Concept explainers
(a)
Interpretation:
Lewis structure for the
Concept introduction:
Lewis structure is a convenient way to convey information such as which atoms are bonded to each other by which type of bond. Only valence electrons take part to draw Lewis structure.
Valence electrons that participate in bond formation are called bonding electron pairs whereas electrons that do not take part in bonding and that remain as non-bonding electrons are termed as lone pair of electrons.
Lewis structure is drawn from the total valence electron count of each atom in the molecule. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom. Electrons that participate in forming the bond are bonding electrons. Remaining electrons are distributed first to outer atoms such that each atom completes its octet other than hydrogen.
Answer to Problem 1.44P
Lewis structure for
Explanation of Solution
The given molecule
Thus the skeleton structure for
Remaining two valence electrons are contributed as lone pair of electrons to the outer atom which is nitrogen.
Hence the complete Lewis structure for
Lewis structure for
(b)
Interpretation:
Lewis structure for
Concept introduction:
Lewis structure is drawn from the total valence electron count of each atom in the molecule. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom. Electrons that participate in forming the bond are bonding electrons. Remaining electrons are distributed first to outer atoms such that each atom complete its octet other than hydrogen.
Answer to Problem 1.44P
Lewis structure for
Explanation of Solution
In
Remaining
Lewis structure for
(c)
Interpretation:
Lewis structure for
Concept introduction:
Lewis structure is drawn from the total valence electron count of each atom in the molecule. Valence electrons participate in bond formation are called bonding electron pairs whereas electrons that do not take part in bonding and that remain as non-bonding electrons are termed as lone pair of electrons. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom.
Lone pair of electrons contributed to outer atoms to complete octet except hydrogen.
Answer to Problem 1.44P
The Lewis structure for
Explanation of Solution
Carbon is the central atom in
Remaining six electrons are contributed as lone pairs to the outer atom oxygen but one electron is involved in bonding with complete octet of oxygen atom.
Lewis structure is drawn from the total valence electron count.
(d)
Interpretation:
Lewis structure for
Concept introduction:
Lewis structure is drawn from the total valence electron count of each atom in the molecule. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom. Electrons that participate in forming the bond are bonding electrons. Remaining electrons are distributed first to outer atoms such that each atom completes its octet other than hydrogen.
Answer to Problem 1.44P
Lewis structure for
Explanation of Solution
In
Eight electrons from total
Therefore the Lewis structure for
Lewis structure is drawn from total valence electron count.
(e)
Interpretation:
Lewis structure for
Concept introduction:
Lewis structure is drawn from the total valence electron count of each atom in the molecule. Valence electrons that participate in bond formation are called bonding electron pairs whereas electrons that do not take part in bonding and that remain as non-bonding electrons are termed as lone pair of electrons. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom.
Lone pair of electrons contributed to outer atoms to complete octet except hydrogen.
Answer to Problem 1.44P
Lewis structure for
Explanation of Solution
The given molecule
Remaining
Hence the Lewis structure for
Lewis structure is drawn from total valence electron count.
Want to see more full solutions like this?
Chapter 1 Solutions
ORGANIC CHEMISTRY PRINCIPLES & MECHANISM
- (a) Draw Lewis structure of the following: (i) H3PO4 (ii) N3 - (b) How many hydrogen atoms are present in 10 g of sugar? (c) Calculate formal charge of each atom of CH3O-arrow_forwardDraw a Lewis Structure for each of the following species and assign formal charge where appropriate. Using electronegative values from the period table that was provided identify polar covalent bonds and label the atoms δ+ and δ−. For each of the molecules indicate whether or not it has a dipole moment. (a)CH5N (b) HCN (c) H2CO (d) CH3NC(e) CH3SOCH3 (f) H6BNarrow_forwardDraw Lewis structures for the following compounds and ions, showing appropriateformal charges.(a) [CH3OH2 ]+ (b) NH4Cl (c) (CH3)4NCl(d) NaOCH3 (e) +CH3 (f) -CH3(g) NaBH4 (h) NaBH3CN (i) (CH3)2O¬BF3(j) [HONH3]+ (k) KOC(CH3)3 (l) [H2C“OH]arrow_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_forwardConvert each of the following molecular models into a skeletal structure, and give the formula of each. Only the connections between atoms are shown; multiple bonds are not indicated (gray=C, red =O, blue =N, ivory = H)arrow_forwardFor each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-Narrow_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_forwardDraw the Lewis structures for each of the following ions or molecules. Give the number of electrons in each species. Remember to enclose ion s in square brackets with the charge as a superscript outside the right bracket. (a) SO 2 (b) XeO 2 F 2 (Xe is the central atom) (c) ClF 3 (d) ClO 2 F (Cl is the central atom) (e) BrO 4 -arrow_forwardWhich two species have the same number of lone electron pairs in their Lewis structures?(a) H2O and H3O+(b) NH3 and H3O+(c) NH3 and CH4(d) NH3 and NH4+arrow_forward
- Calculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forwardConvert each of the following molecular models into a skeletal structure, and give the formula of each. Only the connections between atoms are shown; multiple bonds are not indicated (gray = C, red = O, blue = N, ivory = H).arrow_forwardDraw Lewis structures for the following compounds.(a) ammonia, NH3 (b) water, H2O(c) hydronium ion, H3O+ (d) propane, C3H8(e) dimethylamine, CH3NHCH3 (f) diethyl ether, CH3CH2OCH2CH3(g) 1-chloropropane, CH3CH2CH2Cl (h) propane-2-ol, CH3CH(OH)CH3(i) borane, BH3 (j) boron trifluoride, BF3Explain what is unusual about the bonding in the compounds in parts (i) and (j)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