Which group of elements wants to give away 2 electrons?
they give them away or share them with group 6 because they need 2 more electrons to have a full outer energy level
Elements in group three basically have THREE electrons in their outtermost orbitals.However, reactivity increases down the group with Thalium(Tl) being the most reactive as its outtermost electrons are further away from the nucleus.These elements react by losing 3 electrons and therefore they all have a valency of +3.
The number of valence electrons determine the chemical properties of a particular element. For example, elements in group 1 tend to donate its valence electron away to produce its stable +1 ion. It also explains the formation of -1 ions from group 17 elements (halogens).
The groups in The Periodic Table of Elements categorize elements according to the number of electrons in the outer shell. Atoms wish to obtain a complete outer shell eg. 2 electrons in the first shell, 8 in the rest. Group 1 elements have 1 electron in the outer shell (valence electrons). To obtain a complete outer shell, the atoms give their electron away. Group 7 elements have 7 valence electrons and require 1 more electron… Read More
you need two atoms depending how many electrons they want to get or get rid of like water hydrogen wants to give away one electron and oxygen wants to get two electrons that is how it becomes H2O
Because the electrons get further away from the nucleus meaning it's much harder to gain another electron which they need to complete the reaction.
Valence electrons are the electrons in the furthest electron shell from the nucleus. For the first three rows, essentially, the number of valence electrons is the number of squares the element is away from the beginning of the row at the left. For example. Sodium is the first (group 1) it has 1 valence electron. Magnesium is the second, it has 2 valence electrons.
Group-2 elements have 2 valence electrons. They can form positive ions with charge 2.
Generally speaking, the metals give away electrons during a reaction. Not all metals are equally reactive, however. The metals of group 1 (the alkali metals) all have 1 valence electron. This 1 electron is given away very easily, making this group the most reactive of all the metals. They are so reactive, in fact, that these elements do not exist by themselves; only in compounds.
The elements that have 5 or more or sometimes 4 electrons tend to need to gain electrons to form an octet, resulting in high electronegativity because they take electrons away from other elements.
An element from group eighteen from the periodic table is commonly referred to as a "noble" or "inert" gas. These elements have filled electron shells, and therefore they do not share, take or give away any electrons. As a group they do not react with othere elements to form compounds (with only a couple of rare exceptions).
The elements in group 16 on the periodic table will form -2 ions. These elements have 6 valence electrons, which means they need 2 more to achieve noble gas electron configuration. When they gain these 2 electrons, they will have a -2 charge (remember, electrons are negative.) Group 16 consists of oxygen and sulfur (far and away the 2 most common), as well as selenium, tellurium, and polonium (a lot less common.)
Why do atoms of group 1 elements lose electrons to form cations where as atoms of group 17 elements gain electrons to form anions?
By doing so, both end up having a noble gas configuration, with 8 valence electrons (known as an octet). They do this to become chemically stable. They become stable as they have filled their outer shell of electrons. Atoms of groups 1 elements have only 1 electron in their outer shells, which means to stabilize themselves it is easier for them to give this one atom away, rather than trying to gain 7 more. Once… Read More
Group 1 elements (alkali metals) want to give away their single electron in a compound to become stable at 8, while the Group 17 elements (halogens) want to gain an electron since they are so close to becoming stable at 8 electrons.
The attraction between the atomic nucleus and electrons is less strong.
Why doatomsof group1elements lose electrons to form cations while of group17 elementsgain electrons to form anions?
Atoms of group1 elements lose electrons because they have a low ionization energy; therefore it is easier for other elements, with a high electronegativity, to pull the single electron away from the group1 atom's valence shell rather than the element in group1, which has a low electronegativity, to pull an electron away from another atom. Atoms of group 17 gain electrons because they have a high electronegativity. Because of their high electronegativity, it is easier… Read More
They are further away from the nucleus.
In the short form: elements are striving to completely fill valence shells of electrons to reach a quantumly stable energy state. They react to take electrons away from elements willing to give up electrons or share outer shell electrons with elements they aren't strong enough to steal from.
What is the best reason that the atomic radius generally increases with atomic number in each group of elements?
The best reason that the atomic radius generally increases with atomic number in each group of elements is that the valence electrons are in a higher principle energy level so they sit farther away than the last energy level.
Calcium is a metal. Metals give away their electrons off to non-metals. So i would say when calcium is combining with another atom it wants to give away its electrons so it can be an ion.
Yes, aluminum is reactive with other elements. Being a metal, it likes to give its outer electrons away to have an empty outer electron shell, and being in the 3A column, it has 3 electrons to give away, so it is quite reactive.
The elements from group 1-13 or IA-IIIA (including all of the B groups) tend to form cations. Related Information: A cation is an element or molecule with a positive charge. This means that the element or molecule has lost one of its original electrons, making it less negative and therefore more positive. So elements that have an affinity to give away their electrons tend to form cations. In order for elements to want to give… Read More
The oxygen, nitrogen, and fluorine groups love to steal electrons from other elements, making them negatively charged ions, whereas most metals up to the carbon group like to give away electrons, making them positively charged ions. I hope that's what you were asking.
Both groups are one electron away from a stable outer shell, group 17 needs to gain one and group 1 needs to lose one.
Fluorine will attract more electrons because it has the highest electronegativity. Carbon does not have a strong attraction because it wants to give away electrons.
when you go down a group you get more shells and in those shell are electrons the further away the electrons are from the protons and neutrons the less energy you need to pull of the electrons.
