Inorganic Chemistry Chapter 2

Study Notes

Inorganic chemistry focuses on the synthesis and behavior of inorganic and organometallic compounds.
It plays a crucial role in various industries, including catalysis, materials science, pigments, surfactants, coatings, medications, fuels, and agriculture.

The periodic table organizes elements by atomic weight, chemical symbols, and atomic numbers.
It reveals periodic trends in properties among atoms.
Vertical columns (groups) contain elements with the same number of valence electrons, leading to similar properties.
Glenn T. Seaborg reconfigured the periodic table in the mid-20th century, placing actinoids below lanthanoids and discovering all trans-uranium elements from 94 to 102.
Seaborg was awarded the Nobel Prize in Chemistry in 1951; element 106 is named Seaborgium (Sg) in his honor.
The periodic table highlights that chemical elements are organized by family traits, essential for understanding chemistry's foundational structure.

Physical properties show distinct trends:
- Atomic Radius: Varies predictably across periods and groups.
- Ionic Radius: Differences between cations and anions.
- Ionization Enthalpy: Energy required to remove an electron.
- Electron Gain Enthalpy: Energy change when an electron is added to an atom.
- Electronegativity: Measure of an atom's ability to attract electrons in a bond.
Chemical properties reflect:
- Periodicity of Valence or Oxidation States: Trends in how elements lose or gain electrons.
- Anomalous Properties of Second Period Elements: Unique traits influencing chemical behavior.

Ionic Bond: Formed through the transfer of electrons between atoms.
Covalent Bond: Involves the sharing of electron pairs between atoms.
Coordinate Covalent Bond: A type of covalent bond where one atom provides both electrons.
Metallic Bond: Characterized by a "sea of electrons" that allow conductivity and malleability.
Hydrogen Bond:
- Intermolecular H-bond: Bonds between molecules affecting boiling and melting points.
- Intramolecular H-bond: Bonds occurring within a molecule influencing its structure.

Mole: A unit measuring the amount of substance, defined as containing exactly 6.022 x 10²³ particles.
Molar Mass: Total mass of one mole of a substance, used for conversions.
Mass Percentage of Element: Percentage of a specific element's mass in a compound.

Types of Solution: Different methods of combining solute and solvent.
Concentration of Solution:
- % w/w: Weight percent concentration.
- Mole Fraction (x): Ratio of the number of moles of a component to the total moles in the mixture.
- Molarity (M): Moles of solute per liter of solution.
- Molality (m): Moles of solute per kilogram of solvent.
- Normality (N): Equivalent concentrations of a solution.

Ionic Solids: Formed from ionic bonds, characterized by high melting and boiling points.
Metallic Solids: Composed of metal atoms, exhibiting electrical and thermal conductivity.
Molecular Solids: Composed of molecules held together by intermolecular forces.
Network Solids: Atoms connected by covalent bonds in a continuous network, resulting in high strength and melting points.