1. Unit 1: Matter and Energy

TC3 CHEM 1XX Syllabus; Dr. Zisk

1st Semester

1. Unit 1: Matter and Energy...

A. Matter

i. Definitions

Start with atoms, smallest matter, then build...

Seven major concepts:

1)Elements, 2)compounds, 3)mixtures

Don't forget looser term "substances"

Use of 4)physical, 5)chemical properties/separations

Distinguish 6)homogeneous and 7)heterogeneous mixtures

ii. Density and constant composition of compound introduces math

d=m/v but solve for m or v...show them

Water 11% hydrogen, 3g hydrogen means how much oxygen?

iii. Mention phases, but note unit #2

B. Energy

i. Four Questions:

What is it? Can do work...don't forget KE vs PE, and subtypes

What's "conservation"? Gets converted, but never destroyed

In chem, where's it come from? bonds formed ...Endo/Exo

What's temperature? Is it heat?

ii. Segue into heat capacity; the hot(water vs. Pb) in the hand demo

iii MC∆T=∆H

Explain delta

Relates heat and temperature

Mass of given C will change T in relation to H in or out

iv. Celsius-Kelvin (abs. zero)

2. Unit 2 Phases...

A. Graph of temp vs time

i. The plateaus?

ii. Phases at all points?

Introductory description of phases (macro and micro)

Arrangements and structure

Motions

Energy differences

Clear definition of exo-, endothermic

In terms of bonds forming, breaking

On T vs. t the diagonal arrow up/rt=endo, down/lft=exo

iii. FP/MP and BP

iv. KE and PE changes as we go?

B. Heats of fusion and vaporization (see the plateaus on temp:time)

i. Calculations

C(s)≠C(l), C(g)

KEY: use mC∆T when there is a ∆T; m∆H when isn't.

ii. Representing bond -strength, intermolec forces

C. Advanced description of molecular transition between phases

i. Describe motions, energies and bonds

Kinetic theory of gases, of matter

Boltzman distributions of E vs #, T=peak=avgKE

Intermolecular forces: strong/solid, weak/gas

ii. First Definition of Equilibrium (see unit 7 below for more)

Put a lid on a liquid evaporating

Define torr, mm , atm

Define vapor pressure

Boiling vs. evaporation

Effects of ∆(P, V, T) on g-l equilib

iii. Sublimation, deposition (high intermolec forces; high vap P)

iv. Phase diagram

3. Unit 3: Gas laws...

A. Start with a balloon for all of these

i. Sealed, so no change in amount of gas

ii. Students can discover the inverse relat of P to V

iii. The laws can be summarized

What's a constant...what's it mean?

PV and V/T stay at a constant level

Try P1V1=P2V2 etc.

B. Now leave the balloon and do the math implied above;

i. What's really happening in the vessel with ∆(P, V, T)?

ii. Brackets with dots, compress 'em

iii. Non-ideality at the extreme compression

iv. Non-ideality with extreme cold

D. Look at two-colored set of dots=two gases in mixture

i. Talk about "exerting" pressure, impacts of dots

ii. Each dot contributing a fraction of the total

G. Also, Avagadro/Dalton give us 22.4L=1mole; 1mole=6x1023

Unit 4: Atomic structure & e-config...

A. Follow the paradigms--

i. Democritus-- smallest particle;

ii. Charge and the atom; Rutherford and arrangement

iii. Einstein; Planck; Bohr; Schroedinger/Heisenberg

iv. Summarize the current cloudy paradigm

B. Construct a table of parts showing name, mass, charge, size.

C. Symbols for elements are the key to parts:

i. A, Z, and ion charge tell p's, n's and e's (not in that order)

ii. What's ion?! We haven't defined electron movement!!... Shortly, not now...

iii. Isotopes

D. Most important: Electrons around a nucleus

i. Shells, or "levels"

ii. Movement between levels

Students graph me climbing on chairs, desks, cabinets etc.

No in-between places; energy release upon falling, absorb to climb

Hence the image of quantized transitions, the Bohr Model

iii. E=hƒ; ƒ=c/w; are they comfortable yet with powers of ten?

iv. Radiation; spectra; fingerprints

continuous vs. discrete

bright-line vs absorption

again, E=hƒ

E. E-config In Total...recall/compare to Bohr model

i. Energy level=shell; s-p-d=subshells; arrows are orbitals.

ii. How many subshells, orbitals, electrons per energy level?

iii. Defining the variations in sub-shells

iv. Defining the ordering of energy of orbitals

v. Filling rules; the "discrepancies" at d and f, and at half-filled- and filled-minus-one

vi. Configuration notations and meaning; excited states notations

vii. Filling order; config given Z?

viii. Quantum numbers (treat this lightly)

F. Nuclei again, get ready for the next unit:

i. recall Z, p's and n's;

ii. Let's define amu, gaw, gmw;

iii. Look at that mole now.

vi. practical uses

medicinal

reactors

Unit 5: Bonding; Chemical Formulas at first glance ...

