Physical and Chemical Classification of Matter

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Matter is classified based on its physical and chemical properties. Matter is anything that possesses mass and occupies space. Based on the physical state, matter is primarily classified into three types, namely, solid, liquid and gases. In solids, the particles are closely packed together. In liquids, the particles are loosely packed together whereas, in gases, the particles are very loosely packed. Based on chemical states, matter is classified depending on the chemical composition, namely, homogenous and heterogeneous.

Key Takeaways: Physical classification, Chemical classification, Matter, Solid, Liquid, Gas, Homogeneous, Heterogeneous.

What is Matter?

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Matter is anything that has mass and occupies space. In physical terms matter can be classified primarily into 3 states, such as,

  • Solids
  • Liquids 
  • Gases

Recent scientific study has added two more states of matter such as Plasma and Bose-Einstein Condensate.

In chemical terms, matter is classified into two types based on their chemical composition, such as,

  • Homogeneous mixture
  • Heterogeneous mixture.

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Physical Classification

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Physical classification is the most basic classification of matter. Physically matters are classified into 

  1. Solid State: Substances that are rigid and possess a definite shape. Examples: chair, book, pen, table, etc. 
  2. Liquid State: Substances that can flow and can occupy the shape of the container that it occupies. Examples: Water, kerosene, drinks, etc. 
  3. Gaseous State: Substances that can both take the shape and volume of the container that it occupies. Examples: Nitrogen, Hydrogen, Oxygen, etc. 

Physical Classification of Matter

Physical Classification of Matter

Here is a tabular description of the basic differences between solids, liquids and gases 

Solids Liquids Gases
Fixed Shape No Fixed Shape No Fixed Shape
Fixed Volume Fixed Volume No Fixed Volume
High density Moderate Density Low Density
Not capable of filling their container Capable of filling their container Capable of filling their container
Cannot be compressed Cannot be compressed Can be compressed easily
Cannot Flow Can flow Can flow easily
Particles are closely packed Particles are not as closely packed as solids Particles are loosely packed
The force of attraction between particles is strong The force of attraction between particles is not as strong as solids They have a very weak force of attraction between particles
Kinetic energy is very low Kinetic energy is more than solids Maximum Kinetic Energy

Chemical Classification

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Matters are classified chemically into two. 

  • Homogenous: Materials that have a uniform composition and identical properties throughout or materials that only have one phase. 
  • Heterogenous: Materials that have a number of phases whose different phases can be separated from each other by distinct boundaries. 

What are Mixtures? 

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A substance when it contains different matter in varying amounts that make up its composition is called a mixture. Mixtures can be separated using physical processes such as evaporation, condensation, sublimation, etc. Mixtures can further be classified into two:

  • Heterogeneous Mixture: These are mixtures whose constituent particles can be separated. For example, if we add sand to water, we can easily remove these two by just filtration process.
  • Homogenous Mixture: Homogeneous mixtures are those whose compositions are thoroughly mixed and take complex physical processes to separate. For example, sugar dissolved in water. 
Homogenous Mixture Heterogeneous Mixture
Components are thoroughly mixed thoroughly making them indistinguishable from one another. Substances remain separate and can be easily distinguished from one another.
No visible boundaries to help distinguish from one component to another. Clear visible boundaries making it barely an inconvenience to separate one component from another.
Uniform composition throughout the mass of the mixture No uniform composition throughout the mass of the mixture

Homogeneous and Heterogeneous mixture

Homogeneous and Heterogeneous mixture


What are Pure Substances?

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Substances that have a constant composition are called pure substances. All the components of the pure substance are composed of the same kind of particles and properties. For example, any sample of sucrose (sugar) will have 6.5% hydrogen, 42.1% carbon and 51.4% oxygen by mass. Any sample of sucrose will also have the same physical characteristics as well, such as colour, sweetness, melting point, etc. Pure substances are further classified into two: Elements and Compounds.

Elements

Elements are pure substances where it is impossible to further break down pure substances into simpler substances with the help of chemical changes. Some common examples of elements include gold, silver, iron, aluminium, oxygen, etc. There are about 100 elements that exist out of which about 90 are naturally occurring. All the elements are arranged according to their atomic numbers in the periodic table.

