Group-14 elements share electrons. they form covalent bonds.
The elements in the group 4A of the Periodic Table include carbon, silicon, germanium, tin, lead and the artificially produced ununquadium. These elements can form ions as they are able to gain and lose electrons.
They do not naturally form ions. According to the Octet Rule each atom will want to get a full outer shell of electrons. Most of the time this is eight electrons. The noble gases already have a full outer shell and therefore will not will not lose or gain electrons. Any loss or gain of electron would not satisfy the octet rule.
Yes, they form positive ions as Zn+2, Ga+3, Sn+2
Group 4 elements, i.e. carbon and silicon, do not form ionic bonds with other elements. Instead, they form covalent bonds.
Yes they do they form +8 ions
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.
For s and p block elements, in groups 1 to 3 the group number is equal to the number of positive charges formed when the element loses electrons, and for groups 5, 6 and 7, the number of negative charges is equal to (8 - group number).
Elements in group 8 all have 8 valence electrons, this is why these elements are in group 8, they are called noble gases, some examples are Argon, Xenon,
none of the elements in the periodic table have a charge unless they gain (- charge) or lose (+ charge) an electron, or they can get delta charges which depends on what they are bonded too, that is what i learned in A2 chem a few monthes agoThe above information is absolutely correct... but here is a bit more information specifically for group 1A elements. All elements in group 1A can have a +1 charge as ions. Group 1A elements, such as sodium (Na), have 1 valence electron in their outer shell. When forming ionic compounds, sodium ions tend to donate this one electron to an element (in ionic form) that has 7 electrons in its outer shell. Thus, satisfying each atoms octet rule (haveing 8 electrons in their outer shell), as well as forming a neutral ionic compound.
Elements in Group 18 already have an octet of electrons, which is a full outer shell of 8 electrons. An octet of electrons makes the element stable, so it does not need to react with any other elements to gain or lose electrons.
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
8
Most of the elements in the top right of the period table (but not "group 8" - the furthest column to the right) will readily form anions (negatively charged ions) that can then form ionic bonds. Examples are O, N, P and S
Most of the elements in the top right of the period table (but not "group 8" - the furthest column to the right) will readily form anions (negatively charged ions) that can then form ionic bonds. Examples are O, N, P and S
It can be. An ion is an atom with more or less electrons than protons. But having 8 valence electrons (simply) means it has a full outer shell. But the noble gases already have a full shell without being an ion.
e kasi gwapo ka. :) pa-add sa fb! ireneoctaviano17@Yahoo.com
they have one valence electron, and they form ions with a 1+ change.they have one valence electron, and they form ions with a 1- charge.they have one valence electron, and they form ions with a 2+ charge.they have one valence electron, and they form ions with a 2- charge.
Most of the elements in the top right of the period table (but not "group 8" - the furthest column to the right) will readily form anions (negatively charged ions) that can then form ionic bonds. Examples are O, N, P and S
The octet rule states that all elements form ions to reach 8 valance electrons, or the nearest noble gas. If an element is a noble gas, it already has 8 valance electrons, therefore does not need to form ions to bond with other ions, thus becoming un-reactive.
Most of the elements in the top right of the period table (but not "group 8" - the furthest column to the right) will readily form anions (negatively charged ions) that can then form ionic bonds. Examples are O, N, P and S
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.
For s and p block elements, in groups 1 to 3 the group number is equal to the number of positive charges formed when the element loses electrons, and for groups 5, 6 and 7, the number of negative charges is equal to (8 - group number).