Concept explainers
Interpretation:
The Lewis structure for each of the given molecule or ion is to be written. Resonance structures are to be included if necessary.
Concept Introduction:
Lewis model represents the molecules by the electron dot model which is based on the octet rule.
In ionic compounds, octet configuration is attained by the loss and gain of electrons.
In covalent compounds, octet configuration is acquired by sharing of electrons between the constituent atoms.
Lewis model represents the molecules by the electron dot model which is based on the octet rule.
While writing the Lewis structure of a covalent molecule, these steps are followed:
First, the correct skeleton is written for the molecule.
A total number of valence electrons are calculated.
Distributea total number of valence electrons in such a way that it completes the octet configuration of all the constituent atoms.
If any atom lacks the octet configuration the double or triple bonds are added.
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Check out a sample textbook solutionChapter 10 Solutions
Introductory Chemistry (5th Edition) (Standalone Book)
- Draw 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_forwardWrite Lewis structures for these compounds. Show all valence electrons. None of them contains a ring of atoms. (a) Hydrogen peroxide, H2O2 (b) Hydrazine, N2H4 (c) Methanol, CH3OHarrow_forwardAcetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) is 11.30 kJ/mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forward
- An elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forwardFormic acid has the chemical formula HCOOH. It is a colorlessliquid that has a density of 1.220 g/mL. (a) The carbonatom in formic acid is bound to one H and both O’s. Drawthe Lewis structure for formic acid, showing resonance ifpresent. (b) Formic acid can react with NaOH in aqueoussolution to produce the formate ion, HCOO-. Write thebalanced chemical equation for this reaction. (c) Draw theLewis structure of the formate ion, showing resonance ifpresent. (d) How many milliliters of a 0.100 M solution ofNaOH would it take to completely react with 0.785 mL offormic acid?arrow_forwardAcetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forward
- 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_forwardWhich of these statements about resonance is true?(a) When you draw resonance structures, it is permissibleto alter the way atoms are connected.(b) The nitrate ion has one long N¬O bond and two shortN¬O bonds.(c) “Resonance” refers to the idea that molecules areresonating rapidly between different bonding patterns.(d) The cyanide ion has only one dominant resonancestructure.(e) All of the above are true.arrow_forwardWrite Lewis structures for the following: (c) C2F6 (contains a C¬C bond), (d) AsO3 3 -, (e) H2SO3 (H is bonded to O), (f) NH2Cl.. Arrange the bonds in each of the following sets in order of increasing polarity: (a) C¬F, O¬F, Be¬F; (b) O¬Cl, S¬Br, C¬P; (c) C¬S, B¬F, N¬O. What is the Lewis symbol for each of the following atoms or ions? (a) K, (b) As, (c) Sn2 + , (d) N3 Write electron configurations for the following ions and determine which have noble-gas configurations: (a) Cd2+, (b) P3-, (c) Zr4+arrow_forward
- Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forward18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)arrow_forwardDraw a Lewis structure for each of the following molecule: (a) chlorodifluoromethane, CHCIF2 (b) propanoic acid C2H5CO2H (basic structure pictured below) (c) acetonitrile, CH3CN ( the framework is H3C-C-N) (d) allene, H2CCCH2arrow_forward
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