I’m unsure how to do this illustration of periodic trends lab. Any help would be
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I’m unsure how to do this illustration of periodic trends lab. Any help would be great. I’m unsure how to do this illustration of periodic trends lab. Any help would be great. I’m unsure how to do this illustration of periodic trends lab. Any help would be great. AT&T; LTE Illustration of Periodic Trends Illustration of Periodic Trends Visually represent periodic trends. Observe periodic trends in atomic size and ionization the number of protens moving down group, the addition of another energy level at a distance further from the nucleus causes a substantial increase in atomic size Periodic trends are properties of elements that ca be related to the element's position on the periodic table There are many periodic trends: electren configuration, metallik character, valence electrons, ion charge, et al In this activity, you will explore the periodk trends of atomic size and ionization energy is the energy required to remove the outermost electron fremm a peutral ground-state atem Ionization energy is directly related to the distance between the outermost electron and the nucleus. The Atomic size is actually reported ascloser the electron is to the nucleus, the atomic radius, the typical distance from the center of the nucleus to the outermost electron position. The primary factor in determining the size of an atom is the location of that outermost electron. more difficult it will be to remove while an electron far from the nucleus will be easier to remove. Therefore, ionization energy is inversely proportional to atomic If atomic size decreases going periodic table, additional electrons are entering the electron cloud in the same across a period on the periodic table bringing the outermost electren cleser to the nucleus, ionization energy will iscrease as you progress across that electren. These electrons being in the same shell are the same distance from the If atomic size increases going down a group on the periodic table, the outermost electron will be further from the influence of the nucleus, lonization energy will therefore decrease as you pregress down a group on the periodic on the periodic table. However, as each additional electren is added going across the period, an additional proton is added to the nucleus as well. These additional protons provide a greater nuclear charge, which pulls the electrees in more tightly. This results in a decrease in atomic radius going across the periodic table left to visual representation of the magnitude of atomic size and ionization energy and display these on a periodic table thereby illustrating the relationship between these properties and the pesition of the element on the periodic table. Tracking down a group on the periodic table, the most important change affecting atomic size is the addition of another energy level or shell. Even though there is a significant increase in The periodic table provided in the lab kit for this activity includes the main group elements only and excludes the Previous NextExplanation / Answer
Questions:
1. https://en.wikipedia.org/wiki/Atomic_radius
2. https://en.wikipedia.org/wiki/Ionization_energies_of_the_elements_(data_page)
3. a) As you go down in a group, the atomic size gradually increases.
b) Reason: The size of the outer shell increases(1, 2, 3, ....up to 7), as a result, the outer shell electrons are loosely held by the nuclear attraction. Hence, the atomic size increases.
4. a) As you go from left to right across a period, the atomic size gradually decreases.
b) Reason: The nuclear charge increases, as a result, the outer shell electrons are firmly held by nuclear attraction. Hence, the atomic size decreases.
5. a) As you go down in a group, the ionization energy gradually decreases.
b) Reason: As the outer shell electrons are loosely held by the nuclear attraction, less energy is required to remove the electron from the outer shell. Hence, the ionization energy decreases.
6. a) As you go from left to right across a period, the ionization energy gradually increases.
b) Reason: As the outer shell electrons are firmly held by nuclear attraction, more energy is required to remove the electron from the outer shell. Hence, the ionization energy increases.
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