Write the Lewis symbols for the ions in each ionic compound. d. K₂O

Verified step by step guidance

1. Identify the ions present in the compound K2O. Potassium (K) and oxygen (O) are the elements involved.
2. Determine the charges of the ions. Potassium (K) is in Group 1 of the periodic table and typically forms a +1 ion (K^+). Oxygen (O) is in Group 16 and typically forms a -2 ion (O^2-).
3. Write the Lewis symbol for the potassium ion (K^+). Since it loses one electron to form a cation, it will have no dots around it, just the symbol K with a positive charge.
4. Write the Lewis symbol for the oxide ion (O^2-). Oxygen gains two electrons to achieve a full octet, so it will have eight dots around it, representing the filled valence shell, and a 2- charge.
5. Combine the Lewis symbols to represent the ionic compound K2O, ensuring the overall charge is neutral. Two K^+ ions will balance the charge of one O^2- ion.

Key Concepts

Lewis Symbols

Lewis symbols, or Lewis dot structures, represent the valence electrons of an atom as dots around the element's symbol. This notation helps visualize how atoms bond and interact in chemical compounds. For ions, the Lewis symbol indicates the loss or gain of electrons, showing the resulting charge.

Ionic Compounds

Ionic compounds are formed through the electrostatic attraction between positively charged cations and negatively charged anions. In the case of K2O, potassium (K) donates electrons to oxygen (O), resulting in K+ and O2- ions. Understanding the formation of these ions is crucial for writing their Lewis symbols.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in chemical bonding. The number of valence electrons determines an element's reactivity and the type of bonds it can form. In ionic compounds, the transfer of valence electrons leads to the formation of stable electron configurations for the resulting ions.