Summary
Summary - Unit 2 - Bonding and Structure
- Institution
- PEARSON (PEARSON)
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BONDING AND STRUCTUREof attraction
IONIC BONDING-strong electrostatic force
ions
between oppositely charged between
wo
COVALENT BONDS-strong electrostatic attraction
doesn't show
tions
me are mobile of electrons between then
nuclei and the shared pair
edge of the ion
↑ live aion is no Of e-
energy
f
-
more
shared
difficult to measure Hive carion required stronger force sum of atanic
Fedva
↑
ionic radius
f smaller ions i
cathode ↑ -
mode
of attraction
e
repulsion between
the
pairs surrounding
I
-
electron properties of - central arou
shape
ausing
a
<
migrain high charge
high melting >
-
greater e-density -
· >
electrons
- points Y
IONIC between
:
strength
↑ apans
increased change
↓ BUNDING densing shared e-pair come from
am doubeasa
only one of the banding
e-density falls to zero
tive ions are smaller aroms
between ions
EVIDENCE FOR - t
f
IONS
Y
Ioni than their dative covalent
RADII
separate
7 - - banding
arans
L ↳ e
. Als
+
.
g
t greater band
!
physical N3-
↳ ordinary
high melling
increases down
strength COVALENT shape
I properties me group
↓
Oneless
,
five ions are
BONDING
!
!
points
-
examples
same shape
/
↓
S
larger than their
Pi and Signa -
a
↓
smong attractice
E
- banding
atoms ~
nuclear
brittle ↓ electrostatic force
iOnS W
↓ no e-) no. protons
of attraction
increases
2
Pitt bonds
sigma 6
.
small force
ion ↓ ↓ bands
↓
can't conduct
e .
g .
moving one
held
↓
ions are
diameter respective to pull of nucleus overlap of p-orbitals
electricity are shared more
closely and
AlCI + AlC >
-
AlzCs
another layer over more
orbitals lying above
when solid overlap of dimer
↓ e- below the ceries of
↓ lying between the
ionsle
I -
arons
8
like charges centres of atoms
less attraction
will be adjacent 6
Der e-
SS
fixed and repel
0 + 0 - 00
conduct S P 6
-
act arlita
F-
when molten or 0 + os
dissolved
& +-
p6
-
↓
overlappinone To*
ELECTRONEGATIVITY-ability
in a covalent bond
of an atom to attract the
bonding o · Al
higher
boilinga
↑
Y
I
I
↓ shielding
stronger than
↓ valence e-
London forces
distance
from
↑
the
nucleus
between
polar molecules
&
M
asymmetrical
- -
act in PERMANENT
addition to
no. protonst
-
DIPOLE-DIPOLE FORCES I D
London e .
.
g
atomic radiit closer valence
e- are
FX --- H FT
H
-
forces
-
to the nucleus -
⑧
- ①
-
↓ ALWAYS pais
show lone
significant difference
POLARITY nelectronegativity
LON
n
active &
sep
the angle between a
covalent bond is always
POLAR COVALENT BOND -
unequal 1800
distribution of e-in bond
a
creating
g
charge separation (dipole Must have
a occur betw
available love simple
pair of e-
↑ alcohols,
carboxylic
between H acids , proteins and ,
and , F , 0
N < HYDROGEN >
- anides can all
SYMMETRICAL MOLECULES :
f BONDING
H-band
dipoles
-of individualbond
conco use 2
g NU3 He O HE
higher
. .
,
~
,
.
e
. polar (Cly
g
us non-polar Ch3( water ca
I chance of
t
form t o hydrogen can cause
anomalously dipoles to
bonds per high boiling points
Fo
Molecule
↓ paise-
lane ↓ I
in ice molecules general
hydrogen bonds act
are held
further increase
in addition
Lo
apart by hydrogen
bonds ↓ Landon forces
& more e-
low
density
↓
METALLIC BONDING-strong electrostatic attraction between
increased
metalians and delocacised e- London forces
↑ delocalised
strength
require lots of ↑ protons strength A
&
M
energy to break no .
of decocalised
e-per alon
no of
↑
.
protons
the less soluble
↑
bands
strong electrostatic form new
it is in wave
size metal ions and bands
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