Chapter 4 :
Chemical bonding and structure
Forces
intramolecular forces intermolecular forces
(inside molecule (between molecules
-
ionic bonding -London forces
(metal-nonmetal) van der
XE > 1 7. Waals forces -
Permanent dipole
forces
-metalic bonding
(metal-metal)
-
hydrogen bondin
-
covalent bonding
I nonmetal-nonmetall
-E = 17 .
Electronegativity -
is an ability of an atom
to attract to electrons in a covalent bond
NaCl-sodium chloride-table salt
Na Nat Iss" Cp
15252635
I 15:25 2 po3s"3p5 111525 [poss" >ps
lonic bonding is electrostatic attraction
between oppositively charged ions
ODO-lattice
GDD
structure
,Topic : Lewis structures for compound and ions
Octate rule
H
NH3 5i
3 /
.
= 5)
3
n - Hil
S electrons 4 H
2
=
pairs
Nozt 5
je
3
=
t
2+ 6 12
(0 0]
=
17 --
e- = n =
=s pairs
-
not okay ,
be max, number
NO, 52
-
5
123
of electrons is 8
-
2 + 6e =
18e
=
+
17e e
= g pairs
(E -
N =
0]]-
Patie (co-ordinate) bonding
NHin H
I
H -
N1 H
+
u" proton
-
+
I
H
[H--H]
+
-
H- > H or or
n
↓
! CO carbon monoxide
ye
+=
IC = 01
5 pairs
, dative bond
E 5 pairs
C -g )
-2
- IC=
-
they share
one electron with each other
SO2
= 6 paira GE5 Q
=
03
/x
1 181
- El
BFz
P electron
t
ze
3 7 + =
21
-
24e
= 12 pairs IEI deficient (place for
a more electrons)
Icel
H
AlCl3
- IN -H ammonia donates
electron pair
↓
IFI
I
If-B1
-
IET
it =
BFn-
4) Work out Lewis structures
a . H2S t ze H H
-
Ge
Se- -
4 pairs
I
b .
PCI3 +
5e-
7x3 = 2/e-
-- II
26e-- 13 pairs @l
Chemical bonding and structure
Forces
intramolecular forces intermolecular forces
(inside molecule (between molecules
-
ionic bonding -London forces
(metal-nonmetal) van der
XE > 1 7. Waals forces -
Permanent dipole
forces
-metalic bonding
(metal-metal)
-
hydrogen bondin
-
covalent bonding
I nonmetal-nonmetall
-E = 17 .
Electronegativity -
is an ability of an atom
to attract to electrons in a covalent bond
NaCl-sodium chloride-table salt
Na Nat Iss" Cp
15252635
I 15:25 2 po3s"3p5 111525 [poss" >ps
lonic bonding is electrostatic attraction
between oppositively charged ions
ODO-lattice
GDD
structure
,Topic : Lewis structures for compound and ions
Octate rule
H
NH3 5i
3 /
.
= 5)
3
n - Hil
S electrons 4 H
2
=
pairs
Nozt 5
je
3
=
t
2+ 6 12
(0 0]
=
17 --
e- = n =
=s pairs
-
not okay ,
be max, number
NO, 52
-
5
123
of electrons is 8
-
2 + 6e =
18e
=
+
17e e
= g pairs
(E -
N =
0]]-
Patie (co-ordinate) bonding
NHin H
I
H -
N1 H
+
u" proton
-
+
I
H
[H--H]
+
-
H- > H or or
n
↓
! CO carbon monoxide
ye
+=
IC = 01
5 pairs
, dative bond
E 5 pairs
C -g )
-2
- IC=
-
they share
one electron with each other
SO2
= 6 paira GE5 Q
=
03
/x
1 181
- El
BFz
P electron
t
ze
3 7 + =
21
-
24e
= 12 pairs IEI deficient (place for
a more electrons)
Icel
H
AlCl3
- IN -H ammonia donates
electron pair
↓
IFI
I
If-B1
-
IET
it =
BFn-
4) Work out Lewis structures
a . H2S t ze H H
-
Ge
Se- -
4 pairs
I
b .
PCI3 +
5e-
7x3 = 2/e-
-- II
26e-- 13 pairs @l
