General Chemistry  !" #$ 

   
   
 !"

 •

  #    • 
$
 (Chemical Bonding) • "%
&

'()  *  
!  + • !"  " (Lewis Structure) '() VSEPR • '() ! < ++  (Molecular Orbtial Theory; MO) • '()
 G+ (Valence Bond Theory; VB)       
'()  * * 
! K        
 
K


2

 (Chemical Bonding) 1.
6""" (Ionic bond)

6""" L M K KS 

 L  M <  M   N! $ S  N
  M&K $   EN  (An attractive force that holds atoms together to form molecules)  NZ [  M < S\\] (coulombic attraction) • "
N
 • "" EN ; : *K  _  → S (! K) (O*K  "P 
M&) • "" EN = :   _  → S  (! K) • O 
N <

M + (g) + X− (g) → MX(s) + lattice energy

 N%K    & 1.
S  (Ionic Bond) 2.
!  + (Covalent Bond) 3.
! K (Metallic Bond)

3 4

2.
?  (Covalent Bond) 3.
? (Metallic Bond)

?  L M K K $   EN
? L  M  ! KS *Z M (K *   (  EN  )   
[*      EN O)  G+  _ *
O*K"P M& •  G+  _ ! K L S*    S  " • "" EN = : S  * "   _  •   _  "OK  M <   "     - - - - + - - + - + ------+ - - - + - +

- -

------Sea of - - - electrons  - - - - + + - + - () - - - -

- + - + - - + + - - - -

------

- - - -

+ - + - + - +

------+ + - + Shared - - - - electrons  E"F"  
 F    5 6

1
 
 (Bond Energy)
 
O ; (Average Bond Energy)

 
 KL
   
 (Bond dissociation
 
O ; Nq 
" 
 energy, D) L
  * *" 
   "OK
    *! $   (N! )
*! $ ( N)  

H2(g)→2H(g) D(HfH) = 436 kJ/mol

   *! $   [ 
 " 
    C-H • → CH4(g) CH3(g) + H(g) D(H-C)CH4= 436 kJ/mol • → CH3(g) CH2(g) + H(g) D(H-C)CH3= 368 kJ/mol • → CH2(g) CH(g) + H(g) D(H-C)CH2 = 519 kJ/mol • CH(g) →→→ C(g) + H(g) D(H-C)CH = 335 kJ/mol

7 8

 S" " R (Heat of Reaction)     T  S" " R

 QR  L    
Q  "T [K
    #    S & (" & )  S
#T("Z %r+) CH4(g) + Cl2(g) →→→ CH3Cl (g) + HCl(g)  S" " R (∆Hrxn)L
 s     S*<L #    "PK S [ H DD rxn ∑ −=∆ ∑ • ∑ D(

" & ) = 4D(C-H) + D(Cl-Cl) reactants products reactants !"" !#$ !"" !#$ • ∑ D (

Z %r+ ) = D(C-Cl) + 3D(C-H) + D(Cl-H) %"!*"+ %"&'!() products ∆ • ∆H N  #   

Hrxn = 4D(C-H) + D(Cl-Cl) – [D(C-Cl) + 3D(C-H) + D(Cl-H)] rxn × × • ∆H N * 

L*K #    ( <
) = (4 414 + 243) – (339 + 3 414 + 431) kJ/mol = –104 kJ/mol rxn #    &[ 104 kJ/mol

9 10

 
 (Bond Length)  
O ; " ?_T `

 
 LKK <  "
 ! N O K  &" M < S   "$ 
 O"$ KL "P %
 "$

!  +"
+

 • 
  >
< >
" •

  <
< <
"

Bond Bond Length Energy

11 12

2 _
 a
! "
 (Bond Polarity)

_
 L$  M& L  106.0° a
! "
 L [  "Z
 2
      _  * *"
K    "  
"%
&
!  +M&<  EN  & 104.0° " P EN  &"  [ 
! $   "<    $
[S   _ * K &"[S"O" GM • ° ° [ 
!  +  & H2O = 104.5 • H2S = 92 Xδδδ+−−−Yδδδ-  ;" EN " Y >>> X
O!"! $   $
 [ON  v<    _ *! $ H + F H F

δδδ+ δδδ- 13 14

ef  ;#S"$ 
?  f"" (Octet Rule)

f""     G+  _   * (  1. $$g " "  " (Lewis Structure) [    _ KL x"qL*K< 8A)[ "P  
     2. ef ?_ ""$ (Molecular Orbital, MO)      !   "#(% &
') • * S   $* s  p block 3. ef
 E (Valence Bond, VB) • * S  "  + •   ! q
  Be B  Al *  f"" H  He g E"F"$ "

Noble Gas (8A) valence e−−− <<< 8 valence e−−− = 8

15 16

1. $$g " "  " (Lewis structure) ? S $$g_Q"F"

G.N. Lewis " "
!  +K *
 !"  "KL!" [$   _  ! $ [NS  f"" (Octet rule) L q""#Q `  (Lewis|s dot structure) N   
L "  G+  ?S ;g S

;"#S  E"F"$   _  "
!  +K * Qr 
L [ [    _ KL x"qL*K< 8A)GM ! $ O*K&! $  "P  "$
!"  "  • "*[q
 G+  _     • * [$  G+  _  • * S   $* s  p block

Carbon Hydrogen CHCH44 17 18

3 ? S  " " ?_   ? S  "

!"  "! $ 1.  Q"" (S"   valence electron   )   •
!  +L*   _ "  gQ  ""#?_ • KM
 "  _  (2 shared electrons) 2. $g   E"F" " _""#?_ 6"""$: 
;g  "F"T $g  g_$ " 6""" • − }  
  [$ 2 [$ (:) KL KM" ( ) } 6"""$ : $g  "F"T $g  g_$  " 6""" ♦   _  * *"
   bonding electron 3.  ;"""QS 
Q ; ( T "" $"" ♦   _  S "
  non-bonding electron  ) ?Q#S 2 "F"#  S
Q ; T
 4.  E"F"#S$"" #S$8 ( S H T $ 2) H H 5. "F" ; "#S$"" (" g  T 8) H C H H−C−H 6. uS g   E"F" ;"" 6T$ 8 #S H H "F" ;6TT 
 (unshared pair electron) " "" N N N≡N "$`  S
=T "
  7. g   E"F" S" T $ ;6QSg  S" 1. 19 20

 "T ? S  " " NF3  "T ? S  " " HCN

1. ""  " N 1. ""  " C 2. g   E"F" = 5 + (7x3) = 26 "F" (g   E"F" " N = 5 F = 7) 2. g   E"F" " HCN 1 + 4 + 5 =10 "F" 3.  
Q ;  T "" $""  3.  
Q ;  T "" $"" ;
 F N F F N F H C N ,- F F 4.  "F" " ""  #S$ 8 ( " 2) 4.  "F" " "" #S$ 8 H C N F N F

F 5. "F" ; "#S$"" (10-10 = 0) 5. "F" ; "#S$"" (26-24 = 2 .!"/$012/1$34 "F") 6.  "F" ;6TT 
 " """$` (N)  S
 F N F F N F F N F =T "
  g""  "F"$Q ,- ,- F F F H C N H C N H−C≡N

21 22

S" S " f"" g_{"  (Formal charge)

1. ?_ ; "F"y  ; T g_{"  y T  T g   E"F" " ""Q ; $ " ""#? S  " y     a
• ClO2  "F"  T $ 19 • NO  "F"  T $ 11 ! " ?_"T T ` • NO2  "F"  T $ 17    g_{"  " "" 2. ?_ ;""  "F"S" T 8 • = − − 1 BNV BF3 B  "F"T $ 6 formal charge 2 eee • BeH Be  "F"T $ 6 2 • V  E"F" " ""Q ; 3. ?_ ;""  "F"  T 8 • N  E"F" ;6T6QS S
 • PCl5  "F" T $ 10 F • B  E"F"! Q ; S
"$""! • XeF4  "F" T $ 12 F S F

F • SF4  "F" T $ 10

23 24

4  "T g  g_{"  " T"" ?EE (Resonance)

|
[IO3] O−−−I−−−O *! $ KLS "P  [O   "S  O  1    CO2  SO2 +1 -1 -1 +1 • −−−1 +2 −−−1 ≡ − − ≡ I = 7  2  ½ (6) = +2 O−−−I−−−O O≡≡C −−OO = C = OO − C ≡≡ O • O = 6  6  ½ (2) = -1 +1 +1 O S S [$ = +2  1  1  1 = -1 −−−1 O O -1 O-1 O |
[NHH 3C 2COO]  Q <[O
    #+ &  R ?EE !   H H O [O
 [     [   O  KL"  
 + H−N−C−C   N   G+ 5 
 3
 - [  _ *
 H H O P  [N P S[N 

25 26

?EE (Resonance) ? S Lewis  ;y66QS

K *
[!"* N!"  !"  " O3 +1 +1 NSS   "$  K   & O O 1. NS )  "$ O O O O -1 -1 2. !"  [$\+ O "$ [ 
 
K O &" 3.     EN "< [$\+ N  " ! $ O3 S
& 2   !"  4.     S [$\+ 

  !"!G G+ (Resonance structure) O≡ C −−− O O = C = OO − C ≡≡≡ O CO2 +1 0 -1 0 0 0 -1 0 +1 1.278 Å O 1.278 Å − N N N N N N N N N O O N3 -2 +1 0 -1 +1 -1 0 +1 -2

27 28

ef  ~_T"F"#  E  ~ " _T"F"

Valence Shell Electron Pair Repulsion(VSEPR) L'()  * 

  
 (
 
< KL
") N O<! $ KLS M  
! G+   _ "
 $  &   $[ [O ! !"! $ [M&<[O $  _  *    _    "
   _ !   S[ON 
Z  $  _ M&  $ • 2   _ 
[q
 G+  _ &   _  (P $  _   *K‚ [  <[M •   _ N $   (<  _ ; electron pair) "PZ  $  _ LSS  ) ♦ "F" S

(2, 4, 6   _    
 L
 , <, " )   $  _  >>> >>> >>> >>> ♦ "F"=T?QQQ ; (2   _ ) =T?QQQ ;
 
=T
Q ; "F"Q ; ♦ "F"?QQQ ; (1   _ )
  $  _ "
[ P EN   •  $  _ [[    *KK "$ 
L*K  
M& (Z [ ) Z  "$ Q  u   ; _Q

29 30

5  gQ T " _T"F"(m+n)    =T ?_?Q VSEPR

_T"F"" gy"F" S
 "6T S
F6QS 1.  "< !"  " 2.  "<  AXmEn 180° • A    • X 
   120° !  m L g  _T"F" ; S
 • E  $  _    SS "
 109.5° !  n L g  _T"F" ;6T6QS S
 3. O[   O K $  _  (m+n) 90,120° 4.
[ O K<  _ !   ( 
L&   "$ ) KL   _ !   ( 
L&  "$ ) 90° 5. O<! $ !  <[[ O K


31 32

=T " ?_ =T " ?_

2  $  _  (n+m=2)
4  $  _  (n+m=4) • AX2 +" • AX4 4"89,+
3  $  _  (n+m=3) $,89.$ • • AX3 :;; XA 3E 8$=> $,89.$ X• A 2E $<$" (<120°) • AX E 2 2 $<$" (<109.5°)

33 34

=T " ?_ =T " ?_

5  $  _  (n+m=5)
6  $  _  (n+m=6)

• AX 8$=?@0> • AX 5 $,89.$ 6 4":1=,+

X• A 4E =, X• A E 8$=> 5 89,89.$ !48 • AX3E2 89,89.$ • +" AX4E2 :;; •XA 2E3

35 36

6  "T    =T ?_  "T    =T ?_*

= " = AXmEn  T _T =T ?_
! $      1   *K
[  "F"
CH4     H H H C O H H C H AX E 4 0 H H

AX4 AX2E2  ;S _ "
NH3 E H ∼∼∼ ° AX E 109.5 H N H 3 1

∼∼∼104.5°

37 38

_
 ; ;6* ~ " T EN T"_
*

 EN    (EN  $ ) 120°°° >120°°° >120°°° PI PBr PCl PF AX3 3 3 3 3

<120°°° <120°°° EN(X) 2.66 2.96 3.16 3.98 H Cl angle 102.0 101.5 100.3 97.8 H 109.5°°° H >>109.5°°° <109.5°°° °°° H >109.5
 EN    (EN  $) H <<109.5°°° H X H >109.5°°° AsH PH NH <109.5°°° AX3 3 3 3 A EN(A) 2.17 2.19 3.04 X 90°°° >90°°° °°° X <90 angle 91.6 93.8 107.0 °°° 120 >120°°°

39 40

_
 = " * a
! " ?_ (Polarity of Molecule)

"PO"<   "S [$
! $ a
! " ?_L"%
&"$ (net dipole)
$
*! $

104.5°°° 90°°° 107°°° AX E AX E AX E 2 ? 3 ? 4 ?
"%
&! $ KS ! "%
&
$
  +

AX H O 4 AX2E2 110°°° 104°°° | || 118°°° H–C–C–O–H AX3 | H

41 42

7  "T a
! " ?_ 2. ef ?_ ""$" (MO Theory)

BCl ef ?_T ""$ (Molecular Orbital Theory) 3  
!  +! * +  ! $

NH3 "" "" ?_ AO + AO MO

CHCl3
""$ " ?_ (MO) L <  _ *
SF ! $  [+    (AO)   5 Z  "  (Linear Combination of Atomic Orbital, LCAO)
HCN
[O MO   M&[O AO &K

43 44

  S ?= ""$   S ?= ""$*

+  ! $  [GK L (overlap)  AO
 ES" ;" " ""$ " "" (AO Overlap)
$$  (Bonding): N AO    ;"  ( ) " L AO  GK L[ N MO  Q""$#  ;"""
; ‚!  u   ‚! •
$$   (Antibonding): N AO    ;"  ( )T  $$
 (bonding molecular orbital, BMO) +  [  Q""$#  ;"""Q  u S" (
 
;)  *K‚M&*  LK  "P 
M& • $$S 
 (antibonding molecular orbital, AMO) +  ~~ Q$
  " ?= ""$ (Molecular Orbital Diagram) L ZZ  "  [  *K‚M&*  LK  "P    
 MO   AO
 ES" ;" " AO gQ ‚!6QS ;" 1sA − 1sB Antibonding antibonding • AO 
*   • AO    K"

Energy 1s 1sA B • AO  <  v K" 1s + 1s Bonding A B bonding

45 46

  ES" ;" " ""$* Q " ?= ""$

<+  *      MO M&<   AO y
sigma bond ( σ,σ*): GK L  1-lobe  Aos z (head-on overlap) x σσσ bonding σ antibonding
pi-bond ( π,π*): GK L  2-lobe  AOs 2s orbital
GK LK+   A  B (side-on overlap)

πππ bonding πππ antibonding πππ bonding
delta-bond ( δ,δ*): GK L  4-lobe  AOs

A(p ) B(p ) A(s) B(s) A( s) B(px) x x A(py) B(py) A(s) B(py)

