Inorganic Chemistry Basics

Inorganic Chemistry

Definition and Scope

• Branch of chemistry that deals with the study of inorganic compounds, which are typically derived from mineral sources
• Involves the study of the properties, preparation, and reactions of inorganic compounds

Types of Inorganic Compounds

• Acids: compounds that donate H+ ions (e.g. HCl, H2SO4)
• Bases: compounds that accept H+ ions (e.g. NaOH, Ca(OH)2)
• Salts: ionic compounds formed from the reaction of acids and bases (e.g. NaCl, CaCO3)
• Oxides: compounds containing oxygen and another element (e.g. CO2, Fe2O3)

Periodic Trends in Inorganic Chemistry

• Atomic Radius: decreases from left to right across a period, increases down a group
• Electronegativity: increases from left to right across a period, decreases down a group
• Ionization Energy: increases from left to right across a period, decreases down a group

Main Group Elements

• Alkali Metals (Group 1): highly reactive, lose one electron to form a +1 ion (e.g. Li, Na, K)
• Alkaline Earth Metals (Group 2): less reactive, lose two electrons to form a +2 ion (e.g. Mg, Ca, Sr)
• Halogens (Group 17): highly reactive, gain one electron to form a -1 ion (e.g. F, Cl, Br)
• Noble Gases (Group 18): unreactive, do not easily form ions (e.g. He, Ne, Ar)

Transition Metals

• Characteristics: exhibit multiple oxidation states, form colored ions, and are often used as catalysts
• Examples: Fe, Cu, Zn, Ag, Au

Coordination Compounds

• Definition: complexes formed between a central metal atom and surrounding ligands
• Nomenclature: use prefixes to indicate the number of ligands and the metal's oxidation state
• Examples: [Fe(H2O)6]3+, [Cu(NH3)4]2+

Acid-Base Chemistry

• Arrhenius Theory: acids donate H+ ions, bases accept H+ ions
• Brønsted-Lowry Theory: acids donate H+ ions, bases accept H+ ions, and conjugate acid-base pairs form
• pH: a measure of the concentration of H+ ions, with a pH of 7 being neutral