CHEM 1061: CHAPTER 8
24 Cards in this Set
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Metals are:
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- shiny solids
- moderately high melting points
- good conductors of heat and electricity, malleable
- tend to LOSE ELECTRONS and FORM CATIONS
- easily OXIDIZED
- strong reducing agents
- BASIC in aqueous solutions
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Trends in Metallic Behavior:
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INCREASE down a group
DECREASE across a period
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What type of oxide do main-group nonmetals form?
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Covalent Oxides: acidic in aqueous solutions
N2O5(s) + H2O(l) --> 2HNO3(aq)
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What type of oxides do some metals and metallics form?
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Amphoteric Oxides: acids OR bases in water
Al2O3(s) + 6HCl(aq) --> 2AlCl3(aq) + 3H2O(l)
Al2O3(s) + 2NaOH(aq)--> 2NaAl(OH)4(aq)
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What type of oxide does a main-group metal form?
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Ionic Oxides: basic in aqueous solutions
Bi2O3(s) + 6HNO3(aq) --> 2Bi(NO3)3(aq) + 3H2O(l)
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Exclusion Principle (Pauli)
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Each orbital may contain a maximum of 2 electrons which MUST have opposite signs
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Effective Nuclear Charge (Zeff)
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The nuclear charge an electron actually experiences
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Shielding
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Protects other electrons from the nuclear charge
Effects energies of atomic orbitals
Shielding by other electrons reduces the full nuclear charge to an effective nuclear charge
The further away from the nucleus an electron is the LOWER Zeff for that particular electron
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Quantum Numbers:
n
l
ml
ms
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n - level
l - sublevel
ml - orbital
ms - spin
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Spin Quantum Number ms
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Direction of electron spin
[+1/2] OR [-1/2]
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Electron Configuration and Group Trends:
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- elements in the same GROUP have the same OUTER electron configuration
- elements in the same GROUP exhibit similar CHEMICAL behavior
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Configuration Exceptions
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Chromium (Cr Z=24)
Copper (Cu Z=29)
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Electron configuration of Chromium
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Full
1s22s22p63s23p64s13d5
Condensed
[Ar]4s13d5
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Electron Configuration of Copper
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Full
1s22s22p63s23p64s13d10
Condensed
[Ar]4s13d10
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Why is the 4s sublevel filled before the 3d sublevel?
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4s orbital is LOWER in energy than 3d
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Outer Electrons
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Electrons in the HIGHEST energy level - highest n value
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Valence Electrons
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Electrons involved in forming compounds
- main group: valence electrons are the outer electrons
- transition elements: valence electrons include the outer electrons and any (n-1)d electrons
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Periodic Table Trends in Atomic Size
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INCREASES down a group
DECREASES across a period
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Periodic Table Trends in Ionization Energy (IE)
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DECREASES down a group
INCREASES across a period
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Periodic Table Trends in Electron Affinity
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DECREASES down a group
INCREASES across a period
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Partial Orbital Diagram
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Shows only the highest energy sublevels being filled
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Condensed Electron Configuration
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Has the elements symbol of the PREVIOUS noble gas in square brackets
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Aufbau Principle
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Electrons are ALWAYS placed in the LOWEST energy sublevel available
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Hund's Rule
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When orbitals of EQUAL ENERGY are available, the LOWEST energy electron configuration has the maximum number of unpaired electrons with parallel spins
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CHEM 1061: FINAL