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Chemistry
11th
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36 Terms
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1
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Aufbau Principle
* filling orbitals in order of increasing energy
* came from the word __***aufbauen***__ which means __***build***__
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Au (Gold)
does not follow aufbau principle
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Diamagnetic
no unpaired electron ↓ (-1/2 )
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Paramagnetic
has unpaired electron ↑ (1/2)
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No. Types of Quantum Numbers
4
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Principal quantum number
describes “shell” and “size” or orbitals
7
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Azimuthal Quantum Number
describes the shape of the orbital
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Pauli Exclusion Principle
* Filling the orbitals with two electrons in opposite spins
* like charges repel = unlike charges attract
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n (definition)
* main energy level of electron
* principal quantum number
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s
sublevel in the first energy level
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Spin Quantum Number (m*s*)
describes the spin of electron (1/2 or -1/2)
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Electron Configuration
representation of the arrangement of electrons
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Electric Structure of Atoms
series of energy levels that are possible for a bound electron to occupy
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Shell
Energy level of atom/electron
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Subshell (Sublevel)
tells the shape of orbital denoted as s, p, d, f
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Energy levels
* n increases = energy increases
* \
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F orbitals (Fundamental)
* seven orbitals
* known as most diffused shape
* maximum of 14 electrons
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P orbitals (Principal)
* 3 orbitals
* dumbbell shape
* maximum of 6 electrons
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s orbitals (sharp)
* 1 orbital
* spherical shape
* maximum of 2 electrons
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D orbitals (diffused)
* 5 orbitals
* maximum of 10 electrons
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Electron Configuration
arrangement of electrons within their respective sublevels
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s, p, d, f table
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Noble gases
* inert gases
* all ends with p⁶ configuration (except helium)
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Duet rule
stable with only 2 electrons
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Octet Rule
stable with 8 electrons
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Noble Gas Configuration
use of noble gases in shortening the Electron Configuration
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Orbital Diagram
reconstruct the electronic configuration.
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Hund’s Rule of Multiplicity
All orbitals with the same energy must be filled up before pairing with another electron
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Magnetic Quantum Number
shows the orientation of the orbital in space
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Chemical Bonding
basic fundamental that explains other concepts such as molecules and reactions
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Lewis Dot Structure
representation of valence electrons
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Octet Rule
atoms tend to lose, gain, or share electrons until they have achieved an outer shell that contains an octet of electrons
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Ionic Bonds
electrostatic attraction between two oppositely charged ions cause by electrons transferring from one atom to another.
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Properties of Ionic Compound
* High melting and boiling point
* Conducts electricity
* Solid at room temperature
* Hard and brittle
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Outermost shell
Valence Electron
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Paired dots
lone pairs
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