Hoi-Ting
Wu
a,
Kiana
Mortezaei
a,
Teresa
Alvelais
a,
Grace
Henbest
a,
Courtney
Murphy
a,
Ellen J.
Yezierski
*b and
Jack F.
Eichler
*a
aDepartment of Chemistry, University of California, 501 Big Spring Road, Riverside, California 92521, USA. E-mail: jack.eichler@ucr.edu; Tel: +(951) 827-3794
bDepartment of Chemistry and Biochemistry, Miami University, 360B Hughes Laboratories, Oxford, Ohio 45056, USA. E-mail: yeziere@MiamiOH.edu; Tel: +(513) 529-2819
First published on 29th May 2021
Implementation of the flipped classroom approach into STEM courses has been popularized in the last decade and has generally been reported to improve student performance outcomes. In a flipped classroom setting, students typically first encounter course content in the online format and subsequently engage in some form of active learning during the in-person class meetings. Although the flipped classroom approach can promote increased student engagement and provide an opportunity to apply content encountered in the classroom, this structure does not generally give students opportunities for discrete concept development prior to the application phase of learning. In an effort to build concept development activities into a flipped classroom structure, five learning cycle activities were implemented in a large enrollment first-term general chemistry course that has previously implemented the flipped classroom design. Four of these learning cycle activities incorporated PhET simulations as part of the exploration phase of learning, and all five activities were facilitated during the in-person class meetings to initiate the learning cycle. The activities were designed to help students explore models and engage in concept development. The application phase of the learning cycle was facilitated by flipped classroom modules or in-person classroom activities that included whole-class questioning coupled with collaborative think-pair-share discussion. Performance gains in conceptual understanding were evaluated by employing a one-group, pre-post-post research design. Non-parametric Friedman's tests indicate a significant main effect across time for each concept development activity, and post hoc Wilcoxon signed rank tests indicate the post-test and final exam scores are significantly higher than the pre-test scores for each activity (p < 0.001 for each pre-post and pre-final pairwise comparison). The findings reported herein demonstrate that concept development activities can be successfully integrated with flipped classroom modules and the combination of the introductory learning cycle activities and flipped classroom application activities led to knowledge gains that persisted through the end of the course. In total, creating this type of blended learning environment appears to help students achieve understanding of core general chemistry concepts.
Although the flipped classroom structure has been identified as a possible way to reduce cognitive load relative to the delivery of content in a traditional lecture format (Seery, 2015), the initial steps of concept development are not well-understood or deliberately supported by the usual pre-class content. This is likely because students typically only have a listening and/or note-taking role in the online learning space. Thus, there is an opportunity and a need to build concept development into the flipped classroom design. This could be achieved by including an in-class activity prior to the asynchronous online learning module, in which exploration and concept development are facilitated through sense-making of phenomena, models, and data. This modification is aligned with a pedagogical method known as the learning cycle (Lawson and Karplus, 2002), which includes exploration, term introduction or concept development, and application phases of instruction. As mentioned above, the flipped classroom already has a strong application component in which the in-class activities build upon the pre-class online content. However, the exploration and concept development phases cannot be readily integrated into pre-class asynchronous learning activities, and to our knowledge incorporating preliminary concept development into a flipped classroom structure has not been reported. There are reports of incorporating POGIL (Process Oriented Guided Inquiry Learning) activities in the in-person portion of the flipped classroom (Hibbard et al., 2016; Canelas et al., 2017). Though POGIL involves collaborative group learning that aims to facilitate conceptual understanding through exploration, explanation, and sense-making processes (Moog and Spencer, 2008), the studies reported by Hibbard et al. and Canelas et al. were built on flipped classroom structures in which the POGIL activities were completed after the pre-class learning assignments.
In the present study, learning cycle activities that promoted exploration and concept development were implemented as introductory in-class activities prior to standard flipped classroom modules, which were then followed by in-class activities centered on whole-class questioning and think-pair-share group learning. The learning cycle activities were developed for five foundational learning objectives in the first-term general chemistry curriculum, four of which employed PhET simulations to engage students in the exploration phase of the learning cycle. PhET interactive simulations‡ were integrated in the concept development activities, because they can provide immediate feedback to users and are designed to support student connection-making and focus on active knowledge construction (D’Angelo et al., 2014).
Because the in-person classroom activities associated with flipped classroom implementations are often built on some form of collaborative group learning, this aspect of the flipped classroom is broadly grounded in Vygotsky's social constructivism framework (Vygotsky, 1978). Social constructivism emphasizes the importance of the collaborative nature of learning, and posits that cognitive functions are closely linked to social interactions. Classroom exercises such as peer-led team learning, POGIL, and even less formal think-pair-share activities are partially rooted in social constructivism due to the dependency upon collaborative work that supports learning in these interventions. The impact of social constructivism on the flipped classroom assumes collaborative group learning is embedded in the in-person classroom activities, and it should be noted that the opportunities for group interactions may indeed vary across different flipped classroom implementations.
Von Glasersfeld has proposed that constructivism is a framework in which knowledge is constructed in the mind of the learner from experience, and the function of cognition is to organize such experiences (Von Glasersfeld, 2001). This view of constructivism can be explicitly connected to classroom instruction through the learning cycle instructional model (Lawson and Karplus, 2002). The learning cycle engages students in iterative progressions of exploration of phenomena, concept invention/term introduction, and application. The learning cycle is particularly germane to our thinking about the flipped classrooms, because as noted above, the in-class active learning that follows the pre-class modules is typically an application activity. The learning cycle is notable for its student-centeredness and the opportunities it affords for students to build knowledge from experiencing phenomena in the exploration phase and making sense of the findings from the exploration in the concept invention/term introduction phases. It is important to consider that a teacher-centered lecture is antithetical to the experienced-focused exploration phase of the learning cycle. Applying the constructivist framework underlying the learning cycle, the current study aims to help students develop conceptual knowledge through the exploration and concept invention activities that take place in class prior to more typical flipped classroom structures.
Four of the activities described here incorporated PhET simulations as part of the exploration phase of the learning cycle. The use of PhET simulations as a way to promote investigative inquiry and foster sense-making in chemistry instruction has been previously reported (Lancaster et al., 2013), and the use of the PhET Atomic Interactions simulation§ within the exploration phase in a concept development activity was described by Minahall and Yezierski (Minshall and Yezierski, 2021). The implementation of the Atomic Interactions activity followed a quasi-experimental design in which each new version of the activity was tested to evaluate the quality of the material in term of students’ learning outcomes. The present study builds upon this work, with the aim to further extend the learning benefits of interactive simulations to other foundational concepts in the general chemistry curriculum.
Three new activities that incorporated PhET simulations were used in addition to the previously reported Atomic Interactions activity, and one additional activity used a static POGIL model to engage students in concept exploration (Moog and Farrell, 2002). Students worked through the learning cycles in small and collaborative groups in class before interacting with the flipped classroom modules or in-person instruction that incorporated whole-class questioning with think-pair-share collaborative learning. The learning cycle activities provided students the opportunity to engage in concept development by making observations within the simulation/model, respond to concept development questions, engage in group discussion, verbally articulate their thinking, and receive feedback on that thinking from peers. The students then built on that conceptual foundation as they progressed through the subsequent flipped classroom modules and whole-class questioning activities. Five learning objectives addressed in most first-term general chemistry courses were chosen and targeted for the learning cycle activities, because the authors have routinely observed that students often struggle with core concepts related to these five learning objectives (see Table 1). These five topic areas are included in the General Chemistry Anchoring Concepts Content Map (Holme and Murphy, 2012), suggesting these are pertinent to most undergraduate general chemistry courses.
Learning cycle activity title | Version and year of PhET simulation | Learning cycle activity sheet and teaching notesa | Learning objectives students will be able to: |
---|---|---|---|
a The activity sheets, pre/post/post test items, and detailed teaching notes are available to download from the PhET website. | |||
Nuclear Atom | N/A | Nuclear atom POGIL activity (Moog and Farrell, 2002). | (1) Identify the atomic number and mass of atoms for different elements; |
(2) Identify the importance of atomic number in identifying atoms of different elements; | |||
(3) Identify different isotopes of the same element; and | |||
(4) Use the total number of protons and electrons to determine if ions are present and determine the charge of the ion. | |||
Coulomb's Law | 1.0.9, 2019‡‡ | https://phet.colorado.edu/en/contributions/view/5909 | (1) Predict how electrostatic attraction/repulsion changes as a function of distance between charged particles; |
(2) Predict how electrostatic attraction/repulsion changes as a function of the magnitude of charge between charged particles; and | |||
(3) Describe the concept of electrostatic attraction/repulsion in preparation for applying it to atoms. | |||
Atomic Interactions | 1.1.0, 2019§ | https://phet.colorado.edu/en/contributions/view/5860 | (1) Predict how the potential energy of a bond changes with changing interatomic distance; |
(2) explain how attractive and repulsive Coulombic forces impact the potential energy of a chemical bond; and | |||
(3) Predict if bond making and bond breaking events are exothermic or endothermic. | |||
Molecular Shape | 1.2.8, 2019§§ | https://phet.colorado.edu/en/contributions/view/5910 | (1) Use Lewis structures to determine the number of bonded atoms and number of non-bonding electron pairs on the central atom of a molecular structure; |
(2) Predict the molecular geometry and molecular shape of structures using the VSEPR model; and | |||
(3) Predict if the real bond angle is approximately equal to or less than the ideal bond angle for different types of molecular shapes. | |||
Molecular Polarity | 1.0.15, 2019¶¶ | https://phet.colorado.edu/en/contributions/view/5911 | (1) Explain the difference between a bond dipole and a molecular dipole; |
(2) Use electronegativity and knowledge of molecular shape to predict if molecules possess a net molecular dipole or not; and | |||
(3) Use electrostatic potential maps to explain if a net molecular dipole exists or not. |
The theoretical and methodological frameworks described above were integrated within a first quarter general chemistry course to address the following research questions:
1. How can the use of introductory learning cycle activities foster conceptual learning for five foundational concepts in a first-term undergraduate general chemistry course?
2. How will knowledge gains (if realized) persist over the course of the term?
3. How can analyses of incorrect student responses provide insight about lingering inaccurate chemical ideas?
Students were informed through a verbal consent process that their performance on the pre- and post-test assessments would be evaluated for research purposes (under approved IRB protocol HS-10-135). They were also informed that all pre/post/post test data would be reported in aggregate form (i.e., all data would be reported in a way that would not reveal individual student identities) and that they could request to have their test data excluded at any time. During the course of the study no students requested to have their data excluded from the analysis.
To help students develop the preliminary concepts independently while engaging with the activities, they were divided into ad-hoc groups of 3–4 students to explore the PhET simulations (Table 1) and complete the activity sheets. The students were instructed to write their answers on the worksheet. The course instructor and two graduate student teaching assistants were available to assist and answer questions as needed, and the instructor had the simulation running on the classroom projector. If points of confusion arose regarding the using the simulation, the instructor would demonstrate parts of the simulation for the class; however, students needed to make their own observations and document results. The activity sheets and detailed teaching notes for the activities that included the PhET simulations, along with the activities sheet and teaching notes are available online (see Table 1). The Nuclear Atom activity is a POGIL worksheet that includes a static drawing in lieu of a PhET simulation (Moog and Farrell, 2002).
