The Quantum Model of the Atom Chapter 4 Section 2

Bohr’s Problems Why did hydrogen’s ________exist around the nucleus only in ____________orbits? Why couldn’t the electron exist in a ___________number of orbits with slightly different energies? Why didn’t the Bohr model work for ____ atoms?

Louis de Broglie French scientist in the 1920s Observed that the behavior of ________ is similar to the behavior of _________ Suggested that _________be considered _________ Other experiments confirmed that electrons have ____________properties

Electrons are Like Light Electrons can be __________. Electrons can show __________patterns These are properties of __________!

Electrons as Particles and Waves Electrons were determined to also have a dual ___________nature, like _______. So……..where are they in the __________? _____________________ was a German physicist that tried to detect electrons.

Heisenberg Uncertainty Principle ________have about the same energy as a _________of light When trying to detect an ________, and the photon of light ______________ __________ ___________________________: it is impossible to determine simultaneously both the position and the velocity of an electron

Schrödinger Wave Equation ________________was an Austrian physicist Said that electrons travel in __________ Only waves of __________energies, and therefore __________, provide solutions to the wave equation:

Quantum Theory The foundation for modern ___________ theory was laid by Heisenberg’s _______________ and Schrödinger’s ________________. ______________________: describes mathematically the wave properties of electrons and other very small particles moving very fast

Quantum Theory Electrons do ______travel around the nucleus in ________orbits. They exist in certain regions called _____________. __________: a three-dimensional _____ around the nucleus that indicates the __________location of an __________.

The Quantum Model- The Electron Cloud ______________- Statistical area where electrons should exist around the nucleus. This is not a nice and neat set of circular paths ______________location of electrons but we can _______________represent where most of the electrons should “be.”

Electron Cloud

Quantum Numbers ________________: numbers (4 of them) that specify the properties of _______ _______and the properties of ________ in those orbitals The first 3 quantum numbers result from solutions to the ____________________. The fourth quantum number describes a fundamental state of the _________(its spin) that occupies an orbital

Principle Quantum Number (n) It indicates the ________________ occupied by the electron and is symbolized by _____. As n ________, the electron’s ______and its average __________from the nucleus ____________. ______number of ___________in a main energy level is indicated by _____.

Angular Momentum Quantum Number (l) It indicates the _________of the orbital; which indicates the ________of orbital. Energy __________: orbitals of different ________within a particular main energy level.

Angular Momentum Quantum Number (l) For a specific _______energy level, the number of orbital ________possible is equal to _____. Actual values for l start at 0 and increase up to (n-1). The different shapes are designated ___, ____, _____, and ____, each with a specific number of orbitals.

Orbitals Energy level n=1: only ___sublevel, “___” All s orbitals (s sublevel) are __________. One s orbital can hold ____electrons. There is one s orbital in ____energy level Designated as ___, ___, ___, ___, etc. If you have one electron in the 1s orbital, it is designated as ____, if you have two electrons, then ____.

Other Sublevels The p sublevel has ___orbitals, each capable of holding ___electrons for a total of ___electrons. The d sublevel has ___orbitals, each capable of holding ___electrons for a total of ___electrons. The f sublevel has ___orbitals, each capable of holding ___electrons for a total of ___electrons.

Magnetic Quantum Number (ml) It indicates the ___________of an orbital around the nucleus ___orbitals are __________, so they only have _______possible orientation ___orbitals are “___________” shaped and have ___possible orientations according to the Schrödinger’s equation.

Quantum Mechanical Model An _______is the region of space where there is a high probability of finding an electron in an atom. In the quantum mechanical atom, orbitals are arranged according to their size and shape. The higher the energy of an orbital, the larger its size. s-orbitals have a spherical shape

Shapes of p-Orbitals Recall that there are three different p sublevels. p-orbitals have a dumbbell shape. Each of the p-orbitals has the same shape, but each is oriented along a different axis in space.

Location of Electrons in an Orbital The orbitals are the region of space in which the electrons are most likely to be found. An analogy for an electron in a p-orbital is a fly trapped in two bottles held end-to-end.

Shapes of d Orbitals Recall that there are five different d sublevels. Four of the d orbitals have a clover-leaf shape and one has a dumbbell and doughnut shape. There are seven f orbitals:

Spin Quantum Number (ms) Indicates the two fundamental _______ states of an electron in an orbital Has only two possible values: ___and ___ A single orbital can hold a maximum of _____electrons, but they must have ____________spin states.

Progression of Models- Summary Electron Cloud (or Quantum) Model Chapter 5