Printer Friendly

Analysis and Validation of Dipole Moment Calculations in Chemistry Teaching.


The attitude of the students is generally recognized as an important factor in the success of the learning process. This is particularly true in the case of the chemistry, in which some topics are inherently difficult, and methods of traditional teaching have focused their learning process in the transmission of knowledge (teacher dictates the content and the student "learns" writing). Quantum chemistry, in general, is not commonly well appreciated by high school students, so little in higher education [1, 2] and perhaps one of the aspects that takes this discipline to be considered as one of the toughest in the practice of teaching.

Enhancing students' understanding of chemistry concepts has been a major goal of researchers in Chemistry Teaching during the last decades. One of the resources that has been used since the 1960s as a tool for learning is the computer [3]. In 1972, in the University of Lancaster, England, chemical B. J. Duke organize a course in Quantum Chemistry in order to motivate the introduction of computational techniques in chemistry teaching [4]. In their experiment, Duke used a program to calculate the properties of aromatic compounds by the quantum chemistry molecular orbital methods described in the Mulliken Theory. In 1988, in the University Chemical Laboratory Cambridge, United Kingdom, Colwell and Handy were using computers as a teaching tool for Molecular Orbital Theory [5]. Other researchers have also worked with the use of computers in Chemistry Teaching, enabling the computational chemistry definitely conquer its place among the methodologies that investigate chemical phenomena [6-8].

In an attempt to recognize limitations of the traditional form of teaching chemistry, both in high school and higher education, it has been proposed several methodological alternatives. In this sense, new teaching materials were developed. One of the main objectives of these methods and materials alternative is to promote a more participatory attitude of students in their learning process. It is crucial that students learn how to construct, decode and use structural representations early in a sequence of chemistry courses, otherwise much of what follows will simply be an exercise in memorization [9].

In this paper, we present an alternative proposal to the understanding and interpretation of the dipole moment of diatomic molecules, present content in the curriculum of physical chemistry and quantum chemistry disciplines in undergraduate chemistry courses.

Teaching computational chemistry

Curriculum of physical chemistry undergraduate is traditionally built around the themes of thermodynamics, quantum mechanics, molecular spectroscopy, electrochemistry and chemical kinetics. The Quantum Chemistry teaching still represents a challenge to chemistry students, due to the novelty of the abstract concepts and to the quantity calculations involved [10]. However, the use of computational quantum chemistry has been widely considered in the understanding of various issues of chemistry (Analytical, Inorganic, Organic, Physical Chemistry, Environmental Chemistry, Food Chemistry etc.) and can be attractive for students correlating their areas. Quantum computational chemistry is an inherently multidisciplinary field of study that transcends the traditional barriers separating chemistry, biology, physics and mathematics [8]. Thus, computational chemistry is a perfect tool to make the interconnections between chemistry and other sciences.

Computational chemistry is commonly presented in chemistry courses graduation in physical chemistry disciplines and focus generally on basic theory, including the wave-particle behaviour and the resolution of the Schrodinger equation for simple systems that can be evaluated analytically. As defined by IUPAC, Computational chemistry is a discipline using mathematical methods for the calculation of molecular properties or for the simulation of molecular behaviour. It also includes, e.g., synthesis planning, database searching, combinatorial library manipulation [11]. Specially as regards the molecular models, role of the computational chemical is, together with the statistical thermodynamics, language integration and chemical concepts, allowing the interpretation and rationalization of macroscopic properties for reasons at atomic-molecular level [12-16].

In this sense, computational Chemistry content graduation can be considered as complex for the understanding of the student, due to the need to comprehend abstract concepts that are largely non-intuitive, and advanced mathematical concepts, such as linear algebra and differential and Integral Calculus. Johnson and Engel published in 2011 the results of a two-year job at a major university on the integration of computational chemistry in physical chemistry curriculum of undergraduate courses [17]. Use of teaching methods in chemistry and physics has been studied at different levels of education, and research [18] shown few studies have focused on the impact of interest to teachers about their choice of teaching methods. Furthermore, the chemistry education community has paid little attention to determining discipline-specific aspects of chemistry that can lead to learning difficulties and misconceptions [19].

Dipole moment

As is known, an electric dipole ([micro]) is a vector which is characterized in the direction between two electrical charges, towards +q to -q and module given by the distance d between them [16,20]:

[mu] = q x d (1)

Pauling [20] describes that a molecule has electric dipole moment if its center of positive charge does not coincide with its center of negative charge. That is, the vector of the molecular dipole is given by [delta].r, being [delta] partial atomic charge and r the bond distance (Figure 1).

Dipole moments values can be determined with great accuracy by microwave spectroscopy and molecular resonance methods [20]. The coulombic model describes dipole moments of binary hydrides as the resultant of the dipolar contributions of the hydride ions and the electron pairs around the positively charged central atom [21]. Basically, what defines a molecule as a whole is polar or non-polar is the disposition of its bonds; for highly symmetric molecules, the resulting dipole should be null. For a molecule with more than two atoms, the dipole moment depends of the size of polarities of individual bonds as well as of the molecule geometry. The bond dipoles and the dipole moments are vector quantities. The total dipole polyatomic a molecule is the sum of their bond dipoles. When total dipole of the molecule is "zero", even if the bonds are polar, the geometry of the molecule imposes that total dipole moment is zero, makes the molecule is non-polar. Already if the molecule have a dipole moment of total nonzero, the molecule is polar. Although the international system unit of dipole moment is the coulomb meter (Cm), it is still common to use of the Debye (D) unit (1 Debye = 3.336x[10.sup.-30] C.m), in homage to Peter Debye, pioneer of experimental investigation of the dipole moments of the molecules [22].

All heteronuclear diatomic molecules are polar, single or multiple bonds are formed between the A and B atoms, the dipole moment of the AB molecule is related to the polar character of the bonding, the dipole moment of the bond itself is the molecular dipole moment. In the case of polyatomic molecules, the vector sum of the bond dipoles resulting in the total dipole [23] (figure 2).

In first approximation, the dipole moment of a triatomic molecule may be solved by the technique of vector addition that describes the resulting dipole [micro]res of the sum of two dipole moments [[mu].sub.1] and [[mu].sub.2] that make between them an angle [theta] given by Equation 2.

[[mu].sub.res] = [([[mu].sup.2.sub.1] + [[mu].sup.2.sub.2] + 2[[mu].sub.1][[mu].sub.2] cos[theta]).sup.1/2] (2)

When the two dipole moments are equal, Equation 2 is simplified:

[[mu].sub.res] = [[mu].sub.1](1 + cos[theta]) [square root of (2)] (3)

One difficulty for calculating dipole moments should the positions and magnitudes of partial charges used in the molecule [16]. In this sense, quantum chemistry arises as an ally to teaching and research in the calculation of partial charges, which are included in the output of many computer packages molecular structure calculations. Knowing the charge density qi on each atom and the bond distances, we can calculate the dipole moment. First, the charge density of each atom is represented as a vector of length qi of the some arbitrary origin in the direction of the atom i. If the vector is collinear with a bond and the origin is an atom, the vector represents a moment dipole bond. All vectors not need represent dipole moments of bond, because they do not need be all collinear with the bond [23]. When vectors represent all the charge densities, the vector sum is the total dipole moment. Table 1 describes some experimental values [24-26] of the dipole moment for molecules used in our survey.

A program widely used in the visualization in quantum chemistry calculations is the GaussView [27]. The dipole moment can be observed through of the menu "Results" in the option "Summary" (Figure 3) or on the output file.

Molecule dipole module used in the example has a value of 1.9819 D.


Proposed method to dipole moment calculation

Partial ionic nature of chemical bonds and their relationship with the dipole moment has been understood since the 1930s in the pioneering work of Linus Pauling [28]. He supposed that a bond between two identical atoms could be considered a covalent bond; already in the bond between different atoms, one atom is more electronegative than the other, so the covalent character not is more one hundred percent, then the bond must have an ionic contribution. Thus, it sets the ionic character (CI) of a bond (Equation 4).

[mathematical expression not reproducible] (4)

where [DELTA][chi] is the Pauling electronegativity difference [20,29,30] between the bonded atoms ([DELTA][chi] = [chi]A - [chi]B). From this, Pauling [29] proposed that the ratio of the experimental electric dipole moment and calculated dipole moment (assuming that the binding was completely ionic) would give %CI real of a polar covalent bond (Equation 5).

%CI = 100 ([[mu].sub.exp]/[[mu].sub.calc]) (5)

With this equation, we have a kind of experimental ionic character. However, we cannot have a dipole moment calculation that is completely analytical and theoretical.

We developed a proposal for calculations of the dipole moment of form alternative to the computational methods of quantum chemistry. Initially we solved the problem of calculating the charge of the dipole from the ionic character defined by Pauling (Eq. 4). We propose that the charge of the dipole ([delta]) can be given by the ionic character product Pauling (Eq. 4) by the elementary charge, ([mathematical expression not reproducible]) 1.602x[10.sup.-19] C. It is usually difficult to find analytical expressions that university students use to estimate bond distances. Once again we took the opportunity to stand out also an expression developed by Pauling [31,32]. We can with this, perform the calculation of the bond distance (r) in a systematic form:

r = [R.sub.A] + [R.sub.B] - 0.6log n (6)

where [R.sub.A] and [R.sub.B] are respectively the radii of the atoms A and B, n is the bond type (for single, double and double-resonant bond, respectively, n = 1, 2 and 1.5). We have reached an expression that uses only the atomic radii as empirical data:

[mathematical expression not reproducible] (7)

We use the analytical proposal (Equation 7), results of computational quantum chemistry and experimental data to develop this work with university students, through a critical analysis of the results (which included opinion survey). We can make a comparison separately, between greatness bond distances, charge and dipole, for analytical calculation, computational and experimental data.

Context of the study and method

Main objective was to investigate and treat perceptions of students about a new proposed analytical method for dipole moment calculation in chemistry teaching. Responses are grouped into categories that reflect different perceptions of students: analytical prediction; computational prediction and; and inaccuracy in the results data.

Development of this study followed the molds of a qualitative research. Among the main features that set qualitative research, Creswell [33] identifies the following: Qualitative research uses the natural environment as a direct source of data and the researcher as its main instrument; data collected is predominantly descriptive; meaning people attribute to things and their lives are in the research focus of attention; analysis the data tend to follow an inductive process. Research was conducted by the authors of this article and has been reviewed and revised by experts for its content validity. Eighty-seven (87) students of the degree course in chemistry at a university in Brazil participated. Ages of students varies 17-30 years old and these belonged to three classes in which each consisted of 32, 30 and 25 students. Data from this study were collected in 2015 and 2016 by means of a questionnaire. For students of the second semester of 2015 (32 students), we have named as Class A. For of the first semester 2016 (30 students) as Class B and for students of the second semester of 2016 (25 students) as Class C. It stands out that the students involved in this research attended the same discipline, which is given every semester in the course.

Our pedagogical approach used computational and analytical technique to describe the dipole moment of simple molecules. To evaluate this approach the questionnaire included two questions:

1[degrees]) Calculate the dipolar molecules (HF, HCl, HBr, HI, LiF, LiCl, LiBr, LiI, NaF, NaCl, NaBr, NaI, KF, KCl, KBr, KI, CsCl, HO, NO and SO).

2[degrees]) Of the values found, what would you use in your research? Justify.

The answers are presented as written by the participants, preserving typos, text writing errors, conceptual errors, etc. Names were removed and data that could identify subjects.


Assessment of students' perceptions

Aiming to analyze the students' perception of the dipole moment, analytical and computational calculations were performed. Students were invited to discuss the importance of the results, comparing them with the analytical, experimental and computational results.

Experimental Data ([[mu].sub.exp])

Dipole moment of the molecules analyzed were experimentally described in Table 1, according to data presented in the literature [24-26].

Analytical Prediction ([[mu].sub.a])

Using equation 7 for the calculation of what we call analytical dipole moment ([[mu].sub.a]), the values found by the students to the first question of the questionnaire are described in Table 2.

Students use to calculate the distance between molecules, data from the atomic radius and electronegativity found by Pauling [20,2 9-31].

Computational Prediction ([[mu].sub.c])

Hoffmann, Schleyer and Schaefer [34] already warned that studies involving calculations of molecules for which no experimental evidence is yet available were growing very rapidly. The authors suggested that the computations performed be described in a circumspect way [34]. One of the electronic structure calculation methods atoms, molecules and solids, with currently most successful is the Density Functional [11]. Density Functional Theory (DFT) is a theory that deals with the quantum mechanical description of molecular systems in terms of the electronic density. Dipole moments were calculated by Kohn-Sham density functional theory. Although the calculation of the electric dipole is still a challenge, even bigger than the calculation of molecular geometries, Kohn-Sham density functional theory was well validated against experimental results for dipole moments and it is known for giving acceptably accurate dipole moments [35-38].

