Interpretation:
To explain the reason why oxygen has two bonds and two unshared pair of electrons in covalent compounds.
Concept Introduction:
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
Lewis structure of a molecule can be determined as-
- 1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.
If the molecule is an anion, add the same number of electrons as the charge present on the ion.
If it is a cation, subtract the same number of electrons as the charge present on the ion.
2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).
3. Therefore number of bonds formed =
4. Remaining electrons are called as lone pairs.
5. Assign formal charges to atoms.
Trending nowThis is a popular solution!
Chapter 3 Solutions
Introduction to General, Organic and Biochemistry
- 3-67 Why does nitrogen have three bonds and one unshared pair of electrons in covalent compounds?arrow_forward3-70 Draw a Lewis structure of a covalent compound in which oxygen has: (a) Two single bonds and two unshared pairs of electrons (b) One double bond and two unshared pairs of electronsarrow_forward3-63 What is the difference between (a) a bromine atom, (b) a bromine molecule, and (c) a bromide ion? Draw the Lewis structure for each.arrow_forward
- 3-25 Why are carbon and silicon reluctant to form ionic bonds?arrow_forward3-68 Draw a Lewis structure of a covalent compound in which nitrogen has: (a) Three single bonds and one unshared pair of electrons (b) One single bond, one double bond, and one unshared pair of electrons (c) One triple bond and one unshared pair of electronsarrow_forward3-64 Acetylene (C2H2), hydrogen cyanide (HCN), and nitrogen (N2) each contain a triple bond. Draw a Lewis structure for each molecule. Which of these are polar molecules, and which are nonpolar molecules?arrow_forward
- 3-66 Why can’t second-row elements have more than eight electrons in their valence shells? That is, why does the octet rule work for second-row elements?arrow_forward3-31 Why does electronegativity generally increase going from left to right across a row of the Periodic Table?arrow_forward3-41 Describe the structure of sodium chloride in the solid state.arrow_forward
- 3-79 Answer true or false. (a) The letters VSEPR stand for valence-shell electron-pair repulsion. (b) In predicting bond angles about a central atom in a covalent molecule, the VSEPR model considers only shared electron pairs (electron pairs involved in forming covalent bonds). (c) The VSEPR model treats the two electron pairs of a double bond as one region of electron density and the three electron pairs of a triple bond as one region of electron density. (d) In carbon dioxide, OCO, carbon is surrounded by four pairs of electrons and the VSEPR model predicts 109.5° for the OCO bond angle. (e) For a central atom surrounded by three regions of electron density, the VSEPR model predicts bond angles of 120°. (f) The geometry about a carbon atom surrounded by three regions of electron density is described as trigonal planar. (g) For a central atom surrounded by four regions of electron density, the VSEPR model predicts bond angles of 360°/4 = 90°. (h) For the ammonia molecule, NH3, the VSEPR model predicts HNH bond angles of 109.5°. (i) For the ammonium ion, NH4, the VSEPR model predicts HNH bond angles of 109.5°. (j) The VSEPR model applies equally well to covalent compounds of carbon, nitrogen, and oxygen. (k) In water, HOH, the oxygen atom forms covalent bonds to two other atoms, and therefore, the VSEPR model predicts an HOH bond angle of 180°. (l) If you fail to consider unshared pairs of valence electrons when you use the VSEPR model, you will arrive at an incorrect prediction. (m) Given the assumptions of the VSEPR model, the only bond angles it predicts for compounds of carbon, nitrogen, and oxygen are 109.5°, 120°, and 180°.arrow_forward2-97 Explain why the Ca3+ ion is not found in chemical compounds.arrow_forward3-87 Consider the molecule boron trffluoride, BF3. (a) Write a Lewis structure for BF3. (b) Predict the FBF bond angles using the VSEPR model. (c) Does BF3 have polar bonds? Is it a polar molecule?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning