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1) Fill completely with electrons the first subenergy (closest to nucleus therefore least amount of energy those electrons have) 2) Electrons. The way we says it is maximum 2 electrons in each orbital. 3) Electrons are filled into each orbitals (also called degenerate) before any orbital can have two electrons in it. 4) 3 subenergy levels ("s", "p", and "d") subenergy level. 5) There are 5 "d" orbitals in each "d" subenergy level 6) Since there are two different types of subenergy levels, s brings 2 electrons and p orbital brings 6 for a total of 8electrons. 7) No since in third energy level there are 3 different subenergy levels (s, p, d) therefore 8) atoms of the same element different by mass (# of mass). Carbon-13, C-13, 136C. 9) #n= Mass number - Atomic number 10) Atomic Number 11) Electron in the highest energy level. Column column L to R not including "d" & "f" blocks. Part II 1) ( As 33e-) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3 [5 valence electron] 2) (Bi 83e-) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p3 [5 valence electron] 3) (Cs 55e-) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1 [1 valence electron] Part II (2nd one) Note: p+ - proton, e- - electron, n0 - neutrons a) Ca-42 (Calcium-42), 20p+, 20e-, 22n0 b) C-13 (Carbon-13), 6p+, 6e-, 7n0 c) U-238 (Uranium-238), 92p+, 92e-, 146n0 Part III See Atomic mass table for actual atomic mass. |