Concept explainers
(a)
Interpretation:
The Lewis structure of
Concept Introduction:
A covalent bond is a bond that results from the mutual sharing of electrons between atoms. Lewis structures are representations of the covalent bond. In this, Lewis symbols show how the valence electrons are present in the molecule.
The steps to draw the Lewis structure of the molecule are as follows:
Step 1: Find the central atom and place the other atoms around it. The atom in a compound that has the lowest group number or lowest electronegativity considered as the central atom.
Step 2: Estimate the total number of valence electrons.
Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.
Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.
The formula to calculate formal charge of the atom is as follows:
(b)
Interpretation:
The Lewis structure of
Concept Introduction:
Refer to part (a)
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Chemistry: Principles and Practice
- Write Lewis dot symbols for the following atoms and ions. (a) I (b) I− (c) S (d) S2−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_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
- Based on the Lewis structure for H3C—NH2, the calculated value for the formal charge in the nitrogen atom is (a) -2 (b) +3 (c) -3 (d) +2 (e) 0arrow_forward(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?arrow_forwardAnswer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) ® N2(g) Using the table of average bond energies below, determine the enthalpy change, AH, for the reaction. Average Bond Energy (k) mol-1) Bond N-N 160 N=N 420 N°N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g)® 2 NH3(g) AH° = -92.2 kJ Predict the sign of the standard entropy change, AS', for the reaction. Justify your answer. (C) The value of AG° for the reaction represented in part (b) is negative at low temperatures but positive at high temperatures. Explain.arrow_forward
- The cyanate ion, NCO– , has three (3) possible Lewis structures. (a) Draw these three structures and assign formal charges in each. (b) Which Lewis structure is dominant?arrow_forwardWrite 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_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_forward
- Draw 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_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_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
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning