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

Avogadro's Number

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