Química Sebenta Bonitinha

[Audio] Mariana . . . Mendonça How are you? Q What's up? O_O Wow :-O : :O g o 000 ☒ @ Hydrogen atoms * Hydrogen atoms are composed of only one electron that orbits around the nucleus. Orbital the area in space around the nucleus where there is a high probability of finding an electron =D As a consequence of the orbital depending on three independent variables, one for each spatial coordinate, there are 3 quantum numbers , in harmony with what was found when solving the problem of free refractory in a one dimensional potential well, where only one Α quantum appeared. Quantum Numbers : N principal quantum number n = 1, 2, 3, ... . . . (positive integers) ↳ characterizes the size of the orbital l Secondary or Azimuthal Quantum Number . . . . 1=0 . . n 1 and the µ 2dg 4g (a symbol for the symbol atomic mass unit).

[Audio] I am Magnetic quantum number. . . _ l , , . , 0 mp plus f ¥ characterizes the orientation in space of the orbital. ⇒ The set of orbitals with the same value of n constitutes a layer, of the same energy level, and is designated for hydrogen atoms as . It is also commonly said that they are degenerated. =D Within a layer, the orbitals with the same l value constitute a sublayer (sublevel). 21 plus 1 Number of orbitals in each sublevel (number of allowed values for mp) in Number of orbitals in each level equals number of orbitals per n p 4 9 f O 0 1 O 1 2 7.mn#I-fi o In the atom's space..

[Audio] Graphical representations of orbitals → s orbitals have spherical symmetry ^ probability ps 2 s n.AE! . =L The as orbital is zero if for r _ r, which corresponds to a surface where the probability of finding the electron is zero (nodal surface) . In the case of s orbitals à of surfaces . Generally, for an orbital ln.lt, the number of nodal surfaces is given by n-1 and the number of nodal surfaces is given by n 11H (surface of Isoprobability) → Indicates the relative probability of finding an electron at a certain distance from the nucleus =D The energy for hydrogen atoms is solely dependent on the principal quantum number, nl, which means that all orbitals of a given level are degenerate) c = -¥. ai ÷ × It 4 aitogenes.

[Audio] Magnetic Spin Quantum Number = ± 1 The quantum number ms characterizes the ms spin 2 rotation of the electron around an axis that passes through its center of observation. An orbital is characterized by a set of quantum numbers (n, me), l An electron is characterized by a set of quantum numbers (n, l, Ms) for polyhedral atoms → The constituent electrons of atoms exert repulsive forces among themselves, and are attracted by the nucleus . Thus, the potential Vlsçy ,a) of the Schrödinger equation contains , losing spherical symmetry due to inter tunicle repulsion forces, making it impossible to obtain an analytical solution of the equation . of Schrödinger. In polyatomic atoms , the energy takes on different values for a given n value, depending on the value of the azimuthal quantum number l , although very slightly , . The energy depends on the magnetic quantum number , me , and the spin magnetic number , Ms . ⇒ ::*::*::: 'radial of the Na ion ÷:* IA . ÷; Ionization potential of a sodium atom.

[Audio] The maximum internal states correspond to the electronic filling of the n quantum principal levels 1 and 2. The 3s orbitals belong to the 3rd level which is still to be filled. The 3s orbitals are more penetrating than the 3p orbitals, because an electron in a 3rd level has a greater probability of being found closer to the nucleus, experiencing a stronger attraction from the nuclear charges. Electronic filling: The total energy of an atom is equal to the sum of the energies of its constituent electrons. The 5s and 7s orbitals follow the Wismesser empirical rule. The 3rd and 2nd level orbitals with lower energy are those with a lower value of the sum of the n quantum numbers, and for equal values of (n plus l), the orbitals with a lower n have lower energy. Pauli's Exclusion Principle states that in a poly electronic atom, no two electrons can have the same set of quantum numbers. (The maximum number of electrons per orbital is 2)..

[Audio] Construction principle of Autbau (Principle of minimum energy) ↳ arrangement of orbitals in increasing order ↳ electronic filling of orbitals one by one in the order according to the increasing principle of energies found in 11 of Pauli's exclusion , until all electrons are distributed by orbitals Í Hunt's rule: When electrons are distributed equally, they tend to occupy the orbitals that do not yet contain electrons. When multiple equivalent orbitals are present and a single atom is occupied by a single electron, the spin angular moments align in order to have the same direction and sense 1 electron 3 4 electrons 1%1 1 2 behind 1 1 5 electrons 11111 3 electrons 11 1 6 electrons 111111 Note: Electrons with arrows pointing in the same direction are said to have parallel spins. Electrons with arrows pointing in opposite directions are said to have anti parallel spins..

[Audio] Mariana Mendonça Pb . Properties ↳ Periodic Table The electron configurations of the last layer correspond to similar chemical properties. Group 1 Group 18 Period 9 elements c ✓ representative s d p Period 7 / f → elements of inner transition elements Energy → The energy required to remove an electron from an atom or ion ✗, (free from interactions) and fundamental / electrons occupying in their gaseous state if ionization energy . the lower energy orbitals), designates plus plus and plus E; → ✗ ✗ (g) (g).

[Audio] Shielding Effect =D The atomic number Z is reduced by the number of protons whose attraction is shielded by the remaining electrons of the atom. Representing this as S (called shielding coefficient), the effective atomic number will be given by Z-Eff = Z S.

[Audio] Examples: µ Co : dealing dpb 3 i3 p ' there 3 d' 4 po 11 sa) ( ai 2pA 13 i3po ) 13N ) there is hpo) 2 = 23.1 _ ? S = 1 10 0.35 plus 0.85 x 15 plus 10 x 1.0 , lo) and f (4 s = 27 23.1 = 3.9 Zef , Co) = ? s = 6 x 0.35 plus 18 x 1.0 2 µ ( 3d s = 27 6.9 ↳ Note: The p orbitals are more penetrating than the d or f orbitals, which means that electrons in s and p orbitals experience less shielding from the immediately interior electrons. Ionization Energy , * Energy required to remove an electron from an atom or ion in its perfect gaseous state (free from interactions) and its ground state (electrons occupying the lower energy orbitals), plus Ei → Xtcgl plus 1 e Xlgl =D Difference between the energy of the stationary electron (conventionally set to zero) and the energy of the electron in the orbital under the influence of the nucleus..

[Audio] The effective atomic ionization energy depends on the following factors: En, which is the principal quantum number..

[Audio] → Occupancy degree of the orbital is mutually ↳ Electrons sharing the same orbital repel each other, the E ; is lower than in the case of isolated electrons. Example, if I have 2 electrons in the same orbital, they will repel each other, so the energy of the orbital (E ;) will be lower than the energy of two isolated electrons. → Inversion of trend Note: The E ; of higher order are always greater than those of lower order, since there are fewer electrons causing less interelectronic repulsion. Therefore, the electrons are more attached to the nuclei. Electronegativity or electroaffinity → Electroaffinity is the energy released in the formation of one mole of negative ions from one mole of neutral atoms in the gas state and in their ground state. × Plus, 1 is → 11 E a → Represents the difference between the electro free energy (rest) filled and the energy of that electron in the unoccupied or semi orbital of lower energy of the negative ion. Electronegativity (ei) is of order zero..

[Audio] Electronegativity (10) → The tendency of an atom in a molecule to attract electrons towards itself in a bond ↳ plays an important role in the establishment of chemical bonds → Cannot be measured experimentally → Is mainly measured by: the ability of an atom to hold onto its eletron (law of the conservation of eletron) the tendency to capture the electron from another atom (Ea) Electronegativity according to Mulfikem D= (Ei plus Ca) 12 Variation of Electronegativity = Increases along the period > from left to right = Decreases along the group > from top to bottom Note: The ionic radius is proportional to the Iei.

[Audio] Molecules and So . & : ← Coordination Compounds Chemical Bonding When two non metals bond with each other , neither of them wants to lose their electron so they have to share them ↳ Covalent Bond → When a metal and a non metal bond, the metal will easily give up electrons with lower energy ( smaller E:) ⇒ transfer from the metal to the non metal ↳ Ionic Bond = P When we have multiple metal atoms, each one will easily give away its valence electrons and attract the electrons from neighboring atoms ⇒ free electrons , shared by all elements of the atom groups ↳ Metallic Bond Mariana Mendonça.

[Audio] Difference between the energy of the Energy of Binding Set of Species in the state of lowest potential energy (when they are bound) and the same set at infinite distance (not bound) bond length distance between the centers of the bound species when they have a minimum potential energy Ep equilibrium distance µ Bon Approximation of Unified Description of Chemistry Oppenheimer repulsion in fixed nuclei position, attraction at equilibrium (mechanical energy in nucleus) ¥ t A H H B / Now, we can solve the Schrödinger equation for the case of AB monoelectronic system and adapt it for polyelectronic systems..

[Audio] Molecular Orbital Theory (M-O-T--) Linear Combination of Atomic Orbitals Method (L-C-A-O-) Assumptions → Nuclei are located at equilibrium internuclear distances (Born Oppenheimer approximation) =D Molecular orbitals are linear combinations of all atomic orbitals from all atoms. → Electrons are distributed among the molecular orbitals according to the principles of Minimum Energy and Pauli Exclusion, with the simplification criteria that there is only simultaneous contribution. =D Criterion of Energy Similarity of two or more atomic orbitals; if their energies are similar, there is only simultaneous contribution from two orbitals. → Criterion of Atomic Coalescence; if their coalescence is non zero, their signs are the same. ^ ✓ Sinusoidal.

[Audio] Molecular orbital shapes Ligand molecular orbital whose electrons have a bonding effect, that is, they are located in the internuclear region, causing the nuclei to approach → The energy of the bonding molecular orbitals is always lower than the energies of the atomic orbitals. Molecular orbitals whose electrons are in Anti bonding molecular orbital, located outside the internuclear zone, causing the anti bonding effect, resulting in the nuclei moving farther apart. =D The energy of the anti bonding molecular orbitals is always higher than the energies of the atomic orbitals. Distonia internuclear Equilibrium ^A The anti bonding diagram..

[Audio] and for Diagmatism Magnetism increased great mass Paramagnetism.

[Audio] Examples: ① OM energy diagram for H and O# . . . -ÇIHI . g-: ' Its ', qs is ' 11 is Eiltbf H Ha H OL = 1 Ha: q Diamagnetic ② OM energy diagram for He and O# .÷ . . . ' ' . t: -ÇIHI ' # ' 1s ,qs is ' M-→ Eiltbf He Hez He 01 = 0 Hea: A gigaanion would have higher energy than separate He atoms, making them unstable..

[Audio] ③ Energy diagram of OM for HeI and O o# -ÇIHI. t: 1:-p ls . ' qs is ls i ' µ -→ Eilttf There Is Hezt Hj a f HeI : aiai Paramagnetic Diatomic Molecules 2nd period ÍrnE/t.i iiniii.io#-0002p The Tops , Top of / \ \ / Gapn .-0*1 . 62A l , -0 : . ' -0 . '' 21 , gzs , '' 21 \O/ #* O ÷ :-O ' i 1A ls..

[Audio] Example: Fluorine molecule , F : ls' There dps E -10-1--1 , -9in Oh d i iiiwi.ir ; Diamagnetic . LP , Ü as iiapy , Cover LP '→i Magnetization : 10 , 62¥ , 10: ' 21 , Ozs r 21 ( \# ✓À ' 10: :X There are 'i.fr Oxygen molecule , O : Has dps c^ -9: i iiim.ir: OE 10-6--2 . LP , 1¥ . Has iiapy , Fdp , LP 2 :X Magnetization : 10 , Paramagnetic . 62¥ , *: ' 21 , Ozs r 21 \# ' ¥: Has info.

[Audio] Energy variation of Ls and Xp orbitals along the 2nd period of the TP Energy → Effective nuclear charge % o. . o _. o... o? N increases along the 30.00\↳ period as 2 'o fde 5 'n -6 life b d greater stabilization of the mixtures of p orbitals , more penetrating than the Ls orbitals There is a mixture of p orbitals up to Na Example: OM energy diagram for La # ç _p i.: f (l) q p _Í , Take out i q q _ | e 03 jr.it ar ; ar ' 1111 i i E:(G) I µ Ãdpy , a 'Í 'n i.I , | , 111 , i # . i . . Y ' ai q % . % La \ 1 Ls ! µ -1. % Diamagnetic.

[Audio] Influence of K on the P Resonance Integral Energy dt oaaaa.9.NAME p Resonance Integral Electronegativity Heteronuclear Diatomic Molecules = D Considered A and B as two different atoms, and, for simplicity, characterized by energies of only one orbital from each one of them E and EB, such that E-A-C-E, the electronic orbital molecular behavior will be similar to what it would be in the atom, while in the anti bonding orbital, it will have a similar behavior to the isoprobability surfaces in atom B..

[Audio] Molecules of HF are formed by a leu)n of C and Eiltt) atoms, with ls, ds, dpy, and dpz orbitals. The atom of fluorine is at 17.4, and the 2ps orbitals are virtually non existent in IF. The identical orbitals of the fluorine have a negligible amount of IF. If the atom in orbit is not a diamagnetic, it is a nonbonding. The percentage of ionic character is between 3.10-0.9. Examples of this can be seen in compounds like Nact where the difference in electronegativity is 3¥17, resulting in a percentage of 70% C 1. In O£-0 molecules, the difference in electronegativity is 3.04-3.44, resulting in a percentage of 4%. This leads to consequences in the asymmetry of the electron cloud..

[Audio] Dipole moment , µ in ° is equal to the product of the electron charge (e) and the distance (d) between the two charged particles. Example: Hf Tp Xih = 2.20 kkk z.gg m = 0.092 × 10^-10 D-H-F = 1.79 i %C. I = 55% c TP 510 M %fE-xexdui.es 10 0.092 × 10^-4 < ⇒ µ 0.55 × 1.6×10^-19 C. m (coulomb. meter) a ⇒ M 8096×10^ -7 ( ⇒ µ , = 2.4 D (Debye) Relationship between electronegativity (x) and percentage ionic character C-C-I-) % 101 Kali Kali 3.5 I-K-B _ 16 9..

[Audio] Relationship between electronegativity and bonding energy → The higher the electronegativity of the element, the stronger the attraction and therefore, the higher the bonding energy → The greater the difference in electronegativity, the greater the difference in energies between the orbitals involved in bonding (the higher the p) and therefore, the stronger the tendency for molecule formation. Valence bond = D The valence bond describes the formation of a bond between two atoms as the combination of two half filled atomic orbitals from each atom in the valence shell..

[Audio] Concept of Hybrid Atomic Orbital =D A hybrid orbital is a mathematical linear combination of two atomic orbitals, resulting in a wave function. In this aspect, it is similar to a molecular orbital, but with a significant difference. While the atomic orbitals contributing to the formation of a MO belong to different atoms, the different orbitals contributing to the formation of a hybrid orbital belong to the same atom and have the same geometric center. =D Hybridization involves a redistribution of electron density around the nucleus, as if the isolated atom anticipates its future bonding state and prepares its meteoric cloud accordingly. The maximum number of atomic orbitals can combine to form a hybrid atomic orbital, and the angle formed between the hybridized orbitals depends on their geometric centers. ① Angles formed between hybrid orbitals can create a linear orbital with µ = 180 degrees. 2 A linear orbital with µ = 120 degrees can be formed with 2 quoi q ↳µ ③ An orbital s with µ = 109027 degrees can be formed with 3 spi orbitals. ④ An orbital s with µ = 1090.27 degrees can be formed with 4 lsxssp orbitals. ⑤ An orbital s with µ = 109027 degrees can be formed with 5 lsxssp orbitals..

[Audio] Energy of Notable Hybrid Orbitals ^ ↳ Hybrid orbitals possess a remarkable energy level ^ ↳ . . . . ÷ It is found that an electron has higher energy when occupying a hybridized s orbital (with 1, 2, or 3) than when occupying a pure s orbital, but lower energy than when occupying a p orbital. The cost of hybridization is a function of the atom's electronic structure specifically, the number of electrons. The greater the number of electrons, the smaller the difference will be between the energy of a hybridized and non hybridized atom. This is due to the difference in energy levels between the orbitals..

[Audio] Geometry of hybrid orbitals number of orbitals Geometry of combined type of hybrid orbitals hybridization s Bipiramidetrigonal sp3d 6 Octahedral sp3d ::*::/ : 2 Linear sp :/ Relevant hybridization mode method for predicting the type of hybridization: → The geometry around the central atom is dependent on: the number of bonded neighboring atoms (number of partially filled orbitals) the number of paired electrons..

[Audio] ① Beta Be: 1st idã Hits electronic configuration in hybridized state of Be Be: ls' Lsp Lsp pjpi hybridization ⇒ Linear geometry 11809 There are two bonds between the beryllium orbital (sp) 1¥ µ and the first orbital of hydrogen ② B-H-Z H: ls B: hybridized electronic configuration of B Lsp; pi B: hybridized sp; asp hybridization ⇒ Triangular planar geometry 11207 There are three bonds between the orbitals of Boron and the 1st orbital of H ④B-H atoms µ tt spa . µ H atoms.

[Audio] ③ C-H-4 'c: The electronic configuration in the hybridized state of C (itidspj 2spjdspjdsp.cl ligand electrons) 'hibridation sps ⇒ Tetrahedral Geometry (109.027 degrees) A-H-I This molecule is polar. ④ NH Nitidiapinapjdpi H electronic configuration in the hybridized state of C : tidsp; Lsp; Lsp; Lsp; paired isolated ligand pairs → µ # O → nonpolar molecule H-A-O Oitidiapiapjdpi H electronic configuration in the hybridized state of C (itidsp; Lsp; Lsp; Lsp; paired isolated ligand pairs) → µ # O → nonpolar molecule..

[Audio] NotA: Central Atom = number of partially filled orbitals, number of ligations plus number of non bonding pairs and disadvantages of hybridization for atoms of the 2nd period advantages: 1N , O , (F) → hybridization allows minimization of electronic repulsions between bonding and non bonding pairs 2 Be , B C → In these elements, it allows an increase in bonding capacity 3 An asymmetric hybrid orbital allows for greater overlap through the larger lobe compared to any pure orbital..

[Audio] Disadvantage 1 The hybrid electronic configuration is more energetic than the non hybridized configuration for the previously indicated atoms. However, as the atoms become hybridized, there is a overall decrease in energy due to a higher number of bonds and a reduction of electron repulsions. Functional Groups =D Alcohol ( C 0H ) ( 0H ) =D Carboxylic acid ( CÍOH ) l cooh ) =D Aldehyde ( c H ) → Ketone ( c = o ) Hydrocarbons =D Aliphatic Hydrocarbons C Hz) students ( ex , ethane CH, = C-H-A ) students ( ex . propane C-H-A students ( ex . ether HC = CH ) HA Aromatic Hydrocarbons Benzene Aromatic hydrocarbon skaters.

[Audio] Students Ex. H , H H Y Y Y H C H H Is is H H C C C H l t H H ¥ ¥ f, methane ethane propane x H H H I | c c Propane [ Methane HÍ ! H Is → ia HH ' I H d-Ê ethane HIÉ ? Is Butane µ ÊI } µ;t t, # Hybridization 5 ' angles 11090.27 and O µ nonpolar molecules Students H H H H H H P H c c c c c c 11 ] Wow, amazing!!!.

[Audio] Students H H H C H R H C C C H C C H H C C Ç . Brogue C-tine} Self Hybridization sp hybridization, ' ) 11809 11090.27 Covalent Crystals → This type of chemical bond between atoms with high bonding capacity (C, Si, Ge) allows for three dimensional aggregates with such a large number of atoms that the overall structure acquires macroscopic dimensions. Diamond Graphite ^ * a 30M bands o # (sp) 4 N E is and o * lspa) 3 N # 40 M Í . Í | , and , 2 N 2ps ! Ã _ ' , 1 1 11 Í q q _ q . ' i : I % Ã 2 N µ ! t 40 M ! 111 i , ! ! spz ; (i) Glsps) 4 N o dsqf ! ! , 30 M C Clspz) CC ÇI Mcconn i 111111 olspz) 3 N o c aspaz) cccz) Icksdin.

[Audio] Mariana ÷:&:* Mendonça ÷⇐¥Ç , €, *¥ ü¥¥ ÷÷É . Intermolecular Interactions = Van der Waals bonds (permanent dipole) Keesom Interactions (permanent dipole induced dipole) Debye Interactions (permanent dipole) London Interactions (instantaneous dipole induced dipole) = Hydrogen bonds Keesom Interactions → The efficiency of the interaction depends on: Permanent dipole VS. Relative orientation of permanent dipoles Distance → depends on the dipole moments (increasing these by 4) and = ÷ ÷ çiçir \ depends on the sixth power of the distance between the centers of the dipoles =E The boiling temperature increases with the dipole moment in small molecules. This demonstrates the significant contribution of Keesom interactions to the strength of intermolecular interactions in small molecules..

[Audio] Debye interactions: permanent dipole vs induced dipole London interactions I and 2 ionization powers EL = 2¥77 TI of each of the atoms a and q → polarizability → The magnitude of the induced dipole depends on various factors: Electron polarizability Volume of the electron cloud Higher molar mass → Higher number of electrons = larger electron cloud → Higher polarizability → stronger interactions. Molecule shape Larger surface area → Larger induced dipole → stronger interactions..

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[Audio] Hydrogen Bonding Connections H N H N O N f H N N H O O H O F H O N H F F H F H F O → The hydrogen bond is formed by 3 atoms → Hydrogen bonding also occurs between chlorine and sulfur atoms, but they are much weaker. Examples ⑨ H ② O H O ③ Hydrogen bonds are also formed between other atoms, such as carbon and nitrogen, in compounds like CH, O H O ④ This is due to the attraction between positively charged hydrogen and negatively charged molecules. ⑤ These bonds are responsible for many important properties of molecular compounds, such as high melting and boiling points. ⑥ Other properties include miscibility, which is the ability to mix with other substances, and viscosity, which is the thickness or resistance to flow..

[Audio] Viscosity → Viscosity should be proportional to the strength of intermolecular interactions =D It also depends on the shape and molecular conformations: lower for more spherical molecules if very long molecules can entangle viscosity resistance of a liquid to flow → Stronger intermolecular forces ⇒ higher viscosity → higher temperature ⇒ lower viscosity surface tension =P Surface tension is the energy per unit area =D Translates into a force parallel to the surface, although it is due to a force that acts on each molecule perpendicular to the surface..

[Audio] Polymers Mariana Mendonça Polymers =D Polymers: composed of small repetitive units (MONOMERs) Monomers or Meros Enzymatic Reaction.

[Audio] Polymerization reactions = p Addition reactions Initiation → activation of the monomer → chain growth Propagation Termination → completion of the polymerization reaction → The monomers that undergo this type of reaction first need to be activated in order to react with each other. The reactive species can be: a radical (radical reaction), a cation (cationic reaction), or an anion (anionic reaction). D Condensation reactions = Denominated condensation polymerization when the addition reaction is based on the use of catalysts. The break of double bonds results in a sequential bonding of vinyl polymers and the resulting polymers are called This occurs when the monomers have functional groups, therefore an initiator is not necessary. The reactivity of the monomers is equal to the reactivity of the growing polymers. During the polymerization reaction, water is eliminated. For the reaction to lead to a polymer, both monomers must be bifunctional, meaning they have 2 functional groups..

[Audio] Ring opening polymerization Ring opening polymerization occurs when the addition reaction involves the splitting of rings to form a linear polymer. Intermolecular interactions in tangles of rubber or elastomers result in a termoset with indeformable covalent bonds. When melted, the polymer will not fuse but will degrade. In contrast, a thermoplastic with single crosslinks will melt at a certain temperature. In the solid state, the polymer can be amorphous, with a glass transition temperature (Tg). In the melted state, molecular movement allows for mass transfer. It is difficult to determine the freezing point (Tf) of a polymer. The glass transition temperature (Tg) is used to describe the transition between the solid and liquid state of an amorphous polymer..

[Audio] Factors that determine TV =D Chain flexibility 1 Rigid ⇒ 1 TV chains → Presence of side groups entanglement causing loss of mobility → Intermolecular forces → Tacticity except for polyvinyl alcohol, atactic polymers are amorphous Average molecular weights ^ Mn Mw 3.ral at t % weight per molecular Index of polydispersity : Measure of heterogeneity of molecular size Factors that affect molecular weight after polymerization From the presence of reactive impurities =D Chemical action ⇒ Ultraviolet radiation From Enzymes =D Ultra sound → Bacterial agents =D Mechanical stress.

[Audio] Crystalline polymers exhibit: greater mechanical strength greater opacity greater resistance to solvents greater density when undergoing plastic deformation, which is achieved when the stress is no longer proportional to the deformation, resulting in irreversible and permanent deformation → From an atomic perspective, plastic deformation corresponds to the breaking of bonds with the original neighboring atoms and the formation of new bonds with new neighboring atoms, as a large number of atoms or molecules move in relation to each other. =D After the stress is removed, they do not return to their original positions, unlike in elastic deformation. low ductility Fracture ÷ , brittle ⑥ > Elastic plastic rupture.

[Audio] Polymer Properties and Structure Thermoplastic Fibers Thermosetting Elastomers ✓ 5 v v Crystalline Crystalline Amorphous Amorphous Crystalline Amorphous Semi.

[Audio] .am#*--EE-j EEsaas Mariana %EE.%dE.EE#*.EEWamg:←Ea*→ . jqqi.ee#:mwwTTE.gg#&sqETTLIn Mendonça %EE.%EE.ME#*..GHBaqa;jogEMEEEE E ax a.az. -1€ ⇐ *.ae#i::-%eEYoI # f⇒⇒ , www.?HEwEEZ**jE**Ümy www.T.wwj#Ee**......*HY →A ⇒⇒* .EE#Ii:**E---yf-:----f ⇒HÁ t.IT#!*.E--------E***------------I ggq.fr?.W.TT*k!Ek.Ia ! vimeo.ia.TT?aET* .EE#*.=GgpgfEIE étienne Belágua .EE#GB$.&ijpFgib! IR Elements → Metals are materials with common characteristic properties: high density high malleability and ductility high thermal and electrical conductivity =B. These elements are characterized by low ionization energies and . low electro negativities , meaning low electron affinity. Crystal Structures of Metals . → Structures described as rigid rod packing → Structures defined as different ways of filling interstitial spaces: spaces between spheres =L The most common structures are: Face centered cubic ( F-C-C-) Hexagonal close packed ( H-C-P-) Body centered cubic ( B-C-C-) Simple cubic ( SC).

[Audio] Simple Cubic C-C-S-) ° µ: The simple cubic structure is made up of eight atoms positioned at the corners of a cube, with one atom at each vertex. The distance between adjacent atoms is equal to the edge length of the cube. The structure is also known as face centered cubic (C-C-C-), as there is one atom in the center of each face of the cube. The number of atoms in this structure is equal to one times the number of vertices, which is eight. The diagonal of the cube is four times the edge length, making the structure more compact..

[Audio] Face Centered Cubic (F-C-C--) has 8 atoms per vertex and 6 atoms per face. Total number of atoms = 16 per unit cell plus 18 face atoms. Hexagonal close packed (H-C-P--) has 6 atoms per unit cell..

[Audio] Types of Interstices → Tetrahedron → empty space inside 4 atoms = D Octahedron → empty space inside 6 atoms Number of Interstices Type of octahedral tetrahedral Structure C-F-C 4 6 12 Referring to µ..} @ A Ccc | Note: The number of Tetrahedral Interstices in a compact structure is equal to twice the number of atoms that make it up. The number of Octahedral Interstices in a compact structure is equal to the number of atoms that make it up..

[Audio] C-L-O-A for metals Application of T-O-M Band Theory (of energy) → Metallic bonding of low electronegativity atoms C^ ¥ Eu , #x p ' . í x i f.dk! . . i Ey = xt B Y Coulomb integral A AL A . Resonance integral p = Low electronegativity ⇒ Low value of p → Formation of macroscopic clusters → Displacement of reaction → Band formation.