Identify the atom represented by this electron configuration and elaborate on its bonding properties. 1s22s22p63s23p64s23d5 a) .chromium is a transition with a half full-valence orbital and can form up to six bonds. b) antimony is a metalloid that can form five covalent bonds or three metallic bonds. c) manganese is a transition metal that can form up to five stable ionic bonds d) bromine is a non-metal that forms one ionic bond or a variable number of covalent bonds.

            The given electronic configuration represents Manganese.

Explanation:
                   The given electronic configuration is

                                  1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d⁵

As the valence shell is 4 in electronic configuration so it is present in 4rth period in periodic table. And according to definition of transition elements, transition elements has partially filled d-orbital. i.e.

                                                  (n - 1)d
As, n = 4
So,
                                                  (4 - 1)d

                                                      3d

So tracking 4rth period, we found Mn with given electronic configuration.
Also,
        "Manganese is a transition metal that can form up to five stable ionic bonds". It means that the five electrons present in d-orbital are transferred and Mn converts into Mn⁺⁵.

Most likely a is the answer - because  you generate   38 atp's but also consume an atp.   each atp gives approx. less than 4 kcal so probably a is the closest answer.

Oxygen= 88ghydrogen= 12g