Ionic Bonding Concepts

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Questions and Answers

What is the process of forming cations primarily dependent on?

  • Ionization energy (correct)
  • Atomic mass
  • Chemical reactivity
  • Electron affinity

Which property of ionic bonds makes ionic crystals brittle?

  • They form organized crystal lattices. (correct)
  • They can easily deform when stressed.
  • They have strong intermolecular forces.
  • They are weaker than metallic bonds.

Anions form when metals gain electrons.

False (B)

Define ionization energy.

<p>The energy required to release one mole of electrons from a gaseous neutral atom.</p> Signup and view all the answers

The ionic charge of elements in the main groups can be derived from their position in the periodic table.

<p>True (A)</p> Signup and view all the answers

What is the ionic charge of the zinc ion?

<p>Zn2+</p> Signup and view all the answers

The strong electrostatic attraction forces between cations and anions create an __________ bond.

<p>ionic</p> Signup and view all the answers

The formula for calcium chloride is CaCl______.

<p>2</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Cation = Positively charged ion formed by losing electrons Anion = Negatively charged ion formed by gaining electrons Ionization Energy = Energy required to remove an electron from an atom Electron Affinity = Energy released when an electron is added to an atom</p> Signup and view all the answers

Match the ions with their corresponding formulas:

<p>Hydroxide = OH- Ammonium = NH4+ Nitrate = NO3- Sulfate = SO42-</p> Signup and view all the answers

Which of the following statements about ionic bonds is true?

<p>Ionic bonds result from the transfer of electrons. (C)</p> Signup and view all the answers

Electrons in an ionic lattice structure are free to move in any direction.

<p>False (B)</p> Signup and view all the answers

Which of the following ions is a polyatomic cation?

<p>NH4+ (C)</p> Signup and view all the answers

What is the result of combining a sodium ion (Na+) and a chlorine ion (Cl−)?

<p>Sodium chloride (NaCl)</p> Signup and view all the answers

Transition metals always have a single ionic charge.

<p>False (B)</p> Signup and view all the answers

Ionic compounds are always composed of ______ and ______.

<p>cations, anions</p> Signup and view all the answers

What is the correct formula for aluminium oxide?

<p>Al2O3 (D)</p> Signup and view all the answers

Cations derived from non-metals end in -IDE.

<p>False (B)</p> Signup and view all the answers

What is the name of the cation with the formula Fe2O3?

<p>iron (III) cation</p> Signup and view all the answers

Sodium chloride (NaCl) separates into ___ and ___ ions when dissolved in water.

<p>Na+, Cl-</p> Signup and view all the answers

Which of the following is a property of ionic compounds?

<p>Brittle (A)</p> Signup and view all the answers

Match the following anions with their respective non-metal elements:

<p>Fluoride = Fluorine Chloride = Chlorine Bromide = Bromine Iodide = Iodine</p> Signup and view all the answers

Most ionic compounds are soluble in water.

<p>True (A)</p> Signup and view all the answers

The cation magnesium is represented as ___ in chemical notation.

<p>Mg2+</p> Signup and view all the answers

Flashcards

Bond strength

The strength of a bond between two atoms in a molecule. It is a measure of how much energy is required to break the bond.

Covalent bond

A bond where atoms share electrons, resulting in a more stable configuration.

Ionic bond

A bond where one atom loses electrons and another gains electrons, resulting in a stable ionic compound.

Malleability

The ability of a substance to be hammered or pressed into different shapes without breaking.

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Brittleness

The tendency of a substance to break or shatter under pressure.

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Cation

A positively charged ion formed when an atom loses electrons.

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Anion

A negatively charged ion formed when an atom gains electrons.

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Ionic compound

A chemical compound that contains both cations and anions, held together by electrostatic forces.

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Ionic Ratio

The ratio of cations to anions in an ionic compound, represented by the smallest whole numbers.

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Metal Cations

Positively charged ions formed when metal atoms lose electrons.

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Naming Cations with Multiple Charges

The charge of a cation is indicated by a Roman numeral in parentheses after the element name. For example, Fe(II) represents the iron cation with a +2 charge.

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Non-metal Anions

Negatively charged ions formed when nonmetal atoms gain electrons. Most nonmetal anions have a -ide ending to their names. For example, oxygen becomes oxide (O²-).

