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Atomic Structure
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Atomic Structure Atomic Number = Number of Protons or Electrons
Atomic Weight = Number of protons and the number of Neutrons Example Magnesium Atomic Number = 12 Atomic Weight = AMU or grams/mole
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Atomic Structure Elemental Name Atomic Number Abbreviation Weight
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Atomic Model Concept Democritus (465 BC) Greek Philosopher
Matter is made up of discrete particles, can not be divided infinitely First to use the term atomas (Atom)
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Atomic Model Concept John Dalton (1766-1844) English school teacher
Developed the first Atomic Model Differentiated atoms based on mass Atoms can not be changed but can combine to form compounds
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Thompson Model J.J. Thompson (1856-1940)
Experimented with Cathode rays and magnetism Identified negatively charged particles in elements Particles were called electrons
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A02119MV CATHODE RAY TUBE
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Rutherford Model Ernest Rutherford (1871-1931)
Alpha particles were deflected when passing through a gold foil. The Positively charged proton was identified as the reason. Determined that the Atom is mostly empty space.
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Gold Foil Experiment
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a02120mu
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Chadwick Model James Chadwick (1891-1974)
Atoms were more massive than could be explained Needed additional weight without effecting the charge. Identified Neutrons as the additional component.
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Quarks and Leptons Two currently recognized groups of fundamental particles, which are subatomic and indivisible Represent the smallest known units of matter Six quarks and six leptons are the basic building blocks for everything in the universe.
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Bohr’s Model Niels Bohr (1885-1962)
Utilized the science of spectroscopy Determined that electrons could only exist in definite energy levels.
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Devised the Solar System Model
Bohr’s Model Devised the Solar System Model
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Quantum Model Werner Heisenberg (1901-1976)
Bohr’s model only worked well for atoms with one electron. The laws of motion did not account for the movements of all electrons Determined a rationale to explain and describe their movements.
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The Heisenberg Uncertainty Principle!
Quantum Model The Heisenberg Uncertainty Principle! It is impossible to know both the energy and exact position of an electron at the same time
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Quantum Model This replaced Bohr’s precise orbits with three dimensional regions of probable positions. A orbital then became a map of where the electron is most likely to be at any given time Electrons exist in energy levels
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Quantum Model For the first 112 elements there are only 7 possible energy levels that can be identified or determined.
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Electron Cloud Model
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Quantum Model Subdivides all but the first principle energy level into sublevels The sublevels contain other divisions called orbitals The orbitals contain electrons
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s p d f Quantum Model There are four sublevels
They are identified by the letters s p d f
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Energy level Sublevels
2 sp 3 spd 4 spdf 5 spdf 6 spd 7 sp
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Different Sub-levels F D P S
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Quantum Model The s sublevel is the simplest of all and only contains one orbital which can hold two electrons. The s sublevel is found in all levels An orbital can not contain more than two electrons
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Sublevels Total Electron Capacity
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Quantum Model The p sub level contains only three orbitals which can hold two electrons each. This sub level can contain a maximum of six electrons
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Sub Electrons s p
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Quantum Model The d sublevel contains five orbitals which can hold two electrons each. This sub level can contain a maximum of ten electrons
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Sub Electrons s p d
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Quantum Model The f sublevel contains seven orbitals which can hold two electrons each. This sub level can contain a maximum of fourteen electrons
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Sub Electrons s p d f
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4th and 5th Energy Levels F D P S
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Quantum Model The quantum model is only a mathematical picture of something we can not see. It describes something in terms we can understand and help account for some of the properties of electrons.
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Energy level Sublevels Electron Total
sp 8 spd 18 spdf 32 spdf 32 6 spd 18 7 sp 8
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Quantum Model Sublevels can also be ranked according to energy
The further a sub level is away from the nucleus the more energy it has. There is a filing order that can be used to understand energy levels
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Quantum Model Some levels overlap
Because of this, part of a higher level may have a slightly lower energy capability than the one underneath it.
