, WEEK 1 ATOMIC STRUCTURE
Atoms structure
, of atomsElements Atomic number Mass number
, , , ,
Atomic notation
Isotopes, The mass number Relative atomic mass Electron
, .
arrangement
building blocks of matter
Atoms Basic Electron lots of space .
Tiny
:
. :
,
cover
volume their orbits determines how
Atom structure :
no
of proton
=
no
of election big the atom is ↑
occupy
Proton (Positive Nucleus
charge) ( )
·
+
-
Neutron (No
charge) ↳ Locate in the middle of the atom
Almost the whole mass of atom
Electron
(Negative charge) 3
More aroundthe nucleus is concentrated in it
Electron shell
.
eg
↳
Carries electrons The mass number ⑬
Nazementa
3 Total protons & neutrons
-
-
· Mass number is
atomic number roughly
alwaysthe double the The atomic number ⑪
(Only first elements 20
↳ Number of protons/electrons
Building blocks of
Elements :
all matter.
carbon-12
.
eg
.
Isotopes Different forms of the same element
: VS
carbon-13
↳ same number of protons but a different number
of neutrons Most elements have different isotopes but one or two stable ones.
only ,
Different isotopes Reactivity
identical Different mass properties
↳
physicaldifferent
: =
,
slightly
Mass
Spectrometry Accurate instrumental technique usedto determine the
:
relative
isotopic mass & the relative abundance of
each
isotope. Stage Vaporization Ionization Acceleration
Deflection Detection
G
:
O
&
⑤
③
O Converts
sampleto gaseous stage.
:
②:
Vaporized sample bombarded with electrons,
B creating positively charged
kinetic
ions.
faster than heavier ones
energy, lighter
:
Ions
gaining ions
movingratio
same -
④Ions
⑤
separated based ontheir
mass-to-change
.
Separated ions hit detector informationthen processed to generate a spectrum
:
a , mass .
Relative Atomic Mass (Ar)
Calculating
Average weighted for isotopes
mass . (mass num of
No need to addTo
isotope x
in calculation
Abundance (9) t ...
100
. In
eg What is the Ar of boron?
"B
a
sample of boron ,
20 %
of the atoms are "B and 80 % are .
, If there are 100 atoms then ,
20 atoms would be "B and 80 atoms will be
"B
(20 x 10) + (80 x11)
&
Ar of Boron =
100
= 10 .
8/
In
sample of 79 0% of the atoms are* Mg
magnesium magnesium
eg a
. ,
, .
26
are and 11 0 % are Mg
10 0. %
Mg
is the
.
.
What Ar of ?
magnesium
If there are 100 atoms the 79 , ,
10 ,
and 11 atoms would be
"4Mg "Mg . ,
and
"My respectively .
(79x24) +
(10 x 25) + (11x26)
Ar of Magnesium
=
100
=
24 32/ .
Electron
Arrangements / First shell <x
.
n= 1
& Electron shell
L
capacity vs
Electron
Arrangemento YXElement y**
Second shell . n= 2 The octet rule
eg
.
2 8 8
,2
?
7
.
why
, ,
XX But outer electron should
The
Maximum number of electrons &
2n2 be 8/2 electrons to become stable
.
eg n = 1 (First shell) .
2 .
1
2
= 2 so eg Iron (Fe) is 2 8 14
. , . ,
n= 2 (Secondshell) .
2 2 .
=
S
Duplet Rule .
(Third shell) 32 18 Octet
n =
3 .
2 .
= is
usually more stable than
duplet.
, WEEK 2 MEASUREMENTS & CALCULATIONS
Measurements & Units (SI) Derived units Temperature scales The mole
Elementary entities Molar
-
, , . , ,
mass Molar volume of
gases, Ideal gas equations Empiricalformula
,
,
but not
identicate
Mass
Weight
: Measure
:
Measure
of the
of the
quantity of matter it contains
gravitational pull it experiences .
[Proportional
Density Mass/volume Number carbon-12
mole
exactly 12g of of atoms
=
1 =
in
Mole Unit amount :
of of substance/Measurement .
of chemical amounts
Calculation of Mole
+103
Avogadro's constant 6 02 For mole calculations.
=
.
Fez0s + 3C0- 2Fe +
3CO2 Number of entities = Num of moles x (6 02 x103)
eg
.
.
=
3 molesmoles moles
-
1 mole Relative Formula Mass (Mr) eg CO2 :
Mr = 12 +
(16 2)
+
.
Number of moles =
Mass/Mr Mass =
Number of Moles x
Mr
(grams)
Ideal Gas Equation : Relates pressure volume number of moles and
, ,
temperature for a gas.
this law under all , Gas contant 8 315K "mot"
that
obeys
:
A .
gas
conditions is called ideal PV nRT
Temperature (Kelvin)
/g
= -
-
Pressure(Pa) Volumn (m3) Number moles
of
Empirical Formula Simplest ratio of : constituent elements in a
compound
7
Y
Molecular
formula ?
What's this ?