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Polyatomic Anions

Polyatomic ions are groups of atoms that act as a single unit with a net charge. Some polyatomic ions have the -ate ending in their names, such as nitrate, sulfate, carbonate, and phosphate.

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Properties of Ionic Compounds

Ionic compounds generally have a high melting point, are hard, brittle, soluble in water, conduct electricity as a liquid or when dissolved, but do not conduct electricity as a solid.

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Dissolution of Ionic Compounds

The process of dissolving an ionic compound in water, where the ions separate and become surrounded by water molecules, is represented by a chemical equation.

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Ionization Energy (Ei)

The energy required to remove one mole of electrons from a gaseous atom, forming a cation. This energy is always positive, because it takes energy to remove an electron from an atom.

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Electron Affinity (Ea)

The energy released or absorbed when a gaseous atom gains an electron, forming an anion.

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Ionic Lattice

A three-dimensional, repeating structure formed by the close packing of positively and negatively charged ions held by ionic bonds.

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Salts

Solid compounds consisting of ionic lattices, formed when a metal reacts with a non-metal.

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Formula Unit

The smallest repeating unit in a crystal lattice that defines its entire structure, containing the same ratio of ions as the chemical formula of the salt.

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Study Notes

Ionic Bonding

  • Cations: Form when metals lose electrons. The energy required (ionization energy) depends on the attraction of the nucleus to the electron. Smaller nuclear pull means easier electron loss, hence lower ionization energy. The first ionization energy (Ei₁) is the energy to remove one mole of electrons from a gaseous atom. Ionization energy increases with greater nuclear charge and smaller main quantum number, with the formation of X2+ requiring multiple ionization energies (Ei₁ + Ei₂ +...).

Anions

  • Anions: Form when non-metals gain electrons. The energy exchanged (electron affinity (Eₐ)) is negative when an electron is absorbed by a gaseous atom. Electron affinity increases with greater nuclear charge and smaller main quantum number.

Ionic Bonds

  • An ionic bond results from the transfer of electrons between atoms, creating oppositely charged ions, which are attracted to each other by strong electrostatic forces. These ions form a giant, three-dimensional structure called an ionic lattice.

Salt Structures

  • Salts form ionic crystalline structures. Essentially 90% of minerals are ionic compounds.
  • Sodium chloride (NaCl) is an example, exhibiting a positively charged sodium cation (Na+) and a negatively charged chlorine anion (Cl-). These ions arrange in a crystal lattice structure.
  • The repeating structure is called a formula unit in the crystal structure.
  • Ionic bonds are stronger than metallic bonds, and ionic crystals are typically brittle rather than malleable.

Finding Ionic Charges

  • Main group elements' ionic charges can be deduced from their position on the periodic table (PTE). Transition metals' charges must be memorized.
  • Some metals can form different ions, indicated in brackets after the name with Roman numerals (e.g., Fe2+, iron(II) ion / Fe3+, iron(III) ion).
  • Polyatomic ions' charges must be memorized.

Ionic Compound Formulas

  • Ionic compounds always contain cations and anions. Cations can be monoatomic or polyatomic; anions similarly.
  • Cations (positive) must balance the total negative charges of the anions to maintain charge neutrality.
  • Subscripts in the formula show the ratio of ions (e.g., CaCl2 signifies 2 chloride ions for every calcium ion).

Naming Ionic Compounds

  • Metal cations use the element name (e.g., Mg2+, magnesium cation).
  • For cations with multiple possible charges, a Roman numeral in parentheses shows the charge (e.g., Fe2+, iron(II)).
  • Non-metal anions' names add "-ide" to the root name (e.g., sulfur becomes sulfide; oxygen becomes oxide).
  • Polyatomic ions have specific names.

Ionic Compound Properties

  • High melting and boiling points due to strong electrostatic attractions between ions.
  • Brittle: Disruption of the crystal lattice structure leads to fracture.
  • Soluble in polar solvents (like water) due to ion-dipole interactions.
  • Conduct electricity when molten or dissolved (ions are mobile).

Dissolution of Ionic Compounds

  • Ionic compounds dissolve in water when ions separate from each other; this process is represented by an equation. (e.g., NaCl(s) → Na+(aq) + Cl-(aq).)

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