Chem Bridging Manual 2020 PDF

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School of Chemistry and Molecular Bioscience University of Wollongong

Chemistry Bridging Course Handbook

2020

NAME

Tutorial Group

Tutor

Tutorial Room

Group 1 I IA

The Periodic Table of the Elements

1

H Hydrogen

1.01 3

Group 18 VIII VIIIA

Group 2 II IIA

4

Li

Be

Lithium

Beryllium

6.94

9.01

11

12

Na

Mg

Sodium

Magnesium

22.99 19

24.31 20

6 Symbol Name

C

Atomic number

Carbon

12.01

Mean relative atomic mass

Group 3 IIIB

Group 4 IVB

Group 5 VB

Group 6 VIB

Group 7 VIIB

Group 8 VIIIB

Group 9 VIIIB

Group 10 VIIIB

Group 11 IB

Group 12 IIB

21

22

23

24

25

26

27

28

29

30

2

Group 13 III IIIA

Group 14 IV IVA

Group 15 V VA

Group 16 VI VIA

Group 17 VII VIIA

5

6

7

8

9

4.00 10

Ne

He Helium

B

C

N

O

F

Boron

Carbon

Nitrogen

Oxygen

Fluorine

Neon

10.81

12.01

14.01

16.00

19.00

20.18

13

14

15

16

17

18

Al

Si

P

S

Cl

Ar

Aluminium

Silicon

Phosphorus

Sulfur

Chlorine

Argon

26.98 31

28.09 32

30.97 33

32.07 34

35.45 35

39.95 36

K

Ca

Sc

Ti

V

Cr

Mn

Fe

Co

Ni

Cu

Zn

Ga

Ge

As

Se

Br

Kr

Potassium

Calcium

Scandium

Titanium

Vanadium

Chromium

Manganese

Iron

Cobalt

Nickel

Copper

Zinc

Galium

Germanium

Arsenic

Selenium

Bromine

Krypton

40.08 38

44.96 39

47.87 40

50.94 41

52.00 42

54.94 43

55.85 44

58.93 45

58.69 46

63.55 47

65.38 48

69.72 49

72.61 50

74.92 51

78.96 52

79.90 53

83.80 54

39.10

37

Rb

Sr

Y

Zr

Nb

Mo

Tc

Ru

Rh

Pd

Ag

Cd

In

Sn

Sb

Te

I

Xe

Rubidium

Strontium

Yttrium

Zirconium

Niobium

Molybdenum

Technetium

Ruthenium

Rhodium

Palladium

Silver

Cadmium

Indium

Tin

Antimony

Tellurium

Iodine

Xenon

85.47 55

87.62 56

88.91 57*

91.22 72

92.91 73

95.94 74

(98.91) 75

101.07 76

102.91 77

106.42 78

107.87 79

112.41 80

114.82 81

118.71 82

121.76 83

127.60 84

126.90 85

131.29 86

Rn

Cs

Ba

La

Hf

Ta

W

Re

Os

Ir

Pt

Au

Hg

Tl

Pb

Bi

Po

At

Caesium

Barium

Lanthanum

Hafnium

Tantalum

Tungsten

Rhenium

Osmium

Iridium

Platinum

Gold

Mercury

Thallium

Lead

Bismuth

Polonium

Astatine

Radon

132.91 87

137.33 88

138.91 89**

178.49 104

180.95 105

183.84 106

186.21 107

190.23 108

192.22 109

195.08 110

196.97 111

200.59 112

204.38 113

207.2 114

208.98 115

(208.98)

