Chapter 4: Atoms and Elements
|
|
- Jordan Strickland
- 7 years ago
- Views:
Transcription
1 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 1 Chapter 4: Atoms and Elements Bonus Problems: 27, 29, 33, 35, 45, 51, 53, 67, 69, 73, 83, 87, 93, 95, 107, 109 Early Ideas on Matter: Philosophers (Chinese- yin/yang; Greeks-earth/wind/fire/water) speculated about the nature of stuff without relying on scientific evidence Leucippus (fifth century BC) and his student Democritus ( BC) first suggested the material world when broken down to the extreme would consist of tiny particles called atomos, meaning indivisible. Alchemists through the middle ages physically experimented with matter aiming to create gold from base metals and an elixir for everlasting life. Englishman Robert Boyle ( ) is generally credited as the first to study the separate science we call chemistry and the first to perform rigorous experiments. Antoine Lavoisier ( ) discovered the mass of combustion products exactly equals the mass of the starting reactants. Law of Mass Conservation (Law of Conservation of Matter); Mass is neither created nor destroyed in chemical reactions Joseph Proust ( ) studied copper carbonate, the two tin oxides, and the two iron sulfides. He made artificial copper carbonate and compared it to natural copper carbonate, showing that each had the same proportion of weights between the three elements involved (Cu, C, O). He showed that no intermediate indeterminate compounds exist between the two tin oxides or the two iron sulfides. Law of Definite Proportions (Law of Constant Composition); Elements combine together in specific proportions. All samples of a given compound, regardless of their source or how they were prepared have the same proportions of their constituent elements. These early ideas led to the foundation steps in atomic theory. Atomic theories explain the behavior of atoms. We will cover Dalton s Indivisible atom, J.J. Thomson s Plum Pudding model, Rutherford s Nuclear model of the atom, the Bohr s Quantum (orbit) model that mathematically only works for one electron systems and the Orbital Wave Mechanical model. The first three models are found in Chapter 4 while the last two are found in Chapters 9. You are to write a paper with references on these five models due Feb 14 th.
2 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 2 Dalton s Atomic Theory (1808): 1. Elements are composed of tiny, indivisible particles called atoms. 2. Atoms of a given element are identical in properties, but atoms of one element are different from the atoms of all other elements. 3. Compounds form when atoms of two or more different elements combine in whole number ratios. Chemical reactions do not create or destroy atoms, they are just rearranged. Dalton s atomic theory led to another scientific law Law of Multiple Proportions: When two elements form two different compounds, the masses of element (B) that combine with 1g of element (A) can be expressed as a ratio of small whole numbers. Example: CO(1 g C to 1.33 g O) vs CO 2 (1 g C to 2.67 g O) J. J. Thomson ( ); By the mid-1800 s new experiments gave data that was inconsistent with an indivisible atom. Cathode ray tubes (CRT) contain very low pressures of a gas and have high voltage passed through electrodes on either end. Experiments with CRT gave radiation that is negatively charged. The same negative charged substance that fluoresced (gave off light) was found using many different gases. By 1897, JJ Thomson published a paper that concluded the cathode rays are streams of negatively charged particles, later known as electrons.
3 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 3 Plum Pudding Model; This experiment led to a divisible neutral atom which must have both negative and positive charges. JJ Thomson called his atomic theory the Plum Pudding Model of the atom. A positive sphere like pudding contains particles (plums) of negatively charged electrons. Since the atom is neutral, there must be a positively charged electric field as well. Thomson assumed there were no positively charged particles since none showed up in the experiment. He predicted he mass of the atom comes from the mass of electrons. In 1909 Robert Millikin; Robert Millikin measured the charge of an electron ( x Coulombs) through an oil drop experiment performed numerous times over 5 tedious years. Using Thomson s charge to mass ratio ( x 10 8 C/g) the electron mass was accepted as x g, about 2000 times smaller than a single H atom. This caused the question: What is the major contributor of an atom s mass.
