CHAPTER I * ATOMIC STRUCTURE & BONDING
Fundamental Concepts
→ Atom is a basic unit of an element that can
undergo chemical change
electrons
protons neutrons
→
nucleus " "
Atomic number (2) =
protons Avogadro number
=
6-022×10 MOI
→
Atomic number (2) is the number of in the nucleus of an atom of an element
protons
→
Atomic mass (A) is sum of the masses of protons and neutrons in nucleus .
Atomic mass = Mass of protons t mass of neutrons
→
Atomic models → Classical mechanics
↳ Quantum mechanic
describe atomic & subatomic
electron have specified values of energy
e- may change but must make quantum jump
energy
A-B AA
Bohr 's Model wave mechanical models .
Pauli Exclusion Principle =
only one e- can
-
revolve around the atomic
-
every e- is characterised by >
Size have a
given set
¢ Shape of the & QN
parameters ; Quantum Numbers
nucleus discrete orbitals 4
Spatial
☒Spin
in -
orientation
+ orientation
-
e- quantiaed = have specific -
e-
position is considered to be the
energy values of e-
probability an
being various
change emery by quantum jump locations around the
-
nucleus .
LOOK AGAIN LATER ! ! !
Cn -
1)
[µ/ f
①"" " " " " " " "" ^ ° " "
n ↑ , orbital larger e- higher energy , ˢ
% I 2é
,
1<=1
→ n =
principal QN less bound to nucleus
tigthly
0
0 E- S E
→ e =
momentum ,
S
☐ ee
P
e ⇐ , p • e- 8
.m m =3 spzd , µ, µ, , ,
, , ,
,,,
me
→ . ,, ,
S P d
spdt-e-l-l-l.EE
→ Ms =
4ᵗʰ QN @ spin quantum number N=4 3
ˢ %¥%% I 3 :
f E- 145
Is
Electron
Configuration
<
<
2s 2p
↓ <
<
3s
4s 4p
3p 3d
4d Af
A
<
5s 5p 5d 5f 5g
Principle Hund 's Rule Pauli Exclusion Principle <
6s Cop Cod Gf 6g 6h
Fd
E goes into each e-
<
7s Zp 7-↑ 7g 7h Fi
lower energy orbitals every must have
-
- -
filled before higher States until all of number
are different quantum
orbitals them full
energy are
SP
3p64s23d ?
'
. . .
before pairing up ←
. .
_
$sÉ2s22p•3s3pp•4s23
3pᵗ3d'°4s*
- -
0M
DO
?⃝
Fundamental Concepts
→ Atom is a basic unit of an element that can
undergo chemical change
electrons
protons neutrons
→
nucleus " "
Atomic number (2) =
protons Avogadro number
=
6-022×10 MOI
→
Atomic number (2) is the number of in the nucleus of an atom of an element
protons
→
Atomic mass (A) is sum of the masses of protons and neutrons in nucleus .
Atomic mass = Mass of protons t mass of neutrons
→
Atomic models → Classical mechanics
↳ Quantum mechanic
describe atomic & subatomic
electron have specified values of energy
e- may change but must make quantum jump
energy
A-B AA
Bohr 's Model wave mechanical models .
Pauli Exclusion Principle =
only one e- can
-
revolve around the atomic
-
every e- is characterised by >
Size have a
given set
¢ Shape of the & QN
parameters ; Quantum Numbers
nucleus discrete orbitals 4
Spatial
☒Spin
in -
orientation
+ orientation
-
e- quantiaed = have specific -
e-
position is considered to be the
energy values of e-
probability an
being various
change emery by quantum jump locations around the
-
nucleus .
LOOK AGAIN LATER ! ! !
Cn -
1)
[µ/ f
①"" " " " " " " "" ^ ° " "
n ↑ , orbital larger e- higher energy , ˢ
% I 2é
,
1<=1
→ n =
principal QN less bound to nucleus
tigthly
0
0 E- S E
→ e =
momentum ,
S
☐ ee
P
e ⇐ , p • e- 8
.m m =3 spzd , µ, µ, , ,
, , ,
,,,
me
→ . ,, ,
S P d
spdt-e-l-l-l.EE
→ Ms =
4ᵗʰ QN @ spin quantum number N=4 3
ˢ %¥%% I 3 :
f E- 145
Is
Electron
Configuration
<
<
2s 2p
↓ <
<
3s
4s 4p
3p 3d
4d Af
A
<
5s 5p 5d 5f 5g
Principle Hund 's Rule Pauli Exclusion Principle <
6s Cop Cod Gf 6g 6h
Fd
E goes into each e-
<
7s Zp 7-↑ 7g 7h Fi
lower energy orbitals every must have
-
- -
filled before higher States until all of number
are different quantum
orbitals them full
energy are
SP
3p64s23d ?
'
. . .
before pairing up ←
. .
_
$sÉ2s22p•3s3pp•4s23
3pᵗ3d'°4s*
- -
0M
DO
?⃝
