introduction to chemistry 061
TRANSCRIPT
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Introduction to
306860 Chemistry 061Semester 2, 2012
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Lecturer
Khor Ee Huey BSc in Chemistry and Biology (Campbell)
MSc in Analytical Chemistry (Warwick)
PhD in Chemical Engineering (Curtin)
Research Interest Water and Wastewater Treatment
Analytical Sciences
Membrane Technology
CFD Simulation
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Teaching Team
Jason Chia Angnes Tiong
Evelyn Chiong
Wong Wei Ning
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ApplyDiscipline
Knowledge
ThinkingSkills
InformationSkills
CommunicationSkills
TechnologySkills
LearningHow toLearn
InternationalPerspective
CulturalUnderstanding
ProfessionalSkills
Curtins
GraduateAttributes
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Unit Learning Outcomes:
1 Apply the concepts and principles of chemical foundations andstates of matter to basic problem solving.
2
Evaluate chemistry related problems and phenomena creativelyand critically.
3 Carry out laboratory practical using correct techniques with
accuracy, precision and safety.
4
Produce laboratory notebook on practical work using effectivecommunication skills and critical thinking skills at a levelappropriate for tertiary education.
Apply discipline knowledge, Learning how to learn
Thinking skills
Professional skills, Cultural understanding
Information skills, Communication skills
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Unit Syllabus
Basic concepts Atoms, Molecules & Ions
Mole, Equation & Stoichiometry
Electronic configuration &Periodic Table
ChemistryFoundation
Chemical bonding
Shape and Polarity of Molecules
Intermolecular forces and statesof matter.
Structure of solids
Understandingon Matter
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Learning activities(per week)Face-to-face:
1 hours lecture
1 hours tutorial
2 hours laboratory (fortnightly)
Group/Self-study (suggestion):
2 hours on lab preparation and LecQuiz
1 hour reading text book
2 hours attempt on tutorial questions
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Assessment Summary
Assessment item Worth Due
Laboratory Notebook 20% Two weeks after
each lab session
Tutorials 10% EachWeek
Quizzes 30% Refer to Unit
Outline
Final examination 40% Week 16
Total 100%
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Assessment item Worth Due
Laboratory 20% Two weeks after
each lab sessionLaboratory Notebook 15%
Marking scheme can be found from the Moodle
Laboratory Worksheet 5%
Preparation done before the every lab sessions
Submission system: Laboratory notebook should be ring-bound and submit toAdministrative Assistant (Lydia) for endorsement before the
submission deadline.
Laboratory worksheet/ workplan should be submitted torespective tutor during laboratory session before theexperiment starts.
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Experiment Title: Students Name and ID: Mark:
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Experiment Title:
Name of Instructor:
Students Name and ID: Mark:
Excellent
(6)
Proficient
(4)
Beginning
(2)Presentation &
Appearance
Notebook is well organised or bound neatly with all
pages numbered and follows the format given.
Writing is neat and legible. Pen is used exclusively;
mistakes crossed out with single line; note is made
to explain mistake.
Notebook is bound or fairly organised but
with some headings missing and most
pages numbered with minor mistakes in
formatting.
Most writing is neat and legible. Pen isoften used; no notes are made to explain
mistake.
Notebook is unbound and messy. The
work is poorly organised with major
format error and no pages number is
included.
Writing is difficult to read. Pen is notused consistently; excessive crossing out
of mistakes showing careless work.
Introduction Clear statements of objective and valid hypothesesare provided based on literature review.
Introduction is well written with significant and
relevant information like definition of keywords,
reaction equations, physical data included.
Moderately appropriate objectives and
hypotheses are provided with little
evidence from literature research.
Some introductory and background
information provided is provided with
errors
Unclear objectives and off-the-mark or
irrelevant hypothesis.
Fail to include background information
from literature review.
Methodology &
Safety
Clear diagram and flow chart is included to describe
procedure. Equipment set up sketch on procedures
is properly labelled. MSDS data was used to suggest relevant safety
precautions. Safety precautions are rational and well
thought.
Flow chart is provided but with minor
errors. Modification in procedure is not
included. Safety precautions are given but too
generic. Information from MSDS data was
not used to suggest relevant safety
precautions
Diagrams and flow chart not included at
all. Experimental procedure is difficult to
follow. Modification in procedure is notrecorded.
Safety precautions are not always stated
Lack of attention in providing critical
safety information from MSDS.
Results &
Calculation
Accurate and complete and measurement data are
recorded in appropriate table with correct significant
figures and units.
Observations are recorded correctly if there is any.
Calculation is correct with step-by-step working
shown clearly.
Data are mostly complete. Data tables
are presented with minor errors spotted
such as incorrect significant figures and
missing units.