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d sub level probability cloud
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Filling Order Energy level (1-7)
3d __ p __ 3p __ s__ n=4 3s __ n=3 2p __ 2s __ Increasing energy 1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p
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1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p Filling Order
Energy level (1-7) 1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p 2s 2p 3s 3p 4s 3d
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Increasing energy 1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p
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Quantum Model Worksheet Room Filling order per Hotel Management
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p Guests Per Floor Room 6d Room 6s Room 6p Energy Level 6 Room 5d Room 5f Energy Level 5 Room 5s Room 5p Room 4d Room 4f Room 4s Room 4p Energy Level 4 Room 3d Room 3s Room 3p Energy Level 3 Room 2s Room 2p Energy Level 2 Energy Level 1 Room 1s Element: __________ Atomic Number: ____ Atomic Weight: ______ Number of Protons: ____ Number of Electrons: _____ Number of Neutrons: ____
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Quantum Model Practice
How many electrons can a d sublevel hold? 10
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Quantum Model Practice
How many electrons can a d orbital hold? 2
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Quantum Model Practice
What type of sublevel is found in all principle energy levels? s
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Quantum Model Practice
Which of the following orbitals is the highest in energy? ( 2s, 3d, 4s) 3d
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Quantum Model Worksheet Room Filling order per Hotel Management
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p Guests Per Floor Room 6d Room 6s Room 6p Energy Level 6 Room 5d Room 5f Energy Level 5 Room 5s Room 5p Room 4d Room 4f Room 4s Room 4p Energy Level 4 Room 3d Room 3s Room 3p Energy Level 3 Room 2s Room 2p Energy Level 2 Energy Level 1 Room 1s Element: __________ Atomic Number: ____ Atomic Weight: ______ Number of Protons: ____ Number of Electrons: _____ Number of Neutrons: ____
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Electron Configuration
Arrangement of electrons Example – Li 1s22s1
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Element: __________ Atomic Number: ____ Atomic Weight: ______
Electron Configuration 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p Element: __________ Atomic Number: ____ Atomic Weight: ______ Number of Protons: ____ Number of Electrons: _____ Number of Neutrons: ____
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(start with the smallest and work up)
Aufbau Principle The arrangements of electrons in an atom may be determined by the addition of electrons to a smaller atom. (start with the smallest and work up)
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Aufbau Principle This means that each successive element has one additional proton and one additional electron. As a rule electrons fill the least energetic orbital possible.
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Orbital notation Picture of the electron configuration 1s H ___ H 1s1
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Orbital notation He 1s2 Picture of the electron configuration He ___
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Aufbau Principle When two electrons have filled up a sub-level they move in opposite directions from each other. This is known as “spin” ___
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Hund’s Rule States that when electrons fill a sublevel, all orbitals receive one electron before any receive two Examples: Carbon, Oxygen
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Carbon (6) Electron configuration 1s 2s 2p
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Carbon (6) Orbital notation 1s 2s 2p ___ ____ ___ ___ ___
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Oxygen (8) Electron configuration 1s 2s 2p
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Oxygen (8) Orbital notation 1s 2s 2p ___ ____ ___ ___ ___
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Titanium (22) ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p 3s 3p 4s 3d 4p 1s 2s 2p s 3p ___ ___ ___ ___ ___ ___ ___ ___ ___ 4s 3d p ___ ___ ___ ___ ___ ___ ___ ___ ___
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Arsenic (33) ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p 3s 3p 4s 3d 4p 1s 2s 2p s 3p ___ ___ ___ ___ ___ ___ ___ ___ ___ 4s 3d p ___ ___ ___ ___ ___ ___ ___ ___ ___
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Quantum Numbers Quantum numbers describe the location and energy levels of electrons. They are a zip code for the location of electrons based on four different aspects of the electron position
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Quantum Number First Position
The energy level from 1-7 in which the electron is located N = main energy level Example: N2 (energy level 2)
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Quantum Number Second Position
The sub-level in which the electron is located (s-f) L = sub-level s = p = d = f = 3 Example: (N2,L1)
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Quantum Number Third Position
The position within the sub-level based on the available positions peculiar to each. M = Orbital value ( 0 or +/-) p ____ ____ ____ = Example: (N2,L1,M-1)
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Quantum Number Fourth Position The Spin of the electron
S = Spin ( +1/2 or - 1/2) p ____ ____ ____ = + 1/2 Example: N2,L1,M-1,S+1/ or (2,1,-1,+1/2)
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Quantum Number Practice
What is the quantum number for this electrons position? Second energy level, p sub-level, middle orbit, positive spin. (2,1,0,+1/2)
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Quantum Number Practice
What is the quantum number for this electrons position? Third energy level, d sub-level, first orbit, negative spin. (3,2,-2,-1/2)
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Quantum Number Practice
What is the quantum number for this electrons position? Fifth energy level, f sub-level, sixth orbit, negative spin. (5,3,2,-1/2)
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Quantum Number Practice
1s 2s 2p 3s 3p 4s 3d 4p 1s 2s 2p s 3p ___ ___ ___ ___ ___ ___ ___ ___ ___ 4s 3d p ___ ___ ___ ___ ___ ___ ___ ___ ___
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Quiz A Quiz B Element 1 – Lithium Element 2 - Sulfur
Element 1 – Sodium Element 2 -Oxygen
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Shorthand Notation Ne 1s2 2s2 2p6 Mg 1s2 2s2 2p6 3s2 Mg [Ne] 3s2
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Shorthand Notation Ti [Ar] Ar 1s2 2s2 2p6 3s23p6
Ti 1s2 2s2 2p6 3s23p6 4s23d2 Ti [Ar]
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Where does the Filling Order come from?
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p
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1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p D block = N - 1 F block = N - 2
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Atomic Particles
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Atomic Mass Atomic mass is the average mass of all naturally occurring forms of that element. Atomic Mass is measured in “Atomic Mass Units” or AMU AMU Unit = (1/12 of carbon atom) AMU of Arsenic (As) = 74.92
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(Atomic Number = protons /electrons)
Atomic Mass Atomic Mass Number is the number of particles in the atom (protons + neutrons) Atomic Number is their specific ID based on number of protons or electrons (Atomic Number = protons /electrons)
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Atomic Mass Element AMU Mass # Atomic # H 1.008 1 1 C 12.01 12 6
Na
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Isotopes Atoms of the same element always have the same number of protons Some atoms of the same element can have different number of neutrons, these are called isotopes. Isotopes have a different mass number. (AMU=protons + neutrons)
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Isotopic Notation Describes the exact composition of an atom. Example:
Boron Boron AMU = AMU=12 B B
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Isotopic Notation Boron Boron Isotope 11 12 5 5 AMU = 11 AMU=12
AMU = AMU=12 Protons = Protons = 5 Neutrons = Neutrons = 7 B B
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Isotopic Notation Practice
Bromine Bromine AMU = AMU= Protons = Protons = Neutrons = Neutrons = Br Br
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Isotopic Notation Practice
Bromine Bromine AMU = AMU=86 Protons = Protons = 35 Neutrons = Neutrons = 51 Br Br
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Isotopic Notation Practice
Barium Barium AMU = AMU= Protons = Protons = Neutrons = Neutrons = Ba Ba
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Isotopic Notation Practice
Barium Barium AMU = AMU=145 Protons = Protons = 56 Neutrons = Neutrons = 89 Ba Ba
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Isotopic Notation Practice
Nickel Nickel AMU = AMU= Protons = Protons = Neutrons = Neutrons = Ni Ni
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Isotopic Notation Practice
Nickel Nickel Isotope AMU = AMU=145 Protons = Protons = 28 Neutrons = Neutrons = 117 Ni Ni
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Valence Electrons The electrons in the outermost energy level are the ones most likely to be involved in chemical bonding. They are what give elements their physical properties. These electrons are known as the valence electrons.
