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General Chemistry - Review for final exam: (Make sure you bring
... 32. What did the following say about orbital systems: a. Hund b. Aufbau c. Pauli 33. List parts of the visible electromagnetic spectrum & label in terms of frequency, wavelength, & energy. 34. What is the formula for the speed of light? 35. How is a photon created as an atom is heated? 36. Accordin ...
... 32. What did the following say about orbital systems: a. Hund b. Aufbau c. Pauli 33. List parts of the visible electromagnetic spectrum & label in terms of frequency, wavelength, & energy. 34. What is the formula for the speed of light? 35. How is a photon created as an atom is heated? 36. Accordin ...
Slide 1
... photo-electric effect: light behaves as a particle Discovery of the nucleus: Rutherford scattering experiment Today: Atomic spectra: emission and absorption. Evidence for atomic energy levels Bohr’s model of the hydrogen atom Continuous emission: black-body radiation ...
... photo-electric effect: light behaves as a particle Discovery of the nucleus: Rutherford scattering experiment Today: Atomic spectra: emission and absorption. Evidence for atomic energy levels Bohr’s model of the hydrogen atom Continuous emission: black-body radiation ...
atomsagain
... To describe one electron, we give the following information: •n – this is called the shell Shells are labeled by numbers 1, 2, 3, . . . •l – this is called the subshell Subshells are denoted by letter s, p, d, f, g •m – this is called the orbital orbital depends on choice of axes •ms – this is ...
... To describe one electron, we give the following information: •n – this is called the shell Shells are labeled by numbers 1, 2, 3, . . . •l – this is called the subshell Subshells are denoted by letter s, p, d, f, g •m – this is called the orbital orbital depends on choice of axes •ms – this is ...
Chapter 10 - Lecture 3
... Structures of many-electron atoms • Because of electron correlation, no simple analytical expression for orbitals is possible • Therefore ψ(r1, r2, ….) can be expressed as ψ(r1)ψ(r2)… • Called the orbital approximation • Individual hydrogenic orbitals modified by presence of other electrons ...
... Structures of many-electron atoms • Because of electron correlation, no simple analytical expression for orbitals is possible • Therefore ψ(r1, r2, ….) can be expressed as ψ(r1)ψ(r2)… • Called the orbital approximation • Individual hydrogenic orbitals modified by presence of other electrons ...
Notes - Ms. Dawkins
... A neutron has about the ______________ ___________ as a proton. They are grouped together in the ______________________. Atoms are extremely ________________. The electron cloud is about _______________ times the size of the __________________. Electrons are much smaller than _____________________ ...
... A neutron has about the ______________ ___________ as a proton. They are grouped together in the ______________________. Atoms are extremely ________________. The electron cloud is about _______________ times the size of the __________________. Electrons are much smaller than _____________________ ...
chapter
... • Atoms with full valence shells are unreactive • When the valence shell is not full, an atom tends to lose, gain, or share electrons to achieve a full outer shell • Elements in the same vertical column (group) of the periodic table have similar chemical properties ...
... • Atoms with full valence shells are unreactive • When the valence shell is not full, an atom tends to lose, gain, or share electrons to achieve a full outer shell • Elements in the same vertical column (group) of the periodic table have similar chemical properties ...
Chemistry I – Semester I Final Review
... - list and define common metric base units and prefixes - construct conversion factors from equivalent measurements and apply techniques of dimensional analysis (factor-label method) in problem solving - report measurements to the correct number of significant digits - express large and small number ...
... - list and define common metric base units and prefixes - construct conversion factors from equivalent measurements and apply techniques of dimensional analysis (factor-label method) in problem solving - report measurements to the correct number of significant digits - express large and small number ...
Chapter 7-8-9
... 1. How many moles are in 220 g of CO2? 2. One mole of (NH4)2HPO4 contains _?_ moles of hydrogen atoms. 3. The atomic mass of sodium is 23. The number of moles in 46g of sodium is ________. 4. The molar mass of ammonia is _________. 5. What is the number of molecules in 4.25 g of ammonia? 6. How many ...
