UNIT 1NCCS 1.1.2 & 1.1.3

•I understand the relationship between energy and a quanta•I understand the difference between an electron’s ground state and an electron’s excited state•I will describe how an electron absorbs and releases light•I will understand that electromagnetic radiation (light) is made up of photons•I will use the Bohr Model on the Reference Guide to identify wavelengths and type of electromagnetic radiation released by an electron transition•I will explain that according to the Bohr Model, electrons are found in fixed energy orbits•I will analyze diagrams related to the Bohr model of the hydrogen atom in terms of allowed, discrete energy levels in the emission spectrum. •I will explain that according to the Bohr Model electrons gain absorb or emit energy and move up or down to another orbit•I will explain that according to the Bohr Model that electrons closer to the nucleus are in lower energy state. •I will describe what the wave/particle duality of electrons means

Properties of LightThe Wave Description of Light

• Electromagnetic radiation is a form of energy that exhibits wavelike behavior as it travels through space.

• Together, all the forms of electromagnetic radiation form the electromagnetic spectrum.

Electromagnetic Spectrum

Properties of Light, continued• Wavelength (λ) is the distance between

corresponding points on adjacent waves.

• Frequency (ν) is defined as the number of waves that pass a given point in a specific time, usually one second.

Properties of Light, continued• Frequency and wavelength are

mathematically related to each other:

c = λν• In the equation, c is the speed of light (in

m/s), λ is the wavelength of the electromagnetic wave (in m), and ν is the frequency of the electromagnetic wave (in s−1).

Wavelength and Frequency

Section 1 The Development of a New Atomic ModelChapter 4

Wavelength and frequency are inversely proportional to each other whereas frequency and energy of a wave are directly proportional to each other

The Photoelectric Effect• the photoelectric effect refers to the emission of

electrons from a metal when light shines on the metal.

The particle description of light is explained by the particle wave duality theory which is a theory that proposes that all matter exhibits the properties of not only particles, which have mass, but also waves, which transfer energy.

• A quantum of energy is the minimum quantity of energy that can be lost or gained by an atom.(sometimes referred to as a “packet of energy”)

Photoelectric Effect

The Photoelectric Effect, continuedThe Particle Description of Light• German physicist Max Planck proposed the following

relationship between a quantum of energy and the frequency of radiation:

E = hν• E is the energy, in joules, of a quantum of

radiation, ν is the frequency, in s−1, of the radiation emitted, and h is a fundamental physical constant now known as Planck’s constant; h = 6.626 × 10−34 J• s.

The Photoelectric Effect, continuedThe Particle Description of Light,

continued

• A photon is a particle of electromagnetic radiation having zero mass and carrying a quantum of energy.

• The energy of a particular photon depends on the frequency of the radiation.

Ephoton = hν

The Hydrogen-Atom Line-Emission Spectrum

• When investigators passed electric current through a vacuum tube containing hydrogen gas at low pressure, they observed the emission of a characteristic pinkish glow.

• When a narrow beam of the emitted light was shined through a prism, it was separated into four specific colors of the visible spectrum.

• The four bands of light were part of what is known as hydrogen’s line-emission spectrum.

Hydrogen’s Line-Emission Spectrum

Bohr Model of the Hydrogen Atom• Niels Bohr proposed a hydrogen-atom model that

linked the atom’s electron to photon emission.

• According to the model, the electron can circle the nucleus only in allowed paths, or orbits.

• The energy of the electron is higher when the electron is in orbits that are successively farther from the nucleus.

• The lowest energy state of an atom is its ground state.

• A state in which an atom has a higher potential energy than it has in its ground state is an excited state.

• When an electron falls to a lower energy level, a photon is emitted, and the process is called emission. When the electron falls all the way back to the lowest energy level, it is in the ground state.

• Energy must be added to an atom in order to move an electron from a lower energy level to a higher energy level. This process is called absorption. The electron is in an excited state.

Bohr Model of the Hydrogen Atom, continued

Photon Emission and Absorption

QUESTIONS USING THE NCCS REFERENCE TABLE

If an electron in an hydrogen atom moves from the fourth energy level to the second:(a)What is the value of the wavelength in nanometer

emitted by the photon?(b)What is the value of the wavelength in meters

emitted by the photon??(c) What color of light would you see (d) What is the frequency of that photon

1 nm = 1 x 10-9 m

410 nm = 4.10 x 10-7 m

ANSWER:(a)486 nm(b)4.86 x 10-7 m(c)Blue(d)c = λf

f = c/λ = (3 x 108m/s) / (4.86 x 10-7 m) = 6.17 x 1014 s-1 or = 6.17 x 1014 Hz