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Valence Electrons 1s2 2s2 2p6 3s23p6 Example : Argon (Ar)
Electron Structure by energy (2,8,8) Electron configuration Valence Electrons = 8 1s2 2s2 2p6 3s23p6
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Valence Electrons 1s2 2s2 2p6 3s23p3 Example : Phosphorus(P)
Electron Structure by energy (2,8,5) Electron configuration Valence Electrons = 5 1s2 2s2 2p6 3s23p3
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Electron Dot Symbols Valence electrons determine how atoms bond
Electron Dot symbol is a short hand way of representing atoms.
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Electron Dot Symbols
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Na Electron Dot Symbols Sodium (Na)
Electron Structure by Energy = (2,8,1) Valence Electrons = 1 Na
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Al Electron Dot Symbols Aluminum (Al)
Electron Structure by Energy = (2,8,3) Valence Electrons = 3 Al
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Cl Electron Dot Symbols Chlorine (Cl)
Electron Structure by Energy = (2,8,7) Valence Electrons = 7 Cl
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O Electron Dot Symbols Oxygen (O) Electron Structure by Energy = (2,6)
Valence Electrons = 6 O
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O Electron Dot Symbols Orbital notation ___ ____ ___ ___ ___ . . . . .
1s 2s 2p ___ ____ ___ ___ ___ O . . . . . .
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Ionic Charges Electrons can be lost, gained or shared during chemical bonding. This process can cause the charge of an atom to become unbalanced either positively or negatively. The atom does not lose its identity because the number of protons is the same.
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Ionic Charges An atom in its normal state is neutral in charge.
Atoms that lose an electron become positively charge ( + or cation ) Atoms that gain an electron become negatively charged. (- or anion)
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Na - 1 electron = Na Na 1+ Ionic Charge Sodium (Na)
Electron Structure by Energy = (2,8,1) Valence Electrons = 1 Na electron = Na Na 1+ Positive Ion (cation) .
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Electron Dot Symbols Fluorine (F) Electron Structure by Energy = (2,7)
Valence Electrons = 7 F electron = F F -1 Negative Ion (anion) . . . . . . . . . . . . . . .
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Flame test A flame test is a procedure used in chemistry to detect the presence of certain elements, primarily metal ions, based on each elements characteristic emission spectrum. The test involves introducing a sample of the element or compound to a hot, non-luminous flame, and observing the color that results.
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Flame Color An atom consists of a nucleus with electrons orbiting around it. The electrons location is based on the filling order (Quantum theory). Each orbit or shell has an occupancy limit and no more than that number can be there. 1s2 2s2 2p6 3s23p3
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Flame Color Electrons have a tendency to be as close to the nucleus as they can, because that is a lower energy state. The farther from the nucleus, the more energy the electron must have.
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Flame Color If an atom is "zapped" by some kind of energy ( e.g. heat, electric discharge, electromagnetic radiation), One or more electrons may pick up enough energy to be knocked into a more distant, and more energetic, shell.
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Flame Color After a short interval the electron drops back into a lower shell. When it returns to a lower shell it now has too much energy.
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Flame Color This surplus is emitted in the form of a photon - a tiny particle of light
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Properties of Light Visible light is a form of electromagnetic radiation. This radiation exhibits wave like behavior as it travels through space. The speed of light is 3.00 x 108 meters/second
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Properties of Light
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Flame Color The color of the light (i.e. its wavelength) is determined by the difference in energy levels of the two shells between which the electron fell. Because electrons can be knocked out of more than one shell, and they can be bumped up by more than just one level 4s
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Flame Color They also can return to their original level in one big transition, or in several stages. 4s
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Flame Color The end result is that an element which is excited produces light of a number of colors. The exact mix of colors is characteristic of that element and serves to identify it. The mix is called the spectrum of that element.
