An atom of an element has an atomic number of 9 and a mass number of 19:

(a) State the number of protons and neutrons in the nucleus of this atom.

  • The atomic number tells us the number of protons in the atom. For an atom with an atomic number of 9, there are 9 protons.

  • The mass number is the sum of the protons and neutrons. Therefore, the number of neutrons is the mass number minus the atomic number:

    Neutrons=Mass number−Atomic number=19−9=10 neutrons

So, this atom has 9 protons and 10 neutrons.

(b) State the number of electrons in this atom.

In a neutral atom, the number of electrons is equal to the number of protons. Therefore, this atom has 9 electrons.

(c) Show with electron cross-dot diagrams the formation of ions by this atom.

This atom has an atomic number of 9, which corresponds to fluorine (F). Fluorine has 7 valence electrons and needs one more electron to complete its octet.

  • Fluorine gains one electron to form an anion (F⁻):

    Electron dot structure:

    :F: + e⁻ → :F:

(d) Write the electronic configuration of this element.

For fluorine (atomic number 9), the electronic configuration is:

1s2 2s2 2p5\text{1s}^2 \, \text{2s}^2 \, \text{2p}^5

This means fluorine has 2 electrons in the first shell and 7 electrons in the second shell.

(e) Point out its group in the periodic table.

Fluorine is in Group 17, which is the halogen group in the periodic table.

(f) Point out its period in the periodic table.

Fluorine is in Period 2 of the periodic table.