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Quantum chemistry

Bob Jones PPT Notes -- Chapter 5b

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Chemistry
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ion
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Periodic Trends 1 Sizes of Atoms Increase from top to bottom on the periodic table Why? There are higher energy levels, and electrons are farther from the nucleus. Atomic Radii Sizes of Atoms Decrease from left to right on the periodic table Why? There are more protons in the nucleus attracting more electrons (electrostatic attraction). Atomic Radii Atomic Radii 4 p. 113 of Chemistry textbook (BJU Press) Question Why do atoms get larger as you go down the periodic table? They are heavier. They are less dense. Electrons are further from the nucleus. Electrons are bigger. 5 (Comparing the size of an atom to that of its ion, not going across or up the table) Sizes of Atoms Ionic Radii Sizes of Atoms Atoms that lose outer electrons have smaller positive ions (metals).

Bob Jones PPT Notes -- Chapter 4b

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Chemistry
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Block
Aufbau principle
Quantum number
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The Electron Structure of the Atom The quantum model emphasizes the wave nature of electrons. The Quantum Model Quantum numbers are solutions to the wave equations of electrons. Scientists use a set of 4 quantum numbers to determine an electron?s location around an atom. Quantum Numbers Electrons exist in principal energy levels that correspond to Bohr?s orbits: 1, 2, 3, 4, 5, ? Principal energy levels are divided into 4 types of sublevels: s, p, d, and f. Where are the Electrons? The sublevels contain orbitals. Each orbital can hold up to two electrons. Where are the Electrons? Identifies the principal energy level Correlates to Bohr?s orbits n = 1, 2, 3, 4, 5, 6, or 7 for the ground state e?. The total number of e? in a level is 2n2. Principal Quantum Number (n) Level Total # e? 1

Chemistry The central science Summary Chapter

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Quantum chemistry
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electron
Lewis structure
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Lewis Symbols As a pictorial understanding of where the electrons are in an atom, we represent the electrons as dots around the symbol for the element. The number of electrons available for bonding are indicated by unpaired dots. These symbols are called Lewis symbols. Place the electrons on four sides of a square around the element symbol.
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Chemistry The central science Summary Chapter 9

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Molecular orbital
Orbital hybridisation
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VSEPR theory
Antibonding
Lewis structure
Valence bond theory
Unpaired electron
molecular geometry
Technology

Chapter 9- Molecular Geometry and Bonding Theories 9.1 Molecular Shapes Lewis structures give atomic connectivity: they tell us which atoms are physically connected to which atoms. Whenever two atoms or ions are strongly attached to each other we say there is a chemical bond. Three general types of chemical bonds: ionic , covalent and metallic. We will encounter 11 basic molecular shapes: The shape of a molecule is determined by its bond angles. Bond angles The angles made by the lines joining the nuclei of the atoms in a molecule Consider CCl4: Experimentally we find all Cl?C?Cl bond angles are 109.5?. Valence Shell Electron Pair Repulsion (VSEPR) model.

Chemistry The central science Summary Chapter 6

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electron configuration
electron
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Energy level
Technology

Hot Objects and the Quantization of Energy Heated solids emit radiation (blackbody radiation) The wavelength distribution depends on the temperature (i.e., ?red hot? objects are cooler than ?white hot? objects). In 1900 Max Planck solved the problem He investigated black body radiation. He proposed that energy can only be absorbed or released from atoms in ?chucks? of some minimum size . These amounts are called quanta. A quantum (meaning ?fixed amount?) is the smallest amount of energy that can be emitted or absorbed as electromagnetic radiation. The relationship between energy and frequency is: . The Photoelectric Effect and Photons The photoelectric effect provides evidence for the particle nature of light and for quantization.

