Concept explainers
Interpretation:
For each of the molecule that contains an expanded octet, Lewis structure is to be determined.
Concept Introduction: Expanded octets are an exception of Lewis structure where central atoms in a Lewis structure have more than eight electrons in their valence shells.
Lewis structure represents valence shell electrons, as dots are the
For molecules which obey the octet rule must have eight electrons in their valence shell. In the molecule, the total number of electron groups around the central atom is equal to the sum of lone pairs, a single bond, a double bond and triple bond around the central atom.
Want to see the full answer?
Check out a sample textbook solutionChapter 10 Solutions
Introductory Chemistry (5th Edition) (Standalone Book)
- Write 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_forwardCyanogen (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_forwardAn 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_forward
- Write Lewis structures for the following molecules or ions. (Assign lone pairs, radical electrons, and atomic charges where appropriate.) (a) BrF3 (b) AsF5 (c) BI3 (d) AsF6−arrow_forwardThe two compounds nitrogen dioxide and dinitrogen tetraoxide are introduced in Section 3.13. (a) NO2 is an odd-electron compound. Draw the best Lewis diagrams possible for it, recognizing that one atom cannot achieve an octet configuration. Use formal charges to decide whether that should be the (central) nitrogen atom or one of the oxygen atoms. (b) Draw resonance forms for N2O4 that obey the octet rule. The two N atoms are bonded in this molecule.arrow_forwardDraw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.) (Assume the central atom does not contain an expanded octet.) (a) bromine dioxide (BrO2) (b) beryllium bromide (BeBr2) (c) phosphorus pentafluoride (PF5)arrow_forward
- Draw 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_forwardKeeping in mind that some elements violate the octet rule, draw a Lewis structure for each compound: (a) BeH 2; (b) PCl 5.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_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_forwardDraw 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_forward(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning