An element forms a negative ion when ionized. On what side of the periodic is the element located? Explain Pls
88039
The right side.  Things that ionize into neg ions are ( CL, Flourine, Iodide)  Those colums.
799741
as i have explained with the formation of ionic compounds. this is an ionic compound like table salt (NaCl)\nLithium gives up the one outermost electron to Chlorine which has a stable octet.\nLithium then has just two. Remember, this is the first orbital (s orbital) with a maximum of two electrons.
1094903
Positive ions (Cation) are formed by a neutral atom losing electron(s), and Negative ions (Anion) are formed by atom gaining electron(s).  \n\nThe exact number of electrons an atom gains or loses are predictable.  Atoms gain or lose electrons so that they turn isoelectric with the closest neighboring Noble Gas.
739878
I am not sure what you are asking but the answer could be a monoatomic ion. The positive being a cation and the negative being an anion.\n\nYou might ask over at http://forums.mychemistrytutor.com though.
708251
You should expect a molecular compound to form between N and O (as opposed to an ionic compound).  This is because N and O are both nonmetals.  An ionic compound will form when a metal and a nonmetal combine.  I believe that this is what your question is getting at.
10055
The radius of a positive ion will be smaller than that of a neutral atom.\n\nThe postive ion will be missing an electron that would have otherwise been occupying an orbital on the outside, therefore reducing the size of the atomic radius.
819578
1)  At the centre, you have the nucleus (positively charged) and, around that, there are the electronic orbitals (negatively charged).\n2)  By losing one or more electrons, to produce a cation (positively charged), e.g. Na+, Ca++, Al+++\nOr by gaining one or more electrons, to produce an anion (negatively charged), e.g. Cl-, O--, N---\n3)  An ion.
872496
An ion is an atom or group of atoms that normally are electrically neutral and achieve their status as an ion by loss (or addition) of an electron(s). The simplest ions are the proton (a hydrogen ion, H+, positive charge), and alpha particle (helium ion, He2+, consisting of two protons and two neutrons) . A negatively charged ion, which has more electrons in its electron shells than it has protons in its nuclei, is known as an anion (pronounced an-eye-on) due to its attraction to anodes. A positively-charged ion, which has fewer electrons than protons, is known as a cation (pronounced cat-eye-on) due to its attraction to cathodes. An ion with a single atom is called a monatomic ion, and an ion with more than one is called a polyatomic ion. Larger ions containing many atoms are called molecular ions. The process of converting into ions and the state of being ionized is called ionization. The recombining of ions and electrons to form neutral atoms is called recombination. A polyatomic anion that contains oxygen is sometimes known as an oxyanion .\n\nIons are denoted by a superscript with the sign of the net electric charge and the number of electrons lost or gained, if more than one. For example: H+, SO42−.\n\nA collection of non-aqueous gas-like ions, or even a gas containing a proportion of charged particles, is called a plasma, often called the fourth state of matter because its properties are quite different from solids, liquids, and gases. Astrophysical plasmas containing predominantly a mixture of electrons and protons, may make up as much as 99.9% of the visible universe [1]. The positively charged proton is about 1836 times more massive than the negatively charged electron.
798559
positive ions are formed by removing electrons from the atoms and hence the ionic radius for positive ion is always less than that of atomic radius
694929
The alkali metals, also known as Group 1.  They are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr).  The single valence electron is so easily given away that the elements lower down in the group react explosively with water.  Because they are so highly reactive, they are not found in elemental form in nature, only as ionic compunds.  They are stored under mineral oil to prevent reactions with the moisture in air.\n\nHydrogen is also in Group 1, but its single electron is held very close to the nucleus (a single proton), which means that the electron is not easily given away.  Hydrogen can form a positive or negative ion, because it can also easily accept a second electron to fill its valence shell.  Thus, it is not an alkali metal and is not a member of the family you are asking about.  However, under extremely high pressure, as occurs near the core of Jupiter, hydrogen does take on a metallic structure and behaves as an alkali metal.
473338
It's all the elements in the d-block of the periodic table. Basically, the group starting from column three to column twelve. These transition metals commonly have many oxidation states and have either partially filled d-orbitals or full d-orbitals (like mercury). They also form complex ions quite readily.\n\nIf all of that doesn't make sense, just remember it's the metals in that "lowered" part in the middle.
696955
larger...a negative ion has an electron added that the neutral atom does not have.
783373
This depends on how many electrons the element has to lose or gain to complete its outer layer. If the element is on the right side of the periodic table then it will gain electrons. The left side will lose electrons. How many electrons can be determined by how far away the element is from the nearest side of the periodic table.\n\nTHere is of course more technical depth to this however this thumb rule will do. For more info type ionisation into wikipedia. that should help...
873114
→ Atomic radius decreases → Ionization energy increases → Electronegativity increases →\n\nIn general, the degree of electronegativity decreases down each group and increases across the periods, as shown below. Across a period, non-metals tend to gain electrons and metals tend to lose them due to the atom striving to achieve a stable octet. Down a group, the nuclear charge has less effect on the outermost shells. Therefore, the most electronegative atoms can be found in the upper, right hand side of the periodic table, and the least electronegative elements can be found at the bottom left. \n\nGenerally speaking, atomic ionization energies decrease down a group of the periodic table, and increase left-to-right across a period. Ionization energy exhibits a strong negative correlation with atomic radius.
911430
Cations are positive.\nAnions are negative.
980772
A negative ion will be larger than the atom; a positive ion will be smaller than the atom.
813548
The answer is a) Krypton.\n\nThe bromide anion exists as Br-.\nWith the single negative charge, you know that it has an extra electron, therefore it's electron config is like the noble gas nearest to it on the periodic table: krypton.