The symbolic algebra program Maple and the spreadsheet Microsoft Excel were used in an attempt to reproduce the Gaussian fits to a Slater-type orbital, required to construct the popular STO-NG basis sets. The successes and pitfalls encountered in such an approach are chronicled. C omputational chemistry, in particular, those based on ab initio quantum chemistry, has become a standard tool for many research groups and enjoys increasing use in the undergraduate curriculum. 1 One of the choices that must be made when employing these techniques is that of basis set, which is a set of functions, centered on the nuclei, which when taken as a linear combination comprise the molecular orbitals. It is this author's experience that the majority of students employing computational chemistry do not really comprehend the nature of a basis set (other than as something specified in an input file necessary to run a calculation) nor the effort required to construct them. Standardized basis sets have become common in the practice of computational chemistry. One of the most common, the STO-NG basis set, was developed over 40 years ago for the atoms H and Li through F. 2 Soon thereafter, the basis sets were extended to He, Ne, and Na through Ar. 3 Further extension of these basis sets did not come until a decade later, when basis sets for K, Ca, and Ga through Kr; 4 Rb, Sr, and In through Xe; 5 and Sc through Zn and Y through Cd 6 were published, at which point the development of the STO-NG series of basis sets appears to have stopped. One of the purposes of this article is to delineate, in part, how the STO-NG basis sets are constructed.Although few research groups use the STO-NG basis sets nowadays in production calculations, their historical importance, simple construction and efficiency of calculation makes them valuable as tools in chemical education. The most commonly used of these is the STO-3G basis set, as illustrated by the following examples. The atomic charges and dipole moments for the isoelectronic first-row hydrides and the atomic charges of their protonated forms were calculated by Greenberg, Liebman, and co-workers in a discussion of how they relate to concepts such as acidity and proton affinity. 7 The changes of the bonding σ orbital in hydrogen fluoride as a function of bond distance are illustrated by Lipkowitz. 8 The optimized bond lengths for the interstellar molecules HC 2n+1 N, n = 1−7, have been calculated by a Spanish collaboration. 9 The use of common programs to reproduce some of the very early calculations on hydrogen molecule has been espoused by Duke and O'Leary. 10 The same authors also criticize the indiscriminate use of simple molecular orbital theory to discuss the orbital energy diagram of the first-row homonuclear diatomic molecules, especially for dinitrogen. 11 Ben-Amotz and co-workers showed that, for the set of molecules cis-and trans-dichloroethene, and for methanol and methanol-d 1 , application of the scaling factor 0.8246 for the HF/STO-3G vibrational frequencies resulted in a root-mean-...