18. 1. What makes certain combinations of atoms form lonie bonds rather than other kinds of bonds? 2. Where will the bonding electrons most likely be found in an fonic bond? 3. Why is a purely ionic bond impossible in an lonic compound? 4. Compare the polarity of a pure covalent bond with that of an ionic bond. 8. 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 lonic compound represent What does it not represent? 7. What is true of the sum of all charges in an ionic compounds 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. 10. Write the electron dot notations for the following ionic com- pounds. Be sure to include the charges of the ions. a. beryllium chloride (BeCl ) b. sodium oxide (Na, O)

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### 1. What makes certain combinations of atoms form ionic bonds rather than other kinds of bonds?
Ionic bonds form between atoms that have significantly different electronegativities, typically between metals and nonmetals. Metals tend to lose electrons and form positive ions (cations), while nonmetals tend to gain electrons and form negative ions (anions). The large difference in electronegativity leads to the transfer of electrons from the metal to the nonmetal, resulting in the formation of ionic bonds.

### 2. Where will the bonding electrons most likely be found in an ionic bond?
In an ionic bond, the bonding electrons are not shared between the atoms as in covalent bonds. Instead, the electrons are transferred from the metal to the nonmetal, resulting in the formation of cations and anions. Therefore, the bonding electrons are most likely found around the anion, as it has gained the 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 compounds due to the polarizing effect of the cation on the anion. Even in compounds that are predominantly ionic, there is some sharing of electron density, which means that the bond is not purely ionic.

### 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 no polarity. 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 and high polarity in ionic bonds.

### 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 lithium (Li) and fluorine (F). The compound formed would be lithium fluoride (LiF). This bond is strong because lithium has a low ionization energy and readily loses one electron to form a cation, while fluorine has a high electronegativity and readily gains an electron to form an anion. The large difference in their electronegativities leads to a 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 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's electron dot notation? Why must this be so?
The sum of all charges in an ionic compound's electron dot notation must equal zero. This is because ionic compounds are electrically neutral overall, meaning that the total positive charge from the cations must balance the total negative charge from the anions.

### 8. How are particles arranged in an ionic compound?
In an ionic compound, particles are arranged in a regular, repeating three-dimensional lattice structure. This arrangement maximizes the attractive forces between oppositely charged ions and minimizes repulsive forces between like-charged ions, resulting in a stable structure.

### 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 the bonding electrons. In ionic bonds, there is little to no sharing, while in covalent bonds, there is significant sharing.

### 10. Write the electron dot notations for the following ionic compounds. Be sure to include the charges of the ions.
a. **Beryllium chloride (BeCl₂)**:
   - Beryllium (Be) has 2 valence electrons and forms a $$ \text{Be}^{2+} $$ ion.
   - Each chlorine (Cl) atom has 7 valence electrons and forms a $$ \text{Cl}^{-} $$ ion.
   - Electron dot notation: 
     $$
     \text{Be}^{2+} : \text{Cl}^- : \text{Cl}^-
     $$

b. **Sodium oxide (Na₂O)**:
   - Sodium (Na) has 1 valence electron and forms a $$ \text{Na}^{+} $$ ion.
   - Oxygen (O) has 6 valence electrons and forms a $$ \text{O}^{2-} $$ ion.
   - Electron dot notation:
     $$
     \text{Na}^+ : \text{Na}^+ : \text{O}^{2-}
     $$

This concludes the detailed solutions to the questions provided. If you have any further questions or need clarification, feel free to ask!
1. **Ionic bonds form when atoms with large electronegativity differences share electrons, leading to the transfer of electrons from metals to nonmetals.** 2. **In ionic bonds, bonding electrons are found around the anion, as they have gained electrons.** 3. **Purely ionic bonds are impossible because there's always some covalent character due to the polarizing effect of cations on anions.** 4. **A pure covalent bond has no charge separation, while an ionic bond has significant charge separation, making it highly polar.** 5. **Lithium and fluorine form the strongest ionic bond, resulting in lithium fluoride (LiF).** 6. **Electron dot notation for ionic compounds shows valence electrons and electron transfer but doesn't represent the 3D lattice structure.** 7. **The sum of all charges in an ionic compound's electron dot notation equals zero, ensuring electrical neutrality.** 8. **Particles in ionic compounds are arranged in a regular, repeating 3D lattice to maximize attractive forces between ions.** 9. **True: The degree of electron sharing defines the bond type—more sharing is covalent, less is ionic.** 10. **Electron dot notations for BeCl₂ and Na₂O show the transfer of electrons from metals to nonmetals, resulting in cations and anions.**

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