0
The group that has a substantial affinity for electrons is group 17, the halogens. These elements have 7 valence electrons which makes them have the highest affinity for electrons.
Wiki User
∙ 9y ago
Wiki User
∙ 11y agoMost of the time group 17 wants to "steal" elctrons because they have one electron missing from their outermost electron cloud and want to fill it
Wiki User
∙ 12y agoAlkali Metals
Wiki User
∙ 11y agoThe halogens in group 17.
Wiki User
∙ 11y agoHalogens
Add your answer:
Earn +20 pts
Why do halogens in group 7 have such have such high electron affinities?
Because they only need 1 electron to get the inert/noble gas structure and thus be extremely stable.
Why do the halogens in group 7a have such high electron in affinities?
Mostly they are highly electronegative and they only need one electron to fill their outer shell in a noble gas octet configuration.
How many valence electron does a group 18 element have?
8
Which group of elements on the periodic table tends to form ions?
Group one, not including element 1 (helium) tend to form ions.
Based on their placement on the periodic table what about ion formation is correct There is more than one correct statement?
A Group 6A element gains two electrons A Group 2A element loses two electrons A Group 3A element loses three electrons A Group 3A element loses three electrons group 1a element loses one electron group 7a gains one electron
Which element group have the most negative electron affinities?
Fluorine flourine is the most electronegative element
Which element has the lowest electron affinity Is it nitrogen?
No, nitrogen does not have a low electron affinity. Electron affinity increases as you go up and to the right on the periodic table. Thus, Groups I and II elements (ex. Cs, Ba, Sr, etc.) have LOW electron affinities and the halogens in Group VII (Br, Cl, F, etc) have the HIGHEST electron affinities. Chlorine has the HIGHEST electron affinity on the periodic table.(Fluorine is an exception in this case.)
Why do halogens in group 7 have such have such high electron affinities?
Because they only need 1 electron to get the inert/noble gas structure and thus be extremely stable.
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)
Why do the halogens in group 7a have such high electron in affinities?
Mostly they are highly electronegative and they only need one electron to fill their outer shell in a noble gas octet configuration.
If an element has 1 valence electron what group is it in?
That element would be in the Alkali Metals (group one)
What element in group 2 is most likely to loose and electron?
radium as the ,negative, electrons in it's outer shell are least affected by the ,positive, nucleus.
Which statement best describe why the halogens in group 7a have such high electron affinities?
C. They gain electrons easily because they are just... that's enough for you to get if right
What are the Every element in group one has one electron in its outer shell Every element in group two has two electrons in its outer shell?
Both statements are true:Every element in group I has one electron in its outer shell andEvery element in group II has two electrons in its outer shell
How many valence electron does a group 18 element have?
8
An element that has the electron configuration Ne3s23p5 is in which period?
It is in group 17.
What is the period block and group of the element with the electron configuration Ar 3d74s2?
the element belongs to 4th period, 9th group, it is a d block element. the element is cobalt
