My Degree

1. Faculty of Science My Degree Code for Success 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. Research and Information Skills FAQs

2. 0 • 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.au Adam Ron

3. 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 0 • Not sure about something – ask Sophie! • First Year Enquiry Office (10 am - 3.15 pm) • firstyear@chem.usyd.edu.au Sophie

4. 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

5. Syllabus and Learning Outcomes • firstyear.chem.usyd.edu.au/chem1101/syllabus.shtml • firstyear.chem.usyd.edu.au/chem1101/learningoutcomes.shtml • Lecture 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

6. 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 0

7. 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 Union Laboratory 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 0

8. 0 • 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 SiggiSchmid (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.au • ronald.clarke@sydney.edu.au

9. check your university email regularly 0 or read it with gmail

10. Overview of this Course The 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.

11. Assumed Knowledge We 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.

12. 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) surrounded by 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 spectrometry 1932 J Chadwick discovered the neutron. This gives a fairly complete picture of the nucleus as composed of charged protons and uncharged neutrons.

13. How Mass Spectrometry Works Figure 19.1 Blackman 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.

14. Mass Spectrometry Aston’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/

15. Nucleons - The Sub-Atomic Particles Not present in stable atoms. 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.

16. Nuclides and Isotopes • The composition of any nucleus is defined by two numbers. • Theatomic numberis 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. • Themass numberis the total number of nucleons (protons and neutrons) in the nucleus. • E.g. has an atomic number of6and a mass number of12. • A nuclideis an atom with a particular mass number and atomic number. • Nuclei with the same atomic number but different mass numbers are calledisotopes.

17. Nuclei with the same atomic number but different mass numbers are calledisotopes. E.g. Carbon may exist as a number of isotopes Unstable nucleus; prepared by nuclear reaction in a cyclotron. Stable nucleus; accounts for 98.89% of natural carbon. Unstable nucleus; trace amounts present in living matter. Unstable nucleus. Stable nucleus; accounts for 1.11% of natural carbon.

18. Theatomic mass of an elementis 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 is the reference for a.m.u scale. Mass of nuclide taken from a reference table