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Semester 1 Final Exam Study Guide
Semester 1 Final Exam Study Guide

... Br-81 ...
Electron Configuration Class Notes
Electron Configuration Class Notes

Student - Davison Chemistry Website
Student - Davison Chemistry Website

Ch. 4-2 PowerPoint
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... behave as both a particle and a wave. What about electrons?  Louis De Broglie stated that electrons could be considered waves confined to a space around an atomic nucleus. ...
Chemical Bond - Cobb Learning
Chemical Bond - Cobb Learning

The Periodic table
The Periodic table

... The Energy of an electron:  In 1926 Schrodinger showed that laws of quantum mechanics could be used to characterize the motion of electrons.  A quantized property is a property that can have only certain values.  The energy of an electron is quantized, only certain behavior patterns are allowed. ...
Grade 11 Chemistry E.. - hrsbstaff.ednet.ns.ca
Grade 11 Chemistry E.. - hrsbstaff.ednet.ns.ca

Arrangement of Electrons in Atoms
Arrangement of Electrons in Atoms

... Pass a current through gas at low pressure it excites the atoms Ground state: lowest energy state of an atom Excited state: atom has higher potential energy than it has in ground state ...
CHAPTER 6 PRACTICE TEST Name Relevant Equations E = hν E
CHAPTER 6 PRACTICE TEST Name Relevant Equations E = hν E

... 10. Which of the following represents the ground state electron configuration for the Mn2+ ion? (A) [Ar] 3d5 (B) [Ar] 3d44s1 (C) [Ar] 3d34s2 (D) [Ar] 3d54s2 (E) [Ar] 3d74s2 ...
Quantum Numbers, Orbitals, Electron Configurations, Periodic Trends
Quantum Numbers, Orbitals, Electron Configurations, Periodic Trends

... Convert the numbers is questions 1a – 1d into scientific notation. a) c) b) d) Convert the following numbers that are in scientific notation into decimal form. a) 1.2340 × 107 d) 7.0 × 104 b) 3.980 × 102 e) 5.00134 × 10-4 c) 9.23 × 10-5 f) 6.626 × 10-34 A box measures 2.56 in × 4.21 in × 12.00 in. W ...
Quantum Numbers, Orbitals, Electron Configurations, Periodic Trends
Quantum Numbers, Orbitals, Electron Configurations, Periodic Trends

... Convert the numbers is questions 1a – 1d into scientific notation. a) c) b) d) Convert the following numbers that are in scientific notation into decimal form. a) 1.2340 × 107 d) 7.0 × 104 b) 3.980 × 102 e) 5.00134 × 10-4 c) 9.23 × 10-5 f) 6.626 × 10-34 A box measures 2.56 in × 4.21 in × 12.00 in. W ...
Atomic Structure - River Dell Regional School District
Atomic Structure - River Dell Regional School District

Lecture 4
Lecture 4

... Note on spectroscopic notations (they are actually used). There are letters associated with values of orbital angular momentum. The first few are: For example, state with n=1 l=0 is referred to as 1s, n=2 l=0 is referred to as 2s, n=2 l=1 is referred to as 2p, and so on. While the energies are the s ...
LIST OF TOPICS COVERED DURING THIS COURSE
LIST OF TOPICS COVERED DURING THIS COURSE

... The following should serve as a checklist for your notebook. The topics below include all topics that have been covered this semester and are testable on your final exam. These topics should be studied from a variety of source including inclass notes, homework questions, lab questions, assignments, ...
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H CH 4 Homework

... 6. Distinguish between the ground state and the excited state. Ground state is the initial state of the electron. Excited state is after it absorbs energy 7. According to Bohr, how is a line spectrum produced. Electron falls from the excited state and emits a photon 8. What is the major difference b ...
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Worksheet Key - UCSB C.L.A.S.

Honors Chemistry
Honors Chemistry

... returns to the ground state? 14. What are the 4 sublevels of orbitals that can determine the shape of the orbitals? 15. In order to give an electron an address it must be a given a quantum number with 4 different parts. What are these 4 numbers? 16. Write the electron configurations for the followin ...
Chapter 37 Early Quantum Theory and Models of the Atom
Chapter 37 Early Quantum Theory and Models of the Atom

... Experimenting with cathode rays in 1897, J.J. Thomson had discovered negatively charged 'corpuscles', as he called them, with a charge to mass ratio 1840 times that of a hydrogen ion. In 1913, Robert A. Millikan measured the charge of an electron, one of the fundamental physical constants. His exper ...
Final Exam Chemistry B2A Mr. Kimball`s Class 2003
Final Exam Chemistry B2A Mr. Kimball`s Class 2003

Ch. 5 Electrons in Atoms
Ch. 5 Electrons in Atoms

... unique shade of light generated by a certain element passes thru a prism and is separated into different freq it contains - Again, Bohr could explain Hydrogen with a single electron, but not the complexities of more electrons - As a particle. - Almost exclusively as a wave ...
FYS 3520-Midterm2014
FYS 3520-Midterm2014

... c) Fission decay. Discuss why the fission decay problem differs from that of neutron and gamma decay. d) Fission to neutron competition. Why are 235U, 233U and 239Pu fissile when hit by thermal neutron, while 238U and 232Th are not? e) Draw by hand the dependence of the fission cross section vs ener ...
Unit 1: Kinematics - Pre University Courses
Unit 1: Kinematics - Pre University Courses

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Lecture 2

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Worksheet

... READING GUIDE: 5.1 – Revising the Atomic Model (p. 128-133) Atomic Theory and Electrons 1) Summarize the contributions of each of the following individuals to our understanding of the atom and atomic structure (you may have to look back into CH 4 for the first 3…or the summary on page 133). Include ...
Tutorial 3 - answers • Complete the following table, giving either the
Tutorial 3 - answers • Complete the following table, giving either the

... All second ionisations energies are > first ionisation energies as an electron is being removed from an already positive ion. The value for Na will be very high as the electron is taken from a core (n=2) shell. There will be a general increase in second ionisation energy from Mg to Ar. ...
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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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