Concept explainers
(a)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
(b)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
(c)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
(d)
Interpretation:
Nature of the bond is whether nonpolar covalent or polar covalent or ions has to classified.
Concept introduction:
Nature of the bond:
Nature of the bond is based on the electronegativity difference between the bonded atoms.
Non polar covalent bond is formed when the electronegativity difference between the bonded atoms is less than 0.5.
Polar covalent bond is formed when the electronegativity difference between the bonded atoms is 0.5 to 1.9.
The ions formed when the electronegativity difference between the bonded atoms is more than 1.9.
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Chapter 1 Solutions
Organic Chemistry
- Which statements are true about electronegativity? (a) Electronegativity increases from left to right in a period of the Periodic Table. (b) Electronegativity increases from top to bottom in a column of the Periodic Table . (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity. (d) The higher the atomic number of an element, the greater its electronegativity.arrow_forwardIdentify the electron pair geometry, the molecular structure of each, and the polarity of the following molecules: (a) ClNO (N is the central atom) (b) Cl2CO (C is the central atom) (c) Cl2SO (S is the central atom) (d) SO2F2 (S is the central atom) (e) XeO2F2 (Xe is the central atom) (f) ClOF2 + (Cl is the central atom)arrow_forward(a) Complete the Lewis structure for vinyl chloride by showing all unshared pairs of electrons. (b) Predict the H-C-H, H-C-C, and Cl-C-H bond angles in this molecule. (c) Does vinyl chloride have polar bonds? Is it a polar molecule? Does it have a dipole?arrow_forward
- Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) COarrow_forwardIn each case, tell whether the bond is ionic, polar cova- lent, or nonpolar covalent. (a) Br, (e) SiH, (d) SrF, (c) HCl (g) N, (b) BrCl 2 (f) CO (h) CsCl 4.arrow_forwardThe atomic number of sulfur is 16. Sulfur combines withhydrogen by covalent bonding to form a compound, hydrogensulfide. Based on the number of valence electrons in a sulfuratom, predict the molecular formula of the compound.(A) HS(B) HS2(C) H2S(D) H4Sarrow_forward
- 3. The following are some molecules:H2, HF, CO2, H2O, Cl2, NH3, CH4, CHCl3 (a) Which of the above molecules do/does not contain polar bond? Explain your answer. (b) Which covalent bond has the highest bond polarity among the eight molecules? (c) (i) Which of the above molecules are non-polar molecules? (ii) Explain why these molecules are non-polar. 4. (d) Draw a diagram to illustrate the formation of hydrogen bonds in H2O.arrow_forwardDraw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+arrow_forward3. Using electronegativity difference, indicate the type of bond between the following atoms: (a) Li-Cl(b) C-Br(c) F-Cl(d) Br-Brarrow_forward
- Which of the following is a resonance structure of compound X? N (A) OH NH (B) X NH O NH (C) N (D)arrow_forwardWhich of the following compounds are likely to have covalent bonds or are likely to have ionic bonds ? (a) CF4 (b) NaF (c) CH4 (d) MgBr2arrow_forwardDraw Lewis structures for the following compounds. Remember to enclose ions in square brackets. On your answer sheet, state the number of valence electrons in each compound. (a) NaCN (b) CH 3 Br (c) Ca(OCl) 2arrow_forward
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning