Name or state the following with reference to the elements of the first three periods of the periodic table.
(a)Noble gas with duplet arrangement of electrons.
(b) Metalloid in period 3
(c) Valency of elements in groups 14, 15
(d) Noble gas having electronic configuration 2, 8, 8.
(e) Group whose elements have zero valency
(f) A covalent compound formed by an element in period 2 and a halogen.
(g) Non-metallic elements present in the period 3 of group 15 and group 16
(h) An electrovalent compound formed by an alkaline earth metal and a halogen.
(i) Bridge elements of period 3 of groups 1, 2, and 13.
(j) Alkali metal in period 3 that dissolves in water giving a strong alkali.
(k)Typical elements of groups 14 and 15
(l) An alkaline earth metal in period 3.
Name or state the following with reference to the elements of the first three periods of the periodic table.
(a)Noble gas with duplet arrangement of electrons.
(b) Metalloid in period 3
(c) Valency of elements in groups 14, 15
(d) Noble gas having electronic configuration 2, 8, 8.
(e) Group whose elements have zero valency
(f) A covalent compound formed by an element in period 2 and a halogen.
(g) Non-metallic elements present in the period 3 of group 15 and group 16
(h) An electrovalent compound formed by an alkaline earth metal and a halogen.
(i) Bridge elements of period 3 of groups 1, 2, and 13.
(j) Alkali metal in period 3 that dissolves in water giving a strong alkali.
(k)Typical elements of groups 14 and 15
(l) An alkaline earth metal in period 3.
(a) Helium(He) is the noble gas having atomic no. 2 is an element that completes its duplet(Only two electrons in the outer shell).
He: 2
(b) Silicon(Si) is the element in a period 3 that is metalloid(Metalloids are the elements that have both the characters of metals and non-metals).
(c) Valency from groups 13 to 18 calculated by the following formula:
Valency of an element: group no. - 10
So,
Valency of group 14: 14-10
= 4
Valency of group 15: 15-10
= 5
(d) Noble gas having configuration 2, 8, 8 is Argon as Argon has an atomic no. of 18
(e) Group 18 has zero valencies because they have 8 electrons in their outer shell so they don't need any other no. of an electron to complete their octet that's why they are called zero group elements.
(f) Carbon(C) is an element belonging to the second period and the halogen that is chlorine(Cl) forms a covalent bond(covalent bond forms when sharing of electrons takes place).
(g) The non-metallic element present in periods 3 and groups 15 and 16 are Phosphorus(P) from group 15 and Sulphur(S) from group 16.
(h) NaCl is a compound that is formed by the alkali metal sodium(Na) and the halogen that is chlorine(Cl).
(i) Some of the elements we have which show the properties of the elements that are diagonally placed to them in another group.
These elements are known as bridge elements. They are:
Lithium(Li: group-1) and Magnesium(Mg: group-2)
Beryllium(Be: Group-2) and Aluminium(Al: Group-13)
(j) Alkali metal that presents in period 3 that forms strong alkali when dissolving in water is Sodium(Na).
(k) Typical elements are those elements that have a fixed oxidation state(Oxidation no. is a no. of total loss or gain of electrons in order to form an ion).
Typical elements of period 2 belonging to groups 14 and 15 are carbon and nitrogen respectively.
Typical elements of period 3 belonging to groups 14 and 15 are silicon and phosphorus respectively.
(l) The alkaline earth metals are metals belonging to 2 groups they are called alkaline earth metals because they dissolve in water to form an alkali solution and they are mostly found in earth crusts so they are called alkaline earth metals.
(a) Helium(He) is the noble gas having atomic no. 2 is an element that completes its duplet(Only two electrons in the outer shell).
He: 2
(b) Silicon(Si) is the element in a period 3 that is metalloid(Metalloids are the elements that have both the characters of metals and non-metals).
(c) Valency from groups 13 to 18 calculated by the following formula:
Valency of an element: group no. - 10
So,
Valency of group 14: 14-10
= 4
Valency of group 15: 15-10
= 5
(d) Noble gas having configuration 2, 8, 8 is Argon as Argon has an atomic no. of 18
(e) Group 18 has zero valencies because they have 8 electrons in their outer shell so they don't need any other no. of an electron to complete their octet that's why they are called zero group elements.
(f) Carbon(C) is an element belonging to the second period and the halogen that is chlorine(Cl) forms a covalent bond(covalent bond forms when sharing of electrons takes place).
(g) The non-metallic element present in periods 3 and groups 15 and 16 are Phosphorus(P) from group 15 and Sulphur(S) from group 16.
(h) NaCl is a compound that is formed by the alkali metal sodium(Na) and the halogen that is chlorine(Cl).
(i) Some of the elements we have which show the properties of the elements that are diagonally placed to them in another group.
These elements are known as bridge elements. They are:
Lithium(Li: group-1) and Magnesium(Mg: group-2)
Beryllium(Be: Group-2) and Aluminium(Al: Group-13)
(j) Alkali metal that presents in period 3 that forms strong alkali when dissolving in water is Sodium(Na).
(k) Typical elements are those elements that have a fixed oxidation state(Oxidation no. is a no. of total loss or gain of electrons in order to form an ion).
Typical elements of period 2 belonging to groups 14 and 15 are carbon and nitrogen respectively.
Typical elements of period 3 belonging to groups 14 and 15 are silicon and phosphorus respectively.
(l) The alkaline earth metals are metals belonging to 2 groups they are called alkaline earth metals because they dissolve in water to form an alkali solution and they are mostly found in earth crusts so they are called alkaline earth metals.
