chemistry
YOU CAN
DO IT
.
Done
by Fatima
:
Alameri
Shortest
between 2
*
distance
waves
frequency [u)
number of
Per
Seco ne
waves
④ wavelength
DO
the
that
pass
Yun [HZ]
it
"
from
org in
crest
& frequency
"
"
origin
NOT affect
to
OR
to
"
trough
amplitude
wave
Stthomas
Fength
→
frequency
Common
properties
f¥÷÷÷÷÷÷÷÷
⑦ transverse
waves
..
\
l
'
,
\
L
G
-
-
]
quantum
⑦ electromagnetic
could be
of
only
energy
or
Flame
When
radiation
emitted
quanta
in
"
discrete
units
"
.
test
.
metal
ions
arehe§pfsftTTd
-
exited
-
here
Y
Atomic Emission
÷÷÷÷÷÷÷÷÷÷÷÷÷÷÷f¥÷÷i
Atomic Absorption
spectrum
spectrum
:÷÷÷÷÷÷
""
-
when exited
energy
atom release their
.
"
the wavelength absorbed
=
Wavelength
"
emitted
102
Bohr 's atomic
-
L
model
⑧ ⑧
CAN & I
WILL
Ground state
the lowest
energy
level
Bohr represented each
* Quantum # of
orbital
expressed
orbit
n
each
by
"
by g.anthem
atom
farther from
"
the
gain energy
newdes = more
energy
"
number rn
Electron
:i
of the hydrogen atom
transitions
"
"
n
=3
Exited state
when
.
i:c:::÷÷÷:::
.
when the
limitations
of Bohr model
electron
.
.
1 Bohr’s model explained the atomic
.
emission spectrum of HYDROGEN.
when the
energy of the
electron release to
But he didn’t explain why other
elements have unique emission spectra.
:
n
=3
Bohr’s model seemed to prove that
Could have different energy levels.
But it didn’t explain why these specific
energy levels existed .
Bohr’s model identified the placement of some electrons.
But it didn’t explain why atoms behave the way they do
chemically.
Compare
electron
n
/
cloud
energy of the
release
to
1. 2
Louis de Broglie
any moving particle
Quantum
Whole
act
numbers
orbit the
like
of
machanical
electrons that
-
will
an
nucleus
wavelength
a
WAVE
atom
only
.
.
in
-
.
Heisenberg
you CANNOT
uncertainty principle
with
interact
or
measure
withoutdisturbingit.it
impossible
an
object
that it is
sates
velocity # position
the exact
particle
f
at
⑤ the only
the
quantity
be measured
for
pro billing
in
de
-
predicts
→
wavelength
wave
charters tics
)
a
.
can
I
occupy
to
.
I
②
-
-
I -1
.
constant
①Photon
interact
② Both veocity
MV
↳
that
-
equation
plank 's
I. =h_
✓
region
that all moving
Particles have
of
is :
②
Broglie
know
time
electron
an
certain
a
same
to
velocity
+
with
position
an
are
electron
at rest
modified
mass
Quantum
④
Machaut cat model
|made
Schrodinger
apply
on
⑤I
by
I
,
"
exepte
all elements
HYDROGEN
↳
s
-
%t
J's
•o
-
of
the equation give the probability
finding
electron
at
↳
given point
.
ma
q¥_E
jpg
Ig Dls
S
1. 2
orbital
atomic
-
90% probility to find
electrons closer to the
neucless ,
&
10% outside
.
arms
.
0
less
chance
!
)
Principle quantum
-
describe the
,
* as
you
energy
move
sublevel
# Ma
.
S
spherical
p
shape
dumbell
d
out
increase
-
⑧
relative
' " ""
F
4
number
f
.
the
size
µ)
Principle
Energy
energy
level
sub level
( )
n
How
the total
-
'
-
2
2
3-
3
4
4-
-
s
Sp
Spd
spdf
"
Ex :3
25
35
each orbital have only 2
3px,3py,3pz
4px,4pyx.4pz
(
-
Np
de
Forbis
d)
[
can hold
-7
-
the
Z
Px
orbits
oppiste
f
.
