We think you have liked this presentation. If you wish to download it, please recommend it to your friends in any social system. Share buttons are a little bit lower. Thank you!
Presentation is loading. Please wait.
Published byTravon Benet
Modified over 2 years ago
Atomaire bindingen - ionische binding - covalente binding - metallische binding
Ionic bonding 1 E between a Li atom and a F atom
Ionic bonding 2 E gives Li + F - molecule Ionization Potential (IP) Electron Affinity (EA) Energy cost: E = IP(Li) – EA(F)
Ionic bonding 3 Ionic binding curve: electron transfer Coulomb attraction ions Pauli repulsion Binding curve has stable minimum !!
Ionic bonding 4 only works between very dissimilar atoms !!
Ionic bonding in solids NaCl structureCsCl structure Na + Cl - Cs + common salts have ionic bonding structure determined by relative size ions
Covalent bonding 1 Model system: one electron in two wells wells far apart wells close ES < EAES < EA electron wants to pull wells close !!
Covalent bonding 2 H 2 molecule: two electrons in two wells E H atom H 2 molecule allowed by Pauli
Covalent bonding 3 He 2 molecule? four electrons E He atom He 2 molecule no electronic bonding in He 2 no stable He 2 molecule !! because of Pauli exclusion principle
Hetero-atomic covalent bonding E H F molecule polar bond !! H atomF atom
Poly-atomic covalent bonding 1 H 2 O molecule 2 2 covalent bonding gives directional bonds !!
Poly-atomic covalent bonding 2 CH 4 molecule: tetraeder C hybrid orbital
Covalent bonding in solids C, Si,... have covalent bonding diamond structure and compound semiconductors: GaAs,...
Metallic bonding in solids 1 positive ions metal: one electron in many wells has a wave-like character (delocalized)
Twee verschillende metalen met elkaar in contact contact-potentiaal
Volgende (laatste) hoor-college: Quantum theorie van electrische geleiding Isolatoren vs. (half)geleiders, supergeleiders Terugblik op de gehele stof
6-5 Molecular Geometry. VSEPR Theory VSEPR theory – states that repulsion between the sets of valence-level electrons surrounding an atom causes these.
Properties of Bonds 1.Polarity 2.Bond Order 3.Bond Length 4.Bond Energy.
IGCSE. Why do atoms bond? What is an ionic bond?
Atoms and Bonding Chapter 6.1 cont.... Compounds and Bonding A compound is a substance that is composed of atoms of two or more different elements that.
Chapter 6: Chemical Bonds When the highest occupied energy level of an atom is filled with e, the atom is stable and not likely to react. In other words,
Ions & Electrons Quiz QUESTION ONE Which one of these is an ion? A Na B Na + C Cl 2 DH2ODH2O.
Ch. 13: Bonding Formation of Binary Ionic Compound.
Molecular bonding. Molecular Bonding and Spectra The Coulomb force is the only one to bind atoms. The combination of attractive and repulsive forces creates.
1 STM surface image of gold. 2 Using atoms as a footprint of chemistry: Energy of incoming radiation = Energy of photo electron + Energy difference K-L.
Chemistry Unit 4 Bonding Why do atoms bond? -to become more stable -a full valence shell of electrons -valence shell = outside shell How do atoms bond?
Do Now Describe the difference between an ionic bond and a covalent bond.
Chemical Bonds and Molecular Geometry. Electrons Valence electrons Those electrons that are important in chemical bonding. For main-group elements,
Electron Configurations. Quantum Theory Electrons are found in orbitals Defined by quantum numbers n, l and m. Like seats in a theatre organized in section,
Unit 10: Chemical Bonding Section 1: Ionic and Covalent Bonding.
Properties of Ionic and Covalent Compounds. Ionic Compounds Representative Unit: Formula Unit Bond Formation: Transfer of one or more electrons between.
ELECTRON AND PHONON TRANSPORT The Hall Effect General Classification of Solids Crystal Structures Electron band Structures Phonon Dispersion and Scattering.
Periodic Trends. Describe factors that affect electron position around a nucleus. Include: nuclear charge, distance, shielding. Explain periodic trends.
Why do atoms form bonds? To attain a noble gas configuration. How do atoms form bonds? By gaining, losing, or sharing electrons. Gain or loss of electrons.
Solids AMORPHOUS- THOSE WITH MUCH DISORDER IN THEIR STRUCTURE. CRYSTALLINE- HAVE A REGULAR ARRANGEMENT OF COMPONENTS IN THEIR STRUCTURE.
Ionic Bonding & Covalent Bonding. Ionic Bonding Ionic Bonding – TRANSFER of electrons Metals + Nonmetals = Ionic Bond.
BONDING. CONDUCTIVITY The ability of a substance to conduct electricity SOLUBILITY The ability of a substance to dissolve in a liquid (mostly water) Lab.
Chemical Bonding Chap. 6 What is a bond? a strong attractive force that exists between the e - of certain atoms. 1.
NOTES Ionic vs. Molecular Compounds. AKA Salts Formula units Molecular compounds Molecules IONIC / IONIC COVALENT / MOLECULAR.
Covalent Bonding What is a covalent bond?. Covalent Bonding What is a covalent bond? How is a covalent bond different from an ionic bond?
Lecture 2711/07/05. Ionic bond Ionic compounds Valence electrons are transferred from one atom to another Metal + non-metal NaCl Bonding.
Polarizability More electrons are further from the nucleus Nucleus has less pull on far off electrons The more electrons the more “polarizability” More.
Solid State Electronics EC 210 – EC 211 Prof.Dr. Iman Gamal Eldin Morsi 1.
1 Materials Science Concepts MATS-535 Electronics and Photonics Materials Scope a – Atomic Structure and Atomic Number b – Bonding and Type of Solids Dr.
Bond Types. Bond Types: At the conclusion of our time together, you should be able to: 1. Identify 5 different bond types 2. Explain each bond type 3.
HONORS CHEMISTRY Section 6.1 – Introduction to Chemical Bonding.
Ch. 6 Chemical Bonding What type of atom is stable or neutral in nature? Noble Gases – outer energy level is satisfied What is a chemical bond? An attraction.
Combining Matter Chapter 3 Section 2. Compounds Compounds are substances composed of atoms of two or more elements combined chemically Represented by.
Objectives Be able to explain why atoms sometimes join to form bonds Be able to explain why atoms sometimes join to form bonds Be able to explain why.
Physics 440 Condensed Matter Physics a.k.a. Materials Physics Solid-State Physics.
Molecular Orbitals: combine atomic orbitals (AOs) from all the atoms in a molecule into the same number of molecular orbitals. MOs have different shapes,
Notes 6 - Ions & Chemical Bonding. Unstable Atoms ► In order to be stable, an atom needs a certain number of valence electrons 2 valence e - if it only.
Electronegativity What is it? Electronegativity is the power of an atom to attract electrons in a bond.
Screening As a free electron approaches a positive cation, it will be attracted to the nucleus. But, it is also repelled by any electrons orbiting the.
Review: The H 2 Molecule E R eV 2 anti-bonding states 2 bonding states 2 protons two 1 s states each 4 states total alternative representations.
Chapter 4 Bonding. Metal + Nonmetal A nonmetal will take electrons from a metal. This transfer of electrons results in ions. The type of bond formed is.
Objectives Know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.
Chapter 6 Chemical Bonding. Introduction Chemical Bonding - mutual electrical attraction between the nuclei and valence electrons of different atoms that.
King Abdulaziz University Chemical and Materials Engineering Department Chapter 2 ATOMIC STRUCTURE AND INTERATOMIC BONDING Session II.
Types of Substances Unit 6 – Part II. Types of Substances Ionic Solid –3-D repeating pattern of + and – ions Crystal lattice Held together by ionic attractions.
Table of Contents Title: Combining Matter (Bonds) Page #: 25 Date: 10/16/12.
WHAT ARE IONIC BONDS? Section In an atom, the number of protons (+) equals the number of electrons (-). This is a neutral atom. When an atom gains.
Ionic Bonding. CA Standards Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons.
Dr. Jie ZouPHY Chapter 43 Molecules and Solids.
Chemical Bonding Why do bonds form?to lower the potential energy between positive and negative charges positive charges protons cations negative charges.
Born-Haber Cycle Section 15.2 (AHL). Lattice Enthalpy Of an ionic crystal: the heat energy absorbed (at constant pressure) when 1 mol of solid ionic compound.
© 2017 SlidePlayer.com Inc. All rights reserved.