Lecture 4: Uncertainty
Yeonjei Jung
UNIST
October 5, 2015
Yeonjei Jung
Uncertainty
Oct 5, 2015
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1. Assessing Risk
We incorporate risk and uncertainty into our models of decision
making because they can cause consumers and rms to modify
decision abou
1. Which of the following substances are largely ionic, and which are covalent?
(a) HF (b) HI (c) PdCl2 (d) BBr3 (e) NaOH (f) CH3Li
Answer: (a), (b), (c), (d), (f), and (g) are polar covalent, but (e) is ionic.
2. Which of the following pairs of structure
Assignment #6 ( Chapter 6)
1. (a) Which element from each set has the largest atomic radius?
(i) Ba, Ti, Ra, Li
(ii) F, Al, In, As
(b) Which eletment form each set has the smallest ionization energy?
(i) Tl, Po, Se, Ga
(ii) Cs, Ga, Bi, Se
2. How many lite
Assignment #4 ( Chapter 4)
1. Assign oxidation numbers to each atom in the following substances:
(a) Ethane, C2H6, a constituent of natural gas H =1, C -3
(b) Borax, Na2B4O7, a mineral used in laundry detergents
O-2, Na+1, B +3
(c) Mg2Si2O6, a silicate mi
Assignment #5 ( Chapter 5)
1. The MRI (magnetic resonance imaging) body scanners used in hospitals operate with 400 MHz
radiofrequency energy. How much energy does this correspond to in kilojoules per mole?
E = hv
= (6.626*10-34)*(400*106)
= 2.65*10-25 J
Assignment #6 ( Chapter 6)
1. (a) Which element from each set has the largest atomic radius?
(i) Ba, Ti, Ra, Li
(ii) F, Al, In, As
(b) Which eletment form each set has the smallest ionization energy?
(i) Tl, Po, Se, Ga
(ii) Cs, Ga, Bi, Se
(a,i) Ra, (a,ii)
Assignment #5 ( Chapter 5)
1. The MRI (magnetic resonance imaging) body scanners used in hospitals operate with
400 MHz radiofrequency energy. How much energy does this correspond to in
kilojoules per mole?
= 400 MHz = 400 106 s-1
E= (6.62610-34 Js)(400
Assignment #4 ( Chapter 4)
1. Assign oxidation numbers to each atom in the following substances: (a) Ethane, C2H6, a constituent of natural gas (b) Borax, Na2B4O7, a mineral used in laundry detergents (c) Mg2SiO4, a silicate mineral
2. The solubility of a
Assignment #1 (Chapter 1)
1. A 105 mL sample of water at 292.4 K was heated for 9 min, 23s so as to give a constant
temperature increase of 3.0 oF/min. What is the final temperature of the water in degrees
Celsius?
Answer: 34.9 oC (T(final) = T + (3.0(t(m
Chapter 7. The Crystalline Solid State
Formulas and Structures
Thermodynamics of Ionic Crystal
Formation
Molecular Orbitals and Band Structure
Superconductivity
Bonding in Ionic Crystals
Imperfections in Solids
Silicates
1
Kinds of Solids
Amorphous
Chapter 5. Molecular Orbitals
Formation of MO from AO
Homonuclear Diatomic Molecules
Heteronuclear Diatomic Molecules
Molecular Orbitals for Larger Molecules
1
Molecules from Atoms
2
Molecules from Atoms
Amplitudes of wave functions added
Amplitudes of
[ACE32101]
2011 December 10
Problem Set IV
Problem 1
Page 218; 6.29
Ans)
Problem 2
Page 218; 6.30
Ans)
[ACE32101]
2011 December 10
Problem 3
Page 218; 6.20 (Please use Table 6.8)
Ans)
Problem 4
Page 218; 6.27
[ACE32101]
2011 December 9
Problem Set III
Due: December 1st
Problem 1
On the basis of molecular orbitals, predict the shortest bond, and provide a brief
explanation.