-
up to
/ Py /
]
2 electrons
[
Pz
"
P can hold upto 6 electrons]
"
+2
(sohu.is/-7dxy/dyZ/dxz/dx2-y/dz
a)
do
the electron
have to be
.
11 orbit
/¥
•
-
electrons
AO
4s
.
"
.
32=92
2py,2pz
Zpx ,
levels
energy
(X. y )
S
orbitals ?
""
①axiofP
"
of
amount
"
-
A
I know
can
each
electron
will
BET.sn: it
'
[
"
"
f- hold up to 14]
go
is::
orbitals
'
(p
]
hold upto 20
electron
configuration
-
←
arrangement of
Aufbal
from
the
electrons
principle
largest
less
to
come
befors
energy
* note
"
it
3d
have
4S
higher energy
'
.
- lowest
energy
d
electron configuration
highest energy
Hydrogen
* atomic number :
I
.
Electrons I
* Electron
configuration
*
*
outermost
highest
shell
energy her
:
orbital notation :
* Velence
→
*
Shell : 11
highest principle
* Blocks :
energy
S
b
because of
1501
:
I
:
2g
2-
the "
-
electron
electron configuration
of NITROGEN
④
orbital
notation :
FTII
Ipx
⑦ electron
configuration
When I
have d block
Vel ence shell
add dts electrons
to
get
shell
(highest
*
.
15 25
-
-
2py Zpz
②p3
\
Priciple energy
level
:
.
2
the Vel ence
.
⑦ Vetere
electrons
:
5
ceseuyons
④ electron
⑤ Block :p
dot diagram
:
N:
*i; ji i: :÷¥÷÷÷i
hydrogen
so
have
subtract
the electron
2 electrons
it
from
configuration
.
electron configuration of Neon
* electrons :
10
configuration :
25 2p6
* electron
15
*
-
-
Orbital notation :
'
* velence
Shell
:
2
* Valence electrons :
8
*Block :
P
* Nobad
[ He]
gas
"
* Electron
-
-
notation :
2ps
dot
:
:
-
structure
:
electron
*electrons :
* electron
17
configuration
15-25
-
* orbital
configuration
2ps
-
:
35
3ps
-
notation :
7¥
Px
Py
Pz
* velence shell :
3
* velence electrons :
7
* block
:
P
* herbal
[
Ne]
gas
35
-
notation :
3ps
*electron dot structure
:
:
÷,
n
.
of chlorine
Exceptaliens
of electrons configurations
4S
III
.
3d
IB
one
will
move
3d
to
If each
it
one
from 451
because :
of
d
will be
is
filled
Stable
If
.
CHAPTER
2
2.1
orgm°zed33k#.gowne↳,n,to4group
10 Antoine Lavoisier
metals
non
-
metals
earths
gases
.
÷
÷÷÷÷÷÷÷÷÷
H÷t
:i÷÷÷÷÷÷÷÷÷
3 ① Lothar Meyer
- •
2 ① John
Newlands
arranged 14
known elements
increasing
atomic
according
to :
mass
a
4 ① Dmitri Mendeleev
"÷÷
. . . ..
elements .
:::÷:÷::: ::::
am
Periodic law
elements
increasing
.
Period
#
atomic
.
.
#s÷÷÷÷:÷÷:÷÷÷÷
arrange
order of
!÷÷:÷
A
Wich is
eachapeayjgeds.hauediffJ.at
÷:*
+ the properties repeated
regular
in
:
.
symbol
-
↳
atomic
mass
.
interval
.
⑦
a
③
2. I
AM represent've
elements
group [2. 2) & [13-18]
I
* it show
#
wide
Physical
-
&
chemical
Mth transition
group
of
range
properties
.
elements
[3-12]
* inched the
2
row
below *
Metals
shiny
elements
,
that
are
good
conductors
of heat &
* Alkaline
*Alkali metals
-
elements
highly
in
reactive
group
electricity
I
exept
earth metals
the 2nd group
highly reactive BUT
hydrogen
.
Alkali metals
are
transition elements
Transition
* less
Inner
transition
metals
the 2
rains
metals
below the table
reactive
group
[3-12]
*
-
-
*
-
-
Nobat
group 18
very
gases
-
nonmetals
unreactive
Halogens
elements
higley
in
group
reactive
27
more
reactive
.
s
p
-
-
2.2
2
6
S&p
d- so
f- → 14
*
ighst-fnper.g.gl#eyel
"
they
are
blocks
representative
elements
:3
velence electrons
[group #)
"
15252153 ③p④
6
↳
I
group 16
highest
energy level
/ :/ :/ /÷ ÷÷
#
Highest Princip
E
level
#
l
2
terce
period
velence
electron
-
l
l
2
2
l
2
6
6
16
6
7
7-
Group
7
8
-
17
18
:
-
Elements
o
§
GROUP
the same
in
g
( en Ce
→
S
→
group 15
ve
have
similar
properties
.
electrons
d block
&
trans ti ons
-
the filled S
orbital
[se coned highest
the
is
example
4S
[1/2
→
[ D
n
is
highest
the
energy
level
)
metals
energy
level
.
-
:
3d
[I
]
to
-
]
electrons
How
•
example :
to know the velence electrons [group ]
of d
Add Cdts)
electrons
-
4
45
L
3d
2+41=6
f block
to
inner transition
metals
p
* to
know
the
f-
(n 2)
-
Example
:
Gs 4f
→
orbital
lanthanide
÷
[ actinide
S
S
p
d
f
2. 3
Radii
Atomic
*
radius
*
*
Atomic
(size of
half
radii
-
Singel
ar
-
plural
radius
]
the
It depend
atom
the distance between 2
of 2
youT.LT
on
the
type of bonds
metalInon metal nudie
identical bonded
atoms
metal bond
.
nonmetal bond
⑧
00
Howdoseoneaeomaeypeofaemi.a.b.nu
-
* Atom Size
is effected
by
closely
bonded
crystal
:
y
To T
-
lattice
the radius
in
-
to
a
neighboring
atom
Group
the electron clouds
.
overlap
is
one
I.at?I e:Ii sI:iIeesnebe:yeen
" " ""
bonded
.
trends
Fff
3
be
:c.ie:S: .
.
.mu?s:: : : :on.:.i: eas
.
•
G-
⑤ period
trends
FE
.
-
decreases
WHY?
I electron
&
increase
the
same
as
Protons
(
(
move
you
will
across
atractt
the electrons
effective nudie charge
electron
static
the period
force
.
[in
→
the
same
Wich will
.
half
*
is
.
],
shell
decrease
the size
.
atoms
.
Ionic
what
gain
is
or
ions
lose
Radii
.
?
electron
gain
⑥
↳
electrons
=
-
'
•
:÷ ÷: ÷→s¥*ef*÷ ÷ ÷ ÷
iii.
mitral
•
Cation
mental
*
atoms
,
the
their velence
to
have
the
Anion
lose
electrons
period
* non
behind e
9
neaves
no
bat
*
gas
* size
decrease
[less
]
because
is
.
in
"
"" "
their
more
electrons
①
non
Trends
""
: :÷÷÷÷
electrons
m¥
)
electrons
negative charge
:c
a
[gain
metals
-
metal
period
o
-
decrease
group
⑧ Trends
¥1
in
group
group
→
15-17
+
→
ions
-
ions
-
•
group
-
•
-
1-14
de
increase
15
-
17
dsgaion
.
sizes
how
many
electrons
C)CE et
Rule :
* Don't
Oct
=
8 electrons
ve
-
lose
3
or
gain
more
electrons
.
than
in
hence shell
.
the
Ionization
-
b
energy requires
to
remove
1 electron
[always in the
① group
ag.g tf
/
trend
-
high
ionization
energy
-
energy
-
higher
thehioenn.in?:tifnneneu7I?YP
holds the
,
more
will be
-
⑤ Period
* the
[So
-
→ low ionization
]
shell
outermost
trends
Group 18
electrons
energy
required]
has
ionization
highest
energy
.