Chapter 7

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Aufbau principle
Technology

Claire Rafson Chapter 7: Atomic Structure and Periodicity 7.1- 7.3 Wavelength and frequency are inversely related C= speed of light = 2.9979 X 10^8 m/s Photoelectric effect- Einstein. Phenomenon in which electrons are emitted from the surgace of a metal when light strikes it. E=mc^2 ?. M= mass Dual nature of light Diffraction- light is scattered from a regular array of points or lines. Change in E= hv 7.4- quantum model- made by Bohr. Model for the hydrogen atom. Electron in a hydrogen atom moves around the nucleus only in certain orbits. Ground state- lowest possible energy state. 7.5- quantum mechanical model- Heisenberg, Broglie, and Schrodinger probability distribution- intensity of color is used to indicate probability value near a given point in space. 7.6-

Chapter 8 Solutions

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Valence electron
electron configuration
Atomic orbital
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electron
Technology

Periodic Properties of the Elements Review Questions 8.1 A periodic property is one that is predictable based on the element's position within the periodic table. 8.2 The relative size of the sodium and potassium ions is important to nerve signal transmission. The pumps and channels within cell membranes are so sensitive that they can distinguish between the sizes of these two ions and selectively allow only one or the other to pass. The movement of ions is the basis for the transmission of nerve signals in the brain and throughout the body. 8.3 The first attempt to organize the elements according to similarities in their properties was made by the German chemist Johann Dobereiner. He grouped elements into triads; three ele-

Chapter 8 Test Banks

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electron configuration
Valence electron
Effective nuclear charge
Paramagnetism
Quantum number
Technology

? Chemistry: A Molecular Approach (Tro) ? Chapter 8 ?? Periodic Properties of the Elements ? 1) ?? Give the ground state electron configuration for Se. ? A) ?? [Ar]4s23d104p4 ? B) ?? [Ar]4s24d104p4 ? C) ?? [Ar]4s23d104p6 ? D) ?? [Ar]4s23d10 ? E) ?? [Ar]3d104p4 ? Answer: ?? A ? 2) ?? Give the ground state electron configuration for I. ? A) ?? [Kr]5s24d105p6 ? B) ?? [Kr]5s24d105p5 ? C) ?? [Kr]4d105p6 ? D) ?? [Kr]5s25p6 ? E) ?? [Kr]5s25d105p6 ? Answer: ?? B ? 3) ?? Give the ground state electron configuration for Sr. ? A) ?? [Kr]5s24d2 ? B) ?? [Kr]5s24d105p2 ? C) ?? [Kr]5s2 ? D) ?? [Kr]5s25d105p2 ? E) ?? [Kr]5s24d10 ? Answer: ?? C ? 4) ?? Give the ground state electron configuration for Pb. ? A) ?? [Xe]6s26p2 ? B) ?? [Xe]6s25d106p2 ? C) ?? [Xe]6s25f146d106p2 ? D) ??

APBIOLOGY

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Biology
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Proton
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#AP Bio #CampbellBiology #Chapter 1 #Quiz

Chapter?1 Introduction:?Themes?in?the?Study?of?Life Multiple-Choice?Questions 1) Which?of?the?following?properties?or?processes?do?we?associate?with?living?things? A) evolutionary?adaptations B) energy?processing C) responding?to?the?environments D) growth?and?reproduction E) all?of?the?above Answer: E Topic: Overview Skill: Knowledge/Application 2) Which?of?the?following?is?not?a?theme?that?unifies?biology? A) interaction?with?the?environment B) emergent?properties C) evolution D) reductionism E) structure?and?function Answer: D Topic: Concept?1.1 Skill: Knowledge/Application 3) Which?of?the?following?sequences?represents?the?hierarchy?of?biological?organization?from?the?least?to?the?most complex?level? A) organelle,?tissue,?biosphere,?ecosystem,?population,?organism

APBIOLOGY

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#AP Bio #CampbellBiology #Chapter 1 #Quiz

Chapter?1 Introduction:?Themes?in?the?Study?of?Life Multiple-Choice?Questions 1) Which?of?the?following?properties?or?processes?do?we?associate?with?living?things? A) evolutionary?adaptations B) energy?processing C) responding?to?the?environments D) growth?and?reproduction E) all?of?the?above Answer: E Topic: Overview Skill: Knowledge/Application 2) Which?of?the?following?is?not?a?theme?that?unifies?biology? A) interaction?with?the?environment B) emergent?properties C) evolution D) reductionism E) structure?and?function Answer: D Topic: Concept?1.1 Skill: Knowledge/Application 3) Which?of?the?following?sequences?represents?the?hierarchy?of?biological?organization?from?the?least?to?the?most complex?level? A) organelle,?tissue,?biosphere,?ecosystem,?population,?organism

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