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.
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.
The noble gases, column 18 in a wide form periodic table.
It tends to increase. As you go down a group, the outer electron gets further away from the nucleus and is thus not held as tightly which makes it more available and thus reactive.
Group that tend to form -1 ions include group VIIA
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
Elements on the right of the periodic table but not in group 0/8 tend to gain electrons. Those in group 7 tend to gain 1 electron and those in group 6 tend to gain 2.
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
The noble gases, column 18 in a wide form periodic table.
Maybe there is no pattern...no it fals