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atomic number
number of protons in the nucleus
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mass number
sum of protons and neutrons
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isotopes
same atomic numbers but different mass numbers
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ionization potential
energy required to remove an electron
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When is ionization potential lower?
when the electron is further away from the nucleus, which is why it becomes easier to take it away
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a high ionization potential means ___? why?
means that this atom is very stable bc it is almost impossible to take electrons from it
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electron affinity
energy that is released by adding an electron to an atom
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electronegativity
how much an atom loves electrons / ability of an atom to attract other electrons, increases up and to the right
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Heisenberg Uncertainty Principle
one cannot determine simultaneously the location and momentum of an electron -- you can only give a probability of where an electron is instead of a location
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What does it mean for an electron to be quantized?
they can only have certain energies, cannot be in between energy levels
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Atomic Radius increases in what direction?
to the left and to the bottom
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Formula for electron capacity in each shell?
2n^2
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Maximum number of electrons in shell 1?
2 electrons
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Max number of electrons in shell 2?
8 electrons
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Max number of electrons in shell 3?
18 electrons
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What are degenerated orbitals?
orbitals with the same energy, for ex. 3 p-orbitals are all the same energy
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Aufbau principle
electrons occupy the nearest nucleus/orbital first in order from lowest to highest energy
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Hund's rule
if orbitals have the same energy, you occupy each orbital first with a single electron and after all have one electron each, you fill them with a second one
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The closer the orbital is to the nucleus, the ____ the energy
the lower the energy bc it requires less energy than if the orbital was big and the electron was further away
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Octet Rule
atoms are most stable if they have a filled shell or an outer shell of eight electrons
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the least electronegative atom?
Hydrogen
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What are electronegative atoms and where are they located?
- elements with electron-attracting capabilities
- located on the far right and top of periodic table
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What are electropositive atoms and where are they located?
- elements with electon-donating capabilities
- located on the far left
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Ionic Bond
- bond between two atoms caused by electrostatic attraction of plus and minus charged ions
- involves transfer fo electrons between two atoms of widely different electronegativities
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Covalent Bond
- bond formed by sharing of electrons (in pairs) between two atoms
- have similar electronegativities
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Bonding electron pair
outer-shell electron pair involved in a covalent bond
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Non-bonding electron pair
a lone outer-shell pair that is NOT involved in a bond between atoms
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Polar Covalent Bond
- exists between atoms that form a covalent bond but have diff electronegativities
- the bond is unequal
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Localized electrons
electrons fixed between two atoms
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What kind of bonds are localized vs delocalized?
- localized - sigma bonds
- delocalized - pi bonds and triple bonds
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The more resonance forms you have…
the more stable the molecule (meaning it is low in energy)
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Resonance Structures
lewis structures with the same connectivity but differ in the locations of the electrons
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Resonance Hybrid
an average of the resonance forms of a certain molecule
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Why are bonding MOs lower in energy than AOs?
otherwise no bond will be able to form
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Bond Dissociation Energy
the energy needed to break or dissociate a bond
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Homolytic Cleavage
- bond cleavage in which the each atom gets one electron back
- no charge involved, fairly stable
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Heterolytic Cleavage
bond cleavage in which the bonding electrons are unevenly divided between the two par
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Homolytic Bond Formation
bond formation in which the bonding electron are evenly divided between the two atoms that form the new bond
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Heterolytic Bond Formation
bond formation in which the bonding electrons are unevenly divided between the two atoms that form the new bond
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Exothermic Reaction
energy is released
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Endothermic Reaction
energy is absorbed
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What if an empty AO interacts with a fully filled AO?
results in lewis acids and bases
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Orthagonal Orbitals
- non-interacting orbitals
- if two AOs approach each other and the anti bonding and bonding interactions are the same, no bond will form
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