For the study was performed an optimization of the molecules and DFT method [39,40] was used together with the B3LYP hybrid functional [41,42] defined as:

B3LYP = 0,20Ex(HF) + 0,80Ex(Slater) + 0,72DEx[(B88).sup.GGA] + 0,19Ec[(VWN).sup.LDA] + 0,81DEc[(LYP).sup.GGA]

where Ex is the exchange energy Ec is the correlation energy, and HF, B88, VWN, LYP are the Hartree-Fock, Beck [43], Vosko-Wilk-Nusair [44], and the Lee-Yang-Parr [41] terms, respectively. The LYP term gives the local and the non-local correlations, whereas excess of the local correlation is given by the VWN term [45]. Although the extremely popular B3LYP functional is implemented in the Gaussian programs differently than Becke intended [34,46]. Basis set of Pople 6-311++g(d,p) was chosen to be used with the computational method already described [47]. Basis set is frequently used in various systems, because it includes polarization functions and diffuse, besides of dividing the valence shell improves the results when compared to the other sets minimum bases. This basis set has proved suitable to describe the molecules.

Through this method, the students found the values for which we denote by computational dipole moment ([[mu].sub.c]). This step was important to approximate the theoretical chemistry software to the reality of students, so that they themselves take ownership of this technology. We use the descriptors "accuracy" and "precision" that are well-defined in the computer-based world of the quantum chemist, according to Hoffmann, Schleyer and Schaefer [34].

Accuracy in predicting the data

Results of analytical calculation carried out by the students are compared with the computational and experimental data (Table 3), contributing to the validation of our technique.

Data in Table 3 show analytical calculations obtained, in their majority, present accuracy of better than 90% and in the computational calculations, the results show accuracy above 75%. We also note that only one (HF) of the analytical calculations showed the percentage of precision below 60%, which indicates a degree of confidence to discussions on the dipole moment. Figure 4 shows a summary of these data.

We can say that study of the dipole moment, of diatomic molecules, beyond the experimental data found in the literature, the use of computational and analytical methods could contribute to the understanding of their properties.

Student's assessment in relation to data

As regards the second question of the questionnaire (Of the values found, what would you use in your research? Justify.) We present some answers these students.

One student reports differences between the methods and suggests that the analytical dipole moment is the most suitable for their research: "As there was a very significant difference from the real value of the molecule, the value that most closely approximates the real value, and that would bring more security in the approximation of the desired result, would be calculated by the dipole moment of the ionic character".

This opinion is perceived in other students "I would use the analytical because it is closer to the experimental value" and "the value of the GaussView gave 10.9234 D, while the analytical value done by the dipole moment gave 10.368 D. So would use in my research the analytical value that was 10.368 D." referring to KCl molecule.

Figure 5 summarizes the results obtained comparing the answers of students, in which it describes that the analytical method may be the most suitable for use in the calculation of the dipole moment.

Choice of the analytical method (71.26% of students) possibly identifies a Cartesian feature; the value that most closely approximates the actual value should be considered the "most effective", as highlighted by one of the students: "In a survey, it would use the value that had a smaller margin of error in relation to the experimental value given".

Many of the answers found for the choice of the analytical method, present in common the described by these two students: "I would use the analytical value, because it is closer to the experimental value" and "I'd use the analytical value, it is nearest the experimental value", confirming a view that the closer to the actual value, better is the method.

As regards the answers of students considering the computational method as the most suitable for use in their research (19.54% of students), we highlight the following affirmations: "I'd use the computer, because the computer performs calculations better" and "the Gaussian is a program specially created to carry out chemical calculations on the computer, so it has the best results". In these affirmations, we see the appreciation of the use of computers as "the machines that solve all our problems". Nevertheless, we cannot think that is just use the computer that all our problems will be solved [11].

Already a small group of students reported they would use only the experimental value (9.19% of students), because for these the analytical and computational methods have different values of the actual value. One of those students says "calculations by Gaussian or analytical aren't accurate in relation to the experimental because the molecules depend on several factors about experimental, therefore in some the values are different, thus in some substances uses Gaussian and others analytical".

