Development of Complex Curricula for Molecular Bionics and Infobionics Programs within a consortial* framework**
Consortium leader
PETER PAZMANY CATHOLIC UNIVERSITY
Consortium members
SEMMELWEIS UNIVERSITY, DIALOG CAMPUS PUBLISHER
The Project has been realised with the support of the European Union and has been co-financed by the European Social Fund ***
**Molekuláris bionika és Infobionika Szakok tananyagának komplex fejlesztése konzorciumi keretben
***A projekt az Európai Unió támogatásával, az Európai Szociális Alap társfinanszírozásával valósul meg.
PETER PAZMANY CATHOLIC UNIVERSITY SEMMELWEIS
UNIVERSITY
WORLD OF MOLECULES
Computational chemistry methods
semmelweis-egyetem.hu
(Molekulák Világa )
(Számítógépes kémiai módszerek)
Compiled by dr. Péter Mátyus
with contribution by dr. Gábor Krajsovszky
Formatted by dr. Balázs Balogh
Table of Contents
World of Molecules: Computational chemistry
semmelweis-egyetem.hu
1. Introduction 4 – 7
2. ‘Classical’ Mechanics methods 8 – 9
3. Quantum Mechanics (QM) methods 10 – 12
4. Basic sets 13 – 15
5. Basics 16 – 21
6. Examples 22 – 53
I. Introduction
World of Molecules: Computational chemistry
Computational chemistry, molecular modelling, etc.
a branch of chemistry that uses principles of computer science to assist in solving chemical problems
Examples for calculations:
• structure (i.e. the expected positions of the constituent atoms)
• energies
• electronic charge distributions
• dipoles moments
• vibrational frequencies
• reactivity
• spectroscopic quantities
Computational chemistry
World of Molecules: Computational chemistry
Experimental vs. Computational chemistry
Experimental definition of the Computational problem
Design of the experiment assemble the installation
Choose method build up the system
Carry out the experiment Run the calculations Evaluation
of the results
?
World of Molecules: Computational chemistry
1. ‘Classical’ Mechanics (Newton) methods
Molecular Mechanics based on Force Field Methods
• MM3
• Sybyl
• Amber
2. Quantum Mechanics (QM) methods
Schrödinger equation with approximations
• Semi-empirical models
• Ab Initio models
• Density Functional Theory (DFT) models
Teoretical models
World of Molecules: Computational chemistry
Molecular Mechanics (MM) based on Force Field Methods
• Hooke's law,
• van der Waals interactions
• electrostatics
Molecules are considered as a collection of balls (atoms) and springs
(bonds) structures and energies are determined by employing Newtonian physics
Calculations cannot be performed without knowing some parameters from experimental results (force constants, bond lengths and angles, torsions angles, etc.)
‘force field’ is the collection of equations and parameters
‘Classical’ Mechanics methods
World of Molecules: Computational chemistry
Molecular Mechanics methods
E = E covalent + E noncovalent
E bond + E angle + E torsion E electrostatic + E van der Waals
q2
- q2
+
electrostatic van der Waals
Distance distortion
Angle distortion
Dihedral distortion
Hook’s law: F = - k x
x – displacement of the end of the spring F – force exerted by the spring
k – spring constant (force constant)
Coulomb’s law:
F – magnitude of the electrostatic force q1 and q2 – charges
r – distance between the two charges
Ke– proportionality constant (Coulomb force constant)
22 1
r q k q F = e
World of Molecules: Computational chemistry
Schrödinger equation, describes how the quantum state of a physical
system changes in time. It is as central to quantum mechanics (as Newton's laws are to classical mechanics).
Quantum Mechanics (QM) methods
Total energy
Wavefunction Kinetic energy
Potential energy
If we could find an exact solution for the Schrödinger equation of a
molecular system, we would know everything there is to know about that system. But we can’t. At least, not exactly… → approximations
World of Molecules: Computational chemistry
( x, y, z ) Ψ(x, y, z) E Ψ(x, y, z)
m V 8π
h
22
2
⎟⎟ =
⎠
⎜⎜ ⎞
⎝
⎛ − ∇ +
Schrödinger Equation
Nuclei don't move
Electronic Schrödinger equation
Guess how electrons affect each other from idealized problem
parameterization
Density Functional Theory models Electrons move independently
Molecular "solutions" written in terms of atomic solutions
Hartree-Fock
Molecular orbital methods
Semi-empirical models
MOLLER-PLESSET models
Ab initio Hartree-fock
models
Mix in excited states to account for electron correlation
HΨ = EΨ Born-Oppenheimer approximation
Hartree-Fock approximation
LCAO
approximation
Atomic orbitals don't interact + Parameterization
World of Molecules: Computational chemistry
Quantum Mechanics (QM) methods
Semi-empirical methods: (MNDO, AM1, PM3 etc.)
