Question

What is the difference between nuclear symbol and isotope notation when representing an atom. Create an example of both.

Answer 1

I am not sure what you exactly ask. When we simply write the symbol of the element you are told how many protons the element contain and how many electrons the element possess in its electronic neutral state. Example of these could be:
\[\Large \sf H ~~~ C ~~~ N ~~~ O\]
WIth this notation we sorta neglect all information about the amount of neutrons, which is very convent in chemistry as the reaction between elements is mostly determined by the electrons of the elements.

When studying atomic physics the amount of neutrons may become relevant and it is therefore much more appropriate to use isotope notation. Examples of these could be:
\[\Large \sf _{1}^{1}H ~~~ _{1}^{2}H ~~~ _{1}^{3}H ~~~ _{6}^{12}C ~~~ _{6}^{13}C ~~~ _{6}^{14}C\]
Using this notation we provide information regarding the amount of protons and nucleo number / mass number. All of the examples above are usually by chemists shortened as the amount of protons within any element throughout the isotopes are the same and specified by the element symbol, thereby it become:
\[\Large \sf ^{1}H ~~~ ^{2}H ~~~ ^{3}H ~~~ ^{12}C ~~~ ^{13}C ~~~ ^{14}C\].

Answer 2

nucleon number*