SolnsChap14EVENZum7e

68 a yes both have four sets of electrons about the p

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: )2(π2p)4(σ2p)2, B.O. = 3, diamagnetic (0 unpaired e−) N2 (1st excited state): (σ2s)2(σ2s*)2(π2p)4(σ2p)1(π2p*)1 B.O. = (7 − 3)/2 = 2, paramagnetic (2 unpaired e-) The first excited state of N2 should have a weaker bond and should be paramagnetic. 68. a. Yes, both have four sets of electrons about the P. We would predict a tetrahedral structure for both. See part d for the Lewis structures. b. The hybridization is sp3 for P in each structure since both structures exhibit a tetrahedral arrangement of electron pairs. c. P has to use one of its d orbitals to form the π bond since the p orbitals are all used to form the hybrid orbitals. d. Formal charge = number of valence electrons of an atom – [(number of lone pair electrons) + 1/2 (number of shared electrons)]. The formal charges calculated for the O and P atoms are next to the atoms in the following Lewis structures. O -1 Cl +1 P Cl Cl 0 O Cl P 0 Cl Cl In both structures, the formal charges of the Cl atoms are all zeros. The structure with the P=O bond is favored on the basis of formal charge since it has a zero formal charge for all atoms. CHAP. 14 592 70. COVALENT BONDING: ORBITALS - EVEN-NUMBER PROBLEMS For carbon, nitrogen, and oxygen atoms to have formal charge values of zero, each C atom will form four bonds to other atoms and have no lone pairs of electrons, each N atom will form three bonds to other atoms and have one lone pair of electrons, and each O atom will form two bonds to other atoms and have two lone pairs of electrons. Following these bonding requirements gives the following two resonance structures for vitamin B6: O b a H O H g HC H C C f O C HH c C d e C O N C C C H O H H H H C C C HH C H C H C C N O H H H a. 21 σ bonds; 4 π bonds (The electrons in the three π bonds in the ring are delocalized.) b. Angles a), c), and g): ≈109.5°; angles b), d), e), and f): ≈120° c. 6 sp2 carbons; the five carbon atoms in the ring are sp 2 hybridized, as is the carbon with the double bond to oxygen. d. 4 sp3 a...
View Full Document

This note was uploaded on 01/26/2014 for the course CHEM 001 taught by Professor Giancoli during the Fall '12 term at UPenn.

Ask a homework question - tutors are online