(a)
Interpretation:
The name of
Concept Introduction:
A covalent bond is formed by mutually sharing of electrons between the atoms of two non-metals.
This bond formed may be polar or non-polar depending on the electronegativities of the two atoms of the elements involved in the formation of the covalent bond.
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.
The two types of atoms in a binary covalent compound are named in this order-first the less electronegative element and then the more electronegative element.
(b)
Interpretation:
The name of
Concept Introduction:
A covalent bond is formed by mutually sharing of electrons between the atoms of two non-metals.
This bond formed may be polar or non-polar depending on the electronegativities of the two atoms of the elements involved in the formation of the covalent bond.
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.
The two types of atoms in a binary covalent compound are named in this order-first the less electronegative element and then the more electronegative element.
(c)
Interpretation:
The name of
Concept Introduction:
A covalent bond is formed by mutually sharing of electrons between the atoms of two non-metals.
This bond formed may be polar or non-polar depending on the electronegativities of the two atoms of the elements involved in the formation of the covalent bond.
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.
The two types of atoms in a binary covalent compound are named in this order-first the less electronegative element and then the more electronegative element.
(d)
Interpretation:
The name of
Concept Introduction:
A covalent bond is formed by mutually sharing of electrons between the atoms of two non-metals.
This bond formed may be polar or non-polar depending on the electronegativities of the two atoms of the elements involved in the formation of the covalent bond.
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.
The two types of atoms in a binary covalent compound are named in this order-first the less electronegative element and then the more electronegative element.
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Chapter 3 Solutions
Introduction To General, Organic, And Biochemistry
- 3-119 Perchloroethylene, which is a liquid at room temperature, is one of the most widely used solvents for commercial dry cleaning. It is sold for this purpose under several trade names, including Perciene®. Does this molecule have polar bonds? Is it a polar molecule? Does it have a dipole?arrow_forward3-25 Why are carbon and silicon reluctant to form ionic bonds?arrow_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. Using electronegativity difference, indicate the type of bond between the following atoms: (a) Li-Cl(b) C-Br(c) F-Cl(d) Br-Brarrow_forwardWrite a chemical formula for a compound that containstwo chlorine atoms to every one oxygen atom. (a) Cl2O(b) ClO2(c) 2ClO(d) Cl(O2)2arrow_forwardDraw a Lewis structure for each of the following molecules: (a) chlorodifluoromethane, CHClF2 (b) propanoic acid, C2 H5CO2H (basic structure pictured below) (c) acetonitrile, CH3CH (the framework is H3C-C-N) (d) allene, H3CCCH2arrow_forward
- Write Lewis formulas, including unshared pairs, for each of the following. Carbon has four bonds in each compound. (a) Propane (C3H8) (c) Methyl fluoride (CH3F) (b) Methanol (CH4O) (d) Ethyl fluoride (C2H5F)arrow_forwardWrite the Lewis structures for each of the following:(a) NH2−(b) N2F4(c) NH2−(d) NF3(e) N3−arrow_forwardName each ionic compound. In each of these compounds,the metal forms only one type of ion. (a) CsCl (b) SrBr2 (c) K2O (d) LiFarrow_forward
- 2. Draw the Lewis structures for each of the following ions or molecules. Give the number of electrons in each species. Remember to enclose ions in square brackets with the charge as a superscript outside the right bracket. (a) Br 20 (c) BrF 3 (e) PCI 4* (b) IOF 3 (I is the central atom) (d) ASF 3arrow_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_forward3. 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_forward
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning