Chapter 3: Electronic Structure + Periodic Properties of Elements

wavelength (λ)

distance between 2 crests (meters or nanometers)

frequency (𝜈)

number of cycles per second (1/s, S^-1, Hz)

speed of light in a vacuum

c = 3.00 × 10⁸ m/s

Planck

-equation: E=hv

-constant: 6.262 × 10^-34J.s

energy

capacity to do work

work

force applied through distance

force

any push or pull on an object

joule

SI unit of energy, 1J = kg (m/s)²

photoelectric effect

light shining on the surface of metal can cause electrons to be ejected (only ejected if the photons have sufficient energy)

photons

tiny packets or particles of light

Bohr’s Model

nucleus in the middle, electrons surrounding in circular orbits with quantized energy levels

Equation for energy of an electron in orbit

E = -k/n²

What is the value of the constant “k”

2.18 × 10^-18J

What happens to the energy of an electron as it gets further from the nucleus?

it decreases

de Broglie Equation

wavelength = h/ mv

constructive interference

two wavelengths in the same period combine to increase amplitude

destructive interference

waves in opposite periods combine to create a flat line with no amplitude

electron defraction

means that electrons do have wavelike tendencies and the orbits are not perfectly circular