δδδ bonding 47 48

8 Q "
* Molecular Orbital Diagram*

~~ Q$
  " ?_ ""$ L ZZ 
Sigma antibonding (σ*)
Pi antibonding (π*) "  
 MO   
 AO
AOs [ " KLO  •  O [S  AMO (E 
) •  " [S  BMO (E ) E >>> E >>> E
Sigma bonding (σ)
Pi bonding (π) AMO AO BMO
P AO  GK L EAMO EAO EBMO
"P*GK LM&  


s+s px+px py+py σ > π > δ

49 50

Q$
  " MOs*
  ES" ;" " AO„s

AOs Q$
 T 
AOs Q$
 T 
Sigma bonding
Pi bonding E > E > E E > E > E > E AMO AO BMO AMO AO-H AO-L BMO s+s py+py • • ∆Ed: destabilization energy AMO g $S  AO-H • • ∆∆∆Es: stabilization energy BMO g $S  AO-L

px+px

y Q " ""$ ‚!$  ES" x AO: Atomic orbital  ;" " AO BMO: Bonding Molecular Orbital z AMO: Antibonding Molecular Orbital 51 52

Molecular Orbital Diagram  $g_"F"# MOs

σ 2 σσσ 2 σσσ 2 πππ 4 πππ 4 σσσ 2 EE--configurationconfiguration: ( 2s) ( 2s*) ( 2px) ( 2p) ( 2p*) ( 2px*) 1. "*[q
 G+  _  2.   MO    _ S S  2    "   3. [   _ *"* MO  
 O "$  4. P MO 
*K[ )†$ + E n e r ner gy E 5. [O  _ * MO Z [O  _   [  "
 6.  !   _ O        +  N  σ, π, δ, σ*, π*, δ*

53 54

9  $g_"F"# MOs "Q$
(Bond order)

H2 molecule
He2 molecule
 
LO _ 
!  + KL"P ! $ !  <[[O  _ * Antibonding

Antibonding BMO  AMO •  
 = ½ (  _ * BMO |   _ * AMO) • ! $    
"<[ "P 
 H1s H1s

He1s He1s

Bonding Bonding

+ – 2 2 σ 2 H2 H2 H2 H2 = (σσσ1s) He2 = (σσσ1s) (σ1s*) Bond energy = 431 kJ/mol (K 2 )  
 : 1 0.5 0.5

55 56

MO Diagram of Li2 & Be2 MO Diagram of N2 & O2

 q
 valence electrons
( q
 valence electrons) i
L 2 (2 x 3 electrons)
e B 2 (2 x 4 electrons) N2 ( ) O2 • Li = 1s2 2s1 • Be = 1s2 2s2 • N = 1s2 2s2 2p3 • O = 1s2 2s2 2p4 • Bond order = 1 • Bond order = 0 (no bond) •  
 = 1 •  
 = 2 •  "  +  σp  πp • • N $8 MO ?+. B2 : C2  O  MO  E n e r r gy ne E E n e r ner gy E

σσσ 2 σ 2 σ 2 σ 2 σ 2 σ 2 σ 2 MO of Li2 ( 1s) ( 1s*) ( 2s) MO of Be2 (σ1s) (σ1s*) (σ2s) (σ2s*) σσσ 2 σσσ 2 πππ 4 σσσ 2 σ 2 σ 2 σ 2 π 4 π 2 MO of N2 ( 2s) ( 2s*) ( 2p) ( 2px) MO of O2 (σ2s) (σσ2s*) (σσ2px) (ππ2p) (ππ2p*) 57 58

$ TF " ?_ 3. ef
 E (Valence Bond Theory)

6Q"(Diamagnetic)"  [O  _ " M&  ef
 E (VB) L'()  *  
! "  " K _  O ! $ Nv<+   +* ! 
[GK LK AO  

 (Paramagnetic) "    _   O*K   <*K
!  +   
 L   M < " K _ O    _ K  • AO 489$8=89.40!* "P"
!  + • *['() MO "P  organic molecule S  M&'() !"  "
GK L AO N$$ S
 (Bonding) & (
  σ,π,δ)
S* +      _  _  (  2   _ )* "
 G [K Z& K _ 59 60