Needs to resite the first 20 -
elements
Atoms structure
, of atomsElements Atomic number Mass number
, , , ,
Atomic notation
Isotopes, The mass number Relative atomic mass Electron
, .
arrangement
building blocks of matter
Atoms Basic Electron lots of space .
Tiny
:
. :
,
cover
volume their orbits determines how
Atom structure :
no
of proton
=
no
of election big the atom is ↑
occupy
Proton (Positive Nucleus
charge) ( )
·
+
-
Neutron (No
charge) ↳ Locate in the middle of the atom
Almost the whole mass of atom
Electron
(Negative charge) 3
More aroundthe nucleus is concentrated in it
Electron shell
.
eg
↳
Carries electrons The mass number ⑬
Nazementa
3 Total protons & neutrons
-
-
· Mass number is
atomic number roughly
alwaysthe double the The atomic number ⑪
(Only first elements 20
↳ Number of protons/electrons
Building blocks of
Elements :
all matter.
carbon-12
.
eg
.
Isotopes Different forms of the same element
: VS
carbon-13
↳ same number of protons but a different number
of neutrons Most elements have different isotopes but one or two stable ones.
only ,
Different isotopes Reactivity
identical Different mass properties
↳
physicaldifferent
: =
,
slightly
Mass
Spectrometry Accurate instrumental technique usedto determine the
:
relative
isotopic mass & the relative abundance of
each
isotope. Stage Vaporization Ionization Acceleration
Deflection Detection
G
:
O
&
⑤
③
O Converts
sampleto gaseous stage.
:
②:
Vaporized sample bombarded with electrons,
B creating positively charged
kinetic
ions.
faster than heavier ones
energy, lighter
:
Ions
gaining ions
movingratio
same -
④Ions
⑤
separated based ontheir
mass-to-change
.
Separated ions hit detector informationthen processed to generate a spectrum
:
a , mass .
Relative Atomic Mass (Ar)
Calculating
Average weighted for isotopes
mass . (mass num of
No need to addTo
isotope x
in calculation
Abundance (9) t ...
100
. In
eg What is the Ar of boron?
"B
a
sample of boron ,
20 %
of the atoms are "B and 80 % are .
, If there are 100 atoms then ,
20 atoms would be "B and 80 atoms will be
"B
(20 x 10) + (80 x11)
&
Ar of Boron =
100
= 10 .
8/
In
sample of 79 0% of the atoms are* Mg
magnesium magnesium
eg a
. ,
, .
26
are and 11 0 % are Mg
10 0. %
Mg
is the
.
.
What Ar of ?
magnesium
If there are 100 atoms the 79 , ,
10 ,
and 11 atoms would be
"4Mg "Mg . ,
and
"My respectively .
(79x24) +
(10 x 25) + (11x26)
Ar of Magnesium
=
100
=
24 32/ .
Electron
Arrangements / First shell <x
.
n= 1
& Electron shell
L
capacity vs
Electron
Arrangemento YXElement y**
Second shell . n= 2 The octet rule
eg
.
2 8 8
,2
?
7
.
why
, ,
XX But outer electron should
The
Maximum number of electrons &
2n2 be 8/2 electrons to become stable
.
eg n = 1 (First shell) .
2 .
1
2
= 2 so eg Iron (Fe) is 2 8 14
. , . ,
n= 2 (Secondshell) .
2 2 .
=
S
Duplet Rule .
(Third shell) 32 18 Octet
n =
3 .
2 .
= is
usually more stable than
duplet.
, WEEK 2 MEASUREMENTS & CALCULATIONS
Measurements & Units (SI) Derived units Temperature scales The mole
Elementary entities Molar
-
, , . , ,
mass Molar volume of
gases, Ideal gas equations Empiricalformula
,
,
but not
identicate
Mass
Weight
: Measure
:
Measure
of the
of the
quantity of matter it contains
gravitational pull it experiences .
[Proportional
Density Mass/volume Number carbon-12
mole
exactly 12g of of atoms
=
1 =
in
Mole Unit amount :
of of substance/Measurement .
of chemical amounts
Calculation of Mole
+103
Avogadro's constant 6 02 For mole calculations.
=
.
Fez0s + 3C0- 2Fe +
3CO2 Number of entities = Num of moles x (6 02 x103)
eg
.
.
=
3 molesmoles moles
-
1 mole Relative Formula Mass (Mr) eg CO2 :
Mr = 12 +
(16 2)
+
.
Number of moles =
Mass/Mr Mass =
Number of Moles x
Mr
(grams)
Ideal Gas Equation : Relates pressure volume number of moles and
, ,
temperature for a gas.
this law under all , Gas contant 8 315K "mot"
that
obeys
:
A .
gas
conditions is called ideal PV nRT
Temperature (Kelvin)
/g
= -
-
Pressure(Pa) Volumn (m3) Number moles
of
Empirical Formula Simplest ratio of : constituent elements in a
compound
7
Y
Molecular
formula ?
What's this ?
Needs to resite the first 20 -
elements
