The atom questions | form five Chemistry

State the following:

1. Postulates of Bohr`s atomic model
2. Shortcomings of Bohr`s atomic model.

Define the following:

1. Principal quantum number.
2. Azimuthal quantum number.

Given the quantum number, n=3. Answer the following questions:

1. List all possible orbitals present in this quantum energy.
2. Write possible values of m_l and m_s for this quantum number.

The mass spectrum of an element enables the relative abundance of each isotope of the element be determined.  Data relating to mass spectrum of an element X whose atomic number is 35_z as indicated in the table below. Study the data and answer the questions that follows;

1. Define the term isotope.
2. Write the conventional symbols for the two isotopes of element X.
3. Calculate the relative atomic mass of X to three significant figures.

State the following :

1. Pauli`s exclusion principle.
2. Aufbau building principle.
3. Hund`s rule of maximum multiplicity.
4. Half-filled and full-filled orbital rule.

Write down the electronic configuration of each of the following species using orbtal diagrams:

1. Cl^-
2. K
3. Ca²⁺
4. F

Element Z occurs naturally as a mixture of ⁶⁹Z and ⁷¹Z.

1. Briefly explain the sisgnificance of the numbers 69 and 71 and give a term which describes these two components in the natural element.
2. If ⁶⁹Z and ⁷¹Z have relative atomic mass of 69.8, find the percentages of ⁶⁹Z and ⁷¹Z in a sample of Z.

Write the atomic number of an atom with electronic configuration of 1s² 2s² 2p⁶ 3s² 3p⁵ .

X occurs naturally as ³⁷X and ³⁵X. Given that the relative atomic mass of X is 35.5, determine the percentage of ³⁷X and ³⁵X in the sample of element X.

“The motion of the electron in an atom is not a simple rotation around an orbit , but rather a three dimensional standing wave which obeys Schrodinger equation”.

1. In which atomic model is this statement based?
2. Name other two atomic models that attempt to explain the structure of the atom.