How many valance electrons do atoms in group 1 group 2 and groups 15 to 17 have?
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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 they have given the electron away there are more protons than electrons in the atom and so the atom become positively charged: a cation. The reverse of this applies for group 17 - it is easier for them to gain electrons, thus becoming negatively charged and an anion. ( Full Answer )
How do the outer-shell electron configurations for ions of elements from groups 1 and 2 and 15 and 16 and 17 compare with those of the noble gases?
Answer . Elements in Group 1 have 1 more electron than the noble gas in the row above it. Elements in Group 2 have 2 more electrons than the noble gas in the row above it. Elements in Group 15 have 3 less electrons than the noble gas in the same row as it. Elements in Group 16 have 2 less ele…ctrons than the noble gas in the same row as it. Elements in Group 17 have 1 less electrons than the noble gas in the same row as it. ( Full Answer )
The atoms in Group 17 elements gain electrons to form anionsbecause they are trying to get 8 electrons in their valence shells.If they gain an extra electron they will have an octet.
Group One on the periodic table consists of. Li - Lithium . Na - Sodium . k - Potassium . Rb - Rubidium . Cs - Cesium . All of these elements all have plus one (+1) valence electrons which means they have one too many so they will give it up when bonding occurs.
Alkali metals (Group 1) donate one electron (per atom) to one atom of Halogens (Group 17)
Group 5A elements are in the fifteenth column, comprising nitrogen,phosphorous, arsenic, antimony, and bismuth. The outer shellcontains valance electrons.
Barium BA is in Group 2 Recall that atoms in Group 1 lose one electron to form ions with a 1 charge What type of ion does barium probably form?
barium will lose two electrons to form an ion with a plus 2 charge. Thus, the resulting ion in reactions of barium is Ba2+. Read more: http://wiki.answers.com/What_type_of_ion_would_barium_form_if_group_1_loses_one_electron_to_form_ions_with_a_1_plus_charge#ixzz17vdoXVSf .
The chemical properties of elements in group 1 (the alkali metals) are:\nThey are the most reactive metals therefore they are always found in compounds in nature. Reactivity increases as atomic number increases, due to a lower IE (ionization energy).\nThey react with elements in group 17 to give the… general formula MX (M is the metal and X represents any members of group 17. \nM + X --> MX\nExample\nNa + Cl --> NaCl\n. \nThe chemical properties of elements in group 17 (the halogens) are:\nIt is the only group that contains all three phases of matter.\nThey occur in nature only in compounds because of their high reactivity. Reactivity decreases as atomic number increases due to lower electronegativitie ( Full Answer )
If the atoms are of the same element, it is called, I believe, a molecule.. If it is of two or more different elements, it is called a compound.
elements of group 6 - colloum 10 gain 2 valence electrons when they form ionic bonds
Both groups are one electron away from a stable outer shell, group 17 needs to gain one and group 1 needs to lose one.
Their valance electrons form an octet. Each compound wants to have 8 valence electrons (which forms an octet). Groups 1 and 2 have 1 and 2 valence electrons respectively. 16 and 17 have 6 and 7 respectively. So together, they form 8..
Why do atoms of group 1 elements lose electrons to form cations where as atoms of group 17 elements gain to form anions?
Because in each instance that is the lowest energy ion that the element can form. This is correlated with developing an electron shell structure like that of the noble gas with the atomic number closest to the atomic number of the element. PORKE MAMEAN MUCHA VERGA HAHAHA PINNCHII CULEROS
The ionic charges of group 1 and 2 metals are +1 and +2respectively. Group 15 & 16 the simple mono-atomic ions are -3and -2. Group 17 ions are -1. This can be explained by thefollowing elemnts in groups 1 and 2 lose 1 or 2electrons respectively to achieve a noble gas configuration whereasgroups 15…, 16 and 17 gain electrons (3,2 1respectively) ( Full Answer )
Look for the highest numbered atom in the group: radium. Also barium has an empirical radius similar to the radius of radium: 215 pm.
Elements in group 15 (or group 5) are non-metals. Thus, elements in group 1 lose electrons, forming positively charged cations, which are gained by elements in group 5, forming negatively charged anions. The attraction between anions and cations is known as an ionic bond. Example, the reaction betw…een sodium and nitrogen: 2 Na(s) + 3 N2(g) --> 2 Na3N(s) The formula is due to sodium having a valency of 1 and nitrogen having a valency of 3. These 'cross over' producing the symbolic formula Na3N. ( Full Answer )
One valence electron, the number of v.e's is equal to the group number if this is counted from 1 to 8.
Two of the halogens (group 17) and one of the earth alklides (group 2) Example: 2 Cl - + Ca 2+ --> CaCl 2
6, as indicated by its presence in Group 16 of a wide form periodic table.
Group II elements (also called alkaline earth metals), have two valence electrons. To fill their outer shell, they therefore become ions with two positive charges, such as magnesium: Mg -> 2e - + Mg 2+
Group 2 metals have 2 valence electrons. In fact, the number of valence electrons of elements can be deduced from the group number (e.g. group VII elements have 7 valence electrons).
