Question

the table shows the electronic structures of four elements .
P - 2,6 Q - 2,8,1 R - 2,8,7
S - 2,8,8
a) Identify which element (s) will form covalent bonds which carbon​
please

Answer 1

P and R can form covalent bonds with carbon.

• The compound P has an electronic configuration 2,6 or $1s^22s^22p^4$. Thus it is oxygen. It has a partially filled valance shell and can form a covalent bond with carbon.
• The compound Q has an electronic configuration 2,8,1 or $1s^22s^22p^63s^1$. Thus it is Na. It has a partially filled valance shell so, it can easily lose its electron to form ions and can't form a covalent bond with carbon.
• The compound R has an electronic configuration 2,8,7 or $1s^22s^22p^63s^23p^5$. Thus it is Cl. It has a partially filled valance shell and can form a covalent bond with carbon.
• The compound S has an electronic configuration 2,8,8 or $1s^22s^22p^63s^23p^6$. Thus it is Ne. It has a filled valance shell and can't form a covalent bond with carbon.

Answer 2

Answer:

P and R element will form covalent bonds with carbon