Concept explainers
a)
Interpretation: EN difference for
Concept introduction: Atom is said to be electronegative if it has tendency to attract electrons towards itself in a bond. Higher the electronegativity of element, more will be attraction of electrons and vice-versa. Dipole moment is a measure of bond polarity in molecule. It is defined as product of charge and distance of separation between opposite charges. Polar molecules consist of dipole moments due to presence of charges in them whereas non-polar molecules do not have dipole moments.
b)
Interpretation: Partial positive and partial negative charges to
Concept introduction: Atom is said to be electronegative if it has tendency to attract electrons towards itself in a bond. Higher the electronegativity of element more will be attraction of electrons and vice-versa.
c)
Interpretation: Difference between
Concept introduction: Atom is said to be electronegative if it has tendency to attract electrons towards itself in a bond. Higher the electronegativity of element, more will be attraction of electrons and vice-versa.
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Chapter 4 Solutions
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- A student draws the picture of ammonia (NH3) in the box below, left, and predicts it will be a flatmolecule with HNH bond angles of exactly 120°. Unfortunately, the student left something out. a. What did the student omit from his drawing? b. What is the actual HNH bond angle of ammonia (based on the draw g above, right)? c. Explain why water, ammonia, and methane (shown below) all have about the same bondangles (close to 109.5°) even though they have different numbers of bonds.arrow_forward3-31 Why does electronegativity generally increase going from left to right across a row of the Periodic Table?arrow_forwardGive typed full explanation Look at figure 3-22 that shows the electron density that occurs abound the Si-O bond. This electron density map gives the "shape" of the O and Si atoms when they are bonded together. Think about the answer in Q9 and choose the best response below: (Select answer choice) a. This figure shows that the Si and O atoms, when they bond together, do not form spheres, which is due to the fact that the Si-O bond is strongly covalent and these shared electrons affect atomic shape. This change in shape limits the applicability of Pauling's Coordination principle since that principle is based on the geometry of perfect spheres. b. This figure shows that the Si and O atoms, when they bond together are close to perfect spheres, which is due to the fact that the Si-O bond is strongly covalent. This figure shows that Pauling's Coordination principle should apply very precisely to any substance that contains Si-O bonds c. This figure shows that the Si and O atoms, form in a…arrow_forward
- 5. |- The molecule pictured below is acrylonitrile, the building block of the synthetic fiber Orlon. No explanations required H H H-c=C-c=N: a) Which is the longer carboncarbon bond? b) Which is the stronger carbonncarbon bond? c) Which is the most polar bond? Explain. Indicate the polarity of this bond by writing the partial charges and drawing its dipole moment.arrow_forwardFor the formula CH,CF2, *draw the Lewis structure in your work* (which I will grade when you upload it). 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 CH)? 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 sp3 would be typed as "sp3". Is the molecule overall polar…arrow_forwardetic cation; (e) 1.17 Identify the formal charge on each atom in the following species. Assume that all valence electrons are shown. H H-N H 7 H C-C H/ H H-C C=C C-C Z=1: H •F: -C Ö: :0:arrow_forward
- 10. Indicate if the bond is polar or nonpolar (in box). If non-polar write non-polar, If polar, show direction of dipole. (2pts) O-C H-CI C-C C-N 11. Determine if the following sets of molecules are identical molecules, different molecules, or isomers (if so, indicate what kind). (3pts) H Br H H F HTH CI CI H Br H. Br Br 17arrow_forwardResonance, hybridization, Lewis structures: Draw the lowest energy alternative resonance structure for acetamide Part A Draw the lowest energy alternative resonance structure for this compound. Interactive 3D display mode NN H₂C Draw the structure on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Advanced Template toolbars. The single bond is active by default. [1] A NH,₂ H 12D EXP.¹ CONT ● L Marvin JS by ChemAxon H C N O S CI Br I P Farrow_forwardtion 3 of 30 a) Which molecules have polar bonds? H. 1. CH, CH, CH; H,C CH, CH, Cl H.arrow_forward
- e) Which of the following using either the polar arrow or partial charges (δ+ & δ-) correctly represents the polarity of the Te⎯Se bond in TeSe3? (choose the correct letter from A – D) f) TeSe3 is a (choose either polar or nonpolar) molecule because (choose correct letter from A – E) A. its’ bond dipole moments reinforce each other to give a non-zero net dipole moment. B. it is a symmetrical molecule with a non-zero net dipole moment pointing toward S in the molecule. C. its’ bond dipole moments reinforce each other to give a net dipole moment equal to zero. D. it is an unsymmetrical molecule whose dipole moments cancel out each other to give a zero net dipole moment. E. it is a symmetrical molecule whose dipole moments cancel out each other to give a zero net dipole moment.arrow_forward2. 3-42. The gas boron trifluoride (BF3) has a trigonal planar configuration as shown in Fig. P3.42. The B-F bond length is 1.3 Angstrom. Adjacent fluoride molecules form a 120° angle. Find the distance between adjacent fluoride molecules. F F B 120° F Figure P3.42 Planar configuration of boron trifluoride.arrow_forward2. Consider the resonance structures below may only A C. yongary] B C D a. On each structure (A-D) show all lone pair electrons. b. Provide arrows that show electron movement from A to B, B to C, and C to D. Which is the "most contributing” resonance form (A, B, C, or D)? Explain your choice. d. Draw the resonance hybrid for this molecule (use “delta” 8+ or - to show partial charges).arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
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