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53 Cards in this Set
- Front
- Back
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What observations are quantum numbers used to explain?
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Low & high resolution line spectra
Spectra in a magnetic field Ferromagnetism and paramagnetism |
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What an orbital?
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A region of space where an electron may be found
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When working with quantum numbers, what does the number and letter represent?
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The number represents the main energy level (shell) and the letter represents the sub shell
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What do the quantum numbers state?
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Shells can be composed of four different parts for they have orbitals within the orbits
Each can have up to seven electron spaces In each space an electron can have a positive or negative spin |
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Describe the principle quantum number.
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Relates to the main energy level of an electron
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What happens when electrons absorb energy?
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The electrons move to a higher orbit (further away from the nucleus)
Dark line spectra |
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What happens when electrons release energy?
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The electrons move to a lower orbit closer to the nucleus
Line Spectra |
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Describe the secondary quantum number.
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Relates to the shape of an electron orbital
Describes the sub shells Sub shells are additional electron energy that formed part of a main energy level An energy level is a staircase |
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Describe the magnetic quantum number
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Describes the orientation of the electron in space along the x,y,z axis
Color lines split into multiple lines when line spectra was exposed to a magnetic field If orbits are oriented in space in different planes, the energies of the orbits are different when the atom is near a strong magnet |
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Describe the spin quantum number
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Determines the type of electron according to its spin
Paired electrons have opposite spins that "cancel each other out" |
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What is ferromagnetism?
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A collection of atoms that all line up in the same direction
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What is paramagnetism?
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Involves individual atoms
Each electron spins on its axis and will behave like a tiny magnet |
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What is the secondary quantum number equal to?
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n-1
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Describe S orbitals
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L=0
Sphere shape One orbital |
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How many electrons can be in one orbital?
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only two!
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Describe P orbitals
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L=1
Dumbbell shape Three orbitals |
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What are the four orbital shapes?
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Sharp, principle, diffuse and fundamental
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Describe D orbitals
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L=2
Flower shape Five orbitals |
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Describe F orbitals
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L=3
Odd shape Seven orbitals |
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Describe the periodic table
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Each s,p,d or f block indicates the last orbital that is to be filled with electrons
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Why are S & P blocks considered to be valence electrons?
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They have the highest N value
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How do atoms become as stable as possible?
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By obtaining a completely full, empty or half full shell
Electrons can also move around to achieve these configurations |
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What is the Pauli exclusion principle?
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No two electrons in an atom can have the same four quantum numbers. If an electron is in the same orbital with another electron, it must have opposite spin.
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Wha is the Aufbau principle?
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The lowest energy orbitals are filled first and must be completely filled before moving up an energy level
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What is Hund's rule?
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If you have several orbitals at the same energy level, one electron is placed into each of the orbitals before a second electron is added to the orbitals
AKA electrons must be spread out horizontally as much as possible before doubling up pairs |
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What are anions? How are they dealt with in electron configurations?
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Ions with a negative charge
Add the number of electrons corresponding to the ion charge to the total number of electrons before distributing the electrons to the orbitals |
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What are cations? How are they dealt with in electron configurations?
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Ions with a positive charge
Draw the diagram for the neutral atom and then remove the corresponding number of electrons from the orbital with the highest principle quantum number |
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What is Heisenbergs uncertainty principle?
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The act of measuring an electrons energy or location changes the energy or location
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What is the Lewis Theory of Bonding?
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Electrons are most stable when they are paired.
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What do metals and non metals do?
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Exchange electrons (ionic)
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What do non metals do?
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Share electrons (covalent)
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What is the valence bond theory?
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Atomic orbitals overlap to form new hybrid orbitals containing a pair of electrons with opposite spin
This results in a decrease in energy |
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Describe sigma bonds
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Formed by the head to head overlap of atomic orbitals along the internuclear acis
The overlap is maximum The orbital is symmetrical A strong bond |
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Describe pi bonds
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A sidewise overlap of atomic orbitals perpendicular to the internuclear axis
The overlap is minimum The orbital is not symmetrical A weak bond |
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What does is mean when something is SP3 hybridized?
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It has four SP3 hybrid orbitals
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What are intramolecular forces?
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The force that holds together the atoms in a molecule.
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What are intermolecular forces?
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The force holding molecules together
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AX2
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Linear
180 degrees |
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AX3
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Planar triangular
Flat 120 degrees |
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AX2E
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Planar triangular
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AX4
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Tetrahedral
109 degrees |
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AX3E
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Pyramidal
107 degrees |
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AX2E2
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Bent
105 degrees |
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AXE3
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Linear
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AX5
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Trigonal bipyramidal
90 degrees or 120 degrees |
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AX4E
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See saw
All angles are the same |
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AX3E2
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T Shaped
90 degrees |
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AX2E3
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Linear
180 degrees |
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AX6
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Octahedral
All angles are 90 degrees |
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AX5E
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Square pyramidal
90 degrees |
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AX4E2
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Square planar
90 degrees |
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AX3E3
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T shapes
90 degrees |
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AX2E4
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Linear
180 degrees |
