Figure 2: Atomie radi(from l spanhd C10Iwchnotes mesdsern atomis Atomic Radii (p
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Figure 2: Atomie radi(from l spanhd C10Iwchnotes mesdsern atomis Atomic Radii (pm) 8A 1A 2A 3A A 5A 6A 373 152 112 9577757372 186 160 143 118 110 103 100 98 135 122 120 119 114 112 248 215 167 140 140 142 1 131 265 222 10 146 150 168 040) (141) Explaining the trend in atomic radius: As one compares elements across a period, the major differences are the number of electrons in the outermost shell and the total number of protons 1. an increased number of electrons in the outermost shell 2. a greater number of protons in the nucleus 12) How would each of these affect the atomic radius across a period? (Hint: They are opposite affects.) 13) Based on the periodic trend you saw above, which of these is dominant?Explanation / Answer
12) Atomic radius decreases from left to right across a period in the periodic table. As we move from left to right across a period , valence electrons are being added in the same energy level. But at the same time, positively charged protons are added to the nucleus. Addition of proton increases the nuclear pull over the electrons and now the nucleus pulls the electrons more closer to it. As a result from left to right in a period, atomic radius decreases.
13) From the above trend, it is quite evident that a greater number of protons in the nucleus has a more significant effect than increased number of electrons.
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