Instructor: Dr. Lee Hanlan Office: BLU 9706 Phone: 778-782-4409 e-mail: [email protected] Course Web Sites: Go To: www.chemistry.sfu.ca click on course websites (lower left corner) select the appropriate course site (C
Key Idea: Molecules must collide to react.
However, only a small fraction of collisions produces a reaction.
Arrhenius: An activation energy (threshold energy) must be
overcome to produce a chemical reaction.
Thomson Atomic Model (1903)
An atom consists of a diffuse cloud of positive charge with the negative
electrons embedded randomly in it. This model is often called plum (or
raisin) pudding model.
Observed cathode ray (produced at the negative e
Atomic Size and Group Anomalies
Atomic size increases down a group.
Large increase in atomic radius in going from first to second member.
First element shows properties that are quite different from the others.
Hydrogen is a nonmetal but lithi
Atomic Structure and Periodicity
Radiant energy that exhibits wavelength-like behavior and travels
through space at the speed of light in a vacuum.
Example: The sun light, energy used in microwave oven, the x-rays used
Acids and Bases
Acids and Bases
Arrhenius Concept: Acids produce H+ in solution, bases produce OH ion.
Brnsted-Lowry: Acids are H+ donors, bases are proton acceptors.
HCl + H2O
Cl + H3O+
Proton is transferred from t
Chemistry 1154 Fall 2015 Test 1
Thursday, October 1, 2015
Time: 1 hour 50 minutes
This exam consists of eight pages of questions, the formula sheet, and a periodic table. Please
ensure that you have a complete paper and, if you do
Acid and Base Multiple Choice
21. Consider the following acid-base equilibrium:
In the reaction above, the Brnsted-Lowry acids are
A. H2O and OH
B. HCO3 and OH
C. H2O and H2CO3
D. HCO3and H2CO3
22. Consider the following solu
Equilibrium Multiple Choice
7. Consider the following graph:
When equilibrium is reached, the rate of the forward reaction is
A. 0.00 mol/min
C. 1.0 mol/min
D. 3.0 mol/min
8. Consider the following equilibrium:
Reaction Kinetics Multiple Choice
1. Consider the reaction:
Ca (s) + 2H2O (l) Ca(OH)2 (aq) + H2 (g)
At a certain temperature, 2.50 g Ca reacts completely in 30.0 seconds.
The rate of consumption of Ca is
A. 0.00208 mol/min
B. 0.0833 mol/min
Solubility Multiple Choice
13) In 0.20M Na2CrO4, the ion concentrations are
14) Which of the following compounds is the least soluble in water?
The next six questions pertain to the situation described below.
A circuit is constructed with four resistors, one inductor, one battery and a switch as shown. The
values for the resistors are: R1 = R2 = 73 Q, R3 = 62 Q and R4 = 100 Q. The i
Atomic Spectrum of Hydrogen
When H2 molecules absorb energy, some of the H-H bonds are broken and
resulting hydrogen atoms are excited. The excess energy is released by
emitting light of various wavelengths to produce the emission spectrum of
Pure substance is one with constant composition. Pure substances can be
isolated by separation techniques distillation, filtration, chromatography.
is a substance with constant composition that can be broken down into
elements by chemical
Second Order Rate Law
The reaction is first order in A if a plot of ln[A] versus t is a straight line.
The integrated rate law for a first order reaction can also be expressed in
terms of a ratio of [A] and [A]o as follow:
Half-Life of a
Quantitative Measure of Matter (Chapter 2) Precision and Accuracy Errors Significant Firgures
Quantitative Measure of Matter
Numbers: Exact Numbers -counted or defined -no uncertainty
Units and Calculations (Chapter 3)
Basic Concepts of Matter Chapter 4
The science devoted to the study of matter, its composition, its structure, its properties, and the changes it undergoes (via reactions). Matter: anything that occupies space and has mass
Lecture 4: Atoms, Molecules, Subatomic Particles
Atoms and Subatomic Particles
Atoms and Molecules: Chapter 4.10 and 4.11 Structure of the Atom and Subatomic Particles: Chapter 5.1 5.5 inclusive You are not responsible for the sections on nuclear chemistr
Other Atomic Species
Ions -obtained when electrons are added to, or removed from a neutral species Cation -a positively charged ion -the result of removing 1 or more electrons from a neutral species Anion -a negatively charged ion -the result of
From last notes: Pure substances Chemical formula Chapter 6 Basic Structure of the Periodic Table How electrons reside in atoms
The Periodic Table
Mendelev, 1869 arranged elements in order of increasing atomic mass led to natural grouping of ele
How many electrons?
per shell 2n2 varies with type of subshell 2
From last notes: shells, subshells and orbitals, Chapter 6.3 6.6 How electrons reside in atoms, electron configurations Chapter 6.7 6.8
per subshell per orbital
Subshell # of orbit
Electron Configurations of Simple Ions
Anions: Electrons added to form anions follow the Aufbau rule, Hunds rule and the Pauli Exclusion principle F + e1s22s22p5 F1s22s22p6
Electron configurations ( from last notes) Electron configurat
Points to note:
Ionic vs Molecular compounds ( select information from Chapter 7) Introduction to Nomenclature (Chapter 8) Naming ionic compounds
valence electrons are in the outer most regions of the atom ions form by losing or gaining electron
Naming Binary Molecular Compounds
generally contain two different non-metallic elements
Ionic vs Molecular compounds (from last notes) Introduction to Nomenclature (Chapter 8) Naming ionic compounds (from last notes) Naming molecular compounds
Determination of Percent Composition
Chemical Calculations: The Mole and Chemical Formula
Law of Definite Proportions (John Dalton) A given compound always contains the same proportion, by mass, of the elements. Decompose samples of a
What is the Mass of one Mole ?
Molar Mass of an Element The mass in grams that is numerically equivalent to the atomic mass of that element. units of molar mass are: grams/mole atomic mass of 12C: 12 amu 1 mole of 12C atoms weighs 12 g/mole
Chemical Calculations, Chapter 9: Determining empirical and molecular formula from experiment data How can we determine, experimentally, the number of moles of each element that are present in a sample of an unknown pure compound?