which group has a valence shell electron configuration ns1?
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Explanation: In an electron configuration under the general form of ns1 , the n represents the period number and the 1 represents the group number, and therefore, the element would be in group 1.
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The electron configuration of N3- is N3-: 1s22s22p6 .
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Hydrogen (H), lithium (Li), and sodium (Na), as group 1 elements, have just one electron in their outermost shells. They are unstable as single atoms, but can become stable by losing or sharing their one valence electron.
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Hydrogen ( Hstart text, H, end text), lithium ( Listart text, L, i, end text), and sodium ( Nastart text, N, a, end text), as group 1 elements, have just one electron in their outermost shells. They are unstable as single atoms, but can become stable by losing or sharing their one valence electron.
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Group 6A elements have 2 valence electrons in an s orbital and 4 valence electrons in p orbitals.
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Nitrogen is a Group 5A element, so it has 2 valence s electrons, and 3 valence p electrons.
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Each H atom (group 1) has 1 valence electron, and the O atom (group 16) has 6 valence electrons, for a total of 8 valence electrons.
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All the Group 1 elements - lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr) - have one electron in the outer shell.
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Transition Metals So the valence electrons for a transition metal are the ns and (n-1)d electrons. This means that manganese (Mn) has the electron configuration [Ar]4s²3d⁵ and 7 valence electrons.
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All the elements in Group 2 have two electrons in their valence shells, giving them an oxidation state of +2. Covers the elements beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr) and barium (Ba).
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Silver has 1 valence electron. In terms of orbitals, it has the following electron configuration: 4d^10,5s^1.
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Nitrogen has 5 electrons in its n=2 (outer) shell. There is a quick way of identifying the number of valence electrons - it is the same as the Group number (not for d-block elements, though).
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Potassium, an element in Group 1 of the periodic table(alkaline metals) has 1 valence electron. Number of valence(outer shell) electrons corresponds to the element's group number and therefore it has 1 valence electron.
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is the same as the number of electrons in its outer shell. An element in group 1 has 1 electron in its outer shell. An element in group 2 has 2 electrons in its outer shell.
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In which period and group is the element whose electron configuration is [Kr]5s1? It is Rubidium (Group 1, Period 5).
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The two most reactive groups of elements are the alkali metals and the halogens, because of their valence electrons. Those groups have 1 and 7 valence electrons, respectively, making them desperate to bond to something, to achieve a stable configuration of 8.
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To determine: The number of valence electrons present in the element having valance electron configuration ns2np4. The unknown element has 6 valance electrons. The valance electron configuration ns2np4 shows that there are 6 electrons in the valance shell. Therefore, the unknown element has 6 valance electrons.