This document contains notes on intramolecular forces and intermolecular forces from the IEB SAGS document. It also includes all the IEB definitions from the SAGS as well as detailed explanations on all the concepts in this section.
" a molecular bond (bond between atoms within molecules )
ionic bond
mega , , , , ☐on ,
1. Valence electrons ( group number )
>
electrons in the outermost
energy level of an atom
Aufbau diagram
3s
%
} 5 valence electrons electron
configuration
:
1522522ps 353ps
Zp
25
Is
2.
Valency
>
amount of electrons gained / lost / Shared to complete the outermost energy level
number of bonds an atom
•
can form
non -
metals
3. Covalent bonds :
bond which occurs between 2h atoms which share at least one pair of
electrons
> non -
metal atoms
> outermost orbitals overlap so unpaired electrons can be shared
attraction between electrons and
positively charged
>
negatively charged nuclei
( equal sharing of electrons )
pure covalent bond ( non
pdar# symmetrical distribution of charge
-
>
electron pair is
equally shared between the atoms (2 atoms of the same element )
>
tendency of
electronegativity is a measure of the an atom to attract a
bonding pair
?
lone pairs are pairs that do not take part in the chemical
bonding process
i
>
t
- -
>
- -
- -
, The
electronegativity (pauling ) scale
decrease down and increase across a
electronegativityes
-
>
a
group
a period
>
factors contributing :
1. The
charge on the nucleus (9 charge ,
T attractive force
,
P electronegativity /
2. The size of the atom ( t size ,
closer the nucleus is to the electron
pair T electronegativity
,
/
Polar covalent bonds →
unequal sharing of electrons leading to a dipole forming
(as a result of electronegativity difference,
is not shared
equally
>
bonding pair
( bigger pair closer )
>
different electronegativity values value pulls electron
> uneven distribution of charge
•
higher electronegativity value has a
slightly negative charge (
8- )
lower
electronegativity value has a
slightly positive charge (8-1)
•
.
'
St
8-
-
+ CI >
-
CI > -
CI
2, I 3,0
Dative covalent bonds
>
forms when a lone pair of electrons from one atom is shared with another atom which
empty orbital
has an in its outermost
energy level
Ammonium ions ( NHI)
>
formed when a
hydrogen bond ( Ht ) forms a dative covalent bond with an ammonia
molecule ( NH 5) +
+ -
-
^
. . - i
i
.
-
+ -
. : -
> -
: - - .
-
. . . .
- -
-
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