0
I would have to answer by asking about the ongoing line segment that joins the origin and a variable point in a system of polar or spherical coordinates. What is the length of a radius vector?
Wiki User
∙ 11y ago
Wiki User
∙ 14y agoGenerally, it gets stronger.
Elements like to have a full outer orbit. They have to fill up their inner orbits before they fill up their outer ones.
Toward the left side of the Periodic Table, elements have fewer electrons on their outer orbits, so it is easier for them to give up electrons to acheive a full outer orbit. (By giving up electrons on the outer orbit, it gets rid of the outer orbit, and the full inner orbit now becomes a full outer orbit.)
Toward the right side, the outer orbits have more electrons; they are almost full. It is easier for them to take some electrons to acheive a full outer orbit.
Way on the right, the noble gases, neither want to give up nor take any electrons. They already have full outer orbits.
Wiki User
∙ 15y agoWhen you move across a period beginning with Group 1, electron affinity tends to increase as you move across a period because of the increasing nuclear charge.
Wiki User
∙ 13y agoI believe the electron affinity decreases since when you move left or right, you increase.
Wiki User
∙ 14y agoThe electron affinity (of an element) increases as you move from left to right.
Wiki User
∙ 14y agoElectron affinity tends to inscrease across a group because of more nuclear charge and strength.
By: SYEDA SANA AAMIR
Wiki User
∙ 12y agoAs you move down a group, the electron affinity decreases.
Add your answer:
Earn +20 pts
Halogen with the least-negative electron affinity?
The halogen with the least-negative electron affinity is astatine. Electron affinity and electronegativities decreases down a group. Since astatine is the last halogen located in Group 17 as you move down the column from fluorine, it has the least negative electron affinity.
Why does elctronegativity decrease as you go down a group on the periodic table?
the electron affinity decreases down the group because new electrons continuously add in a outer shells that are far away from nucleus,so these electrons are less attracted to the nucleus and that's why releases less energy when added
Why do metals in Group 1 get more reactive nearer the bottom of the Group?
The reactivity of an element largely depends on its electronic configuration. All the 1st group elements have one electron each in the outer most s-orbital. Their reactivity is due to the loss of this electron and formation of a uni positive ion. The ease with which the element loses the electron dictates its activity. As we go down the group, the distance between the outer most orbital and nucleus increases and hence the ease with which the element loses the electron increases as we go down the group. So naturally the reactivity increases. However in the case of 7th group elements(halogens) the electronic configuration is s2p5. They acquire stability by acquiring another electron. This is called electron affinity. This increases as we go up a group. So we find the more reactive element at the top of the group. We can generalize this like this. The reactivity of an element depends on the ease with which it acquires the nearest iner gas electronic configuration.
Why does the reactivity of the group 17 increase as you go down the group?
that's because.... group 1 (e.g Na, K) those tend to lose one electron to gain noble gas electron configuration. they can achieve that by just losing one electron from their outer shell. as you go down the group 1, element gets bigger in size, which means there is more space between nucleus (which is in center of atom) and electron of outer shell. the more far away they are the less attraction force between them. so its easier for potassuim to lose one electron than for lithuim. so that means potassium will easily give up 1 electron to react with non metal or other element therefore it is more reactive than lithuim but in case of non metal, the opposite happens but simple to understand. as you go down the group 7 (halogen- Cl, Br, I) element will get bigger therefore force between nucleus and outer electron is getting smaller. they have to gain 1 electron in order to fill the outer shell (to gain noble gas electron configuration.) as florine is more smaller in size than clorine it is more reactive because florine has more tendency to pull extra electron from metal or other element towards its side. so it easily gain 1 electron to react. .... its very simple once you understand....
Why basic character of alkali metals increases down the group?
Basic character depends upon electron loosing tendency of an element which increases down the group,SO basic character of alkali metals increases down the group
Halogen with the least-negative electron affinity?
The halogen with the least-negative electron affinity is astatine. Electron affinity and electronegativities decreases down a group. Since astatine is the last halogen located in Group 17 as you move down the column from fluorine, it has the least negative electron affinity.
What are the trends and exceptions to the trends in electron affinity?
Down the group electron affinity decreases Across a period electron affinity increases. However, it should be noted that chlorine is having higher electron affinity than flourine due to the small size of fluorine atom)
What is the trend for electrons?
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.
What is electron affinity . write down its trend in periods and group?
The electronegativity increase in a period from left to right; in a group decrease by descending.
What happens as we move down columns on the periodic table?
As you move down a column (group) in the periodic table, the electronegativity decreases, the ionization energy decreases, the electron affinity decreases, and the atomic radius increases.
Why does chlorine have more electron affinity than fluorine although it is below fluorine in periodic table?
Generally electron affinity goes up as you go from left to right across the periodic table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine.(Note that the most electronegative element is fluorine however; 'electronegativity' is not exactly the same as 'electron affinity'.)Electronegativity is the ability of an atom in a molecule to draw bonding electrons to itselfElectron affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.The reason that the electron affinity is not as high as might otherwise be predicted for fluorine, is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).
Why is the electron affinity for clorine is greater than the electron affinity for iodine?
Generally electron affinity goes up as you go from left to right across the periodic table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine.(Note that the most electronegative element is fluorine however; 'electronegativity' is not exactly the same as 'electron affinity'.)Electronegativity is the ability of an atom in a molecule to draw bonding electrons to itselfElectron affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.The reason that the electron affinity is not as high as might otherwise be predicted for fluorine, is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).
What happens to the energy of the electron as it falls down the electron transport chain?
pie
Why the electron affinity of fluorine is less than that of chlorine?
Generally electron affinity goes up as you go from left to right across the Periodic Table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine (note that the most electronegative element is fluorine however).The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).Note that there are a number of other exceptions to the general rule of electron affinity increasing towards the upper right corner -- see the Related Questions links to the left for an explanation of some of those other exceptions.See also the Web Links to the left for more information about electron affinities and the fluorine-chlorine exception.
Why does elctronegativity decrease as you go down a group on the periodic table?
the electron affinity decreases down the group because new electrons continuously add in a outer shells that are far away from nucleus,so these electrons are less attracted to the nucleus and that's why releases less energy when added
Which halogen has the lowest first ionization potential?
The outer electrons in bigger halogens are further from the nucleus and so they feel less attraction and so are easier to remove. Therefore, astatine has the lowest ionisation potential of the halogens.
How do you determine electron affinity?
Measure the equilibrium constant for the reaction of thermal electrons with a species at different temperatures. this has been done with an electron capture detector. another way to measure it is to make a negative ion and shine light on it and measure the energy of the electrons removed by this process Dr.Edward Chen
