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Inorganic Exam 1

CHEM 3353 Okstate

TermDefinition
3D Electrical Conductivity Capability of a metal to pass the flow of a electric current Best: Ag; Worst: Plutonium
Metalloids Form anionic complexes and anions Examples: Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te)
Chemically Weak Metals Can form anionic complexes but NOT anions Examples: Aluminum (Al), Gallium (Ga), Indium (In), Tin (Sn), Thallium (Tl), Lead (Pb), Bismuth (Bi)
Shielding for ns or np electrons Electrons in same (ns,np) group contribute 0.35 Electrons in (n-1) contribute 0.85 each Electrons in (n-2) contribute 1 each
Shielding for nd or nf electrons Electrons in same nd or nf group contribute 0.35 All electrons to the left shield 1.00 All electrons to the right don't shield
Allred-Rochow Electronegativity Will be given equation, will only need to plug in Zeff as solved through Slater's rules
Alpha Emission 4/2 He (right)
Beta Emission 0/-1 e (right)
Positron Emission 0/+1 e (right)
Electron Capture 0/+1 (left)
Neutral Hydrogen Non-polar molecules with London forces Will not react vigorously with water Examples: H2S, H2Se, PH3
Positive Hydrogen When H is bonded to N, O, or F Will not react vigorously with water Examples: NH3, H2O, HF, HCl
Negative Hydrogen EH4 (E=Si, Ge, Sn but not C) VERY reactive with H2O and O2 Examples: B2H6
Element-Deuterium Stronger bond than element-protium E-D has a lower zero-point energy
Zero Point Energy Effects strength of bond Lowest Vibrational Energy Level
Normal Oxides M2O Examples: Li2O, Na2O, K2O, Rb2O, Cs2O
Peroxides M2O2 Examples: (No Li) Na2O2, K2O2, Rb2O2, Cs2O2
Superoxides MO2 Examples: (No Li or Na), KO2, RbO2, CsO2
Delta H Atomization All Alkali Metals are soft Typical metal values between 400-600 kJ/mol Elements with higher melting points have higher of this
Normal Oxides dissolved in water M2O + H2O -> 2M+ + 2OH-
Peroxides dissolved in water M2O2 + H2O -> 2M+ +2OH- + H2O2
Superoxides dissolved in water MO2 + H2O -> 2M+ +2OH- + H2O2 + O2
High Charge Density Covalent Bonding Hydrated solid salts (Group 1: only Li+ salts)
Low Charge Density Ionic Bonding
High Lattice Enthalpy Radii of cation and anion are similar in size Want small-small or large-large; not small-large
Five Species present at Schlenk Equilibrium EtMgBr, Et2Mg, MgBr2, Mg2Br2Et2(OEt2)2 (x2 but different configurations)
Carbide C^(4-) Only Be forms true C^(4-) Big tell is product of CH4 (g)
Acetylides All other group 2 elements form this instead of Carbides (-:C=-C:-)
Equation for acidic zinc salt Zn(NO3)2 -(H2O)-> [Zn(OH2)6]^(2+) + 2NO3- Due to octahedral configuration (acidic)
Mercury (I) Always find in form Hg2^(2+) Hg+ has a single 6s electron to share with a neighbor Hg+ ion
Alternation Effect Electronegativity Increases Ga has a full (n-1)d subshell for first time d orbital has two angular nodes (poor shielding)
Inert Pair Effect Tendency of two electrons in outermost atomic s-orbital to remain unshared Example: Thallium shows +1 instead of +3 due to retaining 6s^2 electron and loses 6p^1 electron since 6s orbital is very large and harder to remove than 6p
(3c,2e) in B2H6 Total number of electrons=12 Due to structure (Dimer structure) would need 16 electrons which leads to middle having this bond formation
Bonds orders of B2H6 Terminal BH bonds: 1 B-H-B bonds: 1/2
MO diagram Both pairs of electrons located in the sigma bonding plane Different planes (top to bottom): sigma* antibonding, sigma nonbonding, sigma bonding
Created by: kedurkee
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