-
increase
WHY?
""
""÷÷÷÷÷
"" " " "
"
* Seco need
-
ionization energy
energy required to remove the 2nd electron
higher than the first
* third ionization
energy
-
.
-
energy required
-
to remove the
higher than
3rd electron
the second
.
Electronegativity
b
[attract'o/shaving
Unit =
]
electrons
paintings
> electronegtivity > attraction
-0-0-0
x
①
It
×
-0
Cl
⑦
e
-0
Shane
① period
electrons
trends
si
-
increase
Group
trends
*
..
÷÷÷÷÷i÷÷:
Chapter
3
3. I
electron dot
chemical bond :
-
force
that holds 2
Boron example
or
① Got
more
→
by
atoms
.
[attract between atoms
ion
formation
→
no
to
have the
lose
electrons
:*
pseudo
no bat
gas
Fake
-
Getting
Stai
,
+3
configuration
-
blog by
:
.
.
* Non
gain
formation
ion
Anion
*
nearest
with +2
①
B.
]
ions
Negative
cation t
*When atom
or
-
metals
electrons
:÷÷÷÷:i::÷
" "" i
::
Chlorine → chloride
group
charge
I
+
2
+2
13
+3
18
O
I
:÷÷÷÷÷÷÷÷÷:÷
:
OCurrin
a
-
group
12-24
:
•
electron static force
:÷ ÷ ÷ ÷ ÷ ÷ ÷ ÷/*
Positive
structure
3. 2
:÷÷÷÷÷÷÷÷÷÷÷÷÷÷÷
① Ionic bond
electrostatic force that holds
oppositely charged
:÷÷÷÷
a
-
4
:
ONLY 2 elements
contain
✓↳
cation
+
Na
Anion
+
Cl
→
Nat
t
CT
t
energy
2. electron configuration
Is
[Ne]3
-
3. Orbitit
→
[ Ne] [ AD
-
Na
CI
II
17
+
energy
notation
f
.
④ is t
ti
t
+
Na
Oi Oi
Oi
7¥
(l
+
Qi Qi
octet
7iQ
Omi
I Na
4. Electron dot
Na.o
÷!
:
Ci
-
structure
→
[ Nat tf !! :]
:
-
+
energy
How
calculate the overall
to
total
charge
in
compound
=
charge
°
E×=
①
exchange
the signs
without
.
µ
②
[other
element
]t÷)
][
number
element
t
3Na(÷÷
)
+
d
3-3/2=0
overall
I
1Nms
-)
+
LED
j
µ⑦
H
.
3
( Naz N)
charge
is
Zero
Write the
Ex
of
ratio
elements
.
:
Na CI
AI Clz
Mg3 Nz
I :L
I :3
3: 2
lattice
Crystal
↳
3 dimensional
[
[
-
why
arrangement
ions
t
surrounded
ions
-
does
by
surrounded
crystal
it is effected
-
by
ions
-
by t
]
]
ions
depends
How
strongly
attract
parties
.
Physical properties
number of
" °"
q
shapes ?
-
is
"Z"
.
lattice
have different
-
of particles
↳ " ded
-
f Mg
Melting
Point
Ability
of
material
to conduct
-
depends
on
high melting
electricity
the
charged
freely
→
→
=
liquid
.
no
No
state
=
boiling
it
moving
conduct
good
particles
electricity
conductor
electrolyte liquid
=
require
amount
point
to
of
of
electricity
solution
conduct
that
electricity
.
is
large
a
energy
break the
bond
:
Solid
Point
lattice , because
mooring
particles
Example
boiling
-
&
hardness
crystal
ionic
strong
①
Energy
endothermic
exothermic
b
b
energy
is
absorbed
Formation
of
energy
compound
ionic
is
is released
always
→
exothermic
lattice energy z
energy required
*
to
separate 1
moi
of
ions
Whenever ionic compound
if it
is
absorbed
the
is
formed :
same
amount
it will break
apart
of
energy
released
to
Lattice energy
.
is effected
by
:
- *
Size of atom
[
ionic
radii ]
tonic
charges
[ cation &
anion
charges]
Small size
to
more
large charge
&
lattice
energy
more
lattice
energy
3.3
Formula
unit
the chemical formula
[represents
the
simplest
of
of
ratio
Oxidation numbers
d
compound
ionic
the ions
]
charge of monoatomic ion
[number of electrons transferred ]
.
