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General Chemistry for Engineering I
McMaster University
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Browse the full collection of course materials, past exams, study guides and class notes for CHEM 1E03 - General Chemistry for Engineering I at McMaster University verified by our …

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Randall Dumont; Linda Davis

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Class Notes

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CHEM 1E03 Lecture 1: CHEM 1E03 - LECTURE 1

CHEM 1E03 Lecture Notes - Fall 2018 Lecture 1 - Final examination

CHEM 1E03 Lecture Notes - Lecture 2: Work Function, Photon

Start at the bottom: matter is made of atoms (and ions). Properties of atoms and ions are determined by their electronic structure the arrangement of t

CHEM 1E03 Lecture Notes - Lecture 2: Black-Body Radiation, Work Function, Electric Field

CHEM 1E03 Lecture 2: CHEM 1E03 - LECTURE 2

CHEM 1E03 Lecture 3: CHEM 1E03 - LECTURE 3

CHEM 1E03 Lecture 3: Lecture 3

An electron can be ejected from the atom - this is called ionisation. For lower energy photons (i. e. lower frequency), an excited state of the atom ca

CHEM 1E03 Lecture Notes - Lecture 3: Magnetic Quantum Number, Rydberg Constant, Quantum Mechanics

Quantum mechanics tells us that an atom has a discrete set of energy levels (only certain energies are allowed) Re = 2. 179 x 10-18 j rydberg energy ne

CHEM 1E03 Lecture 4: CHEM 1E03 - LECTURE 4

CHEM 1E03 Lecture Notes - Lecture 4: Pauli Exclusion Principle, Principal Quantum Number, Matter Wave

CHEM 1E03 Lecture 4: Lecture 4

For the hydrogen atom, the orbital energy depends only on the principal quantum number. The number of orbitals with energy e(n) is. 1 + 3 + 5 + + 2n -

CHEM 1E03 Lecture Notes - Lecture 5: Ionic Radius, Electron Configuration, Atomic Radius

CHEM 1E03 Lecture 5: periodic table continued, chapter 4 - periodic properties, atomic/ionic radius

CHEM 1E03 Lecture 5: CHEM 1E03 - LECTURE 5

CHEM 1E03 Lecture Notes - Lecture 5: Effective Nuclear Charge, Atomic Radius, Ionic Radius

The electron configuration of be, b, and c: Repulsion between the two 2p electrons in c is minimised when the electrons have the same spin they are in

CHEM 1E03 Lecture 6: CHEM1E03-LECTURE 6-CO1

CHEM 1E03 Lecture Notes - Lecture 6: Group 3 Element, Ion

Ionization energy (ie for short in my notes) 1st ie ( i 1 ) - energy needed to eject an electron from an atom in the gas phase - the energy change for:

CHEM 1E03 Lecture 6: CHEM 1E03 - LECTURE 6

CHEM 1E03 Lecture Notes - Lecture 6: Diamagnetism, Noble Gas, Paramagnetism

See if there are unpaired electrons in electron configuration. When you ionize it you take an electron away. Therefore it is harder to take an electron

CHEM 1E03 Lecture Notes - Lecture 6: Electron Affinity, Ion

Li > be > b > c > n > o > f > ne. The effective nuclear charge is approximated by core charge, the charge of the nucleus plus the (negative) charge on

CHEM 1E03 Lecture 7: CHEM 1E03 - LECTURE 7

CHEM 1E03 Lecture 7: CHEM1E03-LECTURE 7-C01

CHEM 1E03 Lecture Notes - Lecture 7: Sulfuric Acid, Chemical Polarity, Metallic Bonding

Electrons are bound, in a deep well , to take them out requires energy. To take an e that is originally free is an exothermic rxn. General trends of ea

CHEM 1E03 Lecture Notes - Lecture 7: Electron Affinity, Effective Nuclear Charge, Amphoterism

In nature, atoms are constantly interacting, chemically and otherwise: chemical properties: depend on the number of valance e- and the enc (effective n

