Modern Atomic Model and EMR

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Presentation transcript:

Modern Atomic Model and EMR

Understand how line spectra are created. Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Understand how line spectra are created. Additional KEY Terms Spectroscopy Emission Quantum Line spectrum

Composed of radiated waves of both electrical and magnetic energy. Maxwell (1860) - all energy radiated from objects (including visible light) is electromagnetic radiation. Composed of radiated waves of both electrical and magnetic energy.

Amplitude: height of the wave from origin to crest. Wavelength (λ - “lambda”): distance from point to the same point on the next wave. Frequency (ν – “nu” or ƒ): number of wavelengths, or cycles, that pass a point per unit time. Frequency measured in cycles per second (s-1), or the SI unit hertz (Hz) Amplitude: height of the wave from origin to crest. Wavelength and frequency do not affect amplitude Wavelength and frequency are inversely related

Types of Electromagnetic radiation f and λ determine what you see or hear, amplitude determines how loud or bright

c = λƒ c = λν All EMR radiates at 3.00 x 108 m/s in a vacuum. This universal value (c) is a product of the wavelength and frequency of the radiated energy. “speed of light” c = λƒ c = λν

Sunlight (white light) shone through a prism separates into a continuous spectrum of colours. Each colour represents light of a different frequency – increasing frequency - ROY G BIV

Planck (1900) Elements give off a unique colour of light when burned - used to detect the presence of a metal This is known as a Colour Element green copper yellow sodium red strontium yellow-green barium orange-red calcium purple potassium purple-red lithium If the light emitted is focused through a prism, a spectrum with distinct lines is produced.

Disclaimer – This is not as simple as my drawing.

Energy emitted by a heated element can be separated – producing emission spectrum. (line spectrum)

The colored lines of the atoms (or Spectral Lines) are a kind of "signature" for the atoms.

Spectroscopy and spectrophotometry are techniques used to determine a substance’s emission spectrum

Planck's law: postulated that energy can only be gained or lost in discrete amounts – quanta. Quantum is the minimum amount of energy gained or lost by an atom. Energy contained in a quantum was directly related to the frequency of radiation emitted. E = hf

E = hf E – energy of a quantum (Joules) h – Plank’s constant (6.626 x 10-34 J s) f – frequency of absorbed or emitted EMR

Understand how line spectra are created. CAN YOU / HAVE YOU? Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Understand how line spectra are created. Additional KEY Terms Spectroscopy Emission Quantum Line spectrum