What experimental evidence led Thomson to conclude that an electron has a negative charge and is very light?
Thomson believed that the rays were particles because a paddle wheel was set in motion by the ray. He concluded that the beam was negatively charged because the ray came from the negative electrode.
Which of the following is are not the limitations of Bohr’s model?
(i) It could not explain the intensities or the fine spectrum of the spectral lines. (ii) No justification was given for the principle of quantisation of angular momentum. (iii) It could not explain why atoms should combine to form bond. (iv)It could not successfully applied to single electron atoms.
Which statement is wrong about the orbitals?
According to Hund’s rule the pairing of electrons in the orbitals of a particular subshell does not takes place until all the orbitals of a subshell are singly occupied. Moreover, the singly orbitals must have the electrons with parallel spin. i.e. ∴ Option (a) is the incorrect option.
Which statement is true spacing between energy levels?
1. Spacing between energy levels n=land n = 3 in hydrogen atom is less than that of n = 2 and n=3. 2. Spacing between energy levels n=land n-2 in hydrogen atom is equal to that n=2 and, n=3.
Which one is the wrong statement total orbital angular momentum of electron in’s orbital is equal to zero?
Total orbital angular momentum of electron us ‘s’ orbital is equal to zero. An orbital is designated by three quantum numbers while an electron in an atom designated by four quantum numbers. The value of m for dz2 is zero. ∴ Orbital angular momentum is zero.
Which one is the wrong statement the uncertainty principle is?
The correct option is : (c) The energy of 2s-orbital is less than the energy of 2p-orbital in case of hydrogen-like atoms. Explanation : In case of hydrogen like atoms, energy depends on the principal quantum number only. Hence.
How many p-orbitals exist in the N 2 shell?
three orbitals
Which two quantum sublevels will fill after 4f?
After the 4f orbitals are filled, boxes are shown for the rest of the elements formed by adding 5d and 6p electrons. The seventh period contains boxes for the elements formed by filling the 7s, the 5f (the actinide series shown below the table), and finally the 6d sublevels.