Chemistry presentations

Periodic Table

Groups
 Groups run vertically in the periodic table.
 They are numbered from 1 – 18.
 Elements in the same groups have the same
number of electrons in the outer energy level.
 their chemical properties are same.

Group 1 : Alkali Metals
 Contains : Metals
 Valence Electrons : 01
 Reactivity : Very Reactive
 Properties : Solids
Soft
Very reactive with water
Shiny
Low density

Group 2 : Alkaline-Earth Metals
 Contains : Metals
 Valence Electrons : 02
 Reactivity : Very reactive but
less reactive than
alkali metals.
 Properties : Solids
Silver colored
More dense than
alkali metals.

Group 3-12 : Transition Metals
 Contain : Metals
 Valence Electrons : 1 or 2
 Reactivity : Less reactive than alkali
and alkaline-earth metals.
 Properties : Higher density
good conductors of heat
and electricity.

Group 3-12 : Transition metals
Below main table
 Contain : The Lanthanide and
Actinide Series.
 These two rows are pulled out of
sequence and placed below the
main table to keep the table from
being to wide.
 Lanthanides - 58 to 71.
 Actinides – 89 to 103.

Lanthanides : Rare Earth Element
 Lanthanides follow the transition metal 57 Lanthanum
in period 6.
 Valance Electron : 3
 Reactivity : Very reactive
 Properties : High luster but tarnish easily.
High conductivity for electricity.

Actinides : Rare Earth Elements
 Actinides follow the transition metal 89 Actinium in
period 7.
 Valance Electrons : 3 ( but up to 6 )
 Reactivity : unstable
 Properties : All are radioactive
mostly made in laboratories.

Metalloids
 These elements have characteristics of metals and
non metals.
 Elements from groups 13-17 contain some metalloids.
 A zig-zag line that seperates metals from metalloids.
 Properties : They are ductile and malleable.
They are solid that can be dull or
shiny.
They conduct heat and electricity
better than non metals but not as
well as metals.

Group 13 : Boron Group
 Group 13 : Boron group
 Contains : 1 metalloid and 4 metals.
 Valence Electrons : 3
 Reactivity : Reactive
 Properties : solid at room temperature.

Group 14 : Carbon Group
 Contains : 1 non-metal,2 metalloids
and 3 ,metals.
 Valence Electron : 4
 Reactivity : Varies
 Properties : solid at room temperature.

Group 15 : Nitrogen Group
 Contains : 2 non-metals,2 metalloids,
1metal.
 Valence Electrons : 5
 Reactivity : Varies
 Properties : All are solid at room
temperature accept
nitrogen.

Group 16 : Oxygen Group
 Contains : 3 non-metals, 1 metalloid,
2 metals.
 Valence Electron : 6
 Reactivity : Reactive
 Properties : All are solid at room
temperature accept
oxygen .

Group 17 : Non-Metals
 Contains : Non-Metals
 Valence Electron : 7
 Reactivity : very reactive
 Properties : Poor conductors
React violently with
alkali metals to form
salt.
Never found un combined
in nature.

Group 18 : Noble Gases
 Contains : Non-metals
 Valence Electron : 8 (2 for he )
 Reactivity : Unreactive
 Properties : colourless, odourless
gases at room temp.
Outermost energy level
full.
All found in atmosphere.

Electronic Configuration
DIVYESH SONDARVA
SEMESTER– 3
ROLL NO – 37

Atom
 The smallest component of an element having the chemical
properties of element, consisting of a nucleus containing
combinations of neutron and
protons and electron.
 Electrons are bound to the nucleus by electrical attraction.
 Number of protons determines the identity of the element.

Structure of Atom

What is Orbital?
 An electron cloud having an energy state described by given
values of the n, m, and m quantum numbers.

Orbitals in Sublevels
Sublevel Orbitals electrons
s 1 02
p 3 06
d 5 10
f 7 14
g 9 18

Electron Configuration
 The way electrons arranged around the nucleus.
1s1
row no
shell no
possibilities are 1-7
7 rows
subshell
possibilities are
s, p, d, or f
4 subshells
valence e-
possibilities are:
s: 1 or 2 p: 1-6
d: 1-10 f : 1-14
Total e- should equal
Atomic

Three rules are used to build the electron
configuration:
Aufbau principle.
Pauli Exclusion Principle.
Hund’s Rule.

Aufbau Principle
 Electrons occupy orbitals of
lower energy first.

Pauli Exclusion Principle
 An orbital can hold only two electrons and they must have
opposite spin.
 Electron Spin Quantum Number (ms):
+1/2, -1/2

Hund’s Rule
 In a set of orbitals, the electrons will fill the orbitals in a way that would
give the maximum number of parallel spins (maximum number of unpaired
electrons).

Filling Order diagram

Orbital diagram for hydrogen
Orbital
Diagram for
Hydrogen

Orbital diagram for helium
Orbital
Diagram
for Helium

Orbital diagram for lithium
Orbital
Diagram for
Lithium

Orbital diagram for beryllium
Orbital Diagram
for Beryllium

Orbital diagram for boron
Orbital Diagram
for Boron

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