How Atoms Differ Objectives Covered in this Presentation: 7. Locate the three fundamental particles...
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Transcript of How Atoms Differ Objectives Covered in this Presentation: 7. Locate the three fundamental particles...
How Atoms DifferHow Atoms DifferObjectives Covered in this Presentation:Objectives Covered in this Presentation:
7. Locate the three fundamental particles in the atom; 7. Locate the three fundamental particles in the atom; indicate the relative mass and charge of these particles. indicate the relative mass and charge of these particles. 8. Indicate what the atomic number and mass number of an 8. Indicate what the atomic number and mass number of an atom represent. atom represent. 9. Calculate the mass number when given the number of 9. Calculate the mass number when given the number of protons and neutrons. protons and neutrons. 10. Indicate which isotope is used as the standard for atomic 10. Indicate which isotope is used as the standard for atomic mass. mass. 11. Write the nuclear symbol for an atom. 11. Write the nuclear symbol for an atom. 12. Determine the number of protons, neutrons, and 12. Determine the number of protons, neutrons, and electrons when given the atomic number and mass number. electrons when given the atomic number and mass number. 13. Calculate average atomic mass from relative abundance. 13. Calculate average atomic mass from relative abundance. 14. Define isotope and identify which nuclides are isotopes 14. Define isotope and identify which nuclides are isotopes of the same element when given the atomic number and of the same element when given the atomic number and mass number of these nuclides. mass number of these nuclides.
Atomic structureAtomic structure
ProtonsProtons: positive particles in nucleus: positive particles in nucleus
NeutronsNeutrons: particle with no charge in the : particle with no charge in the nucleusnucleus
ElectronElectron: particle with negative charge : particle with negative charge orbiting the nucleus orbiting the nucleus
Subatomic Subatomic particlesparticles
QuarksQuarks: make up protons and neutrons : make up protons and neutrons
Six types: up, down, strange, charm, Six types: up, down, strange, charm, truth (top) and beauty (bottom)truth (top) and beauty (bottom)
((I am not making up those names, I am not making up those names, nuclear physicists can be weirdnuclear physicists can be weird.).)
Subatomic Particles Subatomic Particles (Cont)(Cont)
Other subatomic particles include Other subatomic particles include leptons, neutrino, tau, muon etc. leptons, neutrino, tau, muon etc.
Atomic SymbolsAtomic SymbolsSI symbols used internationally.SI symbols used internationally.
Based on Greek, Latin, a person’s Based on Greek, Latin, a person’s name, or location discovered.name, or location discovered.
Examples: Iron <Latin Ferrum>: FeExamples: Iron <Latin Ferrum>: Fe
Silver <Latin Argentum>: AgSilver <Latin Argentum>: Ag
Atomic SymbolsAtomic Symbols
11stst letter capitalized letter capitalized
22ndnd and 3 and 3rdrd letter lower case letter lower case
MUST be printed in traditional lettersMUST be printed in traditional letters
NO cursive NO cursive
Aluminum: Al not Aluminum: Al not AlAl
Cobalt: Co not CO or coCobalt: Co not CO or co
Atomic NumberAtomic Number
Equal to the number of protonsEqual to the number of protons
The number of protons for an element The number of protons for an element nevernever changes changes
Atomic NumberAtomic Number
In a In a stablestable atom, the number of atom, the number of protons = electronsprotons = electrons
The positive and negative charges are The positive and negative charges are equal and the overall charge is neutralequal and the overall charge is neutral
Nuclear ChargeNuclear Charge
If electrons are gained, the number of If electrons are gained, the number of electrons is greater than the number electrons is greater than the number
of protons and the charge is of protons and the charge is ____________________
Electric ChargeElectric Charge
If electrons are lost, the number of If electrons are lost, the number of electrons is less than the number of electrons is less than the number of
protons and the charge is protons and the charge is ____________________
Atomic MassAtomic Mass
May be noted as mass weight, or May be noted as mass weight, or atomic weightatomic weight
Equals: protons + neutronsEquals: protons + neutrons
Atomic MassAtomic Mass
Each proton and each neutron have Each proton and each neutron have an atomic mass of 1 amu. (Atomic an atomic mass of 1 amu. (Atomic mass units).mass units).
Electrons are so tiny (.00005 amu) Electrons are so tiny (.00005 amu) that their mass is negligible.that their mass is negligible.
Atomic Mass is an Atomic Mass is an AverageAverage
Remember: the number of protons for Remember: the number of protons for any element does not changeany element does not change
The number of neutrons does vary.The number of neutrons does vary.
Example: All carbon atoms have 6 Example: All carbon atoms have 6 protons. Most carbon atoms has 6 protons. Most carbon atoms has 6 neutrons, but very few have 8.neutrons, but very few have 8.
6P + 6N = 12 amu6P + 6N = 12 amu
6P + 8N = 14 amu6P + 8N = 14 amu
If you have 9 carbon atoms with 12 If you have 9 carbon atoms with 12 amu and 1 carbon atom with 14 amu, amu and 1 carbon atom with 14 amu, what is the average amu?what is the average amu?
If you have 9 carbon atoms with 12 If you have 9 carbon atoms with 12 amu and 1 with 14 amu, what is the amu and 1 with 14 amu, what is the
average amu?average amu?
9 atoms X 12 amu = 1089 atoms X 12 amu = 108
1 atom X 14 amu = 141 atom X 14 amu = 14
108 + 14 = 122108 + 14 = 122
122/10 =12.2 amu122/10 =12.2 amu
IsotopesIsotopes: atoms of the same element : atoms of the same element with different numbers of neutrons with different numbers of neutrons and slightly different amu.and slightly different amu.
The greater the number of protons for The greater the number of protons for an element, the greater the number of an element, the greater the number of isotopes.isotopes.
Periodic Table History:Periodic Table History: 1869 1869 Mendeleev created 1Mendeleev created 1stst Periodic Table. Periodic Table. He arranged it by atomic mass and He arranged it by atomic mass and successfully predicted unknown successfully predicted unknown elements.elements.
Modern Periodic Table: Modern Periodic Table:
Arranged by atomic numberArranged by atomic number
List element nameList element name
Element symbolElement symbol
Atomic numberAtomic number
Atomic massAtomic mass
PeriodsPeriods: (rows) all elements in the row : (rows) all elements in the row have the same number of energy have the same number of energy levelslevels
FamiliesFamilies: (column) have the same : (column) have the same number of valence electrons and number of valence electrons and oxidation state.oxidation state.
Valence electrons:Valence electrons: number of number of electrons in the outer most energy electrons in the outer most energy levellevel
Oxidation stateOxidation state: number of electrons : number of electrons needed to be gained or lost to have 8. needed to be gained or lost to have 8.
Using the periodic tableUsing the periodic table
Protons = atomic numberProtons = atomic number
Electrons = ?Electrons = ?