Atomic Structure

p-orbital contains a maximum of 6 electrons.

The shape of an s-orbital is spherical.

Two electrons in an atomic orbital have opposite spins (one has clockwise and the other anticlockwise).

It is double dumbbell shaped.

The atomic number of carbon is 6. It contains 4 electrons in the outermost shell. Hence, the number of unpaired electrons is 2.

It is the electronic configuration of neon.

Arsenic (At. no. 33) belongs to 15^th group as its outer shell configuration is 3d¹⁰ 4s² 4p³, which contains 15 electrons.

Sc⁺ means that one electron has been donated, i.e. its electronic configuration would be less than one electron from scandium.

It shows that this element contains 7 electrons in its outermost shell and it needs 1 electron more to complete its octet. Hence, it is the most electronegative element.

It represents the ground state of chromium.

According to the Aufbau principle, 4s will have lower energy than 3d, 4p and 5s.

The principal quantum number 'n' represents the relative overall energy of each orbital and the energy of each orbital increases as the distance from the nucleus increases.

The electronic configuration of chromium is 1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁵, 4s¹. Therefore, by the removal of 3 electrons it results in 3 unpaired electrons in the outer shell.

Magnetic quantum number defines the orientation in space.

The electronic configuration of iron is [Ar] 3d⁶ 4s². Hence, its two outermost shells are incomplete.