Lectures 1-2
... MO diagrams relate the energies of molecular orbitals to the atomic orbitals from which they were derived. If the total energy of the electrons is lower using molecular orbitals (the middle column), the molecule forms. If the total energy of the electrons is lower using atomic orbitals (the two outs ...
... MO diagrams relate the energies of molecular orbitals to the atomic orbitals from which they were derived. If the total energy of the electrons is lower using molecular orbitals (the middle column), the molecule forms. If the total energy of the electrons is lower using atomic orbitals (the two outs ...
Regents_Chem_Core_for_review
... IV.2 Two major categories of compounds are ionic and molecular (covalent) compounds. (5.2g) IV.3 Chemical bonds are formed when valence electrons are (5.2a): • transferred from one atom to another (ionic) • shared between atoms (covalent) • mobile within a metal (metallic) IV.4 In a multiple covalen ...
... IV.2 Two major categories of compounds are ionic and molecular (covalent) compounds. (5.2g) IV.3 Chemical bonds are formed when valence electrons are (5.2a): • transferred from one atom to another (ionic) • shared between atoms (covalent) • mobile within a metal (metallic) IV.4 In a multiple covalen ...
Chemistry - nyostrander.us
... 3. State the model that first included electrons as subatomic particles. [2] The Thomson model first included electrons (the negatively charged particles). _________________________________________________________________________ 4. State one conclusion about the internal structure of the atom that ...
... 3. State the model that first included electrons as subatomic particles. [2] The Thomson model first included electrons (the negatively charged particles). _________________________________________________________________________ 4. State one conclusion about the internal structure of the atom that ...
Exam 2-1
... Einstein’s explanation of the photoelectric effect. Rutherford’s experiment with a beam of α particles passing through gold foil. Boer’s model of the atom. Faraday’s experiment of the electroplating of metals. Binnig and Rohrer’s demonstration of the scanning tunneling microscope. ...
... Einstein’s explanation of the photoelectric effect. Rutherford’s experiment with a beam of α particles passing through gold foil. Boer’s model of the atom. Faraday’s experiment of the electroplating of metals. Binnig and Rohrer’s demonstration of the scanning tunneling microscope. ...
CHEM 400 - El Camino College
... possible Lewis structure. Remember that resonance structures are considered when a single Lewis structure cannot be given to adequately describe the experimentally observed properties of a molecule or a polyatomic ion. Remember that resonance structures differ from each by the location of certain el ...
... possible Lewis structure. Remember that resonance structures are considered when a single Lewis structure cannot be given to adequately describe the experimentally observed properties of a molecule or a polyatomic ion. Remember that resonance structures differ from each by the location of certain el ...
CHM1045 General Chemistry and Qualitative Analysis
... Stipulating the maximum number of electrons that can be accommodated in the various principal energy levels, sublevels, and orbitals. Generating the spectroscopic electronic configuration of elements and ions. Relating the number of paired or unpaired electrons in a species to their diamagnetism o ...
... Stipulating the maximum number of electrons that can be accommodated in the various principal energy levels, sublevels, and orbitals. Generating the spectroscopic electronic configuration of elements and ions. Relating the number of paired or unpaired electrons in a species to their diamagnetism o ...
View
... 3. Method and details of the calculations The quantum chemical calculations were performed using the software MOLCAS-6.0.7 The complete active space (CAS) SCF method8 was used to generate molecular orbitals and reference functions for subsequent multiconfigurational second order perturbation calculat ...
... 3. Method and details of the calculations The quantum chemical calculations were performed using the software MOLCAS-6.0.7 The complete active space (CAS) SCF method8 was used to generate molecular orbitals and reference functions for subsequent multiconfigurational second order perturbation calculat ...
Elementary my dear Watson review
... are involved and the numbers tell us how many atoms of each kind are involved. For example, water (H20) is made up of 2 atoms of hydrogen and 1 atom of oxygen. For example, carbon dioxide (CO2) is made up of 1 atom of carbon and two atoms of oxygen. ...
... are involved and the numbers tell us how many atoms of each kind are involved. For example, water (H20) is made up of 2 atoms of hydrogen and 1 atom of oxygen. For example, carbon dioxide (CO2) is made up of 1 atom of carbon and two atoms of oxygen. ...
K,7th Grade Test Review: Atoms and Chemical Reactions PART
... 1. __________ is the smallest unit of an element that is still that element. 2. __________ is a substance that cannot be broken down into similar substances by physical or chemical changes. 3. Protons and neutrons have a __________ of 1 unit. Electrons have almost none. 4. An atom with more protons ...
... 1. __________ is the smallest unit of an element that is still that element. 2. __________ is a substance that cannot be broken down into similar substances by physical or chemical changes. 3. Protons and neutrons have a __________ of 1 unit. Electrons have almost none. 4. An atom with more protons ...
Corso di Fisica Moderna
... With the use of spectroscopy in the late 19th century, it was found that the radiaAon from hydrogen, as well as other atoms, was emiNed at specific quanAzed frequencies. It was the effort to exp ...
