How many protons, electrons, and neutrons are in i- and li+ ?

These are two questions and two answers.

Question 1: protons, electrons, and neutrons in I⁻

53 protons, 54 electrons, and a variable number of neutrons. One possibility is 74 neutrons, if it is the most stable isotope, iodine-127.

Explanation:

1) I⁻ is the anion of the atom I

2) One negative charge means that one electron has been added to the neutral atom of I.

3) The element I has atomic number 53 (you see this is a periodic table).

4) The atomic number 53 means that it has 53 protons.

5) The neutral atom has the same number of electrons than protons, i.e. 53. Since the anion I⁻ has one additional electron, it has 54 electrons.

6) The number of neutrons is not a fixed quantity. Different isotopes of the same element have different number of neutrons.

7) The isotope iodine-127, which is the only stable isotope of iodine has 74 neutrons.

The number of neutrons is calculated as the mass number (127) less the number of protons (53): 127 - 53 = 74.

Question 2: protons, electrons, and neutrons in Li⁺

3 protons, 2 electrons, variable number of neutrons, may be 3 or 4 depending of the isotope.

Explanation:

1) Li⁺ is the cation of the atom Li

2) One positive charge means that one electron has been removed from the neutral atom of Li.

3) The element Li has atomic number 3 (you see this is a periodic table).

4) The atomic number 3 means that it has 3 protons.

5) The neutral atom has the same number of electrons than protons, i.e. 3. Since the anion Li has one less electron, it has 2 electrons.

6) The number of neutrons is not a fixed quantity. Different isotopes of the same element have different number of neutrons.

7) There are two natural stable isotopes of lithium.

The isotope lithium-7, has 4 neutrons, and the isotope lithium-6 has 3 neutrons.

The number of neutrons is calculated as the mass number less the number of protons (3):

i) 7 - 3 = 4

ii) 6 - 3 = 3

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.