(a) Draw the electron-dot structures for potassium and chlorine.
(b) Illustrate the formation of potassium chloride (KCl) by the transfer of electrons.
(c) Identify the ions present in the compound KCl.
(Atomic number: Potassium (K) = 19, Chlorine (Cl) = 17)

(a) The electron-dot structures for potassium (K) and chlorine (Cl) can be represented as follows:

Potassium (K):
K: ●

Chlorine (Cl):
Cl: ● ● ● ● ● ● ● ●

In the electron-dot structure, each dot represents a valence electron.

(b) To show the formation of KCl by the transfer of electrons, we need to consider the valence electrons of potassium and chlorine.

Potassium (K) has one valence electron (located in the outermost energy level), while chlorine (Cl) has seven valence electrons.

Since potassium has one valence electron and chlorine needs one more electron to achieve a stable electron configuration, potassium transfers its valence electron to chlorine.

The transfer can be represented as follows:

K: ● → K⁺: ●
Cl: ● ● ● ● ● ● ● ● + e⁻ → Cl⁻: ● ● ● ● ● ● ●

The electron transfer results in the formation of potassium ion (K⁺) and chloride ion (Cl⁻).

(c) The compound KCl consists of potassium ion (K⁺) and chloride ion (Cl⁻).