Elements in group 1 have 1 electron in their outer shell. Group 7 electrons have 7 electrons in their outer shell. This means that the group 1 element needs to give its electron to the group 7 element so that they both have full outer shells, making them stable. By a school boy in yr. 10
The groups in The Periodic Table of Elements categorize elements according to the number of electrons in the outer shell. Atoms wish to obtain a complete outer shell eg. 2 electrons in the first shell, 8 in the rest. Group 1 elements have 1 electron in the outer shell (valence electrons). To obtain a complete outer shell, the atoms give their electron away. Group 7 elements have 7 valence electrons and require 1 more electron to obtain a complete outer shell. They can receive the electron given from the group 1 elements. This creates a charge in the atoms. Group 1 elements have more protons than electrons and so have a positive charge. Group 7 elements have less protons than electrons and so have a negative charge. The negatively charged atoms (anions) and the positively charged atoms (cations) are attracted to each other.
Hydrogen- a group 1 element, reacts really well with fluorine- a group 7 element. It forms an ionic bond when the anions and cations form a 3D fixed lattice.
The group 1 and 2 elements have much lower electronegativity value than group 17 elements and therefore lose electrons to the group 17 elements. The group 17 elements require only one more electron to have a full valence shell and thereby acquire the stable electron configuration of the next higher atomic number noble gas. The group 1 and 2 elements achieve a stable electron configuration when they lose all their outermost (valence) electrons and thereby acquire the electron configuration of the next lower atomic number noble gas. One group 1 element will combine with one group 17 element and one group 2 element will combine with two group 17 elements. Examples include NaF, and MgCl2.
Group 1 atoms only need to lose 1 electron in order to achieve a noble gas configuration, and group 7 atoms only need to gain 1 electron to achieve a noble gas configuration.
group 1 elements have to 'lose' one electron to fill their outermost shell of electrons
group 7 elements have to 'gain' one electron to complete their outermost shell of electrons
Did you mean group 7 or 17? Well if a group 1 and 7 element reacts it is called a Metal-Metal bond , which can be broken down into three subgroups: covalent, dative, and symmetry. If you ment Group 1 and 17 then it is an Ionic bond.
The elements in group 1 combine easily with other elements to form compounds because they are trying to get rid of their extra electrons. That is why, for example, potassium will react strongly in water. Hope this helps.
there are 7 electrons in the outer energy level of group 17 elements
sodium is of hydrogen family that is group 1 and chlorine is of fluorine family that is group 17
group 1
Francium would react most violently with hydrochloric acid but all of them would react violently. Cesium and Rubidium would certainly react explosively. Potassium would be very violent and catch fire. Sodium would be quite violent.
Groups 1 and 2 are highly reactive.It consist of alkali metals and alkaline earth metals.They react violently with water.
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Group 17 elements are acceptors of electrons and group 1 elements ar donor of electrons.
The alkali metals in group 1 react by losing one electron.
group 1 elements.
Did you mean group 7 or 17? Well if a group 1 and 7 element reacts it is called a Metal-Metal bond , which can be broken down into three subgroups: covalent, dative, and symmetry. If you ment Group 1 and 17 then it is an Ionic bond.
Group 1 and group 2 elements are reactive metals and react readily with water. They also react readily at high temperatures with oxygen. Over the millenia any free deposits would react to form compounds.
Fluorine (F) is the most reactive element. It can react with almost anything.
The elements in Group 1 of the Periodic Table are highly reactive in water, and, only slightly less reactive in Oxygen. Group 2 elements are also quite reactive in Oxygen, but not quite as reactive as those elements in Group 1.
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Group 17 or halogens will combine readily with group 1 elements.