based on the Hartree–Fock formalism makes many approximations
obtains some parameters from empirical data
Ab Initio models: Hartree–Fock (HF)
solve the molecular Schrödinger equation associated with the molecular Hamiltonian do not include any experimental data, being derived directly from theoretical principles solution is an exact one; they are all approximate quantum mechanical calculations
Density Functional Theory (DFT) models:
often considered as ab initio method, although uses parameters derived from empirical data (or from more complex calculations)
total energy is expressed in terms of the total one-electron density rather than the wave function can be very accurate for little computational cost
Quantum Mechanics (QM) methods
World of Molecules: Computational chemistry
Basis Sets
Basis Sets used by Semi-Empirical models:
Slater type functions (combinations of Gaussian functions) Considers only valence electrons (+ parameterized)
• AM1: upper main group elements + Zn
• PM3: main group elements + transition metals
• MNDO: many main group elements + Zn
Basis sets are a set of functions used to create the molecular orbitals expanded as a linear combination of such functions with the weights or coefficients to be determined. These functions are:
• atomic orbitals (centered on atoms)
• centered on bonds or lone pairs
• functions centered in the two lobes of a p orbital
World of Molecules: Computational chemistry
Basis Sets
Basis Sets used by Ab Initio (HF) models: (Non–empiric!)
Based on the Hartree-Fock self-consistent field (HF-SCF) method using Gaussian functions and includes all electrons with minimal approximation.
Large collection of methods and levels of theory for electron correlation and basis functions
• STO-3G Minimal basis set – unreliable energetics
• 3-21G(*) Split-valence / Double Zeta – excellent results
• 6-31G* Polarized basis set – highly accurate
• 6-311+G** Extended basis set – highly accurate Basis Sets used by DFT models:
Based on electron density and includes electron correlation
World of Molecules: Computational chemistry
Which computational method should I choose?
“Choose your method wisely, and interpret your results with care”
Molecule size (number of atoms)
CPU time / memory
Correlated methods
conformational analysis, starting geometries for other calculations, basic questions of structure and shape basic description of structure and bonding, vibrational spectra, starting geometries for higher level calculations
more accurate prediction of structure and properties, NMR spectra, relative
energies of isomers, qualitative description of transition states and reactions
excited states, UV spectra, transition state energies, structures with unusual bonding schemes, most accurate
predictions of structure and properties
Ab initio models
Semi-empirical models Molecule mechanics
World of Molecules: Computational chemistry
II. Basics
World of Molecules: Computational chemistry
Atom coloring conventions in SPARTAN-ban
*van der Waals radii of atoms is shown in „preferences”
World of Molecules: Computational chemistry
*
wire / ball & wire
Molecule display methods in SPARTAN
tube / ball & sticks
Space Filling (CPK) World of Molecules: Computational chemistry
Calculation methods in SPARTAN
Equilibrium Geometry
specifies that the nearest energy minimum will be located Transition State Geometry
the nearest first-order saddle point (energy maximum in one dimension and energy minima in all other dimensions or commonly known as a transition state) will be located
Equilibrium Conformer/ Conformer Distribution / Conformer Library characterizes the conformers available to a molecule based on different criteria Energy Profile
steps along a user-defined coordinate Similarity
quantifies the likeness among molecules based either on
• structure
• chemical functionality
• between molecules and a template (e.g. pharmacophore)
World of Molecules: Computational chemistry
Atoms (and molecules) are made up of nuclei surrounded by a electron cloud. The size and shape of the electron cloud that defines the size and shape of the molecule. The size and shape of an electron cloud is described by the electron density (the number of electrons per unit volume).
Consider a graph of electron density in the hydrogen atom as a function of distance from the nucleus.
Electron Density Surfaces
distance from nuclei
electron density
Electron cloud lacks a clear boundary.
While electron density decays rapidly with distance from the nucleus, it is never falls to zero. If atoms and molecules ‘rub up against each other’, their electron clouds overlap and merge to a small extent.
World of Molecules: Computational chemistry
A surface formed by a set of interpreting spheres (atoms) with specific van der Waals radii, and which is intended to represent overall molecular size and shape. If Space Filling (left) display model is selected the van der Waals radii of atoms are shown. The size of spheres in ‘Ball and wire’
models (right) is correlated with the van der Waals radii, but not equal!
van der Waals Surface
World of Molecules: Computational chemistry
III. Examples
World of Molecules: Computational chemistry
Example 1: rotamers of n-butane
Each point of the energy diagram represents a certain conformational
isomer of the n-butane. The energy of these isomers can be calculated and plotted as a function of the dihedral angle. Those are on the bottom of the energy valleys are low energy conformers.
60° 120° 180° 240° 300° 360°
H H
H CH3 H
CH3 H H
H CH3 CHH3
CH3 H
H CH3 HH
H CH3
H CH3 H
H
C H3 H
H CH3 HH
H H
H CH3 H C H3
H H
H CH3 CHH3
0.7 2.9 5.8 rel. E (kcal)
0° dihedral angle
World of Molecules: Computational chemistry
Example 1: rotamers of n-butane
World of Molecules: Computational chemistry
Example 2: Claisen rearrangement of allyl vinyl ether
CH2 CH2
O O
C H2 O
Allyl vinyl ether undergoes Claisen rearrangement. The mechanism of this reaction presumes a chair arrangement of the reactant.
Is this chair arrangement the lowest-energy conformer (global minimum) or is additional energy required to properly orient the molecule this way? To find out, all the conformers of allyl vinyl ether must be identified and its energy to be evaluated. The energy of best chair-like structure and that of the actual global minimum must be compared.
World of Molecules: Computational chemistry
Conformer 001 is the lowest energy conformer (global minimum) but in this structure the distance of key atoms are to far to form a new bond. No arrangement is possible starting from this conformer.
Conformer 005 (a local minimum) has the shortest distance between the key atoms. The energy of this structure is higher than conformer 001, but the rearrangement may be possible.
This indicates some energy is required to the formation of the transition state geometry.
5,31 Å 3,70 Å
Molecule001 Molecule002
C C dist. E (MM) difference E (ab-initio) difference Molecule001 5.31 Å 69.9645177 ~ 8.4 kcal/mol -705715.538 ~ 6.1 kcal/mol
Molecule005 3.70 Å 78.4275912 -705709.437
Example 2: Claisen rearrangement of allyl vinyl ether
World of Molecules: Computational chemistry
Example 3a: π-electron system of butadiene
HOMO – highest occupied molecular orbital LUMO – lowest unoccupied molecular orbital E
AO
1 2
3 4
ψ1 ψ2 ψ3
ψ4
π∗
π π∗
π E1
E2 HOMO
LUMO
HOMO-1 LUMO+1
bonding MOsnon-bonding MOs
World of Molecules: Computational chemistry
Example 3a: π-electron system of butadiene
World of Molecules: Computational chemistry
Ψ
1Ψ
2Ψ
3Ψ
4∗ Ψ
5∗
Ψ
6∗
Example 3b: π-electron system of benzene
World of Molecules: Computational chemistry
Example 3b: π-electron system of benzene
World of Molecules: Computational chemistry
Example 4: hydrogenation of benzene
benzene 1,3-cyclohexadiene cyclohexene cyclohexane
H2 H2 H2
Compound E (kJ/mol)
benzene (bnz) -602341
1,3-cyclohexadiene (chd) -605282
cyclohexene (che) -608405
cyclohexane (cha) -611524
hydrogen molecule (H) -2948
Ebnz + EH = -605290 Echd = -605282
ΔE ≈ 7 kJ/mol
Echd + EH = -608231 Eche = -608405
ΔE ≈ -175 kJ/mol
Eche + EH = -611354 Echa = -611524
ΔE ≈ -170 kJ/mol Ebnz + EH < Echd Echd + EH >> Eche Eche + EH >> Echa
benzene 1,3-cyclohexadiene cyclohexene cyclohexane
>> > >
World of Molecules: Computational chemistry
Example 4: hydrogenation of benzene
World of Molecules: Computational chemistry
Example 5: addition vs. substitution
cyclohexene
+Br2 Br
Br
Br
+
HBrvs.
1-bromocyclohexene trans-1,2-dibromo-
cyclohexane
Br
Br
Br
+
HBrvs.
bromobenzene trans-5,6-dibromo-
cyclohexa-1,3-diene benzene
+Br2
Label E (kJ/mol)
trans-1,2-dibromo-cyclohexane (chp1) -14052494
1-bromocyclohexene(chp2) -7328885
trans-5,6-dibromo-cyclohexa-1,3-diene (bzp1) -14046251
bromobenzene (bzp1) -7322809
hydrogen bromide (HBr) -6723497
Echp1 = -14052494 < Echp2 + EHBr= -14052382
Ebzp1 = -14046251 > Ebzp2 + EHBr = -14046306
alkenes → addition arenes → substitution World of Molecules: Computational chemistry
Example 5: addition vs. substitution
World of Molecules: Computational chemistry
Example 6: Electrophylic aromatic substitution (S
EAr)
W = Wheland intermediate arenium ion σ-complex
W E
r Y H CH3
CH3 H
CH3
δH+ δ+
δ+
δ+
Y
Y Y
CH3
Y
Y H CH3 Y
H CH3
Y H CH3
Y H CH3 + CH3+
- H+ slow
fast Y Y = CH3, OCH3
Hammond's Postulate!
Alkylation (methylation)
CH3
toluene
OMe
anisol
Y
CH3 H
Y
CH3 H
Y
CH3H
o-intermediate m-intermediate p-intermediate
World of Molecules: Computational chemistry
Example 6: Electrophylic aromatic substitution (S
EAr)
World of Molecules: Computational chemistry
The electrostatic potential map projects the value of the electrostatic potential to the electron density surface. According to the conventional coloring, red represents the negative potential, while blue represents the positive potential. Colors in between (such as orange, yellow, green) represent the intermediate values of the potential.
Example 7: Electrostatic potential map
The main advantages of this presentation are its clarity and its compactness. The main disadvantage is that it provides only information about the contact surface and does not reveal how deep electron-rich and electron-poor areas extend beyond the surface.
World of Molecules: Computational chemistry
Electrostatic potential map for p-tert-butylphenol shows oxygen to be red, its attached (acidic) hydrogen to be blue, the π faces of benzene to be orange or yellow and the tert-butyl group to be green.
Example 7: Electrostatic potential map
World of Molecules: Computational chemistry
Example 7: Acidities of Carboxylic Acids
O
OH Cl
H H
chloracetic acid pKa = 2.85
O
OH Cl
H Cl
dichloracetic acid pKa = 1.48
O
OH Cl
Cl Cl
trichloracetic acid pKa = 0.7 O
OH H
formic acid pKa = 3.75 O
OH C
H3
acetic acid pKa = 4.75 O
OH benzoic acid
pKa = 4.19
O
OH CH3
CH3 C
H3
pivalic acid pKa = 5.03
Sareant, E.P., Dempsey, B., Ionization constants of Organic Acids in Aqueous Solution, IUPAC no. 23, Permagon Press, 1979.
World of Molecules: Computational chemistry
Example 7: Acidities of Carboxylic Acids
World of Molecules: Computational chemistry
The LUMO map projects the absolute value of the lowest-unoccupied molecular orbital (the LUMO) onto an electron density surface. According to the conventional coloring, blue indicates the high concentration of the LUMO, while red indicates the low concentration. For example, given that the LUMO designates space available for a pair of electrons, a LUMO map indicates where nucleophilic attack would likely occur.
Example 8: LUMO map
World of Molecules: Computational chemistry
LUMO map for cyclohexenone shows concentration in two regions:
• over the carbonyl carbon (1)
• over the β carbon (2)
These areas ara consistent with both a possible carbonyl addition and Michael (conjugate) addition.
Example 8: LUMO map
World of Molecules: Computational chemistry
1.
2.
Michael addition is a nucleophylic addition of a carbanion or another nucleophyle to an α,β unsaturated carbonyl compound. Electron-
withdrawing substituents on the nucleophyle (groups such as acyl and cyano) leads to asymmetric Michael additions.
C C EWG H H
H
HY
base Y CH2 CH2 EWG
H
H H
N
Acrylonitrile
H
H H
N O
O
Nitroethane
H
H H
NH2 O
Acrylamide
H
H H
Styrene
Example 8: LUMO map
World of Molecules: Computational chemistry
Example 8: LUMO map
World of Molecules: Computational chemistry
Example 9: S
N2 reaction of bromide and methyl chloride
The SN2 reaction goes through a transition state with trigonal bipyramid geometry, in which the entering and leaving groups are colinear. The energy and the structure of the intermediate steps can be modelled, the changes in electrostatic charges and in bondlenghts can be plotted.
intermediate
reaction coordinate E
SN2
SN1
World of Molecules: Computational chemistry
Br-
+
C ClH
H
H Br C
+
Cl-H
H H
C Cl
H
H H
Br
Example 9: S
N2 reaction of bromide and methyl chloride
World of Molecules: Computational chemistry
Example 10: estimating reaction speed by LUMO energy
CH2 ED
+
CH2 EA
ED
EA
ED (electron donor) = R, OR
EA (electron acceptor) = CN, CHO, CO2H diene dienophil
HOMO
LUMO
Energy
diene dienophil
better electron acceptors better electron donors
In a Diels-alder reaction an ‘elctron rich’ diene reacts with an ‘electron deficient’ dienophile. The better π-electron donor the substituent of the diene is or the better π-electron acceptor the
substituent of the dienophil is the higher the reaction rate will be (the faster the reaction will be).
World of Molecules: Computational chemistry
CH2 N
acrylonitrile
CH2 N N
1,1-dicyanoethylene
N N
cis-1,2-dicyanoethylene
N
N
transz-1,2-dicyanoethylene
N N N
tricyanoethylene
N N N
N
tetracyanoethylene log10 = 0 log10 = 4.64 log10 = 1.94
log10 = 7.61 log10 = 5.66
log10 = 1.89
Example 10: estimating reaction speed by LUMO energy
World of Molecules: Computational chemistry
Example 10: estimating reaction speed by LUMO energy
World of Molecules: Computational chemistry
Example 11: Thermodynamic vs. kinetic control
+
OO
O
O
H H
O O
O
H H
O O
+
The yield of different products in chemical reactions is depended on the conditions under which they are carried out. High temperatures and long reaction times favor the most stable (thermodynamic) products. Low temperatures and short reaction times favor the most easily formed (kinetic) products. For example, in Diels-Alder cycloaddition the kinetic product is the endo adduct, whereas it seems likely that the less-crowded exo adduct is the thermodynamic product.
„endo” product „exo” product
World of Molecules: Computational chemistry
E Emax Emin Eact Erctn
endo -202.064243 -117.005624 -349.503866 85.058619 147.439623
exo -202.355946 -116.373315 -356.166563 85.982631 153.810617
„endo” product „exo” product
Eact Eact
Erctn Erctn
Example 11: Thermodynamic vs. kinetic control
World of Molecules: Computational chemistry
Example 12: IR spectra simulation
Molecules have different vibrations, such as stretch, bend or twist. These vibrations persist even if the molecule is cooled to absolute zero. These vibrations are the basis of infrared (IR) spectroscopy. If the frequency of the light which irradiates the compound matches the frequency of a
particular molecular motion, the light will be absorbed. IR spectroscopy is important for identifying molecules as different functional groups vibrate at noticeably different and characteristic frequencies, especially in the so called ‘fingerprint region’.
The Spectra dialog of SPARTAN lists 45 vibrational frequencies for cyclohexanone. The motions of these vibrations can be displayed on the model of the molecule. The frequency at 1700 1/cm is corresponding to the CO (carbonyl) stretch. The experimental IR spectrum can be downloaded from a database and can be compared with the calculated spectrum.
