1. OXYGEN,
SODIUM AND
PHOSPHORUS

2. I would be talking on the
following points
•Defining the element
•Some chemical and physical properties
•The element in the periodic table
•Uses/ biological role of the element
•Isotopes of the element
•Some interesting facts.

3. Each element is given a unique chemical symbol. The same
chemical symbol is used all over the world. The first letter is
always a capital letter. If in case there is a second letter
also, it is a small letter. These chemical symbol always come
from either their Greek, Latin or English names. The symbol
for :
•Oxygen is “O”
•Phosphorus is “P”
•Sodium is “Na” which derived from its Latin name Natrium .
CHEMICAL SYMBOL

4. ETYMOLOGY
•OXYGEN: The word oxygen arrived from a Greek word “oxy”
meaning ‘a sharp acid’ and “gen” or “genes” meaning ‘formation’ as at that
time it was mistakenly thought that oxygen is an important constituent in
the formation of acids..
•SODIUM: The symbol of the sodium element is Na which comes
from the Latin name for a common sodium compound called natrium from
the Greek word 'nítron‘ meaning a natural salt.
•PHOSPHORUS: The word Phosphorus originates from the
Greek words “phos” meaning light and “phoros” meaning bearer creating
the term ’bringing light’ as phosphorus white phosphorus oxidizes in air
and glows in the dark.

5. ATOMIC NUMBER
Each element is given an atomic no. Atomic
no. is the no. of protons and electrons in
the atom.
 The atomic no. of oxygen is 8.
 The atomic no. of sodium is 11.
 The atomic no. of phosphorus is 15.

6. The elements in the
periodic table

7. OXYGEN
 Oxygen has 6 electrons in its
valence shell, hence it lies in the VI
A group in the periodic table.

8.  Sodium has 1 electron
in its valence shell, so it
SODIUM lies in the I A group.

9. PHOSPHORUS
 Phosphorous has 5
valence electrons, and
thus lies under the V A
category of periodic
table..

10. STATE
Each element is defined as a solid liquid or a gas at
the normal room temperature. These are the states
of matter. The following are of oxygen, sodium and
phosphorus:
•OXYGEN: oxygen occurs as a gas at the normal
room temperature.
•SODIUM: sodium occurs as a solid in the room
temperature.
•PHOSPHOROUS: it is a solid at normal room
temperature.

11. PROPERTIES
Chemical properties Physical properties
 How an element reacts  Related to its appearance
with other elements.  Odour, density, colour and
 Change in the inner shape.
structure (atomic
structure).

12. OXYGEN PHYSICAL
PROPERTIES????
CHEMICAL
PROPERTIES????? OXYGEN

13. WHAT IS OXYGEN????
 Oxygen can be referred
to as an essential
gas, colourless and vital
for life.
 It is the most abundant
element .
 Oxygen constitutes 21%
of the atmosphere.
 It is also found in
water(as a constituent of
water molecule), rocks
and minerals and many
organic compounds.

14. PHYSICAL PROPERTIES
 Oxygen can change
from gas to a liquid at a
temperature lesser
than -218.4 degree
Celsius, that means its
melting point is -218.4
degree Celsius. It can
then be solidified. Solid
oxygen has pale blue
colour.
 Colour : colourless.

15. PHYSICAL PROPERTIES
 It is tasteless and
odourless.
 Phase : gas
 Density : oxygen is denser
than air, with a density of
1.429 g/cubic cm.
 Conductivity : it is a poor
conductor of electricity and
heat
 Solubility : it is slightly
soluble in water alcohol
and some other liquids

16. CHEMICAL PROPERTIES
 Flammability :It does
not burn.
 It supports combustion
but does not burn.
 It forms some very
common compounds
with hydrogen (water),
ferrous (rust/ iron
oxide), carbon ( carbon
dioxide).

17. CHEMICAL PROPERTIES
 Formula :the formula
for oxygen is O2. It is in
its molecular form to
make a stable
configuration. Ozone
gas is O3.

18. OXYGEN, A NON-METAL
 Each element is
categorized into groups
on the basis of some
properties. Oxygen is in Pure
substance
the Non-Metal group.
 Non metals have these
properties: elements compounds
• Poor conductivity, good
insulators, non-
metallic, exist as metals Non-metals --
solids/gases at the room
temp.(EXCEPTION IS
BROMINE).

19.  Naturally occurring
oxygen is composed of
three stable isotopes, with
a total of 4, 16O, with 8
neutrons 17O, with 9
neutrons and 18O, with 10
neutrons, 16O being the
ISOTOPES
most abundant (99.762%
natural abundance).

20. BIOLOGICAL ROLE, USES
 Respiration: oxygen plays an important infact the most
important role in aerobic respiration. Glucose breaks
down into energy, carbon dioxide and water in the
presence of oxygen.