For this student the fact of having to use a method for a particular molecule and another method for another molecule, makes with that the use of the experimental data are more effective in their research. Such reflection is seen in another student response, in which he described that "I would use in my research the experimental value, because the percentage of error is very small comparing the two values". In this sense, we can consider that for these students only results obtained experimentally are correct, in their opinion no other method can be used as an approximation of the actual value.

We observed that, unfortunately, most of the students gave little importance to the experimental result. Laboratory work is an established part of courses in chemistry in higher education. Reid and Shah [48] argue that the experimental activities need to be reconsidered at higher education levels. They describe that there is a need for clarification of aims and objectives, and these need to be communicated to learners. In addition, seeing the activities in the laboratory in the context of what goes on before and after, as well as other learning, will enhance the learning potential. There is a need to prepare students for use of the laboratory as well as develop follow-up activities. These may enrich and enhance the whole laboratory experience, and enable it to contribute more effectively to the overall learning of students in chemistry [48].

Lastly, in relation the class, we obtained a positive evaluation for the use of the analytical method, being identified in all of them. Students of Class A (65.6%) consider that the analytical method is most suitable for use in their academic research. For Classes B and C the percentage is higher, 70% and 84% respectively. However, is interesting to note that some students (12.6% of class A; 10% of class B and; 4% of class C) considered the experimental value as the best to use in their calculations, without questioning how the data was obtained experimentally, this is, what the method used to obtain the values.

Worth mentioning, that the proposed method was valid in our survey, in which students consider it more appropriate to perform in their research. Although, we cannot ignore other factors that may have led to these students opting for the analytical method, such as: difficulty in handling computer programs, distrust of computational results, little contact with lab activities, reliability in mathematical calculations--as they performed the mathematical calculations, they believe that are more accurate.


Aim of this study was to present a new approach for the calculation of the dipole moment. This new approach can help students understand how an analytical method can predict physical properties of a molecule and interpreting your accuracy in relation to the experimental data. Admitted, this work opens up a new perspective on didactic strategies for the quantum chemistry teaching and can be used as a pedagogical tool [17,49].

We have extensively tested our approach with different molecules, and it is too early to draw definitive conclusions about the real impact that this new approach can cause in teaching quantum chemistry and physical chemistry, it is evident that all its features are susceptible of application to the daily work of teachers and students. However, it is believed that the results obtained in this study highlights the educational potential of using didactic strategies for analysis and interpretation of dipole moments.


The authors would like to thank Rural Federal University of Pernambuco, the research group LEUTEQ, and our students that inspire us to find effective ways to teach.


[1] Simpson, R. D.; Oliver, J. S. Sci. Educ. 1990, 74, 1. [CrossRef]

[2] Gibson, H. L.; Chase, C. Sci. Educ. 2002, 86, 693. [CrossRef]

[3] Suppes, P.; Morningstar, M. Science 1969, 166, 343. [CrossRef]

[4] Duke, B. J. J. Chem. Educ. 1972, 49, 703. [CrossRef]

[5] Colwell, S. M.; Handy, N. C. J. Chem. Educ. 1988, 65, 21. [CrossRef]

[6] Varnek, A. A.; Dietrich, B.; Wipff, G.; Lehn, J.-M.; Boldyreva, E. V. J. Chem. Educ. 2000, 77, 222. [CrossRef]

[7] Hessley, R. K. A. J. Chem. Educ. 2004, 81, 1140. [CrossRef]

[8] Lipkowitz, K. B.; Jalaie, M.; Robertson, D.; Barth, A. J. Chem. Educ. 1999, 76, 684. [CrossRef]

[9] Underwood, S. M.; Reyes-Gastelum, D.; Cooper, M. M. Chem. Educ. Res. Pr. 2016, 17, 365. [CrossRef]

[10] Leal, R. C.; Neto, J. M. M.; Lima, F. D. C. A.; Feitosa, C. M. Quim. Nova 2010, 33, 1211. [CrossRef]

[11] Leite, B. S. Tecnologias no ensino de quimica: teoria e pratica na formacao docente, 1st ed., Appris, Curitiba, 2015.

[12] Pauling, L.; Wilson Jr, E. B. Introduction to Quantum Mechanics: with applications to Chemistry, Dover Publications, Inc., New York, 1935.

