Aufbau's principle does not deal with the filling of electrons in the degenerate orbitals (i.e. orbitals having same energy) such as px, py and pz

The carbon atom has six electrons. According to Aufbau principle, the electronic configuration is 1s²,2s²,2p² 
It can be represented as below,

In this case, in order to minimise the electron-electron repulsion, the sixth electron enters the unoccupied 2p_y orbital as per Hund's rule. i.e. it does not get paired with the fifth electron already present in the 2P_x orbital

s-orbitals: For Is orbital, l = 0 and m = 0, f(θ) = 1/✓2 and g(φ) = 1/✓2π. Therefore, the angular distribution function is equal to 1/✓2π.i.e it is independent of the angle θ and φ. Hence, the probability of finding the electron is independent of the direction from the nucleus. The shape of the s orbital is spherical.

p-orbitals :
(a) For p orbitals l = 1 and the corresponding m values are -1,0 and + 1. The angular distribution functions are quite complex
(b) The three different m values indicates that there are three different orientations possible for p orbitals. These orbitals are designated as p_x,p_y and p_z and the angular distribution for these orbitals shows that the lobes are along the x, y and z axis respectively.
(c) The 2p orbitals have one nodal plane

d-orbitals :
(a) For 'd' orbital I= 2 and the corresponding m values are -2, -1,0 +1,+2.
(b) The shape of the d orbital looks like a clover leaf.
(c) The five m values give rise to five d orbitals namely d_xy,d_yz,d_zx,d_x² -y² and d_z2.
(d) The 3d orbitals contain two nodal planes.