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Does a small atomic radius correspond with a high or low electronegativity?
Wiki User
∙ 7y ago
A small atomic radius corresponds more closely to a low electronegativity.
Wiki User
∙ 7y ago
Wiki User
∙ 7y agoSmall radii low electronegativity.
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What are 3 atoms that have the highest electronegativities?
C.Atoms with a small atomic radiusD.Atoms to the right on the periodic table
How is the radius of an atom related to the atoms attraction for outer level electrons?
As the radius of an atom increases, the attraction between the positively charged nucleus and the negatively charged outer level electrons decreases. This is because the outer level electrons are farther away from the "home base." So, as atomic size (radius) increases, the nucleus has less and less a hold on those outermost electrons. For this reason, cesium (Cs, atomic #55) has very large atomic size and very low electronegativity. Fluorine (F, atomic #9) has very small atomic size but large electronegativity.
How small is uranium or big?
If you think to atomic radius: approx. 170 pm.
What element have the smallest atomic radius?
Atomic Radius gets greater down the periodic table and gets smaller to the right in the periodic table. This means, in order of atomic radius, that the five smallest elements are Helium, Neon, Fluorine, Oxygen, and Hydrogen in that order. Check all of it out at http://www.ptable.com/ under properties>radius
Elements, like calcium, located toward the top of a group have a high attraction for their valence electrons because they have a _?
small atomic radius.
Electronegativity increases when atoms .?
B. are located on the right on the Periodic TableC. have a small atomic radius
Why does fluorine form only one oxoacid?
Unlike the other halogens, fluorine can only bond with one oxygen atom because of its small atomic radius and high electronegativity.
Is polonium big or small?
If you think to the atomic radius the empirical atomic radius of polonium is 168 pm.
Elements like francium located at the bottom of a group have a lower attraction for their valence electrons because they have a?
large atomic radius.large atomic radius.
Does francium have a small radius?
The covalent atomic radius of francium is 260 pm and this value is not small.
What are 3 atoms that have the highest electronegativities?
C.Atoms with a small atomic radiusD.Atoms to the right on the periodic table
How is the radius of an atom related to the atoms attraction for outer level electrons?
As the radius of an atom increases, the attraction between the positively charged nucleus and the negatively charged outer level electrons decreases. This is because the outer level electrons are farther away from the "home base." So, as atomic size (radius) increases, the nucleus has less and less a hold on those outermost electrons. For this reason, cesium (Cs, atomic #55) has very large atomic size and very low electronegativity. Fluorine (F, atomic #9) has very small atomic size but large electronegativity.
Why is the electronegativity of galilium higher than that of aluminum?
Gallium, and geranium for that matter, have higher electronegativity's than aluminum (and silicon) because of their d-block contraction. The 3d-electrons do not shield the increased nuclear charge on these elements in the fourth period after the first row of transition metals. This gives them an unusually small atomic radius and a higher electronegativity.
How small is uranium or big?
If you think to atomic radius: approx. 170 pm.
What element have the smallest atomic radius?
Atomic Radius gets greater down the periodic table and gets smaller to the right in the periodic table. This means, in order of atomic radius, that the five smallest elements are Helium, Neon, Fluorine, Oxygen, and Hydrogen in that order. Check all of it out at http://www.ptable.com/ under properties>radius
Why does electronegativity change?
Electronegativity changes from atom to atom because the force between the protons in the nucleus and the electrons in the outer shell changes from atom to atom. This changes because as you move from left to right on the periodic table each additional electron added is not dignificantly farther away from the nucleus but the charge in the nucleus increases so it attracts that electon with a greater force. As you move from the top to bottom of the periodic table the electronegativity decreases because as you move from one period down to the next the energy levels of the outer electrons increase, and so does their distance from the nucleus. The farther away the electron from the protons the less force there is between them.
Elements, like calcium, located toward the top of a group have a high attraction for their valence electrons because they have a _?
small atomic radius.