... 1. How many moles are in 220 g of CO2? 2. One mole of (NH4)2HPO4 contains _?_ moles of hydrogen atoms. 3. The atomic mass of sodium is 23. The number of moles in 46g of sodium is ________. 4. The molar mass of ammonia is _________. 5. What is the number of molecules in 4.25 g of ammonia? 6. How many ...
final exam practice test - Clayton State University
... b. The presence of lone (unshared) pairs of electrons affect the dipole moment of a molecule. c. Generally, as electronegativity differences increases in diatomic molecules, the dipole moments increase. d. The dipole moment equals the product of charge and distance of separation of the charges. e. B ...
... b. The presence of lone (unshared) pairs of electrons affect the dipole moment of a molecule. c. Generally, as electronegativity differences increases in diatomic molecules, the dipole moments increase. d. The dipole moment equals the product of charge and distance of separation of the charges. e. B ...
Electron Configurations
... • According to the Heisenberg Uncertainty Principle we can not know the exact position and motion of electrons with complete certainty. • We can only describe the probable locations of electrons. • We will describe the location of electrons when the atom is at its lowest energy . • These are called ...
... • According to the Heisenberg Uncertainty Principle we can not know the exact position and motion of electrons with complete certainty. • We can only describe the probable locations of electrons. • We will describe the location of electrons when the atom is at its lowest energy . • These are called ...
section_2_review_set
... 1. What is the claim to fame for the proton? determines the element 2. What is the claim to fame for the electron? creates the chemical bonds 3. What is the claim to fame for the neutron? stabilizes the nucleus 4. What is the mass of each of the following particles?: proton 1; neutron 1; electron 0. ...
... 1. What is the claim to fame for the proton? determines the element 2. What is the claim to fame for the electron? creates the chemical bonds 3. What is the claim to fame for the neutron? stabilizes the nucleus 4. What is the mass of each of the following particles?: proton 1; neutron 1; electron 0. ...
Chemistry 102 Summary June 25th - Bohr model only works for one
... Specific wave functions are called orbitals. Orbitals define the allowed energy states where electrons can reside. There are four basic shapes: s, p, d and f Shapes represent where an electron will reside 90 % of the time in that allowed energy state. From Heisenberg – the exact location cannot be d ...
... Specific wave functions are called orbitals. Orbitals define the allowed energy states where electrons can reside. There are four basic shapes: s, p, d and f Shapes represent where an electron will reside 90 % of the time in that allowed energy state. From Heisenberg – the exact location cannot be d ...
Shiny, Happy Pretest - Alex LeMay – Science
... _____22. In a reaction, nothing is created or destroyed; the mass of the reactants before the reaction is the same as the mass of the product after the reaction. _____23. When nature chemically combines substances, they always combine with a set amount of one substance and a set amount of the other. ...
... _____22. In a reaction, nothing is created or destroyed; the mass of the reactants before the reaction is the same as the mass of the product after the reaction. _____23. When nature chemically combines substances, they always combine with a set amount of one substance and a set amount of the other. ...
Bohr Model Notes - Northwest ISD Moodle
... 2 electrons can fit in the first energy level. 8 electrons can fit in the second energy level. 18 electrons can fit in the third energy level. Valence Electrons – electrons found in the outermost energy levels. Magnesium has 2 valence electrons. Rule of Eight – Elements that have the maximum n ...
... 2 electrons can fit in the first energy level. 8 electrons can fit in the second energy level. 18 electrons can fit in the third energy level. Valence Electrons – electrons found in the outermost energy levels. Magnesium has 2 valence electrons. Rule of Eight – Elements that have the maximum n ...
Solid - burgess
... 3. the properties of the compound are different from the properties of the elements that make up the compound 4. can be separated only by a chemical reaction 5. two types of compounds a. ionic i. formed by the attraction between two or more elements that transfer electrons known as ions ...
... 3. the properties of the compound are different from the properties of the elements that make up the compound 4. can be separated only by a chemical reaction 5. two types of compounds a. ionic i. formed by the attraction between two or more elements that transfer electrons known as ions ...
Problem set VI Problem 6.1 Problem 6.2 Problem 6.3 Problem 6.4
... direction, i.e. |Sx , +i. When this beam goes through a Stern-Gerlach apparatus with an inhomogeneous magnetic field in the z-direction (SGz), it splits into two beams of equal intensity, i.e. | h+| Sx , +i |2 = | h−| Sx , +i |2 = ...
