An element should release two of its outermost electrons to obtain +2 ion. The elements in group 2A are the most likely elements to have this configuration. These are known as Alkali Earth Metals.
The elements in the 2nd group have 2 valence electrons. Elements give away their valence electrons to get stable electron configuration. The elements in the 2nd group such as beryllium, magnesium, calcium, strontium, barium likely to have positive ion with charge of 2.
Group II elements (the alkaline earth metals). This is because this particular group of elements have two extra electrons in their electronic configurations. They need to lose these two electrons to attain the stable noble gas configuration. So they will have a tendency to lose them to other atoms or group of atoms, in the process incurring a double positive charge (since there will now be two less electrons than protons). So Be, Mg and Ca will all form positive ions (cations) with a charge of +2. They are represented by Be2+, Mg2+ and Ca2+ respectively. But, other elements like copper and barium will also form cations of charge +2.
Elements are neutral. Two neutral atoms combine to make a neutral compound. Ions have charges. But two ions, each having a charge of +1, would not combine to make an ion having a charge of +2, because they would repel each other. Positively charged ions combine with negatively charged ions to make neutral compounds.
An element should release two of its outermost electrons to obtain +2 ion. The elements in group 2A are the most likely elements to have this configuration. These are known as Alkali Earth Metals.
The elements in the 2nd group have 2 valence electrons. Elements give away their valence electrons to get stable electron configuration. The elements in the 2nd group such as beryllium, magnesium, calcium, strontium, barium likely to have positive ion with charge of 2.
Group II elements (the alkaline earth metals). This is because this particular group of elements have two extra electrons in their electronic configurations. They need to lose these two electrons to attain the stable noble gas configuration. So they will have a tendency to lose them to other atoms or group of atoms, in the process incurring a double positive charge (since there will now be two less electrons than protons). So Be, Mg and Ca will all form positive ions (cations) with a charge of +2. They are represented by Be2+, Mg2+ and Ca2+ respectively. But, other elements like copper and barium will also form cations of charge +2.
Alkaline earth metals
Be, Mg, Ca, Sr, Ba, Ra
These metals all form ions with a +2 charge and enter into ionic
Group 2 (alkaline earth metals) elements form cations of +2 charge.
Group 16 (oxygen family) elements form anions of -2 charge.
Most likely a group 2 element, such as oxygen, sulphur, etc
Group-2 elements have 2 valence electrons. They can form positive ions with charge 2.
calcium and magnesium
Fluorine is a nonmetal. It is located in group 17 of the periodic table. It tends to obtain an electron to form the fluoride ion.Fluorine is the element with highest electronegativity. So it does not tend to lose electrons. It is in the 17th group of the periodic table.
As you move down a group in the periodic table, the ionic radius tends to increase due to the addition of new electron shells. Across a period from left to right, the ionic radius generally decreases as the increasing nuclear charge pulls the electrons closer to the nucleus, resulting in a smaller radius.
Silicon has a larger atomic radius than bromine. This is because as you move down a group on the periodic table, atomic radius tends to increase. Bromine is located further to the right on the periodic table and has a smaller atomic radius compared to silicon.
Acidity tends to increase from left to right across a period and decrease down a group on the periodic table. Basicity follows the opposite trend, increasing down a group and decreasing from left to right across a period.
Alkali metals group tends to form ions.They give single electron to gain positive charge.For example : Sodium give one electron to become Na+ ion.
halogens or group 17
Fluorine is a nonmetal. It is located in group 17 of the periodic table. It tends to obtain an electron to form the fluoride ion.Fluorine is the element with highest electronegativity. So it does not tend to lose electrons. It is in the 17th group of the periodic table.
It tends to increaseThe atomic radius increases down the group
Group one, not including element 1 (helium) tend to form ions.
It decreases when going down a group.
All elements in the 7th family/group (2nd from the right) on the Periodic Table.
ionic
Non-metal elements tend to gain electrons to achieve a full outer electron shell and become stable. This allows them to attain a more stable configuration similar to the nearest noble gas.
Alkali metals group tends to form ions.They give single electron to gain positive charge.For example : Sodium give one electron to become Na+ ion.
You are good at questions dude
Noble gases tend to be chemically unreactive due to their full outer electron shells, making them stable and less likely to form compounds with other elements.
Maybe there is no pattern...no it fals