<span>Mass of nitrogen = 14.0067
</span>
Mass of oxygen = 15.9994
In this compound nitrogen = 36.86 /
14.0067 = 2.63
<span>And oxygen = 63.14 / 15.9994 = 3.95 <span>
now we have: N----- 2.63 and O----3.95
by dividing both with the smallest number we get
</span></span>
<span>N-------2.63/2.63 = 1<span>
<span>O-------3.95/2.63 = 1.5
To get whole numbers we multiply both by 2
</span></span></span>
N= 1 x 2 = 2
And O = 1.5 x 2= 3
<span>So, the empirical formula is N</span>₂O₃.
Idk really but i hope you figure out the answer im not on that yet.
Noble gases
Explanation:
Electronic configuration 1s² 2s² 2p⁶
The element belongs to the group of the noble gases.
- The noble gases have complete outer shell configuration of their atoms.
- we can infer that the configuration above is for an element in the p-block because the last sub-level filled is the p-orbital.
- The elements therefore belongs to the p-block
- The block is from group 111A to O
- Only the halogens and noble gases fits this picture from the option.
- The outer most p-subshell have three orbitals requiring 6 electrons to fill them up.
- This makes a complete and stable configuration.
- The highest energy level of 2 is also made up of 8 electrons, an octet.
- This is why we can conclude that they are noble gases.
Learn more:
Noble gas brainly.com/question/1781595
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