Little attention is given to observation.
Calculation is mostly correct, but workings
steps are not clear and method used may
not be fully described.
Data recorded is incomplete. Data tables
are messy and spotted with major
mistakes (significant figures and units).
Observations are completely missing or
inaccurate.
Calculation and working are incomplete
and with major mistakes.
Discussion &
Conclusion
All inferences are supported by appropriate
experimental results.
Conclusion is clear and compared with hypothesis
being tested.
Possible source of errors identified.
Recommendation for improvement included are
relevant, logic and viable.
Inferences are documented but not all
supported by experimental data.
Conclusions is not clear and not
compared with hypothesis being tested
Sources of errors are identified but too
generic. Recommendation and
suggestions may not be viable.
Findings are not summarised. Inferences
are not supported by experimental data.
There is no conclusion included.
Little or no attempt to identify sources o
errors. Recommendations and
suggestions are completely missing.
6 points
6 points
6 points
4 points
4 points
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Comments:
Points
Collected
Mark Points
Collected
Mark Points
Collected
Mark Points
Collected
Mark
30 20 23-22 15 15 10 8-7 5
29-28 19 21 14 14-13 9 6 4
27 18 20-19 13 12 8 5-4 3
26-25 17 18 12 11-10 7 3 2
24 16 17-16 11 9 6 2-1 1
26 points
17 marks
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Cooperative Team Learning
4-5 students in one team 5 team roles for laboratory work
Team manager
Researcher Technician
Data analyst
Safety officer
If only 4 members in the team,
the team manager will also play
the role of the researcher
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Format Description Worth
MCQ +
Subjective
4-5 Questions 5
Review Quizzes (20%)Date Week 5, 7,9, and 11
Time Tutorial sessions
Venue Tutorial venues
Scope TBA
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Lecture Quiz (10%)Date Starting in Week 1 for 10 consecutive lectures
Dateline Before Friday of the following week
Venue Moodle access
Scope Lecture for that week
Criteria Have to attend lectures
Format Description Worth
Part A Short Answer Question
Part B Self- reflection Questions
Total 1
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Format Description Worth
Part A 15 Multiple Choices Questions 30
Part B 5 Short Answer Questions 35
Part C 3 Long Answer Question 35
Total Scoring Mark 100
Final Examination (40%)Week 16
Duration 2 hour 10 mins (10 mins reading time)
Scope All topics
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http://moodle.curtin.edu.my/ Announcement Lecturers timetable (consultation hours)
Lab schedule
Lecture slides Tutorial Lab Manual
Mark Sheet
Useful links
http://moodle.curtin.edu.my/http://moodle.curtin.edu.my/ -
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Important note:
Attendance & Punctuality Switch off or silent mode mobile phone
Late submission of assignment (-10% per day)
Deferral F-IN, F
Plagiarism
No Spoon Feeding
No free rider
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What to Expect??
Independent learningCritical thinking
Analytical thinking
Problem solving skills
Team work
Communication
G d R l
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Ground Rules:Laboratory Session:
Students must read and prepare before each experiment.
Students must follow the rules and regulation in the
laboratory strictly.
It is students own effort and responsibility to complete the
lab 10-min before time.
Tutorial:
Students must attempt all the tutorial questions before
class.
Be punctual for every class.
Do not wait for solutions from lecturers before even trying
the questions.
G d R l
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Lecture:
Respect other's cultural and religious traditions,beliefs, values and languages.
Do not interrupt when someone is speaking.
Do not make noise during lecture except for
discussion.Other:
Respect lecturers personal teaching timetable.
Make appointment before consultation via formal
written email (student account only!) Students are responsible for their own behaviour.
Ground Rules:
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Topic 1:Chemistry Foundation
Semester 2, 2012
i bj i
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Describe common steps in scientific methods
Use significant figures and rounding to reflect the
certainty of quantitative data
Use percent of error and relative precision to
compare accuracy and precision of experimental
data
Learning Objectives:
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A systematic approach to research andexperiment
What is scientific method?
S i tifi M th d
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Scientific Method
HYPOTHESIS
Tentativeexplanation.
EXPERIMENT
Controlledobservations
that testhypothesis
SCIENTIFIC LAW
Summary ofaccepted
relationship which
supported by manyexperiments.
THEORY/MODEL
Tested hypothesis/
explanationsupported by manyexperiments.
Prediction
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Theory
an explanation of a set of related
observations or events based upon
proven hypotheses and verifiedmultiple times by detached groups of
researchers.
Examples:
Atomic theory/model Theory of evolution
Theory of relativity
The quantum theory
Law
A statement of fact to describe an
observation or relationship that is
always true when tested.
