what is the charge on a typical ion for group 1A? how can i figure out the answear to a question like this.. then group 7A,6A,2A
Group 1A has one electron in the outer orbit, it is lost on ionization, and the charge on the metal ion is +1. Group 7a has seven electrons, it gains one electron (octet rule), so the charge is -1.
how do you know how many electrons the group has?
would group 2A be 2+
Yes
Group IA has 1 electron in its outer shell; group IIA has 2 electrons in its outer shell; group IIIA has 3 electrons in its outer shell; group VIA has 6 electrons in its outer shell ( and needs to gain two more); group VIIA has 7 electrons in its outer shell (and needs to gain one more). The "B" groups don't follow such a nice pattern but at least ONE of the valences of the B elements will be the group it is in; i.e., Ti is in group IVB and one of the common valences of Ti is +4. It also has +3. Cu, Ag, and Au are in group IA and all have valences of +1. Cu also has +2, Ag has no other COMMON valence, and Au also has +3. Zn, Cd, and Hg are in group IIB and all have valences of +2. Zn and Cd have no other common valence but Hg also has +1. I hope this additional informatin is useful.
To figure out the charge on a typical ion for Group 1A, you need to consider the number of valence electrons in the atoms of that group. Group 1A contains elements such as lithium, sodium, and potassium, which have one electron in their outermost shell. When these atoms are ionized, they tend to lose that one electron, resulting in a positive charge of +1 on the metal ion.
For Group 7A, such as fluorine, chlorine, and bromine, these elements have seven electrons in their outermost shell. To achieve a stable and full outer shell, they tend to gain only one electron, resulting in a negative charge of -1 on the ion.
Similarly, for Group 6A, such as oxygen and sulfur, these elements have six electrons in their outermost shell. To achieve stability, they tend to gain two electrons, resulting in a negative charge of -2 on the ion.
For Group 2A, such as beryllium and magnesium, these elements have two electrons in their outermost shell. They tend to lose those two electrons to achieve stability, resulting in a positive charge of +2 on the ion.
Knowing the number of valence electrons for each group is crucial in determining the likely charge on their ions.