CHEM 120 Spring 2017 Introduction to Inorganic Chemistry Instructor Dr. Upali Siriwardane (Ph.D. Ohio State)
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1 CHEM 120 Spring 2017 Introduction to Inorganic Chemistry Instructor Dr. Upali Siriwardane (Ph.D. Ohio State) Office: 311 Carson Taylor Hall ; Phone: ; Office Hours: MWF 8:00-9:00 and 11:00-12:00; TR 10:00-12:00 Contact me trough phone or if you have questions Online Tests on Following days March 24, 2017: Test 1 (Chapters 1-3) April 7, 2017 : Test 2 (Chapters 4-5) April 28, 2017: Test 3 (Chapters 6,7 &8) May 12, 2017 : Test 4 (Chapters 9, 10 &11) May 15, 2017: Make Up Exam: Chapters 1-11). 1
2 Chapter 3 Atomic Structure and the Periodic Table Table of Contents 3.1 Internal Structure of an Atom 3.2 Atomic Number and Mass Number 3.3 Isotopes and Atomic Masses 3.4 The Periodic Law and the Periodic Table 3.5 Metals and Nonmetals 3.6 Electron Arrangements Within Atoms 3.7 Electron Configurations and Orbital Diagrams 3.8 The Electronic Basis for the Periodic Law and the Periodic Table 3.9 Classification of the Elements Copyright Cengage Learning. All rights reserved 2
3 Section 3.1 Internal Structure of an Atom Subatomic Particle A very small particle that is a building block for atoms. Return to TOC Copyright Cengage Learning. All rights reserved 3
4 Section 3.1 Internal Structure of an Atom Three Types of Subatomic Particles The atom contains: Electrons found outside the nucleus; possesses a negative electrical charge; smallest mass. Protons found in the nucleus; positive charge equal in magnitude to the electron s negative charge. Neutrons found in the nucleus; no charge; virtually same mass as a proton. Return to TOC Copyright Cengage Learning. All rights reserved 4
5 Section 3.1 Internal Structure of an Atom Charge and Mass Characteristics Return to TOC Copyright Cengage Learning. All rights reserved 5
6 Section 3.1 Internal Structure of an Atom The nucleus is: Small compared with the overall size of the atom. Extremely dense; accounts for almost all of the atom s mass. Positively charged center of an atom. Return to TOC Copyright Cengage Learning. All rights reserved 6
7 Section 3.1 Internal Structure of an Atom Charge Neutrality of an Atom An atom as a whole is electrically neutral (no net electrical charge). # of Protons = # of Electrons Return to TOC Copyright Cengage Learning. All rights reserved 7
8 Section 3.2 Atomic Number and Mass Number Atomic Number (Z) # of protons in the nucleus of an atom. Mass Number (A) sum of the # of protons and the # of neutrons in the nucleus of an atom. Copyright Cengage Learning. All rights reserved 8
9 Section 3.2 Atomic Number and Mass Number Complete Chemical Symbol Notation Mass number Atomic number A Symbol Z Chemical symbol Na Copyright Cengage Learning. All rights reserved 9
10 Section 3.2 Atomic Number and Mass Number Element A pure substance in which all atoms present have the same atomic number. All atoms with the same atomic number have the same chemical properties and are atoms of the same element. Copyright Cengage Learning. All rights reserved 10
11 Section 3.3 Isotopes and Atomic Masses Isotopes Atoms of an element that have the same number of protons and the same number of electrons but different numbers of neutrons. Show almost identical chemical properties; chemistry of atom is due to its electrons. Physical properties are often slightly different because they have different masses. In nature most elements contain mixtures of isotopes. Copyright Cengage Learning. All rights reserved 11
12 Section 3.3 Isotopes and Atomic Masses Two Isotopes of Sodium Na Na Number of Protons = 11 Mass number = 23 Number of Neutrons = 12 Number of Protons = 11 Mass number = 24 Number of Neutrons = 13 Copyright Cengage Learning. All rights reserved 12
13 Section 3.3 Isotopes and Atomic Masses Exercise A certain isotope X contains 23 protons and 28 neutrons. What is the mass number of this isotope? Identify the element. Copyright Cengage Learning. All rights reserved 13
14 Section 3.3 Isotopes and Atomic Masses Exercise A certain isotope X contains 23 protons and 28 neutrons. What is the mass number of this isotope? 51 Identify the element. Vanadium Copyright Cengage Learning. All rights reserved 14
