Electrons in Atoms and the Periodic Table

Blimps, Balloons, and Models of the Atom

This section introduces the importance of atomic models by relating them to real-world events and technologies, such as the Hindenburg disaster and modern blimps.

• Hydrogen Gas: Used in the Hindenburg for buoyancy due to its low density, but highly reactive and flammable.

• Helium Gas: Used in modern blimps; it is inert and non-flammable due to its stable electron configuration (two protons, two electrons).

• Reactivity of Hydrogen: Hydrogen atoms are so reactive that they form diatomic molecules (H2).

• Inertness of Helium: Helium's electron configuration makes it chemically stable and unreactive.

• Key Question: What makes hydrogen reactive and helium inert? Atomic models help explain these properties.

Models of the Atom

Atomic models explain the observed chemical properties and periodic trends among elements.

• Reactivity Trends: Group 1A elements (e.g., hydrogen, lithium, sodium) are highly reactive; noble gases (e.g., helium, neon, argon) are inert.

• Mendeleev's Periodic Law: When elements are arranged by increasing atomic number, certain properties recur periodically.

• Bohr Model: Electrons travel in fixed orbits around the nucleus at specific distances.

• Quantum-Mechanical Model: Electrons exist in orbitals, which are probability maps rather than fixed paths.

• Key Contributors: Niels Bohr, Erwin Schrödinger, and Albert Einstein contributed to the development of quantum mechanics.

Light: Electromagnetic Radiation

The interaction of light with atoms was crucial in developing atomic models. Light is a form of electromagnetic radiation, not matter, and travels at the speed of light ( m/s).

• Wave-Particle Duality: Light exhibits both wave-like and particle-like properties (photons).

• Wavelength (\(\lambda\)): The distance between adjacent wave crests.

• Frequency (\(\nu\)): The number of cycles or crests passing a point per second.

• Relationship: Wavelength and frequency are inversely related:

Visible Light and the Electromagnetic Spectrum

Visible light is a small part of the electromagnetic spectrum, which includes gamma rays, X-rays, ultraviolet, visible, infrared, microwaves, and radio waves.

• Visible Light: Ranges from red (750 nm, longest wavelength) to violet (400 nm, shortest wavelength).

• Color Perception: Objects appear colored based on the wavelengths they reflect; e.g., a red shirt reflects red light.

• Energy and Wavelength: Shorter wavelength = higher frequency = higher energy per photon.

Electromagnetic Radiation: Photons

Light can be described as a stream of photons, each carrying a specific amount of energy depending on its wavelength.

• Photon: A particle of light; a packet of electromagnetic energy.

• Energy of a Photon: , where is Planck's constant.

• Shorter Wavelength: Higher energy per photon (e.g., violet light vs. red light).

Example: Ordering Electromagnetic Radiation

• Wavelength (increasing): X-rays < visible light < microwaves

• Frequency (increasing): Microwaves < visible light < X-rays

• Energy per photon (increasing): Microwaves < visible light < X-rays

Chemistry and Health: Radiation Treatment for Cancer

High-energy electromagnetic radiation (X-rays, gamma rays) can ionize atoms and molecules, which is used in cancer treatment but can also damage healthy cells.

• Ionizing Radiation: Can remove electrons from atoms, causing molecular damage.

• Medical Use: Targeted to destroy cancer cells, but may also harm healthy tissue.