Principle Quantum number describes?
The principal quantum number (n) describes the size of the orbital.
Example: Orbitals for which n = 2 are larger than those for which n = 1.
The atoms of different isotopes of the same element differ from each other in the number of:
Isotopes of an element will contain the same number of protons and electrons but will differ in the number of neutrons they contain.
In other words, isotopes have the same atomic number because they are the same element but have a different atomic mass because they contain a different number of neutrons.
The radius of the nucleus of an atom is approximately:
The proton distribution can be characterized by an average radius. It is found that nuclear radii range from (1-10) x 10-15 m.
An element has 18 electrons, and 20. neutrons. Its charge is -2. What is its mass number?
► Mass no = no. of proton + no. of neutron
Here no. of proton is 2 less than no. of electron as the charge on element is -2
► Hence no. of proton = 18 - 2 = 16,
► No. of neutron = 20
Hence mass number is 16 + 20 = 36
Which of the following statements is not correct about the characteristics of cathode rays?
Characteristics of cathode rays are:
Hence the correct answer is option B.
Which model describes that there is no change in the energy of electrons as long as they keep revolving in the same energy level and atoms remains stable?
Bohr Model of atom:
Bohr explained the stability through the concept of revolution of electrons in different energy levels.
The change in the energy of an electron occurs when it jumps from lower to higher energy levels. When it gains energy, it excites from lower to higher and vice versa.
Thus energy is not lost and the atom remains stable.
The number of radial nodes for 3p orbital is:
► Number of radial nodes = n - 1 – 1
► For 3p orbital, n = 3 – 1 – 1 = 1
► Number of radial nodes = 3 – 1 – 1 = 1.
Atomic mass of an element is equal to the sum of?
Atomic Mass is the sum of no. of protons and neutrons.
Thomson’s plum pudding model explained:
Postulates of Thomson’s atomic model
Which of the following conclusions could not be derived from Rutherford’s α -particle scattering experiment?
Concept of electrons moving in a circular path of fixed energy called orbits was put forward by Bohr and not derived from Rutherford's scattering experiment.
Out of a large number of circular orbits theoretically possible around the nucleus. The electron revolves only in those orbits which have a tired value of energy Hence, these orbits are called energy level or stationary states.
The charge on electron was determined by:
The charge on electron was determined by milliken by using oil drop experiment
The nature of positive rays depends on?
The positive charges in these rays, other than negative cathode rays (which are electrons), depend on the gas that is used because they are cations - atoms with mostly one electron missing and thus one positive charge. So, if you accelerate, argon cations and protons over the same electric potential, the particles in the rays will have the same kinetic energy, but the argon ions will be much slower, as they are much heavier than the protons.
The nucleus of a tritium atom, 3H, contains
Tritium (3H) is a radioactive isotope of hydrogen. The nucleus decays (by emitting an electron and an antineutrino), changing from a triton (one proton and two neutrons) to a 3He nucleus (two protons and one neutron).
Which of the following is true about electron?
Electron carries unit negative charge and has a mass of 9.1 x 10-31 kg, while proton has a mass of 1.67 x 10-27 kg.
Neutron is a fundamental particle which carries?
A neutron is a sub-atomic particle with no net electrostatic charge, with a very similar mass to a proton.