Chapter 2 Lecture Outline PDF

Chapter 2 Lecture Outline Prepared by Jan Henri G. Carpizo, RMT University of Pangasinan 1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproducti...

Chapter 2 Lecture Outline Prepared by Jan Henri G. Carpizo, RMT University of Pangasinan 1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.  2.1 Elements An element is a pure substance that cannot be broken down into simpler substances by a chemical reaction. Each element is identified by a one- or two-letter symbol. Elements are arranged in the periodic table. The position of an element in the periodic table tells us much about its chemical properties. 2 2.1 Elements 3 2.1 Elements 4  2.1 Elements A. Elements and the Periodic Table The elements in the periodic table are divided into three groups—metals, nonmetals, and metalloids. Metals: They are located on the left side of the periodic table. They are good conductors of heat and electricity. Metals are shiny solids at room temperature, except for mercury (Hg), which is a liquid. 5  2.1 Elements A. Elements and the Periodic Table Nonmetals: They are located on the right side of the periodic table. Nonmetals have a dull appearance They are usually poor conductors of heat and electricity. Nonmetals can be solids, liquids, or gases at room temperature solid liquid gas sulfur bromine nitrogen carbon oxygen 6  2.1 Elements A. Elements and the Periodic Table Metalloids: These are located on the solid line that starts at boron (B) and angles down towards astatine (At). Metalloids have properties intermediate between metals and nonmetals Only seven elements are Metalloids: boron (B) antimony (Sb) silicon (Si) tellurium (Te) germanium (Ge) astatine (At) arsenic (As) 7  2.1 Elements The Elements of Life 8  ACTIVITY Locate each element in the periodic table and classify it as a metal, nonmetal, or mettaloid. a. Titanium b. Chlorine c. Krypton d. Palladium e. Arsenic f. Cesium g. Selenium h. Osmium 9 2.1 Elements 10  2.1 Elements C. Compounds Compound: a pure substance formed by chemically combining two or more elements together. A chemical formula consists of: Element symbols to show the identity of the elements forming a compound. Subscripts to show the ratio of atoms in the compound. H 2O C 3H 8 2 H atoms 1 O atom 3 C atoms 8 H atoms 11  2.1 Elements C. Compounds Compounds can be drawn many ways: Different elements are represented by different colors: 12  2.2 Structure of the Atom All matter is composed of the same basic building blocks called atoms. Atoms are composed of three subatomic particles: 13  2.2 Structure of the Atom Nucleus Electron Cloud Nucleus: Electron cloud: location of protons location of electrons and neutrons comprises most of the dense core of the atom atom’s volume location of most of the atom’s mass 14  2.2 Structure of the Atom Opposite charges attract while like charges repel each other. Protons and electrons attract each other, but two electrons repel each other. 15  2.2 Structure of the Atom From the periodic table: 3 Atomic number (Z) is the number of protons Li in the nucleus. Every atom of a given element has the same number of protons in the nucleus. Different elements have different atomic numbers. A neutral atom has no net overall charge, so Z = number of protons = number of electrons 16  2.3 Isotopes A. Isotopes, Atomic Number, and Mass Number Isotopes are atoms of the same element that have a different number of neutrons. the number of protons (Z) Mass number (A) = + the number of neutrons Mass number (A) 35 Cl Atomic number (Z) 17 # of protons = 17 # of electrons = 17 # of neutrons = 35 – 17 = 18 17  Activity How many protons, neutrons, and electrons are contained in an atom of: 1. Argon (Ar), which has an atomic number of 18 and a mass number 40? 2. Z = 14, A= 28 3. What is the mass number of an atom that contains 42 protons, 42 electrons, and 53 neutrons? 18  ACTIVITY For each atom give the following information: 1) atomic number, 2) mass number, 3) Number of Protons, 4) Number of neutrons, 5) number of electrons 50 118 50 68 50 78 195 78 117 78 19  2.3 Isotopes B. Atomic Weight The atomic weight is the weighted average of the masses of the naturally occurring isotopes of a particular element reported in atomic mass units. From the periodic table: 6 atomic number C element symbol 12.01 atomic weight (amu) 20  2.3 Isotopes B. Atomic Weight HOW TO Determine the Atomic Weight of an Element Example What is the atomic weight of chlorine? Step List each isotope, it’s mass in atomic mass units, and it’s abundance in nature. Isotope Mass (amu) Isotopic Abundance Cl-35 34.97 75.78% = 0.7578 Cl-37 36.97 24.22% = 0.2422 21  2.3 Isotopes B. Atomic Weight HOW TO Determine the Atomic Weight of an Element Step Multiply the isotopic abundance by the mass of each isotope, and add up the products. The sum is the atomic weight of the element. 34.97 x 0.7578 = 26.5003 amu 36.97 x 0.2422 = 8.9541 amu 35.4544 amu = 35.45 amu 4 sig. figs. Answer 4 sig. figs. 22  2.4 The Periodic Table A. Basic Features of the Periodic Table A row in the periodic table is called a period, and a column in the periodic table is called a group. Main group elements: They consist of the tall columns on the right and left of the Periodic Table. The groups are numbered 1A–8A. Transition metal elements: These are in the 10 short columns in the middle. The groups are numbered 1B–8B. Inner transition elements: They consist of the lanthanides and actinides. There are no group numbers assigned. 23  2.4 The Periodic Table A. Basic Features of the Periodic Table 24  2.4 The Periodic Table B-1 Characteristics of Groups 1A and 2A Elements that comprise a particular group have similar chemical properties. Properties of Both Groups Group Group soft and shiny metals Number Name low melting points 1A Alkali metals good conductors of heat and electricity 2A Alkaline earth elements react with water to form basic solutions 25  2.4 The Periodic Table B-2 Characteristics of Groups 7A and 8A Group Group Number Name Properties exist as two atoms joined together 7A Halogens very reactive very stable 8A Noble gases rarely combine with any other elements 26  2.4 The Periodic Table C. The Unusual Nature of Carbon Carbon’s ability to join with itself and other elements gives it a versatility not seen with any other element in the periodic table. Elemental forms of carbon include the following carbon-only structures: diamond graphite buckminsterfullerene 27  2.5 Electronic Structure An electron is confined to a specific region around the nucleus, giving it a particular energy. The regions occupied by electrons are called principal energy levels or shells (n). The shells are numbered n = 1, 2, 3, etc. Electrons in lower numbered shells are closer to the nucleus and are lower in energy. Electrons in higher numbered shells are further from the nucleus and are higher in energy. 28  2.5 Electronic Structure Shells with larger numbers (n) are farther from the nucleus and can hold more electrons. The distribution of electrons in the first four shells: Number of Electrons Shell (n) in a Shell 4 32 3 18 increasing increasing number of energy 2 8 electrons 1 2 29  2.5 Electronic Structure Shells are divided into subshells, identified by the letters s, p, d, and f. The subshells consist of orbitals. An orbital is a region of space where the probability of finding an electron is high. Each orbital can hold two electrons. Subshell Number of Orbitals s 1 increasing p 3 energy d 5 f 7 30 2.5 Electronic Structure 31  2.5 Electronic Structure The s orbital has a spherical shape. The p orbital has a dumbbell shape. 32  2.6 Electron Configuration The electron configuration shows how the electrons are arranged in an atom’s orbitals. The ground state is the lowest energy arrangement. Rules to Determine the Ground State Electronic Configuration of an Atom Rule Electrons are placed in the lowest energy orbital beginning with the 1s orbital. Orbitals are then filled in order of increasing energy. 33  2.6 Electron Configuration Rules to Determine the Ground State Electronic Configuration of an Atom 34  Electron Configuration Rules to Determine the Ground State Electronic Configuration of an Atom Rule Each orbital holds a maximum of 2 electrons. Rule When orbitals are equal in energy: 1 electron is added to each orbital until all of the orbitals are half-filled. Then, the orbitals can be completely filled. 35  2.6 Electron Configuration Orbital Diagrams An orbital diagram uses a box to represent each orbital and arrows to represent electrons. an orbital a single, an electron unpaired pair electron Two electrons must have paired spins (opposite directions) to fit into the same orbital. 36  2.6 Electron Configuration A. First-Row Elements (Period 1) Orbital Electron Element Notation Configuration H (Z = 1) 1s1 1 electron 1s He (Z = 2) 1s2 2 electrons 1s 37  2.6 Electron Configuration B. Second-Row Elements (Period 2) Orbital Electron Element Notation Configuration Li (Z = 3) 1s22s1 3 electrons 1s 2s C (Z = 6) 1s22s22p2 6 electrons 1s 2s 2p Ne (Z = 10) 1s22s22p6 10 electrons 1s 2s 2p 38  2.6 Electron Configuration The electron configuration can be shortened by using Noble Gas Notation. Write the Symbol of the previous Noble Gas, then add the electronic configuration of the additional electrons. Electron Noble Gas Configuration Notation element: C 1s22s22p2 nearest He 1s2 noble gas: [He]2s22p2 39  2.6 Electron Configuration C. Other Elements Orbital Element Notation Ca 20 electrons 1s 2s 2p 3s 3p 4s 4s is lower in energy; it is filled before 3d. Noble Gas Electron Notation Configuration 1s22s22p63s23p64s2 [Ar]4s2 40  Electron Configurations and the Periodic Table FIGURE 2.8 The Blocks of Elements in the Periodic Table  2.7 Valence Electrons The chemical properties of an element depend on the number of electrons in the valence shell. The valence shell is the outermost shell (the highest value of n). The electrons in the valence shell are called valence electrons. Be Cl 1s22s2 1s22s22p63s23p5 valence shell: n = 2 valence shell: n = 3 # of # of valence electrons = 2 valence electrons = 7 42  2.7 Valence Electrons A. Relating Valence Electrons to Group Number Elements in the same group have similar electron configurations. Elements in the same group have the same number of valence electrons. The group number, 1A–8A, equals the number of valence electrons for the main group elements. The exception is He, which has only 2 valence electrons. The chemical properties of a group are therefore very similar. 43  2.7 Valence Electrons A. Relating Valence Electrons to Group Number Group number: 1A 2A 3A 4A 5A 6A 7A 8A Period 1: H He 1s1 1s2 Period 2: Li Be B C N O F Ne 2s1 2s2 2s22p1 2s22p2 2s22p3 2s22p4 2s22p5 2s22p6 Period 3: Na Mg Al Si P S Cl Ar 3s1 3s2 3s23p1 3s23p2 3s23p3 3s23p4 3s23p5 3s23p6  ACTIVITY Identify the total number of electrons, the number of valence electrons, and the name of the element with each electronic contfiguration 1s22s22p63s23p2 1s22s22p63s23p64s23d104p65s24d105p66s24f145d10 45  2.7 Valence Electrons B. Electron-Dot Symbols Dots representing valence electrons are placed on the four sides of an element symbol. Each dot represents one valence electron. For 1 to 4 valence electrons, single dots are used. With > 4 valence electrons, the dots are paired. Element: H C O Cl # of Valence electrons: 1 4 6 7 Electron-dot symbol: H C O C l 46  2.8 Periodic Trends A. Atomic Size The size of Increases atoms increases down a column, as the valence e− are farther from the nucleus. Decreases The size of atoms decreases across a row, as the number of protons in the nucleus increases, pulling the valence electrons in closer. 47  2.8 Periodic Trends B. Ionization Energy The ionization energy is the energy needed to remove an electron from a neutral atom. Na + energy Na+ + e– Ionization Decreases energies decrease down a column as the valence e− get farther away from Increases the positively charged nucleus. Ionization energies increase across a row as the number of protons in the nucleus increases. 48