These notes compile grade 11 and grade 12 chemistry work from extra lessons, online videos and resources, various textbooks and more. These notes provide in depth summaries with explanations, examples, practice questions and more providing the only work you need to study for finals. I studied from ...
·
greater END = more polar
(not attached
more freely to single stom)
~
onic bonding :
the transfer of electrons usually from a metal (or immtim ions) to a non-metal (or polyatomic ions ) with electrostatic
subsequent
Attraction between cations and anions
* ions.
charged atom/group of atoms
.
· am
properties
:
·
exist as
crystalline solids of room temp .
·
cations & anions held together by strong electrostatic force.
forces
·
determined by electrostatic
lattice structure
large hence high B.P
ions in
of needed to overcome forces
btwn
amount
energy ,
·
do NOT conduct electricity when solids Cons locked in position -
don't move)
·
do conduct when molten/in aqueous solution (ions separated free flow of charge)
electricity to move cur rent
-
= -
·
dissolve in water.
readily
metal donates electrons to form a cation (t) & non-metal accepts electrons to form anion (1
forces
=
very strong electrostatic of attraction ; form giant ionic lattices
, Lewis notation :
·
hir 2 Li +" Liz
killm
oxide
~
·
electron on product side
e
+ze ↳
positive formed , e-given away
.
·
electron on reactant side
O + 2 - 26 ↳ ion formed
negative
.
C
+
+ 02- ↳
CaC
:
Covalent bonding :
a sharing of at least one pair of electrons by two non-metal atoms
forms molecules s
properties :
low M P B B . . .
.
P
not
readily soluble in water
.
do not conduct electricity (no movement of electrons
*
Non-Polar (Pure) Covalent :
an equal sharing of electrons
no difference in electronegativity btwn
·
atoms
* Polar Covalent :
an inequal forming last
sharing of electrons
leading to a dipole result of
electronegativity difference)
electronegativity : a measure of the tendancy of an atom to attract a bonding pair of electrons
NOTE i n :
liquid/solid must be forces btwn molecules
to be to one another otherwise would
causing attracted ,
move apart 3 become
gas
.
, *
Simplest Molecule :
diatomic elements : Iz , Bra ,
Cla ,
Ea ,
On , Na ,
He
Lewis :
Couper :
&
H * H H -
H
1) He
2) Oz : 0
=
0
·
Shape : linear
molecules .
·
non-polar
3) N2 & NN : NEN
4) (12 ** Cl -
Cl
nature of molecule
symmetry
yes
·
To
&
even distribution uneven distribution
of charge of charge
(non-polar (polar
i ↑
do not dissolve
dipole moments
cancelled
net dipole = c
electronegativity :
·
most =
Flourine
·
large --
negative ions small - >
positive ions
going down group Valence shell further from
·
,
value decreases -
nucleus3 filled orbitals boon
.
"
increasesacross periods -
share - unequally to form molecule/
transfer to form ions
-
>
-
equal sharing covalent bond
pure
=
>
unequal sharing polar covalent bond.
-
=
>
transfer ionic bond
-
:
.
increasing bond polarity
END : Mor or
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