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stationary state
... • Some particles are deflected by large angles near 180 degree, which can not be explained by Thomson’s atomic model. • In Rutherford’s atomic model, all the positive charges and most of the mass are confined in a very small “nucleus” of the atom. ...
... • Some particles are deflected by large angles near 180 degree, which can not be explained by Thomson’s atomic model. • In Rutherford’s atomic model, all the positive charges and most of the mass are confined in a very small “nucleus” of the atom. ...
How to balance chemical equations File
... This equation shows you what happens in the reaction, but it doesn’t show you how much of each element you need to produce the ammonia. To find out how much of each element you need, you have to balance the equation — make sure that the number of atoms on the left side of the equation equals the num ...
... This equation shows you what happens in the reaction, but it doesn’t show you how much of each element you need to produce the ammonia. To find out how much of each element you need, you have to balance the equation — make sure that the number of atoms on the left side of the equation equals the num ...
The Periodic table
... A region of space within an electron subshell where an electron with a specific energy is most likely to be found. S subshell=1 orbital, p subshell=3 orbitals, d subshell=5 orbitals, f subshell=7 orbitals. Maximum number of electrons in a subshell is always 2. S orbital=spherical, p orbital ...
... A region of space within an electron subshell where an electron with a specific energy is most likely to be found. S subshell=1 orbital, p subshell=3 orbitals, d subshell=5 orbitals, f subshell=7 orbitals. Maximum number of electrons in a subshell is always 2. S orbital=spherical, p orbital ...
Chapter 4 Notes
... atoms as they return to lower energy states • Light is given off in very definite wavelengths • A spectroscope reveals lines of particular colorslight passed through a prism; specific frequencies ...
... atoms as they return to lower energy states • Light is given off in very definite wavelengths • A spectroscope reveals lines of particular colorslight passed through a prism; specific frequencies ...
Chapter 4
... not as particles, but more as waves (like light waves) which can gain or lose energy. But they can’t gain or lose just any amount of energy. They gain or lose a “quantum” of energy. A quantum is just an amount of energy that the electron needs to gain (or lose) to move to the next energy level. In ...
... not as particles, but more as waves (like light waves) which can gain or lose energy. But they can’t gain or lose just any amount of energy. They gain or lose a “quantum” of energy. A quantum is just an amount of energy that the electron needs to gain (or lose) to move to the next energy level. In ...
Honors Chemistry Final Review
... When given the formula, and writing the name for ionic compounds, remember to place the names in the same order as they appear in the formula. Remember, that if a transition metal, tin or lead appears, you will need a Roman Numeral. The Roman Numeral indicates the charge of the metal ion, and while ...
... When given the formula, and writing the name for ionic compounds, remember to place the names in the same order as they appear in the formula. Remember, that if a transition metal, tin or lead appears, you will need a Roman Numeral. The Roman Numeral indicates the charge of the metal ion, and while ...
The Wizard Test Maker
... dioxide has a much higher melting point than CuO? (A) Copper is a metal and silicon is a metalloid. (B) Copper dioxide has the greater dipole moment. (C) Van der Waals forces are only important in CuO. (D) SiO2 is a network covalent solid. (E) SiO2 is a body centered lattice; CuO is a face centered ...
... dioxide has a much higher melting point than CuO? (A) Copper is a metal and silicon is a metalloid. (B) Copper dioxide has the greater dipole moment. (C) Van der Waals forces are only important in CuO. (D) SiO2 is a network covalent solid. (E) SiO2 is a body centered lattice; CuO is a face centered ...
Section 4.8: The Structure and Properties of Solids
... orthorhombic lattice structure of linear H–Cl molecules. 5. Doping means adding a small amount of an additional element, such as boron or arsenic, to a semiconductor. This is done to change the conductive properties of the ...
... orthorhombic lattice structure of linear H–Cl molecules. 5. Doping means adding a small amount of an additional element, such as boron or arsenic, to a semiconductor. This is done to change the conductive properties of the ...
Chapter 6:Electronic Structure of Atoms
... energy of illumination showed that the interaction must be like that of a particle which gave all of its energy to the electron! • This fit in well with Planck's hypothesis that light in the blackbody radiation experiment could exist only in discrete bundles with energy. • Sample Problem pg 379 and ...
... energy of illumination showed that the interaction must be like that of a particle which gave all of its energy to the electron! • This fit in well with Planck's hypothesis that light in the blackbody radiation experiment could exist only in discrete bundles with energy. • Sample Problem pg 379 and ...
QUANTUM CHEMISTRY Model 1: Light and Waves Critical thinking
... Model 3: Atomic Orbitals and Quantum Numbers The wave functions for electrons in atoms are given the special name ‘atomic orbitals’. As explored in worksheet 1, the energy levels of hydrogen-like (one-electron) atoms are determined by a single quantum number, n. For other atoms, more quantities are ...
... Model 3: Atomic Orbitals and Quantum Numbers The wave functions for electrons in atoms are given the special name ‘atomic orbitals’. As explored in worksheet 1, the energy levels of hydrogen-like (one-electron) atoms are determined by a single quantum number, n. For other atoms, more quantities are ...
