Periodic Table

Memorize these element names & symbols: Gases: H hydrogen He helium Ne neon N nitrogen O oxygen F fluorine Cl chlorine Ar argon Liquids: Hg mercury Br bromine

Solids: Li lithium B boron C carbon Na sodium Mg magnesium Al aluminum Si silicon P phosphorus S sulfur K potassium Ca calcium Cr chromium Mn manganese Fe iron Co cobalt Ni nickel Sn tin Cu copper Zn zinc Pb lead As arsenic I Iodine Se selenium Ba barium Ag silver Au gold Pt platinum U uranium

Arrangement of the Elements Russian, Dmitri Mendeleev created The first “accepted” periodic table (1800’s) 1) Increasing atomic number 2) By groups or families: columns elements in a column have very similar properties

Ca I Cu 3) periods Rows (across) Identify the element in: Group 2A, period 4 Group 7A, period 5 Group 1 B, period 4 Ca I Cu

4) Metal, Nonmetal, Metalloid nonmetals metalloids Metals

Properties of Metals high melting pt. (not Hg) shiny good conductors of heat & electricity malleable & ductile easily oxidized: lose e- in chem rxns

Properties of Nonmetals low melting pt. (sol, liq, gas) xenon poor conductors solids are brittle & dull gain e- in chem rxns sulfur carbon Reduction (easily reduced))

Properties of Metalloids (either side of zig zag line) Ex: B, Si, Ge, As, Sb not Al properties are intermediate between metal and nonmetal silicon used in semiconductor industry (computer chips)

Quantum Theory revisited 5) Electron Arrangement Quantum Theory revisited Apartment building analogy atom apartment building nucleus ground floor energy levels floors sublevels apartments orbitals rooms electrons people

s p d f types of orbitals (one room apt.) spherical dumbell

Electron Configuration: The “address” of the e- Principal Quantum Number (n) energy level number of sublevels type of sublevels orbitals max number electrons n2 2n2 1 1 1 1s 1 2 2s 2p 4 8 2 2 2 3 3 3 3s 3p 3d 9 18 4 4 4 4s 4p 4d 4f 16 32 Electron Configuration: The “address” of the e- Ex: 1s22s22p6 no. electrons energy level sublevel

Aufbau Diagram 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 Energy level sublevels max. no. e-

1s1 1s2 1s22s1 N 7 e- 1s2 2s2 2p3 sample electron configurations H 1 e- 1s1 He 2e- 1s2 Li 3e- 1s22s1 1s 2s N 7 e- 1s2 2s2 2p3 1s 2s 2p

Fe 26e- 1s2 2s2 2p6 3s2 3p6 4s2 3d6 3p 4s 1s 2s 2p 3s 3d

Sample problem: Given the electron configuration: 1s22s22p63s23p5 1. How many electrons are unpaired? 1 2. How many electrons are in the outermost energy level ? 7 3s23p5 3. How many energy levels and sublevels are occupied? 3 energy levels (1, 2, 3) 5 sublevels (1s 2s 2p 3s 3p) 4. What element has this ground state configuration? Cl

As Given the configuration: 1s22s22p63s23p64s23d104p3 this is the config. of: As How many electrons are in the outer energy level? 5, 4s24p3 3 2. How many electrons are unpaired?

Short method for e- config. Use noble gases Ex: Cl 17 e- [Ne] 3s2 3p5 1st 10 e- [Ne] 1st 18 e- [Ar] Ex: Ba 56e- [Xe] 6s2 1st 36 e- [Kr] Ex: Zn 30 e- [Ar] 4s2 3d10 1st 54 e- [Xe] 1st 86 e- [Rn] U 92 e- [Rn] 7s2 5f4 Si [Ne] 3s23p2 Pd [Kr] 5s2 4d6 14 e- 46 e-

s & p using the periodic table to write electron configurations 1 1s 2 period # (n) 2p 2s 3 period #(n) -1 3s d 3p 4 3d 4s 4p 5 5s 4d 5p 6 6s 5d 6p 7 7s 6d f Period #(n) -2 6 4f 7 5f

Ex: Na [Ne] 3s1 Ex: P [Ne] 3s2 3p3 Ex: Co [Ar] 4s2 3d7 Ex: Sn [Kr] 5s2 4d10 5p2 Ex: Pu [Rn] 7s2 4f6 1. calcium [Ar] 4s2 2. chlorine [Ne] 3s2 3p5 3. cadmium [Kr] 5s2 4d10

Inner transition metals Families of Elements halogens Noble gases Transition metals Alkali metals Alkaline earth metals Inner transition metals

All have 1 valence electron Group 1A: Alkali metals Na Li 1s2 2s1 All have 1 valence electron Na [Ne] 3s1 outer energy level K [Ar] 4s1 Rb most reactive metals always found combined in nature Cs react with water producing hydrogen gas Fr

Also react w/ water to produce hydrogen gas Group 2A: Alkaline Earth Metals Be 1s2 2s2 all have 2 valence electrons Mg [Ne]3s2 Mg Ca [Ar] 4s2 Sr quite reactive; always found combined w/ other elements in nature Ba Ra Also react w/ water to produce hydrogen gas

most reactive nonmetals Cl Group 7A: Halogens F 1s2 2s2 2p5 Cl [Ne] 3s2 3p5 Br all have 7 valence e- [Ar] 4s2 3d10 4p5 I most reactive nonmetals At form salts when combined with metals; ex: NaCl, KI always found in compounds

filled outer levels makes them stable Group 8 A: Noble Gases He 1s2 Xe Ne 1s2 2s2 2p6 most have 8 valence e- Ar [Ne] 3s2 3p6 Kr chemically inert (unreactive); don’t form compounds Xe Rn filled outer levels makes them stable Ar Kr

Au Ag Transition Metals (B groups) unique property: form bright colored compounds “typical” metals

Inner Transition elements many are synthetic (man made) lanthanide series actinides series La Ac many are synthetic (man made) and radioactive “yellow cake” uranium oxide

Change from left to right across the row Periodicity Trend: property that changes atomic radius, ionization energy, electronegativity Group trend change from top to bottom down a group Periodic trend Change from left to right across the row

I. Atomic Radius Indicates the size of an atom Group trend larger down the group more energy levels makes the atoms larger Li: 2 energy levels K: 4 energy levels

Periodic trend smaller across more protons increases nuclear charge; pulls electrons in closer making the atom smaller Li C Ne +3 +6 +10 arrange these atoms from smallest to largest: Sr, Ne, Ca, S, Al Ne S Al Ca Sr

Li K Energy required to remove an e- from an atom III. Ionization Energy Li K Group trend decreases going down larger atoms hold their valence e- more loosely

Increases across; increase in nuclear charge (more p+) causes electrons to be held more tightly Periodic trend Na Al Cl +13 +17 +11 Ex: Which will lose an electron the easiest? K or Ge ? Mg or Ba ? Al or Cs ?

gains e- easily; very reactive Number from 0-4 that indicates an atom’s attraction for e- IV. Electronegativity F 4.0 gains e- easily; very reactive Cs 0.7 loses e-easily; very reactive group trend Increases going across (not noble gases Periodic trend decreases going down Ex: Arrange these atoms from greatest attraction for e- to least: P, Al, Sr, O O, P, Al, Sr

trends summary Smallest radius Highest I.E. Highest EN (F) Lowest EN Lowest I.E. Largest radius