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OXYGEN,
SODIUM AND
PHOSPHORUS
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.
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
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.
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.
The elements in the
  periodic table
OXYGEN




 Oxygen has 6 electrons in its
  valence shell, hence it lies in the VI
  A group in the periodic table.
 Sodium has 1 electron
           in its valence shell, so it
SODIUM     lies in the I A group.
PHOSPHORUS

 Phosphorous has 5
  valence electrons, and
  thus lies under the V A
  category of periodic
  table..
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.
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).
OXYGEN                     PHYSICAL
                           PROPERTIES????



CHEMICAL
PROPERTIES?????   OXYGEN
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.
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.
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
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).
CHEMICAL PROPERTIES
 Formula :the formula
  for oxygen is O2. It is in
  its molecular form to
  make a stable
  configuration. Ozone
  gas is O3.
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).
 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).
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.
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.
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.
SODIUM
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.
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.
PHYSICAL PROPERTIES
  Melting point: 97.8
   degree Celsius.
  Colour : silver-white
  Boiling point: 552.9
   degree Celsius.
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.
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)
ISOTOPES
 20 isotopes of sodium are
  known, but only 23Na is
  stable. Also, it is the most
  common sodium used.
USES
 Agricultural uses
 Medicinal uses
 Purifying molten metals
 Sodium Carbonate, Sodium Hydroxide – used in
  soap, cleaners
PHOSPHOROUS
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.
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).
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.
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).
Phosphorous, a nonmetal
  Phosphorous is in the
   Non-Metal group.
  It is a brittle solid.
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.
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
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.
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.
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

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O xygen, sodium and phosphorus1

  • 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.
  • 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
  • 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.