Polar Polar Bond Angles Non-Polar Bond Angles Non-Polar

10) Re-draw the following molecules showing the full Lewis structure at the indicated location. .10. b) HCIO3 NO₂

4. Using table 3, predict the molecular geometry of the following molecules: a. The central atom bonded to four substituent atoms and had no lone pair b. The central atom bonded to three substituent atoms and having one lone pair. c. The central atom bonded to two substituent atoms and had one lone pair. d. The central atom bonded to two substituent atoms and had no lone pair.

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If a molecule requires two or more resonance structures to draw it, which of the following statements is true? Select one: A. The molecule does not have a single structure but dynamically oscillates between the resonance structures drawn for it. B. The molecule has lower energy than the computed energy of any of the resonance structures that are drawn for it. O C. The molecule is less stable than any of the resonance structures drawn for it. D. The molecule's resonance structures coexist in an equilibrium with the lower energy form predominating.

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b. Compare the experimental bond length data shown below with your Lewis Structure drawing. Describe any discrepancies that you notice between the two structures.

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Atom A has 4 valence electrons. Atom Z has 6 valence electrons.  For the AZ3-2 ion, answer the following questions about its Lewis dot structure (drawn according to Chm 130 guidelines).  a. How many valence electrons are in the structure? b. How many single bonds are in the structure? c. How many double bonds are in the structure? d. How many triple bonds are in the structure?                                  e. How many lone pairs are on the central atom in the structure?                                f. What is the shape of the structure?                                 g. What are the bond angles of this ion?