There are no prerequisites for this subject, although it is recommended that the student has studied chemistry in high school. Likewise, it would be advisable for the student to know the nomenclature of inorganic compounds, according to IUPAC rules, as well as the most common traditional formulations, and the physical-chemical magnitudes and the units.

The student of Food Science and Technology degree must acquire the conceptual, manual and technical tools that allow him/her to exercise in an important field within the food industry. To do so, it is essential that they acquire a solid knowledge of the fundamentals and bases of Chemistry. The subject of General Chemistry aims to help students to understand in depth the chemical concepts they have acquired during their secondary education, to complete them and to acquire the necessary skills for their application to the practical cases that will be presented, both in their future professional life and when studying other subjects of the curriculum. Specifically, this course will deal with the description of chemical bonding and the study of chemical reactions, stoichiometry, the structure of matter, as well as the periodic properties of the elements.

 General Chemistry is an annual basic subject, which will be taught in the first year and is an essential starting point for the proper learning of other subjects of the degree of Food Science and Technology.

Course competences
Code	Description
CB01	Prove that they have acquired and understood knowledge in a subject area that derives from general secondary education and is appropriate to a level based on advanced course books, and includes updated and cutting-edge aspects of their field of knowledge.
E01	To acquire basic knowledge in chemistry, mathematics, physics to allow the study of the nature of foods, causes of their alteration and fundamentals of their production processes
E03	To know and be able to apply fundamentals of chemistry, as well its applications in analytical chemistry, organic chemistry, physical chemistry and inorganic chemistry in the field of the Food Science and Technology
E05	To know the composition, phyco-chemical properties, nutritional value and sensory properties of foods
G01	To develop the aptitude to gather and interpret information and data to issue critical judgments that include a reflection on relevant topics of social, scientific or ethical nature.
G02	To possess a correct oral and written communication. To transmit information, ideas, problems and solutions to a both specialized and not specialized public.
G04	To develop the necessary skills of learning to undertake later studies with a high degree of autonomy.
G07	To possess ability of organization and planning, initiative, entrepreneurship and aptitude to be employed in teamworks. To possess capacity of resolution of specific problems of the professional area and to develop the critical reasoning and decision making.
G08	To know the principles and the theories of Basic Science as well as the methodologies and applications of the chemistry, physics, biology and mathematics that are necessary to acquire the specific knowledge of the Degree.

Course learning outcomes
Description
Homogenize the knowledge of Chemistry already acquired by students in the Middle Education courses and complete certain aspects that have not been previously studied with the necessary depth.
Learn to work autonomously in a laboratory and know how to interpret the experimental results obtained.
Know the fundamentals of molecular structure, chemical thermodynamics and chemical kinetics.
To ensure that the student acquires the basic terminology of Chemistry and knows how to use it, as well as being able to establish relationships between the different concepts.
Having a basic knowledge of some electrochemical phenomena and their applications
Know the different units correctly.
Know the basic concepts and principles of Chemistry, so that the essential foundations are laid so that they can successfully face the study of the different branches of the discipline.
Additional outcomes
Not established.

• Unit 1: Chemical formulation. Chemical reactions and equations. Stoichiometry. Concentration units. Limiting reagent. Reaction yields
• Unit 2: Origins of the quantum theory of the atom. Electrical nature of matter: Thomson and Mullikan experiments. Fundamental particles: electrons, protons and neutrons. Rutherford's atomic model. The atomic nucleus. Dual nature of electromagnetic radiation: Planck equation. Dual nature of matter: de Broglie hypothesis. Uncertainty principle. Bohr's atomic model. Atomic spectra: hydrogen emission spectrum.
• Unit 3: Atomic structure. Schrödinger equation: wave function. Probability. Solution of the wave equation for hydrogenoid atoms. Quantum numbers and atomic orbitals. Physical meaning and graphical representations of the orbitals of the hydrogen atom. Polyelectronic atoms.
• Unit 4: Periodic properties of the elements. Introduction. Pauli exclusion principle. Auf-Bau principle and electronic configurations. Hund's rule. Periodic classification of the elements: Periodic table. Periodic properties: atomic radii. Ionisation potentials. Electronic affinity.
• Unit 5: Molecular structure: Covalent bonding. Introduction to chemical bonding. Method of approach to molecular geometry: Lewis structures. Valence bond theory. Hybridisation. Theory of molecular orbitals. Application to homonuclear diatomic molecules of second period elements. Application to diatomic heteronuclear molecules of the second period. Ionic character of a covalent bond: electronegativity, Pauling scale. Intermolecular forces: van der waals forces and hydrogen bridges
• Unit 6: Solid state: Ionic and metallic bonding. Introduction. Types and properties of crystalline solids: molecular solids, covalent solids, ionic solids and metallic solids. Crystal structure of ionic solids. Ionic radii. Reticular energy: Born-Haber cycle and Born-Landé equation. Polarisation and covalent character of the ionic bond. Fajans' rules. Introduction to metallic bonding.
• Unit 7: Gases. Pressure of a gas. Gas laws: Boyle's Law, Charles and Gay-Lussac's Law, Avogadro's Law. Absolute temperature scale. Ideal gas equation. Determination of molecular weights and formulas. Dalton's law of partial pressures. Kinetic theory of gases. Graham's law: diffusion and effusion of gases. Real gases
• Unit 8: Chemical Thermodynamics. Work. Heat and its measurement. First Law of Thermodynamics: internal energy. Enthalpy and heat. Thermochemistry: enthalpies of reaction, formation and combustion. Hess's law. Binding energy. Heat capacity. Second Law of Thermodynamics. Spontaneous processes and entropy. Gibbs free energy.
• Unit 9: Solutions. Ideal solutions (non-volatile solutes). Raoult's Law. Colligative properties: non-ideal solutions (Henry's law). Introduction to electrolyte solutions: interactions between ionic solutes and water (strong and weak electrolytes); activity and activity coefficient; properties of the activity coefficients
• Unit 10: Chemical equilibrium (gas phase equilibria) equilibria in solution. Reversible and irreversible reactions. Equilibrium state characteristics Free energy and equilibrium constant Concentration and equilibrium constant Relationship between the different chemical equilibrium constants for a homogeneous gaseous system. Factors affecting the equilibrium position (temperature, concentration, pressure). Acid-base equilibrium. Volumetry.
• Unit 11: Introduction to the laboratory. Safety in the laboratory. The laboratory notebook. Laboratory materials. Preparation of solutions. Precipitation and crystallisation. Filtration techniques Separation of liquids by distillation Recrystallisation of organic products Determination of melting point. Chromatographic techniques. Thin Layer and Column Chromatography. Extraction of caffeine from different sources.

