Chemistry Chapter 4 Notes

Chapter Overview

  • Development of chemical equations and concepts involving ionic and molecular compounds.

Subatomic Particles

  • Types of Particles:
    • Protons: Relative mass 1836, positive charge.
    • Neutrons: Relative mass 1837, neutral charge.
    • Electrons: Relative mass 1, negative charge.

Periodic Table Insights

  • Key Information:
    • Atomic number, symbol, atomic mass, ion charges.
    • Elements arranged in groups (families) 1-18 and periods 1-7.

Properties of Elements

  • Metals:
    • Good conductors of heat and electricity; solid (except mercury); malleable; ductile.
  • Non-metals:
    • Poor conductors; can be solid, liquid, or gas; brittle; non-ductile.
  • Metalloids:
    • Properties of both metals and nonmetals; includes silicon and germanium.

Atomic Structure Diagrams

  • Bohr-Rutherford Diagrams:
    • Show protons and neutrons in the nucleus and electrons in shells.

Ionic Compounds Formation

  • Ionic Compounds:
    • Form from the transfer of electrons between metals (cations) and nonmetals (anions).
    • Metals lose electrons; nonmetals gain electrons.

Writing and Naming Ionic Compounds

  • Binary Ionic Compounds: Composed of two elements (metal + nonmetal).
  • Steps for Writing Formulas:
    1. Identify each ion and charge.
    2. Balance positive and negative charges.
    3. Use subscripts for ratios of ions.
  • Cross-over Method for formulas.

Multivalent Metals

  • Metals with multiple charges can form various ions. Example: Copper (I) vs Copper (II).

Polyatomic Ions

  • Definition: Ions composed of multiple atoms; involved in ternary compounds.
  • Writing Formulas: Similar process as binary compounds but includes polyatomic ion identification.