Exam #1 concept sheet

Disclaimer—THIS IS NOT EXHAUSTIVE BUT IS JUST A GUIDE

Watch for updates—this is in progress!

_{DON’T FORGET YOUR PENCIL AND CALCULATOR}

Chapter 1 & Appendices 1 & 2  

Significant figures

Scientific notation

SI units

Prefixes and power-of-ten meanings (esp. mega, kilo, centi, milli, micro, nano, pico)

Conversion and word problems

Chapter 2     

Subatomic particles

Elements (definition, properties, trends, etc.)

“Atom building” and nuclide notation (^A_ZX^C)

Periodic table

             —atomic numbers and mass numbers

             —column and periods

             —column numbers and family names

             —metals, nonmetals, and metalloids

             —main group, transition metals, and inner transition metals (lanthanides & actinides)

Isotopes (definition, identification, contributions to average atomic mass, etc.)

Ions

             —definition

             —likely charges on ions formed by different atoms

             —names and charges (use the common ion sheet to help—memorize this, please)

Compounds (definition, properties, trends, etc.)

             —ionic and covalent

             —names and formulas (watch—ionic rules different than covalent)

             —percent composition

Some important follow-up points on Chapter 2:

             —There is a periodic repetition of similar properties among the elements (“periodic table”).

             —Elements in columns show similarities in their reactivity/behavior.  The electron arrangement (count) is a  key factor.

             —Elements naturally exist in different forms – for example:

             large collections of atoms (e.g., metals),

             single atoms (e.g., noble gases),

             molecules (e.g., the halogens),

             extended networks (e.g. diamond – carbon),

             etc.

             —Seven elements naturally exist as diatomic molecules – think HOFBrINCl:

             H₂, O₂, F₂, Br₂, I₂, N₂, and Cl₂

             —Most substances that are encountered in nature are not pure elements but are combinations (compounds).

             —The main group elements show quite predictable chemical behavior; the transition metals and inner transition metals are less predictable (more similarities among the columns than main group).

Chapter 3     

The mole

Compounds

             —molar masses

             —percent composition; empirical and molecular formulas

Reactions (reading, balancing, etc.)

Stoichiometry for reactions

             —theoretical amounts needed or produced

             —limiting reactant problems

             —theoretical and actual yields; percent yields

Good luck and try not to stress out!