PHRC 4110 Pharmaceutics I
|
|
- Agatha Thompson
- 5 years ago
- Views:
Transcription
1 CO01: Use interpretive tools for proper data handling CO01.01: Describe basic mathematics and statistic to interpret pharmaceutical data CO01.02: Work with exponents, powers, roots, logarithms, and antilogarithms CO01.03: Interpret straight line equations CO01.04: Convert units CO01.05: Perform dimensional analysis CO01.06: Describe significant figures CO01.07: 07: Calculate equivalent weight CO01.08: Describe basic statistics including mean, median, mode, and standard deviation, precision and accuracy CO02: Define the states of matter and forces in materials determining the property and performance of the CO02.01: Define differences between the states of matter CO02.02: Describe how states of matter change CO02.03: Describe difference between intensive and extensive properties CO02.04: Discuss phase diagrams for a pure substance and a binary system CO02.05: Discuss crystal, amorphous, liquid crystals and polymorphism CO02.06: Describe basic concepts of pressure, temperature, volume and their relationships CO02.07: Define ionic and covalent bonding, intra and intermolecular forces CO02.08: Differentiate the role of intermolecular forces and their roles in defining material property, drug stability, degradation, interaction CO02.09: Differentiate the solution and solid state properties of the materials CO02.10: Discuss factors affecting properties of the material in solution and solid states CO02.11: Describe Van der Waals forces, and their importance in drug product preparation and stability CO02.12: Describe permanent dipoles, induced dipoles, hydrogen bonding, and their importance in drug products CO02.13: Correlate material structure and its intermolecular forces CO03: Describe the basics of thermodynamics, and its application in pharmaceutical dosage forms CO03.01: Define concepts, including internal energy, heat, work, system, surrounding, universe, and apply them to pharmaceutical examples CO03.02: Describe thermodynamic terms and thermodynamic laws CO03.03: Differentiate exothermic and endothermic reactions CO03.04: Define process enthalpies, spontaneous and non-spontaneous reactions or process, entropy and Gibbs free energy CO03.05: Discuss how all processes in relation to drug formulation and development are governed by thermodynamics CO04: Describe electrolyte/non-electrolyte properties of materials, and the effect of ph on drug solubility CO04.01: Describe electrolyte, non-electrolyte, weak and strong electrolytes, and correlate the concept to drug active ingredient CO04.02: Calculate concentrations by molality, molarity, normality, fraction and percent CO04.03: Describe the difference between ideal and non-ideal solutions, the importance of Raoult's and Henry's laws CO04.04: Describe colligative properties, lowering vapor pressure, boiling point elevation, freezing point depression, osmotic pressure CO04.05: 05: Use colligative properties for material characterization (e.g., molecular weight) CO04.06: Define dissociation, association, activity and, ionic strength, and how drug properties may change with the surrounding environment CO04.07: Describe theories of acids and bases, and conjugate pairs CO04.08: Define weak and strong acids and bases with drug examples CO04.09: Calculate ph of strong acids and bases CO04.10: Calculate ph of weak acids and bases on drug examples CO04.11: Discuss the importance of Ka, Kb, pka and pkb, acidity and basicity, and use them in calculations
2 CO04.12: Discuss the importance of water ionization, Kw and pkw, effect of temperature, and use them in calculations CO04.13: Discuss the Le Chateliers' Principle CO04.14: Describe Titration curves CO04.15: Define equivalence points CO04.16: Describe acidic and basic buffers CO04.17: Calculate buffer capacity and maximum buffer capacity CO04.18: Calculate ph of buffered systems CO05: Describe basic concepts of solubility, partitioning, and diffusion CO05.01: Describe the difference between solubility and dissolution rate CO05.02: Define factors affecting solubility and melting CO05.03: Describe solvents and their dielectric constants CO05.04: Discuss the correlation between ph, ionization and solubility CO05.05: Describe approaches to improve solubility or permeability CO05.06: Define BCS Classification, I-IV IV CO05.07: Discuss solvent-solvent, solute-solute, solvent-solute interaction CO05.08: Discuss the correlation between temperature, heat of solution, solubility CO05.09: Define partitioning, partition coefficient ans solubility, partition coefficient and permeability, distribution coefficient CO05.10: Describe diffusion concepts, and factors affecting diffusion CO05.11: Apply Noyes-Whitney equation CO06: Describe drug stability and factors affecting the drug degradation, as well as the rate (kinetics) at CO06.01: 01 Describe stability and factors affecting drug stability CO06.02: Define drug degradation through hydrolysis, oxidation, photolysis, racemization, adsorption, absorption CO06.03: Describe how to maintain drug stability CO06.04: Discuss the importance of excipients in stability and degradation of drug products CO06.05: Describe the importance of reaction law and rate, activation energy CO06.06: Discuss the effect of temperature, ionic strength, catalyst, H, OH, and buffers on reaction rate CO06.07: Define the difference between zero, first and second order reactions CO06.08: Differentiate and identify various reactions CO06.09: Calculate Half-life and shelf life (expiration) CO06.10: Discuss the correlation between Conc. vs time, Rate vs conc. CO06.11: Define rate equations CO07: Define interfacial phenomena, and its role in preparation of dispersed systems, and describe the CO07.01: Identify a dispersed system CO07.02: Describe fundamental differences between solution and dispersion systems CO07.03: Define different dispersed systems, W/O or O/W dispersion systems CO07.04: Define the role of dispersed phase size and how it correlates to Gravity and Brownian forces CO07.05: Discuss the correlation between particle size and charge CO07.06: Define the importance of zeta potential on dispersion stability CO07.07: Describe the differences between Lyophilic, Lyophobic, and association colloids CO07.08: 08: Describe Protective colloids and Gold number CO07.09: Identify sedimentation in suspension and emulsion systems, and suspension flocculation CO07.10: Define emulsions and emulsion instability via coalescence, sedimentation, creaming, Ostwald ripening, and breaking CO07.11: Discuss the effect of temperature and composition on emulsion phase inversion CO07.12: Define surfactants, their structures and their differences CO07.13: Calculate surfactant HLBs CO07.14: Correlate surfactant HLB, O/W and W/O dispersed systems CO08: Learn basic concepts of viscosity and rheology of liquid to semi-solid pharmaceutical dosage forms
3 CO08.01: Describe Newtonian and non-newtonian fluids and dispersed systems CO08.02: Apply Newtonian and non-newtonian principles to suspension, emulsion, diluted dispersed systems and concentrated dispersed systems CO08.03: Discuss why certain fluids display a non-newtonian behavior CO08.04: Define factors that affect fluid flow, such as temperature, shear rate and time CO08.05: Discuss pseudoplastics, dilatants, thixotropy and rheopexy, plastic flow, and hysteresis loop CO08.06: 06: Differentiate laminar and turbulent conditions and their effects on viscosity measurements CO08.07: Describe viscoelasticity, and the effect of time on flow property CO09: Define basic physical pharmacy of polymers and macromolecules used in preparation of CO09.01: Describe polymer applications in pharmaceutical products CO09.02: Define mono-dispersed, and polydispersed polymer systems CO09.03: Discuss molecular weight and molecular weight distribution of a polymer, average molecular weights and how these affect polymer properties CO09.04: Describe glass transition temperature, Tg, and factors affecting Tg CO09.05: Define different polymer structures such as topology, isomerism, crosslinking, linear, branched, cis, and trans CO09.06: Discuss how polymer structure contributes to its role in pharmaceutical application CO09.07: Describe protein structures CO09.08: Define protein stability and formulation CO10: Learn basic concepts of protein binding and complexation, and its role in drug bioavailability CO10.01: 01 Define different classes of complexes and identify pharmaceutical examples CO10.02: Describe chelates, their physical properties, and what differentiates them from organic molecular complexes CO10.03: Describe the forces involved in polymer-drug complexes with pharmaceutical drug delivery applications CO10.04: Discuss the ways that protein binding can influence drug action CO11: Correlate property and application of materials with the focus on controlled drug delivery systems CO11.01: Describe physicochemical principles of materials in traditional and advanced pharmaceutical dosage forms CO11.02: Describe structure-property relationship of materials and how to utilize them in different pharmaceutical applications CO11.03: Describe how material properties are utilized to design different drug release systems including immediate, sustained, delayed, pulsatile, and targeted CO11.04: Discuss material properties in developing modern delivery technologies and systems based on microparticles, nanoparticles, modern polymers, liposomes for traditional and new actives such as proteins and peptides CO12: Describe the biopharmaceutics principles in developing pharmaceutical dosage forms CO12.01: Describe bioequivalence and bioavailability terminology CO12.02: Explain how blood levels versus time curves are used to assess bioavailability of a drug CO12.03: Outline the difference between a generic and reference drug product CO12.04: Recognize the letter code classification of the Orange Book CO12.05: Recognize the pharmaceutical reasons/considerations for a dosage from design CO12.06: Differentiate advantages and disadvantages of the routes of administration CO12.07: Identify the role of the different disciplines involved during initial drug development CO12.08: Describe the factors that influence bioavailability CO12.09: Classify and identify the differences between the four types of absorption mechanism CO12.10: Explain the factors that affect drug dissolution and absorption and stability CO12.11: Recognize the different physiological conditions found in the gastrointestinal tract CO13: Describe biopharmaceutical and analytical aspects of pharmaceutical dosage forms
