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The electronic configuration of group IIA elements typically ends in "s2", where the outermost electron shell has a full s orbital. For example, the electronic configuration of Calcium (Ca), a group IIA element, is [Ar] 4s2. Other examples include Beryllium (Be) with [He] 2s2, Magnesium (Mg) with [Ne] 3s2, and Strontium (Sr) with [Kr] 5s2.
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Which group 0 2 5 or 7 atoms electronic configuration 3s2 3p5?
The group with the electronic configuration of 3s2 3p5 would be group 7, which is the halogens group. This configuration indicates that the atom has 7 valence electrons, matching the group number.
Why are Group 1 and Group 2 elements found in many compounds but not Group 18 elements?
group 18 has completely filled electronic configuration and hence are stable. group 1 and group 2 have 1 and 2 electrons respectively in their valence shells and needs to lose these to attain completely filled electronic configuration. hence they are reactive.
Why is the noble gases a group of un-relative elements?
because they have completely filled electronic configuration.
Which group does the electron configuration 1s2 2s2 sp6 3s2 3p6 3d1 4s2 belongs to?
The electron configuration 1s2 2s2 sp6 3s2 3p6 3d1 4s2 belongs to the group of transition metals. It is the electron configuration of the element titanium (Ti), which is a transition metal with atomic number 22.
What is the name and number of the group to which argon belongs?
It is in Group O or Group 8. Also known as noble gas, they do not react with other elements as they do not have to react to get a stable configuration.
Which group 0 2 5 or 7 atoms electronic configuration 3s2 3p5?
The group with the electronic configuration of 3s2 3p5 would be group 7, which is the halogens group. This configuration indicates that the atom has 7 valence electrons, matching the group number.
What period and group is 1s22s22p63s23p3 in?
The electron configuration 1s22s22p63s23p3 is in the third period and belongs to the halogen group (Group 17) on the periodic table.
Why is hydrogen grouped with elements in group 1a?
valence electrons and electronic configuration.
Why is hydrogen placed with the element in group 1a?
valence electrons and electronic configuration.
How does the electronic configuration of sodium shows the group and period in the periodic table?
The electronic configuration of sodium is 1s2 2s2 2p6 3s1. The outermost electron is in the 3s subshell, indicating that sodium is in Group 1 (alkali metals) since it has 1 electron in its outermost shell. The period is determined by the highest energy level containing electrons, so sodium is in Period 3.
Why are Group 1 and Group 2 elements found in many compounds but not Group 18 elements?
group 18 has completely filled electronic configuration and hence are stable. group 1 and group 2 have 1 and 2 electrons respectively in their valence shells and needs to lose these to attain completely filled electronic configuration. hence they are reactive.
Why is the noble gases a group of un-relative elements?
because they have completely filled electronic configuration.
What is distinctive about the electronic configuration of the group 2 elements?
They all have 2 electrons in their outer shells.
What elements lack a noble gas electron configuration?
Only group 18 elements have noble gas configuration. All other elements lack a noble gas electronic configuration.
What group in the periodic table is this from 3s2 3p5?
This electron configuration belongs to the group 17 elements, also known as the halogens. The 3s2 3p5 configuration specifically corresponds to the element chlorine (Cl).
Which group does the electron configuration 1s2 2s2 sp6 3s2 3p6 3d1 4s2 belongs to?
The electron configuration 1s2 2s2 sp6 3s2 3p6 3d1 4s2 belongs to the group of transition metals. It is the electron configuration of the element titanium (Ti), which is a transition metal with atomic number 22.
Mention the General electronic configuration of nitrogen group elements?
The general electronic configuration of nitrogen group elements is ns2np3, where "n" represents the valence shell. Each element in this group has 5 valence electrons, with 2 in the s orbital and 3 in the p orbital. This configuration gives these elements similar chemical properties, such as the tendency to form covalent bonds.