Example:
law of gravity
Newton's laws of motion
The laws of thermodynamics
Boyle's law of gases
the law of conservation of mass and
energy
Hooks law of elasticity
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Quantitative Observation
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Measurement: number + unit
Unit of measurement: SI Unit mass (kg), length (m), time (s), temperature (K), amount of
substance (mol)
volume (dm3), density (gcm-3)
Number: Scientific notation diameter of the Sun = 1.392 x 106 km
density of the Sun = 2.8 x 10-8 gcm-3
Quantitative Observation
i f
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All measurements should be reported in correct
significant figures: all of the certain digits and oneestimated digits.
Estimated digit indicates the uncertainty of ameasurement which depends on tolerance of
measuring instruments
Reporting values from measurements
C t
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Compare measurements:
Balance A gives reading 3.52 g
Three SF, last digit 2 is estimated digit.
The uncertainty of balance is 0.01 g
The actual value should be in the range of 3.51 to 3.53
Balance B give reading 3.5245 g
Balance B is more accurate than balance A.
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Non-zero numbers are always significant.
72.3 g three significant figures)
Zeros between non-zero numbers are always significant.
60.5 g three significant figures)
All final zeros to the right of decimal place are significant.
6.20 g three significant figures)
Zeros that act as placeholders are not significant.
0.0253 g 3 significant figures)
Counting numbers and defined constants have infinite numberof significant figures. 6 molecules, 60 s min-1)
R
U
L
E
S
SignificantFigures
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Significant figures in arithmetic
Addition andsubtraction
Answer should have same number of digits to theright of the decimal as the measurement with theleast number of decimal digits.
Example 1
2.475 m + 3.5 m + 4.65 m = 10.625 m
Answer should round up to 10.6 m
Example 2
5.36 x 10-4 g6.381 x 10-5 g = 4.7219 x 10-4 g
Answer should round up to 4.72 x 10
-4
g
Si ifi fi i i h i
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Significant figures in arithmetic
Multiplicationand Division
Answer should contain same number of significant figures as themeasurement with the fewest number of significant figures inthe calculation
Example 1
(6.46 x 10-4 g) (3.0 x 1012 cm3) = 2.153333 x 10-16 g/cm3
Answer should round up to 2.2 x 10-16 g/cm3
Example 2
(4.765 x 1011)x(5.3 x 10-4) (7.0 x 10-5) = 3.607785714 x 1012
Answer should round up to 3.6 x 1012
Example 1: Digital Balance
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Example 1: Digital Balance
Report Value: 100.4315 gUncertainty : 0.0001 g
Example 2: Bulb Pipette
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Example 2: Bulb Pipette
Report Value: 25.00 mLUncertainty : 0.03 mL
Example 4: Graduated Cylinder
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Report Value: 8.75 mL
Uncertainty : 0.05 mL
Example 4: Graduated Cylinder
E l 5 B tt
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Example 5: Burette
Initial Reading: 21.30 mL
Uncertainty : 0.05 mL
Final Reading: 49.75 mL
Uncertainty : 0.05 mL
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Burette Reading:
49.75 mL 21.30 mL = 28.45 mL
Value Uncertainty
Final Burette Reading/ mL 49.75 0.05mL
Initial Burette Reading/ mL 21.30 0.05mL
Burette reading/ mL 28.45 0.10mL
A f M t
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Accuracy of Measurement
Accuracy: how close a measured value is to anaccepted value.
Percent of error
=experimental value- accepted valuex100accepted value
P i i f M t
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Precision of Measurement
Precision refers to how close a series of measurements are to one another.
average deviation/ relative precision
standard deviation
A & P i i
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Accuracy & Precision
Systematic vs Random error
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Systematic vs Random error
Low accuracy : large systematic error
Low precision : large random error
Systematic error
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Systematic error
happen in one direction (always higher or lower
than actual value)
Procedural: do not follow procedure correctly, flaw in
procedure. Parallax error.
Instrumental error: balance used is not calibrated
properly. (do not show zero) etc.
Example of Systematic Error:
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Example of Systematic Error:
Example of Systematic Error:
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Example of Systematic Error:
Parallax Error
Random error
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Happen in all direction (first trial higher than actual value
second trial lower)
Do not follow procedure consistently.
Different experimenter.
Record data wrongly.Instrument: pipette has a random delivery error of 0.02 mL.
External conditions:
- temperature and
- humidity of environment
Summary:
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Su a y: Typical steps of scientific method include observation, hypothesis
and experiments.
A theory is a hypothesis that has been supported by manyexperiments to explain an observation.
A law summarizes observations and describes relationships innature.
In quantitative measurement,
Report data in correct significant figures.
Percent of error to reflect accuracy.
Relative deviation to reflect precision.