4 CO13.01: Explain how pharmacists utilize biopharmaceutical analysis to the benefit of the patient CO13.02: Differentiate the terms sensitivity and selectivity requirements for analysis of drug substances CO13.03: Define the term trace analysis and give the common name for drug concentrations (10-9, 10-12, g) CO13.04: Explain why the pharmaceutical analyst must be aware of the metabolism scheme for drug(s) when analyzing a biological sample containing the drug(g) CO13.05: Cite reasons for the need for biopharmaceutical analysis CO13.06: Cite and discuss considerations involved in the selection of an appropriate organic solvent for solvent extraction CO13.07: Define chromatography, mobile phase, and stationary phase CO13.08: List and define the types of chromatograph CO13.09: Define "tr" and "Rf" CO13.10: Name the essential components of gas and liquid chromatography CO13.11: Compare detectors in terms of usefulness CO13.12: Define the validation parameters CO13.13: Distinguish between external, internal and standard addition methods CO14: Describe the FDA steps involved in the drug development and approval processes CO14.01: Discuss the different stages/phases during the drug approval process CO14.02: Identify the main law and standards created from the act and amendments CO14.03: Distinguish the difference between the CFR and the FR CO14.04: Describe Title 21 CFR main requirements CO14.05: Describe the main drug discovery resources CO14.06: Differentiate among the methods of drug discovery CO14.07: Distinguish the terminology of drug nomenclature CO14.08: Describe the main responsibility of pharmaceutics CO14.09: Identify the information included in an IND CO15: Describe pre-formulation studies on drug and drug dosage forms CO15.01: Define the preformulation process and specific timing CO15.02: Identify the objectives of preformulation CO15.03: Cite reasons for molecular optimization CO15.04: Explain the different tests use for bulk characterization CO15.05: Discuss the difference between crystallinity, polymorphism and amorphous materials CO15.06: Identify the techniques use for determining polymorphism CO15.07: Distinguish between hygroscopicity and deliquescent CO15.08: Recognize the parameters and methods used for particle characterization CO15.09: Explain the difference between densities and how to calculate them CO15.10: Recognize the rationale of powder flow CO15.11: Describe the evaluation of mechanical properties of powders CO15.12: Discuss the concept of solubility analysis and why they are used CO15.13: Describe the reasons for stability analysis and the typical setup CO15.14: Relate how physicochemical properties such as solubility and crystallinity modification influence bioavailability CO16: Define the basics of good manufacturing practice in preparation of pharmaceutical dosage form CO16.01: Identify the general provisions -- scope and definition of cgmp CO16.02: Recognize the seven expectations of all GMP CO16.03: Describe reasons for the increase in preparation of patient-specific medications (compounding) CO16.04: Recognize the purpose of the specific section of the Food Drug Modernization Act (Section 127) and how it exempts pharmacy compounding from several government regulatory requirements
5 CO16.05: Describe how the USP/NF helps prepare pharmacies for compounding, what institution promulgated the Good Compounding practices, and develops documents and recommendations for these type of practices (similar to cgmp)
Applied Surfactants: Principles and Applications
Applied Surfactants: Principles and Applications Tadros, Tharwat F. ISBN-13: 9783527306299 Table of Contents Preface. 1 Introduction. 1.1 General Classification of Surface Active Agents. 1.2 Anionic Surfactants.
More informationMiami Dade College CHM Second Semester General Chemistry
Miami Dade College CHM 1046 - Second Semester General Chemistry Course Description: CHM 1046 is the second semester of a two-semester general chemistry course for science, premedical science and engineering
More informationKING KHALID UNIVERSITY
KING KHALID UNIVERSITY COLLEGE OF PHARMACY DEPARTMENT OF PHARMACEUTICS COURSE SCHEDULE MALE SECTION PHYSICAL PHARMACY FOR PHARMACEUTICAL SCIENCES/CLINICAL PHARMACY BY PROF DR MOHAMED FATHY Academic Session
More informationThe University of Jordan
The University of Jordan Faculty: Pharmacy Department: Pharmaceutics and Pharmaceutical Technology Program: BSc. of Pharmacy Academic Year/ Semester: 2013/2014/ 1 st semester Course Name (Course Number):
More informationCHEMISTRY CONTENT SKILLS CHART
I. NATURE OF CHEMISTRY A. Safety B. Fundamental quantitative relationships 1. Metric system a. Prefixes b. Difference between base units and derived units 2. Significant figures 3. Scientific notation
More informationGeneral Chemistry (Second Quarter)
General Chemistry (Second Quarter) This course covers the topics shown below. Students navigate learning paths based on their level of readiness. Institutional users may customize the scope and sequence
More informationCurriculum Guide Chemistry
Chapter 1: Introduction to Chemistry Why is chemistry important in using dominion science? Is chemistry necessary in all aspects of life? How can a chemist advance science for the kingdom of God? 1 Lesson
More informationI. Intermolecular forces and changes in chemical state or phase
General Chemistry II, in broad strokes I. Intermolecular forces and changes in chemical state or phase II. Solutions, solubility, and colligative properties III. Chemical Kinetics -- the study of rates
More informationINTRODUCTORY CHEMISTRY FOR WATER QUALITY TECHNOLOGY I. Chemistry 11 and Principles of Mathematics 12 is strongly recommended.
CHEMISTRY 115 INTRODUCTORY CHEMISTRY FOR WATER QUALITY TECHNOLOGY I Prerequisites: Format: Chemistry 11 and Principles of Mathematics 12 is strongly recommended. 4 hours lecture + 3 hours lab per week
More informationBrunswick School Department Chemistry: Honors Solution Equilibrium
Understandings Questions Knowledge Solutions can be combined to generate a variety of chemical reactions, the rates of which can be measured in a number of ways, depending on the nature of the reaction.