A. Bonds

i. Recall: Electrons interacting with each other

why would nuclei come together?

electrostatics

shared e's vs ions

ii. Look again at Energy

∆H vs Rxn Coordinate-- what's happening here??

Bonding or any chemical∆ is always accompanied by energy∆

Cf units on Kinetics/Equilib and on ElectroChem: Chem doesWork

Foreshadow the Reverse/Forward DG-driven equilib we'll see later

iii. And we need a formalism: Using Lewis dot diagrams

iv. These are, broadly put, valence electrons-- but we'd better definehybridization

Allows VSEPR model

Multiple bonding

Expanded octets

v. Molecular structure

General structures (refer back to bonding)

Molecular dipole; symmetry; range from ionic to VanderWaals

Role of lone pairs...coordinate covalent bonds

vi. The unusual cases:

metallic

networks

B. Formulas

i. Charge-ox.state summing, balancing

ii. Names and endings

iii. Polyatomic ions

Unit 6: Periodic Table ...

A. What's happening to atomic structure across periods or down groups?

B Periodic trends

i. EN, IP, r

ii. Activity (vs. "reactivity)

iii. Ox numbers and valence electrons revisited, with the table as a map

C. The Major Groups

i. Alkali; alkaline earth;

ii. Transition; sub-transition metals;

iii. Metalloids;

iv. Halogens; noble gases

2nd Semester

Unit 7: Chemical Formulas and Equations in some detail...

A. Quantities of interest

Moles; gaw/gaw/aw/fw; amu; M/m

Formulas imply these quantities

B. Mass balanced equations

C. Concentrations; distinct from Ideal Gas Molar Volume conversions

D. Real quantitative problems

Molecular mass and density of ideal gases

Percent composition

Composition and empirical-molecular formulas

Chemical equations and (mass-volume-concentration-number) problems

Diffusion, mass and Graham's Law

Unit 8: Kinetics and Equilibrium; Solutions and Solubility...

A. Defining dynamic equilibrium

Evaporation in a closed container

Saturated solutions with ppt interface

Rates and factor governing them

B. Equilibrium constants and LeChatelier

Steady conc's, but still dynamic; rate(f)=rate(r); T effects

Addition to system with inherent constant forces change

But define in terms of stress or kinetics for true depiction

C. Solution behavior is nice image of kinetics and equilib

Solvation

Attractions

Enthalpy and Entropy as Driving Forces

D. Gibbs Free Energy, Defined and Equation

To do work

Spontaneity

Energy vs reaction progress curves, again

Dominant terms in various cases for the equation

Unit 9: More on Solutions;special cases of Acids and Bases...

A. Dissolving vs dissociation-- is it clear

B. Electrolyte behavior

What is conductivity?

How ions behave, considering metals, fused salts and electrolytic solutions

C. Dissociation in water, and of water itself

D. Define acids and question the utility, history of each model

Arrhenius

Bronsted/Lowry

Lewis

E. Conjugate acid-base pairs

Reactions; can they find the species of interest?

Strength; conjugate of strong is weak and vice verse

Amphoterics

F. Acid or base equilibrium constants

How's their exponential and logarithmic math?

Significance of the product, in water, in syntheses, and in biological systems

Defining autodissoc constant for water, pH/pOH

G. Titrations and other real quantitative problems

Unit 10: RedOx and Electrochemistry Just another equilibrium, another driving force…

A. One species oxidizes another; and is in turn reduced

B. Changes in oxidation state

Element cries to a buddy "I've been robbed, someone stole my electron". Reply "are you sure". Element says "yeah, I'm positive"

C. Look at a whole redox reaction first

Follow the changes

Look at electron flow

It's two halves of a battery

D. Using an activity series

All are given in the series as reductions, as the cathode reaction

Defining stronger/weaker reduction potentials as voltages; ∆G=-nFE

The weaker half reaction, lower on the series, must proceed as ox

E. Now set up two half-cells, and show a whole reaction as summed

Where's voltage obtained, physically and mathematically?

What does it mean to "balance" electrons gained/lost?

G. What are the other parts of the cell?…Find the cathode/anode, and the signs

H Electrolytic cells??

I. Finally, balancing given reactions, and exploring inherent voltage, current.

Unit 11: Organic overview “Here’s where you’d go next year...”

A. Carbon; life; SPONCH

Bonding

General chem-phys characteristics

B. Simplest compounds; homologous series

C. Major groups: -anes/enes/ynes; -ols; -als; -ones; acids; esters; amines/amino-acids

Easily confused sets...

Distinguishing features

What do they do, chemically-physically

Tabulate the nomenclature

D. Major reactions: sub; add; elim; dehydrate; sapon; combust; ferment; polymer; crack! Environmental issues?

Unit 12: Industrial and other Chemical Applications we've mentioned,In Summary..

Haber; Catalyses

Cracking; Syntheses

Plating/batteries; Oxidations; corrosions/preventatives

Metabolic pathways

Nuclear reactors