Answer :
To draw the correct Lewis dot structure for Potassium Fluoride (KF), we'll follow a few steps to understand how the elements interact in this compound:
1. Identify the Elements and Their Configuration:
- Potassium (K): Potassium is an alkali metal located in group 1 of the periodic table. It has one valence electron.
- Fluorine (F): Fluorine is a halogen located in group 17 of the periodic table. It has seven valence electrons and needs one more to complete its octet.
2. Electron Transfer:
- Potassium tends to lose its one valence electron to achieve a stable configuration similar to the noble gas Argon. When it loses this electron, it becomes a positively charged ion, [tex]\( K^+ \)[/tex].
- Fluorine needs one electron to complete its octet and achieve a stable configuration similar to the noble gas Neon. It gains the electron lost by Potassium, becoming a negatively charged ion, [tex]\( F^- \)[/tex].
3. Ionic Bond Formation:
- When Potassium loses its electron and Fluorine gains it, they form an ionic bond. This is because oppositely charged ions attract each other.
4. Draw the Lewis Structure:
- For Potassium fluoride, the Lewis structure will show Potassium as [tex]\( K^+ \)[/tex] and Fluorine as [tex]\( [F]^- \)[/tex].
- In this structure, [tex]\( K^+ \)[/tex] indicates that Potassium has lost an electron, and [tex]\( [F]^- \)[/tex] indicates that Fluorine has a full set of eight electrons, satisfying its octet rule.
Therefore, the correct Lewis dot structure for Potassium Fluoride is [tex]\( K^+ \, [F]^- \)[/tex]. This represents Potassium as a cation [tex]\((K^+)\)[/tex] and Fluorine as an anion [tex]\((F^-)\)[/tex] forming an ionic compound.
1. Identify the Elements and Their Configuration:
- Potassium (K): Potassium is an alkali metal located in group 1 of the periodic table. It has one valence electron.
- Fluorine (F): Fluorine is a halogen located in group 17 of the periodic table. It has seven valence electrons and needs one more to complete its octet.
2. Electron Transfer:
- Potassium tends to lose its one valence electron to achieve a stable configuration similar to the noble gas Argon. When it loses this electron, it becomes a positively charged ion, [tex]\( K^+ \)[/tex].
- Fluorine needs one electron to complete its octet and achieve a stable configuration similar to the noble gas Neon. It gains the electron lost by Potassium, becoming a negatively charged ion, [tex]\( F^- \)[/tex].
3. Ionic Bond Formation:
- When Potassium loses its electron and Fluorine gains it, they form an ionic bond. This is because oppositely charged ions attract each other.
4. Draw the Lewis Structure:
- For Potassium fluoride, the Lewis structure will show Potassium as [tex]\( K^+ \)[/tex] and Fluorine as [tex]\( [F]^- \)[/tex].
- In this structure, [tex]\( K^+ \)[/tex] indicates that Potassium has lost an electron, and [tex]\( [F]^- \)[/tex] indicates that Fluorine has a full set of eight electrons, satisfying its octet rule.
Therefore, the correct Lewis dot structure for Potassium Fluoride is [tex]\( K^+ \, [F]^- \)[/tex]. This represents Potassium as a cation [tex]\((K^+)\)[/tex] and Fluorine as an anion [tex]\((F^-)\)[/tex] forming an ionic compound.
