How does ionic radius change within a group of metals?
Ionic radius increases as you move from top to bottom on the periodic table.
Ionic radius decreases as you move left to right across the periodic table.
The first is straightforward: more shells, more shielding, and less effective nuclear charge because the shells are farther from the nucleus's pull.
The ionic radius increases for nonmetals as the effective nuclear charge decreases because there are more electrons in the shell than there are protons; for metals forming cations, the ionic radius decreases as the metals lose their outer electrons. The issue with the left to right direction is that the shell is becoming more densely packed with electrons.
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The ionic radius tends to increase within a group of metals as you move down the group. This is due to the addition of electron shells as you move down the group, leading to an increase in the atomic size and thus the ionic radius.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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