From the element’s position on the periodic table, predict the valence shell electron configuration for each atom. Tin’s electron configuration is Kr5 s 2 4 d 10 5 p 2. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s 22s 22p 63s 1 configuration.

The chloride ion, #Cl^-#, has a charge of #color (red) (-1)#, meaning, it had gained 1 electron in its outermost orbital. Sn is located in the second column of the p block, so we expect that its electron configuration would end in p 2. (2) electron loss will result to a #color (blue) 'positive'# charge ( #color (blue) (+)#), (1) electron gain will result to a #color (red) 'negative'# charge ( #color (red) (-)#), and The electron configuration for neon is displaystyle 1s22s22p6, with ten total electrons and eight valence electrons. Now, for you to be not confuse, you always have to remember that: Elements usually do this in order to gain the electron stability of the noble gases (octet rule). The outermost electrons surrounding an atom (the valence electrons) are responsible for the number and type of bonds that a. #1s^2#2s^2#2p^6#3s^2#3p^5# = #color (green) '17 electrons'# (just add the superscripts)įor a ground state element to become an ion, it has to either gain or lose an electron in its outermost orbital. Therefore, the ground state electron configuration of the element, chlorine is: #Z# = number of protons = number of electrons (ground state) Since the atomic number is always equal to the number of protons orĪnd in ground state (no charge), the number of protons is equal to the number of electrons, then Based on the periodic table, the atomic number ( #Z# of chlorine is 17.

Be electron configuration