More informationStudy guide for AP test on TOPIC 1 Matter & Measurement
Study guide for AP test on IC 1 Matter & Measurement IC 1 Recall a definition of chemistry Understand the process and stages of scientific (logical) problem solving Recall the three states of matter, their
More informationAP Chemistry Standards and Benchmarks
Standard: Understands and applies the principles of Scientific Inquiry Benchmark 1: Scientific Reasoning Course Level Benchmarks A. Formulates and revises scientific explanations and models B. Understands
More informationPraxis Chemistry Content Knowledge (5245) Study Plan Description of content
Page 1 I. Basic Principles of Matter and Energy; Thermodynamics (14%) A. Matter and Energy of s I will 1. Organization of matter a. pure substances (elements and compounds) b. mixtures (homogeneous, heterogeneous,
More informationStudyHub: AP Chemistry
StudyHub+ 1 StudyHub: AP Chemistry Solution Composition and Energies, Boiling Point, Freezing Point, and Vapor Pressure StudyHub+ 2 Solution Composition: Mole Fraction: Formula: Mole Fraction of Component
More informationCHEMISTRY PHYSICAL. of FOODS INTRODUCTION TO THE. CRC Press. Translated by Jonathan Rhoades. Taylor & Francis Croup
Christos Ritzoulis Translated by Jonathan Rhoades INTRODUCTION TO THE PHYSICAL CHEMISTRY of FOODS CRC Press Taylor & Francis Croup Boca Raton London NewYork CRC Press is an imprint of the Taylor & Francis
More informationIdentify the bonding types molecular, covalent network, ionic, and metallic - in various solids (11.8)
Intermolecular Forces, Liquids, and Solids (Chapter 11) Very brief review of Lewis structures and molecular geometry Draw Lewis structures for and determine polarity of molecules through sp 3 8.45 8.64,
More informationChemistry: The Central Science Twelfth Edition, AP* Edition 2012
A Correlation of The Central Science Twelfth Edition, AP* Edition 2012 to the AP* Chemistry Topics I. Structure of Matter A. Atomic theory and atomic structure 1. Evidence for the atomic theory SECTIONS:
More informationOverview. Lecture 5 Colloidal Dispersions
Physical Pharmacy Lecture 5 Colloidal Dispersions Assistant Lecturer in Pharmaceutics Overview Dispersed Systems Classification Colloidal Systems Properties of Colloids Optical Properties Kinetic Properties
More informationSeymour Public Schools Curriculum
Chemistry Curriculum The intent of this unit is to demonstrate the proper use of lab materials and equipment. Also, correctly answer safety questions, demonstrate safe working practices in the lab as described
More information*blood and bones contain colloids. *milk is a good example of a colloidal dispersion.
Chap. 3. Colloids 3.1. Introduction - Simple definition of a colloid: a macroscopically heterogeneous system where one component has dimensions in between molecules and macroscopic particles like sand
More informationOverview. Types of Solutions. Intermolecular forces in solution. Concentration terms. Colligative properties. Osmotic Pressure 2 / 46
1 / 46 2 / 46 Overview Types of Solutions. Intermolecular forces in solution Concentration terms Colligative properties Osmotic Pressure 3 / 46 Solutions and Colloids A solution is a homogeneous mixture
More informationNorton City Schools Standards-Based Science Course of Study 2003
HIGH SCHOOL ELECTIVE CHEMISTRY (USED AS A YEAR-LONG OR BLOCK-SCHEDULED COURSE) Physical Sciences Standard (PS) 11-12 Benchmarks By the end of the 11-12 program, the student will, Physical Sciences Explain
More informationExam 3 Concepts! CH110 FA10 SAS 33
Exam 3 Concepts! CH110 FA10 SAS 33 Properties of Gases What sorts of elements and compounds tend to be found as gasses at room temperature? What are the physical properties of gases? What is pressure?
More informationFARMINGDALE STATE COLLEGE DEPARTMENT OF CHEMISTRY
FARMINGDALE STATE COLLEGE DEPARTMENT OF CHEMISTRY COURSE OUTLINE: COURSE TITLE: Prepared by: Dr. Victor Huang September 2016 General Chemistry Principles II COURSE CODE: CHM 153 CREDITS: 4 CONTACT HOURS:
More informationCHEM 1310: Review. List of major topics
CHEM 1310: Review List of major topics Chapter 1: Atomic Nature of Matter Atomic theory of matter Atomic masses Moles Elemental analysis Volume & density Chapter 2: Stoichiometry Balancing equations Limiting
More informationBig Idea 1: Structure of Matter Learning Objective Check List
Big Idea 1: Structure of Matter Learning Objective Check List Structure of Matter Mole Concept: Empirical Formula, Percent Composition, Stoichiometry Learning objective 1.1 The student can justify the
More informationPharmaceutics and Pharmaceutical Technology
Pharmaceutics and Pharmaceutical Technology Pharmaceutics and Pharmaceutical Technology Laboratories Lab Name Location Person in Charge Programs Served Courses Served Pharmaceutics A M12-127 Pharmaceutics
More informationPhysical Properties of Solutions
Physical Properties of Solutions Physical Properties of Solutions Types of Solutions (13.1) A Molecular View of the Solution Process (13.2) Concentration Units (13.3) Effect of Temperature on Solubility
