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As you go across a period; Left to right, the electron affinity increases. As you go down a group; top to bottom, the electron affinity decreases.
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What trend is oberserved among the atomic radii of main-group elements down a group. eplain this trend?
The trend of atomic radius increases down a group on the periodic table. This occurs because each successive element down a group has another energy level. As more electrons are added, more energy levels are needed to hold the electrons.
What causes this trend for it to go down on the periodic table?
As you move down the periodic table, atomic size increases due to the addition of electron shells. This increase in distance between the nucleus and the outermost electrons results in a decrease in effective nuclear charge felt by these electrons, which in turn affects properties such as ionization energy and electronegativity, often leading to a downward trend in these values. Additionally, increased electron shielding by inner-shell electrons reduces the attraction between the nucleus and outer electrons, contributing to this trend.
How do you account for the general trend in atomic radius across a row of elements?
The general trend in atomic radius across a row of elements decreases from left to right due to increasing effective nuclear charge, which attracts the electrons closer to the nucleus. As you move across a period, the number of protons in the nucleus increases, resulting in a stronger pull on the electrons and a decrease in atomic radius. Additionally, the shielding effect of inner electrons remains relatively constant, further contributing to the trend.
What is the Periodic Trend For Electronegativity Is Similar To What Other Trend?
The periodic trend for electronegativity is similar to the trend for ionization energy. Both increase across a period from left to right due to the increasing nuclear charge, which attracts electrons more strongly. Additionally, both trends decrease down a group as the distance between the nucleus and valence electrons increases, resulting in weaker attraction. Consequently, elements in the upper right corner of the periodic table, such as fluorine, exhibit the highest electronegativity and ionization energy.
Which property has a trend similar to that of electronegativity?
First ionization energy has a trend similar to that of electronegativity.
What is the trend of oxidation numbers in the periodic table?
Oxidation numbers generally become more positive from left to right across a period and more negative down a group on the periodic table. This trend is due to changes in the number of valence electrons as you move across and down the table, impacting how likely an atom is to gain or lose electrons.
How does the electronegativity trend explain the first ionization energy trend?
The electronegativity trend and the first ionization energy trend both increase as you move from left to right across a period in the periodic table due to the increasing effective nuclear charge. Higher electronegativity indicates a stronger pull on electrons, making it harder to remove an electron, thus increasing the first ionization energy.
Is a trend across a period similar or different for periods 2 3 4 and 5?
Similar for they have the same number of electrons in the last shell
Does the s or d shell lose electrons first?
In general, when the transition metals lose electrons, the s shell electrons are lost before the d shell electrons. This is because the s electrons are higher in energy when the atom is in its ionized state. For example, in elements like iron (Fe), the 4s electrons are lost first, followed by the 3d electrons. This trend is observed across the periodic table, particularly in transition metals.
Why are the noble gases not included in the trend in ionization energy?
Noble gases have stable electron configurations with a full valence shell, so they have a high ionization energy. Their ionization energy values don't follow the typical trend due to their unique electron structure, which makes them less likely to lose or gain electrons easily compared to other elements.
What explains the observed trend in the atomic radii going down the periodic table?
The more energy levels that are occupied by electrons, the larger the atomic radius.
What trend does the ionization energy follow going across the periodic table?
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
