___

• Amann, A. (1992). Must a molecule have a shape?, South African Journal of Chemistry, 45, 29–38.
• Brion, C.E., Cooper, G., Zheng, Y., Litvinyuk, L.V., & McCarthy, I.E. (2001). Imaging of orbital electron densities by electron momentum spectrsocopy—a chemical interpretation of the binary (e, 2e) reaction, Chemical Physics, 70, 13–30.
• Coskun, E. & Alkan, M. (2010). Evaluation of learning and teaching process in Turkish courses, International Electronic Journal of Elementary Education, 2, 3, 387-407.
• Dicks, A. P. (2011). Shake For Sigma, Pray For Pi: Classroom Orbital Overlap Analogies, Journal of Chemical Education, 88, 4, 426-427.
• French, S., Krause, D. (2006). Identity in Physics: A Historical, Philosophical and Formal Analysis. Oxford University Press, Oxford.
• Georgios, T. and Georgios, P. ( 2002). Quantum-Chemical Concepts: Are They Suitable For Secondary Students?, Chemistry Education: Research and Practice In Europe , 3, 2, 129-144.
• Grushow, A. (2011). Is i t Time to Retire the Hybrid Atomic Orbital?, Journal of Chemical Education, 88, 7, 860-862.
• Humphreys, C. J. (1999). Electron seen in orbit, Nature, 401, 49–52.
• Itatani, J., Levesque, J., Zeidler, D., Niikura, H., Pe´pin, H., Kieffer, J.C., Corkum, P.B., Villeneuve, D.M. (2004). Tomographic imaging of molecular orbitals, Nature, 432, 867–871.
• Jacoby, M. (1999). Picture-perfect orbitals, Chemical & Engineering News, 77, 36, 8-10.
• Jenkins, Z. (2003). Do you need to believe in orbitals to use them?: realism and the autonomy of chemistry, Philosophy of Science, 70, 1052–1062.
• Laurikainen, K.V., Montonen, C., Sunnarborg, K. (1994). Symposium on the Foundations of Modern Physics, Editions Frontieres.
• Kochen, S., Specker, E. (1967). The problem of hidden variables in quantum mechanics, Journal of Mathematics and Mechanics, 17, 59–87.
• Labarca, M., Lombardi O. (2005). The ontological autonomy of the chemical world, Foundations of Chemistry, 7, 125–48.
• Liegener, C.M., Del Re, G. (1987a). The relation of chemistry to other Şelds of science: atomism, reductionism, and inversion of reduction, Epistemologia, 10, 269–284.
• Liegener, C. M., Del Re, G. (1987b). Chemistry versus physics, the reduction myth, and the unity of science, Journal for General Philosophy of Science, 18, 1-2, 165–174.
• Litvinyuk, I.V., Zheng, Y., Brion, C. E. (2000). Valence shell orbital imaging in adamantane by electron momentum spectroscopy and quantum chemical calculations, Chemical Physics, 253, 41–50.
• Lombardi, O., Labarca, M. (2005). The ontological autonomy of the chemical world, Foundations of Chemistry, 7, 125–148.
• Lombardi, O., Labarca, M. (2006). The ontological autonomy of the chemical world: a response to Needham, Foundations of Chemistry, 8, 81–92.
• Matta, C.F., Gillespie, R.J. (2002). Understanding and interpreting molecular electron density distributions, Journal of Chemical Education, 79, 1141– 1152.
• Nakıpoğlu, C. (2003). Instructional Misconceptions Of Turkish Prospective Chemistry Teachers About Atomic Orbitals And Hybridization Chemistry Education, Research And Practice, 4, 2, 171-188.
• Ostrosky, V. N. (2005). Towards a philosophy of approximations in the ‘exact’ sciences. Hyle-Int, Journal of Chemical Education, 11, 101–126.
• Özden, M., (2007). Kimya Öğretmenlerinin Kimya Öğretiminde Karşılaştıkları Sorunların Nitel ve Nicel Yönden Değerlendirilmesi: Adıyaman ve Malatya İlleri Örneği, Pamukkale Üniversitesi Eğitim Fakültesi Dergisi, 22,2, 40-53.
• Pascual, J. I., Go´mez-Herrero, J., Rogero, C., Baro´, A. M., Sa´nchez-Portal, D., Artacho, E., Ordejo´ n, P., Soler, J. M. (2000). Seeing molecular orbitals, Chemical Physics Letters, 321, 78-82.
• Petrucci, H. R., Harwood, W. S. (1993). Genel Kimya: Prensipler ve Modern Uygulamalar. (Uyar, T. ve Aksoy, S., Çev.). Ankara: Palme Yayıncılık.
• Primas, H. (1983). Chemistry, Quantum Mechanics and Reductionism, Springer, Berlin.
• Primas, H. (1998). Emergence in exact natural sciences, Acta Polytech Scand, 91, 83–98.
• Scerri, E. R. (2000). Have orbitals really been observed?, Journal of Chemical Education, 77, 1492–1494.
• Scerri, E. R. (2001). The recently claimed observation of atomic orbitals and some related philosophical issues, Philosophy of Science, 68, 76–88.
• Schwarz, W. H. E. (2006). Measuring orbitals: provocation or reality?, Angewandte Chemie International Edition, 45, 1508–1517.
• Schwarz, W. H. E. (2006). Measuring orbitals: provocation or reality?,
• Angewandte Chemie International Edition, 45, 1508–1517.
• Spence, J. C., O’Keefe, M., Zuo, J. M. (2001). Have orbitals really been observed?, Journal of Chemical Education, 78, 877.
• Stefani, C., Tsaparlis, G. (2009). Students’ Levels of Explanations, Models, and Phenomenographic Study, Journal of Research in Science Teaching, 46, 520-536. in Basic Quantum Chemistry: A
• Tsaparlis, G., Papaphotis, G. (2009). High school students' conceptual difficulties and attempts at conceptual change: The case of basic quantum chemical concepts, International Journal of Science Education, 31, 895-930.
• Vemulapalli, G. K., Byerly, H. (1999). Remnants of reductionism, Foundations of Chemistry, 1, 17–41.
• Wang, S. G., Schwarz, W. H. E. (2000). On closed-shell interactions, polar covalences, d shell holes, and direct images of orbitals: the case of cuprite, Angewandte Chemie International Edition, 39, 1757–1762.
• Wooley, R. G. (1978). Must a molecule have a shape?, Journal of American Chemical Society, 100, 1073–1078.
• Wooley, R.G. (1982). Natural optical activity and the molecular hypothesis, Structure Bonding, 52, 1–35.
• Yam, P. (1999). Seeing the bonds, Scientific American, 281, 28.
• Zuo, J.M., Kim, M., O’Keefe, M., Spence, J.C.H. (1999). Direct observation of d-orbital holes and Cu–Cu bonding in Cu2O, Nature, 401, 49–52.
• Zurer, P. (1999). Chemistry’s top Şve achievements, Chemical & Engineering News, 77, 38–40. EK1:
• Aşağıda verilen eksenleri kullanarak 1s, 2p ve 3d orbitallerinin
• şekillerini çiziniz. ****