More informationChemistry: Molecules, Matter, and Change, Fourth Edition Loretta Jones and Peter Atkins Correlated with AP Chemistry, May 2002, May 2003
Chemistry: Molecules, Matter, and Change, Fourth Edition Loretta Jones and Peter Atkins Correlated with AP Chemistry, May 2002, May 2003 ST=Student textbook I. Structure of Matter A. Atomic theory and
More informationProperties of Solutions. Chapter 13
Properties of Solutions Chapter 13 Sodium acetate crystals rapidly form when a seed crystal is added to a supersaturated solution of sodium acetate. Saturated solution: contains the maximum amount of a
More informationRequired Syllabus Information all must be included in the course syllabus
Effective Implementation date: Spring 2018, 201830 Required Syllabus Information all must be included in the course syllabus CHE 112 Course Title: Gen College Chem II/Lab: SC1 Course Credits: 5 Course
More informationContents. Preface XIII. 1 General Introduction 1 References 6
VII Contents Preface XIII 1 General Introduction 1 References 6 2 Interparticle Interactions and Their Combination 7 2.1 Hard-Sphere Interaction 7 2.2 Soft or Electrostatic Interaction 7 2.3 Steric Interaction
More informationVOCABULARY. Set #2. Set #1
VOCABULARY Set #1 1. Absolute zero 2. Accepted value 3. Accuracy 4. Celsius scale 5. Conversion factor 6. Density 7. Dimensional analysis 8. Experimental value 9. Gram 10. International system of units
More informationSecondary Science: Curriculum Map for Chemistry
Secondary Science: Curriculum Map for Chemistry State Stards Checks for Understing Learning Outcomes Adopted Resources Core Ideas CLE 3221.3.2 Analyze chemical nuclear reactions. CLE 3221.3.3 Explore the
More informationChapter 11 Properties of Solutions
Chapter 11 Properties of Solutions Solutions Homogeneous mixtures of two or more substances Composition is uniform throughout the sample No chemical reaction between the components of the mixture Solvents
More informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
CP Chem Review 2 Matching Match each item with the correct statement below. a. activated complex d. activation energy b. reaction rate e. free energy c. inhibitor 1. the minimum energy colliding particles
More informationSpanish Fork High School Unit Topics and I Can Statements Honors Chemistry
Spanish Fork High School 2014-15 Unit Topics and I Can Statements Honors Chemistry Module 1 I Can: Module 2 I Can: Distinguish between elements, compounds, and mixtures Summarize the major experimental
More informationOxnard Union High School District Chemistry Pacing Plan SEMESTER 1
Oxnard Union High School District 2013-2014 Chemistry Pacing Plan SEMESTER 1 Unit and Number of Weeks Introduction to Chemistry 1 ½ weeks CA State Standard & Sub Concepts Investigation & Experimentation
More informationTEACHER CERTIFICATION STUDY GUIDE. Table of Contents ATOMIC STRUCTURE AND THE PROPERTIES OF MATTER
Table of Contents SUBAREA I. ATOMIC STRUCTURE AND THE PROPERTIES OF MATTER COMPETENCY 1.0 UNDERSTAND THE VARIOUS MODELS OF ATOMIC STRUCTURE, THE PRINCIPLES OF QUANTUM THEORY, AND THE PROPERTIES AND INTERACTIONS
More informationCourse Title. All students are expected to take the College Board Advanced Placement Exam for Chemistry in May.
Course Title ERHS Chemistry A (AP) Description/ Target group This is two-semester laboratory course of inorganic chemistry, designed for college bound students entering the fields of science and engineering,
More informationChemistry I-Honors Solution Chemistry Notes
Chemistry I-Honors Solution Chemistry Notes The Solution Process Must consider three sets of interactions and the energy (and entropy) associated with each. (1) Solute-solute interaction (2) Solvent-solvent
More informationHADDONFIELD PUBLIC SCHOOLS Curriculum Map for Accelerated Chemistry
Curriculum Map for Accelerated Chemistry 1st Marking Period 5.1.12.A.1, 5.1.12.A.2,, 5.1.12.A.3,, 5.1.12.B.1, 5.1.12.B.2, 5.1.12.B.3, 5.1.12.B.4, 5.1.12.C.1, 5.1.12.C.2, 5.1.12.C.3,, 5.1.12.D.1, 5.1.12.D.2,
More informationChapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 1-1 Chemistry: Science of Change 1-2 The Composition of Matter 1-3 The Atomic Theory of Matter 1-4 Chemical Formulas and Relative Atomic Masses 1-5 The Building Blocks
More informationI can calculate the rate of reaction from graphs of a changing property versus time, e.g. graphs of volume against time
UNIT 1 CONTROLLING THE RATE OF REACTION I can calculate the rate of reaction from graphs of a changing property versus time, e.g. graphs of volume against time I can use the reciprocal of to calculate
More informationEnfield Public Schools. Advanced (AP/UCONN) Chemistry (0297) Curriculum Writers: Patrick Smith William Schultz
Enfield Public Schools Advanced (AP/UCONN) Chemistry (0297) Curriculum Writers: Patrick Smith William Schultz November 2007 Lab Safety 1. Basic safety rules must be followed in the Advanced Chemistry laboratory.