After the introductory learning cycle activities, students engaged in either a flipped classroom module or an in-person classroom structure that employed whole-class questioning with think-pair-share collaborative group learning (see Fig. 1). A detailed description of the flipped classroom modules and whole-class questioning activities, and how these exercises were timed throughout the term is provided in Appendix 2 (ESI†). For the flipped classroom modules, students were given 3–4 days to watch instructor-created videos and complete the associated online quiz that was due prior to the in-class application exercises. The online videos also included embedded questions that students completed in the Playposit system.¶ For the flipped module in-class application exercises, the instructor briefly reviewed the material from the online videos and introduced the topic to be discussed that day in the in-class worksheet. Students then worked in collaborative groups of 3 or 4 while completing the worksheet, and they had access to the instructor and two graduate student teaching assistants if clarification was needed. Student work was evaluated by converting the free response questions to multiple choice format, and students submitted answers using the classroom polling system (PollEverywhere||). The instructor then used the last 10–15 minutes of the class period to review any questions in which a large proportion of students submitted incorrect responses and concluded by summarizing the main learning objectives. For some topics, it was determined that students should engage with in-class application exercises in the classroom period immediately after the learning cycle activity (see Appendix 2, ESI†). No online pre-class learning modules were included in these instances, and students applied concepts developed during the learning cycle activities in the subsequent class meeting via instructor-led discussion and whole-class questioning that included think-pair-share collaborative group learning. Analogous to the learning cycle activities, student responses to the whole-class questions were submitted using the classroom polling system. The course syllabus provided in Appendix 1 (ESI†) describes how the performance in the in-class polling factored into the overall course grade.
![]() | ||
Fig. 1 Representative examples for how the concept development activities and flipped/hybrid modules were administered. The full schedule of all concept development activities and flipped/hybrid classroom modules is provided in Appendix 1 (ESI†), and the detailed description of the classroom and online learning activities is provided in Appendix 2 (ESI†) (• blue boxes denote learning cycle activities; • green boxes denote application of concepts using whole-class questioning/think-pair-share; • and yellow boxes denote flipped classroom modules). |
Authors EJY and JFE co-wrote all the test items and came to consensus in confirming the content validity of the final set of test items for each activity. The single administration reliability of the test items was evaluated by calculating Cronbach's alpha for the set of test items for each activity, and the ability of the individual items to discriminate between high and low performers was estimated by calculating the item-total correlation values for the items (see Appendix 3, Tables 1 and 2, ESI†). These analyses suggest the scores on items across administrations for each activity were correlated to one another and generally appeared to discriminate between high- and low-performing students. However, the length of the tests only ranged from 2–5 items, making it difficult to arrive at definitive conclusions regarding the reliability of the tests (Tavakol and Dennick, 2011). To gain additional insight about how well the test items measured changes in student knowledge, Sankey diagrams were used to track responses at each time point of test, for each individual item (see Appendix 5, Fig. 1 and 2, ESI†). These data indicate the tests detected clear changes in student knowledge for all the activities except the Coulomb's Law activity, for which the students appeared to demonstrate a high level of a priori knowledge. In total, the item analyses and reliability data suggest the tests were acceptable measures of student knowledge for these five conceptual domains. A detailed summary and explanation of the item analysis and single administration test reliability are provided in Appendix 3 (ESI†).