World of Molecules: Computational chemistry
experimental calculated
World of Molecules: Computational chemistry
Example 12: IR spectra simulation
NH NH COOH
H2N-CH2-COOH Glycine (Gly) G
Proline (Pro) P
CH3 CH3
CH3
CH3 CH3
CH3
CH3 Alanine (Ala) A Valine (Val) V Leucine (Leu) L Isoleucine (Ile) I
S CH3 SH
Methionine (Met) M Cystei (Cys) C OH
Tyrosine (Tyr) Y Tryptophane (Trp) W Phenylalanine (Phe) F
Alifás
Aromás R =
Hidrophobic
Kéntartalmú Polar
R H
H2N COOH World of Molecules: Computational chemistry
R =
NH N
NH2 O
Histidine (His) H
Asparagine (Asn) N
NH2 O
OH
O OH
O
Glutamine (Gln) Q
Aspartic acid (Asp) D Glutamic acid (Glu) E Lysine (Lys) K Arginine (Arg) R
OH Serine (Ser) S
CH3 OH Threonine(Thr) T Positive
Negative
Polar NH NH2
NH2 N
World of Molecules: Computational chemistry
Chirality of amino acids
non chiral!
L = S
D = R L = R
D = S
exception!
Cysteine
Alanine Glycine Serine
World of Molecules: Computational chemistry
Peptide bond, disulfide bond
disulfide bond
Ala Gly
Ser
Cys
peptide bond
World of Molecules: Computational chemistry
Ser
ω dihedral: Cα
i– C’
i– N
i+1– Cα
i+1ψ dihedral: N
i– Cα
i– C’
i– N
i+1Φ dihedral: C’
i-1– N
i– Cα
i –C’
iALAi+1
Cαi+1
↓
↑ C’i+1
↑ Ni+1
ALAi-1
Cαi-1
↓ ↑
C’i-1
↑ Ni-1
ALAi
↑ Cαi
C’i
↓
Ni
↓
Peptide dihedrals
World of Molecules: Computational chemistry
A Ramachandran plot
Gopalasamudram Narayana Iyer Ramachandran, or G.N. Ramachandran, (8 October 1922 - 7 April 2001) is widely acknowledged as one of the most important Indian scientists of the 20th century, best known for his work that led to his creation of the Ramachandran plot for understanding peptide structure. He was the first to propose a triple-helical model for the structure of collagen. He also made other major contributions in biology and physics.
World of Molecules: Computational chemistry
Intramolecular hydrogen bonds in α-helix
Hydrogen bonds ~ 5 - 30 kJ/mol ~ 3 Å
World of Molecules: Computational chemistry
Intramolecular hydrogen bonds in β-sheets
World of Molecules: Computational chemistry
Humán monoamine-oxidase B (MAO-B) enzime UNIPROT database (www.uniprot.org) under the code P27338
Member of the flavine monoamin oxidase family contains 520 aminoacids (in homo sapiens)
may exists as a homdimer or either heterodimer form shows enzime activity only in monomer form
Function in living organism is the oxidative
deamination of both biogen amins and xenobiotics
MAO-B enzime
World of Molecules: Computational chemistry
World of Molecules: Computational chemistry
Cofactor: flavine-adenozine diphosphate (FAD)
RCH2NHR' + H2O + O2 = RCHO + R'NH2 + H2O2.
Located mostly in the cytoplasm, anchored to the membrane of the mitokondria
UNIPROT database:
MAO-B enzime
World of Molecules: Computational chemistry
location the surroundings of the binding site
MAO-B enzime
World of Molecules: Computational chemistry
G-protein-coupled receptors (GPCRS)
ECL = extra cellular loop
ICL = intra cellular loop TM = transmembrane domain
NT =
N-terminal
CT =
C-terminal
World of Molecules: Computational chemistry
Cherezov V. és munkatársai. High-resolution crystal structure of an engineered human beta2-adrenergic G protein-coupled receptor.
Science2007, 318, 1258-1265.
Okada, T.. és munkatársai. The retinal conformation and its environment in rhodopsin in light of a new 2.2 A crystal structure.
J. Mol Biol.2004, 342, 571-583.
PDB ID 1U19 2RH1
Year of publication: 2004 2007
Species: bovine human (+ enterobcteria phageT4)
Protein: rodopsin β2-adrenoceptor (+ antitest)
Resolution: 2.2 Å 2.4 Å
GPCRs deposited in the Uniprot database
World of Molecules: Computational chemistry
volume: 619 Å3 volume: 482 Å3 volume: 584 Å3
α2A model α2B model α2C model
α
2-adrenoceptor binding sites comparison
World of Molecules: Computational chemistry
α
2-adrenoceptor binding sites comparison
subtype A
subtype B
subtype C
ligand: noradrenaline
World of Molecules: Computational chemistry