4 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 4 Ernest Rutherford ( ): In 1910 Ernest Rutherford created an experiment to test Thomson s Plum Pudding model, the gold foil experiment. The results showed that most of the heavy positive alpha particles passed right through a thin gold foil. Surprisingly, a small portion of alpha particles were deflected or even sent back. If Thomson s atomic model was correct, this would be similar to a rifle shot through tissue paper, and no bullet could be deflected. This led to Rutherford s Nuclear Model of the atom. The nuclear model has all the positive charge (protons) densely set in the center (nucleus) and the particles of electrons spread out in a cloud around the nucleus.
5 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 5 Neutrons: It did not make sense to have all the positive particles (protons) so close together in a nucleus, they would repel each other. Additionally, some mass was missing. One of Rutherford s students, James Chadwick ( ), proposed there are neutrons, neutral particles within the nucleus similar to protons. Neutrons were isolated later in Atomic Structure: What we have so far Particle Charge Mass (amu) Mass (g) Electron amu x g Proton amu x g Neutron amu x g 1 amu = x g Solve for the inverse of this number: amu = 1 g Atoms are extremely tiny with diameters around 1-5 x m: 1 angstrom = 1 x m All atoms are surrounded by a cloud of negatively charged electrons (-1). The nucleus contains almost all the mass of an atom. It is positively charged and contains protons (+1 ) and neutrons (0 charge) The nucleus is tiny with a diameter 10,000 times smaller than the atom. Example: a marble (nucleus) in the center of a large football stadium (atom). Neutral atoms have the same number of electrons and protons. Each chemical element (X) has a unique number of protons (atomic number, Z). The number of protons defines the element. Ions have more or less electrons than protons. Cations lose electrons, are positive (metals) Anions gain electrons, are negative (nonmetals) The number of neutrons may vary creating various isotopes. Isotopes are chemically identical. The protons plus neutrons is the Mass Number (A) Nuclide symbols indicate particular isotopes and ions. A Z X
6 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 6 Example 1: Fill in the nuclide symbols chart. Nuclide symbol, A Z X name protons neutrons electrons atomic mass carbon carbon Sulfide ion Potassium ion Periodic Table: Patterns and the Periodic Law Development: 1869 Dmitri Mendeleev (Russia) and Lothar Meyer (Germany) classified known elements (about 65 known at that time) and noted similar physical and chemical properties were found periodically when arranged by increasing atomic weight and grouped together by chemical reactivity. Several holes led to predictions of elements and their properties that were not yet discovered eka-aluminum (Ga) and eka-silicon (Ge). Periodic Law when the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically Ordered elements by atomic mass Put elements with similar properties in the same column Used pattern to predict properties of undiscovered elements Where atomic mass order did not fit other properties, he re-ordered by other properties Example: Te & I
7 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e Henry Moseley developed the concept of atomic numbers. He improved the periodic table by ordering the elements by increasing atomic number. More holes were found, which led to the discovery of more elements and the family of noble gases. The periodic table gives us a great amount of information in an organized manner. Vertical columns are called groups or families. If you are aware of the properties of a couple elements in a group, you can make a good guess at the properties of the other elements in the same group. Periods are the horizontal rows in the periodic table. Many patterns can be seen or predicted following periods and groups. Atomic Weights: The atomic mass scale is arbitrarily defined by international agreement and is based a standard isotope carbon-12, defining its mass to be exactly 12 amu. Weighted average atomic masses take into consideration the natural abundance of all the isotopes of an atom. Masses and isotopic abundances are measured by Mass Spectroscopy.
8 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 8 Mass Spectrum quantifies the results The mass spectrum for zirconium Isotopes: The 5 peaks in the mass spectrum shows that there are 5 isotopes of zirconium - with relative isotopic masses of 90, 91, 92, 94 and 96 on the 12 C scale. The abundance of the isotopes In this case, the 5 isotopes (with their relative percentage abundances) are: zirconium zirconium zirconium zirconium zirconium (This simple example rounds off much more than I generally accept.) Working out the relative atomic mass Using the equation Weighted Atomic Mass = (0.515 x 90)+(0.112 x 91)+(0.171 x 92)+(0.174 x 94)+(0.028 x 96) = 91.3 is the relative atomic mass of zirconium.
