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ws 4 - Diamond and graphite 3.2.15(1).pptx
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∻Solution∻ ‖ 1 ⋮ **Draw the ionic bond in MgO**: In magnesium oxide (MgO), magnesium (Mg) loses two electrons to form a Mg²⁺ ion, while oxygen (O) gains two electrons to form an O²⁻ ion. The ionic bond is formed due to the electrostatic attraction between these oppositely charged ions. The diagram would show Mg²⁺ and O²⁻ with arrows indicating the transfer of electrons. ‖‖ 2 ⋮ **Draw the ionic bond in NaCl**: In sodium chloride (NaCl), sodium (Na) loses one electron to form a Na⁺ ion, and chlorine (Cl) gains that electron to form a Cl⁻ ion. The ionic bond is again due to the electrostatic attraction between Na⁺ and Cl⁻ ions. The diagram would depict Na⁺ and Cl⁻ with an arrow showing the electron transfer. ‖‖ 3 ⋮ **Explain why ionic compounds have high melting points**: Ionic compounds have high melting points due to the strong electrostatic forces of attraction between the oppositely charged ions in the ionic lattice structure. This requires a significant amount of energy to break these bonds. ‖‖ 4 ⋮ **Why do solid ionic compounds not conduct electricity?**: Solid ionic compounds do not conduct electricity because the ions are fixed in place within the lattice structure and cannot move freely. However, when melted or dissolved in water, the ions are free to move, allowing them to conduct electricity. ‖‖ 5 ⋮ **Name 4 examples of ionic compounds**: Common examples of ionic compounds include sodium chloride (NaCl), magnesium oxide (MgO), calcium fluoride (CaF₂), and potassium bromide (KBr). ‖‖ 6 ⋮ **Name the type of force that holds the ions together in an ionic compound**: The force that holds the ions together in an ionic compound is called ionic bonding, which is the electrostatic attraction between positively and negatively charged ions. ‖‖ 7 ⋮ **Under what conditions does sodium chloride conduct electricity?**: Sodium chloride conducts electricity when it is either melted or dissolved in water, as this allows the Na⁺ and Cl⁻ ions to move freely. ‖‖ 8 ⋮ **Describe the structure of a giant ionic lattice**: A giant ionic lattice consists of a three-dimensional arrangement of ions held together by strong ionic bonds. Each ion is surrounded by ions of opposite charge, creating a stable and repeating pattern throughout the structure. ‖ ∻Answer∻ ⚹ Ionic compounds are characterized by their high melting points, electrical conductivity in liquid form, and a lattice structure formed by ionic bonds. ⚹ ∻Key Concept∻ ⚹ Ionic compounds consist of charged ions held together by strong electrostatic forces, resulting in unique properties. ⚹ ∻Explanation∻ ⚹ The properties of ionic compounds, such as high melting points and electrical conductivity under certain conditions, stem from the nature of ionic bonding and the arrangement of ions in a lattice structure. ⚹◊What is the significance of lattice energy in determining the stability of ionic compounds?⍭ Generate me a similar question◊

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