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What has a a greater effect on atomic size nuclear charge across a period or increase occupied energy levels withen a group?
The increase in nuclear charge across a period has a greater effect on atomic size than the increase in occupied energy levels within a group. As you move across a period, the effective nuclear charge increases, pulling electrons closer to the nucleus and resulting in a decrease in atomic size. In contrast, while adding occupied energy levels down a group increases atomic size, the effect of increased nuclear charge across a period is more significant in reducing atomic radii. Thus, nuclear charge plays a more crucial role in determining atomic size within a period.
Why does Fr have the largest atomic radius?
Many energy levels of electrons and low effective nuclear charge/low Coulombic force.
What effect on atomic size is more significant an increase in nuclear charge across a period or an increase in occupied energy levels within a group?
An increase in nuclear charge across a period has a more significant effect on atomic size than an increase in occupied energy levels within a group. As the nuclear charge increases, the attraction between the positively charged nucleus and the negatively charged electrons strengthens, pulling the electrons closer and resulting in a decrease in atomic size. In contrast, while the addition of energy levels down a group increases atomic size due to greater electron shielding and distance from the nucleus, the effect of increased nuclear charge across a period is dominant in reducing atomic size.
What is the reason for the periods on the periodic table?
The periods on the periodic table represent the horizontal rows that indicate the energy levels of electrons in an atom. As you move from left to right across a period, the atomic number increases, and electrons are added to the same principal energy level. This arrangement reflects trends in chemical properties and reactivity, with elements in the same period showing gradual changes in characteristics due to their increasing nuclear charge.
How many energy levels in a astatine?
Astatine has multiple energy levels, but the exact number depends on the context in which you are referring to them. In an atom, astatine can have multiple electron energy levels based on its electron configuration. In a nuclear context, astatine isotopes may have different energy levels related to their nuclear structure and decay modes.
Why does the atomic size decrease as you go from bottom to top?
The nuclear charge increases and electrons are added to successively higher principal energy levels.
How are principle energy levels and energy sub levels related?
Principal energy levels are an atom's major energy levels, ranging in value from 1 to 7. Energy sublevels are contained within principal energy levels, and their number increases as the value of the principal energy level increases.
What has a a greater effect on atomic size nuclear charge across a period or increase occupied energy levels withen a group?
The increase in nuclear charge across a period has a greater effect on atomic size than the increase in occupied energy levels within a group. As you move across a period, the effective nuclear charge increases, pulling electrons closer to the nucleus and resulting in a decrease in atomic size. In contrast, while adding occupied energy levels down a group increases atomic size, the effect of increased nuclear charge across a period is more significant in reducing atomic radii. Thus, nuclear charge plays a more crucial role in determining atomic size within a period.
Why does Fr have the largest atomic radius?
Many energy levels of electrons and low effective nuclear charge/low Coulombic force.
What effect on atomic size is more significant an increase in nuclear charge across a period or an increase in occupied energy levels within a group?
An increase in nuclear charge across a period has a more significant effect on atomic size than an increase in occupied energy levels within a group. As the nuclear charge increases, the attraction between the positively charged nucleus and the negatively charged electrons strengthens, pulling the electrons closer and resulting in a decrease in atomic size. In contrast, while the addition of energy levels down a group increases atomic size due to greater electron shielding and distance from the nucleus, the effect of increased nuclear charge across a period is dominant in reducing atomic size.
What is the term used to label the energy level of electron?
Principal quantum numbers (n).
How does the effective nuclear charge change as you move down a group in the periodic table?
As you move down a group in the periodic table, the effective nuclear charge generally decreases. This is because the number of energy levels or shells increases, leading to more shielding of the outer electrons from the positive charge of the nucleus.
What electron in a - sub shell experiences the greatest effective nuclear charge in a many electron atom?
The electron in the same subshell with the highest principal quantum number will experience the greatest effective nuclear charge in a many-electron atom, as it will be closest to the nucleus. Additionally, electrons in higher energy levels (with higher n values) experience less effective nuclear charge due to shielding effects from inner electrons.
How many principal energy levels are there in period 1?
only 1
Which principal energy level has no f sublevel?
The first two principal energy levels (n = 1 and n = 2) have no f sublevel.
What is the total number of completely filled principal energy levels in an atom of argon in the ground state?
In Neon atom the 10 electrons are present in two principal energy levels, 2 in ist and 8 in 2nd level.
Which electrons will have the higher energy?
Electrons in higher energy levels, further from the nucleus, will have higher energy compared to electrons in lower energy levels. Electrons that are in orbitals with higher principal quantum numbers (n) will have higher energy.
