Concept explainers
(a)
Interpretation:
The compound that has non-polar covalent bond has to be identified.
Concept Introduction:
Non-polar covalent bonds: A covalent bond between atoms with the same electronegativity.
Example:
The atoms share the bonding electrons in the above molecules equally; that is each electron spends as much time in the vicinity of one atom as in that of the other. Such a bond is called as non-polar covalent bond.
The greater the difference in electronegativity between the atoms forming the bond, the closer the bond is to the ionic end of the continuum.
(b)
Interpretation:
The compound that has a bond closest to the ionic end of the bond spectrum has to be identified.
Concept Introduction:
Polar covalent bonds: A covalent bond between atoms with the different electronegativity. Polar covalent bond has slight positive charge one end and negative charge on the other end. The negative end is the end that has more electronegative atom.
Non-polar covalent bonds: A covalent bond between atoms with the same electronegativity.
The atoms share the bonding electrons in the above molecules equally; that is each electron spends as much time in the vicinity of one atom as in that of the other. Such a bond is called as non-polar covalent bond.
Example:
The greater the difference in electronegativity between the atoms forming the bond, the closer the bond is to the ionic end of the continuum.
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Essential Organic Chemistry (3rd Edition)
- Provide all reasonable resonance structures for each molecular structure below. Use curved arrows to show how electrons are moved and dont forget lone pairs. E 1. CH3 CNO E2. CHỌN -1 NCO E3. CHOCN E +1 4. O C S E5. N = N = O E1. CH CNO E2. CH3NCO E3. CH₂OCN E4. O-C-S E5. N-1=N+1=0 E6. CH H₂Oarrow_forwardChoose the compound below that contains at least one polar covalent bond, but is nonpolar. SCl2 CH2Cl2 AsCl5 GeH2Br2 All of the above are nonpolar and contain a polar covalent bond.arrow_forward3. Draw structural formulas for the following covalently bonded molecules, representingeach covalent bond by a line. N2 CH3OH F2 NH3 CO2 CH4 CH2CH2arrow_forward
- Each of the following molecules has one additional resonance form. Draw the additional resonance form and then fill out the table for each labelled atom.arrow_forwardMatch each of the general molecular formulas below with its correct molecular geometry. Note: The sorting box Tri. Bipyramidal stands for trigonal bipyramidal. Items (6 items) (Drag and drop into the appropriate area below) AB5 with no lone pairs on A AB4 with one lone pair on A AB4 with two lone pairs on A AB2 with one lone pair on A AB2 with two AB2 with no lone lone pairs on A pairs on A Categories Bent 120° bond Bent 109.5° bond Tri. bipyramidal Square planar Seesawarrow_forwardWhich of the highlighted chemical bonds in the molecules below is longest? Shortest? In between? Which highlighted bond requires the highest energy to break? Lowest? In between? Answer these questions by completing the second and third columns in the table. compound HI H -Si-H | H H | H-Ge-H | H HICIH Η HIC-H Η length of highlighted bond choose one choose one choose one - V - V energy of highlighted bond choose one - choose one - choose one - ✓ X Śarrow_forward
- Label the resonance structures in each pair as major, minor, or equal contributors to the hybrid. Then draw the hybrid. a. CH3-C-N-CH3 I HH CH3-C=N-CH3 HH b. CHg=c&l, H CH₂-C=CH₂ Harrow_forwardQ.2. Circle the most polar bond and cross out the least polar bond among the following bonds. Br - Br O-H C-H H-Farrow_forwardPredict the splitting pattern of Ha in the structure. На CH-CH3 H3C CH2CH-CH3 H, will be split into a sextet. O None of the other choices. O H, will be split into an octet. O H, will be split into a septet. O H, will be split into a pentet.arrow_forward
- CH3COCH2 CH2NH2 a) # valan ce e 6) # of electrons for sigma c) # of non-bonding e pair d) # Pi bondsarrow_forwardConsider the polarity of the bonds for each of the following molecules. Rank the polarity of each bond from least polar (1) to most polar (5). O-F bond in OF2 F-F bond in F2 Al-F bond in AIF3 C-F bond in CF4 B-F bond in BF3arrow_forward1st drop box : exothermic or endothermic 2nd drop box: higher energy than PCl3, lower energy than PCl3 or same energy as PCl3 3rd drop box: more stable than PCl3, less stable than PCl3 or stable as PCl3arrow_forward
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning