If an electron within an atom has space that is limited by the size of the atom (10^-10 m), what is the minimum uncertainty in its momentum? [h = 6.63 × 10^-34 J s] A)0.52 × 10^-24 kg m/s B)1.05 × 10^-24 kg m/s C)3.31 × 10^-24 kg m/s D)6.63 × 10^-24 kg m/s

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The minimum uncertainty in momentum can be calculated using Heisenberg's uncertainty principle, which states Δx * Δp ≥ ħ/2, where Δx is the uncertainty in position (size of the atom, given as approximately 10^-10 meters), Δp is the uncertainty in momentum, and ħ is the reduced Planck's constant (h/2π). Given h = 6.63 × 10^-34 J s, ħ = h/(2π) = 1.05 × 10^-34 J s. Therefore, Δp ≥ ħ/(2Δx) = (1.05 × 10^-34 J s) / (2 * 10^-10 m) = 1.05 × 10^-24 kg m/s.

If an Electron Within an Atom Has Space That Is