[13] Szabo, A.; Ostlund, N. S. Modern Quantum Chemistry: introduction to advanced electronic structure theory, Dover, New York, 1989.

[14] Cramer, C. J. Essentials of Computational Chemistry: Theories and Models, 2nd ed., Wiley, 2004.

[15] Arroio, A.; Honorio, K. M.; Weber, K. C.; Homem-deMello, P.; Silva, A. B. F. Quim. Nova 2005, 28, 360. [CrossRef]

[16] Atkins, P. W.; Paula, J.; Friedman, R. Quanta, matter, and change: a molecular approach to physical chemistry, Oxford University Press, Oxford, 2009.

[17] Johnson, L. E.; Engel, T. J. Chem. Educ. 2011, 88, 569. [CrossRef]

[18] Herranen, J. K.; Vesterinen, V-M.; Aksela, M. K. Chem. Educ. Res. Pr. 2015, 16, 408. [CrossRef]

[19] Tumay, H. Chem. Educ. Res. Pr. 2016, 17, 229. [CrossRef]

[20] Pauling, L. General Chemistry, 3rd ed., Dover Publications, Inc., New York, 1988.

[21] Sacks, L. J. J. Chem. Educ. 1986, 63, 373. [CrossRef]

[22] Debye, P. Ann. Phys. 1912, 344, 789. [CrossRef]

[23] Rogers, D. W. Computational Chemistry Using the PC, 3rd ed., John Wiley & Sons, Inc., New Jersey, 2003.

[24] Bottcher, C. J. F; Bordewijk, P. Theory of Electric Polarization, Vol. II: Dielectrics in time-dependent fields, Elsevier, Amsterdam, Oxford, New York, 1978. [CrossRef]

[25] Nelson, R. D. J.; Lide, D. R. J.; Maryott, A. A. Selected Values of Electric Dipole Moments for Molecules in the Gas Phase. Washington, D.C.: U.S. Dept. of Commerce, National Bureau of Standards, 1967. [Link]

[26] Hebert, A. J.; Lovas, F. J.; Melendres, C. A.; Hollowell, C. D.; Story Jr., T. L.; Street Jr., K. J. Chem. Phys. 1968, 48, 2824. [CrossRef]

[27] Frisch, M. J.; Trucks, G. W.; Schlegel, H. B.; Scuseria, G. E.; Robb, M. A.; Cheeseman, J. R.; Montgomery Jr., J. A.; Vreven, T.; Kudin, K. N.; Burant, J. C.; Millam, J. M.; Iyengar, S. S.; Tomasi, J.; Barone, V.; Mennucci, B.; Cossi, M.; Scalmani, G.; Rega, N.; Petersson, G. A.; Nakatsuji, H.; Hada, M.; Ehara, M.; Toyota, K.; Fukuda, R.; Hasegawa, J.; Ishida, M.; Nakajima, T.; Honda, Y.; Kitao, O.; Nakai, H.; Klene, M.; Li, X.; Knox, J. E.; Hratchian, H. P.; Cross, J. B.; Adamo, C.; Jaramillo, J.; Gomperts, R.; Stratmann, R. E.; Yazyev, O.; Austin, A. J.; Cammi, R.; Pomelli, C.; Ochterski, J. W.; Ayala, P. Y.; Morokuma, K.; Voth, G. A.; Salvador, P.; Dannenberg, J. J.; Zakrzewski, V. G.; Dapprich, S.; Daniels, A. D.; Strain, M. C.; Farkas, O.; Malick, D. K.; Rabuck, A. D.; Raghavachari, K.; Foresman, J. B.; Ortiz, J. V.; Cui, Q.; Baboul, A. G.; Clifford, S.; Cioslowski, J.; Stefanov, B. B.; Liu, G.; Liashenko, A.; Piskorz, P.; Komaromi, I.; Martin, R. L.; Fox, D. J.; Keith, T.; Al-Laham, M. A.; Peng, C. Y.; Nanayakkara, A.; Challacombe, M.; Gill, P. M. W.; Johnson, B.; Chen, W.; Wong, M. W.; Gonzalez, C.; Pople, J. A.; Gaussian 03, Revision B.03, Gaussian, Inc., Pittsburgh, 2003.