(a) Li2+ Li2 ;
Ans)
(b) F2+ F2 ;
Ans)
(c) He
[ACE32101]
2011 September 19
Problem Set 1 Solution
Problem 1
Consider a hydrogen atom decaying from the state having the principal quantum
number 10 to the state having the principal quantum number 4.
(a) Calculate the energy released.
A
[ACE32101]
2011 November 23
Problem Set III
Due: December 1st
Problem 1
On the basis of molecular orbitals, predict the shortest bond, and provide a brief
explanation.
(a) Li2+ Li2 ; (b) F2+ F2 ; (c) He2+, HHe+, H2+;
[ACE32101]
2011 September 14
Problem Set II
Due: October 20th
Problem 1
Give Lewis dot structures and sketch the shapes of the following.
(a) PSCl3 (P is central); (b) IF4- ; (c) SOCl2; (d) CS2; (e) SO3; (f) XeO3
Problem 2
Ethylene is
Chapter 4. Symmetry and Group Theory
Symmetry Elements and Operations
Points Groups
Properties and Representations of Groups
Examples and Applications of Symmetry
1
Properties of Groups
2
Representations of Groups
Any symmetry operation can be carried
Chapter 6. Acid-Base and
Donor-Acceptor Chemistry
Acid-Base Concepts
Major Acid-Base Concepts
Hard & Soft Acids & Bases (HSAB)
Acid & Base Strength
1
Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that prod
[ACE32101]
2011 September 19
Problem Set 1
Due: September 27th
Problem 1
Consider a hydrogen atom decaying from the state having the principal quantum
number 10 to the state having the principal quantum number 4.
(a) Calculate the energy r
Chapter 4. Symmetry and Group Theory
Symmetry Elements and Operations
Points Groups
Properties and Representations of Groups
Examples and Applications of Symmetry
1
Properties of Groups
2
Representations of Groups
Any symmetry operation can be carried
Chapter 4. Symmetry and Group Theory
Symmetry Elements and Operations
Points Groups
Properties and Representations of Groups
Examples and Applications of Symmetry
1
Properties of Groups
2
Representations of Groups
Any symmetry operation can be carried
Inorganic Chemistry
Code #: ACE32101
Instructor: Prof. Hoi Ri Moon ()
NSB 601-1
Tel: 217-2928
E-mail: [email protected]
Office hours: by appointment
TA: Ok Ji Park () 217-2990
Homepage:
http:/sites.google.com/site/hoirimoon/
Inorganic Chemistry
An int
Chapter 4. Symmetry and Group Theory
Symmetry Elements and Operations
Points Groups
Properties and Representations of Groups
Examples and Applications of Symmetry
1
Point Groups
Molecules with the same
symmetry elements are
placed into point groups.
2
Chapter 4. Symmetry and Group Theory
Symmetry Elements and Operations
Points Groups
Properties and Representations of Groups
Examples and Applications of Symmetry
1
Symmetry
The symmetry properties of molecules and how they can be used
to predict vibr
Chapter 3. Simple Bonding Theory
Lewis dot structure
Valence-shell electron-pair repulsion
(VSEPR): EN & atomic size effects
Molecular polarity
Hydrogen bonding
1
E lectronegativity
EN: the ability of an atom in a molecule
to attract the shared electro
Chapter 2. Atomic Structure
Periodic Table
Bohr Atom
Schrodinger Equation
Periodic Properties of Atoms
1
2
T he Schrodinger Equation
Describes wave properties of electron
(position, mass, total energy, potential energy)
Wave function ()= electron wav
Chapter 3. Simple Bonding Theory
Lewis dot structure
Valence-shell electron-pair repulsion
(VSEPR)
Molecular polarity
Hydrogen bonding
1
Valence-Shell Electron-Pair Repulsion (VSEPR)
Electrons in bonds and in lone pairs can be thought of as
charge clou