Types of Elements

Elements can be further classified into three based on their nature. 

  • Metals: A shiny, malleable, ductile solid which is capable of conducting heat and electricity. 
  • Non-Metals: Substances that are not malleable, shiny or ductile.
  • Metalloids: Substances that show properties that are between that of metals and non-metals. 

Compounds

Pure substances that can be further broken down into simpler substances using chemical changes are called compounds. Such breakdown can either result in the formation of either elements or other compounds themselves. An example of a compound is Mercury(II)Oxide. Mercury(II)Oxide is a crystalline, orange in colour solid. Using heat, it can be broken down into elements mercury and oxygen.

Types of Compounds

Compounds can be further divided into two categories. 

  • Organic Compounds: Organic compounds are matters that contain organic natural occurring substances like carbon, hydrogen, nitrogen, oxygen, etc. They can be obtained from plants and animals. 
  • Inorganic Compounds: Compounds that contain elements that contain something other than the known 114 elements. 

Classification of Chemical Substance

Classification of Chemical Substance


Atoms and Molecules

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  • Atoms can be referred to as the smallest particle of an element that may or may not be able to exist independently.
  • They exhibit the properties of the element that can participate in chemical reactions.
  • Atoms of iron, gold, silver, copper, etc. are capable of existing freely while the atoms of hydrogen, nitrogen, oxygen, etc. are incapable of existing on their own. 
  • Molecules are particles of an element that are formed using two or more atoms that are joined together by strong forces called chemical bonds. There may be two or more identical atoms in molecules as in those found in elements like hydrogen, oxygen, etc. and there may be two or more atoms in a molecule that are different as in the molecules found in water. 
  • Molecules that consist of a singular type of atom are called homoatomic or homonuclear molecules. Examples include sodium, oxygen, ozone, etc.
  • Molecules that are made of atoms of different elements are called heteroatomic or heteronuclear molecules. Examples include water, carbon dioxide, etc. 
  • Another division of molecules is done according to the number of atoms present in the molecule.
  • When the number of atoms in a molecule is one, it is called a monatomic molecule. Examples: Sodium, Magnesium, Iron, Copper etc.
  • When the number of atoms in a molecule is two, it is called a diatomic molecule. Examples: Oxygen, Nitrogen, Hydrogen, etc.
  • When the number of atoms in a molecule is three, it is called a triatomic molecule. Example: Ozone. Any molecule that has more than one atom in it is generally called by the name polyatomic molecule

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Things to Remember

  • Matter is anything that has mass and occupies space.
  • Physical classification of matter is solid, liquid, gases, plasma and bose-einstein condensate. 
  • Chemical classification of matter is heterogeneous and homogeneous mixtures.
  • Chemical substances can be classified into mixtures and pure substances. 
  • Pure substances are those which have a uniform chemical composition. These are further classified into elements and compounds.
  • Elements are pure substances which cannot be broken down into further constituent particles.
  • Pure substances that can be further broken down into simpler substances using chemical changes are called compounds.
  • Atoms and molecules are the smallest particles of an element.
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Previous Year Questions

