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Questions and Answers
What is the process of forming cations primarily dependent on?
What is the process of forming cations primarily dependent on?
Which property of ionic bonds makes ionic crystals brittle?
Which property of ionic bonds makes ionic crystals brittle?
Anions form when metals gain electrons.
Anions form when metals gain electrons.
False
Define ionization energy.
Define ionization energy.
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The ionic charge of elements in the main groups can be derived from their position in the periodic table.
The ionic charge of elements in the main groups can be derived from their position in the periodic table.
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What is the ionic charge of the zinc ion?
What is the ionic charge of the zinc ion?
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The strong electrostatic attraction forces between cations and anions create an __________ bond.
The strong electrostatic attraction forces between cations and anions create an __________ bond.
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The formula for calcium chloride is CaCl______.
The formula for calcium chloride is CaCl______.
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Match the following terms with their definitions:
Match the following terms with their definitions:
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Match the ions with their corresponding formulas:
Match the ions with their corresponding formulas:
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Which of the following statements about ionic bonds is true?
Which of the following statements about ionic bonds is true?
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Electrons in an ionic lattice structure are free to move in any direction.
Electrons in an ionic lattice structure are free to move in any direction.
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Which of the following ions is a polyatomic cation?
Which of the following ions is a polyatomic cation?
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What is the result of combining a sodium ion (Na+) and a chlorine ion (Cl−)?
What is the result of combining a sodium ion (Na+) and a chlorine ion (Cl−)?
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Transition metals always have a single ionic charge.
Transition metals always have a single ionic charge.
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Ionic compounds are always composed of ______ and ______.
Ionic compounds are always composed of ______ and ______.
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What is the correct formula for aluminium oxide?
What is the correct formula for aluminium oxide?
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Cations derived from non-metals end in -IDE.
Cations derived from non-metals end in -IDE.
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What is the name of the cation with the formula Fe2O3?
What is the name of the cation with the formula Fe2O3?
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Sodium chloride (NaCl) separates into ___ and ___ ions when dissolved in water.
Sodium chloride (NaCl) separates into ___ and ___ ions when dissolved in water.
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Which of the following is a property of ionic compounds?
Which of the following is a property of ionic compounds?
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Match the following anions with their respective non-metal elements:
Match the following anions with their respective non-metal elements:
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Most ionic compounds are soluble in water.
Most ionic compounds are soluble in water.
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The cation magnesium is represented as ___ in chemical notation.
The cation magnesium is represented as ___ in chemical notation.
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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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Description
This quiz explores the fundamental concepts of ionic bonding, including the formation of cations and anions, ionization energy, and electron affinity. Understand how the transfer of electrons creates strong electrostatic attractions between oppositely charged ions.
