The Electron Review
Hund's Rule
You split before you pair
Magnesium (Mg) Noble Gas Configuration
[Ne] 3s^2
Chlorine (Cl) Noble Gas Configuration
[Ne] 3s^2 3p^5
Radium (Ra) Noble Gas Configuration
[Rn] 7s^2
Aluminium+3 27 mass number (13 protons) How many electrons?
10
Aluminium has 27 mass number (13 protons and how many neutrons?)
14
Beryllium (Be) Electron Configuration
1s^2 2s^2
Al +3 Electron Configuration
1s^2 2s^2 2p^6
S -2 Electron Configuration
1s^2 2s^2 2p^6 3s^2 3p^6
Mn Electron Configuration
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5
Number of Electrons in Each Energy Level
2, 8, 18
Volume of 1 mole of a gas
22.4 L
Molar Mass of Carbon Dioxide
44.01 g/mol
Number of d orbitals
5
1 mole
6.02x10^23 particles
Probability of locating an electron
95%
Excited State
A state where the potential energy of the atom is higher than the ground state. Unstable
Heaviest Nuclear Particle
Alpha
Bohr Model
Atomic model that contains orbits and shows atoms as a small, positively charged nucleus surrounded by orbiting electrons
Oxidation Number
Charge given to an element when it loses or gains electrons
Spin Quantum Number (s)
Describes spin either upward or downward +1/2 or -1/2
Angular Momentum Quantum Number (l)
Describes the shape of each sublevel (s=0, p=1, d=2, and f=3) Sphere, Dumbells, Clover
Lewis Dot Diagrams
Determine how many valence electrons the element has MAX 8 dots around the element symbol 1st 2 paired and remaining are split d or f element based on electron configuration (highest n value)
Principal Quantum Number (n)
Determines the energy level of the electron (1-7) and the size of the electron cloud
Magnetic Quantum Number (m)
Determines the orientation of orbitals and specifies the exact orbital within each sublevel, each orbital holding 2 electrons. Value of range between -l to +l (s=1 orbital, p= 3 orbitals, d=5 orbitals, f= 7 orbitals)
Orbital Configuration
Diagram consists of a box/line representing each orbital and a half arrow representing each electron DRAW ALL; UPWARD ARROW FIRST
Energy and Frequency
Directly Proportional
Atomic Emission Spectrum
Electron's emit light when releasing absorbed energy
Ions differ in
Electrons (charge)
Wave-Particle Duality
Electrons act like particles (matter) and waves (non-matter)
Frequency and Wavelength
Inversely Proportional
Electron Cloud
Location of the electrons in the quantum mechanical model of the atom (95% probability)
Ground State
Lowest energy state
Gamma Rays
Most dangerous radiation
Isotopes differ in
Neutrons
Aufbau Principle
Niels Bohr & Wolfgang Pauli Electrons enter the lowest energy level first ; Can cause difficulties because of the overlap of orbitals of different energies
Pauli Exclusion Principle
No 2 electrons in an atom can have the same 4 quantum numbers
Stability
Noble Gases are the most stable because their outer shell is full of electrons Full Sub level next most stable (s^2, d^10, f^14) Half-full sub level is the least stable (p^3, d^5, f^7) Created gaining, losing, or sharing electrons for full octet Covalent (share) and ionic bonds (give/take)
Photon
Packet of light; Released energy from excited to relaxed state either all at once or in increments
Heisenberg Uncertainty
Principle that states it's impossible to determine simultaneously both the position and velocity of a particle
Quantum Mechanical Model
Shows orbitals/electron cloud
Quanta
Smallest amount of energy that exists independently discrete units Absorbed by electrons when they get excited and jump to a higher energy level farther from the nucleus (ground to excited state) Exact energy between the energy levels
Molar Mass
The mass of 1 mole of a substance
Electron Configuration
The way electrons are arranged in various orbitals around the nuclei of atoms 2p^6 Energy level, sublevel shape, # electrons in sublevel D block (n-1)
Half Life
Time it takes for half of an atom to decay