9 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 9 Mass: Simple vs. Weighted Average: Simple average: add all the numbers and divide by the count Solve for the simple average... Given: 12.0 g, 16.0 g, 17.0 g Weighted average: Mass = Weighted average takes into consideration the fractional abundance of each number. Fractional abundance is the decimal form of the percent abundance. All fractional abundance values add up to a total of one (1.00) so there is no reason to divide by the count. Solve for the weighted average Given: 12.0 g (80.0%), 16.0 g (15.0%), 17.0 g (5.0 %) Naturally occurring weighted masses for elements are found on the periodic table: Atomic mass = isotopic mass x fractional abundance Atomic mass = (mass A x fract. abund. A ) + (mass B x fract. abund. B ) + (. All the fractional abundance values add up to a total of one (1.00) Example 2: Use the weighted average to solve the average atomic mass found in nature for Si Given the following information on its naturally occurring isotopes Keep appropriate significant figures. 28 Si: amu 92.21% 29 Si: amu 4.70% 30 Si: amu 3.09%
10 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 10 Example 3: There are two naturally occurring isotopes of chlorine. Calculate the percent abundance of each isotope given the following information on the masses and given that the naturally occurring weighted atomic mass of chlorine is amu 35 Cl: amu (1-x) 37 Cl: amu (x) Periodic Table: Organization: family/group period metals nonmetals metalloids/semiconductors, Groups: Main Group Transition Metals Inner Transition Metals or Actinides and Lanthanides Alkali Metals Alkaline Earth Metals Halogens Noble Gas Coinage metals Others
11 C h e m i s t r y 1 2 C h 4 : A t o m s a n d E l e m e n t s P a g e 11 Preview of Chapter 5: Ions: Valence electrons (duet/octet rule) Cations Naming: Cations with known oxidation state of metal Group 1A (+1), 2A (+2), Al and Ga (+3), Zn and Cd (+2), Ag (+1) Name of ion is identical to the name of the atom for cations Variable oxidation state of metal Transition metals and metals below the nonmetal on the right have a variable oxidation state that must be indicated by Roman Numerals in parenthesis (this method is what I expect you to learn. Fe +3, iron (III); Fe +2, iron (II); Cu +1, copper (I); Sn +4, tin (IV) An alternative method differentiates from the higher oxidation number and lower oxidation number using the old form of the name and ic or ous as an ending respectively. (you are not responsible for knowing the ic and ous ending of metal cations) Fe +3, ferric Fe +2, ferrous; Cu +2, cupric; Cu +1, cuprous; Sn +4, stannic; Sn +2, stannous Anions Naming: Group VA (-3); VIA (-2), VIIA (-1) Name of the element root followed by ide. N -3, nitride; S -2, sulfide, Br -1, bromide Counting Atoms by Moles: Avogadro s number: x particles = 1 mole Converting atoms to moles Converting moles to atoms Molar Mass: Solving for molar mass of molecules and compounds O 2 H 2 O CoBr 3
ATOMS A T O M S, I S O T O P E S, A N D I O N S. The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39)
ATOMS A T O M S, I S O T O P E S, A N D I O N S The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39) THE ATOM All elements listed on the periodic table are made up of atoms.
More informationAtomic Theory: History of the Atom
Atomic Theory: History of the Atom Atomic Theory: experimental observations that led scientists to postulate the existence of the atom (smallest bit of an element). 1. Law of Conservation of Mass -During
More informationHistory of the Atom & Atomic Theory
Chapter 5 History of the Atom & Atomic Theory You re invited to a Thinking Inside the Box Conference Each group should nominate a: o Leader o Writer o Presenter You have 5 minutes to come up with observations
More information9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model.
John Dalton was an English scientist who lived in the early 1800s. Dalton s atomic theory served as a model for how matter worked. The principles of Dalton s atomic theory are: 1. Elements are made of
More informationAPS Science Curriculum Unit Planner
APS Science Curriculum Unit Planner Grade Level/Subject Chemistry Stage 1: Desired Results Enduring Understanding Topic 1: Elements and the Periodic Table: The placement of elements on the periodic table
More informationChapter 2 Atoms, Ions, and the Periodic Table
Chapter 2 Atoms, Ions, and the Periodic Table 2.1 (a) neutron; (b) law of conservation of mass; (c) proton; (d) main-group element; (e) relative atomic mass; (f) mass number; (g) isotope; (h) cation; (i)
More informationAtomic Calculations. 2.1 Composition of the Atom. number of protons + number of neutrons = mass number
2.1 Composition of the Atom Atomic Calculations number of protons + number of neutrons = mass number number of neutrons = mass number - number of protons number of protons = number of electrons IF positive
More informationChemistry - Elements Electron Configurations The Periodic Table. Ron Robertson
Chemistry - Elements Electron Configurations The Periodic Table Ron Robertson History of Chemistry Before 16 th Century Alchemy Attempts (scientific or otherwise) to change cheap metals into gold no real
More information2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai,
Ch1 1) Which of the following underlined items is not an intensive property? A) A chemical reaction requires 3.00 g of oxygen. B) The density of helium at 25 C is 1.64 10-4 g/cm3. C) The melting point
More informationElements, Atoms & Ions
Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Elements, Atoms & Ions Chapter 4 1 2 Elements Aims: To learn about the relative abundances of the elements,
More informationChemistry CP Unit 2 Atomic Structure and Electron Configuration. Learning Targets (Your exam at the end of Unit 2 will assess the following:)
Chemistry CP Unit 2 Atomic Structure and Electron Learning Targets (Your exam at the end of Unit 2 will assess the following:) 2. Atomic Structure and Electron 2-1. Give the one main contribution to the
More informationAtoms, Ions and Molecules The Building Blocks of Matter
Atoms, Ions and Molecules The Building Blocks of Matter Chapter 2 1 Chapter Outline 2.1 The Rutherford Model of Atomic Structure 2.2 Nuclides and Their Symbols 2.3 Navigating the Periodic Table 2.4 The
More informationAtoms, Ions and Molecules The Building Blocks of Matter
Atoms, Ions and Molecules The Building Blocks of Matter Chapter 2 1 Chapter Outline 2.1 The Rutherford Model of Atomic Structure 2.2 Nuclides and Their Symbols 2.3 Navigating the Periodic Table 2.4 The
More informationAtoms, Elements, and the Periodic Table (Chapter 2)
Atoms, Elements, and the Periodic Table (Chapter 2) Atomic Structure 1. Historical View - Dalton's Atomic Theory Based on empirical observations, formulated as Laws of: Conservation of Mass Definite Proportions
More informationSCH 3UI Unit 2 Outline Up to Quiz #1 Atomic Theory and the Periodic Table
Lesson Topics Covered SCH 3UI Unit 2 Outline Up to Quiz #1 Atomic Theory and the Periodic Table 1 Note: History of Atomic Theory progression of understanding of composition of matter; ancient Greeks and
More informationATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE
ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE Chapter 3 Vocabulary Words (27 words) Nucleus Atomic number Proton Mass number Neutron Isotopes Electron Atomic mass unit (amu) Energy level Average
More informationNOTES ON The Structure of the Atom
NOTES ON The Structure of the Atom Chemistry is the study of matter and its properties. Those properties can be explained by examining the atoms that compose the matter. An atom is the smallest particle
More information2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England
CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered
More informationPERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes.
1 PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes. Metal Nonmetal Scheme (based on physical properties) Metals - most elements are metals - elements on left
More informationChapter Five: Atomic Theory and Structure
Chapter Five: Atomic Theory and Structure 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 informationCHAPTER 4: ATOMS AND ELEMENTS
CHAPTER 4: ATOMS AND ELEMENTS Problems: 1-70 then after Chapter 9, complete 71-94, 103-104, 107-108, 113-114 4.1 Experiencing Atoms at Tiburon atom: smallest identifiable unit of an element All matter
More informationChemistry: The Periodic Table and Periodicity
Chemistry: The Periodic Table and Periodicity Name: per: Date:. 1. By what property did Mendeleev arrange the elements? 2. By what property did Moseley suggest that the periodic table be arranged? 3. What
More informationTro's "Introductory Chemistry", Chapter 4
1 Introductory Chemistry, 3 rd Edition Nivaldo Tro Atoms and Elements Opening figure showing a shore scene with molecules of O 2, N 2, triethyl amine (CH 3 CH 2 ) 3 N, and rocks made of silicates containing
More informationCHEM 1411 Chapter 5 Homework Answers
1 CHEM 1411 Chapter 5 Homework Answers 1. Which statement regarding the gold foil experiment is false? (a) It was performed by Rutherford and his research group early in the 20 th century. (b) Most of
More information2 The Structure of Atoms
CHAPTER 4 2 The Structure of Atoms SECTION Atoms KEY IDEAS As you read this section, keep these questions in mind: What do atoms of the same element have in common? What are isotopes? How is an element
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 informationElectrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set
Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You
More information47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.
More informationKEY for Unit 1 Your Chemical Toolbox: Scientific Concepts, Fundamentals of Typical Calculations, the Atom and Much More
KEY for Unit 1 Your Chemical Toolbox: Scientific Concepts, Fundamentals of Typical Calculations, the Atom and Much More The Modern Periodic Table The Periodic Law - when elements are arranged according
More informationChapter 2 Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions 1. Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ration of 3:1 by mass. In ethane,
More informationAtomic Theory Part 1
Atomic Theory Part 1 Reading: Ch 2 sections 1 6, 8 Homework: Chapter 2: 39, 47, 43, 49, 51*, 53, 55, 57, 71, 73, 77, 99, 103 (optional) * = important homework question The Atomic Theory (John Dalton, 1803)
More informationEXPERIMENT 4 The Periodic Table - Atoms and Elements
EXPERIMENT 4 The Periodic Table - Atoms and Elements INTRODUCTION Primary substances, called elements, build all the materials around you. There are more than 109 different elements known today. The elements
More informationObjectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory
PAM1014 Introduction to Radiation Physics Basic Atomic Theory Objectives Introduce and Molecules The periodic Table Electronic Energy Levels Atomic excitation & de-excitation Ionisation Molecules Constituents
More informationChemistry. The student will be able to identify and apply basic safety procedures and identify basic equipment.
Chemistry UNIT I: Introduction to Chemistry The student will be able to describe what chemistry is and its scope. a. Define chemistry. b. Explain that chemistry overlaps many other areas of science. The
More information3 CHEMICAL FOUNDATIONS: ELEMENTS, ATOMS AND IONS
3 CHEMICAL FOUNDATIONS: ELEMENTS, ATOMS AND IONS All matter is built up from chemical combinations of elements. As of 2003, there are 114 known elements, of which 88 are naturally occurring; the remaining
More informationCHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004. Name (print) SSN
CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004 Name (print) SSN Pledge: I have neither given nor received aid on this exam: Signature For ALL problems: SHOW ALL WORK TO GET FULL CREDIT
More information( + and - ) ( - and - ) ( + and + ) Atoms are mostly empty space. = the # of protons in the nucleus. = the # of protons in the nucleus
Atoms are mostly empty space Atomic Structure Two regions of every atom: Nucleus - is made of protons and neutrons - is small and dense Electron cloud -is a region where you might find an electron -is
More informationAtomic Structure Chapter 5 Assignment & Problem Set
Atomic Structure Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Atomic Structure 2 Study Guide: Things You Must Know Vocabulary (know the definition
More informationFor convenience, we may consider an atom in two parts: the nucleus and the electrons.
Atomic structure A. Introduction: In 1808, an English scientist called John Dalton proposed an atomic theory based on experimental findings. (1) Elements are made of extremely small particles called atoms.
More informationChapter 5 Periodic Table. Dmitri Mendeleev: Russian Chemist credited with the discovery of the periodic table.
Chapter 5 Periodic Table Dmitri Mendeleev: Russian Chemist credited with the discovery of the periodic table. How did he organize the elements? According to similarities in their chemical and physical
More information4.1 Studying Atom. Early evidence used to develop models of atoms.
4.1 Studying Atom Early evidence used to develop models of atoms. Democritus said that all matter consisted of extremely small particles that could NOT be divided called these particles atoms from the
More informationChapter 1: Moles and equations. Learning outcomes. you should be able to:
Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including
More informationEARLY ATOMIC THEORY AND STRUCTURE
CHAPTER 5 EARLY ATOMIC THEORY AND STRUCTURE SOLUTIONS TO REVIEW QUESTIONS 1. Elements are composed of indivisable particles called atoms. Atoms of the same element have the same properties; atoms of different
More informationWoods Chem-1 Lec-02 10-1 Atoms, Ions, Mole (std) Page 1 ATOMIC THEORY, MOLECULES, & IONS
Woods Chem-1 Lec-02 10-1 Atoms, Ions, Mole (std) Page 1 ATOMIC THEORY, MOLECULES, & IONS Proton: A positively charged particle in the nucleus Atomic Number: We differentiate all elements by their number
More informationPERIODIC TABLE OF THE ELEMENTS
PERIODIC TABLE OF THE ELEMENTS Periodic Table: an arrangement of elements in horizontal rows (Periods) and vertical columns (Groups) exhibits periodic repetition of properties First Periodic Table: discovered
More informationChapter 3. Elements, Atoms, Ions, and the Periodic Table
Chapter 3. Elements, Atoms, Ions, and the Periodic Table The Periodic Law and the Periodic Table In the early 1800's many elements had been discovered and found to have different properties. In 1817 Döbreiner's
More information3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur?
PSI AP Chemistry Periodic Trends MC Review Name Periodic Law and the Quantum Model Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06
More informationStructure and Properties of Atoms
PS-2.1 Compare the subatomic particles (protons, neutrons, electrons) of an atom with regard to mass, location, and charge, and explain how these particles affect the properties of an atom (including identity,
More informationUntitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?
Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core
More informationModels of the Atom and periodic Trends Exam Study Guide
Name 1. What is the term for the weighted average mass of all the naturally occurring isotopes of an element? ans: atomic mass 2. Which is exactly equal to 1/12 the mass of a carbon -12 atom? ans: atomic
More informationThe Models of the Atom
The Models of the Atom All life, whether in the form of trees, whales, mushrooms, bacteria or amoebas, consists of cells. Similarly, all matter, whether in the form of aspirin, gold, vitamins, air or minerals,
More informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
Introduction to Chemistry Exam 2 Practice Problems 1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1.Atoms consist principally of what three
More information******* KEY ******* Atomic Structure & Periodic Table Test Study Guide
Atomic Structure & Periodic Table Test Study Guide VOCABULARY: Write a brief definition of each term in the space provided. 1. Atoms: smallest unit of an element that has all of the properties of that
More informationThe Structure of the Atom
The Structure of the Atom Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Section 4. Early Ideas About Matter pages 02 05 Section 4. Assessment page 05. Contrast the methods
More informationTrends of the Periodic Table Diary
Trends of the Periodic Table Diary Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the
More informationDevelopment of the Atomic Theory
Development of the Atomic Theory Atom The smallest particle into which an element can be divided and still be the same substance. Element A pure substance that cannot be separated into simpler substances
More informationUnit 2 Periodic Behavior and Ionic Bonding
Unit 2 Periodic Behavior and Ionic Bonding 6.1 Organizing the Elements I. The Periodic Law A. The physical and chemical properties of the elements are periodic functions of their atomic numbers B. Elements
More informationMODERN ATOMIC THEORY AND THE PERIODIC TABLE
CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is generally symbolized by the Greek
More informationThe Periodic Table: Periodic trends
Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has
More informationChapter 3, Elements, Atoms, Ions, and the Periodic Table
1. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements? Ans. Mendeleev and Meyer 2. Who stated that the
More informationUnit 3.2: The Periodic Table and Periodic Trends Notes
Unit 3.2: The Periodic Table and Periodic Trends Notes The Organization of the Periodic Table Dmitri Mendeleev was the first to organize the elements by their periodic properties. In 1871 he arranged the
More information2 ATOMIC SYSTEMATICS AND NUCLEAR STRUCTURE
2 ATOMIC SYSTEMATICS AND NUCLEAR STRUCTURE In this chapter the principles and systematics of atomic and nuclear physics are summarised briefly, in order to introduce the existence and characteristics of
More information5.1 Evolution of the Atomic Model
5.1 Evolution of the Atomic Model Studying the atom has been a fascination of scientists for hundreds of years. Even Greek philosophers, over 2500 years ago, discussed the idea of there being a smallest
More informationUnit 3 Study Guide: Electron Configuration & The Periodic Table
Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.
More information6.7: Explaining the Periodic Table pg. 234
Unit C: Atoms, elements, and Compounds 6.7: Explaining the Periodic Table pg. 234 Key Concepts: 3. Elements are organized according to their atomic number and electron arrangement on the periodic table.
More informationAnswers to Review Questions for Atomic Theory Quiz #1
Answers to Review Questions for Atomic Theory Quiz #1 Multiple Choice Questions: 1. c 7. a 13. c 19. a 25. b 31. b 37. a 43. d 2. d 8. c 14. c 20. c 26. d 32. c 38. d 44. b 3. b 9. a 15. b 21. c 27. b
More informationPeriodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More informationCopyrighted by Gabriel Tang B.Ed., B.Sc.
Chapter 8: The Periodic Table 8.1: Development of the Periodic Table Johann Dobereiner: - first to discover a pattern of a group of elements like Cl, Br, and I (called triads). John Newland: - suggested
More information7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions
7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams
More informationCHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING
CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING Essential Standard: STUDENTS WILL UNDERSTAND THAT THE PROPERTIES OF MATTER AND THEIR INTERACTIONS ARE A CONSEQUENCE OF THE STRUCTURE OF MATTER,
More informationUnit 1 Practice Test. Matching
Unit 1 Practice Test Matching Match each item with the correct statement below. a. proton d. electron b. nucleus e. neutron c. atom 1. the smallest particle of an element that retains the properties of
More informationLevel 3 Achievement Scale
Unit 1: Atoms Level 3 Achievement Scale Can state the key results of the experiments associated with Dalton, Rutherford, Thomson, Chadwick, and Bohr and what this lead each to conclude. Can explain that
More informationCHAPTER 2 ATOMS AND THE ATOMIC THEORY
1A 1B 2A 2B A CHAPTER 2 ATOMS AND THE ATOMIC THEORY PRACTICE EXAMPLES The total mass must be the same before and after reaction. mass before reaction = 0.82 g magnesium + 2.652 g nitrogen =.04 g mass after
More informationReview for Atomic Theory Quiz #1
Review for Atomic Theory Quiz #1 Practice Multiple Choice Questions: 1. Which of the following is/are quantitative physical property(s) of matter? a) mass c) density b) volume d) all of the above 2. Which
More informationChapter 2 Atoms and Molecules
Chapter 2 Atoms and Molecules 2-1 Elements and their symbols Most of the chemicals you find in everyday life can be broken down into simper substances Key Concepts: A substance that cannot be broken down
More informationAtoms and Elements. Outline Atoms Orbitals and Energy Levels Periodic Properties Homework
Atoms and the Periodic Table The very hot early universe was a plasma with cationic nuclei separated from negatively charged electrons. Plasmas exist today where the energy of the particles is very high,
More informationPeriodic Table Questions
Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is
More informationIntroduction to Chemistry
1 Copyright ç 1996 Richard Hochstim. All rights reserved. Terms of use. Introduction to Chemistry In Chemistry the word weight is commonly used in place of the more proper term mass. 1.1 Atoms, Ions, and
More informationAAHS-CHEMISTRY FINAL EXAM PREP-REVIEW GUIDE MAY-JUNE 2014 DR. GRAY CLASS OF 2016
AAHS-CHEMISTRY FINAL EXAM PREP-REVIEW GUIDE MAY-JUNE 2014 DR. GRAY CLASS OF 2016 UNIT I: (CHAPTER 1-Zumdahl text) The Nature of Science and Chemistry 1. Explain why knowledge of chemistry is central to
More informationMolecular Models & Lewis Dot Structures
Molecular Models & Lewis Dot Structures Objectives: 1. Draw Lewis structures for atoms, ions and simple molecules. 2. Use Lewis structures as a guide to construct three-dimensional models of small molecules.
More informationB) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
More informationSCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni
SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni Which metal in the list above has the most metallic character? Explain. Cesium as the
More informationCHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals
CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying
More informationCH3 Stoichiometry. The violent chemical reaction of bromine and phosphorus. P.76
CH3 Stoichiometry The violent chemical reaction of bromine and phosphorus. P.76 Contents 3.1 Counting by Weighing 3.2 Atomic Masses 3.3 The Mole 3.4 Molar Mass 3.5 Percent Composition of Compounds 3.6
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationAbout the course GENERAL CHEMISTRY. Recommended literature: Chemistry: science of the matter. Responsible for the course: Dr.
About the course GENERAL CHEMISTRY University of Pécs Medical School Academic year 2009-2010. Responsible for the course: Dr. Attila AGÓCS Optional course for 2 credit points. To have grade at the and
More informationThe Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of
The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of the periodic table. Describe the modern periodic table.
More informationTHE PERIODIC TABLE O F T H E E L E M E N T S. The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27)
THE PERIODIC TABLE O F T H E E L E M E N T S The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27) THE PERIODIC TABLE In 1872, Dmitri Mendeleev created the periodic table arranged
More informationThe Advanced Placement Examination in Chemistry. Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010
The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010 Atomic Theory and Periodicity Part I 1984 1. Which of
More informationNuclear Structure. particle relative charge relative mass proton +1 1 atomic mass unit neutron 0 1 atomic mass unit electron -1 negligible mass
Protons, neutrons and electrons Nuclear Structure particle relative charge relative mass proton 1 1 atomic mass unit neutron 0 1 atomic mass unit electron -1 negligible mass Protons and neutrons make up
More informationChapter 5 TEST: The Periodic Table name
Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based
More informationPeriodic Table Trends in Element Properties Ron Robertson
Periodic Table Trends in Element Properties Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\ch9trans2.doc The Periodic Table Quick Historical Review Mendeleev in 1850 put together
More informationChapter Test. Teacher Notes and Answers 5 The Periodic Law TEST A 1. b 2. d 3. b 4. b 5. d 6. a 7. b 8. b 9. b 10. a 11. c 12. a.
Assessment Chapter Test A Teacher Notes and Answers 5 The Periodic Law TEST A 1. b 2. d 3. b 4. b 5. d 6. a 7. b 8. b 9. b 10. a 11. c 12. a 13. c 14. d 15. c 16. b 17. d 18. a 19. d 20. c 21. d 22. a
More informationChapter 7. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 7 John D. Bookstaver St. Charles Community College Cottleville, MO Development of Table
More informationChapter 4: Elements and the Periodic Table Development of atomic theory
Chapter 4: Elements and the Periodic Table Development of atomic theory Name Date Theory Experiment Democritus 400 BC atomos smallest particle none, philosophical argument Aristotle 350 BC hyle continuous
More informationSample Exercise 2.1 Illustrating the Size of an Atom
Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side
More informationChapter 7 Periodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements 1. Elements in the modern version of the periodic table are arranged in order of increasing. (a). oxidation number (b). atomic mass (c). average atomic mass
More informationIntroduction to Chemistry. Course Description
CHM 1025 & CHM 1025L Introduction to Chemistry Course Description CHM 1025 Introduction to Chemistry (3) P CHM 1025L Introduction to Chemistry Laboratory (1) P This introductory course is intended to introduce
More informationChapter Outline. 3 Elements and Compounds. Elements and Atoms. Elements. Elements. Elements 9/4/2013
3 Elements and Compounds Chapter Outline 3.1 Elements A. Distribution of Elements Foundations of College Chemistry, 14 th Ed. Morris Hein and Susan Arena Copyright This reclining Buddha in Thailand is
More information