These are practice questions to help you prepare for the exam next Tuesday. I\'l
ID: 1052238 • Letter: T
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These are practice questions to help you prepare for the exam next Tuesday. I'll provide the key by email when you email me the message that you've tried these questions: cavalier@sunydutchess.edu Don't forget that there will be a question or two taken from Test 1. Don't assume that you can do well only by memorizing these questions - these are only meant to help you focus your studying. Study all your notes, previous quizzes, the homework problems, etc.. Explain in brief terms how "bright-line spectra" of gases is explained by the Bohr model of the atom. Draw an "energy level diagram" of an atom of silicon (Si. atomic # 14). Show and label levels, sublevels, and orbitals, and draw in the electrons as half arrows. Give the "electron configuration" of an atom of iodine (1, atomic #53). Explain the periodic property of atomic radius across a row. Explain the trend in sizes based on effective nuclear charge. Why is an atom of potassium (K, element #19, mass 39.1 amu) large: than an atom of krypton (Kr, element # 36. mass 83.8 amu, {NOT kryptonite, which is fictional})?Explanation / Answer
3) Atomic number of Iodine I = 53
Electronic configuration of Iodine = 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5
4) Atomic radius in Group:
From top to bottom in a group, atomic radius increases due to increase in number of shells/ number of energy levels with increase in atomic number.
In a group from top to bottom, effective nuclear charge decreases due to addition of new energy levels.
Hence,
From top to bottom in a group, atomic radius increases.
Atomic radius in Period:
From left to right in a period, atomic radius decreases due to '' increase in effective nuclear charge''.
As we across the period, electrons are added to the same energy level and protons are added to the nucleus. Due to more number of protons in the nucleus, effective nuclear charge increases.
Hence, atomic radius decreases from left to right across a period.
5) As we across the period, electrons are added to the same energy level and protons are added to the nucleus. Due to more number of protons in the nucleus, effective nuclear charge increases.
Due to highe effective nuclear charge , Krypton has lesser atomic radius than Potassium.
Since Potassium has only one electron in its outer shell, it has lower effective nuclear charge.
Hence, Potassium is larger than Krypton.
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