N-- Because it has less electrons, the proton pull is smaller on each individual electron, holding them closer to the nucleus and making the radius smaller
Nitrogen does, because it is to the left of Oxygen on the Periodic Table, and as a result, has one less electron and one less proton (don't consider neutrons). The electrons don't make a difference unless it's something like O-3, meaning an ion of Oxygen with 3 additional electrons, which gives it a whole new shell, and therefore a bigger radius.
The protons, however, have a big effect. Because Nitrogen has 1 less proton, it has less of a pull on it's electrons, and therefore doesn't keep them as close at bay as Oxygen does.
Yes. Sulfur and oxygen are both in column 16 of a wide form periodic table, with sulfur below oxygen. This means that sulfur has an additional shell of electrons compared with oxygen, and sulfur has a correspondingly larger radius.
Be because as you move across the periodic table from left to right it decreases and as you go from top to bottom it increases.
which has a larger atomic radius, nitrogen or bromine
The atomic radius (covalent) of selenium is 115 pm.
The atomic radius (covalent) of oxygen is 60 pm.
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Which has the larger atomic radius selenium or oxygen?
Caesium atom has a larger atomic radius.
The negative ionic radius is larger than the neutral atomic radius
Yes Atomic radius of carbon: 60 pm Atomic radius of silicon: 110 pm
Radium has a much larger atomic radius than beryllium.
Yes.
Atomic radius of Si is 111pm.Atomic radius of Pb is 175pm.Therefore lead has a larger atomic radius than silicon.
Caesium atom has a larger atomic radius.
K (potassium) has the larger atomic radius.
K+ has larger radius
The larger the highest energy level, the larger the atomic radius.
The negative ionic radius is larger than the neutral atomic radius
The negative ionic radius is larger than the neutral atomic radius
S has a larger radius. The atomic radius decreases across a period.
Yes Atomic radius of carbon: 60 pm Atomic radius of silicon: 110 pm
For the representative elements (main group elements), atomic radius generally decreases from left to right across a period. Example: B and Fl: Fl has the smaller atomic radius Li and Be: Be has the smaller atomic radius
the larger the highest energy level number, the larger the atomic radius (Apex)
Atomic radius increases down the group. So larger atomic radius are present at the bottom.