Primary electrons make random elastic and inelastic collision either
... effect…. i.e. as to pass though the stronger electric filed, close to nuclei, it will suffer a “quantum jump” to a low energy state, which will make emission of X-ray photon, and it would be all possible energy up to E0… Secondary electron, (<50 eV, normally around 2-6 eV, larger than sample’s work ...
... effect…. i.e. as to pass though the stronger electric filed, close to nuclei, it will suffer a “quantum jump” to a low energy state, which will make emission of X-ray photon, and it would be all possible energy up to E0… Secondary electron, (<50 eV, normally around 2-6 eV, larger than sample’s work ...
Atomic Structure, Eelectronic Bonding, Periodicity, orbitals
... 1. Count the number of electrons brought to the party (element’s group number) 2. For ions we must adjust the number of electrons available. a. Add one e- for each negative charge. b. Subtract one e- for each positive charge. 3. Select a reasonable skeleton a. The least electronegative is the centra ...
... 1. Count the number of electrons brought to the party (element’s group number) 2. For ions we must adjust the number of electrons available. a. Add one e- for each negative charge. b. Subtract one e- for each positive charge. 3. Select a reasonable skeleton a. The least electronegative is the centra ...
No Slide Title
... what atoms are bonded to each other. Put least electronegative element in the center. 2. Count total number of valence e-. Add 1 for each negative charge. Subtract 1 for each positive charge. 3. Complete an octet for all atoms except hydrogen 4. If structure contains too many electrons, form double ...
... what atoms are bonded to each other. Put least electronegative element in the center. 2. Count total number of valence e-. Add 1 for each negative charge. Subtract 1 for each positive charge. 3. Complete an octet for all atoms except hydrogen 4. If structure contains too many electrons, form double ...
Matter Unit - OG
... * Kind of like orbits – in an “electron cloud” *Different energy depending on how close to the nucleus. (Think of a BEE HIVE) < Lower Energy – closer to nucleus.
... * Kind of like orbits – in an “electron cloud” *Different energy depending on how close to the nucleus. (Think of a BEE HIVE) < Lower Energy – closer to nucleus.
Test 4 Review
... Covalent Bonds. Covalent bonds are bonds formed by sharing electrons. The electrons of one atom are attracted to the protons of another, but neither atom pulls strongly enough to remove an electron from the other. Covalent bonds form when the electronegativity difference between the elements is less ...
... Covalent Bonds. Covalent bonds are bonds formed by sharing electrons. The electrons of one atom are attracted to the protons of another, but neither atom pulls strongly enough to remove an electron from the other. Covalent bonds form when the electronegativity difference between the elements is less ...
AP Chemistry
... What is the energy in joules of a mole of photons associated with visible light of wavelength 550 nm? ...
... What is the energy in joules of a mole of photons associated with visible light of wavelength 550 nm? ...
Dr Davids Essential Chemistry Definitions Bk1
... A molecule that is non-superimposable on its mirror image; such a molecule is optically active (meaning that it will rotate the plane of plane polarised light to the right or to the left). Chiral molecules frequently contain one or more asymmetric carbon atoms. Conjugate acid-base pairs: These are f ...
... A molecule that is non-superimposable on its mirror image; such a molecule is optically active (meaning that it will rotate the plane of plane polarised light to the right or to the left). Chiral molecules frequently contain one or more asymmetric carbon atoms. Conjugate acid-base pairs: These are f ...
- gst boces
... 15. Rutherford’s gold foil showed atoms small (+) nucleus & mostly empty space with e*few deflections = small (+) nucleus, most through = mostly empty space 16. Bohr’s model e- in orbits like planets around sun (orbit does NOT equal orbital) 17. Modern, wave-mechanical model e- in orbitals (most pro ...
... 15. Rutherford’s gold foil showed atoms small (+) nucleus & mostly empty space with e*few deflections = small (+) nucleus, most through = mostly empty space 16. Bohr’s model e- in orbits like planets around sun (orbit does NOT equal orbital) 17. Modern, wave-mechanical model e- in orbitals (most pro ...
Chapter 08
... There are two types of attractive forces in covalent molecules: Intramolecular bonding force that holds the atoms together Intermolecular forces between different molecules. Intermolecular forces are weak compared to intramolecular forces. Covalent compounds tend to be gases, liquids, or low-melting ...
... There are two types of attractive forces in covalent molecules: Intramolecular bonding force that holds the atoms together Intermolecular forces between different molecules. Intermolecular forces are weak compared to intramolecular forces. Covalent compounds tend to be gases, liquids, or low-melting ...
Specialization: 010700/02 Physics of atoms and molecules
... In this paper the ab initio calculations are carried out by means of the relativistic coupled cluster method including single and double cluster amplitudes (RCC-SD) of the effective electric field (E_{eff}) interacting with electric dipole moment of the electron (eEDM), hyperfine splitting constants ...
