ipc 03a atoms & elements. atomic structure history: john dalton dalton’s atomic theory:...
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IPC 03A Atoms & Elements
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Atomic Structure History:
John DaltonDalton’s Atomic Theory:
• Proposed that elements are _____________________________identical, indivisible particles called ___________________.
• The name “atom” comes from
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J.J. Thomson“Plum Pudding” Model
He said the atom had _____________ (raisins) immersed in a sea of ______________ ____________________(pudding).
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J.J Thomson’s Cathode Ray Tube Experiment:
• He concluded that the _________________ were made up of very small _______________ charged particles, which he named __________
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Ernest Rutherford“Gold Foil” Experiment
Discovered the ________________________ and that the atom is mostly _____________.
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Rutherford’s Expectation(assuming the plum pudding model)
• Rutherford expected ______ ______________ particles to go ______________ the atom like in this picture.
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Rutherford’s Actual Results• Instead, Rutherford
observed that some of the __________ particles bounced _____________; thus, he concluded there was a ________________ ____________________ nucleus.
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Niels Bohr“___________________”
of the Atom
• Nucleus is in the __________.
• Electrons orbit the ____________.
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Erwin Schrodinger“_______________________”
• The ___________ represents the probable ______________ of an __________.
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James ChadwickDiscovered the ____________
• There was still __________ _____________ from the atom.
• Chadwick solved the problem by discovering the final subatomic particle, the __________________.
Jimmy Neutron
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Exposing Scientist’s Contributions
Atomic Theory
John Dalton J.J. Thompson Rutherford J. Chadwick Niels Bohr Schrodinger
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Atoms consist of three main Subatomic Particles
Atomic mass unit (amu) = ___________ the mass of a __________________________.
Protonsp+
Electronse-
Neutronsn0
Mass
Charge
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Structure of The Atom
____________ is small, dense, and _______ ____________ charged.
___________ are located outside the nucleus in an ________ __________
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Forces Within The Atom
• Electromagnetic Forces keep the electrons in _____________around the nucleus. The negatively charged _________________ are _____________ to the positively charged _____________ in the nucleus.
• Strong Nuclear Forces hold the _______________together by opposing the force of _____________ between the positive charged ____________ so the nucleus won’t break apart. Only acts on very short distances.
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Chemical Symbols
• Elements are the simplest pure substance that _______________________ ____________________.
• Chemical symbols are an _________________ of the element’s name.
• The first letter is ALWAYS ____________ and the second letter is ALWAYS __________!
Element Symbol Origin
Copper Cu Cuprium
Gold Au Aurium
Iron Fe Ferrium
Lead Pb Plumbum
Potassium K Kalium
Silver Ag Argentum
Sodium Na Natrium
Tin Sn Stannum
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An Element- contains one type of atom with a unique number of ______________________.
o The _________________ determines the element.o Ex: Carbon has ____ protons.
o If you _____________ the # of protons, you change the _____________________.o Ex: Nitrogen has ____ protons.
Neutral Atoms have the __________ # of electrons as protons. Ex: neutral Carbon has 6 ________ and 6 ________
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Element Notation• Mass Number (M) –
–Found in the ______________ and makes of up _______ of the atom’s ___________ (99.99%).
• Atomic Number (A) - number of _____________________–Determines the ____________.
XM
A
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Example: Carbon-12
1) What is the atomic number of Carbon?
2) What is the mass number of Carbon?
C12
6
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IsotopesAtoms with the
Same _____________________(same atomic #) Different _______________________________ Different ______________________________
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Sodium Isotopes
1) Atomic number?2) Mass number?3) No. of Neutrons?
4) Atomic number?5) Mass number?6) No of Neutrons?
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Hydrogen Isotopes
• Hydrogen-1• (______________)
• Hydrogen-2• (_______________)
• Hydrogen-3• (______________)
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Hydrogen IsotopesFill in the #protons, #electrons, & #neutrons:
Mass number No. of protons
No. of electrons
No. of neutrons
Hydrogen-1
Hydrogen-2
Hydrogen-3
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Atomic Mass – is the _______________________ of all the element’s natural ________________The most common isotope will have a ________ __________________ of the atomic mass rounded to a ____________________number.
Atomic number =
Atomic Mass =The most common isotope of
silver is ______________.
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Mendeleev’s Periodic Table
• Dimitri Mendeleev – organized information about all the known elements by
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Groups & Periods
• Groups (Families) have similar properties and go down on the periodic table. There are
• Periods go across on the periodic table. There are
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Identify the element in:
Group 2 (IIA), period 4
Group 17 (VIIA), period 5
Group 11, period 4
Look at the Periodic Table:
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Metals, Nonmetals, & Metalloids
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Properties of metals and nonmetals • Metalloids have
both metallic and nonmetallic characteristics –along the staircase.
• Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Astatine
Metals Nonmetals
Luster (shiny silver-gray, gold, copper)
___________________ (all different colors)
Malleable (hammered)
Ductile (drawn into thin wire)
__________Melting Points _________Melting Points
____________Conductors of heat & electricity
_________ Conductors of heat & electricity
________________ electrons ____________ electrons
Silicon is used in computer chips because conduct electricity (metals) yet insulate (nonmetals).
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Energy Levels in an Atom
• Electrons occupy ________ around the _________.
• Each energy level can hold up to ____ electrons where n = the _____________
• The farther away an electron is, the higher the energy it possesses.
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Electrons in Energy Levels
1. What is the most common isotope?
2. How many protons?
3. How many electrons?
4. How many neutrons?
5. How many electrons in the 1st energy level?
6. How many electrons in the 2nd energy level?
7. How many electrons in the 3rd energy level?
Cl35.45
17
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Absorption of Energy
The __________________ absorbs enough __________________ causing the electron to be _________________ and “_____________” to a _____________________________energy level.
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Emission of Energy• The electron
_______________when it falls back to its ___________ _______________ energy level (ground state) in the form of _________ ________________
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Atomic Emission Spectrum (hydrogen)
Each line in the spectrum results from a different ____________ ____________
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Emission Spectrum:
Iron (more e-)
Carbon (less e-)
Continuous Spectrum
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Valence Electrons
• Electrons in the ________ energy level
• Electrons used to form ________ _______
Group # of Valence Electrons
1A (1)
2A (2)
3A (13)
4A (14)
5A (15)
6A (16)
7A (17)
8A (18)
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Octet Rule• In order to become most _______, all atoms
need 8 valence electrons in the outermost energy level.
• ______ ______ already have 8 valence electrons which is why they are _______.
• Other elements _____ or _____ electrons by forming chemical bonds in order to have 8 ________ _______ in the outermost energy level.
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Oxidation Numbers• _____ generally ____
electrons to become more stable.– ______ form ______
ions (charged atoms)
• _________ generally _____ electrons to become more stable.– _________ form
_______ ions (charged atoms)
Group Oxidation #
1A (1)
2A (2)
3A (13)
4A (14)
5A (15)
6A (16)
7A (17)
8A (18)