... direction, i.e. |Sx , +i. When this beam goes through a Stern-Gerlach apparatus with an inhomogeneous magnetic field in the z-direction (SGz), it splits into two beams of equal intensity, i.e. | h+| Sx , +i |2 = | h−| Sx , +i |2 = ...
Honors Chemistry
... Perform calculations involving wavelength, frequency, energy and the speed of light. Perform calculations involving the DeBroglie equation. Interpret basic line spectra for selected gases. Define the uncertainty principle. Assign electron configurations to atoms and ions. Assign quantum numbers to e ...
... Perform calculations involving wavelength, frequency, energy and the speed of light. Perform calculations involving the DeBroglie equation. Interpret basic line spectra for selected gases. Define the uncertainty principle. Assign electron configurations to atoms and ions. Assign quantum numbers to e ...
Stoichiometry - hrsbstaff.ednet.ns.ca
... describing the composition, bonding, and structural formulas for aliphatic hydrocarbons: alkanes, alkenes, and alkynes (straight, branched, and cyclic, maximum two double or one triple bond) describing the bonding shapes around each of the carbon atoms involved in a single, double, or triple bon ...
... describing the composition, bonding, and structural formulas for aliphatic hydrocarbons: alkanes, alkenes, and alkynes (straight, branched, and cyclic, maximum two double or one triple bond) describing the bonding shapes around each of the carbon atoms involved in a single, double, or triple bon ...
KEY Midterm Exam 1 Sept.14, 1999 Chemistry 211 PAGE 1 0f 5
... where 1 marg = 4.8648 grams (exactly). Their scale of atomic masses is based on the isotope 3 2S (atomic mass on earth = 31.972 g/mole), so they define one "elom" of 3 2S as the amount of sulfur atoms in exactly 32 margs of 3 2S. Furthermore, they define Nor, or "Ordagova's number" (after their well ...
... where 1 marg = 4.8648 grams (exactly). Their scale of atomic masses is based on the isotope 3 2S (atomic mass on earth = 31.972 g/mole), so they define one "elom" of 3 2S as the amount of sulfur atoms in exactly 32 margs of 3 2S. Furthermore, they define Nor, or "Ordagova's number" (after their well ...
Take notes on this document while you are watching the recorded
... 1. The lipids are a large and diverse group of naturally occurring organic compounds that are related by their solubility (will dissolve) in nonpolar5 organic solvents (e.g. ether, chloroform, acetone & benzene) and general insolubility in water (do not dissolve in water - repel water; hydrophobic). ...
... 1. The lipids are a large and diverse group of naturally occurring organic compounds that are related by their solubility (will dissolve) in nonpolar5 organic solvents (e.g. ether, chloroform, acetone & benzene) and general insolubility in water (do not dissolve in water - repel water; hydrophobic). ...
Atomic Structure and Periodicity
... The closer an electron is to the nucleus, the more difficult it is to remove A sodium atom does not have as many valence electrons as a chlorine atom does. 3s electrons are lower in energy than 2p electrons Phosphorus and nitrogen are in the same row of the periodic table They each need one electron ...
... The closer an electron is to the nucleus, the more difficult it is to remove A sodium atom does not have as many valence electrons as a chlorine atom does. 3s electrons are lower in energy than 2p electrons Phosphorus and nitrogen are in the same row of the periodic table They each need one electron ...
answer
... these had the empirical formula PtCl4.4NH3 and when reacted with silver nitrate released two chloride ions per formula unit. Write the structural formula of this compound and write the name of this compound. Ag+ will react with uncoordinated Cl- to form AgCl(s). As it reacts with two Clions per form ...
... these had the empirical formula PtCl4.4NH3 and when reacted with silver nitrate released two chloride ions per formula unit. Write the structural formula of this compound and write the name of this compound. Ag+ will react with uncoordinated Cl- to form AgCl(s). As it reacts with two Clions per form ...
Dalton`s Laws worksheet
... c. why elements are characterized by the mass of their atoms d. why compounds combine in fixed mass ratios in chemical reactions 3. Dalton said that elements are different distinguished from each other by: a. the density of their solid forms b. the shapes of their atoms c. the charge on their ions d ...
... c. why elements are characterized by the mass of their atoms d. why compounds combine in fixed mass ratios in chemical reactions 3. Dalton said that elements are different distinguished from each other by: a. the density of their solid forms b. the shapes of their atoms c. the charge on their ions d ...
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.