... In this paper the ab initio calculations are carried out by means of the relativistic coupled cluster method including single and double cluster amplitudes (RCC-SD) of the effective electric field (E_{eff}) interacting with electric dipole moment of the electron (eEDM), hyperfine splitting constants ...
Periodic Table Jeopardy
... A substance that cannot be separated or broken down into simpler substances by chemical means. All atoms in this substance have the same atomic #. ...
... A substance that cannot be separated or broken down into simpler substances by chemical means. All atoms in this substance have the same atomic #. ...
Summer Work
... 5. No two different elements will have the ______________________ atomic number. 6. The ______________________ of an element is the average mass of an element’s naturally occurring atom, or isotopes, taking into account the ______________________ of each isotope. 7. The ______________________ of an ...
... 5. No two different elements will have the ______________________ atomic number. 6. The ______________________ of an element is the average mass of an element’s naturally occurring atom, or isotopes, taking into account the ______________________ of each isotope. 7. The ______________________ of an ...
Chemistry Midterm Review 2006
... 3. Identify which ones have dipole-dipole forces? PBr3, N2, CF4, HBr, H2O 4. Identify which ones have London dispersion forces? , N2, CF4, HBr, SO2 5. Identify which ones have hydrogen bonding? HCl,, H2, HBr, H2O, CH4 6. Define the physical properties of Viscosity, Surface Tension, Boiling Point and ...
... 3. Identify which ones have dipole-dipole forces? PBr3, N2, CF4, HBr, H2O 4. Identify which ones have London dispersion forces? , N2, CF4, HBr, SO2 5. Identify which ones have hydrogen bonding? HCl,, H2, HBr, H2O, CH4 6. Define the physical properties of Viscosity, Surface Tension, Boiling Point and ...
Electrons #1
... We can determine the position of an e- from the nucleus through 4 Quantum Numbers: 1. Principle Number (Energy of e-) 2. Angular Momentum Number (Shape of Orbital) 3. Magnetic Number (Orientation/Position of Orbital) 4. Spin Number (Spin on e- ; +/-) ...
... We can determine the position of an e- from the nucleus through 4 Quantum Numbers: 1. Principle Number (Energy of e-) 2. Angular Momentum Number (Shape of Orbital) 3. Magnetic Number (Orientation/Position of Orbital) 4. Spin Number (Spin on e- ; +/-) ...
Document
... The atoms in metals are built up layer upon layer in a regular pattern, this means they form crystals. They are another example of a giant structure We can think of metallic bonding as positively charged metal ions which are held together by electrons from the outermost shell of each metal atom. ...
... The atoms in metals are built up layer upon layer in a regular pattern, this means they form crystals. They are another example of a giant structure We can think of metallic bonding as positively charged metal ions which are held together by electrons from the outermost shell of each metal atom. ...
Midterm 2 Review slides from November 15
... Bonding strengthens as electrons are added to bonding orbitals strength of bonding in the transition metals increases until the band structure is roughly half-full roughly 6-7 electrons strength decreases with more than 67 valence electrons because some electrons are in antibonding orbitals valence ...
... Bonding strengthens as electrons are added to bonding orbitals strength of bonding in the transition metals increases until the band structure is roughly half-full roughly 6-7 electrons strength decreases with more than 67 valence electrons because some electrons are in antibonding orbitals valence ...
Chemical Bonding
... Draw valence molecular orbital diagrams (i.e. omitting inner shell orbitals) for the following homonuclear diatomic species, H2!, He2+, O2, N2!, C22!, Ne2+, (Na2, Mg2, P2, you can assume that third period diatomics form valence molecular orbitals similar to second period diatomics but with n=3) and ...
... Draw valence molecular orbital diagrams (i.e. omitting inner shell orbitals) for the following homonuclear diatomic species, H2!, He2+, O2, N2!, C22!, Ne2+, (Na2, Mg2, P2, you can assume that third period diatomics form valence molecular orbitals similar to second period diatomics but with n=3) and ...
Equilibrium
... E=Electron Pair ● When molecules exhibit resonance, any structures can be used to predict molecular structure using VSEPR model ● VSEPR works in most cases for non-ionic compounds Sigma and pi bonds ● Sigma Bonds: Bond in which the electron pair is shared in an area centered on a line running betwee ...
... E=Electron Pair ● When molecules exhibit resonance, any structures can be used to predict molecular structure using VSEPR model ● VSEPR works in most cases for non-ionic compounds Sigma and pi bonds ● Sigma Bonds: Bond in which the electron pair is shared in an area centered on a line running betwee ...
Electron Configuration
... electrons are located in orbitals, is also known as the quantum model ◦ States electrons within an energy level are located in orbitals, regions of high probability for finding a particular electrons. ◦ Does not, however, explain how the electrons move about the nucleus to create these regions ...
... electrons are located in orbitals, is also known as the quantum model ◦ States electrons within an energy level are located in orbitals, regions of high probability for finding a particular electrons. ◦ Does not, however, explain how the electrons move about the nucleus to create these regions ...
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.