CH1001_2010(Atom 1)_notes

CH1001CH1001CHEMISTRY: A Central ScienceCHEMISTRY: A Central Science

Department of ChemistrySchool of Pharmacy & Molecular Sciences

AIMS: With CH1002 {PC1005 for Pharmacy students},

CH1001 constitutes the core subject for students who intend

to undertake further studies in chemistry, industrial

chemistry, forensic science, pharmacy, biomedical science,

biochemistry, veterinary science, dentistry,

physiology and pharmacology, and chemical engineering.

It also aims to provide an understanding of basic molecular

principles and their importance in other scientific disciplines,

such as the marine, biological, health, medical, earth and

environmental sciences


! Without CH1002 {PC1005}, CH1001 is a

non-continuing subject

! If you want to use Chemistry as a pre-requisite for studies in

any of the Molecular Sciences (chemistry and/or biochemistry,

advanced physiology and/or pharmacology) or continue in

Pharmacy, Biomedical Sciences, Chemical Engineering etc.,

you will need to be enrolled in CH1002 {PC1005} in

Study Period 2.


Recommended text:

“CHEMISTRY” A. Blackman, S.E. Bottle, S. Schmid, M. Mocerino and U. Wille

(Wiley & Sons Australia, 2008)

OPTIONS:

1. Purchase of the hardcopy of the textbook from the Bookshop, which includes the WileyPLUS registration card (which provides internet access to all tutorial material and tutorial help linked to the electronic version of the text) - $135.80 (with Model Kit, $142.45).

2. The WileyPLUS registration card can be purchased separately and includes internet access to all tutorial material, and tutorial help linked to the electronic version of the text - $72.15 .

3. If you do not take options (1) or (2), you will nevertheless automatically have access to the assessed tutorials on WileyPLUS by virtue of your enrolment in the CH1001 subject, but it will not be linked to any electronic text or tutorial help.

4. The Model Kit can be purchased as a stand-alone item - $18.95.


LECTURESLECTURES (ALL LECTURES IN HLT)• Monday, Wednesday, Friday 10 - 11 am

CH1001 CH1001 CHEMISTRY: A Central ScienceCHEMISTRY: A Central Science

! Please turn off mobile phones! Please enter via the back door after the lecture has commenced (lectures start at 10 am and front doors will be closed)

Lecturing staff:

Professor Richard Keene Assoc.-Prof. Michael Oelgemoeller Dr Greg Watson (Coordinator)

COURSE INFORMATIONCOURSE INFORMATION

1. Synopses, lecture materials, tutorials, practical class assignments etc. are available on the Web through “LearnJCU”

2. Announcements may be made at lectures, and information distributed by E-Mail


PRACTICALS PRACTICALS

You have been assigned to ONE of the following sessions:Tuesday 2-5pm, 6-9pm; Wednesday 2-5pm, 6-9pm; Thursday, Friday 2-5pm


FIRST SESSION . . . is THIS WEEK (Week 1)Go to CH011 aka DB021-011 (ground floor, Molecular Sciences)

YOU MUST ATTEND THE PRACTICAL SESSION IN WEEK 1

Repeat students may apply for exemption from the Practical course if they have already satisfactorily completed it.

In charge of Practical course:

Dr Brian McCool Brian Foster

PRACTICALS PRACTICALS (cont.) (cont.)


YOU NEED:

! LABORATORY MANUAL ($7.50) + REPORT BOOK ($4.95) at JCU Bookshop

! Purchase pipette filler ($9.85) +

safety glasses (SG1/SG2 and SG3 - $8.20) +

laboratory coat ($24.23) at JCU Bookshop

! Adequate footware


You will be assigned to practicals for the following subjects:

AG1002 CH1001 TV1101BZ1001 EA1110

BM1000 and TV1102 start in Week 2, and can be dealt with bysign-up AFTER the above subjects have been assigned

Assignments are posted on notice-boards inMolecular SciencesBiological SciencesVeterinary & Biomedical SciencesMaths/Physics/Earth Sciences

AND posted on LearnJCU

TUTORIALSTUTORIALS


2. There will also be Tutorial sessions held on • Tuesday 12 - 1 pm (CLT aka DA005)• Wednesday 8 - 9 am (NS002 aka DB025-002) • Thursday 12 - 1 pm (CLT aka DA005)

Assign yourself to ONE of these sessions.

