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The electrons in the atom surround the nucleus, and the higher the atomic number of the element the more electrons there are. Unless it is ionised, there will be an equal number of protons in the nucleus and electrons surrounding the atom. Ideas of how the electrons are arranged have evolved from imagining them to be in orbit around the nucleus, like a small solar system, to modern ideas of quantum physics where it is best to imagine them as an electron 'cloud'. However the idea of electron shells is still useful, this is as imagined by Bohr in the twenties of the last century, where concentric shells contain fixed numbers of electrons according to strict rules on their composition. Your query on 'electron shielding' is probably to do with these electron shells, and the more shells there are determines the effective size of the atom. You can read more in the link below
What else can I help you with?
What happens to the atomic radius when an electron is gained?
The negative ionic radius is larger than the neutral atomic radius
The addition of electron shells results in?
The addition of electron shells results in more shielding of electrons from the nucleus.
Why do trend happen in atomic radius?
Trends in atomic radius occur due to changes in the number of electron shells surrounding the nucleus as you move across a period or down a group in the periodic table. As you move across a period from left to right, the effective nuclear charge increases, pulling the electrons closer to the nucleus, decreasing the atomic radius. When moving down a group, additional electron shells are added, increasing the atomic radius due to more electron shielding of the outer electrons.
Elements like francium located at the bottom of a group have a lower attraction for their valence electrons because they have a?
higher atomic number and larger atomic size, causing their valence electrons to be farther away from the nucleus, resulting in a weaker attraction. Additionally, the shielding effect of inner electron shells reduces the effective nuclear charge felt by the valence electrons, further decreasing the attraction.
What happens to the atomic radius when an electron is lost?
the positive ionic radius is smaller than the neutral atomic radius
How does electron shielding explain why it is easier to remove an electron from rubidium than from lithium?
In rubidium, having a larger atomic radius, the attraction force between the atomic nucleus and and the electron from outermost shell is lower.
Why does indium have the largest atomic radius?
Indium has the largest atomic radius among elements in its period because of the shielding effect. With more electron shells, the outer electrons are further from the nucleus, resulting in a larger atomic radius.
What happens to the atomic radius when an electron is gained?
The negative ionic radius is larger than the neutral atomic radius
The addition of electron shells results in?
The addition of electron shells results in more shielding of electrons from the nucleus.
When atoms gains electrons what happens to the atomic radius?
The negative ionic radius is larger than the neutral atomic radius
What do you notice about atomic radius as you look down a group?
Atomic radius generally increases as you look down a group in the periodic table. This is because each successive energy level is farther from the nucleus, leading to larger atomic radii. Additionally, electron shielding by inner electron levels increases, reducing the effective nuclear charge and allowing the outer electrons to be further from the nucleus.
Can you describe the trend in the atomic radius in group 1A?
Atomic radius always INCREASES as you move DOWN the periodic table (simply due to increasing number of electron shells). Atomic radius (sort of counter intuitively) DECREASES as you move ACROSS the periodic table. This is because increasing the number of protons (ie positive nuclear charge) causes electrons in the same energy level to "shrink" toward the nucleus.
Why do trend happen in atomic radius?
Trends in atomic radius occur due to changes in the number of electron shells surrounding the nucleus as you move across a period or down a group in the periodic table. As you move across a period from left to right, the effective nuclear charge increases, pulling the electrons closer to the nucleus, decreasing the atomic radius. When moving down a group, additional electron shells are added, increasing the atomic radius due to more electron shielding of the outer electrons.
Elements like francium located at the bottom of a group have a lower attraction for their valence electrons because they have a?
higher atomic number and larger atomic size, causing their valence electrons to be farther away from the nucleus, resulting in a weaker attraction. Additionally, the shielding effect of inner electron shells reduces the effective nuclear charge felt by the valence electrons, further decreasing the attraction.
What happens to the atomic radius when an electron is lost?
the positive ionic radius is smaller than the neutral atomic radius
What has a larger atomic radius sodium or potassium?
Potassium has a larger atomic radius than sodium. This is because as you move down a group in the periodic table, atomic size generally increases due to additional electron shells being added, leading to increased electron-electron repulsion and a larger atomic radius.
Is there a correlation of electron affinities to atomic radii?
The relation between electron affinity and atomic radius is inversely proportional.