15 Section 3.3 Isotopes and Atomic Masses Atomic Masses Elements occur in nature as mixtures of isotopes. Carbon = 98.89% 12 C 1.11% 13 C <0.01% 14 C Calculated average mass for the isotopes of an 12 element expressed on a scale where C 6 serves as the reference point. Copyright Cengage Learning. All rights reserved 15
16 Section 3.3 Isotopes and Atomic Masses Average Atomic Mass for Carbon 98.89% of 12 amu % of amu = (0.9889)(12 amu) + (0.0111)( amu) = amu Copyright Cengage Learning. All rights reserved 16
17 Section 3.3 Isotopes and Atomic Masses Exercise An element consists of 62.60% of an isotope with mass amu and 37.40% of an isotope with mass amu. Calculate the average atomic mass and identify the element. (62.60% of amu % of )/100 (0.6260)( amu) + (0.0111)( amu) = amu Copyright Cengage Learning. All rights reserved 17
18 Section 3.3 Isotopes and Atomic Masses Exercise An element consists of 62.60% of an isotope with mass amu and 37.40% of an isotope with mass amu. Calculate the average atomic mass and identify the element. Average Atomic Mass = amu The element is rhenium (Re). Copyright Cengage Learning. All rights reserved 18
19 Section 3.4 The Periodic Law and the Periodic Table Periodic Law When elements are arranged in order of increasing atomic number, elements with similar chemical properties occur at periodic (regularly recurring) intervals. Periodic Table Tabular arrangement of the elements in order of increasing atomic number such that elements having similar chemical properties are positioned in vertical columns. Copyright Cengage Learning. All rights reserved 19
20 Section 3.4 The Periodic Law and the Periodic Table The Periodic Table Periods horizontal rows of elements Groups elements in the same vertical columns; have similar chemical properties Copyright Cengage Learning. All rights reserved 20
21 Section 3.4 The Periodic Law and the Periodic Table The Periodic Table Copyright Cengage Learning. All rights reserved 21
22 Section 3.4 The Periodic Law and the Periodic Table Groups Table of common charges formed when creating ionic compounds. Group Charge Alkali Metals (1A) 1+ Alkaline Earth Metals (2A) 2+ Halogens (7A) 1- Noble Gases (8A) 0 Copyright Cengage Learning. All rights reserved 22
23 Section 3.5 Metals and Nonmetals Metal An element that has the characteristic properties of luster, thermal conductivity, electrical conductivity, and malleability. Copyright Cengage Learning. All rights reserved 23
24 Section 3.5 Metals and Nonmetals Nonmetal An element characterized by the absence of the properties of luster, thermal conductivity, electrical conductivity, and malleability. Copyright Cengage Learning. All rights reserved 24
25 Section 3.5 Metals and Nonmetals Selected Physical Properties of Metals and Nonmetals Copyright Cengage Learning. All rights reserved 25
26 Section 3.5 Metals and Nonmetals Dividing Line Between Metals and Nonmetals Copyright Cengage Learning. All rights reserved 26
27 Section 3.6 Electron Arrangements Within Atoms Electron Shells A region of space about a nucleus that contains electrons that have approximately the same energy and that spend most of their time approximately the same distance from the nucleus. Electrons that occupy the first electron shell are closer to the nucleus and have a lower energy than electrons in the second electron shell. Copyright Cengage Learning. All rights reserved 27
28 Section 3.6 Electron Arrangements Within Atoms Electron Subshells A region of space within an electron shell that contains electrons that have the same energy. Subshell Number of Electrons s 2 p 6 d 10 f 14 Copyright Cengage Learning. All rights reserved 28
29 Section 3.6 Electron Arrangements Within Atoms Electron Orbitals A region of space within an electron subshell where an electron with a specific energy is most likely to be found. An electron orbital can accommodate a maximum of 2 electrons. Copyright Cengage Learning. All rights reserved 29
30 Section 3.6 Electron Arrangements Within Atoms Electron Orbitals Subshell Number of Orbitals s 1 p 3 d 5 f 7 Copyright Cengage Learning. All rights reserved 30
31 Section 3.6 Electron Arrangements Within Atoms Electron Orbitals Copyright Cengage Learning. All rights reserved 31
