Ionic Compounds Overview

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Questions and Answers

Which of the following statements correctly describes the relationship between lattice energy and ionic charge?

  • Lattice energy is inversely proportional to the ionic charge.
  • Lattice energy is only affected by the ionic charge when the ions are of similar size.
  • Lattice energy is independent of the ionic charge.
  • Lattice energy is directly proportional to the ionic charge. (correct)

Which of these properties is NOT characteristic of ionic compounds?

  • Good electrical conductivity in the solid state (correct)
  • High melting points
  • Formation of a crystalline structure
  • Brittle nature

Which of the following BEST describes the electron sea model of metallic bonding?

  • A sea of delocalized electrons that are shared equally among all metal atoms. (correct)
  • A sea of negatively charged ions surrounded by a cloud of positive electrons.
  • A sea of positively charged ions surrounded by a cloud of negative electrons.
  • A sea of tightly bound electrons that form a solid structure.

Which of the following properties of metals is NOT directly related to metallic bonding?

<p>The ability to form covalent bonds (C)</p> Signup and view all the answers

Why are metals malleable and ductile?

<p>The delocalized electrons can move freely, allowing the metal ions to slide past each other. (C)</p> Signup and view all the answers

Which of the following is a characteristic of substitutional alloys?

<p>Atoms of similar sizes replace each other in the metallic crystal. (A)</p> Signup and view all the answers

Which of the following factors would lead to a greater lattice energy in an ionic compound?

<p>Decreased distance between ions (C)</p> Signup and view all the answers

What property of ionic compounds allows them to conduct electricity when melted but not in the solid state?

<p>The ions become free to move in the liquid phase. (E)</p> Signup and view all the answers

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Flashcards

Ionic Compounds

Compounds held together by electrostatic attractions between cations and anions.

Crystal Lattice

The repeating pattern of ions in ionic solids forming a crystalline structure.

Cations

Positively charged ions that are smaller than their original atoms after losing electrons.

Anions

Negatively charged ions that are larger than their original atoms due to extra electrons.

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Lattice Energy

The energy required to separate one mole of an ionic compound.

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Metallic Bonding

Bonding occurring in metals where delocalized electrons move freely among cations.

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Ductility

The ability of metals to be drawn into wires due to electron mobility.

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Substitutional Alloys

Alloys formed when similar-sized atoms replace each other in a metallic crystal.

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Study Notes

Ionic Compounds

  • Ionic compounds are formed by electrostatic attractions between positively charged cations and negatively charged anions.
  • Ionic solids have a crystalline structure, with ions arranged in repeating patterns called a crystal lattice.
  • Cations are smaller than their parent atoms because they lose electrons and an entire energy level.
  • Anions are larger than their parent atoms due to electron-electron repulsion, having more electrons than protons.
  • Ionic compounds have high melting and boiling points due to strong ionic bonds.
  • Ionic solids do not conduct electricity in their solid state.
  • Ionic compounds conduct electricity when dissolved in water (aqueous solution) or molten because ions are free to move, allowing electron flow.
  • Ionic solids are hard, brittle, and rigid; they break along cleavage planes where like charges repel.
  • Lattice energy is the energy to separate one mole of an ionic compound.
  • Lattice energy increases with the charge of the ions; larger charge, greater energy.
  • Lattice energy increases as the distance between ions decreases; smaller ions, greater energy.

Metallic Bonding

  • Metallic bonding occurs in pure metals (e.g., silver, gold, zinc, copper).
  • The electron sea model describes metallic bonding as a "sea" of delocalized electrons surrounding metal ions.
  • Metals are excellent conductors because electrons can move freely around cations.
  • The attraction between delocalized electrons and metal cations is the metallic bond.
  • Metals have moderately high melting points due to cation and electron mobility.
  • Metals have extremely high boiling points because separating neutral atoms from delocalized electrons is difficult.
  • Metals are malleable and ductile due to electron mobility.
  • Metal strength generally increases with the number of delocalized electrons.

Alloys

  • Alloys are mixtures of elements with metallic properties.
  • Many alloys are mixtures of two or more metals.
  • Substitutional alloys form when atoms of similar size replace each other in the metallic crystal.
  • Interstitial alloys form when smaller atoms fill the spaces between larger atoms in the metallic crystal.

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