Short answer; Summary: Total number of electrons - number of valence electrons = number of core electrons ^^ Use electron configuration; MUST be used for transition elements as there are many exceptions to the simple rules of thumb given for these elements. Just stick w/ electron configurations here ;) For MAIN Elemental groups ONLY: Group Numbers (1=1 valence E, 2= 2 valence, 13=3.... 18=8 Valence electrons) Long descriptive answer: By core electons, I presume you… Read More
Francium. This is because it has the most energy levels in the alkali group, and the electrons are farther away from the nucleus. This means that the electrons are more easily taken.
The first ionization energy decreases down a column (group) and increases across a row (period). The first ionization energy decreases when going down a group because with increasing period, the number of electron shells also increase, and therefore the electrons in the valence shells of larger elements are further away from the nucleus and experience more 'shielding' from electrons in inner shells. This means that the nucleus of larger elements would not be able to… Read More
Covalent bonds and ionic bonds, the sharing of electrons, and the giving away of electrons between two elements
The "valence" electrons are responsible for chemical reactions and bonding. Valence electrons are found in the outer most orbital of the atom, farthest away from the nucleus.
as you go down a group the elements become more metallic. why? ionization energy decreases. ionization energy is the amount of energy needed to remove the most loosely held electrons. when electrons are lost, a metal is formed. so as you go down a group, the electrons are futher away from the nuclear pull (because the period increases). therefore, not much energy is needed to remove the electrons making it easier to loose them
Except hydrogen, elements in group 1 are very reactive at they can give away their only electron in their valence shell easily to be ionized.
Why are ionic compounds formed when a metal from the left side of the periodic table reacts with a nonmetal from the right side?
One of the ideas regarding the manner in which atoms bond to other atoms is that atoms want to achieve an electron configuration like that of an inert or noble gas. That is, atoms will borrow or loan out electrons to attain a full outer electron shell. If an atom has just one or two electrons in its outer or valence shell, it will tend to loan them out. And if an atom is one… Read More
Does electronegativity increase or decrease as you move down a group on the periodic table of elements?
Electronegativity will decrease down a group. This happens largely because of the size increase of the atoms down a group. Electronegativity speaks to the ability of an atom to attract extra electrons in a bond. The smaller the atom the closer the nucleus and the positive charges can get to the extra electrons and thus attract them much more strongly than if they were far away from each other like in a bigger atom.
They are held into place by the orbitals where they occupy there time. The nucleus basically hold them into space, which is why smaller elements are more reactive. The big elements lose their electrons easier because the electrons in the outer shells (orbitals) are further away from the nucleus and therefore easier displaced.
Group 18 is the most stable group (the noble or inert gases) because their electron configuration makes it difficult for them to react with other elements. The outer valence shell is completely filled already, so they don't need to share, give away, or take electrons to fill it (and thus react with something else.)
Aluminum is an element. It's on the Periodic Table of Elements in group 3. It is a metal. It becomes an ion when it gives away electrons. It could be considered ionic if it bonded with a nonmetal. For example if it bonded with P (phosphorus) that would be an ionic bond
because they almost always give away a valance electron during bonding
Halogens and noble gases do not conduct electricity. As they do not have extra electrons to give away to conduct electricity.
The reactivity of group 17 elements differ as you move down the periods. Group 17 elements are missing 1 electron from their valance shell making them highly votile and reactive. I'll try not to make this confusing: 1. As elements get bigger, they have a higher level of reactivity. (More "pull" needed from protons in the nucleus in order to keep valance shell electrons in orbit). 2. As you move from left to right in… Read More
they are metals (: they give away electrons instead of taking them in because thats an easier way for them to reach 'atom heaven'
All of the elements in the Alkali and Alkaline Earth groups - Groups 1A and 2A are very likely to give their valence shells electrons away. This includes sodium, hydrogen, calcium, potassium and similar elements.
ionization enthalpy decreases down the group from Li to cs because as we move down a group the number of valence electrons goes increasing separating the electrons away from the nucleus ,there is an increasing shielding of the nuclear charge by the inner shell electrons and thus the removal of electrons requires less energy as we move down.
The bottom left of the periodic table of elements features elements with low ionization energies because of the way the periodic table is set up, by the number of valence electrons (elements farther left are more reactive). It takes very little energy to move the few excess electrons away to other atoms.
The alkali metals, group one on the periodic table. Starts with Lithium (Li) and ends with Francium (Fr). Or at least until Ununnunium is discovered, as it will be thenext alkali metal. The reason for their high reactivity is that they have only one valence electron. Valence electrons are the electrons that are involved in forming bonds with other elements. With only one valence electron, the atomic radius (how far away from the nucleus electrons… Read More
MnCl2 Manganese is two electrons away from becoming a noble gas, in fact it has two too many. Chlorine is one away from becoming a noble gas and needs one electron. So two chlorine atoms would have to come to take (steal) manganese's two electrons. So Mn2+ (has two electrons to give) Cl22- (wants to take two electrons)
the electron affinity decreases down the group because new electrons continuously add in a outer shells that are far away from nucleus,so these electrons are less attracted to the nucleus and that's why releases less energy when added
As you go down a group, a shell is added to the atom with every period. This makes the elements bigger and valence shell away from the nucleus. This reduces the force of attraction between nucleus and the valence electrons and thus, the ionization energy is reduced.
Shielding affect acts as a barrier for proton to attract electrons, therefore the electrostatic force (the which attracts electrons to protons) becomes much less and electrons become further away from the nucleus of the atom. Because of this, the atomic size increases as you move down the group.