The Periodic Table Chapter 6 Mendeleevs Periodic Table
Arranged the elementsin the periodic table inorder of increasingmass Mendeleevs Periodic Table Modern Periodic Table elements are arranged in order of increasing atomic number Groups = columns 1-18 elements have similar properties Periods = rows 1-7 equal to the principal energy level The Periodic Law Period Group Three ways to classify elements
Elements can beclassified into metals,nonmetals, andsemimetals. Elements can also beclassified into groupsor families. You should be able todo both. Semimetals Properties of Metals Metals are good conductorsof heat and electricity. They are shiny and lustrous. Metals can be pounded intothin sheets (malleable) anddrawn into wires (ductile). Metals do not hold onto theirvalence electrons very well. They have lowelectronegativity. Properties of Nonmetals
Nonmetals are poorconductors of heat andelectricity. Exception:graphite is agood conductor. Nonmetals are brittle.Ifyou hit them with ahammer, they shatter andturn to powder. Good examples ofnonmetals are sulfur,carbon, and all the gases. More on Nonmetals The seven diatomic molecules are all nonmetals.
Remember that hydrogen isa nonmetal even though it islocated on the left side of thetable with the metals. Nonmetals strongly attracttheir electrons.They havehigh electronegativity valuesand therefore form negativeions. Br2I2N2Cl2H2O2F2 Semimetals Si These elements haveproperties that are in- between those of the metalsand nonmetals. They are very important formaking transistors andcomputer chips. Silicon (Si), germanium (Ge),and tellurium (Te) are shown. Different books includepolonium (Po) and leave outastatine (At). Te Ge Semimetals are also called metalloids. METALS Metals and Nonmetals Nonmetals Metalloids H He Li Be B C N O F
1 He 2 1 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Nonmetals Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 METALS Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Metalloids Cs 55 Ba 56 He 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 decreases increases Reference Table Periodic Table Trends:
1.Across a period, metallic character Why? More electrons in outer shells Less tendency to lose electrons 2.Down a group, metallic character Electrons are in outer shells further from the nucleus Greater tendency to lose electrons decreases increases Which of these sets of elements have similarphysical and chemical properties?
oxygen, nitrogen, carbon, boron strontium, magnesium, calcium, beryllium nitrogen, neon, nickel, fluorine Name 2 elements that have properties similarto those of the element sodium. Any other Group 1 element: Lithium, Potassium, Rubidium, Cesium, Francium Metallic Review Metal Metalloid Nonmetal Metal
Identify each element as ametal, nonmetal or metalloid Gold - Silicon - Sulfur - Barium - Metal Metalloid Nonmetal Metal Identify each property below as morecharacteristic of a metal or a nonmetal
Brittle - Malleable - Poor conductor of electricity - Shiny - Tend to gain electrons - In which pair of elements are the chemicalproperties of the elements most similar? sodium and chlorine nitrogen and phosphorus boron and oxygen Nonmetal Metal Nonmetal Metal Nonmetal Classifying the Elements
Alkali Metals Alkaline Earth Metals Halogens Noble Gases Representative Elements Transition Elements Group 1 (1A) Group 2 (2A) Group 17 (7A) Group 18 (8A) Inert gases Groups 1,2 and 13-17 All Groups 3-12 (B) Label your Reference Periodic Table
1 18 H 1 He 2 1 2 13 14 15 16 17 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 3 4 5 6 7 8 9 10 11 12 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 He 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 Classifying Review Which of the following are transition metals? Cu Sr
Cd Au Al Ge Co Periodic Trends Trends in Atomic Size Trends in Ionization Energy
Trends in Ionic Size Trends in Electronegativity Trends in Atomic Size Atomic Radius one half of the distancebetween the nuclei of two atoms of thesame element Trends in Atomic Size Found on table S Group Trends in Atomic Size
From top to bottom the size trends increases Why? The number of shells (rings) increases Valence electrons get shielded from the nuclear pull Period Trends in Atomic Size From left to right the size trends decreases The size of the rings stay the same The number of protons increase and pull from nucleus is strong Trends in Atomic Size Sample Exercise Which element in each pair has atoms with a larger atomic radius? orlithium or magnesium Carbonor or oxygen Arrange these elements in order of decreasing atomic size: sulfur, chlorine, aluminum, and sodium. Sodium Strontium germanium Selenium Sodium Aluminum Sulfur Chlorine ions Form when electrons are transferred between atoms An ion with a positive charge (lost electrons) is called a An ion with a negative charge (gained electrons) is called an Ionization Energy - the energy required to remove an electron from an atom cation anion Ionization Energy Found on table S
The ability to become a positive charge Group Trends in Ionization Energy From top to bottom IE decreases (easier to take away e-) Why? More layers of shells (rings) Nucleus is too weak to pull in valence Period Trends in Ionization Energy From left to right IE increases Same amount of shells (rings) Nuclear pull increases, ring becomes smaller Ionization Energy This is the energy needed to remove an electron.
It is easier to removean electron from alarger atom becausethe electron is fartherfrom the nucleus andfeels less attraction. Ionization energy Practice
Which element in each pair has a greater first ionization energy? Lithium or or strontium Cesium or Arrange the following groups of elements in order of increasing ionization energy. Be, Mg, Sr Bi, Cs, Ba Na, Al, S boron Magnesium aluminum Sr Mg Be Cs, Ba Bi Na Al S Trends in ionic Size Ion When an atom loses or gains electrons
Cation When an atom loses an electron (becomes positive) Radius becomes smaller than the original atom Why? There is less repulsion between the electrons. Anion When an atom gains an electron (gains electron) Radius becomes bigger than the original atom There is more repulsion between electrons Trends in ionic Size Practice
Which particle has the larger radius in each atom/ion pair? orNa+ S or Ior or Al3+ In each pair, which ion is larger? orMg2+ Cl- or or Cu2+ Na S2- I- Al Ca 2+ P3- Cu+ Trends in Electronegativity
The ability of an atom to attract an electron Found on table S Group Trends in Electronegativity From top to bottom; electronegativity values decrease Why? More atomic shells (rings) Weaker nuclear pull Periodic Trends in Electronegativity From left to right; electronegativity values increase Shells (rings) stay the same Stronger nuclear pull Trends in Electronegativity Practice
Which element in each pair has a higher electronegativity value? Cl or Cor orNe orCa Which element in each pair has a greater attraction for electrons? Ca or O or H or K or F N Mg As O F O S Periodic Property Across a Period Down a Group Metallic Character Decreases Increases Atomic radius Ionization energy Ion Size Electronegativity