CHEMICAL BONDING 1.3 The electron configurations of the designated ions are Number of Electrons Electron Configuration in lon of lo (c) H (d) O 522s-2pr 2px 2p, 9 ()c 1522p°3s5p Those with a noble gas configuration are H, F, and Ca2+ 1. 4 A positively charged ion is formed when an electron is removed from a neutral atom. The equation representing the ionization of carbon and the electron configurations of the neutral atom and the ion A negatively charged carbon is formed when an electron is added to a carbon atom. The addi- tional electron enters the 2p, orbital. C s232p242p 152322p p, 2p Neither Ct nor C has a noble gas elect 1.5 Hydrogen has one valence electron, and fluorine has seven. The covalent bond in hydrogen fluoride arises by sharing the single electron of hydrogen with the unpaired electron of fluorine Combine H and F: to give the Lewis structure for hydrogen fluoride H: F: 1.6 We are told that Ch has a carbon-carbon bond to write the HH Thus, we combine two . C. and six H Lewis structure H: C: C: H of ethane There are a total of 14 valence electrons distributed as shown. Each carbon is surrounded by eight electrons 1.7(b) Each carbon contributes four valence electrons, and each fluorine contributes seven. Thus, CFA has 36 valence electrons. The octet rule is satisfied for carbon only if the two carbons are at- tached by a double bond and there are two fluorines on each carbon. The pattern of connections shown(below left) accounts for 12 electrons. The remaining 24 electrons are divided equally (six each) among the four fluorines. The complete Lewis structure is shown at right below (c) Since the problem states that the atoms in C3 H3N are connected in the order CCCn and all hy drogens are bonded to carbon, the order of attachments can only be as shown(below left)so as to have four bonds to each carbon. Three carbons contribute 12 valence electrons, three hy drogens contribute 3, and nitrogen contributes 5, for a total of 20 valence electrons. The nine Back Forward Main Menu TOC Study Guide Toc Student OLC MHHE Website2 CHEMICAL BONDING 1.3 The electron configurations of the designated ions are: Number of Electrons Electron Configuration Ion Z in Ion of Ion (b) He 2 11s 1 (c) H 1 21s 2 (d) O 8 91s 2 2s 2 2px 2 2py 2 2pz 1 (e) F 9 10 1s 2 2s 2 2p6 ( f ) Ca2 20 18 1s 2 2s 2 2p6 3s 2 3p6 Those with a noble gas configuration are H, F, and Ca2. 1.4 A positively charged ion is formed when an electron is removed from a neutral atom. The equation representing the ionization of carbon and the electron configurations of the neutral atom and the ion is: A negatively charged carbon is formed when an electron is added to a carbon atom. The addi￾tional electron enters the 2pz orbital. Neither C nor C has a noble gas electron configuration. 1.5 Hydrogen has one valence electron, and fluorine has seven. The covalent bond in hydrogen fluoride arises by sharing the single electron of hydrogen with the unpaired electron of fluorine. 1.6 We are told that C2H6 has a carbon–carbon bond. There are a total of 14 valence electrons distributed as shown. Each carbon is surrounded by eight electrons. 1.7 (b) Each carbon contributes four valence electrons, and each fluorine contributes seven. Thus, C2F4 has 36 valence electrons. The octet rule is satisfied for carbon only if the two carbons are at￾tached by a double bond and there are two fluorines on each carbon. The pattern of connections shown (below left) accounts for 12 electrons. The remaining 24 electrons are divided equally (six each) among the four fluorines. The complete Lewis structure is shown at right below. (c) Since the problem states that the atoms in C3H3N are connected in the order CCCN and all hy￾drogens are bonded to carbon, the order of attachments can only be as shown (below left) so as to have four bonds to each carbon. Three carbons contribute 12 valence electrons, three hy￾drogens contribute 3, and nitrogen contributes 5, for a total of 20 valence electrons. The nine C C F F F F C F F C F F H H C H H H H Thus, we combine two C H C to write the Lewis structure of ethane and six Combine H and F to give the Lewis structure for hydrogen fluoride H F C 1s2 2s2 2px 1 py 1 2pz 1 C 1s2 2s2 2px 1 2py 1 e C 1s2 2s2 2px 1 2py 1 C 1s2 2s2 2px 1 e Back Forward Main Menu TOC Study Guide TOC Student OLC MHHE Website