Abstract
This article describes a descriptive-qualitative method for analyzing and reviewing several textbooks for high school as samples commonly used by teachers and students in their teaching–learning to reveal possible misconceptions. This study focused on the subjects of quantum numbers and electronic configuration. From the advanced literature review to analyze the samples the occurrence of various misconceptions was noted. All textbooks described correctly the four symbols of quantum numbers, but none correlates correctly the magnetic-angular quantum number to the Cartesian labeled orbitals. All textbooks consider mistakenly the meaning of aufbau as the building-up energy of orbitals by following (n + ℓ, n) rules on describing the electronic configuration for all atoms. Only one textbook states that the electronic configuration of transition metal atoms (3d series) can be described in the following order of shell (n), thus giving rise to two types of electronic configurations, [Ar] 3d 4s (Type I) beside [Ar] 4s 3d (Type II), leading further misconception. All textbooks described favorably an unpaired electron of ms = + ½ due to the specific agreement, which is a potential misconception in applying Hund’s rule. In drawing the diagram boxes of orbitals, they are arranged in increasing or decreasing the numeric mℓ, due to the specific agreement, and again leading to a potential misconception on describing the quantum number of electrons issued. Three textbooks introduced the terms of the last and the xth electron associated with the quantum numbers, leading to serious further misconceptions. No books stated that the ordering energy of the (n + ℓ, n) rule is true only for the first twenty atoms.
This is a preview of subscription content, log in via an institution to check access.
Similar content being viewed by others
References
Adamson, A.W.: Domain representations of orbitals. J. Chem. Educ. 42(3), 140–145 (1965). https://doi.org/10.1021/ed042p140
Becker, C.: Geometry of the f orbitals. J. Chem. Educ. 41(7), 358–360 (1964). https://doi.org/10.1021/ed041p358
Benigna, J.: Photoelectron spectroscopy in advanced placement chemistry. J. Chem. Educ. 91(9), 1299–1305 (2014). https://doi.org/10.1021/ed500021c
Bills, J.L.: Experimental 4s and 3d Energies in Atomic Ground States. J. Chem. Educ. 75(5), 589–593 (1998). https://doi.org/10.1021/ed075p589
Cardellini, L.: Chemistry: why the subject is difficult? Educ. Quim. 23, 305–310 (2012). https://doi.org/10.1016/s0187-893x(17)30158-1
Carpenter, A.K.: 4s, 3d, what? J. Chem. Educ. 60(7), 562 (1983). https://doi.org/10.1021/ed060p562
Chambers, W.J., Fitzpatrick, N.J.: The Electronic Structures and Stabilities of Hexacarbonylchromium and Nitrogenpentacarbonylchromium. Proc. R Irish Acad Sect. b: Biol. Geol. Chem. Sci. 71, 97–108 (1971). https://doi.org/10.2307/20518891
Day, M.C., Jr., Selbin, J.: Theoretical Inorganic Chemistry. Van Nostrand Reinhold Company, New York (1969)
Dewar, J., Jones, H.O.: The Physical and Chemical Properties of Iron Carbonyl. Proc. r. Lond. Ser. Contain. Pap. Math. Phys. Charact. 76(12), 558–577 (1905)
Friedman, H.G., Choppin, G.R., Feuerbacher, D.G.: The shapes of the f orbitals. J. Chem. Educ. 41(7), 354–358 (1964). https://doi.org/10.1021/ed041p354
Greenwood, N.N.: Principles of Atomic Orbitals, Revised The Royal Institute of Chemistry, London (1968)
Griffiths, A.K., Preston, K.R.: Grade-12 students’ misconceptions relating to fundamental characteristics of atoms and molecules. J. Res. Sci. Teach. 29(6), 611–628 (1992). https://doi.org/10.1002/tea.3660290609
Huheey, J.E.: Inorganic Chemistry, 3rd edn. Harper International SI Edition, London (1983)
IUPAC (1997) Compendium of chemical terminology, 2nd edn (the "Gold Book"), Compiled by A. D. McNaught and A. Wilkinson, Blackwell Scientific Publications, Oxford. Online version (2019) created by S. J. Chalk. https://doi.org/10.1351/goldbook
Keller, R.N.: Textbook Errors, 38, Energy level diagrams and extranuclear building of the elements. J. Chem. Educ. 39(6), 289–293 (1962). https://doi.org/10.1021/ed039p289
Kikuchi, O., Suzuki, K.: Orbital shape representations. J. Chem. Educ. 62(3), 206–209 (1985). https://doi.org/10.1021/ed062p206
Kim, H., Sefcik, J.S., Bradway, C.: Characteristics of qualitative descriptive studies: a systematic review. Res. Nurs. Health 40(1), 23–42 (2016). https://doi.org/10.1002/nur.21768