More informationCI = critical item question or lecture test old Performance/Task: The student will: item General 1
Competencies for CHEM 1110: summary KEY: text delivery method (Chang) x.y where l = lecture x = chapter n = notes evaluation method y = section v = video tape or internet streaming video F = final exam
More informationPine Hill Public Schools Curriculum
Pine Hill Public Schools Curriculum Content Area: Course Title/ Grade Level: AP Chemistry / 11 or 12th grade Unit 1: Mathematics of Chemistry Duration: 1 week Unit 2: Atoms, molecules and Ions Duration:
More informationCOLLOIDAL DISPERSIONS
COLLOIDAL DISPERSIONS Marlyn D. Laksitorini Lab. of Physical Pharmacy and Biopharmaceutics Dept.Pharmaceutics Gadjah Mada School of Pharmacy References Overview 1. Type of Dispersion 2. Example of Colloidal
More informationClassroom: 318 Subject: AP Chemistry Quarter 2 Teacher: van Balveren, Suzanne
Livingston American School Quarterly Lesson Plan Concept / Topic To Teach: Week 1 Week 2 Week 3 Week 4 Equilibrium Equilibrium Acids and Bases Acids and Bases Standards Addressed: College Board canbe formed
More informationSTATE UNIVERSITY OF NEW YORK COLLEGE OF TECHNOLOGY CANTON, NEW YORK COURSE OUTLINE CHEM COLLEGE CHEMISTRY II
STATE UNIVERSITY OF NEW YORK COLLEGE OF TECHNOLOGY CANTON, NEW YORK COURSE OUTLINE CHEM 155 - COLLEGE CHEMISTRY II Prepared by: Nicole A. Heldt, Ph.D. SCHOOL OF SCIENCE, HEALTH, AND PROFESSIONAL STUDIES
More informationCourse Title: Academic chemistry Topic/Concept: Chapter 1 Time Allotment: 11 day Unit Sequence: 1 Major Concepts to be learned:
Course Title: Academic chemistry Topic/Concept: Chapter 1 Time Allotment: 11 day Unit Sequence: 1 1. Nature of chemistry 2. Nature of measurement 1. Identify laboratory equipment found in the lab drawer
More informationBasic Chemistry 2014 Timberlake
A Correlation of Basic Chemistry Timberlake Advanced Placement Chemistry Topics AP is a trademark registered and/or owned by the College Board, which was not involved in the production of, and does not
More informationChapter 13. Properties of Solutions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 13 Properties of John D. Bookstaver St. Charles Community College Cottleville, MO are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed
More informationElizabethtown Area School District Chemistry II Name of Course
Chemistry II Name of Course Course Number: 325 Length of Course: 18 weeks Grade Level: 10-12 Elective Total Clock Hours: 120 Length of Period: 80 min Date Written: June 11, 2007 Periods per Week/Cycle:5
More informationPhysical Properties of Solutions
Physical Properties of Solutions Chapter 12 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 12.1- Types of solutions A solution is a homogenous mixture of 2 or
More informationJEFFERSON COLLEGE COURSE SYLLABUS CHM112 GENERAL CHEMISTRY II. 5 Credit Hours. Prepared by: Richard A. Pierce. Revised Date: August 2009 by Sean Birke
JEFFERSON COLLEGE COURSE SYLLABUS CHM112 GENERAL CHEMISTRY II 5 Credit Hours Prepared by: Richard A. Pierce Revised Date: August 2009 by Sean Birke Arts & Science Education Dr. Mindy Selsor, Dean CHM112
More informationB L U E V A L L E Y D I S T R I C T C U R R I C U L U M Science AP Chemistry
B L U E V A L L E Y D I S T R I C T C U R R I C U L U M Science AP Chemistry ORGANIZING THEME/TOPIC UNIT 1: ATOMIC STRUCTURE Atomic Theory Electron configuration Periodic Trends Big Idea 1: The chemical
More informationProperties of Solutions. Course Learning Outcomes for Unit III. Reading Assignment. Unit Lesson UNIT III STUDY GUIDE
UNIT III STUDY GUIDE Properties of Solutions Course Learning Outcomes for Unit III Upon completion of this unit, students should be able to: 1. Describe how enthalpy and entropy changes affect solution
More informationPhysical pharmacy. The Gaseous State. dr basam al zayady. States of matter
Physical pharmacy Lec 5 dr basam al zayady States of matter The Gaseous State Gas molecules have vigorous and rapid motion that result in collisions not only with one another but also with the walls of
More informationChemistry 112 ACS Final
Chemistry 112 ACS Final Exam at 4 pm in ECTR 118 and you will be done by 6 pm Stop at question 56 Topics covered are below.honestly, the best way to study is to read through your notes multiple times making
More informationCowley College & Area Vocational Technical School
Cowley College & Area Vocational Technical School COURSE PROCEDURE FOR CHEMISTRY II CHM4230 5 Credit Hours Student Level: This course is open to students on the college level in either the freshman or
More informationContents. Preface XIII
V Contents Preface XIII 1 General Introduction 1 1.1 Fundamental Knowledge Required for Successful Dispersion of Powders into Liquids 1 1.1.1 Wetting of Powder into Liquid 1 1.1.2 Breaking of Aggregates
More informationAP Chemistry Syllabus
AP Chemistry Syllabus Course Description: AP Chemistry is equivalent to an introductory college level chemistry class. Students taking this course should have already successfully completed a year of laboratory
More informationMOBILE COUNTY PUBLIC SCHOOLS DIVISION OF CURRICULUM & INSTRUCTION HIGH SCHOOL BLOCK SCHEDULE PACING GUIDE AT A GLANCE
Quarters Objective # Objective 1 & 3 1.A.1 1.0 Understanding as Inquiry A. Foundations 1. Scientific Inquiry a. Identify and clarify research questions and design experiments. b. Design experiments so
More informationUnit title: Chemistry for Applied Biologists
Unit title: Chemistry for Applied Biologists Unit code: K/601/0292 QCF level: 5 Credit value: 15 Aim This unit covers bonding, thermodynamics, reaction rates, equilibrium, oxidation and reduction and organic
More informationChemistry Topics for UIL Dr. Brian Anderson
Dr. Brian Anderson Because this is my first year as Chemistry Director, I will continue the practices set in place by Dr. McCord, with only the two minor changes noted below, to help ensure a smooth transition
More informationChemistry. Atomic and Molecular Structure
Chemistry Atomic and Molecular Structure 1. The periodic table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates
More informationPhysical Pharmacy ( ) Unit 3 / Solutions
Physical Pharmacy (0510219) Unit 3 / Solutions Based on thermodynamics Ideal solution Real solution Classification of Aqueous solution systems Based on particle size True solution Colloidal dispersion
More informationScience. Smyth County Schools Curriculum Map Grade:11/12 Subject:Chemistry
Standards Grade:11/12 Subject:Chemistry 1st Quarter SOL Ch 1a, 1b, 1c, 1e, 1g, 1i, 1h, 1f, 1d, 2a, 2b, 2c, 2d, 2e, 2f, 2g, 2h, 2i, 5c, 5e 2nd Quarter SOL Ch 4a, 4b, 3a, 3b, 3c, 3d, 3e, 5f Content Lab safety,
More informationLiquid in liquid: ethanol in water. Solid in liquid: any salt in water. Solid in solid: brass, bronze, and all alloys
1 of 6 I. The solution process Solutions, colloids, and suspensions Solution: homogeneous mixture, equally dispersed at the molecular level, uniform throughout in its physical and chemical properties Colloid:
More informationProperties of Solutions
Properties of Solutions The States of Matter The state a substance is in at a particular temperature and pressure depends on two antagonistic entities: The kinetic energy of the particles The strength
More informationPreformulation & Solid State Chemistry Services
Preformulation & Solid State Chemistry Services VxP Pharma Purdue Research Park 5225 Exploration Drive Indianapolis, IN 46241 Tel: 317.759.2299 Fax: 317.713.2950 VxP Pharmaprovides manufacturing, testing
More informationName Date Class STATES OF MATTER
13 STATES OF MATTER Each clue describes a vocabulary term. Read the clues and write the letters of each term on the lines. 1. Clue: the energy an object has because of its motion. 2. Clue: results from
More informationStates of matter Part 2
Physical Pharmacy Lecture 2 States of matter Part 2 Assistant Lecturer in Pharmaceutics Overview The Liquid State General properties Liquefaction of gases Vapor pressure of liquids Boiling point The Solid
More informationSolutions. Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility
Solutions Solutions Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility Colligative Properties - Ways of Expressing Concentration
More informationChapter 11 Properties of Solutions
Chapter 11 Properties of Solutions 11.1 Solution Composition. Molarity moles solute 1. Molarity ( M ) = liters of solution B. Mass Percent mass of solute 1. Mass percent = 1 mass of solution C. Mole Fraction
More informationLecture 6. NONELECTROLYTE SOLUTONS
Lecture 6. NONELECTROLYTE SOLUTONS NONELECTROLYTE SOLUTIONS SOLUTIONS single phase homogeneous mixture of two or more components NONELECTROLYTES do not contain ionic species. CONCENTRATION UNITS percent
More informationχ A = P A Gen. Chem. II Exam I review sheet (Ch. 10, 11, 13, 14) Ch. 10 Gases behave physically similarly.
Gen. Chem. II Exam I review sheet (Ch. 10, 11, 13, 14) Ch. 10 Gases behave physically similarly. KMT (Kinetic Molecular Theory): particles in a gas: are in constant rapid motion are tiny compared to the
More informationPhysical Pharmacy. Solutions. Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department
Physical Pharmacy Solutions Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department 10/31/2015 Online access: bit.ly/physicalpharmacy 1 Mixtures a combination of two or
More informationChapter 11 Review Packet
Chapter 11 Review Packet Name Multiple Choice Portion: 1. Which of the following terms is not a quantitative description of a solution? a. molarity b. molality c. mole fraction d. supersaturation 2. Which
More information- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)
68 HOW THINGS DISSOLVE - Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)... what happens? - Water molecules pull the sugar molecules out of
More informationChemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Solutions
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Dr. Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville,
More informationPhET Interactive Chemistry Simulations Aligned to an Example General Chemistry Curriculum
PhET Interactive Chemistry Simulations Aligned to an Example General Chemistry Curriculum Alignment is based on the topics and subtopics addressed by each sim. Sims that directly address the topic area
More informationPrinciples of General Chemistry
Principles of General Chemistry 978-1-63545-004-0 To learn more about all our offerings Visit Knewton.com/highered Source Author(s) (Text or Video) Title(s) Link (where applicable) OpenStax Senior Contributing
More informationFACULTY OF PHARMACY. M. Pharmacy I Semester (Suppl.) Examination, November 2015 (Common To All) Subject: Pharmaceutical Analytical Techniques
M. Pharmacy I Semester (Suppl.) Examination, November 2015 (Common To All) Subject: Pharmaceutical Analytical Techniques Code No. 6001 / S Note: Answer any Five questions. All questions carry equal marks.
