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History of Chemistry Early models of the atom • Democritus- early Greek philosopher • matter made up of tiny indivisible particles called atoms • Dalton- “1st modern atomic theory” 5 Parts to theory 1) All elements made of tiny particles called atoms. 2) Atoms of same element are identical; 3)different atom = different element 4) Atoms bind together in simple whole number ratios. H2O 2:1 correct H1.25O 1.25:1 incorrect (2:1 ratio) 2 H + O H2O (2:2 ratio) 2 H + 2 O H2O2 5)Chemical reactions join or rearrange atoms But atoms can not change into another element Structure of Atom: J.J. Thomson- Plum Pudding Model Or chocolate chip cookie Electron- J.J. Thomson used cathode ray tube to discover electrons, e- have a negative charge Structure of Atom: Proton- positively charged subatomic particle Goldstein- P+ mass 1840 times larger than e- mass Neutron- neutral charged subatomic particle - Discovered by Chadwick - Mass of proton = mass of neutron Rutherford- discovered atoms have a nucleus that e- orbit Rutherford Performed Gold Foil Experiment Shot alpha particles (+ charge) from radioactive lead through gold foil He expected it to go through b/c heavy mass and fast But Some bounced back Concluded it had a dense center called it nucleus Nucleus is most dense has protons & neutrons Almost all atoms mass located in nucleus Mendeleev • Created the first periodic table • Observed when elements are arranged in order of increasing atomic mass then chemical and physical properties appear at regular intervals Based on atomic mass Based on atomic number • The Periodic Table Mendeleev- Arranged by increasing atomic mass, left blank spaces, able to predict properties of missing elements b/c properties repeated • Moseley- arranged in order of increasing atomic number, the one we use today Periodic Law- elements in increasing atomic number will have a periodic repetition of physical & chemical properties Atoms Atomic Number- # protons in nucleus Atoms are electrically neutral so #p = #e Protons = electrons Atoms Mass Number = #p + #n = mass # number of protons + number of neutrons = mass number If given Mass # and proton # you can figure out #of neutrons Mass # - #p = #n Atoms • Shorthand: Mass # Symbol # Protons 1 H 1 4 He 2 figure out for Carbon Atoms 12 C 6 Atoms • Isotope- same # p, different # n; so different mass 1 2 H 1 H 1 3 H 1 • Problems: – Fill in the chart: Element Mass # Be 9 Atomic # # # # Protons Electrons Neutrons 4 20 Na 23 10 11 15 16 • Problems: – Fill in the chart: Element Mass # Atomic # # # # Protons Electrons Neutrons Be 9 4 4 4 5 Ne 20 10 10 10 10 Na 23 11 11 11 12 P 31 15 15 15 16 • Warm up Problems: – Fill in the chart: Element Mass # Mg 24 Atomic # # # # Protons Electrons Neutrons 12 32 K 39 16 19 32 41 • Warm up Answer: – Fill in the chart: Element Mass # Atomic # # # # Protons Electrons Neutrons Mg 24 12 12 12 12 S 32 16 16 16 16 K 39 19 19 19 20 Ge 73 32 32 32 41 3 Main Groups of Elements on PT (Periodic Table) MetalsNon-Metals Metalloids 1 IA 1 18 VIIIA 2 IIA 13 IIIA 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 14 IVA 15 VA 16 VIA 17 VIIA 3 Main Groups of Elements on PT (Periodic Table) Metalso Left side of PT o 80% elements o Conduct electricity o Luster o Ductile o Malleable o Mostly solids w/ some exceptions o 1A Alkali metals o 2A Alkaline Earth Metals o Group B- Transition & Inner Transition Metals 1 IA 1 2 IIA 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 Metals 11 IB 12 IIB 18 VIIIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA o o o o o o o NonmetalsRight side of PT Don’t conduct electricity Aren’t ductile or malleable Can be solids, liquids or gases No luster 7A- Halogens 0- Noble gases 1 IA 1 18 VIIIA 2 IIA 13 IIIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 4 5 6 Metalloidso Border Stair Step o Properties of metals & nonmetals o Used in solar cells & computer chips 7 10 11 IB 12 IIB 14 IVA 15 VA 16 VIA 17 VIIA THE PERIODIC TABLE • The rows across the elements in the periodic table are called periods 1-7 • The columns down are called groups. • groups numbered 1 to 18 or 1A-8A 1 1 IA 1 H Periodic Table 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 1.00797 2 3 3 4 Li Be 6.939 9.0122 11 Na 12 Mg 5 B 5 6 19 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB Ca Sc Ti 22 23 39.102 40.08 44.956 47.90 50.942 37 Rb 38 Sr 39 Y 40 Zr 41 Nb Mo Tc 85.47 87.62 88.905 91.22 92.906 95.94 [99] 55 56 57 72 73 74 75 Ba 21 La 132.905 137.34 138.91 7 87 88 8 O 9 F 8 9 VIIIB 10 11 IB 12 IIB 13 Al 14 Si 15 P 16 S 17 Cl 26.9815 28.086 30.9738 32.064 35.453 K Cs 20 7 N He 4.0026 10 Ne 10.811 12.0112 14.0067 15.9994 18.9984 20.179 22.9898 24.305 4 6 C 18 VIIIA 2 89 Hf V Ta 24 Cr 104 Ra Ac Ku [223] [226] [227] [260] 105 26 Fe 27 Co 51.996 54.9380 55.847 58.9332 42 W 178.49 180.948 183.85 Fr 25 Mn 106 43 44 Ru 45 Rh 101.07 102.905 76 77 Re Os Ir 186.2 190.2 192.2 107 108 109 28 29 30 31 32 33 Ni Cu Zn Ga Ge 58.71 63.54 65.37 65.37 72.59 74.9216 46 47 48 49 Pd Ag Cd In 106.4 107.870 112.40 114.82 78 Pt 79 Au 80 Hg 81 Tl 195.09 196.967 200.59 204.37 50 Sn As 51 Sb 118.69 121.75 82 Pb 83 Bi 207.19 208.980 34 35 18 Ar 39.948 36 Se Br Kr 78.96 79.909 83.80 52 53 Te I 54 Xe 127.60 126.904 131.30 84 85 86 Po At Rn [210] [210] [222] GROUPS or Families • Group 1(1A) are found on the far left side and are called the alkali metals • Group 2(2A) are found on the far left side and are called the alkaline metals • Group 7A(17) are found at the right hand side and are called the halogens. • Group 8A(18) are called the noble gases GROUP 7- halogens are all non- metals they are:-Fluorine,Chlorine,Bromine,Iodine • They have low melting points (this means that the change from a solid to a liquid at a low temperature) • They do not conduct electricity • They go around as pairs of atoms. • We call them diatomic molecules • We write them like this • Fluorine - F2 • Chlorine - Cl2 • Bromine - Br2 • Iodine - I2 What are they like? • • • • Fluorine is a very pale yellow gas Chlorine is a green gas Bromine is a dark red brown liquid Iodine is a black shiny solid THE REACTIONS OF THE HALOGENS • The halogens like to take •The like reactions to take parthalogens in chemical part in chemical reactions • The react with metals to •The react with metals to make salts make salts ••The Themost mostreactive reactivehalogen is fluorine and is halogen fluorine and the least the least reactive is reactive is iodine. iodine. •They get less reactive •as They getdown less the reactive you go groupas you go down the group most reactive Least reactive Uses of the halogens • Iodine is used as an antiseptic • Chlorine is used in swimming pools to kill bacteria • Fluorine is used in tooth paste • Bromine is used photographic film How much does an atom weigh? • Amu- (atomic mass unit) = 1/12 C-12 atom • How many protons in C? • How many neutrons in C? • Atomic Mass of C? • Amu- (atomic mass unit) = 1/12 C-12 atom • How many protons in C = 6 • How many neutrons in C = 6 • Atomic Mass of C =12 • Therefore 1/12th of a C atom is = • to 1 proton • Or = to 1 neutron Relative Atomic Mass 1 p = 1 amu 1 n = 1 amu 1 e- = 0 amu Therefore one carbon atom weighs 12 amu’s © Addison-Wesley Publishing Company, Inc. Isotopes- same # protons different # neutrons 6 3 7 3 Li 0.00000 amu Li 6 3 7 3 Li lithium - 6 0.00000 amu lithium - 7 Li Li-6 = 6.0 amu 6.0 amu Li-7 = 7.0 amu 7.0 amu Isotopes Carbon-12 vs. Carbon-14 © Addison-Wesley Publishing Company, Inc. Isotopes • Chlorine-37 – atomic #: 17 – mass #: 37 – # of protons: 17 – # of electrons: 17 – # of neutrons: 20 37 17 Cl Mass # • mass # = protons + neutrons • always a whole number • NOT on Periodic Table! • Nuclear symbol: Mass # Atomic # 12 6 C Average Atomic Mass • weighted average of all isotopes • on the Periodic Table • round to 2 decimal places • Average atomic mass- is mass on PT -Based on natural abundance of isotopes 1. Change % to decimal 2. Multiply decimal by the mass 3. Add the numbers together • Average atomic mass- is mass on PT -Based on natural abundance of isotopes 1)Change % to decimal 2)Multiply decimal by the mass 3)Add the numbers together Element X has two isotopes. The isotope with a mass of 10.012 amu has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%. Calculate the atomic mass of this element. • Average atomic mass- is mass on PT -Based on natural abundance of isotopes 1)Change % to decimal .1991 and .8009 2)Multiply decimal by the mass 3)Add the numbers together Element X has two isotopes. The isotope with a mass of 10.012 amu has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%. Calculate the atomic mass of this element. • Average atomic mass- is mass on PT -Based on natural abundance of isotopes 1)Change % to decimal .1991 and .8009 2)Multiply decimal by the mass .1991x10.012 = 1.993 .8009 x 11.009=8.817 3)Add the numbers together Element X has two isotopes. The isotope with a mass of 10.012 amu has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%. Calculate the atomic mass of this element. • Average atomic mass- is mass on PT -Based on natural abundance of isotopes 1)Change % to decimal .1991 and .8009 2)Multiply decimal by the mass .1991x10.012 = 1.993 .8009 x 11.009=8.817 3)Add the numbers together 10.810 amu Element X has two isotopes. The isotope with a mass of 10.012 amu has a relative abundance of 19.91%. The isotope with a mass of 11.009 amu has a relative abundance of 80.09%. Calculate the atomic mass of this element. Average atomic mass [Worksheet] • Based on abundance of isotopes 1)Change % to decimal 2)Multiply decimal by the mass 3)Add the numbers together 50.54% of naturally occurring isotopes of bromine have an atomic mass of 78.92 amu. While the other 49.46% of isotopes of bromine have an atomic mass of 80.92amu. Calculate the average atomic mass of bromine. Average atomic mass • Based on abundance of isotopes 1)Change % to decimal .5054 and .4946 2)Multiply decimal by the mass 3)Add the numbers together 50.54% of naturally occurring isotopes of bromine have an atomic mass of 78.92 amu. While the other 49.46% of isotopes of bromine have an atomic mass of 80.92amu. Calculate the average atomic mass of bromine. Average atomic mass • Based on abundance of isotopes 1)Change % to decimal .5054 and .4946 2)Multiply decimal by the mass .5054x78.92= 39.89 .4946 x 80.92= 40.02 3)Add the numbers together 50.54% of naturally occurring isotopes of bromine have an atomic mass of 78.92 amu. While the other 49.46% of isotopes of bromine have an atomic mass of 80.92amu. Calculate the average atomic mass of bromine. Average atomic mass • Based on abundance of isotopes 1)Change % to decimal .5054 and .4946 2)Multiply decimal by the mass .5054x78.92= 39.89 .4946 x 80.92= 40.02 3)Add the numbers together 39.89 + 40.02 = 79.91 50.54% of naturally occurring isotopes of bromine have an atomic mass of 78.92 amu. While the other 49.46% of isotopes of bromine have an atomic mass of 80.92amu. Calculate the average atomic mass of bromine. Average Atomic Mass • Calculate avg. atomic mass of oxygen if abundance is 99.76% 16O, 0.04% 17O, and 0.20% 18O. .9976 x 16 = 15.96 .0004 x 17 = 0.00068 16.00 .002 x 18 = 0.036 amu 16.00 Average Atomic Mass • EX: Find chlorine’s average atomic mass if approximately 8 of every 10 atoms are chlorine35 and 2 are chlorine-37. • • • • 8/10 = .80 2/10 = .20 .80 x 35 = 28.0 .2 x 37 = 7.4 35.4 35.40 amu • Warm up Answer: – Fill in the chart: Element Mass # Atomic # # # # Protons Electrons Neutrons Mg 24 12 12 12 12 S 32 16 16 16 16 K 39 19 19 19 20 Ge 73 32 32 32 41 Dmitri Mendeleev (1869) In 1869 Mendeleev and Lothar Meyer (Germany) published nearly identical classification schemes for elements known to date. The periodic table is base on the similarity of properties and reactivities exhibited by certain elements. Later, Henri Moseley ( England,1887-1915) established that each elements has a unique atomic number, which is how the current periodic table is organized. http://www.chem.msu.su/eng/misc/mendeleev/welcome.html The Periodic Table • A map of the building block of matter. 1 1 IA 1 H Periodic Table 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 17 VIIA 1.00797 2 3 Li 4 5 Be B 6.939 9.0122 3 11 Na 12 Mg 19 K 20 Ca 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 6 37 38 21 Sc 22 Ti 23 V 24 Cr 25 Mn 39 43 Sr Mo Tc [99] 56 57 La 72 Hf Nb 42 87.62 88.905 91.22 92.906 95.94 Ba Zr 41 Rb 55 Y 40 85.47 Cs 73 Ta 74 W 75 Re 132.905 137.34 138.91 178.49 180.948 183.85 186.2 7 87 88 8 O 9 F 4.0026 10 Ne 11 IB 12 IIB 13 Al 14 Si 15 P 16 S 17 Cl 18 Ar 26.9815 28.086 30.9738 32.064 35.453 39.948 26 Fe 27 Co 28 Ni 39.102 40.08 44.956 47.90 50.942 51.996 54.9380 55.847 58.9332 58.71 5 7 N He 10.811 12.0112 14.0067 15.9994 18.9984 20.179 22.9898 24.305 4 6 C 18 VIIIA 2 89 104 Fr Ra Ac Ku [223] [226] [227] [260] 105 106 107 44 Ru 45 Rh 46 Pd 29 30 31 32 33 Ge 63.54 65.37 65.37 72.59 74.9216 78.96 79.909 83.80 47 48 49 Ag Cd In Sn Sb 52 Te Br 36 Ga 51 Se 35 Zn 50 As 34 Cu 53 I Kr 54 Xe 101.07 102.905 106.4 107.870 112.40 114.82 118.69 121.75 127.60 126.904 131.30 76 Os 190.2 108 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 192.2 195.09 196.967 200.59 204.37 207.19 208.980 [210] 109 85 86 At Rn [210] [222] http://www.chemsoc.org/viselements/pages/periodic_table.html Periodic Table: Metallic arrangement 1 IA 1 • Layout of the Periodic Table: Metals vs. nonmetals 2 IIA 13 IIIA 14 IVA 15 VA 18 VIIIA 16 VIA 17 VIIA 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB Metals 10 11 IB 12 IIB Nonmetals •Family: Are arranged vertically down the periodic table (columns or group, 1- 18 or I-VIII A) •These elements have the same number electrons in the outer most shells, the valence shell. 1 IA 1 18 VIIIA Alkali Family: 1 e- in the valence shell 2 IIA 13 IIIA 14 IVA 15 VA 16 VIA 2 3 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 4 5 6 7 Halogen Family: 7 e- in the valence shell 17 VIIA • Notable families of the Periodic Table Halogen Noble Gas Chalcogens Alkali Alkaline (earth) 1 IA 1 18 VIIIA 2 IIA 13 IIIA Transition Metals 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 14 IVA 15 VA 16 VIA 17 VIIA 1 IA 1 H 2 Li 3 4 5 6 7 18 VIIIA 2 IIA Na Mg K Ca 13 IIIA 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 Fe 9 VIIIB 10 11 IB 12 IIB Cu Zn Ag 14 IVA 15 VA 16 VIA 17 VIIA C N O F Al Si P S Cl Br I He e- configuration from the periodic periodic table 1 IA 18 VIIIA 2 IIA 1 H 1s1 2 Li Be 2s1 2s2 Na Mg 3s1 3s2 3 4 5 6 7 13 IIIA 3 IIIB 4 IVB Sc 3d1 Rb 5s1 Ca 4s2 Sr 5s2 Y 4d1 V Ti Cr Mn Fe Co 3d2 3d3 4s13d5 3d5 3d6 3d7 Zr Nb Mo Tc Ru Rh 4d2 4d3 5s14d5 4d5 4d6 4d7 Cs 6s1 Ba 6s2 La 5d1 Hf Ta W Re Os 5d2 5d3 6s15d5 5d5 5d6 Fr 7s1 Ra 7s2 Ac Rf 6d1 6d2 K 4s1 5 VB 6 VIB 7 VIIB Db Sg Bh 6d3 7s16d5 6d5 8 9 VIIIB 14 IVA 15 VA 16 VIA 17 VIIA B 2p1 •B C N O 1 2 3 •2p 2p 2p 2p4 F 2p5 Ne 2p6 Al 3p1 Si 3p2 Cl 3p5 Ar 3p6 He 1s2 10 11 IB 12 IIB Ni 3d8 Cu 4s13d10 Ni 4d8 5s14d10 Zn Ga Ge 3d10 4p1 4p2 Cd In Sn 10 4d 5p1 5p2 As Se Be 4p3 4p4 4p5 I Sb Te 5p3 5p4 5p5 Kr 4p6 Xe 5p6 Hg Tl Pb 5d10 6p1 6p2 Bi Po At 6p3 6p4 6p5 Rn 6p6 Ir Ni 7 5d 5d8 Hs Mt 6d6 6d7 Ag Au 6s15d10 S P 3 3p 3p4 electron behavior • The periodic table can be classified by the behavior of their electrons West (South) METALS Alkali Alkaline Transition These elements tend to give up e - and form CATIONS 1 IA 1 Mid-plains METALLOID These elements will give up e- or accept e- East (North) NON-METALS Noble gas Halogens Calcogens These elements tend to accept e - and form ANIONS 2 IIA 13 IIIA 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 14 IVA 18 VIIIA 15 VA 16 VIA 17 VIIA Warm Up 1) Where are metals located below? 2) What group is known as the halogens? 3) Where are the metalloids located? 1 IA 1 18 VIIIA 2 IIA 13 IIIA 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 14 IVA 15 VA 16 VIA 17 VIIA Dmitri Mendeleev (1869) Based on atomic mass Today's periodic table organized by? http://www.chem.msu.su/eng/misc/mendeleev/welcome.html Periodic Trends • Today we will rationalize observed trends in – Atomic radius – Ionization energy. – Electronegativity Periodic trends based on behavior of (-) electrons and (+) protons Valence Electrons- the outermost electrons that surround an atom Valence Electrons- starting with group 1 = 1 valence egroup 2 = 2 valence egroup 3A = 3 valence etrend continues to group 8A •Atomic Radius: Trends in Atomic Radius •size of atom determine by boundaries of the valence e-. •Atomic radius increases as you move down a group. Why? •Atomic radius decreases as you move across a period. Why? •Atomic Radius: Trends in Atomic Radius •size of atom determine by boundaries of the valence e-. •Atomic radius increases as you move down a group. Why? •Because you are adding more electrons to outer orbits •Atomic radius decreases as you move across a period. Why? •Atomic Radius: Trends in Atomic Radius •size of atom determine by boundaries of the valence e-. •Atomic radius increases as you move down a group. Why? •Because you are adding more electrons to outer orbits •Atomic radius decreases as you move across a period. Why? •Adding more e- BUT also adding MORE P+ which pull in e- •Atomic Radius: Trends in Atomic Radius •size of atom determine by boundaries of the valence e-. •Atomic radius increases as you move down a group. Why? •Because you are adding more electrons to outer orbits •Atomic radius decreases as you move across a period. Why? •Adding more e- BUT also adding MORE P+ which pull in e- Trends in Atomic Radius •Place the following in order of increasing atomic radius •S, P, Ar, Cl, Si Trends in Atomic Radius •Place the following in order of increasing atomic radius •Ar, Cl, S, P, Si •Atomic Radius: Trends in Atomic Radius Trends in Ionization Potential Ionization potential: Energy required to remove valence electron from atom. Trends in Ionization Potential As you move across a period, ionization energy increases. WHY? - As you move across a period, the atomic radius decreases, (atom gets smaller). The outer electrons are closer to + nucleus and more strongly attracted to + center. Therefore, it requires more energy to remove electron Trends in Ionization Potential As you move down a group, ionization energy decreases. WHY? Electrons are further from the nucleus and thus easier to remove “e- SHIELDING" - Inner electrons block protons force of attraction on outer e-. therefore easier to remove outer electron Trends in Ionization Potential Place the following in order of increasing ionization energy: Mg, Ra, Sr, Ca, Ba,Be Trends in Ionization Potential Place the following in order of increasing ionization energy: Ra, Ba, Sr, Ca, Mg, Be Trends in Electronegativity The ability of an atom to attract (steal) electrons to itself: Trends in Electronegativity The ability of an atom to attract (steal) electrons to itself: Which is more electronegative? K or S and why? Trends in Electronegativity The ability of an atom to attract (steal) electrons to itself: Which is more electronegative? S why? b/c small radius of atom means the + nucleus can attract the –e from other atoms Summary of Trend • Periodic Table and Periodic Trends • 1. Electron Configuration 3. Ionization Energy: Largest toward NE of PT 4. Electron Negativity: Most favorable NE of PT 2. Atomic Radius: Largest toward SW corner of PT Periodic Table Patterns • Elements in the same group generally have similar chemical properties. • Properties are not identical, however. Periodic Table Patterns Dmitri Mendeleev came to the conclusion that Elements in the same group generally have similar chemical properties. Periodic Table Predictions Mendeleev, for instance, predicted the discovery of germanium (which he called ekasilicon) as an element with an atomic weight between that of zinc and arsenic, but with chemical properties similar to those of silicon. Electron Configurationenergy stair levels Electrons are found in orbits. an orbital is the shape of the space where there is a high probability of finding electrons The s orbitals are spheres This is the shape of p orbitals z The three 2p orbitals, 2px, 2py, 2pz y x once each 2p orbital is filled with a pair of electrons, then the 3s orbital gets the next two electrons the 3s electrons have a higher energy than 1s, 2s, or 2p electrons, so 3s electrons are generally found further from the nucleus than 1s, 2s, or 2p electrons Summary of Trend • Periodic Table and Periodic Trends • 1. Electron Configuration 3. Ionization Energy: Largest toward NE of PT 4. Electron Negativity: Most favorable NE of PT 2. Atomic Radius: Largest toward SW corner of PT once each 2p orbital is filled with a pair of electrons, then Electron Configurationenergy stair levels General Rules • Aufbau Principle – Electrons fill lowest energy orbitals first. – “Lazy Occupant Rule” General Rules • Hund’s Rule – Within a sublevel, place one e- per orbital before pairing them e- repel each other – “Empty Room Rule” WRONG RIGHT General Rules • Pauli Exclusion Principle – Each orbital can hold TWO electrons with opposite spins. Electron Notations • Orbital Diagram O 8e- 1s 2s • Electron Configuration 2 2 4 1s 2s 2p 2p • Longhand e- Configuration S 16e- 1s2 2s2 2p6 3s2 3p4 Core Electrons Valence Electrons • Shorthand e- Configuration S 16e 2 4 [Ne] 3s 3p J.J. Thomson used cathode ray tube to discover electron Atomic Review Atomic Nomenclature 35 Mass # Cl Symbol 17 # protons Periodic Law- elements increase by atomic number and have a periodic trend or repetition of physical & chemical properties Average atomic mass- mass on PT Based on abundance of isotopes 1)Change % to decimal 2)Multiply decimal by the mass 3)Add the numbers together Electron Configuration Al 1s22s22p63s23p1 s p d © 1998 by Harcourt Brace & Company e- configuration table 1s 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6p 6s La 5d 7s Ac 6d 4f 5f The Periodic Table s1 1 2 3 4 5 6 7 s2 d1 d2 d3 d4 d5 d6 d7 d8 d10 p1 d9 p2 p3 p4 p5 p6 1 2 H He 3 4 Li Be 11 12 Na Mg 19 20 5 6 7 8 B C N O F Ne 13 14 15 16 17 P S 33 34 Al Si 21 22 23 24 25 26 27 28 29 30 31 32 9 10 18 Cl Ar 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 37 41 38 39 40 42 43 44 45 46 47 48 49 50 51 52 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te 55 56 57 72 73 74 75 76 77 78 Cs Ba La Hf Ta W Re Os Ir 87 88 89 104 105 106 107 108 79 80 81 f 84 I Xe 85 86 109 110 111 114 116 118 Uuq Uuh Uuo 112 f1 f2 f3 f4 f5 f6 f7 f8 f9 f1 f1 f1 f1 f1 d p 83 54 Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Uun Uuu Uub s 82 53 58 4 5 59 60 61 62 63 64 65 66 067 168 269 370 471 99 100 101 102 103 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 90 91 92 93 94 95 96 97 98 Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr C. Periodic Patterns • Example - Hydrogen 1 2 3 4 5 6 7 1 1s 1st Period 1st column of s-block s-block Electron Configuration • F • Cl • Al • Br Orbital Diagrams F Cl Al Br 1s 2s 2p 3s 3p 1s 2s 2p 3s 1s 2s 2p 1s 2s 4s 3d 4p 3p 4s 3d 4p 3s 3p 4s 3d 4p 2p 3s 3p 4s 3d 4p Electron Configuration • F 1s22s22p5 • Cl 1s22s22p63s23p5 • Al 1s22s22p63s23p1 • Br 1s22s22p63s23p64s23d104p5 Write Orbital and Electron Configurations • N • Si • Mg • Ga Orbital Diagrams N Si Mg Ga 1s 2s 2p 3s 1s 2s 2p 3s 1s 2s 2p 1s 2s 3p 4s 3d 4p 3p 4s 3d 4p 3s 3p 4s 3d 4p 2p 3s 3p 4s 3d 4p Electron Configuration • N 1s22s22p3 • Si 1s22s22p63s23p2 • Mg 1s22s22p63s2 • Ga 1s22s22p63s23p64s23d104p1 • Now write the above in short hand configuration Electron Configuration • N [He]2s22p3 Electron Configuration • Si [Ne]3s23p2 Electron Configuration • Mg [Ne]3s2 Electron Configuration • Ga [Ar]4s23d104p1 Periodic Patterns • Example - Germanium 1 2 3 4 5 6 7 [Ar] 2 4s 10 3d 2 4p • Notable families of the Periodic Table Halogen Noble Gas Chalcogens Alkali Alkaline (earth) 1 IA 1 18 VIIIA 2 IIA 13 IIIA Transition Metals 2 3 4 5 6 7 3 IIIB 4 IVB 5 VB 6 VIB 7 VIIB 8 9 VIIIB 10 11 IB 12 IIB 14 IVA 15 VA 16 VIA 17 VIIA Electron Stability • Full energy level • Full sublevel (s, p, d, f) • Half-full sublevel 1 2 3 4 5 6 7 Stability • Electron Configuration Exceptions – Copper EXPECT: ACTUALLY: [Ar] 4s2 3d9 [Ar] 4s1 3d10 – Copper gains stability with a full d-sublevel. “5 Facts 5 Pictures” Review Interesting Fact 1- define or explain Interesting Fact 3 define or explain [picture] [Picture] Most Important Concept or Fact 5Describe and explain What you learned [Picture] Interesting Fact 2- define or explain [picture] Interesting Fact 4- define or explain [picture] J.J. Thomson used cathode ray tube to discover electron Atomic Review Atomic Nomenclature 35 Mass # Cl Symbol 17 # protons Periodic Law- elements increase by atomic number and have a periodic trend or repetition of physical & chemical properties Average atomic mass- mass on PT Based on abundance of isotopes 1)Change % to decimal 2)Multiply decimal by the mass 3)Add the numbers together Electron Configuration Al 1s22s22p63s23p1 D. Stability • Electron Configuration Exceptions – Chromium EXPECT: ACTUALLY: [Ar] 4s2 3d4 [Ar] 4s1 3d5 – Chromium gains stability with a half-full dsublevel. Stability • Ion Formation – Atoms gain or lose electrons to become more stable. – Noble Gases . 1 2 3 4 5 6 7 D. Stability • Ion Electron Configuration – Write the e- config for the closest Noble Gas – EX: Oxygen ion O2- Ne O2- 10e- [He] 2s2 2p6 4. Trend in Electron Affinity Electron Affinity: The energy release when an electron is added to an atom. Most favorable toward NE corner of PT since these atoms have a great affinity for e-. Periods- left to right Groups- up & down, numbered 1-18 or 1A-8A, Representative Elements- Group A Elements, Group 1, 2, & 13-18 (8 groups represented)