Activity | Friedman test statistics | W | ||
---|---|---|---|---|
χ 2 | df | p | ||
a W = 0.1 indicates a small effect, W = 0.3 indicates a medium effect, and W > 0.5 indicates a large effect. | ||||
Nuclear atoms | 216.515 | 2 | <0.001 | 0.558 |
Coulomb's law | 72.460 | 2 | <0.001 | 0.187 |
Atomic interaction | 249.213 | 2 | <0.001 | 0.642 |
Molecular shape | 156.071 | 2 | <0.001 | 0.402 |
Molecular dipole | 134.978 | 2 | <0.001 | 0.348 |
Because the Atomic Interactions was previously developed and evaluated by Minshall and Yezierski (Minshall and Yezierski, 2021), it was of interest to compare the results of the current study to this previous report. Additionally, the learning objectives for the Atomic Interactions activity include having students correctly identify the energy changes associated with chemical bond forming and breaking processes. Since students often incorrectly associate bond breaking with an exothermic energy change (Boo, 1998), it was also desirable to determine if the efficacy of this activity would translate to a large enrollment course. As shown in Fig. 2d, approximately 73% of the students incorrectly answered the pre-test questions regarding whether bond breaking and bond making events are exothermic or endothermic. However, most students successfully demonstrated improved performance after the post-test (94% of students answered both test items correctly; see Fig. 2d) and retained this conceptual knowledge on the final exam (97% of students answered both test items correctly; see Fig. 2d). It is noteworthy that a higher percentage of students correctly answered the questions on the final exam using the same activities than the previous study carried out by Minshall and Yezierski, in which 82% of the 34 students were able to able to identify and distinguish between exothermic and endothermic processes (Minshall and Yezierski, 2021). The results from this current study are highly encouraging, as the sample is almost 6 times the size of previous study (231 verse 34 students). It suggests that the activities can be implemented in a large enrollment course without sacrificing student performance gains. This observation might be explained by the implementation of the Coulomb's Law activity‡‡ prior to the Atomic Interactions activity in the present study. Because the knowledge of attractive and repulsive electrostatic forces is required to explain how the potential energy of a chemical bond changes as a function of interatomic distance, we speculate that including the Coulomb's Law activity might have primed students to make better sense of their observations during the Atomic Interactions activity.
To determine if the changes in student performance over time were statistically significant, a non-parametric Friedman test was conducted to evaluate differences among the total number of correct test items at the three time points for each activity. The Friedman's Chi-square value (χ2) for all activities was found to be significant (p < 0.001), indicating the learning cycle activities had a significant effect on student performance (Table 2). The Kendall's Coefficient of Concordance (W) was used to measure the effect size of each activity. A W value of 0.5 or above indicates large differences among the three time points. Most activities have medium or large effect sizes; only the Coulomb's Law activity had a small effect size with this group of students (W = 0.187). The smaller effect size observed for the Coulomb's Law activity is possibly explained by the fact that the concepts addressed in this activity ended up being less challenging than originally expected (see Appendix 5, Fig. 1a–d, ESI†), as the students appeared to have a high level of a priori knowledge on electrostatic attraction/repulsion.
Post hoc pairwise comparisons of the non-normally distributed test scores were conducted using a Wilcoxon-signed rank test (Table 3) to determine if the student performance was significantly different at the three testing points. The effect size (r) for each pairwise comparison was calculated using previous published method (Tomczak and Tomczak, 2014), and the cutoffs for r are as follows: 0.1 (small effect), 0.3 (medium effect), and above 0.5 (large effect) (Cohen, 1988). Students’ test scores improved from the pre-test to both the post-test and final exam, for all five activities (for all post-test/pre-test and final exam/pre-test pairwise comparisons; p < 0.001). The learning cycle activities yield large effect sizes for test performance for the Atomic Interactions and Molecular Shape activities, medium effect sizes for the Nuclear Atom and Molecular Dipole activities, and a small effect size for the Coulomb's Law activity (see post-test/pre-test pairwise comparisons in Table 3). The combination of the learning cycle activities and subsequent flipped modules/in-class exercises yield a medium to large effect for all five conceptual domains (see final exam/pre-test pairwise comparisons in Table 3).
Activity | Pair-wise score comparison | Z | p (2-tailed)a | r |
---|---|---|---|---|
a Significance level adjusted using a Bonferroni correction (α: 0.05/3 = 0.017). b The interpretation guidelines for r are as follows: 0.1 (small effect), 0.3 (medium effect), and above 0.5 (large effect). | ||||
Nuclear Atom | Post-test/pre-test | 8.597 | <0.001 | 0.44 |
Final exam/pre-test | 10.296 | <0.001 | 0.52 | |
Final exam/post-test | 4.101 | <0.001 | 0.21 | |
Coulomb's Law | Post-test/pre-test | 3.488 | <0.001 | 0.18 |
Final exam/pre-test | 7.804 | <0.001 | 0.40 | |
Final exam/post-test | 4.767 | <0.001 | 0.24 | |
Atomic Interaction | Post-test/pre-test | 11.402 | <0.001 | 0.58 |
Final exam/pre-test | 11.708 | <0.001 | 0.59 | |
Final exam/post-test | 1.762 | 0.078 | 0.09 | |
Molecular Shape | Post-test/pre-test | 10.222 | <0.001 | 0.52 |
Final exam/pre-test | 8.131 | <0.001 | 0.41 | |
Final exam/post-test | 5.269 | <0.001 | 0.27 | |
Molecular Dipole | Post-test/pre-test | 8.972 | <0.001 | 0.46 |
Final exam/pre-test | 8.932 | <0.001 | 0.45 | |
Final exam/post-test | 0.340 | 0.734 | 0.02 |
MS Q2. Which would you predict to have the strongest repulsive force to a nearby electron pair? |
A. A non-bonding electron pair |
B. A bonding electron pair |
C. These have the same repulsive force |
MS Q3. Which would you expect to have the smallest bond angle? |
A. NH3 |
B. CH4 |
C. H2O |
D. These would all have the same bond angle. |
MD Q3. Which explains why water molecules are polar and carbon dioxide molecules are non-polar? |
A. Water molecules have a non-linear molecular shape |
B. Carbon dioxide has non-polar bonds |
C. Both molecules have polar bonds |
D. Hydrogen and oxygen have a large electronegativity difference |
MD Q4. Which molecule has a net molecular dipole? |
A. OCl2 |
B. Cl2 |
C. CO2 |
D. BH3 |
In Question 2 of the Molecular Shape test, the desired conceptual learning outcome is that an unbonded electron pair gives rise to the strongest repulsive force to a nearby bonded electron pair. For the question, “Which would you predict to have the strongest repulsive force to a nearby electron pair?”, the most common distractor in the pre-test was the answer “a bonding electron pair.” This was likely because students recognized electrostatic repulsion occurs between bonded atoms, but they neglected to consider the effect of non-bonding electrons on the bond angle between the bonded atoms. Though the number of students who chose this answer decreased from 69 to 12 from pre- to post-test administration, 48 students reverted back to the “a bonding electron pair” distractor on the final exam (see Fig. 3a). Question 3 of the Molecular Shape activity also evaluated students’ understanding of the impact of non-bonding electron pairs on molecular shape. The most common distractor in the pre-test for this item was the answer “CH4,” likely because students associated smaller bond angles with molecules in which more atoms were bonded to the central atom. The number of students who chose this answer decreased from 114 to 26 from pre- to post-test administration, yet 65 students again chose this common distractor on the final exam (Fig. 3b). Overall, most students appeared to make knowledge gains with respect to identifying the impact of non-bonding electron pairs on the electron pair geometries and shapes of molecules. However, given the fact over 10% of the students reverted back to the inaccurate thinking for these two test items as described above, practitioners might consider refining the Molecular Shapes activity to mitigate this reversion in future implementations. Because some students appear to neglect the impact of the non-bonding electron pairs, the activity could guide students to draw out the molecules with all bonding atoms and non-bonding electro pairs (this could be added into Table 2 of the Molecular Shapes activity§§). If students were asked to draw the molecules in this way, and also to use arrows to identify where electrostatic repulsion occurs within the molecule, this might lead to longer lasting knowledge gains for this particular concept.
In Question 3 of the Molecular Dipole activity, the desired learning outcome was for students to understand the relationship between molecular structure and molecular dipoles. In this particular question, students were required to choose the response that explains why water molecules are polar and carbon dioxide molecules are non-polar. Although the number of students who chose the most common distractor decreased from 81 to 39 from pre- to post-test administration, 40 students still answered incorrectly on the final, and over 10% of students reverted from the correct answer on the post-test to the most common distractor on the final exam. The most common distractor stated “hydrogen and oxygen have a large electronegativity difference.” Although this statement is accurate, it does not explain why water is polar molecule and carbon dioxide is not. The students who chose this answer likely only considered the electronegativity difference between the atoms in the bonds in identifying molecular dipoles, without considering how the three-dimensional structure plays a role in giving rise to molecular polarity. For Question 4 in the Molecular Dipoles activity, the number of students who chose the most common distractor decreased from 63 to 20 from the pre- to post-test administration. Though only 33 students chose this distractor on the final exam, over 10% of students who chose this answer on the final reverted back to this common distractor after answering correctly on the post test. Because the most common distractor for this question was “BH3,” we speculate students who chose this answer did so based on comparing its structural formula to the other answer choices, rather than carefully evaluating differences in electronegativity and/or molecular geometry (BH3 was unique among the answer choices in having three atoms bonded to a central atom; see Appendix 4, ESI†). The critical thinking questions in the Molecular Dipole activity explicitly ask students to identify what properties are required for a molecule to possess a net dipole.¶¶ Therefore the observation that over 10% of students continued to incorrectly identify which molecules have net dipoles and/or why net dipoles are present was surprising. In future implementations of the activity, instructors might consider including a post-activity discussion highlighting that the molecular formula should not be used as a heuristic to identify the presence of net molecular dipoles, and that simply determining the presence of polar bonds is not sufficient in identifying molecular dipoles. Instructors might also consider having students draw out the net dipole vectors in addition to the electron density maps, which could help reinforce how both electronegativity differences and molecular shape determine if a net molecular dipole is present.
These observed knowledge gains can be viewed within the context of the constructivist theory of learning. As described in the introduction, Vygotsky's theory of constructivism posits that understanding comes from making meaningful connections through experience between prior knowledge and new knowledge (Vygotsky, 1978). The in-class learning cycle activities allowed students to explore the simulations in a guided fashion, and they constructed informal and general ideas about the subject individually built upon the foundation of previous learning. Vygotsky's theory states that language plays a fundamental role in shaping meanings. Because students wrote down their observations and personal interpretation of the simulations, and then subsequently engaged in group discussions to further extend their concept development, learning was supported by social constructivist principles. Additionally, a cycle of exploration, concept development, and concept application was created by combining the introductory learning cycle activities with the flipped modules/in-class exercises. This suggests the overall knowledge gains observed for the five conceptual domains can also be rooted in Von Glasersfeld's view of constructivism (Von Glasersfeld, 2001). Students were given the opportunity to construct new conceptual knowledge from experience (the exploration and concept development phases in the introductory learning cycle activity), then apply this new knowledge in the online flipped module exercises and in-class collaborative group learning exercises. The totality of this learning experience appears to have to led to both short term and longer-term conceptual understanding for students.
The short duration of the tests for each activity and the fact these measures of student knowledge were only administered to one sample may have limited the rigor of the reliability analysis; however, the item-total correlations and the apparent ability of the tests to detect gains in knowledge suggest the tests were adequate measures of student knowledge. It is also noted the pre-test performance did not impact the students’ grades, whereas the post-test questions counted as extra credit and the assessment questions were integrated as normal questions within the final exam. Because the students did not have the same grade incentive on the pre-test, this could have biased the improved performance on the post-test and final exam. Unfortunately, this limitation is difficult to overcome in a class-based quasi-experimental design, as it is generally not desired to have the pre-test scores impact student grades. The same set of items of were administered three times. Although this lends reliability to the results, it could limit the validity in measuring student knowledge (i.e., students could just be remembering the question and answer). However, this validity limitation is minimized because students were not provided with the answers nor were alerted that the same items would be on subsequent tests. Finally, the test questions were designed by the authors to evaluate conceptual knowledge and determine if students continued to adopt previously observed inaccurate chemical ideas. Despite being designed to probe conceptual understanding, the multiple-choice format of the questions may have limited the ability to fully capture the products of student sense-making and conceptual thinking. Future studies could involve creating items that include some free response questions and/or other methods that more effectively elicit and document student sense-making and conceptual understanding.
It is uncertain that the success of the learning outcomes in this study can be translated to other institutional settings. With the challenges of implementing the activities in a large enrollment course that had a high percentage of first-generation students, significant and positive learning outcomes were observed for each learning cycle activity in the present study. This suggests the inferential statistical claims made regarding performance gains in the present study should generalize to other undergraduate introductory/general chemistry courses. Though the activities need to be implemented in other institutions with different student populations to confirm this notion, the fact the performance gains reported here for the Atomic Interactions activity appear to be comparable to those reported by Minshall and Yezierski (Minshall and Yezierski, 2021) further suggest the learning cycle activities can be successfully implemented in institutional settings with disparate student populations.
With respect to the implementation of the PhET-based learning cycle activities, access to devices could be a potential limitation at some institutions. If laptop or tablet loan programs are not available, instructors could modify the implementation to allow students to share devices. If enough students have access to devices such that at least one student per group can run the PhET simulation, this should allow instructors to facilitate the learning cycle activities. If access to laptops or tablets is even more limited, instructors might consider running the simulation as a demonstration on the classroom projection system, and students could then make the necessary observations and progress through the scaffolded questions.
Using simulations as a means for students to generate observations in learning cycle activities within a non-laboratory classroom setting is a promising approach to integrate concept development activities in higher education introductory chemistry courses. It is hoped the current study, in conjunction with the previous report from Minshall & Yezierski (Minshall and Yezierski, 2021), demonstrates how students can improve conceptual understanding when the learning cycle approach is used with simulation-based activities and will inspire instructors from a variety of institutional settings to engage their students in this approach. With respect to the use of the flipped classroom in higher education chemistry, educational studies generally provide only a vague description of coupling online video tutorials with some form of in-class active learning. To our knowledge no previous reports describe including an in-class concept development activity prior to the cycle of online/in-person learning. We hope the current study gives classroom practitioners a roadmap for how concept development activities can be incorporated into a flipped classroom structure, as well as a more complete picture of what is actually involved in the pre-class online learning and in-class active learning environments that produced the performance gains described herein. If instructors were to put a twist on the flip as described here, they would be creating a blended learning environment that actively engages students in a new way and likely helps students achieve understanding of core general chemistry concepts.
Footnotes |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/d1rp00086a |
‡ PhET Interactive Simulations. From https://phet.colorado.edu/. |
§ PhET Atomic Interactions simulation. From https://phet.colorado.edu/en/simulation/atomic-interactions. |
¶ Playposit is available at: https://go.playposit.com/. |
|| PollEverywhere is available at: https://www.polleverywhere.com/. |
** iLearn/Backboard quiz system. From https://www.blackboard.com/teaching–learning/learning-management. |
†† IBM Corp. Released 2019. IBM SPSS Statistics for Windows, Version 26.0. Armonk, NY: IBM Corp. |
‡‡ PhET Coulomb's Law simulation. From https://phet.colorado.edu/en/simulation/coulombs-law. |
§§ PhET Molecular Shapes simulation. From https://phet.colorado.edu/en/simulation/molecule-shapes. |
¶¶ PhET Molecular Dipole simulation. From https://phet.colorado.edu/en/simulation/molecule-polarity. |
This journal is © The Royal Society of Chemistry 2021 |