Group one elements have one valence electron. In order to achieve a "happy" electron configuration, they try to lose this valence electron. Electrons have a negative charge, so once they lose this electron, they have a +1 charge.
Group 1 elements or alkali metals have one valence electron. If they lose this electron, they will get the nearest noble gas configuration and hence they generally tend to form cations with +1 charge.
Elements in Group 7A, or 17, also called the halogens, form 1- ions because they need one more electron to achieve a noble gas configuration and become stable. They have 7 valence electrons, so they easily gain one more to get 8 valence electrons. The additional negatively charged electron changes the atoms to ions with a 1- charge.
Atoms in group 1A are likely to form ions with a +1 charge because they only have one valence electron.
because they have one electron in their outermost shell which can be easily removed and this removing electron form positive ions.
a group that forms anions with a -1 charge
Group IA: +1 charge Group II2: +2 charge Group IIIB: +3 charge Group IVB: +4 charge Group VB: -3 charge Group VIB: -2 charge Group VIIB: -1 charge
Electronegativity generally increases as you move from left to right from group 1 to group 17 on the periodic table. The noble gases in group 18 generally don't have an electronegativity since they generally don't make compounds.
O2- The ionic charge of something can be determined by it's place in the Periodic Table. Elements in groups 1-3 have a positive charge the same as their group number, e.g. Magnesium (Mg) Is in group 2 so its charge is Mg2+ Elements in groups 5-7 have a negative charge equal to their group number -8 e.g. Oxygen is in group 6 (6-8=-2) So its charge is O2- The noble gases (Group 0) do not have an ionic charge.
A polyatomic ion is a group of atoms with a charge.
a group that forms anions with a -1 charge
Elements in group one of the periodic table; Lithium, Sodium, potassium, rubidium, caesium and rubidium, will form ions with a positive charge of one.
Group IA: +1 charge Group II2: +2 charge Group IIIB: +3 charge Group IVB: +4 charge Group VB: -3 charge Group VIB: -2 charge Group VIIB: -1 charge
The halogens, listed in column 17 of a wide form periodic table.
Group 3 and lanthanides.
Electronegativity generally increases as you move from left to right from group 1 to group 17 on the periodic table. The noble gases in group 18 generally don't have an electronegativity since they generally don't make compounds.
Ions such as fluorine always have a Negative charge- when looking at the periodic table you will see groups 8,7,6,5,4 and 3 on the right side. All noble gases in Group 8 have no charge, but going to the left: 7 = -1 charge 6 = -2 charge 5 = -3 charge 4 = -4 charge This only works for nonmetals, not transition metals so be careful. So, looking at Fluorine it is in Group 7 7 Nonmetals always have a -1 charge. 2 Fluorine Ions * -1 = -2 -2 is your answer. When it meets with a positive ion (Groups 1 and 2 on the left side of the periodic table), the two charges will need to balance. So the positive ion will need to be +2. This can happen naturally (positive ions in Group 2 are +2, so 2F and 1Ca will work) or because there are enough positive ions to balance the charge (positive ions in Group 1 are +1, so having 2F and 2Na will work). Good luck :)
Elements from the group 2 of the periodic table form cations.
O2- The ionic charge of something can be determined by it's place in the Periodic Table. Elements in groups 1-3 have a positive charge the same as their group number, e.g. Magnesium (Mg) Is in group 2 so its charge is Mg2+ Elements in groups 5-7 have a negative charge equal to their group number -8 e.g. Oxygen is in group 6 (6-8=-2) So its charge is O2- The noble gases (Group 0) do not have an ionic charge.
A polyatomic ion is a group of atoms with a charge.
they are the cations
Group 2, alkali earth metals.