CHEM 1E03 Lecture Notes - Fall 2018 Lecture 8 - Ion, Molecular orbital theory, Triple bond

Electronic structure of a set of covalently bonded atoms. Orbitals - electrons go in in pairs. Group 1 atom one val e. They tell us which atom is centr

CHEM 1E03 Lecture 8: CHEM 1E03 - LECTURE NOTES 8

CHEM 1E03 Lecture 8: CHEM1E03-LECTURE 8-C01

CHEM 1E03 Lecture Notes - Fall 2018 Lecture 8 - Electron configuration, Electronegativity, Formal charge

CHEM 1E03 Lecture 9: CHEM 1E03 - LECTURE 9

CHEM 1E03 Lecture Notes - Lecture 9: Lone Pair, Electronegativity, Formal Charge

CHEM 1E03 Lecture Notes - Lecture 9: Formal Charge, Lone Pair, Lewis Structure

Farmers replenish nitrogen in soil which allows clovers to grow which gets n from atmosphere which brings more n into soil yayay babes. Bacteria live i

CHEM 1E03 Lecture Notes - Lecture 10: Molar Mass, Photon, Chemical Formula

Note: this lecture was review of the 2017 chemistry test 1. Question 3 solution: convert 300kg to g = 300,000g, convert this into grams of oxygen 300,0

CHEM 1E03 Lecture 10: CHEM 1E03 - LECTURE 10

CHEM 1E03 Lecture 10: 2017 Test 1 Review

CHEM 1E03 Lecture 11: CHEM 1E03 - LECTURE 11

CHEM 1E03 Lecture Notes - Lecture 11: Formal Charge, Covalent Bond, Trigonal Pyramidal Molecular Geometry

Average bond order: number of bonds / number of variations 5/3. Average formal charge: sum of charges / number of terminal o"s -1/3. Charge minimized l

CHEM 1E03 Lecture 12: CHEM 1E03 - LECTURE 12

CHEM 1E03 Lecture Notes - Lecture 12: Cone, X Window System Core Protocol, Covalent Bond

Molecular geometry: the shape of a molecule, and the position of the nuclei. Electron geometry: the 3- dimensional shape that a molecule occupies in sp

CHEM 1E03 Lecture 13: CHEM 1E03 - LECTURE 13

CHEM 1E03 Lecture Notes - Lecture 13: Sodium Chloride, Supersaturation, Sulfide

Aqueous solutions: (nacl: salts dissolve in water to form electrolyte solutions. Some have extremely small solubility: this occurs because water is pol

CHEM 1E03 Lecture Notes - Lecture 14: Hydronium, Conjugate Acid, Sodium Bicarbonate

CHEM 1E03 Lecture Notes - Lecture 18: Conjugate Acid, Fluorine, Half-Reaction

Equilibrium is always shifted away from stronger base. Pattern: remove an h+ to get the next conjugate base. Diprotic: acts as an acid, conjugate base

CHEM 1E03 Lecture Notes - Lecture 19: Oxidation State

Oxidation agents: an element who"s oxidation number decreases (loses electrons, higher oxidizing number = stronger oxidizing agent, reduction reactions

CHEM 1E03 Lecture Notes - Lecture 20: Bromine Monochloride, Phenolphthalein, Redox Indicator

Example basic: mno4- + i- mno2 + i2. Oxidation numbers in order: +7, -2, -1, +4, -2, 0. Addition of h+: leave alone add 2 water molecules so each side

CHEM 1E03 Lecture 21: October 22 Lecture Notes

Example: if the partial pressures of o2 and so3 are 0. 500 bar, what is the partial pressure of so2. The equilibrium constant is k = 5. 6e4: write the

CHEM 1E03 Lecture Notes - Lecture 22: State Function, Enthalpy, Rice Chart

Solve for x, and then plug this x" back into the equilibrium equations from the ice table to find the pressures of each entity (or the entity in questi

CHEM 1E03 Lecture Notes - Lecture 23: Exothermic Process, Joule

Heat: heat flows from hot to cold in thermal contact, the heat will continue to flow until the temperatures of the two contacting things are the same (

CHEM 1E03 Lecture Notes - Lecture 24: Calorimetry, Joule, Coffee Cup

Work done in chemical reactions: volume increases because mols increase (w > 0), negative work on the system, volume decreases because mols decrease

CHEM 1E03 Lecture Notes - Lecture 25: Calorimetry, Sulfur Trioxide, Joule

Calorimetry and enthalpy change: h = h1 + h2 = -c t, h: enthalpy change: change from conversion of reactants to products, c: heat capacity, t: change i

CHEM 1E03 Lecture Notes - Lecture 26: Electric Potential Energy, Lithium Chloride, Lewis Structure

Reactants: 3(c-h) + 3(c-br) + 1(c-c) 3(h-br) = [6(c-h) + 3(br-br) + 1(c-c)] [3(c-h) + 3(c-br) + 1(c-c) 3(h-br)] = 3(c-h) + 3[br-br] 3[c-br] 3[h-br] Con

CHEM 1E03 Lecture Notes - Lecture 27: Boltzmann Constant, Swedish Krona

For every balanced reaction, there is either: net forward reaction, where the reaction is spontaneous, net reverse reaction, where the reaction is non-

CHEM 1E03 Lecture Notes - Lecture 28: Residual Entropy, Uncertainty Principle, Hydrogen Bond

Further notes on entropy: entropy is a measurable property of a system that measures disorder, you can also measure the change in entropy of a system,

CHEM 1E03 Lecture Notes - Lecture 29: Equilibrium Constant, Conjugate Acid, Lewis Structure

2017 test review: solution: draw out each molecular structure for the compounds provided. Compare and see which statement is false with the provided co

CHEM 1E03 Lecture Notes - Lecture 30: Gibbs Free Energy, Spontaneous Process, Boiling Point

CHEM 1E03 Lecture Notes - Lecture 31: Gibbs Free Energy, Spontaneous Process

Dilute solute higher entropy per mole than concentrated solute. Dilute solute lower gibbs energy than concentrated solute. Lower pressure gas higher en

CHEM 1E03 Lecture Notes - Lecture 32: Voltmeter, Electroplating, Electrochemistry

Electrochemistry: electron transfer reactions of redox reactions, electrons move from reducing agent to oxidizing agent, the net reaction is composed o

CHEM 1E03 Lecture Notes - Lecture 33: Nernst Equation, Gibbs Free Energy, Reduction Potential

Oxidation and reduction half-cell potential: calculate cell potential by, sum of oxidation and reduction half reactions, difference between 2 reduction

CHEM 1E03 Lecture Notes - Lecture 34: Silver Chloride, Membrane Potential, Chemical Equation

CHEM 1E03 Lecture Notes - Lecture 35: Manganese Dioxide, Hydrogen Fuel, Acid Strength

Solution: look for the metal that is lower in the table: anything to the right of fe: cr, zn, al, mg, sr, everything except ag, al, mg, sr. Nickel-cadm

CHEM 1E03 Lecture Notes - Lecture 36: Acid Strength, Acid Dissociation Constant, Rice Chart

CHEM 1E03 Lecture Notes - Lecture 37: Acid Dissociation Constant, Conjugate Acid, This Is The End

Strength of acids: the strength of a neutral acid depends on the stability of the conjugate base, strong acid large pka, weak acid small pka. Largest l

CHEM 1E03 Lecture Notes - Lecture 39: Lattice Energy, Jmol, Silver Chloride

2017 exam solutions were taken up this class: n gas should be larger than zero for there to be an increase of energy. Therefore, the answer is none: yo

CHEM 1E03 Lecture Notes - Lecture 40: Sulfuric Acid, Stoichiometry, Novella

2017 exam solutions: create an ice table to solve for the equations required for each entity to reach equilibrium. The total pressure at equilibrium wi