```

H H H H

| | | |

H - C - C - C - C - H

| | | |

H H H H

```

Here's how the orbitals are involved in forming the covalent bonds:

* Carbon: Each carbon atom has four valence electrons and uses sp³ hybridized orbitals to form four sigma bonds.

* Hydrogen: Each hydrogen atom has one valence electron and uses its 1s orbital to form a sigma bond.

Here's a breakdown:

1. C-C bonds: Each carbon atom forms a sigma bond with its neighboring carbon atom using an sp³ orbital.

2. C-H bonds: Each carbon atom forms four sigma bonds with hydrogen atoms using its four sp³ orbitals. Each hydrogen atom uses its 1s orbital.

Therefore, the orbitals involved in forming the covalent bonds in butane are:

* sp³ orbitals from carbon

* 1s orbitals from hydrogen

Note: There are no pi bonds in butane because all the carbon atoms are bonded to four single bonds (saturated).