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Lecture 38
... The exclusion principle limits the maximum number of electrons in each subshell to 2(2l + 1). ...
... The exclusion principle limits the maximum number of electrons in each subshell to 2(2l + 1). ...
CHAPTER 9 CHEMICAL BONDING I
... The Born-Haber cycle relates lattice energies of ionic compounds to ionization energies, electron affinities, and other atomic and molecular properties. As an example, see the procedure for determining the lattice energy of LiF in Section 9.3 of the text. Lattice energy is based on Coulomb’s law, wh ...
... The Born-Haber cycle relates lattice energies of ionic compounds to ionization energies, electron affinities, and other atomic and molecular properties. As an example, see the procedure for determining the lattice energy of LiF in Section 9.3 of the text. Lattice energy is based on Coulomb’s law, wh ...
PES Topography
... Add much wider functions to describe weakly bound electrons and/or Rydberg states ...
... Add much wider functions to describe weakly bound electrons and/or Rydberg states ...
P1_8 Muonic Atoms - Department of Physics and Astronomy
... quantum mechanical description of the hydrogen atom develops Bohr’s model, where electrons are in bound states described by a wavefunction that satisfies the Schrödinger equation for the hydrogen atom. This article explores what would be the effects if muons replaced electrons in their role in the h ...
... quantum mechanical description of the hydrogen atom develops Bohr’s model, where electrons are in bound states described by a wavefunction that satisfies the Schrödinger equation for the hydrogen atom. This article explores what would be the effects if muons replaced electrons in their role in the h ...
C2 Additional Chemistry Thursday 14 May
... [HT] Draw a diagram to represent bonding in metals. Define a compound Describe the process of making ions to allow ionic bonding to happen Draw the ions made from Group 1 metals Draw the ions made from Group 7 elements Explain why ionic compounds can form giant ionic structures Explain why covalent ...
... [HT] Draw a diagram to represent bonding in metals. Define a compound Describe the process of making ions to allow ionic bonding to happen Draw the ions made from Group 1 metals Draw the ions made from Group 7 elements Explain why ionic compounds can form giant ionic structures Explain why covalent ...
CHEM 120 WEEK 11 LECTURES (INORGANIC WEEK 2) Dr. MD
... Contains only metals, apart from boron. Boron is also the only element which does not form a stable trication (B3+) again will have too high a charge density to be stable. Why do the other elements form tri-cations (M3+ )? Soln. √ Because they have the valence electronic configuration ns2np1 and ...
... Contains only metals, apart from boron. Boron is also the only element which does not form a stable trication (B3+) again will have too high a charge density to be stable. Why do the other elements form tri-cations (M3+ )? Soln. √ Because they have the valence electronic configuration ns2np1 and ...
Lecture 11 - AP Chem Solutions
... compounds containing group 1A ions, nitrate, and ammonium are always soluble. 2) A potassium hydroxide solution is mixed with a solution of zinc nitrate. The potassium ion is always soluble as it is a Group 1A element. Nitrate is also soluble with everything. Thus, K+ and NO3- must be spectator ions ...
... compounds containing group 1A ions, nitrate, and ammonium are always soluble. 2) A potassium hydroxide solution is mixed with a solution of zinc nitrate. The potassium ion is always soluble as it is a Group 1A element. Nitrate is also soluble with everything. Thus, K+ and NO3- must be spectator ions ...
Atomic Concepts
... 17. Noble gases- (fat and happy) stable valence configurations; tend to not bond 18. Hydrogen bonding- H and FON; strong; high melting/boiling points; low vapor pressure 19. Dipole forces- (polar molecules) weak; low melting points, high vapor pressure; soluble in water, conduct as aqueous 20. Nonpo ...
... 17. Noble gases- (fat and happy) stable valence configurations; tend to not bond 18. Hydrogen bonding- H and FON; strong; high melting/boiling points; low vapor pressure 19. Dipole forces- (polar molecules) weak; low melting points, high vapor pressure; soluble in water, conduct as aqueous 20. Nonpo ...
Chemistry
... 9 – 8 Know that chemical reactions can take place at different rates and that reaction rates depend on a variety of factors that influence the frequency of collision of reactant molecules (e.g. shape and surface area of the reacting species, temperature, pressure, the presence or absence of a cataly ...
... 9 – 8 Know that chemical reactions can take place at different rates and that reaction rates depend on a variety of factors that influence the frequency of collision of reactant molecules (e.g. shape and surface area of the reacting species, temperature, pressure, the presence or absence of a cataly ...
Unit 2 Review Questions Fill in the blank In a(n) change, a new
... is a mixture of metals. c. A solid produced when two solutions are mixed together is a(n) ...
... is a mixture of metals. c. A solid produced when two solutions are mixed together is a(n) ...
Observation of the Pairing Gap in a Strongly Interacting Quantum... Fermionic Atoms
... superconductivity and He-3 superfluidity being prominent examples. In an ultracold gas of fermionic atoms, formation and condensation of diatomic molecules have been recently realized. This achievement also opens up a new door to explore the crossover from a molecular Bose-Einstein condensate (BEC) ...
... superconductivity and He-3 superfluidity being prominent examples. In an ultracold gas of fermionic atoms, formation and condensation of diatomic molecules have been recently realized. This achievement also opens up a new door to explore the crossover from a molecular Bose-Einstein condensate (BEC) ...
CH 2 development of atomic theory
... molecules. Each water molecule contains 2 hydrogen atoms and 1 oxygen atom. There would be 2 moles of hydrogen and one mole of oxygen in a mole of water. Therefore, there are 1.2044 X 1024 and 6.022 X 1023 of oxygen in a mole of water. Distinguish between formula unit and molecule, empirical formula ...
