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 stable noble gas configuration.
Hence these two groups are highly reactive and their elements will combine to form large number of compounds.
Between groups 16, 17; polar covalent bond, for example F2O.
With metals - mainly ionic bonds as these groups contain principally non -metals (only tellurium and polonium are metalloids)
with hydrogen covalent bonds
group 1 and 2 are electorpositive elements(metals) so they readilly reacts with group 16 and 17 elements which are electronegative(non-metals).
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Potassium will form ionic compound with group 17 elements (fluorine, chlorine, bromine, iodine) and group 16 elements (oxygen, sulphur, selenium).
Yes, with group 16 elements. Sodium oxide can be given as an example.
Oxygen form oxides and sulfur form sulfides.
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.
Group 1 or group 2 elements with group 16 or group 17 elements. In general, if the electronegativity difference between the two atoms is more than 1.7 in Pauling's scale, then the two atoms form ionic bond.
Potassium will form ionic compound with group 17 elements (fluorine, chlorine, bromine, iodine) and group 16 elements (oxygen, sulphur, selenium).
Yes, with group 16 elements. Sodium oxide can be given as an example.
Yes! Barium is a group 2 metal and so loses two electrons. Oxygen is a group 16 non metal and will readily pick up two electrons. So, they form BaO.
You are doubling the amount of D, so 8*2 = 16 grams of D required.
Oxygen form oxides and sulfur form sulfides.
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For the most part, Group 16 forms -2 ions, therefore they most readily bond with Group 2, which primarily form +2 ions.
Group 16 or the chalcogens.
carbon (group 14, period 2) hydrogen (group 1, period 1) nitrogen (group 15, period 2) oxygen (group 16, period 2) sulphur (group 16, period 3) halogens (group 17, period 2-5)
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 stable noble gas configuration. Hence these two groups are highly reactive and their elements will combine to form large number of compounds.
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.
Oxygen is in group 16 or group 6A