Which one of the following is false? Chlorine (Z=17) has a smaller radius than aluminum (Z=13). Carbon (Z=6) has a higher first ionization energy than boron (Z=5). Potassium (Z=19) has a higher electron affinity than sodium (Z=11). Beryllium (Z=4) has a larger radius than carbon (Z= 6). Chlorine (Z=17) is more electronegative than iodine (Z=53).
Question
Which one of the following is false? Chlorine (Z=17) has a smaller radius than aluminum (Z=13). Carbon (Z=6) has a higher first ionization energy than boron (Z=5). Potassium (Z=19) has a higher electron affinity than sodium (Z=11). Beryllium (Z=4) has a larger radius than carbon (Z= 6). Chlorine (Z=17) is more electronegative than iodine (Z=53).
Solution
The statement that is false is: "Beryllium (Z=4) has a larger radius than carbon (Z= 6)."
Here's why:
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Chlorine (Z=17) has a smaller radius than aluminum (Z=13): This is true. As you move across a period from left to right, the atomic radius decreases. This is because the number of protons increases, which pulls the electrons closer to the nucleus.
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Carbon (Z=6) has a higher first ionization energy than boron (Z=5): This is true. Ionization energy increases across a period from left to right. This is because the atomic radius decreases, so the electrons are closer to the nucleus and more energy is needed to remove them.
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Potassium (Z=19) has a higher electron affinity than sodium (Z=11): This is true. Electron affinity generally increases across a period from left to right. This is because the atomic radius decreases, so the nucleus can attract electrons more strongly.
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Beryllium (Z=4) has a larger radius than carbon (Z= 6): This is false. As you move across a period from left to right, the atomic radius decreases. So, carbon, which is to the right of beryllium, should have a smaller radius.
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Chlorine (Z=17) is more electronegative than iodine (Z=53): This is true. Electronegativity decreases as you move down a group. This is because the atomic radius increases, so the nucleus has less pull on the electrons.
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