Basics Flashcards
Periods
Rows on the Periodic Table
Groups
Columns on the Periodic Table
Group 1
Alkaline Metals
Group 2
Alkaline Earth Metals
Group 7
Halogens
Group 8
Noble Gases
Electronegativity Trend
Increases up and to the right (towards Fluorine the most EN element)
Electronegativity
Is a measure of the tendency of an atom to attract a bonding pair of electron; How badly it wants an electron
Size / Atomic Radius Trend
Increases down (increasing orbitals and shells) Increases left (decreased pull of electrons toward the nucleus)
Ionization Energy
The energy required to remove an electron from the outer shell of a gaseous atom or ion
Ionization Energy Trend
Increases Up and to the Right
Effective Nuclear Charge (Zeff)
The attractive positive charge of nuclear protons acting on valence electrons
Zeff Trend
Increases to the Right (electrons pulled in closer to nucleus)
Electron Affinity
The amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion
Electron Affinity Trend
Increases Up and to the Right (affinity becomes less negative)
Speed of Light (C)
3 x 10 ^ (8) m/s
Planck’s Constant (J)
6.6 x 10 ^ (-34) J x S
Electron Configuration
Where the electrons are (orbitals)
Ex: 1s^(2) 2S^(2) 2p^(6)
Aufbau Principle
“Build up rule” begin with low energy orbitals and move to higher energy orbitals
Hunds Rule
One electron goes in each suborbital before doubling them up
Pauli Exclusion Principle
No two electrons can have the same 4 quantum numbers
Principle Quantum Number (n)
Energy Level; Period in the periodic table
2n^2 = maximum number of electrons in level “n”
Azimuthal Quantum Number (L)
Orbital; Shape 0=S 1=p 2=d 3=f
4L+2 = electrons per orbital
Magnetic Quantum Number (M L)
Sub-Orbital (-L to +L)
Spin Quantum Number (M s)
Direction of electron (+ 1/2 or - 1/2)
Protium
Isotope of Hydrogen with 1 proton and 0 neutrons = mass of 1amu
Deuterium
Isotope of Hydrogen with 1 proton and 1 neutron = mass of 2amu
Tritium
Isotope of Hydrogen with 1 proton and 2 neutron = mass of 3amu
Isotope
Different weight for the same element (protons remain the same and the # of neutrons changes)
Average Mass Formula
Avg. Mass = (Isotope x (% abundance / 100)) + (Isotope x (% abundance / 100)) + ….
