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Reactions of Metals and Their Compounds
Reactions of Metals and Their Compounds

Unit 3 Notes - WordPress.com
Unit 3 Notes - WordPress.com

... a. A maximum of _________ electrons can fit in a single orbital. 3. Main energy levels indicate the general amount of __________________ and ___________________ from the nucleus a given electron in an orbital possesses. a. Each ______________, or period, on the periodic table indicates a main energy ...
valence neutron
valence neutron

... • Recall that an empirical pairing term is included the semi-empirical mass formula to account for their unusual stability. N.B. The pairing term is not accounted for in the shell model, which ignores all interactions between particles!!! • It costs too much energy to break a pair of nucleons and po ...
Rdg: Electron Configuration
Rdg: Electron Configuration

... I. Principle Quantum Number (n) and Sublevels The number of sublevels that an energy level can contain is equal to the principle quantum number of that level. So, for example, the second energy level would have two sublevels, and the third energy level would have three sublevels. The first sublevel ...
lecture notes, page 2
lecture notes, page 2

... Readings for today: Section 1.10 (1.9 in 3rd ed) – Electron Spin, Section 1.11 (1.10 in 3rd ed) – The Electronic Structure of Hydrogen. Read for Lecture #8: Section 1.12 (1.11 in 3rd ed) – Orbital Energies (of many-electron atoms), Section 1.13 (1.12 in 3rd ed) – The Building-Up Principle. ...
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Chapter 5 Electrons in Atoms
Chapter 5 Electrons in Atoms

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Mole Relationships in chemistry
Mole Relationships in chemistry

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Energy and Matter in Chemical Change Science 10
Energy and Matter in Chemical Change Science 10

Ch 2 Sample Exercises PPT
Ch 2 Sample Exercises PPT

Sample Exercise 2.1 Illustrating the Size of an Atom
Sample Exercise 2.1 Illustrating the Size of an Atom

2 is
2 is

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Unit 4 Notes

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Student Text, pp. 650-653
Student Text, pp. 650-653

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hydrogen

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Chapter 42
Chapter 42

Scribed lecture notes 15-849C lecture 1/28/2002 Lecturer: Dave
Scribed lecture notes 15-849C lecture 1/28/2002 Lecturer: Dave

... follows an exponential decay, with the decay rate being faster for higher barriers. One important fact: The figure above shows the electron as having the same energy in the left and right halves of the box. If this is not an allowed state, the electron can tunnel into a state at the right with lower ...
Wave Mechanics
Wave Mechanics

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Ch 8 Bonding and Molecular Structure 06-Nov
Ch 8 Bonding and Molecular Structure 06-Nov

... In the above reactions, nitric acid on the right will give up an H+ to water in an aqueous solution to form the nitrate and a hydronium ion. This is what acids do in aqueous solutions. When not in aqueous solutions, most acids are clear, high boiling point liquids. ...
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Redox

... An area in which effective charges is particularly useful is in understanding the oxidation-reduction reactions of organic compounds In the following reaction, an oxidizing agent is added to a solution of n-propanol, producing propanoic acid. Determine the effective charges of the C atoms in npropan ...
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Detailed Notes CH. 6
Detailed Notes CH. 6

... Students confuse Bohr’s orbits with orbitals; most spellcheckers do not recognize the word “orbital.” Students mistakenly think that spectral lines represent energy levels; consequently . . . Students have difficulties associating a given line in an emission (or absorption) spectrum with a transitio ...
Chapter 4 Section 1 The Development of a New Atomic Model
Chapter 4 Section 1 The Development of a New Atomic Model

... The Hydrogen-Atom Line-Emission Spectrum, continued • When investigators passed electric current through a vacuum tube containing hydrogen gas at low pressure, they observed the emission of a characteristic pinkish glow. • When a narrow beam of the emitted light was shined through a prism, it was se ...
AP Chemistry Summer Work
AP Chemistry Summer Work

Key Words Electronic Homework Problems Questions and Problems
Key Words Electronic Homework Problems Questions and Problems

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Atom

An atom is the smallest constituent unit of ordinary matter that has the properties of a chemical element. Every solid, liquid, gas, and plasma is made up of neutral or ionized atoms. Atoms are very small; typical sizes are around 100 pm (a ten-billionth of a meter, in the short scale). However, atoms do not have well defined boundaries, and there are different ways to define their size which give different but close values.Atoms are small enough that classical physics give noticeably incorrect results. Through the development of physics, atomic models have incorporated quantum principles to better explain and predict the behavior.Every atom is composed of a nucleus and one or more electrons bound to the nucleus. The nucleus is made of one or more protons and typically a similar number of neutrons (none in hydrogen-1). Protons and neutrons are called nucleons. Over 99.94% of the atom's mass is in the nucleus. The protons have a positive electric charge, the electrons have a negative electric charge, and the neutrons have no electric charge. If the number of protons and electrons are equal, that atom is electrically neutral. If an atom has more or fewer electrons than protons, then it has an overall negative or positive charge, respectively, and it is called an ion.Electrons of an atom are attracted to the protons in an atomic nucleus by this electromagnetic force. The protons and neutrons in the nucleus are attracted to each other by a different force, the nuclear force, which is usually stronger than the electromagnetic force repelling the positively charged protons from one another. Under certain circumstances the repelling electromagnetic force becomes stronger than the nuclear force, and nucleons can be ejected from the nucleus, leaving behind a different element: nuclear decay resulting in nuclear transmutation.The number of protons in the nucleus defines to what chemical element the atom belongs: for example, all copper atoms contain 29 protons. The number of neutrons defines the isotope of the element. The number of electrons influences the magnetic properties of an atom. Atoms can attach to one or more other atoms by chemical bonds to form chemical compounds such as molecules. The ability of atoms to associate and dissociate is responsible for most of the physical changes observed in nature, and is the subject of the discipline of chemistry.Not all the matter of the universe is composed of atoms. Dark matter comprises more of the Universe than matter, and is composed not of atoms, but of particles of a currently unknown type.
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