Questions will be put on LearnJCU prior to the Tutorials: the sessions are intended to have problems of the style that would appear in the exam, and with the time to informally work carefully through the answers. Tutorials given by lecturer of particular section of the course.

1. From Week 2, there will be assessable Tutorials assigned on the WileyPLUS Website. These will have a strictly applied time cut-off.

3. The Tutorial session in Week 1 will demonstrate the use of the WileyPLUS system, and from Week 2 the Tutorial sessions will deal with additional questions (not assessable).

ASSESSMENTASSESSMENT

• EXAMINATIONS 60%

- 3 hour examination in June

• On-line TUTORIALS on the WileyPLUS site 10%

- continuous assessment

• PRACTICAL 30%

- continuous assessment

CH1001: CH1001: CHEMISTRY - A Central ScienceCHEMISTRY - A Central Science

DEVELOPMENT OF CHEMISTRYDEVELOPMENT OF CHEMISTRY

! Alchemy

Adam McLean“The Alchemy Web Site”

Alchemy . . .

Alchemy . . .

DEVELOPMENT OF CHEMISTRYDEVELOPMENT OF CHEMISTRY

! Alchemy

! Antoine Lavoisier

! John Dalton

! “Phlogiston Theory”

11 The atom The atom

The atomThe atom

• Chemistry is the science concerned with

the study of matter

! Central to this study is the way matter is

constructed from the simplest building block,

the atom

• Atoms

– Discrete chemical species comprising a central

positively charged nucleus surrounded by 1 or

more negatively charged electrons

– Atoms are always electrically neutral

Atoms, Atoms, moleculesmolecules, ions,, ions,

elements and compoundselements and compounds

• Molecules

– Collections of atoms with a definite structure

held together by covalent bonds

– Covalent bonds involve the sharing of electrons

between neighbouring atoms

• Ions

– Chemical species that have either a positive or

negative electric charge

– Cations are ions with a positive charge e.g. Na+

– Anions are ions with a negative charge e.g. Cl–

Atoms, molecules, Atoms, molecules, ionsions,,


• Elements

– Collections of one type of atom only

– There are 117 (at the moment)

– The Periodic Table (next slide) lists all the

elements

Atoms, molecules, ions,Atoms, molecules, ions,

elementselements and compounds and compounds

• Compounds

– Substances containing two or more elements indefinite and unchanging proportion

– Compounds may be composed of molecules ora covalently-bonded network of atoms

– Do not have individual ‘molecules’ of an

ionic compound

• Sodium chloride, NaCl, simply represents the smallest

repeating unit in an enormous 3D array

of Na+ and Cl– ions


elements and elements and compoundscompounds

IONICIONIC

! transferring of electron(s) from one element to the other (giving

positive CATIONS, Mn+, and negative ANIONS, Xn-)

! formed between a metal and a nonmetal

COVALENTCOVALENT

! sharing of electrons between atoms

! formed between two nonmetals

BONDINGBONDING



IONICIONIC

The atomic theoryThe atomic theory

• Law of conservation of mass

– No detectable gain or loss of mass occurs in

chemical reactions. Mass is conserved.

• Law of definite proportions

– In a given chemical compound, the elements

are always combined in the same

proportions by mass.

Dalton’s Atomic Theory

1. Matter consists of tiny particles (atoms).

2. Atoms are indestructible. In chemical reactions, the

atoms rearrange but they do not themselves break

apart.

3. In any sample of a pure element, all atoms are identical

in mass and other properties.

4. The atoms of different elements differ in mass and other

properties.

5. When atoms of different elements combine to form a

given compound, the constituent atoms in the compound

are always present in the same fixed ratio.


• Chemical equations describe chemical

reactions

– Reactants go on the left hand side

– Products go on the right hand side

– Reactants and products are separated by a

forward arrow

2H2 (g) + O2 (g) " 2H2O (l)reactants products


2H2 (g) + O2 (g) " 2H2O (l)

– The Law of conservation of mass requires the

same number of each type of atom on each

side of the arrow

• When this is the case the reaction is described as

balanced.

