Spectroscopic Methods of Analysis

UV/VIS radiation

Infrared spectroscopy

The energy of a photon is directly proportional to its frequency. This relationship can be expressed by the equation E=hv, where E is the energy, h is Planck's constant, and v is the frequency.

<p>Quantized energy levels imply that atoms and molecules can only exist at specific, discrete energy states.</p> Signup and view all the answers

<p>1.99 x 10^-18 J</p> Signup and view all the answers

<p>1.91 m</p> Signup and view all the answers

<p>Electronic energy levels describe the energy of electrons in atoms and molecules. Vibrational energy levels describe the energies associated with the stretching and bending of chemical bonds. Rotational energy levels relate to the energies associated with the rotation of molecules.</p> Signup and view all the answers

<p>The range of frequencies associated with visible light typically falls between 4.3 x 10^14 Hz and 7.5 x 10^14 Hz.</p> Signup and view all the answers

<p>The Balmer series is a group of emission spectral lines that arise from transitions of the hydrogen atom's electron from higher energy levels to the n=2 energy level. The Balmer series has been instrumental in understanding the quantized nature of energy levels within atoms.</p> Signup and view all the answers

<p>By multiplying the frequency of the emitted radiation by Planck's constant (E=hv), we can determine the energy of the electron transition.</p> Signup and view all the answers

<p>E = hv = hc/λ</p> Signup and view all the answers

<p>10 nm to 400 nm</p> Signup and view all the answers

<p>They are quantized.</p> Signup and view all the answers

<p>Ultraviolet (UV) spectroscopy</p> Signup and view all the answers

<p>It relates the speed of light (c) to the frequency (f) and wavelength (λ) of radiation.</p> Signup and view all the answers

<p>Infrared (IR) spectroscopy</p> Signup and view all the answers

<p>It measures the masses of fragments of a molecule.</p> Signup and view all the answers

<p>Frequency is the number of waves passing a point in one second.</p> Signup and view all the answers

<p>It detects signals from hydrogen atoms.</p> Signup and view all the answers

<p>Radio frequencies range from about 1 mm to 100 km.</p> Signup and view all the answers

<p>Wavelength is inversely proportional to frequency; as wavelength increases, frequency decreases.</p> Signup and view all the answers

<p>The equation represents the energy difference associated with a transition between energy levels in an atom, where ∆E is the energy change, h is Planck’s constant, and ν is the frequency.</p> Signup and view all the answers

<p>Energy quanta refer to the fixed values of energy that electrons can have, which dictate the specific frequencies of electromagnetic radiation they can absorb.</p> Signup and view all the answers

<p>When an electron absorbs electromagnetic radiation, it transitions from a lower energy state (E1) to a higher excited state (E2).</p> Signup and view all the answers

<p>A photon refers to a quantum of energy emitted when an electron falls back from an excited state to its ground state.</p> Signup and view all the answers

<p>The speed of light is a constant that relates frequency and wavelength; specifically, c = λν.</p> Signup and view all the answers

<p>Ultraviolet radiation has shorter wavelengths and higher energy compared to infrared radiation, which has longer wavelengths and lower energy.</p> Signup and view all the answers

<p>This equation signifies that the energy absorbed or emitted during a transition corresponds directly to the frequency of the electromagnetic radiation.</p> Signup and view all the answers

<p>A molecule can only absorb specific frequencies if there are corresponding energy transitions available that match the energy of the radiation.</p> Signup and view all the answers

<p>Planck's constant is a proportionality constant that relates the energy of a photon to its frequency, serving as a key factor in quantifying energy transitions.</p> Signup and view all the answers

Waves with electric and magnetic fields vibrating in specific directions.

Distance between one wave peak and the next, measured in meters.

Number of waves passing a point per second, measured in hertz (Hz).

Measurement of electromagnetic radiation absorbed or emitted by substances.

Uses electron transitions to analyze bonding patterns in molecules.

Measures bond vibration frequencies to identify functional groups in molecules.

Fragments molecules to measure their masses for analysis.

Detects signals from hydrogen atoms for distinguishing isomers.

Related to frequency and wavelength by the equation c = fλ.

Energy levels in atoms and molecules exist in discrete values.

Energy is proportional to frequency and inversely proportional to wavelength: E = hv and v = c/λ.

The energy associated with a photon is given by E = hv, where h is Planck's constant.

Energy levels associated with the vibrations of molecules.

Energy levels relating to the rotation of molecules.

Energy levels that involve the electrons moving between different orbits.

Frequency can be calculated using v = c/λ, where c is the speed of light and λ is wavelength.

A technique that measures vibrational and rotational transitions in molecules.

The spectrum of light emitted by hydrogen atoms, showing discrete lines based on electron transitions.

The proportionality constant in the equation for energy: h = 6.63×10−34 J·s.

Discrete amounts of energy that electrons can absorb or emit.

A particle of light that carries energy proportional to its frequency.

The lowest energy state of an atom where electrons are in their closest orbits.

A state where an electron has absorbed energy and moved to a higher energy level.

The change in energy when an electron moves between levels E1 and E2.

The range of all types of electromagnetic radiation, from low energy to high energy.