Training Activity	Methodology	Related Competences (only degrees before RD 822/2021)	ECTS	Hours	As	Com	Description
Class Attendance (theory) [ON-SITE]	Combination of methods	E01 G04 G08	1.76	44	N	N
Workshops or seminars [ON-SITE]	Project/Problem Based Learning (PBL)	CB01 E01 E03 G01 G02 G04 G08	1.24	31	Y	N
Class Attendance (practical) [ON-SITE]	Practical or hands-on activities	E01 E03 G04 G08	1.52	38	Y	Y
Study and Exam Preparation [OFF-SITE]	Self-study	E01 G04	1.6	40	N	N
Mid-term test [ON-SITE]	Assessment tests	CB01 E03 G01 G02	0.28	7	Y	N
Other off-site activity [OFF-SITE]	Self-study	G04 G07	5.6	140	N	N
Total:			12	300
Total credits of in-class work: 4.8			Total class time hours: 120
Total credits of out of class work: 7.2			Total hours of out of class work: 180

As: Assessable training activity
Com: Training activity of compulsory overcoming (It will be essential to overcome both continuous and non-continuous assessment).

Evaluation System	Continuous assessment	Non-continuous evaluation *	Description
Assessment of problem solving and/or case studies	20.00%	0.00%	Problem-solving by the student will be positively valued, as well as his active participation in class. On the other hand, the student will be able to increase his continuous evaluation grade by giving seminars and questions at the teacher's suggestion.
Laboratory sessions	20.00%	20.00%	Attendance at all practical laboratory classes is mandatory. The skill acquired in the handling of chemical substances as well as of the laboratory material, the student's attitude and the adequate elaboration of the laboratory notebook will be valued. To pass the course it will be essential to have carried out and approved the laboratory practices and the test.
Mid-term tests	60.00%	80.00%	There will be a progress test at the end of each term, compulsory to pass the course by continuous assessment, in which the student must demonstrate that he has acquired the corresponding knowledge.
Total:	100.00%	100.00%

Not related to the syllabus/contents
Hours	hours
Study and Exam Preparation [AUTÓNOMA][Self-study]	26
Mid-term test [PRESENCIAL][Assessment tests]	7

Unit 1 (de 11): Chemical formulation. Chemical reactions and equations. Stoichiometry. Concentration units. Limiting reagent. Reaction yields
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	3
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	7
Study and Exam Preparation [AUTÓNOMA][Self-study]	24

Unit 2 (de 11): Origins of the quantum theory of the atom. Electrical nature of matter: Thomson and Mullikan experiments. Fundamental particles: electrons, protons and neutrons. Rutherford's atomic model. The atomic nucleus. Dual nature of electromagnetic radiation: Planck equation. Dual nature of matter: de Broglie hypothesis. Uncertainty principle. Bohr's atomic model. Atomic spectra: hydrogen emission spectrum.
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	2
Study and Exam Preparation [AUTÓNOMA][Self-study]	4

Unit 3 (de 11): Atomic structure. Schrödinger equation: wave function. Probability. Solution of the wave equation for hydrogenoid atoms. Quantum numbers and atomic orbitals. Physical meaning and graphical representations of the orbitals of the hydrogen atom. Polyelectronic atoms.
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	2
Study and Exam Preparation [AUTÓNOMA][Self-study]	4