① Formulas for
binary
ionic
compound
.
I
2 elements
* cation
Example
:
is
.
first
written
.
-
② potassium
and
from
K←,
charges
the
iodide
groups
-
exchange
"
not
Ks
Is
-
KIU
②
Cesium
and
Cs
Csz
nitride
ONLY numbers
the
"
charge
.
①Formulas for
polyatomic
ionic
compound
-
ion
of
Exampled
fare
② Ammonium
to
made up
more
table
and
than
2 atom
⑨ iPod 89]
phosphate
to
CCNH
)#PO4③
-
,
(NH ) ,
.
3
( POD ,
(NHu)zCpoDJ
② Calcium
is
chlorate
and
""
④@ 10550
(Ca)
.
.
( Clo )+z
,
¢a)CcloDzJ
[just exchange
numbers]
f Oxygen
-
Naming
an
Oxyanionb
.
An element (non
more
*
they
have
)
metal
oxygen
more
atom
d
with 1
or
.
than I oxy anion
.
me%ea.ggxe.no#.eateJi
Example
:
-
I
-
N0③
Nitrite
→
more
oxygen
-
N0②
I
Nitrate
→
less
o
xy
g#
Naming chlorine
* chlorine
1. the
can
oxy anion
form 4 oxyanion
greatest # of oxygen
3 2
.
.
chlorite
perchlorate
2
.
I fewer
than the
greatest
chlorate
fewer
.
.
4
.
the lowest
hypochlorite
one
① Naming
[
ionic compounds
the
name
Monoatomic
cation
cation →
Anion →
monoatomic
Example
Same
'
add
.
first]
name
'
ide
:
NaCl
banion
cation
-
Soudiide
* there
the
some elements
transition
in
who
metals
MORE THAN I
oxidation
have
number
.
Exempt
Fez Oz
Fe O
for
#
o
+10%0 Oxygen
electrons
f
Roman #
f
#
\o
f-
repnesintig
of
'
is in
So
group
we
16 , with
need
to
charge C- 2) ,
make
it
-
z
I
-
'
>
II
2 -
¥+1
-
g
"
Fe
1×2
3
-
4 -
-
z
O
l)oxide
s
-
G
-
7
-
111
IV
v
VI
ru
s
3. 4
metals #
but
Metallic bond
ionic
they share
some
properties
-
attraction between
metallic
electron
:
cation
for delocalized electrons
sea model :
(
metal atoms in
a
Valence electrons
metallic Solid
to
form
'
a
sea
share their
'
of electrons
JB
→
Metal
sea
cation
of
electrons
a
!÷÷÷:÷÷
:c
:
"
.
of metals
properties
1. Melting & boiling
* they
Wich
is
because the bond
2. Malleability
,
-
turn
into
sheet
is
STRONG
very
ductility
,
and
metal
"
-
be
as
a
wire
durability
-
-
flexible
"
points
high
very
are
.
strength
can
.
-
3. Thermal &
electrical
*the
of
movement
around
metals
metals
conductivity
delocalized
cation
good
.
electrons
makes
conductors
.
4. Hardness
*
very
as
hard
to
break
the number
increase
,
it
will be
.
of valence
more
electron
stronger
.
[delocalized]
⑤ Metal
mixture
Alloys
of elements
metallic
-
the properties :
*
a
different
result
of
properties
properties
heating & cooling
similar
metals
atomic
.
alloys
t
replace
.
-
Subtitutioual
-
that has
.
alloys
s
holes
of
size
/
lhterstital
[ interstices)
filled
with
atom
.
is
smaller size
Compare
ion
the
re
pal
if
external force
an
because
the
is
charges
added
is
the
same
metal
they
won't
nepal
,
but
the
shape
will
change
.
.