Explain the important distinctions between each pair of terms: (a) frequency and wavelength; (b) ultraviolet and infrared light; (c) continuous and discontinuous spectra; (d) traveling and standing waves; (e) quantum number and orbital; (f) spd f notation and orbital diagram; (g) \(s\) block and \(p\) block; (h) main group and transition element; (i) the ground state and excited state of a hydrogen atom.

Frequency refers to the count of waves per second, while wavelength refers to the distance over which the wave's shape repeats. Ultraviolet light has higher energy and shorter wavelengths, whereas Infrared light has lower energy but longer wavelengths. Continuous spectra display a continuous band of colors, while discontinuous spectra only show emission at certain wavelengths. Traveling waves move through space, whereas standing waves vibrate in place. In atoms, the quantum number provides information about electrons and their orbits, and an Orbital refers to where an electron is likely to be found. \(s\) block elements have their last valence electron entering an \(s\) orbital, while \(p\) block elements have these in a \(p\) orbital. Main group elements have electrons entering the \(s\) or \(p\) orbitals of the outermost shell, whereas transition elements have these going into the \(d\) orbitals of the penultimate shell. The ground state of a hydrogen atom is its lowest energy state, while an excited state refers to when an electron has absorbed energy and moved to a higher orbital.