116

209.98 117

222.02 118

UUs Uuo

Fr

Ra

Ac

Rf

Db

Sg

Bh

Hs

Mt

Ds

Rg

Cn

Uut

Fl

Uup

Lv

Francium

Radium

Actinium

Rutherfordium

Dubnium

Seaborgium

Bohrium

Hassium

Meitnerium

Darmstadtium

Roentgenium

Copernicium

Ununtrium

Flerovium

Ununpentium

Livermorium

Ununseptium

Ununoctium

223.02

226.03

227.03

261.11

262.11

263.12

264.12

265.13

268

269

272

285

286

289

289

293

294

294

58

59

60

61

62

63

64

65

66

67

68

69

70

71

Lanthanide Series*

Ce

Sm

Eu

Gd

Tb

Dy

Ho

Er

Tm

Yb

Lu

Praseodymium

Neodynium

Promethium

Samarium

Europium

Gadolinium

Terbium

Dysprosium

Holmium

Erbium

Thulium

Ytterbium

Lutetium

140.12

140.91

144.24

144.9

150.36

151.96

157.25

158.93

162.50

164.93

167.26

168.93

173.05

174.97

90

91

92

94

95

96

97

98

99

100

101

102

103

Cerium

Actinide Series**

Pr

Nd

Pm 93

Th

Pa

U

Np

Pu

Am

Cm

Bk

Cf

Es

Fm

Md

No

Lr

Thorium

Protactinium

Uranium

Neptunium

Plutonium

Americium

Curium

Berkelium

Californium

Einsteinium

Fermium

Mendelevium

Nobelium

Lawrencium

238.03

237.05

244.06

243.06

247.07

247.07

251.08

252.08

257.10

232.04

231.04

258.10

259.10

262.11

Copyright Declaration Form This subject handbook contains material copied by the University of Wollongong in reliance on Part VB of the Copyright Act 1968. Subject Coordinator’s Declaration I understand that: In general, almost all material included in subject handbooks / course packs will be protected by copyright  Most authors assign their copyright to the publisher, in which case only the publisher is entitled to provide permission to copy the work  The only circumstances under which I may include material in this subject handbook without the permission of the copyright owner is in reliance upon Part VB of the Copyright Act



I agree that: I am responsible for the copyright compliance and quality of this subject handbook.  I have read the appropriate sections of UOW’s copyright website (www.library.uow.edu.au/copyright), and understand what I may copy in reliance upon Part VB  This handbook does not contain any infringing material  I have provided proper acknowledgement for all material reproduced in this subject handbook 

Subject Coordinator’s agreement

Glennys O’Brien

Date

02/ 02 / 2020

Subject

Chemistry Bridging Corse 2020

TABLE OF CONTENTS

1. Introduction to Atomic Theory ............................................................................................. 4 Tutorial 1 .................................................................................................................................... 9 2. Ions and the Periodic Table of Elements ............................................................................ 15 Tutorial 2 .................................................................................................................................. 20 3. Molecules and Chemical Equations .................................................................................... 25 Tutorial 3 .................................................................................................................................. 33 4. Classes of Reactions ........................................................................................................... 38 Tutorial 4 .................................................................................................................................. 44 5. How Much Matter: Mass and Moles .................................................................................. 47 Tutorial 5 .................................................................................................................................. 51 6. Moles in Chemical Reactions ............................................................................................. 55 Tutorial 6 .................................................................................................................................. 58 7. Limiting Reagent, Excess Reagent ..................................................................................... 62 Tutorial 7 .................................................................................................................................. 67 8. Solution Stoichiometry ....................................................................................................... 70 Tutorial 8 .................................................................................................................................. 75 9. Laboratory Experiments...................................................................................................... 80 Appendix 1 Naming Elements and compounds ...................................................................... 88 Appendix 2 Scientific Notation .............................................................................................. 97 Appendix 3 Significant Figures and Rounding...................................................................... 100 Appendix 4 Dimensional Analysis (Units) ...........................................................................104 Appendix 5 Solubility Rules ................................................................................................. 107 Periodic Tables....................................................................................................................... 109 Answers for Tutorial Questions ............................................................................................. 115 Lecture Notes ......................................................................................................................... 128

1

ORIENTATION My Lecturer: ________________________________________________________ My Tutor: _____________________________________ My Tutorial Number: ____________________________ My Tutorial Room: ______________________________

