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Answer Expert Verified. The second choice is the one that accurately captures the trend in electron affinity. “It tends to be more negative across a period” is the correct way to phrase the trend. The atom has a greater propensity for accepting more electrons in proportion to the negative value of its electron affinity.
What kind of a pattern is observed for the electron affinity?
What kind of a pattern is observed for the electron affinity? Electron affinity grows higher across the periods of a periodic table for the groups and from left to right because the electrons added to the energy levels go closer to the nucleus, which makes the nucleus and its electrons more appealing. This results in an increase in electron affinity.
In terms of electron affinity, which of the following statements is accurate?
Because of this, the proper sequence of electron affinity is as follows: Cl > F > Br.
What are the current trends in electron affinity, and what can we anticipate for the future of these trends?
What are the general tendencies and, more importantly, the exceptions to the general tendencies in electron affinity? The elements in Group 17 have electron affinities that are significantly greater and more negative than those of the elements in Group 1. The electron affinities of the elements in Group 14 are greater (more negative) than those of the elements in Group 15.
How does the electron affinity change as you move from group to group lower on the periodic table? Why?
Generally speaking, the electron affinity will decrease as one moves down a group. This is due to the fact that as one moves down the period table, additional valence shells are introduced, which results in an increase in the atomic radius. Because the new orbital is further away from the nucleus, the attraction between the positively charged nucleus and the new electron is weaker. This is because the nucleus is positively charged.
Basic Introduction, Electron Affinity Trend, and Chemistry
We found 15 questions connected to this topic.
What is the pattern that emerges when one moves down a group in terms of the electron affinity?
Electron affinity decreases down the groups and from right to left across the periods on the periodic table because electrons are placed in a higher energy level further away from the nucleus, resulting in a decrease from the nucleus’s pull. This is because higher energy levels correspond to greater distances.
How does the length of the period affect the electron affinity of a group?
In the periodic table, electron affinity tends to rise from one period to the next, but it can sometimes decrease as one moves down a group. These tendencies do not necessarily hold true everywhere. The increased effective nuclear charge that occurs throughout a period and up a group is the chemical rationale behind the changes that occur in electron affinity as one moves down the periodic table.
What kind of pattern is emerging with EA moving down a group?
A member of the group
The electron affinity goes down as a result of: As a group is subtracted from an atom, additional energy levels are added to it. E- Go further away from the center of the atom. Because of this, elements that are lower down in a group do not exert the same level of pull on other elements as those that are higher up in a group.
When you walk down a column, do you notice a pattern developing in terms of the electron affinity?
By looking at the periodic table, one will see that the atomic radius grows from top to bottom as one moves down a column. Because of this, the electron affinity grows from the bottom of the column to the top of the column.
Which element would have the greatest attraction for electrons and why?
When compared to the other elements, the electron affinity of chlorine is the highest. Because of its huge atomic radius, or size, it has a strong electron affinity, which can be linked to its size. Due to the fact that the electrons in chlorine’s outermost orbital are 3p, they have a significant amount of space that they can share with an incoming electron.
Which of the following best describes the general pattern of electron affinity in halogens?
Since the size of an element grows larger as we proceed downward within a group, this explains why. Hence, the ability to store electrons is reduced, which results in a decrease in electron affinity. Thus, the following should be the order of electron affinity for these electrons: As > I > Br > Cl > F.
Which of the following orders for electron affinity is correct: a/s O se B Cl F c/s O d/o s’e n p f/c n Which of the following orders for electron affinity is correct?
The orders a, b, c, and f are the ones that should be followed, however the orders d and e are the wrong ones. Because of an increase in the effective nuclear charge, the electron affinity of a substance gradually becomes less positive as the atomic number of the substance increases over time.
N or P: Which element has a higher electron affinity?
Carbon has a higher propensity for accepting an electron than nitrogen does because a “p” subshell that is just half filled is more stable.
What kind of pattern do electrons follow?
As one moves from left to right over a period, the forces of attraction become stronger, which causes the atoms to shrink to smaller and smaller sizes. Because of this, the electron moves closer to the nucleus, which ultimately results in an increase in the electron affinity over a period and from left to right. Within a period, electron affinity grows from left to right as one moves clockwise.
What does the long-term pattern look like for the values of ionization energy and electron affinity?
Moving from left to right over an element period typically results in an increase in the amount of ionization energy that is present. As one moves over a period from left to right, the atomic radius decreases, which causes electrons to be drawn more strongly to the (nearer) nucleus.
Which element has a stronger affinity for electrons, fluorine or neon?
In the contemporary version of the periodic table, the electron affinity rises as one moves from the left to the right within a period, but it falls as one moves down the group… Because of this, the electron affinity of noble gases is the lowest of any time. As a result, we are able to draw the conclusion that the electron affinity of fluorine (a halogen) in a period is greater than that of neon.
By traveling along a column in the periodic table, one can see which of the following trends?
By traveling along a column in the periodic table, one can see which of the following trends? The mass of the atomic particles grows.
What kind of pattern does the atomic radius follow all the way across the periodic table? Why is this pattern occurring?
What pattern does the periodic table show for the atomic radius as one moves down a group? What factors contribute to this pattern? Because the shielding effect is more powerful than the massive nuclear force, the atomic radius of elements has a tendency to grow larger as one moves down a group. As a result, the nucleus exerts less of an influence on the atom’s electrons, which results in an expansion of the atomic radius.
The electron affinity trend between groups IA and IIA seems to be decreasing; why is this the case?
When electrons are positioned into orbitals with lower energy, closer to the nucleus, electron affinity, which is the energy involved with the formation of an anion, is exothermic, which means that it is more favorable. Because of this, the electron affinity is reduced as one moves down the periodic table from left to right, and it gets increasingly unfavorable as one moves from one group to the next.
How has the atomic radius changed throughout the course of a period?
In general, the radius of an atom gets smaller as one moves across a period and gets larger as one moves down a group. The effective nuclear charge rises during the course of a period, even when the electron shielding does not change.
What kind of an explanation does the trend of electronegativity offer for the initial ionization energy trend?
When there is a higher ionization energy, it is more challenging to remove an electron from a molecule. By applying the same concepts from the theory of Coulombic attraction, we are able to explain the first ionization energy trends on the periodic table… When an atom’s electronegativity is high, it has a strong ability to draw electrons to itself, and this ability increases as the electronegativity increases.
In which equation is the electron affinity of calcium accurately represented?
Hence, in order to determine the initial electron affinity of calcium, we will begin with the neutral Ca(g) and, after adding one electron, we will have the anion Ca-(g). This indicates that the correct response is a. Ca(g) + e- Ca-
What exactly are electron affinity and electron gain enthalpy, and how are they related?
Electron affinity refers to the amount of energy that is given off by a neutral atom or molecule (when it is in the gaseous phase) when it receives an electron from the surrounding environment. The term “electron gain enthalpy” refers to the change in enthalpy that occurs when an electron is added to a neutral atom or molecule from an external source.