... With the use of spectroscopy in the late 19th century, it was found that the radiaAon from hydrogen, as well as other atoms, was emiNed at specific quanAzed frequencies. It was the effort to exp ...
Answer Sheet to Review Questions
... 31. Fluorine has a higher electronegativity value than iodine and therefore has a greater pull on the shared electrons causing the bond to be more polar. 32. Sulfur (S) 33. It is a symmetrical molecule 34. The electronegativity values of C and O are different and produce a polar bond, while the two ...
... 31. Fluorine has a higher electronegativity value than iodine and therefore has a greater pull on the shared electrons causing the bond to be more polar. 32. Sulfur (S) 33. It is a symmetrical molecule 34. The electronegativity values of C and O are different and produce a polar bond, while the two ...
The Structure of Matter
... • Elements in last (next to last) column require one (two) electron(s) to complete a closed shell • These atoms lose electrons and form negative ions. ...
... • Elements in last (next to last) column require one (two) electron(s) to complete a closed shell • These atoms lose electrons and form negative ions. ...
Document
... 13) List 5 properties of nonmetals. Where are the nonmetals located on the Periodic Table? Where is the most reactive nonmetal located? Brittle, don’t conduct, may be solids, liquids or gases, not ductile, not malleable Right of the zig-zag line Fluorine 14) Name and describe the two main classifica ...
... 13) List 5 properties of nonmetals. Where are the nonmetals located on the Periodic Table? Where is the most reactive nonmetal located? Brittle, don’t conduct, may be solids, liquids or gases, not ductile, not malleable Right of the zig-zag line Fluorine 14) Name and describe the two main classifica ...
Summer Assignment 2015
... 6. Naturally occurring chlorine is 75.78% 35Cl, which has an atomic mass of 34.969 amu, and 24.22% 37Cl, which has an atomic mass of 36.966 amu. Calculate the average atomic mass (that is, the atomic weight) of chlorine. 7. Write the empirical formulas for the following molecules: (a) glucose, a sub ...
... 6. Naturally occurring chlorine is 75.78% 35Cl, which has an atomic mass of 34.969 amu, and 24.22% 37Cl, which has an atomic mass of 36.966 amu. Calculate the average atomic mass (that is, the atomic weight) of chlorine. 7. Write the empirical formulas for the following molecules: (a) glucose, a sub ...
topic 1 sol review homework
... all are diatomics, all have 7 valence electrons, all are halogens 9. The increase in atomic radius of each successive element within a group is due to an increase in the number of a) neutrons b) valence electrons c) unpaired electrons d) principle energy levels 10. According to the modern periodic t ...
... all are diatomics, all have 7 valence electrons, all are halogens 9. The increase in atomic radius of each successive element within a group is due to an increase in the number of a) neutrons b) valence electrons c) unpaired electrons d) principle energy levels 10. According to the modern periodic t ...
Regents Chemistry
... Be able to explain why energy is absorbed when a bond is broken & energy is released when a bond is formed. o ...
... Be able to explain why energy is absorbed when a bond is broken & energy is released when a bond is formed. o ...
atomic theory - unit a
... 2.3 ATOM: smallest particle of an element that retains the chemical identity of the element (John Dalton). • Atomic size: 0.1 - 0.5 nm • 1981 - STM (scanning tunneling microscope) used to "see" atoms Dalton's Atomic Theory - 1808 1) Each element is composed of small particles called atoms. 2) All at ...
... 2.3 ATOM: smallest particle of an element that retains the chemical identity of the element (John Dalton). • Atomic size: 0.1 - 0.5 nm • 1981 - STM (scanning tunneling microscope) used to "see" atoms Dalton's Atomic Theory - 1808 1) Each element is composed of small particles called atoms. 2) All at ...
Chemical bond
A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are ""strong bonds"" such as covalent or ionic bonds and ""weak bonds"" such as Dipole-dipole interaction, the London dispersion force and hydrogen bonding.Since opposite charges attract via a simple electromagnetic force, the negatively charged electrons that are orbiting the nucleus and the positively charged protons in the nucleus attract each other. An electron positioned between two nuclei will be attracted to both of them, and the nuclei will be attracted toward electrons in this position. This attraction constitutes the chemical bond. Due to the matter wave nature of electrons and their smaller mass, they must occupy a much larger amount of volume compared with the nuclei, and this volume occupied by the electrons keeps the atomic nuclei relatively far apart, as compared with the size of the nuclei themselves. This phenomenon limits the distance between nuclei and atoms in a bond.In general, strong chemical bonding is associated with the sharing or transfer of electrons between the participating atoms. The atoms in molecules, crystals, metals and diatomic gases—indeed most of the physical environment around us—are held together by chemical bonds, which dictate the structure and the bulk properties of matter.All bonds can be explained by quantum theory, but, in practice, simplification rules allow chemists to predict the strength, directionality, and polarity of bonds. The octet rule and VSEPR theory are two examples. More sophisticated theories are valence bond theory which includes orbital hybridization and resonance, and the linear combination of atomic orbitals molecular orbital method which includes ligand field theory. Electrostatics are used to describe bond polarities and the effects they have on chemical substances.