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普通化学 (全英文) 教学大纲
... (c).How to fill electrons in different orbitals (d).Be able to draw the electron configuration of the first 20 elements (e).Unpaired electrons, Spin, Paramagnetic and Diamagnetism 2.5.Comparing the atomic orbitals with Bohr’s model of atoms (Classical but incorrect) 2.6.Electron’s states (a).Each st ...
... (c).How to fill electrons in different orbitals (d).Be able to draw the electron configuration of the first 20 elements (e).Unpaired electrons, Spin, Paramagnetic and Diamagnetism 2.5.Comparing the atomic orbitals with Bohr’s model of atoms (Classical but incorrect) 2.6.Electron’s states (a).Each st ...
Honors Chemistry
... Opposites attract : the positive or more metallic ion goes first when writing the formula The farther to the left on the periodic table, the more metallic. When writing a compound’s formula, write the ions’ symbols with the charge. If the charges add up to zero, then just put the symbols together to ...
... Opposites attract : the positive or more metallic ion goes first when writing the formula The farther to the left on the periodic table, the more metallic. When writing a compound’s formula, write the ions’ symbols with the charge. If the charges add up to zero, then just put the symbols together to ...
rev8thgrade - PAMS
... acceleration is always a curve. Objects moving with circular motion are constantly accelerating because direction (and hence velocity) is ...
... acceleration is always a curve. Objects moving with circular motion are constantly accelerating because direction (and hence velocity) is ...
Chemistry (B) Final Exam Study Guide 1
... a. They are greater in magnitude than those between lower energy levels. b. They are smaller in magnitude than those between lower energy levels. c. There is no significant difference in the magnitudes of these differences. d. No answer can be determined from the information given. ____ 58. Bohr's m ...
... a. They are greater in magnitude than those between lower energy levels. b. They are smaller in magnitude than those between lower energy levels. c. There is no significant difference in the magnitudes of these differences. d. No answer can be determined from the information given. ____ 58. Bohr's m ...
AP Chemistry Chapter 7 Review Packet
... The orange-yellow color of sodium-vapor streetlights results from electrons in sodium atoms falling from 3p to 3s orbitals. The wavelength of one orange-yellow line in the spectrum of sodium is 589 nm. a. Write the electron configuration for the ground state of sodium. b. Write the electron configur ...
... The orange-yellow color of sodium-vapor streetlights results from electrons in sodium atoms falling from 3p to 3s orbitals. The wavelength of one orange-yellow line in the spectrum of sodium is 589 nm. a. Write the electron configuration for the ground state of sodium. b. Write the electron configur ...
C2 Revision Quick Questions FT
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
C2 Revision Quick Questions FT
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
C2 revision slides V3 + questions + MS – F
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
... increases number of collisions and increases rate Temperature: Particles have more energy and move faster and collide more often. More particles have energy greater than the activation energy so more successful collisions Catalyst: Catalysts change the rate of chemical reactions but are not used up ...
Valence Bond Theory
... Double and Triple Covalent Bonds Experimental evidence determined that three substances can be formed when two carbons atoms bonded with hydrogen – C2H6(g), C2H4(g), and C2H2(g). Lewis suggested that between the carbon atoms there must a sharing of one, two, and three electron pairs in order to ...
... Double and Triple Covalent Bonds Experimental evidence determined that three substances can be formed when two carbons atoms bonded with hydrogen – C2H6(g), C2H4(g), and C2H2(g). Lewis suggested that between the carbon atoms there must a sharing of one, two, and three electron pairs in order to ...
Sugárkémiai áttekintés Schiller Róbert
... Heavy ions, γ-photons, fast electrons – all of them produce low-energy secondary electrons in the medium (γ: photoeffect, Compton-effect, pair production). The good part of the electron energy is imparted to the atoms/molecules of the medium via Coulomb interaction Er, t ...
... Heavy ions, γ-photons, fast electrons – all of them produce low-energy secondary electrons in the medium (γ: photoeffect, Compton-effect, pair production). The good part of the electron energy is imparted to the atoms/molecules of the medium via Coulomb interaction Er, t ...
File
... (5) Define isotope and state how the atomic structure for isotopes of the same element are similar and different. (6) Calculate the average atomic mass from the relative abundances and masses of each isotope. (7) Define valence electrons and determine the number of valence electrons for an atom. (8) ...
... (5) Define isotope and state how the atomic structure for isotopes of the same element are similar and different. (6) Calculate the average atomic mass from the relative abundances and masses of each isotope. (7) Define valence electrons and determine the number of valence electrons for an atom. (8) ...
Atomic Structure Mini Lab
... To understand how the number of protons, neutrons and electrons determine the properties of atoms Procedure: Obtain a baggie from your instructor Baggies contain the following: White bead represents a proton Purple bead represents a neutron Blue bead represents an electron Count the number of proton ...
... To understand how the number of protons, neutrons and electrons determine the properties of atoms Procedure: Obtain a baggie from your instructor Baggies contain the following: White bead represents a proton Purple bead represents a neutron Blue bead represents an electron Count the number of proton ...
acids and bases - No Brain Too Small
... You get given a table of ions but need to learn their names ...
... You get given a table of ions but need to learn their names ...
pptx - Yale University
... STM, and SNOM, have enabled chemists to “feel” individual molecules and atoms. SPM techniques are not quite good enough yet to study how electrons are distributed in bonds. Because light is scattered predominantly by the charged particles with the smallest mass, the electron distribution in molecule ...
... STM, and SNOM, have enabled chemists to “feel” individual molecules and atoms. SPM techniques are not quite good enough yet to study how electrons are distributed in bonds. Because light is scattered predominantly by the charged particles with the smallest mass, the electron distribution in molecule ...
Chapter 7 Lect. 2
... III. Orbital Shapes and Energies A. Atomic orbital shapes are surfaces that surround 90% of the total probability of where its electrons are 1. Look at l = 0, the s-orbitals 2. Basic shape of an s-orbital is spherical centered on the nucleus 3. Basic shape is same for same l values 4. Nodes = area ...
... III. Orbital Shapes and Energies A. Atomic orbital shapes are surfaces that surround 90% of the total probability of where its electrons are 1. Look at l = 0, the s-orbitals 2. Basic shape of an s-orbital is spherical centered on the nucleus 3. Basic shape is same for same l values 4. Nodes = area ...
Physical Science Week 1
... Molecules (IAN #9) • Matter: Anything that takes up space and has mass. • Atom: The smallest unit of an element that maintains the properties of that element. ...
... Molecules (IAN #9) • Matter: Anything that takes up space and has mass. • Atom: The smallest unit of an element that maintains the properties of that element. ...
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.