ACSI 2022 HL Notes Periodicity (Teacher)

IBDP Chemistry HL/ Periodicity , The Periodic Table Page 1 Anglo − Chinese School (Independent) Year 5 (2022) IBDP Chemistry HL (IBDP syllabus Topic 3 ) 3 .1 Periodic table - Essential Idea: The arrangement of the elements in the periodic table helps to predict their electron configuration. 3 .2 Periodic trends - Essential Idea: Elements show trends in their physical and chemical prope rties across periods and down groups. TEACHER COPY – WITH SUGGESTED SOLUTIONS TOPIC 3 PERIODICITY (Part 1)

IBDP Chemistry HL/Periodicity , The Periodic Table Page 2 3.1 Periodic table Nature of science: Obtain evidence for scientific theories by making and testing predictions based on them – scientists organise subjects based on structure and function; the periodic table is a key example of this. Early models of the periodic table from Mendeleev, and later Moseley, allowed for the prediction of properties of elements that had not yet been discovered. (1.9) Understandings: • The Periodic Table is arranged into four blocks associated with the four sublevels – s, p, d and f. • The Periodic Table consists of groups (vertical columns) and periods (horizontal rows). • The period number (n) is the outer energy level that is occupied by electrons. • The number of the principal energy level and the number of the valence electrons in an atom can be deduced from its position on the periodic table. • The Periodic table shows the positions of metals, non–metals and metalloids. Applications and skills: • Deduction of the electron configuration of an atom of an element from the element’s position on the periodic table, and vice-versa. Guidance: • The terms alkali metals, noble gases, halogens, transition metals, lanthanoids and actinoids should be known. • The group numbering scheme from group 1 to group 18 as recommended by IUPAC should be used. Nature of science Dimitri Mendeleev Mendeleev: The Periodic Law by atomic weight, 1869

IBDP Chemistry HL/Periodicity , The Periodic Table Page 3 3.1 Periodic trends Nature of science: Looking for patterns – the position of an element in the periodic table allows scientists to make accurate predictions of its physical and chemical properties. This gives scientists the ability to synthesize new substances based on the expected reactivity of elements. (3.1) Understandings: • Vertical and horizontal trends in the Periodic Table exist for atomic radius, ionic radius, ionisation energy, electron affinity and electronegativity. • Trends in metallic and non–metallic behaviour are due to the trends above. • Oxides change from basic through amphoteric and acidic across a period. Applications and skills: • Prediction and explanation of the metallic and non-metallic behaviour of an element based on its position in the periodic table. • Discussion of the similarities and diff erences in the properties of elements in the same group, with reference to alkali metals (group 1) and the halogens (group 17). • Construction of equations to explain the pH changes for the reactions of Na 2O, MgO and P4O10 and the oxides of nitrogen and sulfur with water. Guidance: • Only examples of general trends across periods and down groups are required. For ionisation energy the discontinuities in the increase across a period should be covered. • Group trends should include the treatment of the reactions of alkali metals with water, alkali metals with halogens and halogens with halide ions.

IBDP Chemistry HL/Periodicity , The Periodic Table Page 4 The Periodic Table 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 1 1 H 1.01 2 He 4.00 2 3 Li 6.94 4 Be 9.01 Atomic number Element Relative atomic mass Metals Metalloids Non- metals 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00 10 Ne 20.18 3 11 Na 22.99 12 Mg 24.31 13 Al 26.98 14 Si 28.09 15 P 30.97 16 S 32.07 17 Cl 35.45 18 Ar 39.95 4 19 K 39.10 20 Ca 40.08 21 Sc 44.96 22 Ti 47.87 23 V 50.94 24 Cr 52.00 25 Mn 54.94 26 Fe 55.85 27 Co 58.93 28 Ni 58.69 29 Cu 63.55 30 Zn 65.38 31 Ga 69.72 32 Ge 72.63 33 As 74.92 34 Se 78.96 35 Br 79.90 36 Kr 83.90 5 37 Rb 85.47 38 Sr 87.62 39 Y 88.91 40 Zr 91.22 41 Nb 92.91 42 Mo 95.96 43 Tc (98) 44 Ru 101.07 45 Rh 102.91 46 Pd 106.42 47 Ag 107.87 48 Cd 112.41 49 In 114.82 50 Sn 118.71 51 Sb 121.76 52 Te 127.60 53 I 126.90 54 Xe 131.29 6 55 Cs 132.91 56 Ba 137.33 57 † La 138.91 72 Hf 178.49 73 Ta 180.95 74 W 183.84 75 Re 186.21 76 Os 190.23 77 Ir 192.22 78 Pt 195.08 79 Au 196.97 80 Hg 200.59 81 Tl 204.38 82 Pb 207.2 83 Bi 208.98 84 Po (209) 85 At (210) 86 Rn (222) 7 87 Fr (223) 88 Ra (226) 89 ‡ Ac (227) 104 Rf (267) 105 Db (268) 106 Sg (269) 107 Bh (270) 108 Hs (269) 109 Mt (278) 110 Ds (281) 111 Rg (281) 112 Cn (285) 113 Uut (286) 114 Uuq (289) 115 Uup (288) 116 Uuh (293) 117 Uus (294) 118 Uuo (294) † 58 Ce 140.12 59 Pr 140.91 60 Nd 144.24 61 Pm (145) 62 Sm 150.36 63 Eu 151.96 64 Gd 157.25 65 Tb 158.93 66 Dy 162.50 67 Ho 164.93 68 Er 167.26 69 Tm 168.93 70 Yb 173.05 71 Lu 174.97 ‡ 90 Th 232.04 91 Pa 231.04 92 U 238.03 93 Np (237) 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (262)

IBDP Chemistry HL/Periodicity , The Periodic Table Page 5 3.1 Periodic Table In the Periodic Table, elements are arranged in horizontal rows ( periods) and vertical columns (groups) in the order of increasing atomic (proton) number, Z. 3.1.1 Periods • Horizontal rows of elements in the Periodic Table. • They are labelled using numerals: 1, 2, 3, 4, 5, 6, 7. • Period number corresponds to the principal quantum number, n, of the highest occupied energy level in the elements of the period. • Across a period, the chemical properties of the element gradually change from those of reactive metals to metalloids and non–metals (except for period 1). The thick stepped lines on the periodic table on page 4 of the notes separate the elements into metals on the left, for example, aluminium, and carbon on the right, as a non–metal. However, some of the elements, such as silicon and germanium, have physical and chemical similarities to both metals and non–metals. Chemists classify these elements as metalloids. They are poor conductors of electricity and, unlike metals, their conductivity increases with temperature. Some metalloids form amphoteric oxides. Period 1 H He 1s1 1s2 Period 2 Li Be B C N O F Ne [He]2s1 [He]2s2 [He]2s22p1 [He]2s22p2 [He]2s22p3 [He]2s22p4 [He]2s22p5 [He]2s22p6 Period 3 Na Mg Al Si P S Cl Ar [Ne]3s1 [Ne]3s2 [Ne]3s23p1 [Ne]3s23p2 [Ne]3s23p3 [Ne]3s23p4 [Ne]3s23p5 [Ne]3s23p6 3.1.2 Main Group, Transition Elements • A group is a vertical column of elements. They are denoted by numerals: 1, 2, 3, 4, 5… to 18 • The number of valence electrons (outer –shell electrons) can be found from the group number of the s– and