Fundamentals and Applications of Inorganic Chemistry
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Course
Inorganic Chemistry
Institution
Bachillerato
This document provides an overview of inorganic chemistry, highlighting its characteristics, types of compounds, and chemical formulas. It explores the different formulas that represent the composition and structure of inorganic compounds, along with specific examples of important compounds and the...
Inorganic chemistry is the branch of chemistry that studies compounds made of elements
other than primarily carbon and hydrogen, which are the focus of organic chemistry. This
discipline investigates and describes the properties, structures, reactions, and applications
of inorganic compounds, including a wide variety of substances such as salts, acids, bases,
oxides, and metals.
Characteristics of Inorganic Chemistry
Elements involved: It covers almost all elements in the periodic table, especially metals
and nonmetals.
Types of compounds: Includes simple compounds like water (H₂O) and carbon dioxide
(CO₂), as well as more complex compounds such as minerals and metal catalysts.
Chemical bonding: Inorganic compounds typically form ionic bonds (between metals and
nonmetals) or covalent bonds (between nonmetals).
Chemical Formulas in Inorganic Chemistry
Chemical formulas represent the composition and structure of inorganic compounds.
Below are explanations of different types of formulas along with examples.
1. Empirical Formula
Represents the simplest ratio of atoms present in a compound.
Example: Iron(III) oxide has the empirical formula Fe₂O₃, showing that for every 2 iron
atoms, there are 3 oxygen atoms. This formula doesn’t show the exact arrangement of
atoms, just the ratio.
2. Molecular Formula
Indicates the exact number of atoms of each element in a molecule.
Example: Carbon dioxide has the molecular formula CO₂. Each molecule contains one
carbon atom and two oxygen atoms, held together by covalent bonds.
3. Structural Formula
Shows how the atoms are connected within a molecule, indicating the arrangement of
bonds.
Example: Water (H₂O) has a structural formula showing that the oxygen atom is bonded to
two hydrogen atoms via covalent bonds. The angular arrangement of bonds can also be
depicted in more detailed structural formulas.
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