10  Q
#ef VB  Q
#ef VB *


L[+      _  
ˆ‚KL[ !"! GK L AO

[[    _ * 
[[    _ * + 1s 2s 2px 2py 2pz • − − − − − 1s 2s 2px 2py 2pz H =    _   1 AO [ 1
 • C = − − − − −    _   2 AO [ 2
 • N = − − − − −    _   3 AO [ 3
 • O = − − − − −    _   2 AO [ 2
 • F = − − − − −    _   1 AO [ 1

!"  ˆ‚K • C = − − − − −    _   2 AO [  2
? • +[
S  "
&

!  +[GK L AO     _   • H2O [ v+  $
 90° ([ L 104.5) H− H N≡ N • H2 • N2 O H F• H H− F H

61 62

6†$6QE (Hybridization)* 6†$6QE (Hybridization)

P
[  _ * 2s +P< $M&S  2p O*K
$   S 6†$Q""$ L Z"    [O AO     _  M& +  * 
L"+  $ *K  <   1s 2s 2px 2py 2pz
 
L*K"P "
S  M& • C = − − − − −    _   2 AO [ 2
 • S† S G [ S _ L 
  " AO  T • C = − − − − −    _   4 AO [ 4
 #S  
 

&" +KL$ • +  *K   S† +  (Hybrid orbital) ♦  =T Q$
 T T  T 
  &" Š+  &"  (s px py pz) [Z" N +  *K   S† S G  S S† +  4 • [OS† +  =   +     
   v  1s sp3 CH4 p Hybridization • C = − − − − − 3 s sp ""$ " "" 6†$Q""$ " "" 63 64

Q " 6†$Q""$ sp 6†$Q""$

 S† +  M&  [O AO  Z" sp-Hybridization LZ"K • sp  2 ""$ (Linear) s-orbital  p-orbital • sp2  3 ""$ (Trigonal planar) <S† +  [ 
S  sp-hybrid orbital 2 +  • sp3  4 ""$ (Tetrahedral) [ p +  [  N"  • sp3d  5 ""$ (Trigonal bipyramidal) π 3 2
p-orbital  K L[
 • sp d  6 ""$ (Octahedral) 1 KL 2

[O
   S [O AO &K     _   (&+   S† +  ) 2 p p p py pz
S† +  (sp, sp , Œ) "P
G &*  x y z Hybridization sp +   (s,p,d Œ) "P
G  S
  ... s = 2 σ-bond = 2 πππ-bond 65 66

11 sp2 6†$Q""$ sp3 6†$Q""$ sp2-Hybridization LZ"K sp3-Hybridization  [ s-orbital  2 p-orbitals s-orbital  3 p-orbitals
S  sp2-hybrid orbital  3 + 
S  sp3-hybrid orbital  4 +  [  N "K  [  N " K
p-orbital  K L[
 π
S p orbital K L*K"
 π

p p p p x y z px py pz z Hybridization Hybridization sp3 sp2 s s = 4 σ-bond (,-$KT = 3 σ-bond = 1 πππ-bond p-orbital ;4!489$8=89.)

67 68

sp3 d  sp3d2 6†$Q""$  "T   S
?Q
6†$Q

 $*  3 M&S [*  d +  *S† 
 
Bes (1s22 2)
S  [ p  Linear 3 2px 2py 2pz 2p 2p H Be H
sp d Hybridization Hybridization y z 3 sp • 5 sp d hybrid orbitals 2s BeH2 • [  N
 <Š"K  3 2
Cs (1s22 22p2)
sp d Hybridization H 3 2 • 6 sp d hybrid orbitals Tetrahedral 2p 2p 2p • [  N  K x y z Hybridization sp3 C 2s H Cl H

CH3Cl 69 70

 "T   S
?Q
6†$Q
=T (Double Bond)