2

INTRODUCTION Welcome to the Summer Session, Chemistry Bridging Course. Most students undertaking this course have not studied chemistry at school but wish to undertake first year chemistry at university. Look around the lecture theatre, you are not alone!! The aim of the Chemistry Bridging Course is to introduce you to the fundamental concepts in chemistry. In addition to the 3 hours of lectures and tutorials presented each morning of the Chemistry Bridging course, you are strongly advised to spend another 3 hours each day in private study. The following method of study is highly recommended: After each Bridging course lecture / tutorial: • Read over the relevant notes in this manual. • Complete any tutorial problems on the topic not covered in class. • Find the topic(s) covered that day in a chemistry textbook. Read and summarise the appropriate section(s) and attempt relevant problems. • There are some useful websites which have links from the “Box of Useful Tricks” in eLearning website. • Note that summarising the text or applying the principles in some problems means you actively engage in thinking about the concepts, reading alone can mean that your eyes simply slide over the words. During Summer Session you will have a lot more spare time than during Session 1. All the effort that you put into studying Chemistry during the Bridging Course will pay off immensely and make your life a lot easier during Session 1. ABOUT TEXTBOOKS For CHEM104 students: Chemistry Core Concepts Blackman et al 2nd edition. Wiley 2018 For CHEM103 students: Chemistry The Central Science, Brown et al, 14th Global edition, Pearson 2018 Also highly recommended for all students of chemistry: Essential skills for Science and Technology, Zeegers, (Oxford). Numerous introductory chemistry textbooks are available in the university library, section beginning 540. Textbooks used in First Year Chemistry in the past will also be referred to in some instances. Where material is not directly referenced, use the index for that book. Most materials covered in this bridging course you will find in the first few chapters of any comparable text. 3

1. Introduction to Atomic Theory Stamp collectors classify stamps. What classification scheme an individual stamp collector may adopt varies with the purpose of the activity. One might classify according to country of origin, another by date of issue, yet another by philatelic value. Similarly, chemists classify matter. If a chemist reports that A reacted with B to give C, it is essential that other chemists understand what A, B and C are with as great a precision as possible. Clearly then, we must have agreed ways of describing materials and this leads us to various classification schemes. Central to our view of the nature of matter is the concept of an atom. Dramatic changes to atomic theory occurred in the early part of the last century, changes which have dominated our perceptions since. In this topic we introduce some basic ideas, which will allow a smooth transition to a deeper treatment given later in Chemistry 104/103. Here we will consider atoms as the basic building blocks of matter and discuss some of their fundamental properties.

Having completed this topic you should be able to: 1. classify substances according to various properties. 2. name the elements most commonly encountered in chemistry and recognise their symbols. 3. list the three major subatomic particles, their corresponding mass and charge and their location in the atom. 4. know the position of the elements in the main group of the periodic table. 5. begin developing an appreciation of the link between atomic structure and chemical properties. References: Core Concepts: Ch 1 Central Science: Ch1, 2

4

1.1 CLASSIFICATION OF MATTER Matter is stuff. We commonly think of it as anything which has mass and volume. We can choose any set of characteristics to classify matter. Which set we choose will depend on the reasons we have for wanting to classify matter. Some classifications we shall find useful are given below.

Classification by Uniformity If all samples have the same properties, the matter is said to be homogeneous; if not, it is heterogeneous. Within a sample, any portion that is homogeneous, physically distinct and separated from other parts of the sample is called a phase. For example, granite has three (solid) phases. Fog has two phases (water and air). The phase of a material can be used as a classification group itself – see below. Classification by Physical State The chemical behaviour of matter is affected by its physical state. Classifying matter into the three physical states - gas, liquid and solid - and examining the behaviour of these states allows us to gain insight into the nature of matter. Classification by Reactivity We shall meet many of these throughout the course, e.g. metals/non-metals, acids/bases etc. Classification by Composition Matter can be classified by the complexity of its composition. The most complex is a mixture, defined as a sample of matter which can be separated by physical methods into two or more pure substances. It is important to note that the proportions of the components of any mixture can vary. For example, a mixture of coffee, sugar and water can have any proportion of the three. Mixtures can be described as either heterogeneous (e.g. sand and salt) or homogeneous (e.g. sugar and water), which are called solutions. Physical methods of separation are those where the components are separated from one another without changing their chemical composition. For example, evaporating the water from a sugar solution separates the two, but you still have sugar and water. Pure substances have a composition that is fixed and definite. For example, any amount of water we take it always contains 11% hydrogen and 89% oxygen by mass. There are just over one hundred pure substances into which all other pure substances can be decomposed (broken down by chemical means). They are called the elements – matter of fixed and definite composition which cannot be chemically decomposed into more simpler substances. 5

All other pure substances are made up of two or more elements which are called compounds: matter of fixed and definite composition which can be decomposed into elements. The following diagram may be of help to classify substances.

1.2 INTRODUCTION TO ATOMIC THEORY “...there are an infinite number of them, and they are invisible owing to the smallness of their bulk. They move in the void (for there is a void); and by their coming together they effect coming into being; by their separation, passing away.” The notion of an atom goes back at least as far as the...