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The First Year Science eCommunity is a website that provides information and resources to ease your transition and maximise your success as a scientist at Sydney.

The site can be accessed via sydney.edu.au/current_students, by logging into the Learning Management System (icon link can be found on the right) then clicking the ‘eCommunities’ tab in the bar menu.

Faculty of Science

FIRST YEAR CHEMISTRYCHEM1101

Welcome to First Year Chemistry

• Questions or problems with the course?Director of First Year Studies Adam Bridgeman (Room 543a)

adam.bridgeman@sydney.edu.au

• Questions or problems with the labs?Director of First Year Laboratories Ron Clarke (Room 318)

ronald.clarke@sydney.edu.auRon

Adam

FIRST YEAR CHEMISTRYCHEM1101

Need extra help with course work?

• First Year Chemistry Learning Centre

• At the back of Lab D – textbooks, computers etc and….

• Tutors available Mon-Thu, 1-2pm from week 2 for free consultations

• CHEM1101 Discussion Board on eLearning

• Submit your questions and a tutor will reply

Not sure about something – ask Sophie!• First Year Enquiry Office (10 am - 3.15 pm)

firstyear@chem.usyd.edu.au

Sophie

FIRST YEAR CHEMISTRYCHEM1101

Information and Resources

• First Year Chemistry web site: firstyear.chem.usyd.edu.au

• CHEM1101 website: firstyear.chem.usyd.edu.au/chem1101 Access answers to tutorial problems, lecture notes, exam papers etc

• eLearning : elearning.sydney.edu.au/ Access pre-lab quizzes and resources from off-site CHEM1101 Discussion Board

• ChemCAL: chemcal.chem.usyd.edu.au Self-help tutorials and quizzes

FIRST YEAR CHEMISTRYCHEM1101

Syllabus and Learning Outcomes• firstyear.chem.usyd.edu.au/chem1101/syllabus.shtml• firstyear.chem.usyd.edu.au/chem1101/learningoutcomes.shtmlLecture Notes• firstyear.chem.usyd.edu.au/chem1101/lecture_notes.shtml

Username – “chem1101” Password – “carbon12”Textbook• Recommended (single book covers both semesters):

Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry and SI Chemical Data (package), 2012 (John Willey) ISBN: 9781118234228

FIRST YEAR CHEMISTRYCHEM1101

Tutorials

• Start in week 1

• Check answers to homework questions on the web before tutorial

Laboratory Work

• Starts in week 2 – check your timetable

• If you’ve previously passed this lab course, see Enquiry Office about exemption

Assessment

• 15% laboratory assessment (see first lab session for details)

• 15% tutorial quizzes (3 per semester: weeks 5, 9 and 12)

• 10% research assignment on global warming (from week 8 - 11)

• 60% 3 hour exam at the end of semester

FIRST YEAR CHEMISTRYCHEM1101

Laboratory Handbook

• Free – collect during your first lab session in week 2

Safety glasses must be worn

• Obtainable when you get your laboratory book in week 2 or from the UnionLaboratory Coat - Complying to Australian Safety Standards• Obtainable from the Co-Op bookshop, Wentworth Newsagency or Faculty eStore

(http://www.science.usydestore.com.au/) for less than $30 Must be white and long sleeved

Footwear and Long Hair• Covered footwear must be worn during all lab classes – no sandals or thongs • Long hair must be tied back

FIRST YEAR CHEMISTRYCHEM1101

Lecturers• We are very approachable - if you have questions, talk to us!• There are 3 series of this unit – all use the same notes• Weeks 1-7:

Dr Liz New (1), A/Prof Tim Schmidt (2) and Dr Siggi Schmid (3) elizabeth.new@sydney.edu.autimothy.schmidt@sydney.edu.ausiegbert.schmid@sydney.edu.au

• Weeks 8-13: Prof Peter Harrowell (1 and 2) and A/Prof Ron Clarke

peter.harrowell@sydney.edu.auronald.clarke@sydney.edu.au

FIRST YEAR CHEMISTRYCHEM1101

check your university email

regularlyor read it with gmail

FIRST YEAR CHEMISTRYCHEM1101

Overview of this CourseThe lectures begin with the smallest scale and work up from there

(Lectures 1-4)Sub-atomic/nuclear structure(Lectures 5-19)Atomic, electronic and molecular structure (quantum theory)Lectures 20-38 focus on macroscopic chemical processes and forces between molecules.