  1. The temperature of 32C is equivalent to…? [MHT CET 2019]
  2. The IUPAC name of the compound having the formula is…? [JEE 1984]
  3. The hottest region of Bunsen flame shown in the figure below is…? [KCET 2016]
  4. The number of atoms in 4.25 g of NH3 is approximately…? [NEET 1999]
  5. 0.24 g of a volatile gas, upon vaporisation, gives 45 mL vapour at NTP. What will be the vapour…? [NEET 1996]
  6. 1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excess…? [NEET 2004]
  7. 1 cc N2O at NTP contains…?  [NEET 1988]
  8. The number of water molecules is maximum in….? [NEET 2015]
  9. A compound contains atoms of three elements A,B and C. If the oxidation number of…? [NEET 2000]
  10. 25.3g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250mL of solution. If sodium carbonate…? [NEET 2010]
  11. 6.02×1020 molecules of urea are present in 100 mL of its solution. The concentration of solution…? [NEET 2013]
  12. A 55 molar solution of H2SO4 is diluted from 1 litre to a volume of 10 litres, the normality…? [NEET 1991]
  13. A metal oxide has the formula M2O3. It can be reduced by H2 to give free metal and water…? [NEET 1989]
  14. A mixture of 2.3g formic acid and 4.5g oxalic acid is treated with cone. H2SO4. The evolved gaseous mixture…? [NEET 1989]
  15. A mixture of gases contains H2 and O2 gases in the ratio of 1 : 4 (w/w). What is the molar ratio…? [NEET 2015]
  16. The weighted average atomic mass of the naturally-occurring element X is closest…? [NEET 2007]
  17. An organic compound contains carbon, hydrogen and oxygen. Its elemental analysis gave…? [NEET 2008]
  18. The number of oxygen atoms in 4.4g of CO2 is…? [NEET 1989]
  19. Assuming fully decomposed, the volume of CO2 released at STP on heating…? [NEET 2000]
  20. At STP, the density of CCl4 vapour in g/L will be nearest to…? [NEET 1988]

Sample Questions

Ques 1. Classify the below substances into the categories, an element, a compound, a heterogeneous mixture or a homogeneous mixture. (2 Marks)
(i)Table sugar
(ii)Mercury
(iii)Salad dressing
(iv)White wine

Ans. The classification of the substances are:

  1. Table Sugar: Compound
  2. Mercury: Element
  3. Salad dressing: Heterogeneous mixture
  4. White wine: Homogeneous mixture

Ques 2. What are the major differences between solids, liquids and gases? (2 Marks)

Ans. The major differences are:

Solids Liquids Gases
Fixed Shape No Fixed Shape No Fixed Shape
Fixed Volume Fixed Volume No Fixed Volume
High density Moderate Density Low Density
Not capable of filling their container Capable of filling their container Capable of filling their container
Cannot be compressed Cannot be compressed Can be compressed easily
Cannot Flow Can flow Can flow easily
Particles are closely packed Particles are not as closely packed as solids Particles are loosely packed
The force of attraction between particles is strong The force of attraction between particles is not as strong as solids They have a very weak force of attraction between particles
Kinetic energy is very low Kinetic energy is more than solids Maximum Kinetic Energy

Ques 3. Analyse the difference between homoatomic molecules and heteroatomic molecules? (2 Marks)

Ans. The main difference between homoatomic and heteroatomic molecules are:

S. No.  Homoatomic Molecules Heteroatomic molecules
1 The molecules that are formed of only one kind of atom are known as homoatomic molecules. Molecules that are made up of various kinds of atoms are known as heteroatomic molecules. 
2. Example: H2, P2, N2 Example: HCl, NO2, CO2

Ques 4. Identify each of the below as a mixture, a compound or an element (2 Marks)
{i} Gasoline
(ii) Water
(iii) Air
(iv) Nitrogen
(v) Copper
(vi) Sulfur
(vii) Sucrose

Ans. The classification of the following are as follows: 

  1. Gasoline - Mixture
  2. Water - Compound
  3. Air - Mixture
  4. Nitrogen - Element
  5. Copper - Element
  6. Sulfur - Element
  7. Sucrose - Compound

Ques 5. What are the five states of matter? (2 Marks)

Ans. As per physical classification of matter, it is classified into solids, liquids, gases, plasma and bose einstein condensate.

Ques 6. What are solids? (2 Marks)

Ans. Solids are one of the states of matter where constituent particles are tightly packed together. Due to this, solids have a definite shape, structure and rigidity.

Ques 7. What are liquids? (2 Marks)

Ans. Liquids are those states of matter where particles are loosely packed. Liquids can flow and they take the shape of the container in which they are placed.

Ques 8. What are gases? (2 Marks)

Ans. Gases are where the constituent particles are very loosely packed. They take the shape and volume of the container in which they are placed.

Ques 9. What are atoms? (2 Marks)

Ans. Atoms are the basic building units of all matter. Depending on the element’s chemical properties, atoms differ accordingly.