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1. Copper acetate 2. Copper 3. Potassium iodide 4. Magnesium 5. Iron 6. Lithium carbonate 7. Strontium nitrate 8. Sodium chloride Green flame Blue-green flame Violet flame White sparks Yellow sparks Blue flame Red flame Yellow flame
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Is this a physical or chemical change?
Flame Color Is this a physical or chemical change? 1s 1s 1s 2s 1s 2s 2s Protons = 3 Electrons = 3 Protons = 3 Electrons = 3 Protons = 3 Electrons = 3
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Quiz Quiz A Quiz B Mg (12) Ca (20) P (15)) N (7) As (33) Se (34)
Ar (18) P (15) K (19) Quiz B Ca (20) P (15)) Se (34) Cl (17) O (8) Sr (38)
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Quantum Number Practice
Third energy level, d sub-level, first orbit, negative spin. Fifth energy level, f sub-level, sixth orbit, negative spin. Fourth energy level, p sublevel, central orbit, positive spin.
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Quantum Number Practice
Third energy level, d sub-level, first orbit, negative spin. (3,2,-2,-1/2) Fifth energy level, f sub-level, sixth orbit, negative spin. (5,3,2,-1/2) Fourth energy level, p sublevel, central orbit, positive spin (4, 1,0,+1/2)
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You conduct an experiment twice to confirm the density of an object
You conduct an experiment twice to confirm the density of an object. The mass of the object is 3.00 x 103 grams. The volume of displacement of the object you weighed is listed below for each experiment. Determine the observed density from both your experiments as well as the percent error if the actual density is suppose to be 1.58 x 102 grams/liter. A B 1.01 x 101 liters x 101 liters x 101 liters x 101 liters
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Perform the following operation using bridge unit Analysis and Scientific notation.
What is the average acceleration of an object that travels x 103 meters in x 105 seconds. Provide the answer in Kilometers. speed = dist / time Acc = speed / time B What is the average acceleration of an object that travels x 102 meters in 2.31 x 106 seconds. Provide the answer in Kilometers. speed = dist / time Acc = speed / time
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Assignment Atomic Number, Atomic weight, protons, neutrons, electrons.
Isoptic Notation Electron Configuration Orbital Notation Valence number Dot structure
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Quiz A Element 1= Sodium (11) Element 2 = Oxygen (8) Quiz B Element 1 = Beryllium (4) Element 2 = Sulfur (16)
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Filtration Lab Problem: How do you separate salt from sand?
Hypothesis: If I dissolve the salt in water then I can filter it and separate it from the sand. Design: Mix salt and sand Dissolve salt with water Filter the water Evaporate the water Measure the salt and compare results
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Filtration Lab Data: Started with one gram of salt Retrieved 0.75 grams of salt 25% error in experiment Conclusion: The process of separating the salt from sand using water to dissolve it was successful. Additional water was most likely needed needed to dissolve the salt in this experiment and improve the amount retrieved. Reference: Chapter _____ page ____ of the Prentice Hall Chemistry text book.
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Module 4 Test Uncertainty Principle Hunds Rule, Aufbau Principle
Electron Configuration Orbital notation Isoptic Notation Electron Dot Structure Scientists (know primary contribution) Rutherford, Dalton, Chadwick, Heisenberg, Bohr, Thompson, Democritus Honors – Quantum Number, shorthand notation
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Physical or Chemical Change Lab
Problem: Determine if a physical or chemical change occurs. Hypothesis: If the color changes and heat is given off or taken in, the weight changes and/or the pH changes than a chemical change has occurred. Design: Check the pH of the acid Check the color of the acid with reagent Combine with Sodium Bicarbonate Evaluate the color, pH, weight and temperature
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Physical or Chemical Change Lab
Data: Conclusion: Reference: Chapter _____ page ____ of the Prentice Hall Chemistry text book.
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