21. BIOLOGICAL ROLE, uses
Oxygen cylinders are used a high altitudes by the
mountaineers, during space expeditions by the astronauts and
by deep sea divers as their supply of oxygen.
ABOUT 61% of the body is made up of oxygen.
IT is used in the production of steel from the iron ore(55% is
O2)
Oxygen is used in diseases like bronchial
asthma, anemia, trauma(chest injury).
Oxygen is also essential to decay. The process of decay is really
a kind of oxidation, but it will only take place in the presence of
bacteria.

22. OXYGEN, A HAZARD
CUMBUSTION: combustion is an exothermic
reaction in the presence of oxygen. It is referred
to, in general language as fire. Explosion and fire
take place in the presence of oxygen.
However, combustion is a useful process also.

23. SODIUM

24. WHAT IS SODIUM????
 Sodium can be referred
to as a soft, light,
extremely malleable
silver-white metallic
element .
 It constitutes 0.002% of
the universe, 2.3% of
the earth’s crust and
0.14% of the human
body. It is the 6th most
abundant element on
the earth.

25. PHYSICAL PROPERTIES
 Phase : solid
 Density : sodium’s
density is 0.971 g/cubic
cm.
 Conductivity : it is a good
conductor of electricity
and heat.
 Solubility : sodium will
act disastrous if put in
water.
 Sodium is brittle.

26. PHYSICAL PROPERTIES
 Melting point: 97.8
degree Celsius.
 Colour : silver-white
 Boiling point: 552.9
degree Celsius.

27. CHEMICAL PROPERTIES
 Flammability : Sodium itself is
not flammable but when you
combine sodium with water it
produces to sodium
hydroxide which is extremely
flammable gas. When
introduced to a flame though it
turns the flame a bright yellow.
Sodium is not flammable, but
some compounds of it are.
 It forms sodium hydroxide
when reacted with
water, Sodium
Chloride, common salt, when
reacted with Chlorine.

28. SODIUM, A METAL
 Sodium is in the Metal
group.
 Metals have these
properties:
• Good
conductivity, malleabili
ty, ductility, sonority, e
xistence in the solid
form at normal room
temperature(exception
-mercury)

29. ISOTOPES
 20 isotopes of sodium are
known, but only 23Na is
stable. Also, it is the most
common sodium used.

30. USES
 Agricultural uses
 Medicinal uses
 Purifying molten metals
 Sodium Carbonate, Sodium Hydroxide – used in
soap, cleaners

31. PHOSPHOROUS

32. WHAT IS PHOSPHOROUS?
 A highly reactive,
poisonous, non-metallic
element, waxy
occurring naturally in
the solid state.
 It constitutes 0.0007%
of the universe, as
whole, 1.1% of the
human body and 0.99%
of the earth’s crust.

33. PHYSICAL PROPERTIES
 Phase : solid
 Density : 1.82 g/cubic cm.
 Conductivity : black
Phosphorous is a good
conductor of electricity and
heat.
 Solubility :it does not dissolve
well in water.
 WHITE phosphorous is white
in colour. Red phosphorous
varies from orange to purple
colour( due to its chemical
structure).

34. PHYSICAL PROPERTIES
 Melting point: 44.1 °C
 Colour : silver-white
 Boiling point: 280.0 °C
 It is a deadly poison.
 It glows in the dark.

35. CHEMICAL PROPERTIES
 Flammability : Flammability:
it is highly inflammable.
 White phosphorous is the most
reactive of the three allotropes
of phosphorous while
 It forms phosphates as a
constituent(of any compound).

36. Phosphorous, a nonmetal
 Phosphorous is in the
Non-Metal group.
 It is a brittle solid.

37. ISOTOPES
 Twenty-three isotopes
of phosphorus are
known, including all
possibilities from 24P up
to 46P. Only 31P is stable
31
and is therefore
present at 100%
abundance.

38. USES
 A well known use of red phosphorus is the safety match.
The red phosphorus 'safety' matches were invented by
fellow Gustaf Erik in 1855.
 Inflammable bombs.
 Fertilizers
 Steel production
 Pesticides

39. SOME INTERESTING FACTS
 Why does sodium explode in water??
 Sodium (Na; Atomic number: 11) is a highly reactive element
belonging to the alkali group. Since sodium has valency 1 i.e. it has
one lone electron in its outermost orbit, it is highly reactive in nature.
When sodium is added to water, the lone electron of sodium reacts
with the water and displaces H+ ion, thus forming NaOH (sodium
hydroxide). Since this is a highly exothermic reaction, the sudden
release of energy during bond reformation results in explosion.

40. We cannot survive even for 5 minutes without
oxygen.
Sodium was isolated by Sir Humphrey Davy in 1807.
Bones and teeth are 85% phosphorous.
Though is though a metal is isn’t extracted from any
ore but from rock salt and common salt it is isolated.

41. CREDITS AND
REFERENCES
•http://en.wikipedia.org/wiki/Oxygen
•http://en.wikipedia.org/wiki/Sodium
•http://en.wikipedia.org/wiki/Phosphorous
•http://www.webelements.com/
•http://www.youtube.com/watch?v=92Mfric7JUc
•http://www.youtube.com/watch?v=qYMbh-l-fRs
•Class 11 NCERT chemistry book-Part II
•And many more