1) The document describes the structure of materials at different length scales from atomic to macroscopic levels. It discusses how atomic structure influences properties and technological applications of materials.
2) Key concepts covered include the structure of the atom, electronic configuration, periodic table, different types of atomic bonding, and how bonding influences properties like conductivity and strength.
3) Examples calculate the number of atoms in materials and compare properties like electronegativity between elements. Diagrams illustrate different types of bonding and how structure determines properties.
This document discusses crystal structure and properties of solids. It begins by defining long-range order and crystalline structure, noting that most metals, semiconductors, and some other materials have crystalline structure with atoms arranged in a repetitive grid pattern. It then discusses basic terms like unit cell and space lattice, and describes the seven crystal systems and 14 Bravais lattices. Common metallic crystal structures of body-centered cubic, face-centered cubic, and hexagonal close-packed are discussed. Finally, it touches on X-ray diffraction techniques used to analyze crystal structure.
This document discusses Werner's theory of coordination compounds and bonding in coordination compounds. According to Werner's theory, metal atoms in coordination compounds have both primary and secondary valencies. Primary valencies are ionizable and satisfy the compound's oxidation state, while secondary valencies are non-ionizable and satisfy the compound's coordination number through coordinate covalent bonds with electron pair donors like ligands. The document also discusses Sidgwick's effective atomic number rule and how the valence bond theory explains the geometry, hybridization, and magnetic properties of coordination compounds.
1) The document discusses atomic structure and bonding, covering the history of atomic theory from Dalton to Chadwick. It describes the structure of atoms including protons, neutrons and electrons.
2) Atomic number and mass are defined, and electron configuration is explained using quantum numbers. Different types of chemical bonds are covered - ionic formed by electron transfer, covalent by electron sharing, and metallic by delocalized electrons.
3) Secondary bonds such as hydrogen and van der Waals bonds are also summarized. The periodic table is shown organizing elements by electron configuration. Different classes of elements - metals, nonmetals and metalloids - are defined by their bonding properties.
The document discusses electronic structure of atoms including:
1) Electronic configurations of atoms, ionization energies as evidence for electron shells, and emission spectra as evidence for electron shells.
2) Periods and shells are the same thing.
3) Questions about electron configurations, periods, groups, and specific elements are asked.
This document discusses transition metal coordination compounds and their properties. It begins by explaining color and absorption spectra in relation to an artist's color wheel. It then discusses crystal field theory and how ligand bonding splits the d-orbital energies of metal ions. Stronger field ligands create more splitting. This splitting determines the wavelengths absorbed and the observed color. Examples are given of color changes from oxidation state or ligand changes. The spectrochemical series ranks ligands by field strength. Magnetic properties depend on unpaired electrons. Complexes can be high-spin or low-spin depending on the relative energies of pairing and splitting. Examples of splitting patterns and orbital occupancy are shown for octahedral, tetrahedral, and square planar complexes. Hemoglobin and carbon
Molecular orbital theory (MOT) is an alternative model to valence bond theory that explains how atomic orbitals from different atoms combine to form molecular orbitals. The linear combination of atomic orbitals (LCAO) method considers the probability of finding electrons in atomic orbitals from different atoms. According to the LCAO method, molecular orbitals are formed from constructive and destructive interference of atomic orbitals. MOT can be used to explain bonding in homonuclear diatomic molecules like N2 and O2, heteronuclear diatomic molecules like CO and NO, and polyatomic molecules like CO2 and SF6. It can also describe bonding in octahedral transition metal complexes like hexaaquoferrate(II) ion
1) The document describes the structure of materials at different length scales from atomic to macroscopic levels. It discusses how atomic structure influences properties and technological applications of materials.
2) Key concepts covered include the structure of the atom, electronic configuration, periodic table, different types of atomic bonding, and how bonding influences properties like conductivity and strength.
3) Examples calculate the number of atoms in materials and compare properties like electronegativity between elements. Diagrams illustrate different types of bonding and how structure determines properties.
This document discusses crystal structure and properties of solids. It begins by defining long-range order and crystalline structure, noting that most metals, semiconductors, and some other materials have crystalline structure with atoms arranged in a repetitive grid pattern. It then discusses basic terms like unit cell and space lattice, and describes the seven crystal systems and 14 Bravais lattices. Common metallic crystal structures of body-centered cubic, face-centered cubic, and hexagonal close-packed are discussed. Finally, it touches on X-ray diffraction techniques used to analyze crystal structure.
This document discusses Werner's theory of coordination compounds and bonding in coordination compounds. According to Werner's theory, metal atoms in coordination compounds have both primary and secondary valencies. Primary valencies are ionizable and satisfy the compound's oxidation state, while secondary valencies are non-ionizable and satisfy the compound's coordination number through coordinate covalent bonds with electron pair donors like ligands. The document also discusses Sidgwick's effective atomic number rule and how the valence bond theory explains the geometry, hybridization, and magnetic properties of coordination compounds.
1) The document discusses atomic structure and bonding, covering the history of atomic theory from Dalton to Chadwick. It describes the structure of atoms including protons, neutrons and electrons.
2) Atomic number and mass are defined, and electron configuration is explained using quantum numbers. Different types of chemical bonds are covered - ionic formed by electron transfer, covalent by electron sharing, and metallic by delocalized electrons.
3) Secondary bonds such as hydrogen and van der Waals bonds are also summarized. The periodic table is shown organizing elements by electron configuration. Different classes of elements - metals, nonmetals and metalloids - are defined by their bonding properties.
The document discusses electronic structure of atoms including:
1) Electronic configurations of atoms, ionization energies as evidence for electron shells, and emission spectra as evidence for electron shells.
2) Periods and shells are the same thing.
3) Questions about electron configurations, periods, groups, and specific elements are asked.
This document discusses transition metal coordination compounds and their properties. It begins by explaining color and absorption spectra in relation to an artist's color wheel. It then discusses crystal field theory and how ligand bonding splits the d-orbital energies of metal ions. Stronger field ligands create more splitting. This splitting determines the wavelengths absorbed and the observed color. Examples are given of color changes from oxidation state or ligand changes. The spectrochemical series ranks ligands by field strength. Magnetic properties depend on unpaired electrons. Complexes can be high-spin or low-spin depending on the relative energies of pairing and splitting. Examples of splitting patterns and orbital occupancy are shown for octahedral, tetrahedral, and square planar complexes. Hemoglobin and carbon
Molecular orbital theory (MOT) is an alternative model to valence bond theory that explains how atomic orbitals from different atoms combine to form molecular orbitals. The linear combination of atomic orbitals (LCAO) method considers the probability of finding electrons in atomic orbitals from different atoms. According to the LCAO method, molecular orbitals are formed from constructive and destructive interference of atomic orbitals. MOT can be used to explain bonding in homonuclear diatomic molecules like N2 and O2, heteronuclear diatomic molecules like CO and NO, and polyatomic molecules like CO2 and SF6. It can also describe bonding in octahedral transition metal complexes like hexaaquoferrate(II) ion
e RT
Where;
D0 = Diffusion coefficient at infinite temperature
Q = Activation energy for diffusion
R = Gas constant
T = Absolute temperature
This chapter discusses imperfections in crystals and solidification processes. There are several types of imperfections including point defects like vacancies and interstitial atoms, and line defects like dislocations. Solidification involves nucleation of stable nuclei from liquid, growth of these nuclei into a grain structure, and formation of grain boundaries. Single crystals can be grown using the Czochralski process by slowly pulling a seed crystal from a melt. Diffusion, which is temperature dependent, allows for solid state reactions and involves either vacancy or interstitial mechanisms.
The document summarizes key points about crystal field theory and its application to octahedral complexes. It discusses the historical development of metal complexes, assumptions of crystal field theory, and how it can be applied to explain splitting of d-orbitals in an octahedral complex. It also examines factors that affect crystal field stabilization energy, including the nature of the metal ion and ligands. Finally, it describes how crystal field theory can be used to understand the color and magnetic properties of complexes.
Iron, cobalt and Nickel -ligand bonding in metallocene: Differentiation betwe...AI Publications
The electronic structure and geometry optimization of ferrocene, cobaltocene and nickelocene molecules using DFT/B3LYP with the basis set of 6-31G (d) calculations. The Eigen values, Eigen vector and population analysis of the molecules show that the first 13 molecular orbitals in ferrocene, 12 in cobaltocene and 14 in nickelocene have contribution from 2pzorbitals of carbon of (C5H5)− and4s,4pand 3dorbitals of iron, cobalt or nickel, respectively. We found that the extents of involvement of metal orbitals in the three cases are different. In ferrocene the maximum involvement out of 4s and 4porbitals in the order 4pz >4py >4s > 4pxand out of 3d orbitals the order of involvement is 3dyz >3dxz >3d2z>3dx2−y2>3dxy. The involvement of corresponding orbital in cobaltocene with respect to the 4sand 4porbitals is in the order of 4s >4pz >4py >4pxand in 3d orbitals the order is 3dx2−y2>3dxz >3d2z>3dx2−y2 and in the nickelocene molecule it is 4py >4p>4s >4pz and in 3d orbitals the order is 3dyz >3dx2−y2>3dxy >3dxz >3d2z. The total involvement of 3d, 4s and 4porbitals of metal and 2pz orbitals of the ten carbon atoms of both ligands of (C5H5) −in ferrocene, cobaltocene and nickelocene respectively are 42.2528, 40.2388 and 38.3776
The document summarizes four new heterometallic molecular aggregates containing cobalt and lanthanide metals. Compounds 1 and 2 have the formula [(CoII)3(CoIII)2Ln3(μ3-OH)5(O2CtBu)12(L)2]·2H2O and feature distorted cubane cores, while compounds 3 and 4 have the formula [(CoIII)3Ln3(μ3-OH)4(O2CtBu)6(L)3](NO3)2·2CH3CN·2H2O and display hemicubane-like metallic cores. Magnetic studies show significant magnetic entropy changes for 1 and 3, and single molecule magnetic
This document discusses formal charge and how to calculate it in Lewis structures. It provides examples of calculating formal charges for different Lewis structures of the thiocyanate ion. The preferred structure is the one that puts the negative charge on the most electronegative atom (nitrogen) and has the fewest formal charges of largest magnitude. A practice problem is then given to draw the Lewis structures of the cyanate ion and identify the preferred structure based on these guidelines.
The document discusses molecular orbital theory and its application to diatomic molecules. It introduces molecular orbital theory, developed in 1932, which uses linear combinations of atomic orbitals to form molecular orbitals. Bonding molecular orbitals contain electrons and increase stability, while antibonding orbitals contain electrons and decrease stability. The number of molecular orbitals formed equals the number of atomic orbitals combined. Molecular orbital theory can be used to predict the existence of molecules and explain their properties based on molecular configurations and bond orders.
Valence Bond Theory (VBT) explains the nature of metal-ligand bonding in complex compounds. VBT assumes that the central metal atom forms hybrid orbitals with its outer shell orbitals that overlap with ligand orbitals to form sigma bonds. There are two types of hybridization that result in octahedral geometry: d2sp3 for "inner-orbital" complexes with paired electrons, and sp3d2 for "outer-orbital" complexes with unpaired electrons. Examples that form via d2sp3 hybridization, making them inner-orbital complexes, include ferricyanide ([Fe(CN)6]3-), ferrocyanide ([Fe(CN)6]4-
This document summarizes the synthesis and characterization of two novel phosphonate-based cobalt cages. The first cage (Co15) has an inorganic core shaped like a distorted cubic structure composed of pentagonal faces. The second cage (Co12) has an inorganic core resembling a butterfly shape composed of hexagonal and triangular faces forming a tetrahedral geometry. Magnetic characterization shows both cages exhibit intramolecular antiferromagnetic interactions and zero field splitting at low temperatures.
Dipole-directed Assembly of Lines of Dichloropentane on Silicon Substrates by...ioneec
One-dimensional nanostructures at silicon surfaces have potential applications in nanoscale devices. Here we propose a mechanism
of dipole-directed assembly for the growth of lines of physisorbed dipolar molecules. The adsorbate chosen was a halide,
in preparation for the patterned imprinting of halogen atoms. Using scanning tunnelling microscopy, physisorbed
1,5-dichloropentane on Si(100)-231 was shown to self-assemble at room temperature into molecular lines that grew
predominantly perpendicular to the Si-dimer rows. Line formation was triggered by the displacement of surface charge by
the dipolar adsorbate. Experimental and simulated scanning tunnelling microscopy images were in agreement for a range of
positive and negative bias voltages. The geometry of the physisorbed molecules and nature of their binding were evident from
the scanning tunnelling microscopy images, as interpreted by scanning tunnelling microscopy simulation.
Ch-27.1 Basic concepts on structure of solids.pptxksysbaysyag
The document discusses various topics related to materials science including:
1. Common crystal structures of metals such as FCC, BCC, and HCP and how some metals can change structure with temperature.
2. Plastic deformation in metals occurs through slip and twinning which involve the movement of atoms along crystallographic planes.
3. Atomic structure consists of electrons surrounding the nucleus in shells and the number of valence electrons influence material properties and bonding.
4. Primary bonding types are ionic, covalent, and metallic which influence properties like strength, conductivity, and deformation behavior.
The International Journal of Engineering & Science is aimed at providing a platform for researchers, engineers, scientists, or educators to publish their original research results, to exchange new ideas, to disseminate information in innovative designs, engineering experiences and technological skills. It is also the Journal's objective to promote engineering and technology education. All papers submitted to the Journal will be blind peer-reviewed. Only original articles will be published.
This document discusses periodicity and trends in properties across and down periods of the periodic table. It explains that atomic radius generally decreases across periods as nuclear charge increases, outweighing constant screening effects. Atomic radius increases down groups as nuclear charge rises but screening effects also increase. Ionic radius follows similar trends as atomic radius but is smaller for cations and larger for anions. Melting and boiling points are influenced by type and strength of bonding. Metallic bonding results in higher melting points for metals with more delocalized electrons. Network covalent bonding in nonmetals produces high melting points due to needing to overcome many bonds. Molecular nonmetals have weaker van der Waals forces between molecules. First ionization energies also follow trends
Crystal structures determine material properties. Common structures are FCC, BCC, and HCP. FCC materials like copper are soft while BCC like tungsten are hard. HCP materials include magnesium and zinc. Cobalt and chromium can transform between structures with temperature changes. Grain boundaries in materials are weak points that chemicals can attack. Plastic deformation occurs through slip and twinning along crystal planes. Ductile fracture follows plastic deformation while brittle fracture precedes it.
d & f-block elements 12th Chemistry.pdfKapilPooniya
The document discusses trends in the electronic configurations and properties of elements in the d-block of the periodic table. It notes that chromium and copper have anomalous electronic configurations that can be explained by extra stability from half-filled or completely filled subshells. It also describes how atomic radii, density, ionic radii, oxidation states, and magnetic properties generally trend across and down the d-block in the periodic table.
The document discusses the crystal structures of crystalline solids. It describes three common crystal structures - face centered cubic (FCC), body centered cubic (BCC), and hexagonal close packed (HCP). FCC has a total of four atoms in the unit cell and is found in metals like copper and gold. BCC has an atomic packing factor of 0.68 and is exhibited by metals like iron and chromium. HCP has the same coordination number and packing factor as FCC and is found in metals such as magnesium and zinc. Crystallographic directions and planes are also introduced and ways to determine their indices are explained.
1. The document discusses atomic structure and bonding. It describes the structure of atoms in terms of electrons and the nucleus containing protons and neutrons. It also discusses the arrangement of electrons in shells and the significance of noble gas structures and valency electrons.
2. The document then covers the periodic table and periodic trends. It defines properties such as atomic number, mass number, and isotopes. It explains how the periodic table is arranged based on these properties and how elements in the same group have similar properties.
3. The types of bonding are described including ionic bonding between metals and non-metals which forms ionic lattices, and covalent bonding between non-metals which forms molecules by sharing electron
High Tc superconductor based on perovskite oxideSanjeev Ranjan
The document discusses perovskite-type oxides and their role in high-temperature superconductivity. It begins by defining perovskite structures and describing the key properties of superconductors. It then details the author's involvement in searching for higher transition temperature (Tc) superconductors by exploring systems containing transition metal ions that exhibit Jahn-Teller distortions, like copper-containing oxides. This led to the breakthrough discovery of superconductivity above liquid nitrogen temperatures in barium-doped lanthanum copper oxide, with further improvements by substituting yttrium for lanthanum yielding a Tc of 92K in yttrium barium copper oxide.
IRJET- Silicon based Molecular ElectronicIRJET Journal
This document presents a theoretical framework for modeling molecular electronics on silicon substrates. It combines a first-principles description of molecules with a semi-empirical treatment of silicon's bulk band structure. The framework is used to demonstrate negative differential resistance in a molecular resonant tunneling diode when molecular levels are driven by an STM tip into silicon's band gap. Specifically, it shows negative differential resistance peaks for styrene molecules on p-doped silicon at positive biases, and potentially for negative biases on n-doped silicon. This molecular resonant tunneling effect could enable new types of logic and memory devices integrating molecules with silicon technology.
1. A 2D coordination polymer was synthesized using cobalt trimers and the flexible ligand cis,cis-cyclohexane-1,3,5-tricarboxylate.
2. Single crystal X-ray diffraction shows the complex forms a 2D framework with channels and contains trinuclear cobalt secondary building units linked by the ligand.
3. Magnetic characterization reveals spin-canting ferromagnetic behavior at low temperatures based on AC susceptibility measurements. Gas adsorption experiments also show selectivity for CO2 over N2.
This document discusses the valence bond approach to explaining the bonding in octahedral transition metal complexes. It describes how hybrid orbitals are formed from the metal and ligand orbitals, allowing coordinate covalent bonds to form. Octahedral complexes result from sp3d2 hybridization, forming six bonds oriented in an octahedral geometry. The approach can explain magnetic properties and geometries of different complexes, though it has limitations and does not provide quantitative data.
I -s2o.100 Chapter 3 Chemical BondsUWL tnteractive ve.docxadampcarr67227
I -s'2o.
100 Chapter 3 Chemical Bonds
UWL tnteractive versions of these problems may be assigned
in OWL.
Orange-numbered problems are applied.
Section 3.2 What ls the Octet Rule?
3.17 Answer true or false. '
(a) The octet rule refers to the chemical bonding
patterns of the first eight elements of the
Periodic Table.
(b) The octet rule refers to the tendency ofcertain
elements to react in such a way that they achieve
an outer shell ofeight valence electrons.
(c) In gaining electrons, an atom becomes a posi-
tively charged ion called a cation.
(d) When an atom forms an ion, only the number of
. valence electrons changes; the number ofprotons
and neutrons in the nucleus does not change.
(e) In forming ions, Group 2A elements typically
lose two electrons to become cations with a
charge of +2.
(f) In forming an ion, a sodium atom (1s22s22p63s1)
completes its valence shell by adding one elec-
tron to filI its 3s shell (k22s22p63s2).
(g) The elements of Group 6A typically react by ac-
cepting two electrons to become anions with a
charge of -2.
(h) With the exception of hydrogen, the octet rule
applies to all elements in periods 1,2, and 3.
(i) Atoms and the ions derived from them have very
similar physical and chemical properties.
3.18 How many electrons must each atom gain or lose
to acquire an electron configuration identical to the
noble gas nearest to it in atomic number?
(a) Li (b) Cl (c) P (d) Al
(e) Sr (f) S (e) Si (h) O
3.19 Show how each chemical change obeys the octet
rule.
(a) Lithium forms Li* (b) Oxygen forms O
Show how each chemical change obeys the octet rule.
(a) Hydrogen forms H- (hydride ion)
(b) Aluminum forms Al3+
3,2L Write the formula for the most stable ion formed by
each element.
(a) Mg (b) F (c)
(d) s (e) K (I)
3.22 Why is Li- not a stable ion?
3.23 Predict which ions are stable:
(a) I- (b) Se2+ (c) Na* (d) 52- (e) tr12+ (fl Ba8+
3,24 Predict which ions are stable:
(a) Br2- (b) C4- (c) Ca*
(d) Ar* (e) Na* (I) Cs*
a
3.25 Why are carbon and silicon reluctant to foil
bonds?
3.26 Table 3.2 shows the following ions of co14m
and Cu2*. Do these violate the octet rule?
Section 3.3 How Do We Name Anions
and Cations?
5.27 Answer true or false.
(a) For Group 1A and Group 2A elements,fte
of the ion each forms is simply the nare
element followed by the word ion; for
Mg2* is named magnesium ion.
(b) H+ is named hydronium ion, and H is
hydride ion.
(c) The nucleus of H* consists of one proton
neutron.
(d) Many transition and inner transition
form more than one positively charged irn I
(e) In naming metal cations with two diffemed
charges, the suffix -oas refers to the ion
a charge of + 1 and -ic refers to the ion wift
charge of +2.
(f) Fe3* may be named either iron(III) ion or
(g) The anion derived from a bromine atom is
bromine ion.
(h) The anion derived from an oxygen atomis
named oxide ion.
(i) HCO; is named hydrogen carbonate ion- .
0) The prefrx bi- in the name "bicarbonate'im
indicates that this ion h.
BOHR'S MODEL 3 ch4 structure of atom cl ixHarAmritKaur6
1. Bohr's model of the atom refined Rutherford's model by suggesting that electrons orbit the atomic nucleus in fixed shells or energy levels, similar to planets orbiting the sun.
2. Each orbit can only hold a set number of electrons. The location of electrons is described by electronic configurations that show how electrons fill atomic shells.
3. Atoms are represented through electronic configurations that numerically list the shells and number of electrons, or through dot-and-cross diagrams that visually depict electrons and shells.
e RT
Where;
D0 = Diffusion coefficient at infinite temperature
Q = Activation energy for diffusion
R = Gas constant
T = Absolute temperature
This chapter discusses imperfections in crystals and solidification processes. There are several types of imperfections including point defects like vacancies and interstitial atoms, and line defects like dislocations. Solidification involves nucleation of stable nuclei from liquid, growth of these nuclei into a grain structure, and formation of grain boundaries. Single crystals can be grown using the Czochralski process by slowly pulling a seed crystal from a melt. Diffusion, which is temperature dependent, allows for solid state reactions and involves either vacancy or interstitial mechanisms.
The document summarizes key points about crystal field theory and its application to octahedral complexes. It discusses the historical development of metal complexes, assumptions of crystal field theory, and how it can be applied to explain splitting of d-orbitals in an octahedral complex. It also examines factors that affect crystal field stabilization energy, including the nature of the metal ion and ligands. Finally, it describes how crystal field theory can be used to understand the color and magnetic properties of complexes.
Iron, cobalt and Nickel -ligand bonding in metallocene: Differentiation betwe...AI Publications
The electronic structure and geometry optimization of ferrocene, cobaltocene and nickelocene molecules using DFT/B3LYP with the basis set of 6-31G (d) calculations. The Eigen values, Eigen vector and population analysis of the molecules show that the first 13 molecular orbitals in ferrocene, 12 in cobaltocene and 14 in nickelocene have contribution from 2pzorbitals of carbon of (C5H5)− and4s,4pand 3dorbitals of iron, cobalt or nickel, respectively. We found that the extents of involvement of metal orbitals in the three cases are different. In ferrocene the maximum involvement out of 4s and 4porbitals in the order 4pz >4py >4s > 4pxand out of 3d orbitals the order of involvement is 3dyz >3dxz >3d2z>3dx2−y2>3dxy. The involvement of corresponding orbital in cobaltocene with respect to the 4sand 4porbitals is in the order of 4s >4pz >4py >4pxand in 3d orbitals the order is 3dx2−y2>3dxz >3d2z>3dx2−y2 and in the nickelocene molecule it is 4py >4p>4s >4pz and in 3d orbitals the order is 3dyz >3dx2−y2>3dxy >3dxz >3d2z. The total involvement of 3d, 4s and 4porbitals of metal and 2pz orbitals of the ten carbon atoms of both ligands of (C5H5) −in ferrocene, cobaltocene and nickelocene respectively are 42.2528, 40.2388 and 38.3776
The document summarizes four new heterometallic molecular aggregates containing cobalt and lanthanide metals. Compounds 1 and 2 have the formula [(CoII)3(CoIII)2Ln3(μ3-OH)5(O2CtBu)12(L)2]·2H2O and feature distorted cubane cores, while compounds 3 and 4 have the formula [(CoIII)3Ln3(μ3-OH)4(O2CtBu)6(L)3](NO3)2·2CH3CN·2H2O and display hemicubane-like metallic cores. Magnetic studies show significant magnetic entropy changes for 1 and 3, and single molecule magnetic
This document discusses formal charge and how to calculate it in Lewis structures. It provides examples of calculating formal charges for different Lewis structures of the thiocyanate ion. The preferred structure is the one that puts the negative charge on the most electronegative atom (nitrogen) and has the fewest formal charges of largest magnitude. A practice problem is then given to draw the Lewis structures of the cyanate ion and identify the preferred structure based on these guidelines.
The document discusses molecular orbital theory and its application to diatomic molecules. It introduces molecular orbital theory, developed in 1932, which uses linear combinations of atomic orbitals to form molecular orbitals. Bonding molecular orbitals contain electrons and increase stability, while antibonding orbitals contain electrons and decrease stability. The number of molecular orbitals formed equals the number of atomic orbitals combined. Molecular orbital theory can be used to predict the existence of molecules and explain their properties based on molecular configurations and bond orders.
Valence Bond Theory (VBT) explains the nature of metal-ligand bonding in complex compounds. VBT assumes that the central metal atom forms hybrid orbitals with its outer shell orbitals that overlap with ligand orbitals to form sigma bonds. There are two types of hybridization that result in octahedral geometry: d2sp3 for "inner-orbital" complexes with paired electrons, and sp3d2 for "outer-orbital" complexes with unpaired electrons. Examples that form via d2sp3 hybridization, making them inner-orbital complexes, include ferricyanide ([Fe(CN)6]3-), ferrocyanide ([Fe(CN)6]4-
This document summarizes the synthesis and characterization of two novel phosphonate-based cobalt cages. The first cage (Co15) has an inorganic core shaped like a distorted cubic structure composed of pentagonal faces. The second cage (Co12) has an inorganic core resembling a butterfly shape composed of hexagonal and triangular faces forming a tetrahedral geometry. Magnetic characterization shows both cages exhibit intramolecular antiferromagnetic interactions and zero field splitting at low temperatures.
Dipole-directed Assembly of Lines of Dichloropentane on Silicon Substrates by...ioneec
One-dimensional nanostructures at silicon surfaces have potential applications in nanoscale devices. Here we propose a mechanism
of dipole-directed assembly for the growth of lines of physisorbed dipolar molecules. The adsorbate chosen was a halide,
in preparation for the patterned imprinting of halogen atoms. Using scanning tunnelling microscopy, physisorbed
1,5-dichloropentane on Si(100)-231 was shown to self-assemble at room temperature into molecular lines that grew
predominantly perpendicular to the Si-dimer rows. Line formation was triggered by the displacement of surface charge by
the dipolar adsorbate. Experimental and simulated scanning tunnelling microscopy images were in agreement for a range of
positive and negative bias voltages. The geometry of the physisorbed molecules and nature of their binding were evident from
the scanning tunnelling microscopy images, as interpreted by scanning tunnelling microscopy simulation.
Ch-27.1 Basic concepts on structure of solids.pptxksysbaysyag
The document discusses various topics related to materials science including:
1. Common crystal structures of metals such as FCC, BCC, and HCP and how some metals can change structure with temperature.
2. Plastic deformation in metals occurs through slip and twinning which involve the movement of atoms along crystallographic planes.
3. Atomic structure consists of electrons surrounding the nucleus in shells and the number of valence electrons influence material properties and bonding.
4. Primary bonding types are ionic, covalent, and metallic which influence properties like strength, conductivity, and deformation behavior.
The International Journal of Engineering & Science is aimed at providing a platform for researchers, engineers, scientists, or educators to publish their original research results, to exchange new ideas, to disseminate information in innovative designs, engineering experiences and technological skills. It is also the Journal's objective to promote engineering and technology education. All papers submitted to the Journal will be blind peer-reviewed. Only original articles will be published.
This document discusses periodicity and trends in properties across and down periods of the periodic table. It explains that atomic radius generally decreases across periods as nuclear charge increases, outweighing constant screening effects. Atomic radius increases down groups as nuclear charge rises but screening effects also increase. Ionic radius follows similar trends as atomic radius but is smaller for cations and larger for anions. Melting and boiling points are influenced by type and strength of bonding. Metallic bonding results in higher melting points for metals with more delocalized electrons. Network covalent bonding in nonmetals produces high melting points due to needing to overcome many bonds. Molecular nonmetals have weaker van der Waals forces between molecules. First ionization energies also follow trends
Crystal structures determine material properties. Common structures are FCC, BCC, and HCP. FCC materials like copper are soft while BCC like tungsten are hard. HCP materials include magnesium and zinc. Cobalt and chromium can transform between structures with temperature changes. Grain boundaries in materials are weak points that chemicals can attack. Plastic deformation occurs through slip and twinning along crystal planes. Ductile fracture follows plastic deformation while brittle fracture precedes it.
d & f-block elements 12th Chemistry.pdfKapilPooniya
The document discusses trends in the electronic configurations and properties of elements in the d-block of the periodic table. It notes that chromium and copper have anomalous electronic configurations that can be explained by extra stability from half-filled or completely filled subshells. It also describes how atomic radii, density, ionic radii, oxidation states, and magnetic properties generally trend across and down the d-block in the periodic table.
The document discusses the crystal structures of crystalline solids. It describes three common crystal structures - face centered cubic (FCC), body centered cubic (BCC), and hexagonal close packed (HCP). FCC has a total of four atoms in the unit cell and is found in metals like copper and gold. BCC has an atomic packing factor of 0.68 and is exhibited by metals like iron and chromium. HCP has the same coordination number and packing factor as FCC and is found in metals such as magnesium and zinc. Crystallographic directions and planes are also introduced and ways to determine their indices are explained.
1. The document discusses atomic structure and bonding. It describes the structure of atoms in terms of electrons and the nucleus containing protons and neutrons. It also discusses the arrangement of electrons in shells and the significance of noble gas structures and valency electrons.
2. The document then covers the periodic table and periodic trends. It defines properties such as atomic number, mass number, and isotopes. It explains how the periodic table is arranged based on these properties and how elements in the same group have similar properties.
3. The types of bonding are described including ionic bonding between metals and non-metals which forms ionic lattices, and covalent bonding between non-metals which forms molecules by sharing electron
High Tc superconductor based on perovskite oxideSanjeev Ranjan
The document discusses perovskite-type oxides and their role in high-temperature superconductivity. It begins by defining perovskite structures and describing the key properties of superconductors. It then details the author's involvement in searching for higher transition temperature (Tc) superconductors by exploring systems containing transition metal ions that exhibit Jahn-Teller distortions, like copper-containing oxides. This led to the breakthrough discovery of superconductivity above liquid nitrogen temperatures in barium-doped lanthanum copper oxide, with further improvements by substituting yttrium for lanthanum yielding a Tc of 92K in yttrium barium copper oxide.
IRJET- Silicon based Molecular ElectronicIRJET Journal
This document presents a theoretical framework for modeling molecular electronics on silicon substrates. It combines a first-principles description of molecules with a semi-empirical treatment of silicon's bulk band structure. The framework is used to demonstrate negative differential resistance in a molecular resonant tunneling diode when molecular levels are driven by an STM tip into silicon's band gap. Specifically, it shows negative differential resistance peaks for styrene molecules on p-doped silicon at positive biases, and potentially for negative biases on n-doped silicon. This molecular resonant tunneling effect could enable new types of logic and memory devices integrating molecules with silicon technology.
1. A 2D coordination polymer was synthesized using cobalt trimers and the flexible ligand cis,cis-cyclohexane-1,3,5-tricarboxylate.
2. Single crystal X-ray diffraction shows the complex forms a 2D framework with channels and contains trinuclear cobalt secondary building units linked by the ligand.
3. Magnetic characterization reveals spin-canting ferromagnetic behavior at low temperatures based on AC susceptibility measurements. Gas adsorption experiments also show selectivity for CO2 over N2.
This document discusses the valence bond approach to explaining the bonding in octahedral transition metal complexes. It describes how hybrid orbitals are formed from the metal and ligand orbitals, allowing coordinate covalent bonds to form. Octahedral complexes result from sp3d2 hybridization, forming six bonds oriented in an octahedral geometry. The approach can explain magnetic properties and geometries of different complexes, though it has limitations and does not provide quantitative data.
I -s2o.100 Chapter 3 Chemical BondsUWL tnteractive ve.docxadampcarr67227
I -s'2o.
100 Chapter 3 Chemical Bonds
UWL tnteractive versions of these problems may be assigned
in OWL.
Orange-numbered problems are applied.
Section 3.2 What ls the Octet Rule?
3.17 Answer true or false. '
(a) The octet rule refers to the chemical bonding
patterns of the first eight elements of the
Periodic Table.
(b) The octet rule refers to the tendency ofcertain
elements to react in such a way that they achieve
an outer shell ofeight valence electrons.
(c) In gaining electrons, an atom becomes a posi-
tively charged ion called a cation.
(d) When an atom forms an ion, only the number of
. valence electrons changes; the number ofprotons
and neutrons in the nucleus does not change.
(e) In forming ions, Group 2A elements typically
lose two electrons to become cations with a
charge of +2.
(f) In forming an ion, a sodium atom (1s22s22p63s1)
completes its valence shell by adding one elec-
tron to filI its 3s shell (k22s22p63s2).
(g) The elements of Group 6A typically react by ac-
cepting two electrons to become anions with a
charge of -2.
(h) With the exception of hydrogen, the octet rule
applies to all elements in periods 1,2, and 3.
(i) Atoms and the ions derived from them have very
similar physical and chemical properties.
3.18 How many electrons must each atom gain or lose
to acquire an electron configuration identical to the
noble gas nearest to it in atomic number?
(a) Li (b) Cl (c) P (d) Al
(e) Sr (f) S (e) Si (h) O
3.19 Show how each chemical change obeys the octet
rule.
(a) Lithium forms Li* (b) Oxygen forms O
Show how each chemical change obeys the octet rule.
(a) Hydrogen forms H- (hydride ion)
(b) Aluminum forms Al3+
3,2L Write the formula for the most stable ion formed by
each element.
(a) Mg (b) F (c)
(d) s (e) K (I)
3.22 Why is Li- not a stable ion?
3.23 Predict which ions are stable:
(a) I- (b) Se2+ (c) Na* (d) 52- (e) tr12+ (fl Ba8+
3,24 Predict which ions are stable:
(a) Br2- (b) C4- (c) Ca*
(d) Ar* (e) Na* (I) Cs*
a
3.25 Why are carbon and silicon reluctant to foil
bonds?
3.26 Table 3.2 shows the following ions of co14m
and Cu2*. Do these violate the octet rule?
Section 3.3 How Do We Name Anions
and Cations?
5.27 Answer true or false.
(a) For Group 1A and Group 2A elements,fte
of the ion each forms is simply the nare
element followed by the word ion; for
Mg2* is named magnesium ion.
(b) H+ is named hydronium ion, and H is
hydride ion.
(c) The nucleus of H* consists of one proton
neutron.
(d) Many transition and inner transition
form more than one positively charged irn I
(e) In naming metal cations with two diffemed
charges, the suffix -oas refers to the ion
a charge of + 1 and -ic refers to the ion wift
charge of +2.
(f) Fe3* may be named either iron(III) ion or
(g) The anion derived from a bromine atom is
bromine ion.
(h) The anion derived from an oxygen atomis
named oxide ion.
(i) HCO; is named hydrogen carbonate ion- .
0) The prefrx bi- in the name "bicarbonate'im
indicates that this ion h.
BOHR'S MODEL 3 ch4 structure of atom cl ixHarAmritKaur6
1. Bohr's model of the atom refined Rutherford's model by suggesting that electrons orbit the atomic nucleus in fixed shells or energy levels, similar to planets orbiting the sun.
2. Each orbit can only hold a set number of electrons. The location of electrons is described by electronic configurations that show how electrons fill atomic shells.
3. Atoms are represented through electronic configurations that numerically list the shells and number of electrons, or through dot-and-cross diagrams that visually depict electrons and shells.
Research Inventy : International Journal of Engineering and Scienceresearchinventy
Research Inventy : International Journal of Engineering and Science is published by the group of young academic and industrial researchers with 12 Issues per year. It is an online as well as print version open access journal that provides rapid publication (monthly) of articles in all areas of the subject such as: civil, mechanical, chemical, electronic and computer engineering as well as production and information technology. The Journal welcomes the submission of manuscripts that meet the general criteria of significance and scientific excellence. Papers will be published by rapid process within 20 days after acceptance and peer review process takes only 7 days. All articles published in Research Inventy will be peer-reviewed.
Molecular orbital theory describes how atomic orbitals combine to form molecular orbitals through a linear combination of atomic orbitals (LCAO) method. Bonding molecular orbitals are formed by constructive interference and have lower energy, while antibonding molecular orbitals are formed by destructive interference and have higher energy. The bond order is calculated based on the number of electrons in bonding and antibonding orbitals. Molecular orbital theory can explain the magnetic behaviors of molecules like oxygen's paramagnetism.
1997 nucleation of homoepitaxial si chains on si(001) at room temperaturepmloscholte
1) Si dimers initially adsorb at preferred sites on the Si(001) surface, with most occupying C-positions.
2) Interactions between dimers and diffusing adatoms lead to the formation of three-atom clusters like twins and crosses. These can extend into diluted lines of C dimers along [110] and [310] directions.
3) Upon further deposition, the diluted dimer lines transform into epitaxial dimer rows through a process starting at the line ends of reorienting dimers and adding mobile adatoms.
FellowBuddy.com is a platform which has been setup with a simple vision, keeping in mind the dynamic requirements of students.
Our Vision & Mission - Simplifying Students Life
Our Belief - “The great breakthrough in your life comes when you realize it, that you can learn anything you need to learn; to accomplish any goal that you have set for yourself. This means there are no limits on what you can be, have or do.”
Like Us - https://www.facebook.com/FellowBuddycom-446240585585480
The document provides the electronic configurations of various ions of transition metals and lanthanides. It also provides answers to questions related to oxidation states, stability, and properties of transition metal ions and compounds. The key points are:
1) Electronic configurations of ions such as Cr3+, Cu+, Co2+, Mn2+, Pm3+, Ce4+, Lu2+, and Th4+ are given.
2) Mn2+ compounds are more stable than Fe2+ towards oxidation due to the half filled d orbital of Mn2+, making it more stable.
3) Oxidation states of transition metals increase from +2 to higher states with an increase in atomic number due to increasing number of d electrons
This document summarizes periodic trends across Period 3 of the periodic table from sodium to argon. It discusses how physical properties like atomic radius decrease across the period as nuclear charge increases. It also examines how chemical properties vary, such as the reactions of elements with oxygen and chlorine. Oxides of metals are basic while nonmetal oxides are acidic due to differences in bonding. Periodic trends allow prediction of element properties based on position in the periodic table.
Current Ms word generated power point presentation covers major details about the micronuclei test. It's significance and assays to conduct it. It is used to detect the micronuclei formation inside the cells of nearly every multicellular organism. It's formation takes place during chromosomal sepration at metaphase.
When I was asked to give a companion lecture in support of ‘The Philosophy of Science’ (https://shorturl.at/4pUXz) I decided not to walk through the detail of the many methodologies in order of use. Instead, I chose to employ a long standing, and ongoing, scientific development as an exemplar. And so, I chose the ever evolving story of Thermodynamics as a scientific investigation at its best.
Conducted over a period of >200 years, Thermodynamics R&D, and application, benefitted from the highest levels of professionalism, collaboration, and technical thoroughness. New layers of application, methodology, and practice were made possible by the progressive advance of technology. In turn, this has seen measurement and modelling accuracy continually improved at a micro and macro level.
Perhaps most importantly, Thermodynamics rapidly became a primary tool in the advance of applied science/engineering/technology, spanning micro-tech, to aerospace and cosmology. I can think of no better a story to illustrate the breadth of scientific methodologies and applications at their best.
ESA/ACT Science Coffee: Diego Blas - Gravitational wave detection with orbita...Advanced-Concepts-Team
Presentation in the Science Coffee of the Advanced Concepts Team of the European Space Agency on the 07.06.2024.
Speaker: Diego Blas (IFAE/ICREA)
Title: Gravitational wave detection with orbital motion of Moon and artificial
Abstract:
In this talk I will describe some recent ideas to find gravitational waves from supermassive black holes or of primordial origin by studying their secular effect on the orbital motion of the Moon or satellites that are laser ranged.
Sexuality - Issues, Attitude and Behaviour - Applied Social Psychology - Psyc...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
ESR spectroscopy in liquid food and beverages.pptxPRIYANKA PATEL
With increasing population, people need to rely on packaged food stuffs. Packaging of food materials requires the preservation of food. There are various methods for the treatment of food to preserve them and irradiation treatment of food is one of them. It is the most common and the most harmless method for the food preservation as it does not alter the necessary micronutrients of food materials. Although irradiated food doesn’t cause any harm to the human health but still the quality assessment of food is required to provide consumers with necessary information about the food. ESR spectroscopy is the most sophisticated way to investigate the quality of the food and the free radicals induced during the processing of the food. ESR spin trapping technique is useful for the detection of highly unstable radicals in the food. The antioxidant capability of liquid food and beverages in mainly performed by spin trapping technique.
(June 12, 2024) Webinar: Development of PET theranostics targeting the molecu...Scintica Instrumentation
Targeting Hsp90 and its pathogen Orthologs with Tethered Inhibitors as a Diagnostic and Therapeutic Strategy for cancer and infectious diseases with Dr. Timothy Haystead.
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...Leonel Morgado
Current descriptions of immersive learning cases are often difficult or impossible to compare. This is due to a myriad of different options on what details to include, which aspects are relevant, and on the descriptive approaches employed. Also, these aspects often combine very specific details with more general guidelines or indicate intents and rationales without clarifying their implementation. In this paper we provide a method to describe immersive learning cases that is structured to enable comparisons, yet flexible enough to allow researchers and practitioners to decide which aspects to include. This method leverages a taxonomy that classifies educational aspects at three levels (uses, practices, and strategies) and then utilizes two frameworks, the Immersive Learning Brain and the Immersion Cube, to enable a structured description and interpretation of immersive learning cases. The method is then demonstrated on a published immersive learning case on training for wind turbine maintenance using virtual reality. Applying the method results in a structured artifact, the Immersive Learning Case Sheet, that tags the case with its proximal uses, practices, and strategies, and refines the free text case description to ensure that matching details are included. This contribution is thus a case description method in support of future comparative research of immersive learning cases. We then discuss how the resulting description and interpretation can be leveraged to change immersion learning cases, by enriching them (considering low-effort changes or additions) or innovating (exploring more challenging avenues of transformation). The method holds significant promise to support better-grounded research in immersive learning.
The binding of cosmological structures by massless topological defectsSérgio Sacani
Assuming spherical symmetry and weak field, it is shown that if one solves the Poisson equation or the Einstein field
equations sourced by a topological defect, i.e. a singularity of a very specific form, the result is a localized gravitational
field capable of driving flat rotation (i.e. Keplerian circular orbits at a constant speed for all radii) of test masses on a thin
spherical shell without any underlying mass. Moreover, a large-scale structure which exploits this solution by assembling
concentrically a number of such topological defects can establish a flat stellar or galactic rotation curve, and can also deflect
light in the same manner as an equipotential (isothermal) sphere. Thus, the need for dark matter or modified gravity theory is
mitigated, at least in part.
Authoring a personal GPT for your research and practice: How we created the Q...Leonel Morgado
Thematic analysis in qualitative research is a time-consuming and systematic task, typically done using teams. Team members must ground their activities on common understandings of the major concepts underlying the thematic analysis, and define criteria for its development. However, conceptual misunderstandings, equivocations, and lack of adherence to criteria are challenges to the quality and speed of this process. Given the distributed and uncertain nature of this process, we wondered if the tasks in thematic analysis could be supported by readily available artificial intelligence chatbots. Our early efforts point to potential benefits: not just saving time in the coding process but better adherence to criteria and grounding, by increasing triangulation between humans and artificial intelligence. This tutorial will provide a description and demonstration of the process we followed, as two academic researchers, to develop a custom ChatGPT to assist with qualitative coding in the thematic data analysis process of immersive learning accounts in a survey of the academic literature: QUAL-E Immersive Learning Thematic Analysis Helper. In the hands-on time, participants will try out QUAL-E and develop their ideas for their own qualitative coding ChatGPT. Participants that have the paid ChatGPT Plus subscription can create a draft of their assistants. The organizers will provide course materials and slide deck that participants will be able to utilize to continue development of their custom GPT. The paid subscription to ChatGPT Plus is not required to participate in this workshop, just for trying out personal GPTs during it.
PPT on Direct Seeded Rice presented at the three-day 'Training and Validation Workshop on Modules of Climate Smart Agriculture (CSA) Technologies in South Asia' workshop on April 22, 2024.
1. Versatile electronic properties and exotic edge states in single-layer
tetragonal silicon carbides
Chao Yang1, 2
, YueeXie*1
, Li-Min Liu*2
and Yuanping Chen1
1
Department of Physics,Xiangtan University,Xiangtan 411105,Hunan,China.
2
Beijing Computational science Research Center,Beijing 100084,China
*1
Corresponding author: xieyech@xtu.edu.cn
*2
Corresponding author: limin.liu@csrc.ac.cn
Abstract
Three single-layer tetragonal silicon carbides (SiC), termed as T1,T2 and T3, are proposed
by density functional theory (DFT) computations. Although the three structures have the same
topological geometry, they show versatile electronic properties from semiconductor (T1), semimetal
(T2) to metal (T3).The versatile properties are originated from the rich bonds between Si and C
atoms. The nanoribbons of the three SiCalso show interesting electronic properties. Especially, T1
nanoribbons possess exotic edge states, where electrons only distribute on one edge's silicon or
carbon atoms. The band gaps of the T1 nanoribbons are constant because of no interaction between
the edge states.
2. Introduction
The discovery of graphene and itsuniquephysical properties stimulated lots of interest to the
fieldsof two-dimensional (2D) nanostructures.1-4
Vast2Dnanosheets have been proposed based on
variouschemical elements or compounds, in whichsilicene,5, 6
MoS2,7, 8
germanane,9, 10
etc.
aresynthesized successfully and new physical propertiesare found in them.9, 11, 12
This further
promotesthe explorations of new 2D nanomaterials.
Although carbon and siliconboth lie in thefourth column of the periodic table, their 2D
nanosheets are different because of their completely different bonding characteristics. Silicene is a
buckle structure while graphene is a perfect plane.1, 5
Therefore, it is interesting to study what will
happen in the 2D nanosheet consisting of carbon and silicone compound.In the previous studies,
some 2D silicon-carbon compounds including hexagonal rings have been proposed, such as
hexagonalSiC,13, 14
g-SiC2,15
pt-SiC2,16
SiC3,17
etc.These new structuresshowinterestingproperties
such aslarge direct bandgap, improved photoluminescence, and highpower conversion efficiency.
Recently, 2D structures consisting of rectangular rings have drawn much attention gradually.
Liu et al.18
proposed a T-graphene, a 2D tetra-symmetrical carbon sheet, and studied the electronic
properties further. They found that the buckled T-graphene possesses a Dirac point while the planar
structure is a metal. Li et al.19
studied a 2D MoS2 system with the repeated square-octagon rings and
they found that the new MoS2allotrope possess both massless Dirac and heavy fermions near the
Fermi surface. These studies indicate that the 2Dtetra-symmetrical sheets havetheir own unique
physical properties. To the best of our knowledge, 2D silicon carbides consisting of rectangular
rings have never been studied up to date and thus it is nature to ask whatnew electronic properties
do the 2D tetragonalSiChave.
3. In this paper, we proposethree 2DtetragonalSiCsheets,termed as T1, T2 and T3, as shown in
Fig. 1. The cohesive energies and phonon dispersions of these 2Dsheets indicate that they are meta-
stable SiCallotropes. Although the three structures have the same topological geometry, they exhibit
completely different electronic properties,varying from metal to semimetal with Dirac cone and
then to semiconductor. T1 consisting of Si-C bonds is a semiconductor. T2 and T3 consist of three
kinds of bonds, i.e., Si-C, C-C and Si-Si. The former is a semimetal because of its two (Si and C)
rectangular sublattices, while the later is a metal because of the C-C and Si-Si dimers between the
rectangular rings. The electronic properties of nanoribbons of the 2D structures are also studied. We
find that the band gaps of T1 nanoribbons are constant, and in these ribbons there exist exotic edge
states whereelectrons only distribute on the (Si or C) edge atoms of one side.
Models and Methods
The three 2DtetragonalSiCs, named as T1, T2 and T3, are shown in Figs. 1(a-c),
respectively.All structures have the same topological geometry consisting of four-membered
rings.The ratios of C and Si atoms are 1:1. Thefour-membered rings inT1 and T3have two C atoms
and two Si atoms, while those in T2 are pure carbon rings or silicone rings.T1only consists of Si-C
bonds while T2 and T3 consist of three kinds of bonds, C-C, Si-Si and Si-C. These tetragonal 2D
SiCspossibly can be synthesized experimentally by using bottom-up method because of existing of
C, Si and SiC four-membered moleculessuch as the C4H4,Si2C2, Si4, (Si4H4)2-
, etc.20-24
The corresponding calculations were employing theVienna ab initio simulation package
(VASP).25
The interaction between ions and electrons is described by the projector-augmented wave
(PAW) method as the plane-wave basis set with an energy cutoff of 450eV is used.26
The PBE
functional constructed by Perdew, Burke, and Ernzerhof are used to calculate the exchange-
correlation energy.27
The brillouin zone (BZ) is sampled with a 10×10×1 Monkhorst-Pack special k-
4. point grid including the Г point. A vacuum region of 10 Å is added to the crystal plane to ensure
that the wave functions vanish smoothly at the edge of the cell as an isolated system that would be
required. The convergence criterion of the self-consistency process is set to 10-8
eV between two
ionic steps to calculate the phonon dispersion. The performed phonon calculations were using the
Phonopy package28
with the forces calculated by the VASP code.
Results and Discussion
After geometryoptimized, the unit cells of the three single-layer SiCs in Fig. 1 maintain
tetragonal form, but some differences among them are also exhibited. The detailedstructural
parameters are given in Table 1. T1 and T2 are still planarstructures, while T3 becomes a buckled
structure with the distance d≈0.48Å. The rectangular rings in T2 are still perfect, while those in T1
and T3 have a little distortion.The bond lengths of Si-C, C-C and Si-Si are also different in the three
structures.
We first discuss the stability of the three 2D SiCs. The cohesive energies of T1, T2 and T3 are
-6.77, -6.54 and -6.47 eV/atom, respectively, which are higher than that of the hexagonal 2D SiC (-
7.03 eV/atom). On the other hand, we calculatethe phonon dispersions of the three structures, as
shown in Figs. 2(a-c). One can find that there is no soft mode in the whole BZ, indicating the
thermodynamic stability of the three structures. Therefore, T1, T2 and T3 are three new metastable
SiC structures.
On the other hand, we calculatethe phonon dispersions of the three structures, as shown
inFigs.2(a-c). One can find that there is no soft mode in the whole BZ, indicating the
thermodynamic stability of the three structures. Therefore, T1, T2 and T3 are three new metastable
SiC structures.
5. Figures 3(a-c) show the band structures and partial density of states (PDOS) of T1, T2 and T3,
respectively.It is found that the three structures exhibit versatile electronic properties from
semiconductor, semimetal to metal. T1 is a direct band-gap semiconductor with a gap 2.26eV [see
Fig. 3(a)]. Boththe valence band maximum (VBM) and conduction bandminimum (CBM) are
located between the K pathsΓ-X or Γ-M.ThePDOSin right panel of Fig.3(a) indicates that the band
edge state around VBM is dominated by pzorbital of C atoms,while that around CBM is dominated
by pzorbital of silicone atoms.To further exhibit the electronic properties of T1, we calculate the
charge densities of the states at VBM and CBM as shown in Fig. 3(d). One can find that the band
edge states are both induced by strong polar covalent bonds. The VBM is related to the polar
covalentbond where electrons mainly distribute around the carbon atoms, while electrons at CBM
mainly distribute around the silicon atoms. The existing of polar double bonds between the four-
membered ringsis the reason why T1 is a semiconductor, like the case of single layer hexagonal
SiC.16, 29
The band structure of T2in Fig.3(b) indicates that it is a semimetal like graphene, in which a
Dirac point appears near the K point X.Our calculation indicates that the Fermi velocity around the
Dirac point is about 105
m/s close to that of graphene.The zero PDOS at the Fermi level further
demonstrate the semimetallic property of T2. Similar to the case of T1, the bonds between the four-
membered ringsare polar double bonds.Electrons around the Fermi level are localized on C atomsor
Si atoms[see Fig. 3(e)]. However, T2 is a semimetal rather than semiconductor because the
rectangular C ring and silicon ring form two sublattices.The polar double bonds are somewhat
similar to the π and π* bonds in the graphene, and thusinduce two crossing bands at the Fermi level,
i.e. forming the Dirac point.
6. T3 is a metal, as seen from Fig. 3(c) where several bands cross the Fermi level. The PDOS
profile shows that the Fermi level and around are dominated by pzorbitals of carbon and silicon. We
present the charge densities of two states at the Fermi level, as shown inFig. 3(f). One can find that
the bonds in T3 are completely different from those in T1 and T2 because of T3's buckling structure.
In the left panel of Fig. 3(f), there are σ bonds between silicon dimers and banana σ bonds between
atoms silicon and carbon. A conducting network formed by these bonds leads to T3's metallic
character. In the right panel of Fig. 3(f), big π bonds are observed between the carbon dimer and
silicon atom, which also forms a conducting work. Additionally, it is noted that in many cases
silicon or carbon dimers will result in metallic characterof SiC structures, such as single layer SiC2
and reconstructed SiC surface.16, 30-32
Due to the versatile electronic properties of the three SiCs, it is interesting to explore the
properties of their nanoribbons. The configurations fornanoribbonsofT1, T2 and T3 are shown in
Fig. 4.Figures 4(a-c) represented the armchair nanoribbonsof T1, T2 and T3, while Figs. 4(d-f)
represented their zigzag nanoribbons, respectively. The danglingbonds atthe edges are saturated
byhydrogen atoms.The relation between the bandgap of these ribbons and their width is shown in
Fig.5(a). The band gaps of T2 armchair nanoribbonsexhibit remarkableoscillating behaviorwiththe
width increasing, while band gaps of T2 zigzag nanoribbons quickly converge to zero.
Theoscillating behavior is similar to the case in the nanoribbons ofplanar C4 carbon sheet.18, 33
The
nanoribbons with zero band gap are Dirac materials, indicating theyinherit the Dirac point from 2D
sheet.For the T3 structure, nearly all nanoribbons are metal because of the metallic properties of 2D
structure.This is similar to the pt-SiC2 and planar T-graphenewhose 2D sheets and nanoribbonsare
metallic.16, 18
Electronic properties of T1 nanoribbons are completely different from those of T2 and T3
nanoribbons [see Fig. 5(a)]. The band gaps of T1 nanoribbons are constant except small changes
7. induced by quantum size effect at very narrow width.Theband gap of zigzag nanoribbonsis about
2.0eVwhile that of the armchair nanoribbonsis about 1.6eV. Figure5(b) displays the band structure
of armchair nanoribbon with width N1a=8. It is found that the valence and conduction bands closest
the Fermi level are all flat bands. The charge densities in the insets of Fig. 5(b) illustrate that the
electrons in the flat conduction bands are mainly localized on the carbon atoms of upper edge, while
those in the flat valence bands are mainly localized on the silicon atoms of bottom edge. This
demonstrates that the two edge states are related to the flat bands, which are different from the edge
states in the graphene whose edge states are related to the Dirac cone.34
For the widernanoribbons,
the interactionsbetween the two edge states disappear, and thus the flat bands do not shift with the
increase of width. The band gaps of nanoribbons are determined by the flat bands, so the band gap
does not change with the width. The same case occurs in the zigzag nanoribbons (see Fig. 5(c)),
however, the band gap of zigzag nanorbibbons is larger than that of armchair nanoribbons because
of theanisotropyof T1.
