Untitled Flashcards Set

Metals: Bonding, Structure, and Properties

Metallic Bonding

• Definition: Metallic bonding is the electrostatic attraction between positively charged metal ions and a "sea" of delocalized electrons.

• Structure: Metals exist as a lattice of cations surrounded by free-moving electrons.

Properties of Metals

1. Good conductors of electricity – Free-moving electrons carry charge.

2. Good conductors of heat – Delocalized electrons transfer kinetic energy.

3. Malleable and ductile – Layers of atoms can slide over each other without breaking bonds.

4. High melting and boiling points – Strong electrostatic forces require significant energy to break.

5. High densities – Close-packed atomic structure.

Metal Recycling and the Circular Economy

• Metals are mined, refined, manufactured, used, disposed of, and recycled.

• Recycling reduces environmental impact and conserves resources.

• Examples: Aluminum cans, steel, copper wiring.

Ionic Bonding and Structure

Ionic Bonding

• Occurs between metals (cations) and non-metals (anions).

• Electrons are transferred from metal to non-metal, creating oppositely charged ions.

Lattice Structure of Ionic Solids

• Arrangement: A repeating 3D lattice of alternating positive and negative ions.

• Strength: Held together by strong electrostatic forces (ionic bonds).

Properties of Ionic Compounds

1. High melting and boiling points – Strong ionic bonds require much energy to break.

2. Hard but brittle – Applying force disrupts lattice and causes repulsion between like charges.

3. Conducts electricity in molten or aqueous states but not as a solid – Ions must be free to move.

4. Solubility – Many dissolve in water due to interactions with polar water molecules.

Ionic Compound Naming and Formulas

• Common polyatomic ions:

  • Ammonium (NH₄⁺)

  • Carbonate (CO₃²⁻)

  • Hydroxide (OH⁻)

  • Nitrate (NO₃⁻)

  • Sulfate (SO₄²⁻)

• Always soluble ions (SNAPE rule):

  • Sodium (Na⁺)

  • Nitrate (NO₃⁻)

  • Ammonium (NH₄⁺)

  • Potassium (K⁺)

  • Ethanoate (CH₃COO⁻)

Covalent Bonding and Structure

Types of Covalent Substances

1. Discrete (small) molecules – e.g. H₂O, CO₂, CH₄.

2. Covalent lattices – e.g. Diamond, graphite, SiO₂.

Representing Covalent Bonding

• Lewis (electron dot) structures – Shows valence electrons.

• Structural formulas – Shows bonds between atoms.

Electronegativity and Polarity

• Electronegativity: Ability of an atom to attract electrons.

• Bond polarity:

  • Non-polar: Electrons shared equally (e.g. O₂, CH₄).

  • Polar: Unequal sharing (e.g. HCl, H₂O).

• Molecular polarity depends on bond polarity and shape.

Shapes of Simple Molecules

1. Linear – e.g. CO₂

2. Bent (V-shaped) – e.g. H₂O

3. Trigonal pyramidal – e.g. NH₃

4. Tetrahedral – e.g. CH₄

Intermolecular Forces

1. Dispersion forces (London forces) – Weak, present in all molecules, stronger in larger molecules.

2. Dipole-dipole interactions – Between polar molecules.

3. Hydrogen bonding – Strongest, occurs in molecules with H bonded to N, O, or F (e.g. H₂O, NH₃).

Properties of Covalent Substances

• Small molecules:

  • Low melting and boiling points (weak intermolecular forces).

  • Poor conductivity (no free-moving charges).

• Large molecules:

  • Higher melting/boiling points than small molecules.

• Noble gases:

  • Exist as single atoms, very low melting/boiling points (weak dispersion forces).

Diamond and Graphite: Structure and Properties

Diamond

• Each carbon forms 4 strong covalent bonds.

• Properties:

  • Hard (strong bonds).

  • High melting/boiling points.

  • Non-conductive (no free electrons).

Graphite

• Each carbon forms 3 bonds, creating layers.

• Free electrons allow conductivity.

• Properties:

  • Conductive (delocalized electrons).

  • Soft (layers slide over each other).

Instructions for the AI Creating the Practice Test

1. Ensure a variety of question types:

   • Multiple choice

   • Short answer

   • Fill-in-the-blanks

   • Labeling diagrams

   • Explanation questions

2. Cover all key concepts:

   • Metallic, ionic, and covalent bonding

   • Properties of metals, ionic compounds, and covalent substances

   • Structure and bonding explanations

   • Intermolecular forces

   • Naming and writing formulas for ionic compounds

3. Create application-based questions:

   • "Explain why metals conduct electricity."

   • "Compare the structure of diamond and graphite and explain their properties."

   • "Predict whether CO₂ is polar based on its shape and electronegativity."

4. Include recall and problem-solving questions:

   • "Write the formula for calcium nitrate."

   • "Which of the following molecules has hydrogen bonding?"

   • "Identify the shape of NH₃ and explain why it is polar."

This should be a complete resource for your Quizlet and practice tests! Let me know if you need anything adjusted or expanded.