Ladell, J., Post, B., Fankuchen, I.: The crystal structure of nickel carbonyl, Ni(CO)4. Acta Crystallogr. A 5(6), 795–800 (1952). https://doi.org/10.1107/s0365110x52002148
Melrose, M.P., Scerri, E.R.: Why the 4s orbital is occupied before the 3d. J. Chem. Educ. 73(6), 498–503 (1996). https://doi.org/10.1021/ed073p498
Mondal, B.C., Chakraborty, A.: Misconceptions in Chemistry: Its Identification and Remedial Measures. LAP LAMBERT Academic Publishing, Saarbrücken (2013)
Nakhleh, M.B.: Why some students don’t learn chemistry: chemical misconceptions. J. Chem. Educ. 69, 191–196 (1992). https://doi.org/10.1021/ed069p191
Necor, D.C.: Conceptual understanding of students on electron configuration. Int. J. Sci. Res. 8(5), 336–342 (2019)
Nelson, P.G.: Relative energies of 3d and 4s orbitals. Educ. Chem. 29, 84–85 (1992)
NIST Atomic Spectra Database Ionization Energies Data. https://physics.nist.gov/PhysRefData/ASD/ionEnergy.html
NIST Basic Atomic Spectroscopic Data. https://physics.nist.gov/PhysRefData/Handbook/element_name.htm
Özkanbaş, M., Taştan Kirik, Ö.: Implementing collaborative inquiry in a middle school science course. Chem. Educ. Res. Pract. (2020). https://doi.org/10.1039/c9rp00231f
Pilar, F.L.: 4s is always above 3d! Or, how to tell the orbitals from the wave-functions. J. Chem. Educ. 55(1), 1–6 (1978). https://doi.org/10.1021/ed055p2
Portius, P., Bühl, M., George, M.W., Grevels, F.-W., Turner, J.J.: Structure and dynamics of iron pentacarbonyl. Organometallics 38(21), 4288–4297 (2019). https://doi.org/10.1021/acs.organomet.9b00559
Scerri, E.R.: Transition metal configurations and limitations of the orbital approximation. J. Chem. Educ. 66(6), 481–483 (1989). https://doi.org/10.1021/ed066p481
Schwarz, W.H.E.: Recommended questions on the road towards a scientific explanation of the periodic system of chemical elements with the help of the concepts of quantum physics. Found. Chem. 9(2), 139–188 (2006). https://doi.org/10.1007/s10698-006-9020-z
Schwarz, W.H.E.: The full story of the electron configurations of the transition elements. J. Chem. Educ. 87(4), 444–448 (2010). https://doi.org/10.1021/Ed8001286
Stewart, P.J.: From telluric helix to telluric remix. Found. Chem. 22, 3–14 (2020). https://doi.org/10.1007/s10698-019-09334-7
Sunyono, S., Tania, L., Saputra, A.: A learning exercise using simple and real-time visualization TOOL to counter misconceptions about orbitals and quantum numbers. J. Balt. Sci. Educ. 15(4), 452–463 (2016)
Temel, S., Özcan, Ö.: Students’ understanding of quantum numbers: a qualitative study. SHS Web Conf. 48, 01002 (2018). https://doi.org/10.1051/shsconf/20184801002
Vanquickenborne, L.G., Pierloot, K., Devoghel, D.: Transition metals and the Aufbau principle. J. Chem. Educ. 71(6), 469 (1994). https://doi.org/10.1021/ed071p469
Wang, S.G., Qiu, Y.X., Fang, H., Schwarz, W.H.E.: The challenge of the so-called electron configurations of the transition metals. Chem. A Eur. J. 12(15), 4101–4114 (2006). https://doi.org/10.1002/chem.200500945
Wang, S.-G., Schwarz, W.H.E.: Icon of chemistry: the periodic system of chemical elements in the new century. Angew. Chem. Int. Ed. 48(19), 3404–3415 (2009). https://doi.org/10.1002/anie.200800827
Wong, D.P.: Theoretical justification of Madelung’s rule. J. Chem. Educ. 56(11), 714–717 (1979). https://doi.org/10.1021/ed056p714
Yi, P.-F.: Letter to the editor. J. Chem. Educ. 24, 567 (1947)
Acknowledgements
The authors greatly thank for the funding support from the Faculty of Mathematics and Science, Yogyakarta State University.
Author information
Authors and Affiliations
Corresponding author
Ethics declarations
Conflict of interest
There is no conflict of interest to declare.
Additional information
Publisher's Note
Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.
Rights and permissions
Springer Nature or its licensor (e.g. a society or other partner) holds exclusive rights to this article under a publishing agreement with the author(s) or other rightsholder(s); author self-archiving of the accepted manuscript version of this article is solely governed by the terms of such publishing agreement and applicable law.
About this article
Cite this article
Sari, R.L.P., Pratomo, H., Yunita, I. et al. Misconception in chemistry textbooks: a case study on the concept of quantum number, electronic configuration and review for teaching material. Found Chem 25, 419–437 (2023). https://doi.org/10.1007/s10698-023-09475-w
Accepted:
Published:
Issue Date:
DOI: https://doi.org/10.1007/s10698-023-09475-w