[28] Pauling, L. J. Am. Chem. Soc. 1932, 54, 3570. [CrossRef]

[29] Pauling, L. The chemical bond and the structure of molecules and crystals: an introduction to modern structural chemistry, 3rd ed., Cornell University press, New York, 1960.

[30] Allred, A. L. J. Inorg. Nucl. Chem. 1961, 17, 215. [CrossRef]

[31] Pauling, L. J. Am. Chem. Soc. 1947, 69, 542. [CrossRef]

[32] Pauling, L. J. Phys. Chem. 1952, 56, 361. [CrossRef]

[33] Creswell, J. W. Research design: qualitative, quantitative, and mixed methods approaches, 4th ed., SAGE Publications, London, 2014.

[34] Hoffmann, R.; Schleyer, P.; Schaefer, H. P. Angew. Chemie Int. Ed. 2008, 47, 7164. [CrossRef]

[35] Wang, J.; Eriksson, L. A.; Johnson, B. G.; Boyd, R. J. J. Phys. Chem. 1996, 100, 5274. [CrossRef]

[36] Scheiner, A. C.; Baker, J.; Andzelm, J. W. J. Comput. Chem. 1997, 18, 775. [CrossRef]

[37] Prezhdo, O. V. Adv. Mater. 2002, 14, 597. [CrossRef]

[38] Duanmu, K.; Truhlar, D. G. J. Phys. Chem. C. 2014, 118, 28069. [CrossRef]

[39] Kohn, W.; Sham, L. J. Phys. Rev. 1965, 140, A1133. [CrossRef]

[40] Duarte, H. A.; Rocha, W. R. Teoria do Funcional da Densidade, In: Morgon, N. H.; Coutinho, K. (Eds.), Metodos Quimica teorica e Modelagem Molecular. Sao Paulo: Livraria da Fisica, 2007.

[41] Lee, C.; Yang, W.; Parr, R. G. Phys. Rev. B. 1988, 37, 785. [CrossRef]

[42] Becke, A. D. J. Chem. Phys. 1993, 98, 1372. [CrossRef]

[43] Becke, A. D. Phys. Rev. A. 1988, 38, 3098. [CrossRef]

[44] Vosko, S. H.; Wilk, L.; Nusair, M. Can. J. Phys. 1980, 58, 1200. [CrossRef]

[45] Leite, B. S.; Bastos, C. C.; Pavao, A. C. J. Mol. Model. 2016, 22, 295. [CrossRef]

[46] Hertwig, R. H.; Koch, W. Chem. Phys. Lett. 1997, 268, 345. [CrossRef]

[47] Hariharan, P. C.; Pople, J. A. Theor. Chim. Acta. 1973, 28, 213. [CrossRef]

[48] Reid, N.; Shah, I. Chem. Educ. Res. Pract. 2007, 8, 172. [CrossRef]

[49] Leite, B. S. Revista Brasileira de Informatica na Educacao 2014, 22, 55. [CrossRef]

Cristiano Costa Bastos (a), and Bruno Silva Leite * (b)

(a) Universidade Federal Rural de Pernambuco, Departamento de Quimica, Rua Dom Manoel de Medeiros, s/n, Dois Irmaos, CEP: 52171-900, Recife, PE, Brasil.

(b) Universidade Federal Rural de Pernambuco, Unidade Academica de Serra Talhada. Av. Gregorio Ferraz Nogueira, CEP: 56909535, Serra Talhada, PE, Brasil.

* Corresponding author. E-mail:

Article history: Received: 15 June 2017; revised: 29 September 2017; accepted: 13 October 2017. Available online: 25 December 2017. DOI:

Caption: Figure 1. Vector representation of the dipole moment.

Caption: Figure 2. Vector representation of the dipole moment of the water molecule.

Caption: Figure 3. Summary to the HF molecule visualized in the GaussView.
Table 1. Experimental dipole moment ([[mu].sub.exp]).

Molecule   [[mu].sub.exp]   Molecule   [[mu].sub.exp]

HF            1.820 D         NaBr        9.118 D
HCl           1.080 D         NaI            --
HBr           0.827 D          KF         8.558 D
HI            0.448 D         KCl         10.239 D
LiF           6.284 D         KBr         10.603 D
LiCl          7.130 D          KI            --
LiBr          7.226 D         CsCl        10.421 D
LiI            7.43 D          HO         1.660 D
NaF           8.160 D          NO         0.153 D
NaCl          9.000 D          SO         1.550 D

Table 2. Dipole moment values calculated analytically.