2 2 3

<  
sN (1s 2 2p ) Trigonal Pyramidal •
 sigma (σ) [ hybrid orbital • π 2px 2py 2pz N
 pi ( ) [ p-orbital Hybridization H sp3 H 2s H NH3 2 2 2
Os (1s 2 2p ) H Bent 2p 2p 2p x y z Hybridization O sp3 2s H

H2O

71 72

12
=T# H2C=CH2
  (Triple Bond)

<* H2C=CH2  

<   •
 sigma [ sp-orbital + •
 sigma (σ) [ hybrid orbital KL p-orbital •
 pi [ p-orbital + •
 pi (π) 2
 [ 2 p-orbital ♦ N≡N (3
 [ px py pz) ♦ ≡≡≡ + + + HC CH (3
 [ sp px py)

- - - + + + - - - + + + + + + ------

73 74

Coordinate Covalent Bond*
?$$g " "F"

?""Q?  (KL  dative covalent ! K [$ K K "< OS\\] S   *KN Z bond) L
!  +  [*   _  [ S   L P< " "S   KMK "  • " K  &NZ [
! K •
!+  !  + " KL
!  + • '()  "P*  
! KS   [O   $  O    _   '() P
 H2O Coordinate 1. $$g " "F" (Electron sea model) + H2O OH2 H H bond Al3+ +   "GM [$< [$





+ OH →





H2O 2 H N


H + H H N


H H N H H2O  G " G+  _  N N N H2O 3+  L S  " H F H2O OH2 H





F H F •





+ Al
! K [  M < K



→



H N


+


B F H N B F H N B F H O OH





2 2   _  " [$ N F N F N F H2O 75 76

ef u$
  (Energy band theory)   T ?_ (Intermolecular Force)

 AO [S +  ! $ 
 (bonding) +  ! $  
 (anti-bonding)
K! $ L M K S\\]K! $
L  M& [O+  ! $ M&  
[*  KL" [KLN P L  P
 (energy band) • Cohesive Force M K K! $   
  _ [
 S %* P KL L S*  + • Adhesive Force M K K! $      * P GK L&

! KOS\\]S L[  _ "P L S  "*L&! K   K! $ LP< $! Z P P&OS\\]KL P G+   < Type of Intermolecular Forces relative strength Ionic bonds Ions 1000

""$ x Hydrogen bonds Strong dipoles 100  ; T Dipole-Dipole Permanent dipoles 10 ""$ ;u= $g_FS London Induced dipoles 1

77 78

13   Q"   (van de Waals Attraction)
6†?Qg (Hydrogen bond)

  + "+L M K K! $ 
N K! $  &  K! $ GM [ S N   H   L   EN "<   •   [OK   _   F O KL N O*K! $  "%
&"< ! $  &GM S !
 ! $  M K  &    [ dipole- P (permanent dipole)   dipole interaction "Z *K" 
S†! [ [$  L  dipole-dipole interaction [$ K K "< δ δ+δ+δ+ •   K! $   & ! $ L S & P< δ+δ+δ+ δδ–
Boiling Point (°C) K O*K &   dipole-induced dipole interaction δδδ – δδδ – • • • K! $  S &  N K& K - H2O 100.0 • HF 19.5 Hydrogen bond • • δ+δ+δ+ δ+δ+δ+ O (induced dipole) KL&   (temporary fluctuation NH3 -33.3 H2S -60.7 δδδ – • HCl -85.1 ••• CH -161.6 δδδ – dipole)  L q
:"= (London Force) 4 δ+δ+δ+

79 80

$$ˆ‰Q $$ˆ‰Q

 !"  "! $ S S &
H2S
N2O • PH3 3-
PO4
NO2 • H2S H
N 3
BrF3 • lCH C 2 2
PCl5 F
P 5 • 3-
PO4 H C 2O F
S 6 • -
CH OH
BrO3 3 XeF4 • NO+
BeCl2
BrO2
OS 3 H
C 3CH2OH

81 82

14