Ateneo - UPO

Review of the International System of Units. Atom: subatomic particles (protons, neutrons, electrons); mass number, atomic number. Atomic dimensions: angstrom, relative atomic mass, atomic mass unit. Mole and Avogadro’s number. Isotopes: definition, properties, and atomic weight. Ions.
Introduction to atomic models: Thomson model, Rutherford model, Bohr model, and the modern atomic model.
Quantum numbers, electronic configuration, Lewis structures.
Periodic table of elements: history and characteristics. Periodicity of element properties and determination of oxidation numbers.
Review of matter, concept of mass and weight. Pure substances (elements, compounds) and allotropes. Classification of elements (metals, nonmetals, semimetals, noble gases). Molecular compounds and molecular representation; ionic compounds (empirical formula, nomenclature of cations, anions, and polyatomic compounds). Mixtures (homogeneous, heterogeneous).
Solutions and concentration units: theory and exercises on molarity, molality, mass fraction (%), volume fraction (%), mass-volume fraction (%), parts per million (ppm), and dilutions.
Chemical reactions: characteristics and Proust’s law. Stoichiometry and reaction balancing. Redox reactions: characteristics and balancing.
Acids and bases: Arrhenius theory, Brønsted-Lowry theory, concept of conjugate acids and bases, amphoteric electrolytes.
K
a
K
a
​
: strength of acids and bases, ionization constants. Ionic product of water. pH and pOH. Calculation of pH for monoprotic acids, calculation of pH for strong bases.
Buffer solutions: pH of a buffer solution and Henderson-Hasselbalch equilibrium. Blood buffer system.
Formulas and systematic and traditional nomenclature of chemical compounds.
Further study and review of chemical bonds: covalent (nonpolar and polar), dative, ionic, metallic, sigma, and pi bonds

The course aims to provide students with the fundamental knowledge of general chemistry and laboratory chemistry, with particular attention to the basic concepts of the structure of matter, the properties of elements and compounds, chemical reactions, and stoichiometric principles.
The goal is to develop the ability to interpret chemical phenomena, solve simple quantitative problems, and correctly use chemical terminology, preparing students for both basic and applied scientific disciplines.

To successfully follow the course, it is useful to have basic knowledge of mathematics and physics at the high school level, in particular:
elementary notions of algebra and proportions;
concept of physical quantities and units of measurement;
notions of mass, weight, and density.

Lectures supported by multimedia presentations.
Guided classroom exercises on stoichiometry, concentration calculations, balancing reactions, and pH.

Written exam with numerical exercises (stoichiometry, solutions, pH, reaction balancing) and completion and open-ended questions on theoretical concepts.

1. Review of the International System of Units. Atom: subatomic particles (protons, neutrons, electrons); mass number, atomic number. Atomic dimensions: angstrom, relative atomic mass, atomic mass unit. Mole and Avogadro’s number. Isotopes: definition, properties, and atomic weight. Ions.
Introduction to atomic models: Thomson model, Rutherford model, Bohr model, and the modern atomic model.
Quantum numbers, electronic configuration, Lewis structures.
Periodic table of elements: history and characteristics. Periodicity of element properties and determination of oxidation numbers.
Review of matter, concept of mass and weight. Pure substances (elements, compounds) and allotropes. Classification of elements (metals, nonmetals, semimetals, noble gases). Molecular compounds and molecular representation; ionic compounds (empirical formula, nomenclature of cations, anions, and polyatomic compounds). Mixtures (homogeneous, heterogeneous).
Solutions and concentration units: theory and exercises on molarity, molality, mass fraction (%), volume fraction (%), mass-volume fraction (%), parts per million (ppm), and dilutions.
Chemical reactions: characteristics and Proust’s law. Stoichiometry and reaction balancing. Redox reactions: characteristics and balancing.
Acids and bases: Arrhenius theory, Brønsted-Lowry theory, concept of conjugate acids and bases, amphoteric electrolytes.
K
a
K
a
​
: strength of acids and bases, ionization constants. Ionic product of water. pH and pOH. Calculation of pH for monoprotic acids, calculation of pH for strong bases.
Buffer solutions: pH of a buffer solution and Henderson-Hasselbalch equilibrium. Blood buffer system.
Formulas and systematic and traditional nomenclature of chemical compounds.
Further study and review of chemical bonds: covalent (nonpolar and polar), dative, ionic, metallic, sigma, and pi bonds

At the end of the course, students will be able to:
describe the atomic and molecular structure of matter;
interpret atomic models and explain the periodicity of element properties;
correctly apply the concepts of mole, molar mass, concentration, and stoichiometry;
recognize and classify chemical reactions, balance them, and calculate quantitative relationships;
understand the concepts of acidity, basicity, and buffers, including pH calculations in different contexts;
use systematic and traditional chemical nomenclature;
communicate chemical concepts clearly and rigorously, both orally and in writing.