An energy of 2.0 ×10^2 kJ / mol is required to cause a cesium atom on a metal surface to lose an

step 1 In this question, we are given the amount of energy needed to cause a cesium atom to lose an ele

An energy of 2.0 ×10^2 kJ / mol is required to cause a...

An energy of $2.0 \times 10^{2} \mathrm{kJ} / \mathrm{mol}$ is required to cause a cesium atom on a metal surface to lose an electron. Calculate the longest possible wavelength of light that can ionize a cesium atom. In what region of the electromagnetic spectrum is this radiation found?

Key Concepts

Electromagnetic Spectrum

The electromagnetic spectrum encompasses all types of electromagnetic radiation, categorized by their wavelengths or frequencies, ranging from gamma rays to radio waves. Recognizing the region of the spectrum associated with a particular wavelength is important for understanding the energy, potential applications, and interactions of the radiation with matter.

Ionization Energy

Ionization energy is the minimum energy required to remove an electron from an atom in its gaseous state. It is a critical concept in atomic physics and chemistry, indicating how strongly electrons are held in an atom and influencing the atom's reactivity and electronic properties.

Planck-Einstein Relation

The Planck-Einstein relation, given by E = hc/?, connects the energy of a photon to its wavelength (or frequency, via ? = c/?). This relation is fundamental in quantum mechanics and explains how photons can interact with matter, such as causing ionization when their energy matches or exceeds the ionization energy.

Energy Unit Conversion and Avogadro's Number

In many chemical contexts, energy is provided per mole of particles. To use quantum equations like the Planck-Einstein relation, it is often necessary to convert this molar energy into the energy per individual atom or molecule by dividing by Avogadro's number. This conversion is essential for accurate calculations at the atomic or molecular scale.

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