Concept explainers
a)
Interpretation:
Lewis structure must be drawn for methane.
Concept Introduction:
Methane is a molecule with formula CH4.
C is the central atom which is a p block element belonging to group 14.
Lewis structure can be determined from the valence electrons of a central atom.
Total electron pairs will be:
Where V, n, a and c are valence shell electrons of central
b)
Interpretation:
Lewis structure needs to be drawn for carbon dioxide.
Concept Introduction:
Lewis structure can be determined from the valence electrons of a central atom.
Total electron pairs will be:
Where V, n, a and c are valence shell electrons of central atom, number of monovalent atoms attached, anionic charge, cationic charge respectively.
c)
Interpretation:
Lewis structure needs to be drawn for Phosphorous trichloride.
Concept Introduction:
Lewis structure can be determined from the valence electrons of a central atom.
Total electron pairs will be:
Where V, n, a and c are valence shell electrons of central atom, number of monovalent atoms attached, anionic charge, cationic charge respectively.
d)
Interpretation:
Lewis structure needs to be drawn for perchlorate ion.
Concept Introduction:
Lewis structure can be determined from the valence electrons of a central atom.
Total electron pairs will be:
Where V, n, a and c are valence shell electrons of central atom, number of monovalent atoms attached, anionic charge, cationic charge respectively.
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Principles of Modern Chemistry
- Draw 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_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_forwardThere is persuasive evidence for the brief existence of the unstable molecule OPCl. (a) Draw a Lewis diagram for this molecule in which the octet rule is satisfied on all atoms and the formal charges on all atoms are zero. (b) The compound OPCl reacts with oxygen to give O2PCl. Draw a Lewis diagram of O2PCl for which all formal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.arrow_forward
- Draw a Lewis electron-dot symbol for (a) Ba; (b) Kr; (c) Br.arrow_forwardIn addition to ammonia, nitrogen forms three other hy-drides: hydrazine (N₂H₄), diazene (N₂H₂), and tetrazene (N₄H₄).(a) Use Lewis structures to compare the strength, length, and or-der of nitrogen-nitrogen bonds in hydrazine, diazene, and N₂.(b) Tetrazene (atom sequence H₂NNNNH₂) decomposes above 0°C to hydrazine and nitrogen gas. Draw a Lewis structure fortetrazene, and calculate ΔH°ᵣₓₙ for this decomposition.arrow_forwardDraw a Lewis electron-dot symbol for (a) Rb; (b) Si; (c) I.arrow_forward
- Which 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_forwardDraw a Lewis electron-dot symbol for (a) Sr; (b) P; (c) S.arrow_forwardA resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity? (a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar. (b) The farther two atoms are apart in a bond, the larger the dipole moment will be.arrow_forward
- Draw Lewis electron dot diagrams for the following species: (a) AsH3; (b Draw Lewis electron dot diagrams for the following species: (a) AsH3; (b) HOCl; (c) KrF+; (d) PO2 Cl 2 - (centralP atom).arrow_forwardWrite the Lewis symbol for atoms of each of the following elements:(a) Al, (b) Br, (c) Ar, (d) Sr.arrow_forwardA stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule— namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain. 100. The gasarrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning