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How to read about the atoms
The Periodic Table How to read about the atoms
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Reading the Periodic Table
Atomic Number Atomic Symbol Name Atomic Mass
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Practice Ba Barium 137.33 56 C Carbon 12.01 6 O Oxygen 16.00 8 N
Element Symbol Element Name Atomic Mass Atomic Number Ba Barium 137.33 56 C Carbon 12.01 6 O Oxygen 16.00 8 N Nitrogen 14.01 7
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Atomic Number Li 3 3 3 Ar 18 18 18 S 16 16 16 Argon Sulfur Lithium
Tells us how many protons are in the atom Identifying mark of an atom In a neutral atom tells us the amount of electrons! Atomic Symbol Atomic Name Atomic Number # of Protons # of Electrons Li 3 3 3 Lithium Ar Argon 18 18 18 S 16 16 16 Sulfur
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Atomic Mass Cu 63.55 29 35 Ti 47.87 22 26 Es 252 99 153 Copper
Tells us the mass of one atom Most of the mass is in the nucleus Therefore mass = protons + neutrons Atomic Symbol Atomic Name Atomic Mass # of Protons # of Neutrons Cu Copper 63.55 29 35 Ti 47.87 22 26 Titanium Es 252 99 153 Einsteinium
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Practice! Fe Li Ne Iron 26 55.85 26 26 30 Lithium 3 6.94 3 3 4 Neon 10
Element Symbol Element Name Atomic Number Atomic Mass # of Protons # of Electrons # of Neutrons Fe Li Ne Iron 26 55.85 26 26 30 Lithium 3 6.94 3 3 4 Neon 10 20.18 10 10 10
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IONS Cations – atoms with a positive charge Anions – atoms with a negative charge Atom Symbol Atom Name Atomic Number # of Protons # of Electrons Charge Ti N Ca Titanium 22 22 20 +2 Nitrogen 7 7 3 +4 Calcium 20 20 18 +2 Nitrogen 7 7 10 -3
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Practice! W At Er 74 74 74 110 Astatine 85 210 85 85 125 Erbium 68 68
Element Symbol Element Name Atomic Number Atomic Mass # of Protons # of Electrons # of Neutrons W At Er Tungsten 74 183.85 74 74 110 Astatine 85 210 85 85 125 Erbium 68 167.26 68 68 99
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Isotopes A variance in the type of atom Protons stay the same
Neutrons are different!!!
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The Periodic Table
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Alkali Metals Group IA atoms
Highly reactive with the Halogens and Gases Usually form +1 ions 1 valence electron Shiny and Lustrous Exothermic with water Contain S Orbital
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Alkaline Earth Metals Group IIA atoms
Highly reactive with the Halogens and Gases Usually form +2 ions 2 valence electrons Shiny, lustrous, and oxidizes easily Denser than Alkali Contain S Orbital
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Halogens Group VIIA Very reactive Usually form -1 anion
7 valence electrons Very similar properties Only family to change phases as you go down
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Noble Gases Group VIIIA Non-reactive Monoatomic gases Full P orbital
8 valence electrons Similar properties Have brilliant colors when “excited”
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Metaloids Group IIIA – VIIIA Contain P Orbital
Can form anions or cations Have properties of non-metals and metals Used in many circuit board technologies
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Nonmetals Group IIIA – VIIIA Contain S and P Orbital
Referred to as non-metals because they are mostly anions (negative charges) Found in all phases naturally Make up most organic compounds
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Transition Metals +3 +2 +1 Groups IB - VIIIB Hard metallic solids
Most dense atoms Contains D orbital Form multiple cations Three exceptions +3 +2 +1
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Lanthanides and Actinides
Contains 4th orbital F that is “buried” Includes many man made atoms Nearly all are radioactive React readily with high temperature All typically for +3 ions (cations) Used with nuclear energy
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The Periodic Table
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Periodic Trends Energy Levels Sublevels Orbitals
The periodic table can be read as a system of trends What are three trends you already know? Energy Levels Sublevels Orbitals
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Atomic Size
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Atomic Size Size DECREASES going ACROSS the periodic table
Atom size can be read on the periodic table via 2 ways Size DECREASES going ACROSS the periodic table Size INCREASES going DOWN the periodic table
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Atomic Size INCREASE in PROTONS equals an INCREASE in POSITIVE charge
INCREASE in ELECTRONS equals an INCREASE in SHIELDING EFFECT Shielding effect is the effect of inner shell electrons to shield the positive charge of the nucleus from outer shell electrons
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Ionization Energy
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Ionization Energy Energy required to remove an electron from an atom
INCREASES going ACROSS the periodic table DECREASES going DOWN the periodic table INCREASES the closer the electron is to the NUCLEUS ( = what kind of charge?)
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Ionic Radius
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Ionic Radius Radius of an atom changes with loss or gain of electrons
For Cations – Radius DECREASES due to greater pull from the NUCLEUS For Anions – Radius INCREASES due to greater pull from the ELECTRONS
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Electronegativity
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Electronegativity The ability of an atom to attract electrons
INCREASES going ACROSS the periodic table DECREASES going DOWN the periodic table The higher the ionization energy the higher the electronegativity!
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A Deadly Trend
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Radioactivity Marie Curie coined the phrase radioactivity after observing fogging from emitted particles and waves Radiation is particles or waves released by an unstable atom Three types: Alpha α : positive charge, Helium nucleus Beta β : negative charge, electron Gamma γ : no charge, wavelength
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Summary of Trends Atomic Size Decreases Ionic Size Increase
Electronegativity Increases Ionization Energy Increases Radioactivity Increases Atomic Size Increases Ionic Size Increases Electronegativity Decreases Ionization Energy Decreases Radioactivity Increases
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The Periodic Table
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Sublevels and orbitals
Where the electrons live
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Energy Level > Sublevel > Orbital > Electrons
What is an orbital Electrons stay in the electron cloud A good approximation of where the electrons are and how they behave Lower the level, lower the energy Everything is based on a neutral atom that has a full outer energy level We call those electrons Valence Shell Electrons Energy Level > Sublevel > Orbital > Electrons
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Orbitals A region of space around the nucleus where an electron is likely to be found Often found in pairs (2) with opposite spin Energy Level Number of Orbitals Max number of Electrons 1 1 (s) 2 4 (s,p) 8 3 9 (s,p,d) 18 4 16 (s,p,d,f) 32 5 6 7
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Orbitals 2 electrons 6 electrons 10 electrons 14 electrons
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Electron Configuration
Atoms can be mapped based on their electrons! S = the period number = energy level P = the period number = energy level D = the period number – 1 = energy level F = the period number – 2 = energy level Remember the number of electrons for each orbital!!!
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Electron Configuration
Energy Level 1s1 Number of Electrons Na 3s1 3p4 S 4d1 K 5f3 U Sublevel
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Electron Configuration
1s1 1s2 2s1 2s2 2p1 2p2 2p3 2p4 2p5 2p6 3s1 3s2 3p1 3p2 3p3 3p4 3p5 3p6 4s1 4s2 3d1 3d2 3d3 3d4 3d5 3d6 3d7 3d8 3d9 3d10 4p1 4p2 4p3 4p4 4p5 4p6 5s1 5s2 4d1 4d2 4d3 4d4 4d5 4d6 4d7 4d8 4d9 4d10 5p1 5p2 5p3 5p4 5p5 5p6 6s1 6s2 5d1 5d2 5d3 5d4 5d5 5d6 5d7 5d8 5d9 5d10 6p1 6p2 6p3 6p4 6p5 6p6 7s1 7s2 6d1 6d2 6d3 6d4 6d5 6d6 6d7 6d8 6d9 6d10 7p1 7p2 7p3 7p4 7p5 7p6 4f1 4f2 4f3 4f4 4f5 4f6 4f7 4f8 4f9 4f10 4f11 4f12 4f13 4f14 5f1 5f2 5f3 5f4 5f5 5f6 5f7 5f8 5f9 5f10 5f11 5f12 5f13 5f14 Electron Configuration
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Practice time 1s22s1 = 1s22s22p63s1 = 1s22s22p63s23p3 =
1s22s22p63s23p64s1 = 1s22s22p63s23p64s23d8 = 1s22s22p63s23p64s23d104p5= Li Na P K Ni Br
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Practice time N = Cl = Co = Ag = Pb = Cf = 1s22s22p3 1s22s22p63s23p5
1s22s22p63s23p64s23d7 1s22s22p63s23p64s23d104p65s24d9 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f9
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Noble gas notation [Ne]3s1 = [Ne]3s23p3 = [Ar]4s1 = [Ar]4s23d8 =
Just like regular notation, just start with a noble gas to save writing! [Ne]3s1 = [Ne]3s23p3 = [Ar]4s1 = [Ar]4s23d8 = [Ar]4s23d104p5= Na P K Ni Br
![Noble gas notation [Ne]3s1 = [Ne]3s23p3 = [Ar]4s1 = [Ar]4s23d8 =](http://slideplayer.com/slide/12778466/77/images/43/Noble+gas+notation+%5BNe%5D3s1+%3D+%5BNe%5D3s23p3+%3D+%5BAr%5D4s1+%3D+%5BAr%5D4s23d8+%3D.jpg "Just like regular notation, just start with a noble gas to save writing! [Ne]3s1 = [Ne]3s23p3 = [Ar]4s1 = [Ar]4s23d8 = [Ar]4s23d104p5= Na. P. K. Ni. Br.")
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The Periodic Table
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S electrons P electrons Example 1s2 2s2 2p6 3s2 Ar 3p6
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S electrons P electrons D Electrons Example V
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Are these Atoms the same?
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Lets talk energy
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Lewis Dot diagram Diagram that illustrates the valence shell electrons
Used for S and P orbitals D and F are not valence electrons resulting in inaccurate representation of the bonding potential Shows potential bonding of atoms
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? Lewis Dot Diagram 1 4 2 1 2 5 3 6 Column Number IA IIA IIIA IVA VA
VIA VIIA VIIIA Valence Electrons 1 2 3 4 5 6 7 8
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K H F Li S C Lewis Dot diagram Column IA Column IA Column VIIA
Column VIA Column IVA Column Number IA IIA IIIA IVA VA VIA VIIA VIIIA Valence Electrons 1 2 3 4 5 6 7 8
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Group Pop Quiz Carbon Fluorine Magnesium Aluminum Sulfur
Draw the electron configuration, Bohr Model, Energy Diagram, and Lewis Dot diagram for the following atoms: Carbon Fluorine Magnesium Aluminum Sulfur
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