... molecules. Each water molecule contains 2 hydrogen atoms and 1 oxygen atom. There would be 2 moles of hydrogen and one mole of oxygen in a mole of water. Therefore, there are 1.2044 X 1024 and 6.022 X 1023 of oxygen in a mole of water. Distinguish between formula unit and molecule, empirical formula ...
Chemistry Reference Table Review
... 65. What is the half-life and decay mode of Rn-222? (1) 1.912 days and alpha decay (2) 1.912 days and beta decay (3) 3.823 days and alpha decay (4) 3.823 days and beta decay 66. Which notation represents an atom of sodium with an atomic number of 11 and a mass number of 24? (1) 24Na (2) 11Na (3) 13 ...
... 65. What is the half-life and decay mode of Rn-222? (1) 1.912 days and alpha decay (2) 1.912 days and beta decay (3) 3.823 days and alpha decay (4) 3.823 days and beta decay 66. Which notation represents an atom of sodium with an atomic number of 11 and a mass number of 24? (1) 24Na (2) 11Na (3) 13 ...
Chemistry Answers - Heathcote School and Science College
... 1 Complete the spaces to create a set of notes about the structure of atoms. Atoms consist of a central nucleus containing protons and neutrons. The nucleus is small compared to the size of the whole atom. The nucleus is surrounded by electrons in energy levels (also called shells). Atoms have no el ...
... 1 Complete the spaces to create a set of notes about the structure of atoms. Atoms consist of a central nucleus containing protons and neutrons. The nucleus is small compared to the size of the whole atom. The nucleus is surrounded by electrons in energy levels (also called shells). Atoms have no el ...
The ocean is a mixture.
... another and to other metals, but their properties do not fit in with those of any other family. Many transition metals combine chemically with oxygen to form compounds called oxides. They have one or two electrons in the outer level Reactivity: less reactive than alkaline-earth metals Properties: Sh ...
... another and to other metals, but their properties do not fit in with those of any other family. Many transition metals combine chemically with oxygen to form compounds called oxides. They have one or two electrons in the outer level Reactivity: less reactive than alkaline-earth metals Properties: Sh ...
Ch. 9
... • The more electronegative element is written last and w/ ide • Use prefixes to tell you the subscript in each • Mono is not written w/ the 1st word of a compound’s name (Ex: CO2) • Prefixes are sometimes shortened to make a name easier to say (Ex: CO is carbon monoxide not mono oxide) • Sometimes u ...
... • The more electronegative element is written last and w/ ide • Use prefixes to tell you the subscript in each • Mono is not written w/ the 1st word of a compound’s name (Ex: CO2) • Prefixes are sometimes shortened to make a name easier to say (Ex: CO is carbon monoxide not mono oxide) • Sometimes u ...
Orbits and Orbitals
... are used under the fair-use provisions of the copyright law, some are mine. Copyright is retained by the owners! ...
... are used under the fair-use provisions of the copyright law, some are mine. Copyright is retained by the owners! ...
One slide per page
... INTERmolecular forces 5) Induced dipole – induced dipole (or Dispersion or London forces) Generally regarded as being weak, but can in fact be very strong for large molecules e.g. benzene and bromine are liquid at RT I2 and S8 are solid at RT The strength of the ...
... INTERmolecular forces 5) Induced dipole – induced dipole (or Dispersion or London forces) Generally regarded as being weak, but can in fact be very strong for large molecules e.g. benzene and bromine are liquid at RT I2 and S8 are solid at RT The strength of the ...
Six slides per page
... The electrons on a molecule are never stationary, nor rigidly held. When a molecule is brought into the vicinity of other charges, the electrons on the molecule will move in response to this charge. The freedom of the electrons to move around is called the “polarizability” of the molecule. Small and ...
... The electrons on a molecule are never stationary, nor rigidly held. When a molecule is brought into the vicinity of other charges, the electrons on the molecule will move in response to this charge. The freedom of the electrons to move around is called the “polarizability” of the molecule. Small and ...
Lecture 9 - ChemWeb (UCC)
... electronic state? Electrons occupy the molecular orbitals, the overall wavefunction of the state is a product of electrons in orbitals. Molecular orbitals of molecules transform as one of the representations of the molecular point group. The symmetry of the state is the product of the symmetry of oc ...
... electronic state? Electrons occupy the molecular orbitals, the overall wavefunction of the state is a product of electrons in orbitals. Molecular orbitals of molecules transform as one of the representations of the molecular point group. The symmetry of the state is the product of the symmetry of oc ...
SCH4U - Unit 1
... The number of protons in the nucleus is called the atomic number. This number determines the identity of an atom. Atoms are electrically neutral; therefore the number of protons in an atom must equal the number of electrons in an atom. For example, oxygen has an atomic number of 8 and has 8 protons ...
... The number of protons in the nucleus is called the atomic number. This number determines the identity of an atom. Atoms are electrically neutral; therefore the number of protons in an atom must equal the number of electrons in an atom. For example, oxygen has an atomic number of 8 and has 8 protons ...
word doc (perfect formatting)
... 4) Represents an atom of an alkali earth metal Questions 5-8 refer to the following descriptions of bonding in different types of solids. a) Lattice of positive and negative ions held together by electrostatic forces b) Closely packed lattice with delocalized electrons throughout giving ability to c ...
... 4) Represents an atom of an alkali earth metal Questions 5-8 refer to the following descriptions of bonding in different types of solids. a) Lattice of positive and negative ions held together by electrostatic forces b) Closely packed lattice with delocalized electrons throughout giving ability to c ...
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.