Question

Why do dry sodium chloride and the solutions of sodium nitrate and sodium chloride all impart the same color to the flame?

Answer 1

We know that in generally modern periodic table metallic atoms are placed in the left side of the table and non-metallic atoms are placed in the right side of the table. Metalloids and transition elements are placed in between metal and non-metal elements. Below the two rows are there. There are nothing but lanthanides and actinides. These are f-block elements. The atomic number of the element is nothing but the number of electrons or number of protons. The mass number of the atom is nothing but the sum of the number of protons and number of neutrons. In general we move left to right metallic property of the atom decreases. We move right to left and non-metallic property decreases.

Complete answer:
As we know that the colour depends on the wavelength of the atom. Each and every element in the periodic table has a spectrum of the colour. The colour of the salt depends on the ions in the salts.
Here we consider dry sodium chloride and the solutions of sodium nitrate and sodium chloride all impart the same color to the flame, because both cases have the same sodium ion.
According to the above discussion, we conclude dry sodium chloride and the solutions of sodium nitrate and sodium chloride all impart the same color to the flame due to the sodium ion in solution and dry sodium chloride.

Note:
In the world there are a lot of elements in various forms. For study and developing purposes, classification happens. Periodic table used to study the elements in easy form. If one new element is discovered , it means, based on the physical and chemical properties we placed in the periodic table.
In general, modern periodic table ordering is based on the atomic number of the atoms. The lowest atomic number starting from the first and followed by a higher atomic number.
Depending on the energy level of the outermost shell in the atoms, periods are classified and place the atom in respective periods. Depending on the electrons shielding and size and physical behaviour of the atom, groups are coming.