Unit 2 Flashcards
Isotope
atoms that belong to the same element but have different number of neutrons.
Mass Spectrometer
Tool used to determine the % abundance of isotopes of an element.
Electromagnetic spectrum
range of frequencies that covers all electromagnetic radiation and their respective wavelengths and energy. Divided into bands or regions and shows relationship between frequency, wavelength, and energy.
Characteristics of Line Spectrum
a line spectrum only shows certain frequencies
Emission line spectrum
Arrow going down, because the spectrum is produced when an electron loses energy.
Continuous line spectrum
A continuous spectrum in the visible region contains all the colors of the spectrum.
Types of energy released / absorbed
UV radiation: From or to the 1st energy level
Visible Light: From or to the 2nd energy level
Infrared: From or to the 3rd energy level
Emission spectrum of hydrogen atom features
- Each line is a specific energy value
- ## lines get closer together towards the blue end of the spectrum shows convergence towards higher energy end so electrons reaching maximum amount of energy
Subshells
Shells are split into subshells which are given the letters s, p and d. Order of these shells: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 4f
Orbitals
subshells contain one or more atomic orbitals. They exist at specific energy levels and electrons can only be found at these specific levels, not in between. Each atomic orbital can be occupied by a maximum of two electrons
Orbital shapes
S orbital: Big circle in the middle
P orbitals: X diagonal dumbbell Y horizontol dumbbell, Z vertical dumbbell
Ground state
most stable electronic configuration of an atom which has the lowest amount of energy.
Aufbau’s Principle
Electrons are added into orbitals from lower to higher energy.
Pauli Extension principle
only 2 electrons with opposite spins may be filled in a single orbital.
Hund’s rule
In orbitals with equal energy, 1 electron is singly filled with the same spin, then doubly filled.
Exceptions to electronic configuration
Chromium (Cr): (Ar) 4s1 3d5
Copper (Cu): (Ar) 4s1 3d10
Ion’s electronic configuration
- Electron is always lost first from the highest energy orbital.
- Transition Metal always lose electron from 4s orbital first.
When there is at least 1 3d orbital electron filled, 4s orbital is moved up to higher energy than 3d orbital.
