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Arrange the following atoms in order of decreasing atomic radius: Cs K Mg A1 Na Cl P Classify the following bonds as covalent, polar covalent, or ionic. (Use a noble gas core abbreviation.) Na+ Mg2+ cl- K+ Within each group of four atoms or ions presented below, select the species that are isoelectronic with each other: Drag each item to the correct box. What element might M be? Elemental symbol: Write ground-state electron configurations for these ions, which play important roles in biochemical processes in our bodies. ns2 np5 This is the electron configuration of nonmetals.
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ns2 np6 This is the electron configuration of a noble gas. Z = 9: Z = 20: Z = 26: Z = 33: A M2+ ion has four electrons in the 3d subshell and is derived from a metal in the first transition metal series. ns2 This is the electron configuration of an alkali earth metal. Without referring to a periodic table, write the electron configuration of the elements with the following atomic numbers. Group the following electron configurations in pairs that would represent elements with similar chemical properties. He (1s2) is a s- block element but is positioned with the, group 18 elements (ns2 np6) because it has. ns2np6 For each electronic configuration given, choose the electronic configuration of the element that would match its chemical properties. The outer most electronic, configuration is ns2 np1-6. (a) Alkali metal (b) Alkaline earth (c) Halogens (d) Noble gases metals A. Identify the outer electron configurations for the (a) alkali metals, (b) alkaline earth metals, (c) halogens, (d) noble gases.