Unit 4 (de 11): Periodic properties of the elements. Introduction. Pauli exclusion principle. Auf-Bau principle and electronic configurations. Hund's rule. Periodic classification of the elements: Periodic table. Periodic properties: atomic radii. Ionisation potentials. Electronic affinity.
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	3
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	3
Study and Exam Preparation [AUTÓNOMA][Self-study]	14

Unit 5 (de 11): Molecular structure: Covalent bonding. Introduction to chemical bonding. Method of approach to molecular geometry: Lewis structures. Valence bond theory. Hybridisation. Theory of molecular orbitals. Application to homonuclear diatomic molecules of second period elements. Application to diatomic heteronuclear molecules of the second period. Ionic character of a covalent bond: electronegativity, Pauling scale. Intermolecular forces: van der waals forces and hydrogen bridges
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	6
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	5
Study and Exam Preparation [AUTÓNOMA][Self-study]	22

Unit 6 (de 11): Solid state: Ionic and metallic bonding. Introduction. Types and properties of crystalline solids: molecular solids, covalent solids, ionic solids and metallic solids. Crystal structure of ionic solids. Ionic radii. Reticular energy: Born-Haber cycle and Born-Landé equation. Polarisation and covalent character of the ionic bond. Fajans' rules. Introduction to metallic bonding.
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	4
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	2
Study and Exam Preparation [AUTÓNOMA][Self-study]	12

Unit 7 (de 11): Gases. Pressure of a gas. Gas laws: Boyle's Law, Charles and Gay-Lussac's Law, Avogadro's Law. Absolute temperature scale. Ideal gas equation. Determination of molecular weights and formulas. Dalton's law of partial pressures. Kinetic theory of gases. Graham's law: diffusion and effusion of gases. Real gases
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	4
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	2
Study and Exam Preparation [AUTÓNOMA][Self-study]	12

Unit 8 (de 11): Chemical Thermodynamics. Work. Heat and its measurement. First Law of Thermodynamics: internal energy. Enthalpy and heat. Thermochemistry: enthalpies of reaction, formation and combustion. Hess's law. Binding energy. Heat capacity. Second Law of Thermodynamics. Spontaneous processes and entropy. Gibbs free energy.
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	5
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	5
Study and Exam Preparation [AUTÓNOMA][Self-study]	21

Unit 9 (de 11): Solutions. Ideal solutions (non-volatile solutes). Raoult's Law. Colligative properties: non-ideal solutions (Henry's law). Introduction to electrolyte solutions: interactions between ionic solutes and water (strong and weak electrolytes); activity and activity coefficient; properties of the activity coefficients
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	3
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	3
Study and Exam Preparation [AUTÓNOMA][Self-study]	12

Unit 10 (de 11): Chemical equilibrium (gas phase equilibria) equilibria in solution. Reversible and irreversible reactions. Equilibrium state characteristics Free energy and equilibrium constant Concentration and equilibrium constant Relationship between the different chemical equilibrium constants for a homogeneous gaseous system. Factors affecting the equilibrium position (temperature, concentration, pressure). Acid-base equilibrium. Volumetry.
Activities	Hours
Class Attendance (theory) [PRESENCIAL][Combination of methods]	5
Workshops or seminars [PRESENCIAL][Project/Problem Based Learning (PBL)]	9
Study and Exam Preparation [AUTÓNOMA][Self-study]	29

Unit 11 (de 11): Introduction to the laboratory. Safety in the laboratory. The laboratory notebook. Laboratory materials. Preparation of solutions. Precipitation and crystallisation. Filtration techniques Separation of liquids by distillation Recrystallisation of organic products Determination of melting point. Chromatographic techniques. Thin Layer and Column Chromatography. Extraction of caffeine from different sources.
Activities	Hours
Class Attendance (practical) [PRESENCIAL][Practical or hands-on activities]	40

Global activity
Activities	hours

Author(s)	Title	Book/Journal	Citv	Publishing house	ISBN	Year	Description	Link	Catálogo biblioteca
Brown, Lemay, Bursten, Murphy, Woodward	Química. La Ciencia Central			Pearson	978-607-32-2237-2	2014
Chang, Raymond	Química			McGraw-Hill	978-607-15-0928-4	2013
Domínguez Reboiras, Miguel Ángel	Química : la ciencia básica			Thomson Paraninfo	978-84-9732-347-5	2008
Orozco C.; González N.; Pérez A.	Problemas Resueltos de Química Aplicada			Paraninfo	978-84-283-8092-8	2011
Peterson, W. R.	Formulación y nomenclatura química inorgánica : [según la n			EDUNSA, Ediciones y Distribuciones Universitari	84-85257-04-9	1996
Petrucci, Ralph H.	Química general (english version)			Pearson-Prentice Hall	978-84-205-3533-3	2010
Whitten, Kenneth W.	Química general			McGraw-Hill	84-481-1386-1	2002