Molecule       [[mu].sub.a]

HF               3.071 D
HCl              1.505 D
HBr              1.078 D
HI               0.411 D
LiF              8.140 D
LiCl             7.508 D
LiBr             7.191 D
LiI              6.293 D
NaF              9.584 D
NaCl             8.767 D
NaBr             8.381 D
NaI              7.351 D
KF               11.743 D
KCl              10.809 D
KBr              10.368 D
KI               9.211 D
CsCl             12.115 D
HO               1.822 D
NO               0.202 D
SO               1.292 D

Table 3. Values of the dipole moment (in Debye) and
accuracy percentage (A%).

Molecule   [[mu].sub.exp] (a)   [[mu].sub.c]    A%

HF               1.820             1.981       91.11
HCl              1.080             1.403       70.09
HBr              0.827             1.082       69.06
HI               0.448               --         --
LiF              6.284             6.360       98.78
LiCl             7.130             7.087       99.39
LiBr             7.226             7.207       99.74
LiI               7.43               --         --
NaF              8.160             8.250       98.89
NaCl             9.000             9.019       99.77
NaBr             9.118             9.068       99.46
NaI              8.558             8.688       98.47
KF               10.239            10.583      96.63
KCl              10.603            10.923      96.98
KBr              10.421              --         --
KI               1.660             1.831       89.66
CsCl             0.153             0.098       64.11
HO               1.550             1.786       84.72
NO               1.820             1.981       91.11
SO               1.080             1.403       70.09

Molecule   [[mu].sub.a]    A%

HF            3.071       31.25
HCl           1.505       60.64
HBr           1.078       69.53
HI            0.411       97.11
LiF           8.140       70.45
LiCl          7.508       94.70
LiBr          7.191       99.52
LiI           6.293       84.70
NaF           9.584       82.54
NaCl          8.767       97.42
NaBr          8.381       91.92
NaI           11.743      62.78
KF            10.809      94.43
KCl           10.368      97.79
KBr           12.115      83.74
KI            1.822       90.23
CsCl          0.202       67.86
HO            1.292       83.39
NO            3.071       31.25
SO            1.505       60.64

Legend: a [24-26]

Table 4. Choice of methods by students

         Total     Analytical   Computational   Experimental
Class   Students     method        method          Value

A          32      21 (65.6%)     7 (21.8%)      4 (12.6%)
B          30       21 (70%)       6 (20%)        3 (10%)
C          25       20 (80%)       4 (16%)         1 (4%)

Figure 4. Computational precision x Analytical precision.

        % Computational   % Analytical

HF           91,11           31,25
HCl          70,09           60,64
HBr          69,06           69,53
HI               0           97,11
LiF          98,78           78,45
LiCl         99,39           94,7
LiBr         99,74           99,52
LiI              0           84,7
NaF          98,89           82,54
NaCl         99,77           97,42
NaBr         99,46           91,92
KF           98,47           62,78
KCl          96,98           94,43
KBr          99,71           97,79
CsCl             0           83,74
HO           89,66           90,23
NO           64,11           67,86
SO           70,09           83,39

Note: Table made from bar graph.

Figure 5. Choices of students regarding the method.

71% Analytical
20% Computational
 9% Experimental

Note: Table made from pie chart.
COPYRIGHT 2017 Universidade Federal de Mato Grosso do Sul
No portion of this article can be reproduced without the express written permission from the copyright holder.
Copyright 2017 Gale, Cengage Learning. All rights reserved.

Article Details
Printer friendly Cite/link Email Feedback
Title Annotation:Paper on Education
Author:Bastos, Cristiano Costa; Leite, Bruno Silva
Publication:Orbital: The Electronic Journal of Chemistry
Article Type:Report
Date:Oct 1, 2017
Previous Article:Determination of Ultra Trace Copper in Water Samples by Differential Pulse Polarography after Solid Phase Extraction.
Next Article:Organic Chemistry in Portugal from 1900 to 1970: A Contribution to the History of Science.

Terms of use | Privacy policy | Copyright © 2022 Farlex, Inc. | Feedback | For webmasters |