We will make frequent reference to the experimental basis for our understanding throughout. That is, we will relate the molecular-scale theories to macroscopically observable properties.

Some important specific examples will be discussed in detail and examined alongside general principles.

Throughout, I will link the examples to the issues mentioned on the previous slide.

FIRST YEAR CHEMISTRYCHEM1101

Assumed KnowledgeWe assume HSC Chemistry Core.

Some aspects of HSC Options will be covered in this Unit.

For revision, see Web Resources on the First Year Chemistry Web site, and read over the introductory topics in any General Chemistry text

Topics - Atomic and molecular structure, states of matter, elements & compounds, moles, stoichiometry (balancing reactions), classes of chemical reactions, periodic table.

FIRST YEAR CHEMISTRYCHEM1101

1803 J Dalton provided evidence for fundamental indivisible particles - atoms.

1897 JJ Thomson discovered electrons - “cathode rays.”1909 RA Millikan measured the charge of an electron.1909 E Rutherford proposed an atom be composed of a

small positive nucleus (1912) surroundedby a lot of space occupied by electrons.

1913 HGJ Moseley determined the charge on the nucleus.

Rutherford & others regard the atomic weight as being the number of protons and the nuclear charge as being the number of protons minus the number of electrons in the

nucleus.

1913 N Bohr applied quantum theory to electrons in atoms.1920 J Aston finds isotopes by mass spectrometry1932 J Chadwick discovered the neutron.This gives a fairly complete picture of the nucleus as composed of charged protons and uncharged neutrons.

FIRST YEAR CHEMISTRYCHEM1101

In a mass spectrometer, the atoms or molecules to be studied are vaporized and then ionized, usually by an electrical discharge.

In the conventional design of a mass spectrometer, ions follow a curved path and their deflection depends on the mass-to-charge ratio, m/z (sometimes denoted m/e). This deflection was originally recorded as impact on a strip of photographic film, but now use digital current or luminescence detectors.

Figure 19.1 Blackman

How Mass Spectrometry Works

FIRST YEAR CHEMISTRYCHEM1101

Mass SpectrometryAston’s results established the existence of isotopes. (They were already known for radioactive elements, but never shown for stable elements.)

1920 - Aston measured two isotopes of Ne (20 and 22), three of S (32, 33, 34), three of Si (28, 29, 30), six of Kr (78, 80, 82, 83, 84, 86), and many others

http://www-outreach.phy.cam.ac.uk/camphy/massspectrograph/

FIRST YEAR CHEMISTRYCHEM1101

Nucleons - The Sub-Atomic Particles

Particle Symbol Charge Mass (a.m.u.)

proton p +1 1.007276

neutron n 0 1.008665

electron e- -1 0.000549

positron e+ +1 0.000549

The unit of mass is atomic mass units (a.m.u.), defined by setting the mass of the isotope to exactly 12.000000…. 1 a.m.u. ~ 1.66 x 10-27 kg.

126C

Not present in stable atoms.

FIRST YEAR CHEMISTRYCHEM1101

Nuclides and IsotopesThe composition of any nucleus is defined by two numbers.• The atomic number is the number of protons in the nucleus.

• This defines the chemical nature of the atom.• It is equal to the total charge on the nucleus.

• The mass number is the total number of nucleons (protons and neutrons) in the nucleus.

E.g. has an atomic number of 6 and a mass number of 12.

• A nuclide is an atom with a particular mass number and atomic number.

• Nuclei with the same atomic number but different mass numbers are called isotopes.

126C

FIRST YEAR CHEMISTRYCHEM1101

Nuclei with the same atomic number but different mass numbers are called isotopes.

E.g. Carbon may exist as a number of isotopes

116C

126C

136C

146C

Stable nucleus;

accounts for 98.89% of

natural carbon.

Stable nucleus;

accounts for 1.11% of natural carbon.

Unstable nucleus.

Unstable nucleus;

prepared by nuclear

reaction in a cyclotron.

156C

Unstable nucleus;

trace amounts

present in living matter.

FIRST YEAR CHEMISTRYCHEM1101

The atomic mass of an element is the average of the atomic masses and abundances of each of the naturally-occurring isotopes.

E.g. The atomic mass of carbon is 12.01...

That is (12.0000x98.89 + 13.00335x1.11)/100

Mass of nuclide taken from a

reference table

Mass of nuclide is the reference for a.m.u scale.