CHEMCAPER: Periodic Table of Elements

Transcription

1 CHEMCAPER: Periodic Table of Elements Image Source: Periodic Table of Elements. Wikimedia Commons.

2 THEORY PERIODIC TABLE OF ELEMENTS Today we re taking a closer look at the Periodic Table of Elements and continue playing ChemCaper. This lesson is all about the Periodic Table of Elements. Depending on how you approach the topic and use the content of this lesson, this can serve either as an introduction or refresher, depending on how well your students are acquainted with the topic. - Theory: This lesson features a look at the periodic table of elements. - Tasks: Students play the game and attempt to acquire new petticle cards and bond them. - Share & Discuss: This slide focuses on the students opening up and discussing their playing experience for both their benefit and yours. - Tasks After Playing: This slide can be used to assign your students homework, or, if you have time

3 remaining, as additional tasks in the classroom.

4 THEORY PERIODIC TABLE OF ELEMENTS Each element occupies a single square in the table and has its own assigned number (the number of protons in a single atom of that element) Vertical columns are different groups Image Source: Wikimedia Commons Image Source: Wikimedia Commons Horizontal rows are different periods Specific regions of the periodic table can be referred to as blocks in recognition of the sequence in which the electron shells of the elements are filled (pictured in the bottom image). This slide provides resources for teaching your students the periodic table of elements. While virtually everyone knows what the table is, many might not actually know how the organization on the table works, or how to read it. On the next slide are useful sources for understanding the table. The next slide also includes a full-screen version of the table for your convenience. Below are also more elaborate definitions of groups and periods in the table. Groups: Elements in the same group tend to show patterns in atomic radius, ionization energy, and electronegativity. From top to bottom in a group, the atomic radii of the elements increase. Since there are more filled energy levels, valence electrons are found

5 farther from the nucleus. From the top, each successive element has a lower ionization energy because it is easier to remove an electron since the atoms are less tightly bound. Similarly, a group has a top to bottom decrease in electronegativity due to an increasing distance between valence electrons and the nucleus.there are exceptions to these trends, however, an example of which occurs in group 11 where electronegativity increases farther down the group. (source) Periods: Period is a horizontal row in the periodic table. Although groups generally have more significant periodic trends, there are regions where horizontal trends are more significant than vertical group trends, such as the f-block, where the lanthanides and actinides form two substantial horizontal series of elements. Elements in the same period show trends in atomic radius, ionization energy, electron affinity, and electronegativity. Moving left to right across a period, atomic radius usually decreases. This occurs because each successive element has an added proton and electron, which causes the electron to be drawn closer to the nucleus.this decrease in atomic radius also causes the ionization energy to increase when moving from left to right across a period. The more tightly bound an element is, the more energy is required to remove an electron. Electronegativity increases in the

6 same manner as ionization energy because of the pull exerted on the electrons by the nucleus. Electron affinity also shows a slight trend across a period. Metals (left side of a period) generally have a lower electron affinity than nonmetals (right side of a period), with the exception of the noble gases. (source) Image Source: Periodic Table of Elements. Wikimedia Commons. Image Source: Periodic Table Blocks. Wikimedia Commons.

7 THEORY: PERIODIC TABLE OF ELEMENTS Image Source: Wikimedia Commons READ: How to Read the Periodic Table (excellent guide on how to read the table) READ: Dynamic Periodic Table (includes descriptions of each element) READ: SparkNotes: Reading the Periodic Table READ: ClassZone: Reading the Periodic Table READ: ThoughtCo: What the Numbers on the Periodic Table Mean READ: Wikipedia.org: Periodic Table Image Source: Periodic Table of Elements. Wikimedia Commons.

8 PLAY: LESSON GOAL Bond at least 3 petticle cards. What elements do those petticles represent? How many different petticles can you find? Where can you find more information on petticles? The goal is now to explore petticles (in other words, elements) in ChemCaper. The students can find additional petticles either by buying them or receiving them as loot from battle. To bond petticles, they will need a certain merchant (this is covered in the tutorial). You can let the students play until the last 10 minutes of the lesson. Leave this slide open for the duration of play.

9 SHARE & DISCUSS What was most fun about the game? Was there anything you didn t understand? What is your favorite petticle in the game in battle? Use these questions to get the students to talk about the game and their experiences with it, preparing them to work on the tasks on the next slide.

10 SHARE & DISCUSS: TASKS AFTER PLAYING Think of 4 petticles in the game. Find them in the periodic table! What kind of attributes do those petticles/elements have in the periodic table? What do they all mean? What do you think is happening when petticles bond? Element attributes: The attributes in question are the element s group, period, number and mass. What happens when petticles bond: There are three types of bonds (more on those in the next lesson). With covalent bonds, the electrons are shared, as demonstrated in the game.

11 SHARE & DISCUSS: ADDITIONAL TASKS Define what these mean in terms of the periodic table: period, group, block What happens in a group as you go downward? What happens in a period when you go from left to right? Going downward in a group: From top to bottom in a group, the atomic radii of the elements increase. Since there are more filled energy levels, valence electrons are found farther from the nucleus. From the top, each successive element has a lower ionization energy because it is easier to remove an electron since the atoms are less tightly bound. Similarly, a group has a top to bottom decrease in electronegativity due to an increasing distance between valence electrons and the nucleus.there are exceptions to these trends, however, an example of which occurs in group 11 where electronegativity increases farther down the group. (source) Going right in a period: Moving left to right across a period, atomic radius usually decreases. This occurs

12 because each successive element has an added proton and electron, which causes the electron to be drawn closer to the nucleus.this decrease in atomic radius also causes the ionization energy to increase when moving from left to right across a period. The more tightly bound an element is, the more energy is required to remove an electron. Electronegativity increases in the same manner as ionization energy because of the pull exerted on the electrons by the nucleus.electron affinity also shows a slight trend across a period. Metals (left side of a period) generally have a lower electron affinity than nonmetals (right side of a period), with the exception of the noble gases. (source)