Chemistry 1 Lectures
... – Iron can be +2 or +3 – Smaller charge is sometimes named as an ‘ic’ ion higher charge as an ‘ous’ ion – So in ferric chloride (FeCl2) iron ion is Fe2+ – Modern method is to indicate charge on the metal with Roman numerals ...
... – Iron can be +2 or +3 – Smaller charge is sometimes named as an ‘ic’ ion higher charge as an ‘ous’ ion – So in ferric chloride (FeCl2) iron ion is Fe2+ – Modern method is to indicate charge on the metal with Roman numerals ...
File
... 20. Element whose atoms lose electrons in chemical reactions to become positive ions. 21. Groups 3-12 on the periodic table. 22. Scientist who performed the gold foil experiment, and concluded that an atom must be composed of mostly empty space with a small, dense, positively-charged nucleus. 23. An ...
... 20. Element whose atoms lose electrons in chemical reactions to become positive ions. 21. Groups 3-12 on the periodic table. 22. Scientist who performed the gold foil experiment, and concluded that an atom must be composed of mostly empty space with a small, dense, positively-charged nucleus. 23. An ...
Boltzmann/Saha Equation Problems/Questions
... a) As stated in the problem, the ionization energy of hydrogen is the energy required to remove the electron from the ground state - effectively a transition from n=1 to n=inf, which simply corresponds to the energy of the ground state: E1 =χi =13.6 eV. b) According to the Boltzmann equation, at T=8 ...
... a) As stated in the problem, the ionization energy of hydrogen is the energy required to remove the electron from the ground state - effectively a transition from n=1 to n=inf, which simply corresponds to the energy of the ground state: E1 =χi =13.6 eV. b) According to the Boltzmann equation, at T=8 ...
Chemical Bonding II
... In ethylene, H2C=CH2, the sp2 orbitals are used to make one of the bonds between the carbon atoms and the bonds between carbon and hydrogen. These bonds have electron density along the internuclear (bond) axis. This type of bond is called a σ (sigma) bond. ...
... In ethylene, H2C=CH2, the sp2 orbitals are used to make one of the bonds between the carbon atoms and the bonds between carbon and hydrogen. These bonds have electron density along the internuclear (bond) axis. This type of bond is called a σ (sigma) bond. ...
Ch6-Energy in Chemical Reactions-Chemical Reactions
... Chemical Reactions: Enthalpy and Hesse’s Law Calculations Why? In chemistry, the mole is the standard measurement of amount. When substances react according to chemical equations, they do so in simple ratios of moles. However, balances give readings in grams. Balances DO NOT give readings in moles. ...
... Chemical Reactions: Enthalpy and Hesse’s Law Calculations Why? In chemistry, the mole is the standard measurement of amount. When substances react according to chemical equations, they do so in simple ratios of moles. However, balances give readings in grams. Balances DO NOT give readings in moles. ...
transport1
... It’s possible to find specific modes that are independent, that is if one is excited, it does not excite the other: these are the normal modes. For CO2, these are: 1, 2, 3 and 4. Each normal mode q behaves like an independent harmonic oscillator (approximation), so has a series of terms Gq( ...
... It’s possible to find specific modes that are independent, that is if one is excited, it does not excite the other: these are the normal modes. For CO2, these are: 1, 2, 3 and 4. Each normal mode q behaves like an independent harmonic oscillator (approximation), so has a series of terms Gq( ...
Models of the Atom
... Could not explain why emission lines are double, triple or more Could not explain why some lines brighter than others Could not explain how atoms bond Mixed classical and quantum ideas ...
... Could not explain why emission lines are double, triple or more Could not explain why some lines brighter than others Could not explain how atoms bond Mixed classical and quantum ideas ...
Chapt3
... Ionic Compounds -- Ionic Bonding -- electron transfer result from transfer of one or more electrons from one atom to another to yield oppositely-charged particles called ions cation = positive ion ...
... Ionic Compounds -- Ionic Bonding -- electron transfer result from transfer of one or more electrons from one atom to another to yield oppositely-charged particles called ions cation = positive ion ...
Chemistry - Isotopes
... and all higher energy levels are called _______________ states. When an electron “moves” from a higher to a lower energy level, it _____________ one “package” (_________, or __________) of EM radiation. Bohr’s model is commonly called the _______________ model, because he assumed the _______________ ...
... and all higher energy levels are called _______________ states. When an electron “moves” from a higher to a lower energy level, it _____________ one “package” (_________, or __________) of EM radiation. Bohr’s model is commonly called the _______________ model, because he assumed the _______________ ...
Chemistry COS 2011-2012
... Solubility depends on the chemical make up of both the solute and the solvent. Colligative properties depend only on the number of solute particles present. Colligative properties include freezing point depression, boiling point elevation and osmotic pressure. ...
... Solubility depends on the chemical make up of both the solute and the solvent. Colligative properties depend only on the number of solute particles present. Colligative properties include freezing point depression, boiling point elevation and osmotic pressure. ...
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.