– Physical states can also specified in

chemical equations

• Gases, liquids and solids are abbreviated

g, l and s


The structure of the atomThe structure of the atom

• Atoms are comprised of a nucleus and

surrounding electron(s)

– The nucleus occupies less

than 0.1% of the

total atomic volume

– The nucleus is

comprised of

protons and

neutrons


– X is the chemical symbol for any element

– Z is the atomic number, this is the number of protons in

the nucleus

– A is the mass number, this is the number of protons plus

the number of neutrons in the nucleus

XA

Z

– In a neutral atom the atomic number is also

equal to the number of electrons

H – hydrogen

1 proton (Z = 1)

1 electron

0 neutrons (A = 1)


H1

1

• Isotopes

– Atoms of an element with the same number of protons

but different numbers of neutrons

– Radioactive isotopes have unstable nuclei which undergo

spontaneous decay to more stable nuclei

– Nuclide

• Any atomic nucleus

• Radioactive nuclei are called radionuclides


H1

1 H2

1H

3

1

• The chemical symbol is indicative of the atomic number, so it

is common to see a shorthand version

– is written as 1H

• Atomic mass unit (u or amu)

– The mass (1.666 054 ! 10–27 kg) equal to 1/12 the mass

of one atom of 12C

– The masses of all atoms are measured relative to this

– Average atomic masses account for isotopic abundances


H1

1

The Periodic Table of elementsThe Periodic Table of elements

Dmitri Mendeleev

! Elements ordered in order of

atomic weights (mass)

! Elements with similar properties

put in vertical columns (called

“Groups”)

! Led to discovery of a number

of new elements

• Elements may be ordered on the basis of

increasing atomic number (Z)

• The modern periodic table of elements illustrates

this ordering

• The periodic table is organised into:

– Horizontal rows called periods

– Vertical columns called groups




! PERIODS - horizontal rows

! GROUPS - vertical columns (chemical similarities)

- Those labelled “A” are representative or

main group elements (Groups 1-2, 13-18)

- Those labelled “B” are the transition elements

(Groups 3-12)

- Elements 58-71 are the lanthanide elements

- Elements 90-103 are the actinide elements

! COMMON NAMES OF GROUPS:

- IA - alkali metals- IIA - alkaline earth metals- 0 - noble gases- VIIA - halogens

! SYMBOLS


• Metals– Generally good conductors of heat and

electricity, are malleable and ductile and have ametallic lustre

• Non-metals– Elements that do not have these characteristics

• Metalloids (semiconductors)– Lie somewhere between metals and non-metals


Electrons in atomsElectrons in atoms

• Many of the chemical properties of an atom

and its chemical reactivity are determined

by the electrons

– Electrons occupy regions of space called

orbitals

– Each orbital has a characteristic electron

distribution and energy

– An electronic transition occurs when an atom

absorbs a specific amount of energy and an

electron is promoted to a higher energy orbital

to form an excited state.

– Orbitals have definite energies. This is a

fundamental principle of quantum mechanics

call quantisation.


– Electrons have a single negative charge

– Electrons have an intrinsic property called spin

– Spin can only have two values

! spin up

" spin down

– Each orbital within an atom can contain amaximum of 2 electrons, 1 spin up and1 spin down

"#


– Electrons constitute the chemical bonds

that hold atoms together

– Covalent chemical bonds usually consist of

1, 2 or 3 pairs of electrons shared

between atoms

– Chemical reactions often involve reorganising

these electrons in bond-making and

bond-breaking processes

!""""" Redox reactions involve transfer of one or

more electrons between chemical species


• Atoms are the fundamental building block of all

matter

• The existence of atoms was proposed on the basis

of:

– The Law of conservation of mass

– The Law of definite proportions

The atom - The atom - SummarySummary

• The atom is comprised of three subatomic particles;

the electron, proton and neutron

• Elements comprise only a single type of atom. The

Periodic Table arranges all known elements in

order of increasing atomic number

• Electrons occupy regions of space called orbitals

– Energies of electrons in an atom are

determined by the energies of the orbitals, so

electrons in atoms have only certain well-

defined energies

The atom - The atom - SummarySummary

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CH1001_2010(Atom 1)_notes