2) What is the relative atomic mass of a nucleide that has 3 electrons on its third electron shell and 13 neutrons

atomic mass of the nucleide is the sum of the masses of its protons and neutrons. To calculate the relative atomic mass, we need to know the mass of one proton and one neutron.

The mass of one proton is approximately \(1.0073\) atomic mass units (amu), while the mass of one neutron is approximately \(1.0087\) amu. Please note that these values are approximate and may vary slightly.

Now let"s solve the problem step-by-step:

2) To find the relative atomic mass of a nucleide with 3 electrons on its third electron shell and 13 neutrons in the nucleus, we need to determine the number of protons.

Since all atoms are electrically neutral, the number of protons is equal to the number of electrons. Therefore, the total number of electrons is 3.

We know that the atomic number of an element is equal to the number of protons in its nucleus. By finding the atomic number, we can determine the number of protons.

To find the atomic number, we can use the periodic table, which lists the elements in order of increasing atomic number. By referring to the periodic table, we find that the atomic number of aluminum (Al) is 13, which means that it has 13 protons.

The relative atomic mass of an element is the weighted average of the masses of its isotopes. In this case, we only have information about the number of electrons and neutrons, so we assume that the nucleide is an isotope of aluminum (Al).

The atomic mass of aluminum is approximately \(26.9815\) amu. Therefore, the relative atomic mass of the nucleide is also \(26.9815\) amu.

3) To calculate the mass fraction (%) of neutrons in the nucleide of an element with a mass number of 6, we need to find the number of neutrons.

The mass number of an element is equal to the sum of the number of protons and neutrons in its nucleus. In this case, the mass number is 6.

From the information given, we know that the element has two energy levels in its atomic shell, and one electron is located in the outer level. This means that the element has 2 protons (since the number of protons is equal to the number of electrons) and a mass number of 6.

To find the number of neutrons, we subtract the number of protons from the mass number:

\(6\) (mass number) - \(2\) (protons) = \(4\) (neutrons)

Now we can calculate the mass fraction of neutrons. The mass fraction is the mass of neutrons divided by the total mass of the nucleide, multiplied by 100 to get a percentage.

The mass of 1 neutron is approximately \(1.0087\) amu. The total mass of the nucleide (protons + neutrons) is \(1.0073\) amu (mass of 1 proton) + \(4\) (number of neutrons) * \(1.0087\) amu.

The mass fraction of neutrons is:

\(\frac{{4 \times 1.0087}}{{1.0073 + (4 \times 1.0087)}} \times 100\)

Calculating this expression, we find that the mass fraction of neutrons is approximately \(80\)%.

4) Similar to the previous question, to calculate the relative atomic mass of a nucleide with 3 electrons on its third electron shell and 14 neutrons in the nucleus, we need to find the number of protons.

Since all atoms are electrically neutral, the number of protons is equal to the number of electrons. Therefore, the total number of electrons is 3.

To find the atomic number, we can use the periodic table. By referring to the periodic table, we find that the atomic number of silicon (Si) is 14, which means that it has 14 protons.

The relative atomic mass of silicon is approximately \(28.0855\) amu. Therefore, the relative atomic mass of the nucleide is also \(28.0855\) amu.