CHM 1045--General Chemistry I--Fall 2002

### What Do I Need To Learn?

The objectives for each chapter are given in some detail at your textbook's companion web site. You will be responsible for being able to work the types of problems done in class and recitation, suggested end-of-chapter problems, and problems on the CAPA homework set.

In addition, from time to time, there will be certain things you will just have to memorize, as you would a vocabulary in a language course. Below I will list these specific things you will need to learn from memory.

Chapter 1
Metric prefixes.
Approximate English to metric conversions.
Chapter 2
Know the names and symbols of elements 1 to 57, plus W, Pt, Au, Hg, Pb, Bi, At, Rn, Th, U, Np, Pu
Knownames and charges on monoatomic ions (Figure 2.8 )
Know names and charges on polyatomic ions (Table 2.4 )
Know names and formulas of acids and salts (Table 2.5 )
Know organic word stems (Table 2.6 )
Know names and structures of organic classes (Table 2.7 )
Chapter 3
Chapter 4
Strong acids and strong bases (Table 4.1)
Gas-forming reactions (Table 4.2)
Solubilities of common ionic compounds (Table 4.3)
Rules for writing oxidation numbers (page 154)
Chapter 5
Units of pressure
Gas Laws
Molecular Weight from Density
Chapter 6
Energy and work definition
Dimensions and units of energy
Internal Energy and Enthalpy Relationships
Isolated, closed, and open systems, definition
First Law of Thermodynamics
Units of heat capacity and specific heat
Hess's Law
Calculation of Enthalpy of reaction from Standard Enthalpies of Formation
Chapter 7
Names of Scientists and their contributions to explaining atomic structure
Equations for interconverting wavelength, frequency, and energy of light quanta
Relative order of spectral regions (not specific wavelength ranges)
Rydberg equation for energy between Bohr orbits
De Broglie equation (wavelength of a particle from its mass and velocity)
Shapes of s, p, and d orbitals
Allowed quantum numbers, and quantum numbers associated with different orbitals
Chapter 8
Electron configuration of atoms and ions
Number of unpaired electrons in atoms
Trends in atomic and ionic radii, comparison of sizes
Trends in ionization energy and electron affinity, comparison among atoms
Reaction of metal and non-metal oxides with water
Chapter 9
Ionic bonding and lattice energy
Lewis dot structures, resonance structures
Formal charge; oxidation number
Trends in electronegativity, comparison of polarity of bonds
Using bond energies to calculate heats of reaction
Chapter 10
VSEPR description of electron pair (or group) geometry and molecular geometry
Determining polarity of a molecule from bond polarity and geometry
Hybrid orbital description and relating geometry to hybridization
Sigma and Pi Bonding
Molecular orbitals, bonding in diatomic molecules of second row elements
Bonding in aromatic compounds