# Modern Atomic Model and EMR. Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Include: quantum, photon Understand.

## Presentation on theme: "Modern Atomic Model and EMR. Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Include: quantum, photon Understand."— Presentation transcript:

Modern Atomic Model and EMR

Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Include: quantum, photon Understand how unique line spectra are created for each element. Additional KEY Terms SpectroscopyEmission Line spectrum

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

Wavelength and frequency are inversely related 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

Types of Electromagnetic radiation f and λ determine what you see or feel, amplitude determines how bright or hot Memorize this wavelength range…

Sunlight (white light) shone through a prism separates it into a continuous spectrum of colours. The different wavelength for each colour causes them to refract or bend at different angles

All EMR radiates at 3.00 x 10 8 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

The colours seen in fireworks are a result of burning different salts. Red light has a wavelength of 650 nanometres. Calculate the frequency of red light (1 nm - 1.0 x 10 -9 m). ƒλc = ƒ 650 x 10 -9 m = 3.00 x 10 8 m/s ƒ = 4.6 x 10 14 Hz

ColourElement greencopper yellowsodium redstrontium yellow- green barium orange-redcalcium purplepotassium purple-redlithium Burning small amounts of each element gave off a unique colour of light Used to detect a metals presence Planck (1900) Focusing this light through a prism also produces a spectrum, but ONLY distinct lines appear Investigated heating objects and

Energy emitted by a element can be separated – to produce a Line spectrum (emission spectrum) Disclaimer: This is not as simple as my “art” looks

The colored lines of the atoms (or Spectral Lines) are a kind of "signature" for the atoms. C O Spectroscopy and spectrophotometry are techniques used to investigated EMR emissions.

Planck's Radiation Law: Energy is transmitted in discrete amounts – called quanta. EMR is a stream of tiny “packets” of quantized energy carried by particle-like photons. A photon has no mass but carries a quantum of energy

E q = 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 Energy (quantum) contained in a photon is directly related to the frequency of the radiation. So higher frequency waves contained larger “packets” of energy

The blue colour of fireworks is often achieved by heating copper (I) chloride to about 1200 o C. The wavelength of the blue light is 450 nm. What is the quantum of energy emitted by this light? E = hf ƒ = c λ ƒ 450 x 10 -9 m = 3.00 x 10 8 m/s ƒ = 6.7 x 10 14 Hz E = (6.626 x 10 -34 J · s)(6.7 x 10 14 Hz) E = 4.4 x 10 -19 J q

CAN YOU / HAVE YOU? Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Include: quantum, photon Understand how unique line spectra are created for each element. Additional KEY Terms SpectroscopyEmission Line spectrum

Download ppt "Modern Atomic Model and EMR. Describe the electromagnetic spectrum in terms of frequency, wavelength, and energy. Include: quantum, photon Understand."

Similar presentations