# Ch 3 Atomic Structure and the Periodic Table. Figure 3.1 size relationship is not to scale, ratio of average diameters atom/nucleus = 10 5

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1 1 Ch 3 Atomic Structure and the Periodic Table Figure 3.1 size relationship is not to scale, ratio of average diameters atom/nucleus = 10 5

2 2 Atoms are very small and spherical. Radii Range 0.9 x to 2.4 x m pm Recall Figure 1.12 Atomic Mass example: 1 H atom = x g 1atomic mass unit (amu) = x g For H: x g x 1 amu x g = amu

3 Ch 3.1 Internal Structure of an Atom Subatomic particles An atom is characterized by the number of protons (p) that it contains. A proton has a positive electrical charge. p charge = 1.60 x coulombs = +1 relative charge p mass = x g = amu A neutron (n) has no charge associated with it. n mass = x g = amu An electron (e) has a negative electrical charge. e charge = x coulombs = -1 relative charge e mass = x = amu mass of p ~ mass of n >>> mass of e - mass of e - is often ignored 3

4 4 Ch 3.2 Atomic Number and Mass Number Atomic number = Z = # of protons (unique physical property of each element) Mass number = A = # of protons + # of neutrons # of neutrons = For a neutral atom, net electrical charge = zero # of electrons = # of protons = A E complete chemical symbol notation Z

5 5 A 23 E Na Z 11 # p = Z = # n = A Z = = # e - = # p =

6 6 Ch 3.3 Isotopes and Atomic Masses Isotopes are atoms of an element that have the same number of protons and electrons but different numbers of neutrons C C C isotopes have nearly identical chemical properties most elements have at least two isotopes

7 7 Table 3.2 Elements with Z = 1 through 12 The atomic mass of an element is the calculated weighted average mass for the isotopes.

8 8 Chem 101 Grading Scheme Quizzes 180 points 180/1000 = 0.18 Labs 160 points 160/1000 = 0.16 Exams 660 points 660/1000 = Sample calculation of weighted average Quizzes 85 % x 0.18 = 15.3 % Labs 95 % x 0.16 = 15.2 % Exams 55 % x 0.66 = 36.3 % Average % % Weighted Average

9 Cl Cl amu amu % % natural abundance atomic mass of Cl = weighted average mass for the isotopes x 75.77/100 = x 24.23/100 = amu Cu Cu amu amu Atomic weight Cu = amu Which isotope is the more abundant? Answer:

10 Ch. 3.4 The Periodic Law and the Periodic Table Figure 3.2 Dmitri Ivanovich Mendeleev ( ) 10 In 1869 grouped 63 known elements in 1 st periodic table based on atomic weights and similar properties within a group. Modern periodic law - when elements are arranged in order of increasing atomic number, elements with similar chemical properties occur at periodic intervals. Figure 3.4

11 11 Periods of Elements Figure 3.3 Periods # of elements 1 2 H, He > 18 Groups of Elements (Ch 3.4 & 3.9) Groups IA VIIIA IA IIA VIIA VIIIA representative elements alkali metals alkaline earth metals halogens noble gases IB VIIIB Outside rows transition metals inner transition elements lanthanides & actinides Note: The noble gases are also representative elements.

12 12 Ch. 3.5 Metals and Nonmetals Metals Semimetals/Metalloids Nonmetals Semimetals/Metalloids Used in semiconductors. They have physical properties closer to those of metals, whereas their chemical properties are closer to those of nonmetals.

13 13 Fig 3.5 solids at RT, except Hg metallic luster malleable & ductile high thermal & electrical Al Pb Sn Zn clockwise from left Fig 3.5 gas or solid at RT, except Br 2 variety of colors solids are brittle poor (except graphite) good (except diamond) nonductile S 8 Br 2 P 4

14 Ch 3.6 Electron Arrangements within Atoms Supplemental material: Line Spectra and the Bohr Atom Each element has a unique line spectrum 14 demo: noble gas discharge tubes

15 15 Bohr Model Energies of electrons are quantized = limited to certain values. An excited atom releases energy in form of light when an electron falls back to its lower orbit (ground state).

16 16 It is now known that electrons do not exist in planet-like orbits but rather they occupy regions of space about the nucleus called orbitals. Figure 3.8 shapes of orbitals The space in which electrons move rapidly about a nucleus is divided into shells, subshells, and orbitals.

17 17 Electron Shells are specific energy levels n = 1, 2, 3, 4 increasing average distance from nucleus increasing average energy of shells electrons occupy the lowest shell available max # of electrons allowed in a shell = n = 1 2 e - n = 2 8 e - n = 3 18 e - etc. Drill question: Where are the electrons of Mg located? Z = p = 12 e- 1 st shell (n = 1) = 2 e 2 nd shell (n = 2) = 8 e 3 rd shell (n = 3) = e

18 18 Electron Subshells Each shell (n) consists of subshells Subshells are designated Energy levels increase s, p, d, f.. s < p < d < f Max # of subshells = n (shell) 1 st shell n = 1 s 2 nd shell n = 2 s + p 3 rd shell n = 3 s + p + d 4 th shell n = 4 s + p + d + f Max # of electrons in subshells s = 2 e p = 6 e d = 10 e f = 14 e

19 Figure 3.7 Summary so far 19

20 20 Drill Problems 1. What is the max # of electrons in a 5 d subshell? Shell # (n) 5 d subshell max # for d always e, regardless of n 2. What is the max # of electrons in the 4 th shell? s = 2 p = 6 d = 10 f = 14 also can use: 2 n 2 = 2 (4) 2 = 32 e total: 32 e

21 21 Electron Orbital is a region of space within a subshell where an electron with a specific energy is most likely to be found. max of 2 e can be found in 1 orbital subshell # of e # of orbitals s 2 1 p 6 3 d 10 5 f 14 7

22 22 Characteristics of Orbitals: Each type has a specific shape. Fig 3.8 Within the same subshell, orbitals differ mainly in orientation. Fig 3.9 Within a given subshell each orbital has the same. Volume, average distance, and energy increase with increasing shell number (n). Electrons move rapidly and occupy the entire orbital volume. A pair of electrons in the same orbital must be of opposite.

23 Electron Spin Clockwise Counterclockwise spin up spin down A pair of electrons of opposite spin can occupy the same orbital but electrons prefer to be alone Hund s Rule Ch 3.7 Electron Configurations and Orbital Diagrams fill lower energy levels first for a given subshell, first place single electrons pair electrons only with opposite spins 23 1s 2 2s 2 2p 6 3s 2 3p 3 Electron Configuration for P: 1s 2 2s 2 2p 6 3s 2 3p 3 Shorthand representation for P: 1s 2 2s 2 2p 6 3s 2 3p 3 = [Ne]3s 2 3p 3

24 24 Electron-Dot Symbols 6C _ 1s 2s 2p x 2p y 2p z 1s 2 2s 2 2p 2 unpaired electrons Electrons in the s & p orbitals of the outermost shell (valence shell) are called valence electrons and can be shown in an electron-dot symbol or Lewis symbol (also see Chapter 4.2) For the isolated (non-bonded) carbon atom: 4 valence electrons in the 2 nd shell 2 valence e in s are paired, 2 e in p are unpaired.. C all 4 sides in the symbol are equal unpaired electrons must be shown as single dots paired electrons must be shown as pairs

25 25 8O 1s 2s 2p x 2p y 2p z 1s 2 2s 2 2p 4 For the isolated (non-bonded) oxygen atom: valence electrons in the 2 nd shell valence e paired, e unpaired.. : O 2 unpaired electrons Note: The group number of the representative elements corresponds to the of valence electrons in the element

26 Fig 3.10 Order of filling electron subshells 26

27 Figure 3.11 Mnemonic device for remembering subshell filling order 27

28 Ch 3.8 The Electronic Basis for the Periodic Law and the Periodic Table 3Li 1s 2 2s 1 11Na 1s 2 2s 2 2p 6 3s 1 19K 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 37Rb 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 28 Group IA valence electron in s orbital 9F 1s 2 2s 2 2p 5 17Cl 1s 2 2s 2 2p 6 3s 2 3p 5 35Br 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 53I 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 5 Group VIIA valence electrons s 2 & p 5

29 Figure 3.12 Electron configuration and the position of elements in the periodic table. 29

30 30

31 31

32 32 Supplemental Material & Ch 5.9 Properties of Atoms and the Periodic Table A. Chemical properties of an element are related to the position of an element in the periodic table. demo: compare reactivity of Li, Na, K, Ca, Mg with H 2 O same same similar group = valence = chemical electrons properties

33 33 B. Periodic trends in metallic character for representative elements. Metallic character increases with increasing shell number (n) in a group. It decreases with increasing number of valence electrons.

34 34 C. Periodic trends in atomic radii (pm) for representative elements. Within a group, radii increase with increasing shell number (i.e. increasing distance from the nucleus). Across a period, radii decrease as the number of protons in the nucleus increase (i.e. increasing nuclear charge).

35 35 D. The type and number of bonds an element forms are related to its position in the periodic table. Electronegativity is a measure of the relative attraction that an atom has for the shared electrons in a covalent bond. Figure 5.11 in Stoker very different values bonds Chapter 4 similar values bonds Chapter 5

36 36 E. Periodic trends in ionization energies for representative elements. Li Li + + e - neutral atom positive ion electron cation Ionization of atoms requires Ionization Energy (I.E.) Within a period I.E. increases with increasing Z. Down a group I.E. decreases with increased atomic radius.

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