No, maybe, probably, hopefully, yes, absolutely, then again, um, sure?
what are true about cationA.Metals are not likely to form cations.B.Cations are always smaller than the neutral form of the element.C.Cation size decreases as you go down a group.D.All cations are larger than any anion.E.Cations cannot form in nature.
Both thermal conductivity and electrical conductivity tend to be higher in metals than in most other materials.
Non-metals tend to not conduct heat
Boron, Krypton,Neon, and Radon Krypton, Neon and Radon do not gain electrons. Because an atom wants to have eight electrons in their valence shell or their outermost shell, and Krypto, Neon and Radon are Noble Gases which already have eight in their valence shells, so they don't lose or gain electrons. And as for Boron it want's to gain 5 electrons because it only has three in its valence shell.
A halide ion is a halogen atom bearing a negative charge. The halide anions are Flouride (F-), Chloride (C-), Bromide (Br-), Iodide (I-) & Astatide (At-) such ions are present in all ionic halide salts.
It is possible to make positive ions of nonmetals e.g. oxygen, chlorine, by putting enough energy into them. They normally form negative ions when in a spontaneous reaction.
The metals and non metals which tend to form positive ions are cations. It is because of their electronic configuration.
Nonmetals tend to attract electrons to become negative ions.
Non-ionized (stable) nonmetals, or metal ions.
The three classes of periodic elements are:Metals,that usually tend to lose electrons to form positive ions.Semi-metals or MetalloidsNon-metals,that usually tend to accept electrons to become negative ions.
Metals typically have the following physical properties: a lustrous appearance, the ability to change shape without breaking, and excellent conductivity of heat and electricity. Nonmetals typically do not have these physical properties, although there are some exceptions. However it is the chemical difference that really counts. Metals tend to lose electrons to form positive ions, and nonmetals tend to gain electrons to form negative ions.
On the periodic table, Groups 4 - 7 tend to form negative ions. These groups tend to gain electrons, thus forming negative ions.
Metals are positive ions. Everything on the left side of the periodic table is. Basically every element that has 4 valence electrons or less is a positive ion.
The fundamental difference between metals and nonmetals is that metals tend to lose electrons in chemical reactions, and nonmetals tend to gain electrons in chemical reactions (not including the noble gases which are also a type of nonmetal and which are not reactive). In terms of physical properties, metals have a distinctive metallic appearance, shiny and silvery; they are good electrical conductors, they are flexible (although it is possible to formulate less flexible alloys) and usually solid, except for mercury which is liquid. Nonmetals come in other colors, are generally not good electrical conductors, and come in a variety of phases, solid, liquid, or gas.
Non-metal atoms gain an electron, or electrons, from another atom tobecome negatively charged ions. (i.e. anion)You can visit igcsechem.webs.com (advanced) or ks3science.webs.com (basic) to learn more chemistry!
Metals tend to form cations, or ions with a positive charge. Nonmetals tend to form anions, or ions with a negative charge. Remember that ions form to put the element in noble gas configuration with 8 valence electrons. Elements forming ions will take the most direct addition or subtraction of electrons to achieve this.
nonmetals form anions (negative ions). for a more thorough answer, they tend to form negative ions because they have high electron affinity (strong ability to attract electrons) and high ionization energy (very hard to take it's electron) and because metals have low electron affinity (attract electrons weakly) and low ionization energy (very easy to take it's electron), thus, the metal readily gives up it's electron and the nonmetals readily receive it to form negative ions.