Concept explainers
a)
Interpretation: EN difference for each polar bond is to be determined.
Concept introduction: Atom is said to be electronegative if it has a tendency to attract electrons towards itself in a bond. Higher the electronegativity of element more will be attraction of electrons and vice-versa.
b)
Interpretation: Dipole moment arrow for each polar bond should be drawn.
Concept introduction: Dipole moment is a measure of bond polarity in the 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. Dipole moment arrow is directed from element of low electronegativity to element of high electronegativity.
c)
Interpretation: Partial positive and partial negative charges on molecules should be determined.
Concept introduction: Atom is said to be electronegative if it has a tendency to attract electrons towards itself in a bond. Higher the electronegativity of element, more will be the attraction of electrons and vice-versa.
d)
Interpretation: Electron cloud for molecules in order to indicate areas of high and low electron density should be determined.
Concept introduction: Atom is said to be electronegative if it has a 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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Organic Chemistry: A Guided Inquiry
- . Answer the following questions about compound A. [2] [1] A Label the shortest C- C single bond. Explain b. Label the longest C – C single bond. Explain c. Considering all the bonds, label the shortest C – C bond. Explain. d. Label the weakest C – C bond. Explain. e. Label the strongest C - H bond. f. Explain why bond [1] and bond [2] are different in length, even though they are both C– C single а. lain. bonds.arrow_forwardIdentify the molecular and electron geometries around each carbon (left and right). S: H H:C : C:H .. H Left Carbon Right Carbon Mol. Geo.: Mol. Geo.: Electron Geo. Electron Geo: 5.] Use electronegativity values to identify whether the following molecules are polar or nonpolar (explain why?). Indicate the polarity of each bond (towards, or from the central atom) using arrows. The molecular geometry is given in parentheses. (2 points) CH2B12 (tetrahedral geometry with C in the center) Br becavse H- Br Home Seos (trigonal planar with Se in the center) 11 4.arrow_forward1. 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.arrow_forward
- Complete Table 3 (Remember that the values pertain to the Central atoms only. In this table, you will have more than one central atom so report more than one value, ie. 3 / 3) Table 3 Molecules with Multiple Central Atoms Molecule C2H4 H2O2. CH3OH. CH3NH2 Number of Bond Pairs / / / / Number of Lone Pairs / / / / Number of Electron Domains / / / / Molecular Geometry (Shape) / / / / Bond Angle / / / / Polar or Non-Polar Nonpolar Polar Polar Polararrow_forward1. The electron pair in a H - Cl bond could be considered... a. closer to H because Hydrogen has a larger radius and thus exerts greater control over the shared electron pair b. closer to Cl because Chlorine has a higher electronegativity than Hydrogen c. closer to H because Hydrogen has a lower electronegativity than Chlorine d. an inadequate model since the bond is ionic 2. It is important to know the geometry of a molecule because the geometry _______. a. will give the Lewis structure of the molecule b. affects the physical and chemical properties of the substance c. will determine whether the molecule is ionic or covalent d. Both B, and Carrow_forwardor ion: 1. Draw the complete Lewis structure of the molecule or ion. 2. Determine the total number of electron groups (clouds) surrounding the central atom. 3. Determine the electron geometry of the groups around the central atom (linear, trigonal planar, etc.) 4. Determine the molecular shape of the molecule (linear, bent, trigonal planar, etc.) 5. Determine the molecular polarity (polar vs, nonpolar) 6. SCN-, thiocyanate ion (carbon central atom) Lewis structure Total number of electron groups around the central atom Electron geometry Molecular shape Molecular polarityarrow_forward
- A. CHF i. Best Lewis Structure B. HNO (H is connected to one of the O's) i. Best Lewis Structure ii. Electron geometry on the C atom ii. Electron geometry on the N atom iii. Approximate bond angles about the C atom iii. Approximate bond angles around the N atom v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the C atom. v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the N atom. vi. Is the molecule polar or nonpolar? vi. Is the molecule polar or nonpolar?arrow_forwarda.)Draw a Lewis diagram for POBr3 in which all atoms have a formal charge of zero . b.)Draw a Lewis structure for POBr3 in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms. c.)Based on formal charge, which is the best Lewis structure for the molecule?octet rule satisfied for all atoms or smallest formal chargearrow_forward4. Polarity: Circle the molecules that are polar and draw the delta notation around the polar bonds within the molecules that are polar. H3C CH3 H H H- H H. H H H- -H- H- H. H H H H. о N EN H- H. H.arrow_forward
- Q/ For the Lewis structure below…• Draw all of its important resonance structures. Show all charges and lone pair electrons. Use curved arrows to show the flow of electrons leading to each successive structure.• Draw the resonance hybrid. Label the average bond order and average chargesarrow_forwardb. Write the structure showing lone pairs of electrons and draw all possible resonance structures for Use curved arrows to track the movement of electron pairs converting one resonance contributor to the other.: c. Write the structure showing lone pairs of electrons for the molecule below and draw all . Use curved arrows to track the possible resonance structures for anionic species movement of a pair of electrons.arrow_forwardQuestion 48 48. Which of the following statements are true? 1. 11. III. IV. The electrons in each molecule tend to orient themselves around the most electronegative element. Each molecular drawing follows the localized electron model. Both HF and CO₂ are linear molecules and therefore polar. The bond angles of NH3 are slightly less than 109.5° because the lone pair compresses the angles between the bonding pairs. a. I, III, IV b. I, II, IV c. I, II, III d. II, IV e. All of the above statements are correct. C B esc E Q @ 2 W # 3 E $ 4 * R % 5 T < 6 Y & 7 8 Uarrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning