Atoms & the Periodic Table. Chapter Outline. Elements
|
|
- Frank Fisher
- 5 years ago
- Views:
Transcription
1 Atoms & the Periodic Table Chapter Outline What is Atom? Chemical properties of Atoms: the Periodicity Isotopes Electrons in Atom: Quantum physics view Valence electrons and the Periodic Table 2 Elements each Element has a unique number of protons in its nucleus Atomic number: the number of Protons in the nucleus of an atom the elements are arranged on the Periodic Table in order of their atomic numbers each element has a unique Name and Symbol symbol either one or two letters one capital letter or one capital letter + one lower case 4 1
2 The Periodic Table of Elements 5 The Size of Atoms Atomic Mass Unit (amu): 1 amu = g Hydrogen the smallest atom mass of H atom= 1.67 x g ~ 1 amu volume of H atom = 2.1 x cm 3 6 Within an Atom Atoms = (Protons + Neutrons) + Electrons The nucleus (Protons + Neutrons) is only about cm in diameter yet with most of the mass of the atom The electrons move outside the nucleus with an average distance of about 10-8 cm the atom is neutral as #proton (#p) = #electron (#e) Nucleus Proton Neutron Electron 7 2
3 Comparison among Proton, Electron, Neutron Subatomic Particle Mass g Mass amu Location in atom Charge Symb ol Proton 1.67 x nucleus +1 p, p +, H + Electron 9 x ~0 empty space -1 e, e - Neutron 1.67 x nucleus 0 n, n 0 8 Isotopes The same element could have atoms with different masses Examples: 2 isotopes of chlorine atoms in nature: one weighs about 35 amu (Cl-35); another weighs about 37 amu (Cl-37) Carbon-12 (C-12) is much more abundant than C Isotopes all isotopes of an element: chemically identical undergo the exact same chemical reactions the same number of protons different masses due to different numbers of neutrons. Example: C-14 atom has eight neutrons; C-12 atom has six neutrons. identified by their mass numbers protons + neutrons 10 3
4 Isotopes Atomic Number (Z) Number of protons Mass Number (A) Protons + Neutrons Abundance = relative amount found in a sample Example: Cl-35 (75%) vs. Cl-37 (25%) 11 Isotopic Symbol Cl-35 has a mass number = 35, 17 protons and 18 neutrons (35-17). The symbol for this isotope would be 35 Cl 17 Atomic Symbol A = mass number Z = atomic number #neutrons = A - Z A X Z 12 Example: How many protons, neutrons, and electrons in an atom of 238 U 92 Isotopic symbol element atomic number #p #e #n Mass number = Atomic number (# protons, or #p) + #neutrons U = uranium Atomic Number = 92 #p = atomic number = 92 #e = #p = 92 Mass Number = #p + #n 238 = 92 + #n 146 = #n #proton = 92 #neutron = 146 #electron =
5 Write Isotopic symbol for the following two isotopes: a. Hydrogen isotope w/ 1 neutron b. Uranium isotope w/ 143 neutrons (#p + #n) #p Element 2 H U 14 Mass Number is Not the Same as Atomic Mass Atomic mass (or Atomic Weight) is an experimental number determined from all naturally occurring isotopes Mass number refers to the number of protons + neutrons in one isotope natural or man-made When given the relative abundance of all isotopes, we can find the Atomic mass 15 Example: Find the atomic weight of the element chlorine Information: exact mass number Cl-35 (34.97 amu), Cl-37 (36.97 amu); isotopic abundance Cl-35 (75.78%), Cl-37 (24.22%) Atomic weight = sum of weighted atomic mass from all isotopes Mass due to Cl-35 = amu Mass due to Cl-37 = amu Atomic weight = amu 16 5
6 The Modern Periodic Table Elements with similar chemical and physical properties are in the same column columns are called Groups or Families designated by a number and letter at top rows are called Periods each period shows the pattern of properties repeated in the next period 17 The Modern Periodic Table Main Group = Representative Elements = A groups Transition Elements = B groups all metals Bottom rows = Inner Transition Elements = Rare Earth Elements metals really belong in Period 6 & 7 18 Main group vs. Transition metals, Inner transition metals = Metal = Metalloid IA IIA = Nonmetal IIIA VIIIA IIIB VIIB VIIIB IB IIB 6
7 Metals: Physical vs. Chemical Properties solids at room temperature, except Hg reflective surface shiny conduct heat, electricity Malleable (can be shaped) Tend to Lose electrons and form Cations in reactions. Na Na + + e - about 75% of the elements are metals lower left on the table 20 Nonmetals: Physical vs. Chemical Properties Elements found in all 3 states poor conductors of heat or electricity solids are brittle Tend to gain electrons in reactions to become anions: Cl + e - Cl - upper right on the table except H 21 Metalloids: between Metals and Nonmetals show some properties of metals and some of nonmetals also known as semiconductors Properties of Silicon shiny conducts electricity does not conduct heat well brittle 22 7
8 = Alkali Metals = Alkaline Earth Metals = Noble Gases = Halogens = Lanthanides = Actinides = Transition Metals 23 = Transition Metals = Rare Earth Metals = Transuranium element U 24 Important Element - Hydrogen nonmetal colorless, diatomic gas H 2 very low melting point & density reacts with Nonmetals to form molecular compounds HCl is acidic gas H 2 O is a liquid reacts with Metals to form hydrides metal hydrides react with water to form H 2 Nickel-metal hydride (NiMH) used in rechargeable battery HX dissolves in water to form acids 25 8
9 Important Element - Carbon Three forms of pure carbon: Diamond: hardest substance in nature Graphite: soft and slippery solid Buckminsterfullerene: a molecule made of 60 (Images from public domain wikipedia.com) carbon atoms in a sphere 26 Important Element - Carbon Carbon atoms capable of forming robust bonds with many other elements and themselves. Examples: Small molecules: Butane, Sugar, Fatty acid, Vitamins Big molecules (Polymers): Starch, Kevlar, Teflon, Protein, and DNA 27 Group IA: Alkali Metals Usually Hydrogen is included All metals: soft, low melting points Flame tests Li = red, Na = yellow, K = violet Chemical Property: Very reactive. React with water to form basic (alkaline) solutions and H 2. releases a lot of heat Tend to form water soluble compounds, such as table salt and baking soda. colorless solutions lithium sodium potassium rubidium cesium 28 9
10 Group IIA: Alkali Earth Metals Physical properties: harder, higher melting, and denser than alkali metals flame tests Ca = red, Sr = red, Ba = yellow-green Chemical properties: reactive, but less than corresponding alkali metal form stable, insoluble oxides. oxides are basic = alkaline earth reactivity with water to form H 2, Be = none; Mg = steam; Ca, Sr, Ba = cold water beryllium magnesium calcium strontium barium 29 Group VIIA: Halogens nonmetals F 2 & Cl 2 gases; Br 2 liquid; I 2 solid all diatomic very reactive Cl 2, Br 2 react slowly with water Cl 2 + H 2 O HCl + HOCl (chlorine) react with metals to form ionic compounds HX all acids HF weak < HCl < HBr < HI fluorine chlorine bromine iodine 30 Group VIIIA: Noble Gases all gases at room temperature, very low melting and boiling points very unreactive, practically inert very hard to remove electron from or give an electron to 31 10
11 Atomic Orbitals Quantum Physicists including Schrödinger: Electrons move very fast around the nucleus Electrons show up with a particular probability at certain location of the atom Orbital: A region where the electrons show up a very high probability when it has a particular amount of energy generally set at 90 or 95% 32 Quantum-Mechanical Model: Quantum Numbers Three quantum numbers: quantize the energy Principal quantum number, n, specifies the main energy level for the orbital. Also called Shell Number. the higher n value, the higher energy of the electrons, the further away electrons are located from the nucleus 33 Quantum-Mechanical: Quantum Numbers Principal energy shell has one or more Subshells the number of subshells = the Principal quantum number n = 1, one subshell; n = 2, two subshells; n = 3, three subshells Subshell Quantum numbers: s, p, d, f each Subshell has orbitals with a particular shape the shape represents the probability map 90% probability of finding electron in that region 34 11
12 Shapes of Subshells s Orbital p Orbitals: p x, p y, p z d Orbitals 35 f orbitals Tro: Chemistry: A Molecular Approach, 2/e Shapes of f orbitals: 4f orbitals (downloaded from public domain) The coloration corresponds to the sign of function
13 Shells & Subshells 38 How does the 1s Subshell Differ from the 2s Subshell? 39 Subshells and Orbitals Among the subshells of a principal shell, slightly different energies for multielectron atoms, the subshells have different energies: s < p < d < f each subshell contains one or more Orbitals s : 1 orbital p : 3 orbitals d : 5 orbitals f : 7 orbitals within one subshell, different orbitals have the same energy. Example: 2p x, 2p y and 2p z 40 13
14 Electron Configurations Definition: The distribution of electrons into the various energy shells (n = 1,2,3, ) and subshells (s, p, d, f) in an atom in its ground state Each energy shell and subshell has a maximum number of electrons it can hold Subshell s = 2, p = 6, d = 10, f = 14 Shell n: 1 = 2e, 2 = 8e, 3 = 18e, 4 = 32e Electrons fill in the energy shells and subshells in order of energy, from low energy up Aufbau Principal ( Construction in German) 41 Energy 7s 6s 5s 4s 6p 5p 4p 3p 6 d 5d 4d 3d 5f 4f 3s 2p 2s 1s 42 Order of Subshell Filling in Ground State Electron Configurations 1. Diagram putting each energy shell on a row and listing the subshells, (s, p, d, f), for that shell in order of energy, (left-to-right) 2. draw arrows through the diagonals, looping back to the next diagonal each time 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 43 14
15 Spinning Electron(s) in Orbital Experiments showed Electrons spin on an axis generating their own magnetic field Pauli Exclusion Principle each Orbital may have a maximum of 2 electrons, with opposite spin Two electrons sharing the same orbital must have Opposite spins so there magnetic fields will cancel analogous to two bar magnets in parallel: only opposite alignment could stabilize each other. 44 Orbital Diagrams often an orbital as a square the electrons in that orbital as arrows the direction of the arrow represents the spin of the electron unoccupied orbital orbital with 1 electron orbital with 2 electrons 45 How electrons in an atom are filled into orbitals 1. How Electrons fill subshells with multiple orbitals 2. How Electrons fill subshells with higher n number first Energy level 7s 6d 7p 6p 5d 6s 5p 5s 4p 4s 3p 3s 2s 4d 2p 3d 5f 4f 1s 46 15
16 Filling the Orbitals in a Subshell with Electrons Energy shells fill from lowest energy to high Subshells fill from lowest energy to high s p d f Orbitals of the same subshell have the same energy. Three 2p orbitals; Five 3d orbitals Electrons prefer spreading out in orbitals of same subshell before they pair up in orbitals. Hund s Rule Example: 2p 3 _ _ _ instead of 47 Electron Configuration of Atoms in their Ground State Electron configuration: a listing of the subshells in order of filling with the number of electrons in that subshell written as a superscript Kr = 36 electrons = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 a shorthand way : use the symbol of the previous noble gas in [] for the inner electrons, then just write the last set Rb = 37 electrons = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 = [Kr]5s 1 48 Example: Ground State Orbital Diagram and Electron Configuration of Magnesium 1s 2 2s 2 2p 6 3s 2 = [Ne]3s 2 1s 2s 2p 3s 3p 49 16
17 Practice: Write Electron Configuration and Orbital Diagram for the following atoms at the Ground state Calcium Sulfur Potassium Phosphorus 50 Valence Electrons Definition: the electrons in all the subshells with the highest principal energy shell Example: electrons in bold Mg = [Ne]3s 2 O = [He]2s 2 2p 4 Br = [Ar]4s 2 3d 10 4p 5 Core electrons: electrons in lower energy shells Chemists have observed that one of the most important factors in the way an atom behaves, both chemically and physically, is the Number of Valence electrons 51 Valence Electrons Rb = 37 electrons = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 the highest principal energy shell that contains electrons is the 5 th : 1 valence electron + 36 core electrons Kr = 36 electrons = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 the highest principal energy shell that contains electrons is the 4 th : 8 valence electrons + 28 core electrons 52 17
18 Electrons Configurations and the Periodic Table 53 Electron Configurations from the Periodic Table Example: Be 2s 2 B 2s 2 2p 1 C 2s 2 2p 2 N 2s 2 2p 3 O 2s 2 2p 4 Elements in the same period (row) have Valence Electrons in the same principal energy shell. #Valence electrons increases by one from left to right Elements in the same group have the same #valence electron and they are same kind of subshell Example: IIA: Be 2s 2 Ca 3s 2 Sr 4s 2 Ba 5s 2 VIIA: F 2s 2 2p 5 Cl 3s 2 3p 5 Br 4s 2 4p 5 I 5s 2 5p 5 54 Electron Configuration & the Periodic Table Elements in the same Group have similar chemical and physical properties their valence shell electron configuration is the same No. Valence electrons for the main group elements is the same as the Group Number Example: Group IA: ns 1 ; Group IIIA: ns 2 np 1 Group VIIA: ns 2 np
19 s 1 s 2 Electron Configuration & the Periodic Table p 1 p 2 p 3 p 4 p 5 s 2 d 1 d 2 d 3 d 4 d 5 d 6 d 7 d 8 d 9 d 10 f 1 f 2 f 3 f 4 f 5 f 6 f 7 f 8 f 9 f 10 f 11 f 12 f 13 f 14 p 6 56 Electron Configuration from the Periodic Table Inner electron configuration = Noble gas of the preceding period Outer electron configuration: from the preceding Noble gas the next period (Subshells) Element the valence energy shell = the period number the d block is always one energy shell below the period number and the f is two energy shells below Electron Configuration from the Periodic Table 1A 2A 3s 2 3A 4A 5A 6A 7A P 3p 3 8A Ne P = [Ne]3s 2 3p 3 P has 5 valence electrons 58 19
20 Electron Configuration from the Periodic Table 1A 2A 4s 2 3d 10 3A 4A 5A 6A 7A As 4p 3 8A Ar As = [Ar]4s 2 3d 10 4p 3 As has 5 valence electrons 59 Electron configuration & Chemical Reactivity Chemical properties of the elements are largely determined by No. Valence electrons Why elements in groups? Since elements in the same column have the same #valence electrons, they show similar properties 60 Electron Configuration: Noble Gas Noble gases have 8 valence electrons except for He, which has only 2 electrons Noble gases are especially nonreactive He and Ne are practically inert The reason: the electron configuration of the noble gases is especially stable 61 20
21 Everyone Wants to Be Like a Noble Gas! Alkali Metals (Group 1A) have one more electron than the previous noble gas, [NG]ns 1 tend to lose their extra ONE electron, resulting in the same electron configuration as a noble gas forming a cation with a 1+ charge Na Na + Li Li + 62 Everyone Wants to Be Like a Noble Gas! Halogens (Group 7A) one fewer electron than the next noble gas: [NG]ns 2 np 5 Reactions with Metals: tend to gain an electron and attain the electron configuration of the next noble gas: [NG]ns 2 np 5 + 1e [NG]ns 2 np 6 forming an anion with charge 1-: Cl Cl - Reactions with Nonmetals: tend to share electrons so that each attains the electron configuration of a noble gas 63 Everyone Wants to Be Like a Noble Gas! Summary Alkali Metals as a group are the most reactive metals they react with many things and do so rapidly Halogens are the most reactive group of nonmetals one reason for their high reactivity: they are only ONE electron away from having a very stable electron configuration the same as a noble gas 64 21
22 Stable Electron Configuration And Ion Charge Metals: Cations by losing enough electrons to get the same electron configuration as the previous noble gas Nonmetals: Anions by gaining enough electrons to get the same electron configuration as the next noble gas Atom Atom s Electron Config Ion Ion s Electron Config Na [Ne]3s 1 Na + [Ne] Mg [Ne]3s 2 Mg 2+ [Ne] Al [Ne]3s 2 3p 1 Al 3+ [Ne] O [He]2s2p 4 O 2- [Ne] F [He]2s 2 2p 5 F - [Ne] 65 Trends in Atomic Size Down a group valence shell farther from nucleus effective nuclear charge fairly close Across a period (left to right) adding electrons to same valence shell effective nuclear charge increases valence shell held closer 66 Trends in Atomic Size 67 22
23 Metallic Character Metals malleable & ductile shiny, lusterous, reflect light conduct heat and electricity most oxides basic and ionic form cations in solution lose electrons in reactions oxidized Nonmetals brittle in solid state dull electrical and thermal insulators most oxides are acidic and molecular form anions and polyatomic anions gain electrons in reactions - reduced 68 Trends in Metallic Character 69 Ionization Energy (IE) In an atom, electrons ( - charge) are attracted to the nucleus ( + charge). Energy is required to remove the electron from an atom. Na + energy Na + + e - Neutral atom IE Cation Higher IE corresponds to lower Metallic property
24 Trends in Ionization Energy Decreases down a group valence shell farther from nucleus effective nuclear charge fairly close Increases across a period (left to right) adding electrons to same valence shell effective nuclear charge increases valence shell held closer 71 Electron Configuration Affects the Size of Atoms and Metallic Character: Within a Group Within the same Group, from top to bottom: As quantum number n increases for the valence electron(s) valence electron(s) further away from the nucleus Larger Atomic Radius weaker Coulombic force (electrostatic force) withholding valence electrons electrons easier to be lost Stronger metallic character 72 Electron Configuration Affects the Size of Atoms and Metallic Character: Over the Period Within the same Period (row), from left to right: Same quantum number n for the valence electron(s) As Nucleus has increasing number of protons (p + ) Stronger Coulombic force (electrostatic force) withholding valence electrons Valence Electrons closer the nuclues Smaller Atomic Radius Valence electrons harder to be lost Weaker metallic character 73 24
Why Patterns for Charges of Common Cations and Anions? Electrons in Atoms
Electrons in Atoms From Light to Energy of Electrons in Atom Quantum mechanical description of Atom 1. Principal quantum number: Shell 2. Orientation (shape) of : Subshell 3. Orbitals hold electrons with
More informationChapter 8. Periodic Properties of the Element
Chapter 8 Periodic Properties of the Element Mendeleev (1834 1907) Ordered elements by atomic mass Saw a repeating pattern of properties Periodic law when the elements are arranged in order of increasing
More informationATOMS AND ELEMENTS. Evolution of Atomic Theory
ATOMS AND ELEMENTS Chapter Four Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on the smallest
More informationLecture Presentation. Chapter 8. Periodic Properties of the Element. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 8 Periodic Properties of the Element Sherril Soman Grand Valley State University Nerve Transmission Movement of ions across cell membranes is the basis for the transmission
More informationChapter 4 Atoms and Elements
Atoms and Elements Experiencing Atoms Atoms are incredibly small, yet they compose everything. Atoms are the pieces of elements. Properties of the atoms determine the properties of the elements. 2 The
More informationTest Review # 4. Chemistry: Form TR4-5A 6 S S S
Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,
More informationCHAPTER NOTES CHAPTER 14. Chemical Periodicity
Goals : To gain an understanding of : 1. Electron configurations 2. Periodicity. CHAPTER NOTES CHAPTER 14 Chemical Periodicity The periodic law states that when the elements are arranged according to increasing
More informationChapter 4 Atoms Practice Problems
Chapter 4 Atoms Practice Problems 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Which of the following is a
More informationNotes: Unit 6 Electron Configuration and the Periodic Table
Name KEY Block Notes: Unit 6 Electron Configuration and the Periodic Table In the 1790's Antoine Lavoisier compiled a list of the known elements at that time. There were only 23 elements. By the 1870's
More informationThe Periodic Table and Periodic Trends
The Periodic Table and Periodic Trends The properties of the elements exhibit trends and these trends can be predicted with the help of the periodic table. They can also be explained and understood by
More informationCHAPTER 2 Atoms and the Periodic Table
CHAPTER 2 and the Periodic Table General, Organic, & Biological Chemistry Janice Gorzynski Smith CHAPTER 2: & the Periodic Table Learning Objectives:! Elemental Symbols! Metals vs Nonmetals vs Metalloids
More informationUNIT (2) ATOMS AND ELEMENTS
UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called
More informationChemistry B11 Chapter 3 Atoms
Chapter 3 Atoms Element: is a substance that consists of identical atoms (hydrogen, oxygen, and Iron). 116 elements are known (88 occur in nature and chemist have made the others in the lab). Compound:
More informationProfessor K. Section 8 Electron Configuration Periodic Table
Professor K Section 8 Electron Configuration Periodic Table Schrödinger Cannot be solved for multielectron atoms We must assume the orbitals are all hydrogen-like Differences In the H atom, all subshells
More informationTest Review # 4. Chemistry: Form TR4-9A
Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels
More informationCh 7: Periodic Properties of the Elements
AP Chemistry: Periodic Properties of the Elements Lecture Outline 7.1 Development of the Periodic Table The majority of the elements were discovered between 1735 and 1843. Discovery of new elements in
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationPeriodic Table Workbook
Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order
More informationOrganizing the Periodic Table
Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements
More informationMendeleev s Periodic Law
Mendeleev s Periodic Law Periodic Law When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically. Mendeleev s Periodic Law allows us to predict what
More informationChapter 8. Periodic Properties of the Elements
Chapter 8 Periodic Properties of the Elements Mendeleev (1834 1907) Ordered elements by atomic mass. Saw a repeating pattern of properties. Periodic Law When the elements are arranged in order of increasing
More informationDevelopment of the Periodic Table
Development of the Periodic Table John Newlands - Law of Octaves 1864 When arranged in order of atomic mass, every eighth element had similar properties. Dimitri Mendeleev / Lothar Meyer 1869 organized
More informationUnit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate
More informationChapter 7 Electron Configuration and the Periodic Table
Chapter 7 Electron Configuration and the Periodic Table Copyright McGraw-Hill 2009 1 7.1 Development of the Periodic Table 1864 - John Newlands - Law of Octaves- every 8 th element had similar properties
More informationPeriodic Table. Metalloids diagonal between metals and nonmetals. Have metallic and non-metallic properties
Chapter 6 Periodic Table Most elements are metals Metals are shiny, malleable, ductile, and good conductors of heat and electricity Most metals are solid at room temperature Non-metals in upper right corner,
More informationChapter 5 Review 1. The order of elements in the periodic table is based on a. the number of protons in the nucleus. b. the electric charge of the
Chapter 5 Review 1. The order of elements in the periodic table is based on a. the number of protons in the nucleus. b. the electric charge of the nucleus. c. the number of neutrons in the nucleus. d.
More informationElements and the Periodic Table
Chapter 7 Elements and the Periodic Table What are metals like? Think of things that are made with metals like aluminum, copper, iron, and gold. What do they have in common? They are usually shiny, and
More informationPERIODIC PROPERTIES OF THE ELEMENTS
PERIODIC PROPERTIES OF THE ELEMENTS DEVELOPMENT OF PERIODIC TABLE Elements in the same group generally have similar chemical properties. Properties are not identical, however. DEVELOPMENT OF PERIODIC TABLE
More informationDiscovery of Elements. Dmitri Mendeleev Stanislao Canizzaro (1860) Modern Periodic Table. Henry Moseley. PT Background Information
Discovery of Elements Development of the Periodic Table Chapter 5 Honors Chemistry 412 At the end of the 1700 s, only 30 elements had been isolated Included most currency metals and some nonmetals New
More informationNote that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom?
Atomic Structure and the Periodic Table Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on
More informationThe Periodic Law Similar physical and chemical properties recur periodically when the elements are listed in order of increasing atomic number.
The Periodic Law Similar physical and chemical properties recur periodically when the elements are listed in order of increasing atomic number. Each period ends with a completely filled outer shell that
More informationPrinciples of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationChapter 7. Periodic Properties of the Elements. Lecture Outline
Chapter 7. Periodic Properties of the Elements Periodic Properties of the Elements 1 Lecture Outline 7.1 Development of the Periodic Table The periodic table is the most significant tool that chemists
More informationCh. 7- Periodic Properties of the Elements
Ch. 7- Periodic Properties of the Elements 7.1 Introduction A. The periodic nature of the periodic table arises from repeating patterns in the electron configurations of the elements. B. Elements in the
More informationSulfur WHY IS THE PERIODIC TABLE IMPORTANT TO ME? CLASSIFICATION OF ELEMENTS PROPERTIES OF NON-METALS
WHY IS THE PERIODIC TABLE IMPORTANT TO ME? ELEMENTS AND THE PERIODIC TABLE SNCD The periodic table is the most useful tool to a chemist. You get to use it on every test. It organizes lots of information
More informationPeriodic Table of Elements
Periodic Table of Elements The Atomic Nucleus The nucleus is a small, dense region at the center of the atom. It consists of positive protons and neutral neutrons, so it has an overall positive charge.
More informationCHAPTER 2. Atoms,Elements, Periodic Table
CHAPTER Atoms,Elements, Periodic Table 1 Vocabulary Chemistry Science that describes matter its properties, the changes it undergoes, and the energy changes that accompany those processes Matter Anything
More informationPractice Periodic Table Review
Practice Periodic Table Review Name 1. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 2. Which electron configuration represents an atom in the
More informationChapter 2: Atoms and the Periodic Table
1. Which element is a nonmetal? A) K B) Co C) Br D) Al Ans: C Difficulty: Easy 2. Which element is a metal? A) Li B) Si C) Cl D) Ar E) More than one of the elements above are metals. 3. Which element is
More informationTest 3: Lab Safety, Measurements, Matter and Periodic Table
Name: Grade/Group: Subject: Chemistry-7 Teacher: Mrs. Raj Date: Test 3: Lab Safety, Measurements, Matter and Periodic Table Directions: Determine the best answer for each question. Circle your answer on
More informationThe orbitals in an atom are arranged in shells and subshells. orbital 3s 3p 3d. Shell: all orbitals with the same value of n.
Shells and Subshells The orbitals in an atom are arranged in shells and subshells. n=3 orbital 3s 3p 3d Shell: all orbitals with the same value of n n=3 3s 3p 3d Subshell: all orbitals with the same value
More informationChapter 2: Atoms and the Periodic Table
1. Which element is a nonmetal? A) K B) Co C) Br D) Al Ans: C Difficulty: Easy 2. Which element is a metal? A) Li B) Si C) Cl D) Ar E) More than one of the elements above is a metal. Ans: A Difficulty:
More informationUnit Five: The Periodic Table Ref:
Unit Five: The Periodic Table Ref: 10.11 11.2 11.4 History of P.T. Chlorine Bromine Iodine Dobrenier- (1829) Triads groups of three elements of similar chemical and physical properties. Cannizzarro (1860)
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationPeriodic Table Practice Questions
Periodic Table Practice Questions 1. Elements in the Periodic Table are arranged according to their (1) atomic number (3) relative activity (2) atomic mass (4) relative size 2. Elements in a given period
More informationNotes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
More informationMatter has mass and occupies space.
CHEM110 Week 2 Notes (Matter and Energy) Page 1 of 6 Matter has mass and occupies space. Periodic Table Chemists organize matter on the periodic table of the elements (See Week 1 Handout). The periodic
More informationTest Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass
Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following
More informationChapter 7 Periodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements The periodic table is one of the most useful tools available to chemists. Elements are arranged to emphasize the similarities and variations in properties.
More informationChapter 6: The Periodic Table
Chapter 6: The Periodic Table (Lecture Notes) Russian chemist Mendeleev proposed that properties of elements repeat at regular intervals when they are arranged in order of increasing atomic mass. He is
More informationChapter 6 - The Periodic Table and Periodic Law
Chapter 6 - The Periodic Table and Periodic Law Objectives: Identify different key features of the periodic table. Explain why elements in a group have similar properties. Relate the group and period trends
More informationChemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law
More informationChemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
More informationChapter 3: Electron Structure and the Periodic Law
Chapter 3: Electron Structure and the Periodic Law PERIODIC LAW This is a statement about the behavior of the elements when they are arranged in a specific order. In its present form the statement is:
More informationNUCLEAR MODEL. Electron cloud. Electron cloud. Nucleus. Nucleus
37 NUCLEAR MODEL - Atoms are mostly empty space - NUCLEUS, at the center of the atom, contains protons and neutrons. This accounts for almost all the mass of an atom - Electrons are located in a diffuse
More informationChapter 6 The Periodic Table
Chapter 6 The Periodic Table Section 6.1 Organizing the Elements OBJECTIVES: Explain how elements are organized in a periodic table. Section 6.1 Organizing the Elements OBJECTIVES: Compare early and modern
More informationChapter 5. Preview. Lesson Starter Objectives Mendeleev and Chemical Periodicity Moseley and the Periodic Law The Modern Periodic Table
Preview Lesson Starter Objectives Mendeleev and Chemical Periodicity Moseley and the Periodic Law The Modern Periodic Table Section 1 History of the Periodic Table Lesson Starter Share what you have learned
More information- Some properties of elements can be related to their positions on the periodic table.
186 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron
More informationPart I: Structure of Matter
Part I: Structure of Matter What is Matter? Matter is anything with mass and volume (occupies space). Matter is composed of atoms. Note: Atoms are different from cells. Cells are the basic unit of all
More informationUnit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS Review of Atomic Structure What is an atom? The smallest particle of an element that retains the properties of that
More informationA few elements, including copper, silver, and gold, have been known for thousands of years
A few elements, including copper, silver, and gold, have been known for thousands of years There were only 13 elements identified by the year 1700. Chemists suspected that other elements existed. As chemists
More informationPeriods: horizontal rows (# 1-7) 2. Periodicity the of the elements in the same group is explained by the arrangement of the around the nucleus.
The Modern Periodic Table 1. An arrangement of the elements in order of their numbers so that elements with properties fall in the same column (or group). Groups: vertical columns (#1-18) Periods: horizontal
More informationAtomic terms. Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus.
Atomic terms - ATOMIC NUMBER: The number of protons in the atomic nucleus. Each ELEMENT has the SAME NUMBER OF PROTONS in every nucleus. In neutral atoms, the number of ELECTRONS is also equal to the atomic
More informationChapter 7. Periodic Properties of the Elements. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 7 John D. Bookstaver St. Charles Community College Cottleville, MO Development of Table Dmitri Mendeleev and Lothar Meyer independently came to the same conclusion about how
More informationChapter 8. Mendeleev. Mendeleev s Predictions. Periodic Properties of the Elements
Chapter 8 Periodic Properties of the Elements Mendeleev Order elements by atomic mass Saw a repeating pattern of properties Periodic Law When the elements are arranged in order of increasing atomic mass,
More informationCHAPTER 2. Structure of the Atom. Atoms and Elements
CHAPTER 2 Atoms and Elements 1 Atoms Dalton s Atomic Theory - 1808 1. -Element is composed of small, indivisible particles called atoms. 2. -Atoms of an element have identical properties that differ from
More informationChapter 7. Periodic Properties. of the Elements
Chapter 7 7.1 Development of Table in the same group generally have similar chemical properties. Physical are not identical, however. Development of Table Dmitri Mendeleev and Lothar Meyer independently
More informationValence electron- Energy sublevel- Transition element- Period 10. Electronegativity- Alkaline earth metal- 11. Ion- Halogen- 12.
Mrs. Hilliard 1. Valence electron 2. Period 3. Alkaline earth metal 4. Halogen 5. Metalloid 6. Hund s Rule 7. Representative element 8. Energy sublevel 9. Transition element 10. Electronegativity 11. Ion
More informationAtomic Model and Periodic Table Test Review
Atomic Model and Periodic Table Test Review A. Give the family name for each description. 1. I have 1 electron on my outer shell. 2. One of the elements has 35 protons. 3. I have 2 electrons on my outer
More informationCh. 3 Answer Key. O can be broken down to form two atoms of H and 1 atom of O. Hydrogen and oxygen are elements.
Ch. 3 Answer Key 1. The Greeks believed that all matter is made of elements. We currently believe the same thing. However, the Greeks believed that there were 4 elements: earth, water, air and fire. Instead,
More informationPrinciples of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationThe Periodic Table. Atoms, Elements, and the Periodic Table
Atoms, Elements, and the Periodic Table Element: 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
More informationCHAPTER 3. Chemical Foundations
CHAPTER 3 Chemical Foundations 3.1 THE ELEMENTS 118 elements in 92 occur naturally, the rest are synthesized All matter in the universe can be chemically broken down into elements Compounds are made by
More informationChapter 7 Periodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements Development of Periodic Table Elements in the same group generally have similar chemical properties. Properties are not identical, however. Development of
More informationAtomic Structure. Ch 3 Prentice Hall
Atomic Structure Ch 3 Prentice Hall The Nuclear Atom By 1919 Rutherford concluded that the atom has a dense positive center called the nucleus containing what he called protons The electrons surround
More informationPeriodic Table Practice 11/29
Periodic Table Practice 11/29 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the
More informationPrinciples of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationUnit 2 Atomic Theory and Periodicity Review
Unit 2 Atomic Theory and Periodicity Review Section I: History In each box, write the name of the scientist(s) associated with the statement. Choose from among the following: Democritus Thomson Bohr Schroedinger
More informationAtomic Theory and Periodic Table Review: Answers Answers to Practice Multiple Choice Questions:
Atomic Theory and Periodic Table Review: Answers Answers to Practice Multiple Choice Questions: 1. c 11. b 21. a 31. d 41. b 51. d 61. a 71. b 81. d 2. b 12. a 22. b 32. b 42. d 52. b 62. d 72. a 82. c
More informationElectron Configuration! Chapter 5
Electron Configuration! Chapter 5 DO NOW - Finish coloring your periodic tables! (5 min) State at Room Temperature Appearance Conductivity Malleability and Ductility Metals - solid except for mercury
More informationUnit 02 Review: Atomic Theory and Periodic Table Review
Practice Multiple Choice Questions Unit 02 Review: Atomic Theory and Periodic Table Review 1. The number of neutrons in an atom of radioactive C 14 is: a) 6 c) 8 b) 12 d) 14 2. When a radioactive nucleus
More informationPeriodic Table. Modern periodic table
41 Periodic Table - Mendeleev (1869): --- When atoms are arranged in order of their atomic weight, some of their chemical and physical properties repeat at regular intervals (periods) --- Some of the physical
More informationSection 6-1 Notes. Organizing the Elements
Section 6-1 Notes Organizing the Elements Organizing the Elements As new elements were discovered chemists needed to find a logical way to organize them Properties of elements were used to sort them in
More information- Chapter 7 - Periodic Properties of the Elements
- Chapter 7 - Periodic Properties of the Elements Summary 7.1 Development of the periodic table 7.2 Effective nuclear charge 7.3 Size of atoms and ions 7.4 Ionization energy 7.5 Electron affinities 7.6
More informationPeriodic Table of Elements
Periodic Table of Elements chlorine nitrogen helium gold oxygen silver mercury hydrogen neodymium sodium niobium carbon Elements Science has come along way since Aristotle s theory of Air, Water, Fire,
More informationUnit 2 - Electrons and Periodic Behavior
Unit 2 - Electrons and Periodic Behavior I. The Bohr Model of the Atom A. Electron Orbits, or Energy Levels 1. Electrons can circle the nucleus only in allowed paths or orbits 2. The energy of the electron
More informationRegents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
More informationUNIT 5.1. Types of bonds
UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence
More informationUnit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016
Name: PRACTICE QUESTIONS Date: 2/23/2016 1. Which pair of symbols represents a metalloid and a noble gas? 1) Si and Bi 2) As and Ar 3) Ge and Te 4) Ne and Xe 2. What determines the order of placement of
More informationCHAPTER 6. Table & Periodic Law. John Newlands
CHAPTER 6 Table & Periodic Law 6.1 Developing a Periodic Table The periodic table was developed to show the properties of an element by simply looking at it's location. In 1860, chemists agreed on a way
More informationMendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the
Periodic Table Mendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the very stable copper, in the same family.
More informationPeriodic Table. Modern periodic table
41 Periodic Table - Mendeleev (1869): --- When atoms are arranged in order of their atomic weight, some of their chemical and physical properties repeat at regular intervals (periods) --- Some of the physical
More informationPeriodic Trends. Name: Class: Date: ID: A. Matching
Name: Class: Date: Periodic Trends Matching Match each item with the correct statement below. a. electronegativity f. periodic law b. ionization energy g. atomic mass c. atomic radius h. period d. metal
More informationIntroduction period group
The Periodic Table Introduction The periodic table is made up of rows of elements and columns. An element is identified by its chemical symbol. The number above the symbol is the atomic number The number
More informationChapter 3 Classification of Elements and Periodicity in Properties
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
More informationChapter 7 Electron Configuration and the Periodic Table
Chapter 7 Electron Configuration and the Periodic Table Copyright McGraw-Hill 2009 1 7.1 Development of the Periodic Table 1864 - John Newlands - Law of Octaves- every 8th element had similar properties
More informationAtomic structure. The subatomic particles. - a small, but relatively massive particle that carres an overall unit POSITIVE CHARGE
35 Atomic structure - Until the early 20th century, chemists considered atoms to be indivisible particles. - The discovery of SUBATOMIC PARTICLES changed the way we view atoms! PROTON NEUTRON ELECTRON
More information2/15/2013. Chapter 6 6.1
Chapter 6 In a self-service store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing products is easy. You will learn how elements
More informationPractice Packet Unit: 5 Periodic Table
Regents Chemistry: Practice Packet Unit: 5 Periodic Table 1 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help
More information