Ques 10. What are the subatomic particles? (2 Marks)

Ans. Atoms are made up of subatomic particles namely, protons, neutrons and electrons.

  • Protons are positively charged particles.
  • Neutrons have no charge and exist along with protons at the centre of the atom in the nucleus.
  • Electrons are negatively charged and revolve around the nucleus of the atom.

Ques 11. What are molecules? (2 Marks)

Ans. Molecules are those which are made up of two or more atoms of same or different elements. Example, in, H2, H2O, etc, we can see that two atoms of hydrogen forms a molecule and 2 atoms of hydrogen and 1 atom of oxygen forms the water molecule.

Ques 12. What are compounds? (2 Marks)

Ans. Compounds are those which can be broken down into simpler compounds or elements.

Ques 13. What are elements? (2 Marks)

Ans. Elements are those which cannot be further broken down into simpler elements.

Ques 14. Name some of the methods which are used to separate mixtures. (2 Marks)

Ans. Evaporation, condensation, sublimation, filtration, chromatography, etc are some of the methods which are used to separate mixtures.

Ques 15. Is boron solid? (2 Marks)

Ans. No. Boron is a metalloid that shows both characteristics of metals and non-metals.

Ques 16. What is a heterogeneous mixture? (2 Marks)

Ans. A heterogeneous mixture is a mixture that does not mix completely and is not uniform in nature. 

Ques 17. By which process sea water can be purified? (2 Marks)

Ans. Sea water is purified by the process of distillation. Distillation is a process in which the components of a substance or liquid mixture are separated by heating it to a certain temperature and condensing the resulting vapours.

Ques 18. Why do dry resins swell up when kept in water? (2 Marks)

Ans. Dried raisins swell up when kept in water because of the process of osmosis. It is the process where solvent travels through a semi-permeable membrane from a less concentrated solute to a more concentrated solute. 

Ques 19. Boyle’s relates to which state of matter? (2 Marks)

Ans. Boyle’s law relates to gaseous state of matter. Boyle’s law states that the pressure of a gas is inversely proportional to its volume.

Ques 20. Why do water and oil not mix together? (2 Marks)

Ans. Water and oil  do not mix together because of 2 reasons.

  1. Water is polar and oil is not.
  2. The molecules of oil are bigger than that of water. This is why oil has lesser density than water and floats on top of it.

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CBSE CLASS XII Related Questions

1.
A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

      2.
      Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s) takes place. Further show: 
       (i) Which of the electrode is negatively charged? 
       (ii) The carriers of the current in the cell. 
       (iii) Individual reaction at each electrode.

          3.

          Write down the electronic configuration of:
          (i) Cr3+ (iii) Cu+ (v) Co2+ (vii) Mn2+ 
          (ii) Pm3+ (iv) Ce4+ (vi) Lu2+ (viii) Th4+

              4.

              Give the IUPAC names of the following compounds:

              (i)CH3CH(Cl)CH(Br)CH3

              (ii)CHF2CBrClF

              (iii)ClCH2C≡CCH2Br

              (iv)(CCl3)3CCl

              (v)CH3C(p-ClC6H4)2CH(Br)CH3

              (vi)(CH3)3CCH=CClC6H4I-p

                  5.
                  Write the Nernst equation and emf of the following cells at 298 K : 
                  (i) Mg(s) | Mg2+ (0.001M) || Cu2+(0.0001 M) | Cu(s) 
                  (ii) Fe(s) | Fe2+ (0.001M) || H+ (1M)|H2(g)(1bar) | Pt(s) 
                  (iii) Sn(s) | Sn2+(0.050 M) || H+ (0.020 M) | H2(g) (1 bar) | Pt(s) 
                  (iv) Pt(s) | Br2(l) | Br-  (0.010 M) || H+ (0.030 M) | H2(g) (1 bar) | Pt(s).

                      6.

                      Draw the structures of optical isomers of: 
                      (i) \([Cr(C_2O_4)_3]^{3–}\)
                      (ii) \([PtCl_2(en)_2]^{2+}\)
                      (iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

                          CBSE CLASS XII Previous Year Papers

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