Concept explainers
(a)
Interpretation:
All resonance form for nitric acid has to be written.
Concept Introduction:
Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.
According to the concept of resonance, when a single Lewis structure cannot describe a molecule accurately, a number of structures with same energy, position of nuclei, bonding and non-bonding pair of electrons are taken as the canonical structures of the hybrid which describes the molecule accurately.
The formula for the formal charge can be written as
(b)
Interpretation:
All resonance form for nitrate ion has to be written.
Concept Introduction:
Refer part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 6 Solutions
Chemistry: The Molecular Science
- Two substances with empirical formula HNO are hyponi-trous acid ( μ=62.04 g /mol) and nitroxyl (μ=31.02 g/mol).(a) What is the molecular formula of each species?(b) For each species, draw the Lewis structure having the lowestformal charges. (Hint:Hyponitrous acid has an N=N bond.)(c) Predict the shape around the N atoms of each species.(d) When hyponitrous acid loses two protons, it forms the hy-ponitrite ion. Draw cisand transforms of this ion.arrow_forwardWrite the Lewis symbol for atoms of each of the following elements:(a) Al, (b) Br, (c) Ar, (d) Sr.arrow_forwardWrite Lewis dot symbols for the following atoms and ions. (a) I (b) I− (c) S (d) S2−arrow_forward
- Write Lewis dot symbols for (a) Ca2+, (b) N3−, and (c) I −.arrow_forwardCovalent bonds: H―HC―HO―HO═O C≡O Bond energy (kJ/mol):4364154654981080Calculate the enthalpy change (H, in kJ/mol) for the following reaction and indicate whether the reaction is exothermic or endothermic.(*BE for C═Oin CO2)(a) CH4(g)+ H2O(g)CO(g)+ 3H2(g);arrow_forwardWrite Lewis structures for the following molecules or ions. (Assign lone pairs, radical electrons, and atomic charges where appropriate.) (a) SbO43− (b) ICl6− (c) SO32- (d) HOBrOarrow_forward
- Which of the following are not related as resonance structures? OH (A) `NH. NH (B) ОН (C) CH2 (D)arrow_forwardCalculate 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_forwardWhich of the following bonds are polar: (a) P—O; (b) S—F; (c) Br—Br; (d) O—Cl? Which is the more electronegative atom in each polar bond?arrow_forward
- Write the Lewis dot symbols of the reactants and products in the followingreactions. (First balance the equations.)(a) Sr + Se → SrSe(b) Ca + H2 → CaH2(c) Li + N2 → Li3N(d) Al + S → Al2S3arrow_forwardWith reference to the “Chemistry Put to Work” box on explosives, (a) use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin. (b) Write a balanced equation for the decomposition of TNT. Assume that, upon explosion, TNT decomposes into N2(g), CO2(g), H2O(g), and C(s).arrow_forwardWhich 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_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning