Atomic radii become smaller as you go from left to right across a period because the charge in the atom's nucleus becomes larger (increases Z eff). Electron affinity decreases as we proceed down a group for the same reason.Īn atomic radius is total distance from an atom's nucleus to the outermost electron orbital. This causes the electron to move closer to the nucleus, thus increasing the electron affinity. Moving from left to right across a period, atoms become smaller and smaller as the atomic number increases. This is caused by the decrease in atomic radius. Electron affinity increases from left to right across the periodic table. Ionization energy also decreases down a group for the same reason.Įlectron affinity is the amount of energy absorbed when an electron is added to an atom. It is harder to take an electron off a small atom, so ionization energy increases. Ionization energy increases across a period because as the number of protons increases the atomic radius decreases. Ionization energy is the energy it takes to remove an electron from an atom. Why does F have a larger ionization energy that O? Possible Answers Why are ionization energies always positive?ġ0. What is the general relationship between the size of an atom and its ionization energy?ĩ. What is the group called and what number is it? Also name two properties that they would be expected to share.Ĩ. Barium and magnesium are both found in the same group in the periodic table. Are these elements metals or nonmetals? How many valence electrons do they have? Name a property that these two elements share.ħ. Chlorine and bromine are both found in the same group in the periodic table. What is electronegativity and what are its periodic trends?ĥ. What is an atomic radius and what are its periodic trends? Explain.Ĥ. What is electron affinity and what are its periodic trends?ģ. What is ionization energy and what are its periodic trends? Explain.Ģ.
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