The Group number and period number corresponds to the outer most shell and number of electrons present in outer most shell.
For Example:
Oxygen has atomic number 8, and its electronic configurations is,
1s², 2s², 2pₓ², 2py¹, 2pz¹
The outermost shell is 2, means oxygen is present in period 2, and the number of electrons in n = 2 are 6, so the group number is 6 in periodic table.
Lets take another example of Sodium, it has atomic number 11 with electronic configuration;
1s², 2s², 2p⁶, 3s¹
The outermost shell is 3, means sodium is present in period 3, and the number of electrons in n = 3 are 1, so the group number is 1 in periodic table.
Answer:
Fluorine has a higher electronegativity than carbon
Explanation:
Electronegativity trend
-As you go from left to right across the periodic table, the electronegativity increases.
-As you go from top to bottom, the electronegativity decreases.
-We know that both carbon and fluorine are in the same energy level or period 2. However, Carbon is in group 14, which has 4 valence electrons, while fluorine is in group 17, which has 7 valence electrons. Therefore, fluorine has a higher electronegativity because fluorine is desperately wanted to gain 1 more valence electron to become stable (octet rule).
