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CoachThe trend in atomic radius increases down a group. This is because as you move down a group, each element has an additional energy level of electrons, leading to a larger atomic radius. The increased number of electron shells results in greater electron-electron repulsion, causing the outermost electrons to be pushed farther away from the nucleus, thus increasing the atomic radius.
Atomic radii increases as you go down the Periodic Table due to more electrons requiring more energy levels.
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What trend in atomic radius do you see as you go down a group on the periodic?
As you go down a group on the periodic table, the atomic radius tends to increase. This is because each successive element has an additional energy level of electrons, leading to an increase in the size of the electron cloud around the nucleus.
When the three elements se te and br ara arranged in order of increasing atomic radius?
The atomic radii of elements follow a general trend: As you move down a group on the periodic table, atomic radius generally increases. Among the three elements mentioned, Se would have the largest atomic radius, followed by Te, with Br having the smallest atomic radius.
How does the atomic radius change from left to right in Groups 1 and 2?
In Groups 1 and 2 of the periodic table, as you move from left to right, the atomic radius decreases. This trend is due to increasing nuclear charge as electrons are added to the same energy level, resulting in stronger attraction between the nucleus and outermost electrons, causing the atomic radius to decrease.
Why does the change for the atomic radii of elements in period 3 from sodium to argon look similar to period 2?
The atomic radii of elements in period 3 from sodium to argon decrease due to a greater nuclear charge pulling electrons closer to the nucleus. This trend is similar to period 2 because both periods follow the same pattern of increasing nuclear charge as you move across the period, leading to a similar decrease in atomic radii.
Does atomic radius increase left to right in the periodic table of elements?
Generally it decreases. There are a few exceptions: the noble gases tend to be quite a bit bigger than the corresponding halogens, and there's a smaller bump as you go from d-block elements to p-block elements.