More informationI. Instructor: Dave Bugay
Chemistry 1412: General Chemistry II CHEM 1412: General Chemistry II (4-3-1) Topics included in this course are liquids and solids, solutions, ionization theory, chemical equilibrium, thermodynamics, kinetics,
More information3 rd Food Emulsions Short Course November 13 th & 14 th, 2008 University of Massachusetts. David Julian McClements University of Massachusetts
3 rd Food Emulsions Short Course November 13 th & 14 th, 2008 University of Massachusetts David Julian McClements University of Massachusetts Program Objectives Review Basic Principles of Emulsion Science
More informationAdvanced Placement Chemistry Syllabus
Advanced Placement Chemistry Syllabus Course Description: The College Board describes AP chemistry as a course designed to be the equivalent of the general chemistry course usually taken during the first
More informationColloidal Dispersions
Physical Pharmacy Lecture 5 Colloidal Dispersions Assistant Lecturer in Pharmaceutics Overview Dispersed Systems Classification Colloidal Systems Properties of Colloids Optical Properties Kinetic Properties
More information1. Which substance will conduct the current in the solid state? 1. Diamond 2.Graphite 3.Iodine 4.Sodium chloride.
CHAPTER :SOLIDS 1. Which substance will conduct the current in the solid state? 1. Diamond 2.Graphite 3.Iodine 4.Sodium chloride. 2. Molten sodium chloride conducts electricity due to the presence of ions:
More informationMARLBORO CENTRAL SCHOOL DISTRICT-CURRICULUM MAP. Subject: AP Chemistry 2015/16
MARLBORO CENTRAL SCHOOL DISTRICT-CURRICULUM MAP Subject: AP Chemistry 205/6 Title or Topics (Unit organizing idea) Concepts (understandings) Tasks (What students actually do) Major Assessments (Tests,
More informationMixtures and Solutions
Mixtures and Solutions Section 14.1 Heterogeneous and Homogeneous Mixtures In your textbook, read about suspensions and colloids. For each statement below, write true or false. 1. A solution is a mixture
More informationReview of differential and integral calculus and introduction to multivariate differential calculus.
Chemistry 2301 Introduction: Review of terminology used in thermodynamics Review of differential and integral calculus and introduction to multivariate differential calculus. The properties of real gases:
More informationFind molality: mass percent. molality Assume a basis of 100g solution, then find moles ammonium chloride: Find mass water: So molality is:
66 An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is 1.024 g/ml Find: molality, mole fraction, molarity. Find molality: mass percent molality Assume a basis of 100g
More informationChemistry 12 - Learning Outcomes
Chemistry 12 - Learning Outcomes A: Chapt 1. Reaction Kinetics - (Introduction) A1. give examples of reactions proceeding at different rates A2. describe rate in terms of some quantity (produced or consumed)
More informationLO 1.2 SP 2.2] LO 1.3 SP
This is a condensed version of the new curriculum framework for the AP Chemistry course. EU = Enduring Understanding EK = Essential Knowledge LO = Learning Objective SP = Science Practice (separate file
More informationSOLUTIONS. Dissolution of sugar in water. General Chemistry I. General Chemistry I CHAPTER
11 CHAPTER SOLUTIONS 11.1 Composition of Solutions 11.2 Nature of Dissolved Species 11.3 Reaction Stoichiometry in Solutions: Acid-Base Titrations 11.4 Reaction Stoichiometry in Solutions: Oxidation-Reduction
More informationPharmaceutical compounding I Colloidal and Surface-Chemical Aspects of Dosage Forms Dr. rer. nat. Rebaz H. Ali
University of Sulaimani School of Pharmacy Dept. of Pharmaceutics Pharmaceutical Compounding Pharmaceutical compounding I Colloidal and Surface-Chemical Aspects of Dosage Forms Dr. rer. nat. Rebaz H. Ali
More informationSamples of Evidence to Satisfy the AP Chemistry Curricular Requirements
Samples of Evidence to Satisfy the AP Chemistry Curricular What s here? This table presents samples of evidence that address the curricular requirements for AP Chemistry. For each curricular requirement,
More informationApply knowledge of excipients, preformulation studies, stability formulation of pharmaceutical products and drug delivery systems.
Course Title Course Code DOSAGE FORM DESIGN PH702 Lecture : 3 Course Credit Practical : 3 Tutorial : 0 Total : 6 Course Objectives On the completion of the course, students will be able to: Apply knowledge
More information