Answer to Question #177994 in Physical Chemistry for Khairun

Question

1.Write down the electron configuration of the atom when it is in its charged state as stated above. (One sentence)

2.Write down 4 quantum numbers for the electron/s present in its 5th shell.

3.What kind of bond will be formed due to the reaction with the earth element? Explain your reason behind that. Why the compound became soluble? Can it make covalent bond in any way? (Not more than 50 words).

4.Let’s consider, X3+ where the mass number is 41 and electron number is 20. What would be the neutron number? Write the mass number of two possible isobars for this element.

5.Prove Pauli’s exclusion principle for the electron that is present in the 4th shell with the electrons that are present in the 3s orbital of copper.

6.Write down two limitations for each of the Rutherford’s atomic model and Bohr’s model for the element copper. Relate the element for each case while describing the limitations.

Answer 1

The symbols used for writing the electron configuration start with the shell number (n) followed by the type of orbital and finally the superscript indicates how many electrons are in the orbital.

n = 5; l = 2; m = -2, -1, 0, +1, +2; s = + 1/2

There are different nu.bers in each.

There are 4 quantum numbers that specify the orbitals and the element trims within them.

The "shell" is specified by quantum number n.

The possible values of n are integer numbers 1, 2, 3… to infinity.

The next quantum number is l. This can have values as low as 0 and as high as n-1. This quantum number tells you the type of orbital.

Bohr's model of the atom describes electrons orbiting in stable energy levels as opposed to Rutherford's model in which electrons' motion was not described. Electrons orbited the nucleus such that their angular momentum is an integral multiple o.