1.1 Atoms, Electrons, And Orbitals
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Schroedinger calculated energy in hydrogen atom by using equations that treated the electron _
As if it were a wave
Instead of a single energy, schroedinger obtained _
Series of energies
Each of the series of energies corresponded to a different _
Mathematical description of the electron wave
The mathematical descriptions are called _
Wave functions
Wave functions symbolized by Greek letter
Psi 🔱
Probability of finding an electron at a particular spot from nucleus
Square wave function
Most stable state of hydrogen atom is _
Lowest energy
Probability of finding electron at particular point is greatest towards _
Nucleus
Probability of finding an electron decreases as you distance from nucleus but never
Becomes zero
Wave functions are also called _
Orbitals
_ can be used in several different ways
Term orbital
Orbitals described by their size, shape and _
Directional properties
Spherically symmetrical orbitals are called _
S orbitals
Letter s preceded by _ n
Principal quantum number
N specifies shell and is related to _
Energy of the orbital (n = 1, 2, 3, etc.)
An electron on a 1s orbital is likely to be found _ and is lower energy
Closer to nucleus
Electron 1s more strongly held than _
2s
Instead of probability distributions, more common to represent orbitals by _
Their boundary surfaces
The region enclosed by a boundary surface is _
Arbitrary
Arbitrary but is customarily the volume where
Probability of finding an electron is high (90-95%)