32 Section 3.6 Electron Arrangements Within Atoms Orbitals Within the Same Subshell Differ in Orientation Copyright Cengage Learning. All rights reserved 32
33 Section 3.6 Electron Arrangements Within Atoms Electron Spin As an electron moves about within an orbital, it spins on its own axis in either a clockwise or a counterclockwise direction. When two electrons are present in an orbital, they always have opposite spins. Copyright Cengage Learning. All rights reserved 33
34 Section 3.7 Electron Configurations and Orbital Diagrams Rules for Assigning Electrons to Various Shells, Subshells, and Orbitals 1. Electron subshells are filled in order of increasing energy. 2. Electrons occupy the orbitals of a subshell such that each orbital acquires one electron before any orbital acquires a second electron. All electrons in such singly occupied orbitals must have the same spin. 3. No more than two electrons may exist in a given orbital and then only if they have opposite spins. Copyright Cengage Learning. All rights reserved 34
35 Section 3.7 Electron Configurations and Orbital Diagrams Electron Configurations Copyright Cengage Learning. All rights reserved 35
36 Section 3.7 Electron Configurations and Orbital Diagrams Electron Configurations Copyright Cengage Learning. All rights reserved 36
37 Section 3.7 Electron Configurations and Orbital Diagrams Electron Configurations A statement of how many electrons an atom has in each of its electron subshells. An oxygen atom as an electron arrangement of two electrons in the 1s subshell, two electrons in the 2s subshell, and four electrons in the 2p subshell. Oxygen: 1s 2 2s 2 2p 4 Copyright Cengage Learning. All rights reserved 37
38 Section 3.7 Electron Configurations and Orbital Diagrams Orbital Diagrams A notation that shows how many electrons an atom has in each of its occupied electron orbitals. Oxygen: 1s 2 2s 2 2p 4 Oxygen: 1s 2s 2p Copyright Cengage Learning. All rights reserved 38
39 Section 3.7 Electron Configurations and Orbital Diagrams Exercise Determine the expected electron configurations for each of the following. a) S b) Ba Copyright Cengage Learning. All rights reserved 39
40 Section 3.7 Electron Configurations and Orbital Diagrams Exercise Determine the expected electron configurations for each of the following. a) S b) Ba 1s 2 2s 2 2p 6 3s 2 3p 4 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 Copyright Cengage Learning. All rights reserved 40
41 Section 3.8 The Electronic Basis for the Periodic Law and the Periodic Table The electron arrangement in the outermost shell is the same for elements in the same group. This is why elements in the same group have similar chemical properties. Group 1A very reactive Li: 1s 2 2s 1 Na: 1s 2 2s 2 2p 6 3s 1 K: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 Copyright Cengage Learning. All rights reserved 41
42 Section 3.8 The Electronic Basis for the Periodic Law and the Periodic Table Electron Configurations and the Periodic Table Copyright Cengage Learning. All rights reserved 42
43 Section 3.8 The Electronic Basis for the Periodic Law and the Periodic Table Electron Configurations and the Periodic Table Copyright Cengage Learning. All rights reserved 43
44 Section 3.8 The Electronic Basis for the Periodic Law and the Periodic Table Distinguishing Electron Last electron added to the electron configuration for an element when electron subshells are filled in order of increasing energy. This last electron is the one that causes an element s electron configuration to differ from that of an element immediately preceding it in the periodic table. Copyright Cengage Learning. All rights reserved 44
45 Section 3.9 Classification of the Elements 1. A system based on selected physical properties of the elements, in which they are described as metals or nonmetals. 2. A system based on the electron configurations of the elements, in which elements are described as noble-gas, representative, transition, or inner transition elements. Copyright Cengage Learning. All rights reserved 45
46 Section 3.9 Classification of the Elements Classification Scheme on the Periodic Table Copyright Cengage Learning. All rights reserved 46
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