Atomic Structure, Electron configuration, and Ionization Energy Flashcards
What is inside the nucleus?
Protons and neutrons
What is outside the nucleus
Electrons
What subatomic particles have significant weight to them
Protons and Neutrons
What are isotopes?
Atoms of the same element with a different # of neutrons/different weights
What are ions?
Atoms that have gained or lost an electron and have different charges
What are electron configurations used for?
Finding where electrons are in an atom
Where can electrons be found?
In different energy levels of clouds/orbitals
What are the 4 types of orbitals
S orbital - 1 orbital/2 electrons
P orbital - 3 orbitals/ 6 electrons
D orbital - 5 orbitals/10 electrons
F orbitals - 7 orbitals/ 14 electrons
What element types end with S orbitals
Alkali metals, Alkali earth metals, and Helium
What element types end with P orbitals
Nonmetals and metalloids
What element types end with D orbitals
Transitional metals + Lanthanum and Actinium
What element types end with F orbitals
Lanthanoids and Actinoids
What is the Aufbau principle
Lower energy levels should be filled before the next higher one (S orbitals first, then P orbitals and so on)
What is Hund’s Rule
Electrons fill empty orbitals in parallel directions before filling opposite direction (Similar to how people sit in buses or airplanes)
What is the Pauli Exclusion principle
No two electrons can have the same spin direction in an orbit (Only up and down spins)
Shortened version used with electron configuration
Using a noble gas (Full orbital) and adding the amount of orbits to get to the element needed (Ex. Rubidium: [Kr] 5s^1)
What is ionization energy
The energy needed to remove an electron from an atom or ion
“Formula” of removing an electron
Li1 + e- = Li
Li2 + e- = Li1
Li3 + e- = Li2
What factors affect ionization energy
Nuclear charge, Atomic radius, and Electron shielding
Electron shielding
Electrons in sub levels lower than the valence electrons repelling them more than protons in the nucleus can attract (decreases IE)
Valence electrons
Electrons in the last shell of an atom
Atomic Radius
Howe many energy levels or “rings” the atom has that increases down a column (Decreases IE)
Nuclear charge
How many protons an atom has (increases IE)
Why does Ionic energy decrease for each noble gas
Because the farther down the column of noble gases, the larger the atomic radius and the less that protons have an effect on electrons (Atomic radius, Electron shielding)
