Rutgers Chemistry Courses – Chemical Principles 1 in PDF

Spread the love
  •  
  •  
  •  
  •  
  •  
  •  

Rutgers Chemistry Courses – Chemical Principles 1 in PDF by Alex J. Roche Rutgers University, Department of Chemistry. All official syllabi / course can be found in the online web post.

Rutgers Chemistry Courses

Rationale:

Chemistry is the molecular science. Chemists believe that the best understanding of the properties of matter comes from study at the molecular level.
For example, boiling points, acidity, chemical reactivity, taste, smell, drug efficacy, colour, toxicity, etc., can all be understood/predicted/explained by a
consideration of the relevant atoms/ions and the bonds connecting them. This course provides the basic principles that govern the structure (and therefore
the behaviour and reactivity) of atoms, ions and molecules.

(Recommended) Textbook:

Chemistry:

  1. The Molecular Nature of Matter, 7th Edn, Jespersen and Hyslop.
    Or
    2. Chemistry, 10th Edn Chang and Goldsby.
    The following textbooks are also good, and acceptable:
    1. General Chemistry, 4th Edn by McQuarrie, Rock and Gallogly
    2. Chemistry, the Central Science, 10th Edn, Brown, LeMay and Bursten.
    3. Chemical Principles, Atkins and Jones.
    Openstax.org offer two great FREE Chemistry textbooks, at
    https://openstax.org/subjects/science

The following concepts are taught in Chemical Principles 1 lecture:

Matter & Measurement extra that are in the Rutgers Website
Chemical Reactions & Stoichiometry
• Solution Chemistry
The Gas Laws
Thermochemistry and Chemical Energy
Quantum theory and Electronic Structural Models
Periodicity
Chemical Bonding Theories
Molecular Geometries

Course Objectives:

Upon successful completion a student will be proficient at:
-Explanations at the atomic/molecular level,
-Qualitative explanations (illustrations / examples / words),
-Quantitative explanations using math,
-Simple algebraic calculations.

More precisely, the student will be able to:

• Identify the subatomic particles in an atom that differentiate one isotope of an element from another and one type of element from another;
• Predict formulas of molecules and ions, and name common chemical compounds.
• Use dimensional analysis, the metric system and the mole concept to calculate empirical and molecular formulas given basic information for chemical reactions, and further apply these concepts to more complicated limiting reagents and yields.
• Predict qualitative outcomes of chemical equations in solution (e.g. acid/base and redox reactions, etc.), using known patterns (solubility rules), and complete
quantitative calculations (molarity).
• Quantitatively manipulate the gas laws, and qualitatively predict gas behavior based upon the tenets of the kinetic molecular theory of gases, including
deviations from ideality.
• Understand the nature of energy and energy changes in reactions, and calculate calorimetry, and standard enthalpy changes.
• Identify the electronic structure of atoms and ions (e.g. quantum numbers, orbitals, oxidation states, etc.) as well as the periodic relationships among the
elements and associated physical properties (e.g. ionization energy, atomic radius, etc.).
• Differentiate between the basic concepts of chemical bonding (ionic and covalent bonding, bond enthalpy, etc.), and use the accepted bonding theories (of
Lewis structures, Valence Bond Theory, VSEPR, etc.) to predict the relationships between chemical structure and physical properties (dipole moment, etc.).

Old Exams with ANSWERS

Old Examination with Answer by Our DPT Sir


Spread the love
  •  
  •  
  •  
  •  
  •  
  •  

Leave a Comment