Conclusion
In summary, we proposed three single-layer tetragonalSiCs (T1, T2 and T3) and studied their
electronic properties by using the density functional theory (DFT) computations.The analysis of
stability indicates that the three structures are meta-stable allotropes of SiC. T1, T2 and T3 have the
same topological geometry, but their electronic properties are very different. T1 is a direct band-gap
semiconductor,T2is a semimetal whose band structure has a Dirac cone, while T3 is a metal.The
versatile properties are originated from the rich bonds between Si and C atoms. The electronic
properties of nanoribbons of the three 2D sheets are also studied. The results indicatedthe existence
of exotic edge states related to the flat bands in the T1 nanoribbons.Electrons in these states only
8. distribute on the silicon or carbon atoms of one edge. The band gaps of the T1 nanoribbons are
constant because there is no coupling between the edge states in the wider nanoribbons.
Acknowledgments
This work was supported by the National Natural Science Foundation of China (Nos. 51176
161, 51376005 and, 11474243).
Table 1 The structural parameters for T1, T2, T3 and hexagonal 2D SiC, respectively.
Figure 1 Atomic structures for (a) T1, (b) T2, (c) T3, top and bottom panelsare top- and side-view
structures. Blue and black ballsrepresent Siand C atoms, respectively.T1 and T2 are planarstructures,
while T3 is a buckled structure with the distance d ≈0.48Å. The angle parameters areα: 85.6°, β:
94.4°, γ: 92.0°, δ: 88.0°.
Figure 2Phonon dispersions of (a) T1, (b) T2 and (c) T3, respectively.
Figure 3Band structure and PDOS(right panel)for (a) T1, (b) T2 and (c) T3. (d) Partial charge
densities for the states at VBM (left panel) and CBM (right panel). (e) Partial charge densities for
the two states at the Dirac point. (f) Partial charge densities for the two states at the Fermi level.
Left panel corresponds to the point 1 in (c), while right panel corresponds to the point 2 in
(c),respectively.
Figure 4 Armchair nanoribbons for (a) T1, (b) T2 and (c) T3. (d), (e) and (f) are zigzag nanoribbons
for T1, T2 and T3, respectively. Blue and black balls represent Si and C atoms, while the red
ballsrepresent the hydrogen atoms. N1a/1z, N2a/2zand N3a/3z are widths of T1, T2 and T3
armchair/zigzag nanoribbons, respectively.
9. Figure 5 (a) Bandgaps of T1,T2 and T3 nanoribbonsas a function of their widths. (b) Band structure
of T1armchairnanoribbon with N1a=8.(c)Band structure of T1zigzagnanoribbon with N1z=8.Inset:
Partial charge densities for the states in the flat bands.
Table 1
15. 1. A. K. Geim and K. S. Novoselov, Nature Mater, 2007, 6, 183-191.
2. C. e. N. e. R. Rao, A. e. K. Sood, K. e. S. Subrahmanyam and A. Govindaraj,
Angew Chem Int Ed, 2009, 48, 7752-7777.
3. S. Z. Butler, S. M. Hollen, L. Cao, Y. Cui, J. A. Gupta, H. R. Gutiérrez, T. F.
Heinz, S. S. Hong, J. Huang, A. F. Ismach, E. Johnston-Halperin, M. Kuno, V. V. Plashnitsa,
R. D. Robinson, R. S. Ruoff, S. Salahuddin, J. Shan, L. Shi, M. G. Spencer, M. Terrones, W.
Windl and J. E. Goldberger, ACS Nano, 2013, 7, 2898-2926.
4. A. N. Enyashin and A. L. Ivanovskii, Phys Status Solidi B, 2011, 248, 1879-
1883.
5. A. Kara, H. Enriquez, A. P. Seitsonen, L. Lew Yan Voon, S. b. Vizzini, B.
Aufray and H. Oughaddou, Surf Sci Rep, 2012, 67, 1-18.
6. H. Liu, J. Gao and J. Zhao, J Phys Chem C, 2013, 117, 10353-10359.
7. R. S. Sundaram, M. Engel, A. Lombardo, R. Krupke, A. C. Ferrari, P.
Avouris and M. Steiner, Nano Lett, 2013, 13, 1416-1421.
8. R. Ganatra and Q. Zhang, ACS Nano, 2014, 8, 4074-4099.
9. Y. Li and Z. Chen, J Phys Chem C, 2013, 118, 1148-1154.
10. E. Bianco, S. Butler, S. Jiang, O. D. Restrepo, W. Windl and J. E. Goldberger,
ACS Nano, 2013, 7, 4414-4421.
11. C. J. Tabert and E. J. Nicol, Phys Rev Lett, 2013, 110, 197402.
12. D. Y. Qiu, F. H. da Jornada and S. G. Louie, Phys Rev Lett, 2013, 111,
216805.
13. S. Lin, J Phys Chem C, 2012, 116, 3951-3955.
14. X. Lin, S. Lin, Y. Xu, A. A. Hakro, T. Hasan, B. Zhang, B. Yu, J. Luo, E. Li
and H. Chen, J Mater Chem C, 2013, 1, 2131-2135.
15. L. Zhou, Y. Zhang and L. Wu, Nano Lett, 2013, 13, 5431-5436.
16. Y. Li, F. Li, Z. Zhou and Z. Chen, J Am Chem Soc, 2010, 133, 900-908.
17. Y. Ding and Y. Wang, J Phys Chem C, 2014, 118, 4509-4515.
18. Y. Liu, G. Wang, Q. Huang, L. Guo and X. Chen, Phys Rev Lett, 2012, 108,
225505.
19. W. Li, M. Guo, G. Zhang and Y. Zhang, Phys Rev B, 2014, 89, 205402.
20. M. Y. Zhang, C. Wesdemiotis, M. Marchetti, P. O. Danis, J. C. Ray Jr, B. K.
Carpenter and F. W. McLafferty, J Am Chem Soc, 1989, 111, 8341-8346.
21. Y. Chen, Y. Sun, H. Wang, D. West, Y. Xie, J. Zhong, V. Meunier, M. L.
Cohen and S. Zhang, Phys Rev Lett, 2014, 113, 085501.
22. J. Presilla‐Márquez, S. Gay, C. Rittby and W. Graham, J Chem Phys, 1995,
102, 6354-6361.
23. C. C. Arnold and D. M. Neumark, J Chem Phys, 1993, 99, 3353-3362.
24. S. Kim, S. Wang and H. F. Schaefer III, J Phys Chem A, 2011, 115, 5478-
5487.
25. G. Kresse and J. Furthmüller, Phys Rev B, 1996, 54, 11169.
26. P. E. Blöchl, Phys Rev B, 1994, 50, 17953.
27. J. P. Perdew, K. Burke and M. Ernzerhof, Phys Rev Lett, 1996, 77, 3865.
28. A. Togo, F. Oba and I. Tanaka, Phys Rev B, 2008, 78, 134106.
29. E. Bekaroglu, M. Topsakal, S. Cahangirov and S. Ciraci, Phys Rev B, 2010,
81, 075433.
16. 30. M. Sabisch, P. Krüger, A. Mazur, M. Rohlfing and J. Pollmann, Phys Rev B,
1996, 53, 13121.
31. V. Y. Aristov, L. Douillard, O. Fauchoux and P. Soukiassian, Phys Rev Lett,
1997, 79, 3700.
32. L. Gavioli, M. G. Betti and C. Mariani, Phys Rev Lett, 1996, 77, 3869.
33. X. Wang, H. Li and J. Wang, Phys Chem Chem Phys, 2012, 14, 11107-11111.
34. T. Wassmann, A. P. Seitsonen, A. M. Saitta, M. Lazzeri and F. Mauri, Phys
Rev Lett, 2008, 101, 096402.