What is noticeable about all of the ionic charges in Group 1 2 15 16 and 17?
The ionic charges of group 1 and 2 metals are +1 and +2 respectively. Group 15 & 16 the simple mono-atomic ions are -3 and -2. Group 17 ions are -1. This can be explained by the following elemnts in groups 1 and 2 lose 1 or 2 electrons respectively to achieve a noble gas configuration whereas groups 15, 16 and 17 gain electrons (3,2 1 respectively)
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I took days 15 16 and 17 instead of days 1 2 and 3.Then on days 15 16 and 17 I took 1 2 and 3.Is this bad?
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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 electrons 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.
all the elements of group 1 have only one valence electrn so they donate one electron and are always 1 +
The charge for all elements in Group 2A is +2.
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. 1…6 and 17 have 6 and 7 respectively. So together, they form 8..
group1: +1 group2: +2 group15: -3 group16: -2 group17: -1
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 elemen…ts have 7 and 6 valence electrons respectively. Addition of 1 or 2 electrons to group 17 and 16 respectively will give them stable noble gas configuration. Hence these two groups are highly reactive and their elements will combine to form large number of compounds.
It's -3 =P
Group 1 has 1, group 2 has 2, group 15 has 5, group 16 has 6 and group 17 has 7 valence electrons.
group 1 and 2 are electorpositive elements(metals) so they readilly reacts with group 16 and 17 elements which are electronegative(non-metals).
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 .
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.
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..
They make ions with charge of +1. They lose an electron to makepositive ions.