What is the relation between Total energy (TE), Kinetic energy (KE) and Potential energy (PE) of Bohr's orbits?

Relation between Total energy (TE), Kinetic energy (KE) and Potential energy (PE):

Important conclusions:

(1) The minus sign for the energy of an electron in an orbit represents attraction between the +vely charged nucleus and negatively charged electron.

(2) Energy of an electron at infinite distance from the nucleus is zero.

(3) As an electron approaches the nucleus, the electrical attraction increases, energy of electron decreases and it becomes negative.

(4) Energy of an electron increases as the value of ‘n’increases i.e.

(5) Value of ‘n’ remaining unchanged, the amount of energy associated with an electron remains unaltered.

(6) Energy of electron in first, second, third and fourthorbit are –13.6, –3.4, –1.5, and –0.85 eV/atomrespectively.

(7) Although the energy of electron increases with increase in the value of ‘n’ (orbit), yet the difference of energy between successive orbits decreases. Thus E₂ – E₁ > E₃ – E₂ > E₄ – E₃ > E₅ – E₄ >, etc…

How to calculate energy of Bohr's orbits in term of Rydberg's constant

Energy in term of Rydberg’s Constant:

Which of the Hydrogen spectrum series found in visible range of spectrum?

Balmer series of Hydrogen spectrum found in visible range of spectrum while lymen series found in UV range of spectrum and remain series of spectrum found in Infra red of spectrum..

More over only first four line of Balmer series found in visible range and others line of Balmer series Lines  also found infrared part of spectrum.

Of all noble metals, gold has got a relatively high electron affinity. Explain.

The increased effective nuclear charge due to poor screening by inner 4f and 5 d orbitals enhances the attracting ability and hence it has got high electron affinity.

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(11) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(12) Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

(13) Ionization energy of Boron is smaller than Beryllium even though effective nuclear charge is higher?

(14) What are the increasing order of ioni radii of first group elements in water ?

(15) What are the increasing order of molar conductivity of first group elements in water ?

Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

Packing in crystal lattice is not compact due to small size of Li+ and bigger size of CO3 -2 .But O2– being smaller in size can stabilize Li2O.

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(11) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(12) Of all noble metals, gold has got a relatively high electron affinity. Explain.

(13) Ionization energy of Boron is smaller than Beryllium even though effective nuclear charge is higher?

(14) What are the increasing order of ioni radii of first group elements in water ?

(15) What are the increasing order of molar conductivity of first group elements in water ?