18C Section 2. Where will the bonding electrons most likely be found in an jocic bond? 3. Why is a purely ionic bond impossible in an ionic compounde 4. Conpure the polarity of a pure covalent bond with that of an innic bood. 0 5. What two nonradioactive elements could theoretically form the strongest ionic bond? Give the formula for the compound and explain your answer: 6. What does the electron dot notation for an ionic compound represent? What does it not represent? 7. What is true of the sum of all charges in an ionic compound electron dot notation? Why must this be so? 8. How are particles arranged in an ionic compound? 9. (True or False) The character of a bond-whether ionic or co-valent-between two atoms can be viewed as the degree of sharing of the bonding electrons. O 10. Write the electron dot notations for the following ionic com pounds. Be sure to include the charges of the ions. a. beryllium chloride ( \( \mathrm{BeCl}_{2} \) ) b. sodium oride \( \left(\mathrm{Na}_{2} \mathrm{O}\right) \)

Let's address each question step by step: ### 2. Where will the bonding electrons most likely be found in an ionic bond? In an ionic bond, bonding electrons are not shared between atoms as in covalent bonds. Instead, one atom donates electrons to another, resulting in the formation of positively charged cations and negatively charged anions. The bonding electrons are most likely found around the anion, as it has gained electrons, while the cation has lost electrons. ### 3. Why is a purely ionic bond impossible in an ionic compound? A purely ionic bond is impossible because there is always some degree of covalent character in ionic bonds. This is due to the polarizing effect of cations on anions, which can lead to some sharing of electron density. Additionally, no atom is completely electronegative or electropositive; thus, there will always be some overlap in electron clouds, making a purely ionic bond unattainable. ### 4. Compare the polarity of a pure covalent bond with that of an ionic bond. A pure covalent bond occurs when two atoms share electrons equally, resulting in no charge separation and a nonpolar bond. In contrast, an ionic bond involves a complete transfer of electrons from one atom to another, leading to the formation of charged ions. This results in a significant charge separation, making ionic bonds highly polar. ### 5. What two nonradioactive elements could theoretically form the strongest ionic bond? Give the formula for the compound and explain your answer. The two nonradioactive elements that could theoretically form the strongest ionic bond are cesium (Cs) and fluorine (F). The formula for the compound is \( \mathrm{CsF} \). This is because cesium has a low ionization energy, allowing it to easily lose its outer electron, while fluorine has a high electronegativity and a strong tendency to gain an electron. The large difference in electronegativity between cesium and fluorine leads to a very strong ionic bond. ### 6. What does the electron dot notation for an ionic compound represent? What does it not represent? The electron dot notation for an ionic compound represents the valence electrons of the atoms involved and shows the transfer of electrons from the metal to the nonmetal. It does not represent the actual arrangement of ions in the solid lattice structure of the ionic compound or the three-dimensional geometry of the compound. ### 7. What is true of the sum of all charges in an ionic compound electron dot notation? Why must this be so? The sum of all charges in an ionic compound must equal zero. This is because ionic compounds are electrically neutral overall. The positive charges from cations must balance the negative charges from anions to maintain charge neutrality. ### 8. How are particles arranged in an ionic compound? In an ionic compound, particles are arranged in a regular, repeating three-dimensional lattice structure. Cations and anions alternate in this lattice, maximizing the attractive forces between oppositely charged ions while minimizing repulsive forces between like charges. ### 9. (True or False) The character of a bond—whether ionic or covalent—between two atoms can be viewed as the degree of sharing of the bonding electrons. **True.** The character of a bond can indeed be viewed as the degree of sharing of bonding electrons. In purely covalent bonds, electrons are shared equally, while in ionic bonds, there is a complete transfer of electrons, indicating no sharing. ### 10. Write the electron dot notations for the following ionic compounds. Be sure to include the charges of the ions. #### a. Beryllium chloride (\( \mathrm{BeCl}_{2} \)) - Beryllium (Be) has 2 valence electrons and will lose both to form \( \mathrm{Be}^{2+} \). - Each chlorine (Cl) atom has 7 valence electrons and will gain 1 electron to form \( \mathrm{Cl}^{-} \). The electron dot notation is: \[ \text{Be:} \rightarrow \text{Cl:}^- \quad \text{Cl:}^- \] #### b. Sodium oxide (\( \mathrm{Na}_{2}\mathrm{O} \)) - Sodium (Na) has 1 valence electron and will lose it to form \( \mathrm{Na}^{+} \). - Oxygen (O) has 6 valence electrons and will gain 2 electrons to form \( \mathrm{O}^{2-} \). The electron dot notation is: \[ \text{Na:}^+ \quad \text{Na:}^+ \quad \text{O:} \rightarrow \text{O:}^{2-} \] This notation shows the transfer of electrons and the resulting charges of the ions in the compounds.