That varies, element #3 will have 3, element 4 will have 4, etc. However, they all have 2 valence electrons.
Group 1 and 2 elements have 1 and 2 valence electrons respectively. Removal of these electrons will result in stable noble gas electronic configuration. Group 17 and 16 elements have 7 and 6 valence electrons respectively. Addition of 1 or 2 electrons to group 17 and 16 respectively will give them s…table noble gas configuration. Hence these two groups are highly reactive and their elements will combine to form large number of compounds. ( Full Answer )
Group 1 has 1, group 2 has 2, group 15 has 5, group 16 has 6 and group 17 has 7 valence electrons.
A group of 2 or more atoms that act like 1 and have an overall charge is called a polyatomic ion (ion made of more than one atom).
Group 1 elements have 1 valence electron, group 2 has two valence electrons and group 15 has 5 valence electrons.
There isn't any picture available. You can find examples of the dotstructures online or do a simple chemical equation to find outwhich matches up to your needs.
group 1 and 2 are electorpositive elements(metals) so they readilly reacts with group 16 and 17 elements which are electronegative(non-metals).
Group 16 because on the periodic table, there are different columns that represent a greater or lesser amount of valence electrons; and group 16 has the amount of 6 valence electrons.
Group 2 is called the alkali earth metals. They all have 2 electrons in their outermost orbitals. Thus, all of there configurations end with s 2 .
There are 2 valence electrons (electrons in the outer shell) of group 2 elements in the ground (un-ionised or standard) state. This causes them to form +2 ions.
They lose their electrons to become Ions because they have alot of outer shell and as a result, alot of electons. Think of a nucleus of an atom like the positive end of a magnet... The electrons are the negative end and opposites attract... The further away you place two magnets, the weaker the pull…... It is the same with the Alaki Metals (group 1)... This is why they are very reactive metals, because their outer shells are further away from the nucleus meaning it's easier for an electron to find the energy to escape, because the nucleus has a weaker pull on it... ( Full Answer )
They have 7 valence electrons. Just as group 16 has 6 and group 18 has 8.
This is a chemical element. You can find the how many electron in a single atom by using a periodic table.
No. Protons are contained in the nucleus of an atom and electrons are outside of the nucleus in a region called an electron cloud.
The last letter represents how many valence electrons are. So: K: 2e L: 8e M: 5e The valence of the element is 3 (8-no. of valence electrons). Note that that formula is correct for nonmetals only. The element is P and has the electronic configuration [Ne]3s2 3p3 or 1s2 2s2 2p6 3s2 3p3. It h…as to gain 3e to get from 3p3 to 3p6. ( Full Answer )
They are lost. If it has a plus sign beside the ion charge, that means the atom loses electrons. But if it has a negative sign for the ion charge, that means that the atom gains electrons.
They lose two electrons. If it says +2 that means that it loses two electrons, but if it says -2, it means that that atom gains two electrons.
If "group 1" means "column 1 of a wide form periodic table", the answer is 1.
How can you tell how many valence electrons an element has by just the atomic number and group number?
The number of valence electrons in an element is represented by the group number; for example, all elements in group one have one valence electron, all elements in group two have two valence electrons, etc.
Seven due to the fact that on the periodic table all group 17 elements have seven valence(outer) electrons.
Looks like seven valance electrons to me. that would make this group the halogens, 7A.
2 electron groups are in CO2. Proof, I got it wrong on a quiz. :(
The group 1 and 2 elements have much lower electronegativity value than group 17 elements and therefore lose electrons to the group 17 elements. The group 17 elements require only one more electron to have a full valence shell and thereby acquire the stable electron configuration of the next higher …atomic number noble gas. The group 1 and 2 elements achieve a stable electron configuration when they lose all their outermost (valence) electrons and thereby acquire the electron configuration of the next lower atomic number noble gas. One group 1 element will combine with one group 17 element and one group 2 element will combine with two group 17 elements. Examples include NaF, and MgCl 2 . ( Full Answer )
Atomic radius decreases when you go from group 1 to group 2 across a period.
Periodic Table Group Number*: Number of Valence Electrons for Each Atom . 1 : 1 2 : 2 15 : 5 16 : 6 17 : 7 ___________________ *In a wide form periodic table.
Group 1 elements have one valence electron, and group 2 elements have two valence electrons.
Group 1 elements have one valence electron. If they lose one electron, they will attain noble gas configuration and obey octet rule. Hence group 1 elements are reactive and tend to lose one electron. Group 17 elements have seven valence electron. If they gain one electron, they will attain noble ga…s configuration and obey octet rule. Hence group 17 elements are reactive and tend to gain one electron. ( Full Answer )
The most common type of ions are. Monopositive cation for group 1 elements, Dipositive cation for group 2 elements, Trinegative anions for group 15 elements, Dinegative anion for group 16 elements and mononegative anions for group 17 elements..
As we move down the group, number of valence electrons remain the same. only, no. of shell increases.