Answer Sheet Quarterly Review Questions
|
|
- Richard Morton
- 7 years ago
- Views:
Transcription
1 Answer Sheet Quarterly Review Questions 1. Compared to the charge and mass of a proton, an electron has a. the same charge and a smaller mass b. the same charge and the same mass c. an opposite charge and a smaller mass d. an opposite charge and the same mass Explanation: Protons are positively charged and have a mass of amu; electrons are negatively charged and have a mass of amu. See Table O. 2. When alpha particles are used to bombard gold foil, most of the alpha particles pass through undeflected. This result indicates that most of the volume of a gold atom consists of. a. deuterons b. neutrons c. protons d. unoccupied space Explanation: Because most of the particles do not hit anything (pass right through), one can infer the atom is mostly empty space. See hyperlink for more details. 3. A proton has approximately the same mass as a. a neutron b. an alpha particle c. a beta particle d. an electron Explanation: A proton has the same mass as a neutron. An electron has the same mass as a beta particle. An alpha particle has a mass of 4: two protons plus two neutrons. See Ref. Table O. 4. When electrons in an atom in an excited state fall to lower energy levels, energy is a. absorbed, only b. released, only c. neither released nor absorbed d. both released and absorbed Explanation: The ground state is the lowest energy state. To raise the atom to an excited state, energy must be added. To fall back to the ground state (lowest energy), the energy it had absorbed must be released. 5. A neutron has approximately the same mass as a a. an alpha particle b. a beta particle c. an electron d. a proton Explanation: See Reference table O. Protons and neutrons each have a mass of 1 amu. 6. Which symbols represent atoms that are isotopes? a. C-14 and N-14 b. O-16 and O-18 c. I-131 and I-131 d. Rn-222 and Ra-222 Explanation: Isotopes are atoms of the same element (same atomic number) but with a different number of neutrons (different atomic mass). Only choice 2 is correct. Choice 1: C and N are not the same elements. Choice 3: both are the same element but there is no difference in mass. Therefore, they are not isotopes. Choice 4: not the same elements. 7. Which element's ionic radius is smaller than its atomic radius? a. neon b. nitrogen c. sodium d. sulfur Explanation: Elements that lose electrons form positive ions that are smaller than atoms of the same element. Therefore the ionic radius of these ions is smaller than its atomic radius. Only choice 3, sodium, is a metal that will lose electrons. Neon is stable and will neither lose nor gain electrons. N and S will tend to gain electrons, each having a larger ionic radius than atomic radius. 8. Which atom contains exactly 15 protons? a. P-32 b. S-32 c. O-15
2 d. N-15 Explanation: An atom with 15 protons also has an atomic number of 15. Refer to the Periodic Table for element 15 (phosphorus). 9. An ion with 5 protons, 6 neutrons, and a charge of 3+ has an atomic number of a. 5 b. 6 c. 8 d. 11 Explanation: The number of protons is the same as the atomic number. There are 5 protons so the atomic number is also What is the mass number of an atom which contains 28 protons, 28 electrons, and 34 neutrons? a. 28 b. 56 c. 62 d. 90 Explanation: Atomic mass is found by adding protons plus neutrons = 62. Electrons have a mass of nearly 0 so they are not counted in the formula for atomic mass. 11. Which three groups of the Periodic Table contain the most elements classified as metalloids (semimetals)? a. 1, 2, and 13 b. 2, 13, and 14 c. 14, 15, and 16 d. 16, 17, and 18 Explanation: Go to the Periodic Table and note the location of the stepped line dividing metals and nonmetals. Elements next to the left or right of this line are metalloids. Choice three includes 5 metalloids. 12. Which element has the highest first ionization energy? a. sodium b. aluminum c. calcium d. phosphorus Explanation: See Ref. Table S. Phosphorus (P) has a first ionization energy of 1012 kj/mol. 13. Which compound forms a colored aqueous solution? a. CaCl2 b. CrCl3 c. NaOH d. KBr Explanation: Colored aqueous solutions are a characteristic of transition compounds. The only transition compound in the above choices is CrCl3. Cr is a transition element. 14. When a metal atom combines with a nonmetal atom, the nonmetal atom will a. lose electrons and decrease in size b. lose electrons and increase in size c. gain electrons and decrease in size d. gain electrons and increase in size Explanation: Metals tend to lose electrons (becoming smaller ions) while nonmetals tend to gain electrons and become larger ions. 15. According to Reference Table S, which of the following elements has the smallest atomic radius? a. nickel b. cobalt c. calcium d. potassium Explanation: With a radius of 124, nickel has the smallest atomic radius of the elements given. 16. Which element in Group 15 has the strongest metallic character? a. Bi b. As c. P d. N Explanation: From left to right across the period, metallic character decreases. But it increases going down a group (last element in a group will have the most metallic character). Bi is the last element in group 15 so it is the most metallic. 17. Which halogens are gases at STP?
3 a. chlorine and fluorine b. chlorine and bromine c. iodine and fluorine d. iodine and bromine Explanation: Iodine is a solid and bromine is a liquid. The gaseous halogens are chlorine and fluorine. 18. When combining with nonmetallic atoms, metallic atoms generally will a. lose electrons and form negative ions b. lose electrons and form positive ions c. gain electrons and from negative ions d. gain electrons and form positive ions Explanation: Metals tend to lose electrons and form positive ions. A neutral atom of Li has 3 protons (+) and 3 electrons (-). If it loses an electron, the Li atom now has +3 and -2 or a net charge of +1. Metals also have low electronegativities and low ionization energies. 19. Which set of elements contains a metalloid? a. K, Mn, As, Ar b. Li, Mg, Ca, Kr c. Ba, Ag, Sn, Xe d. Fr, F, O, Rn Explanation: Go to the Periodic Table and note the location of the stepped line dividing metals and nonmetals. Elements next to the left or right of this line are metalloids. As (Arsenic) is a metalloid. 20. Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms' a. number of principal energy levels b. number of valence electrons c. atomic numbers d. atomic masses Explanation: Most of the time elements in the same group have the same number of valence electrons. Valence electrons are involved in bonding and this effects how elements react and determines their chemical properties. See also question #11, topic: Nuclear Chemistry. 21. As atoms of elements in Group 16 are considered in order from top to bottom, the electronegativity of each successive element a. decreases b. increases c. remains the same Explanation: See Ref. Table S. 22. The first ionization energy of an element is 736 kj per mole of atoms. An atom of this element in the ground state has a total of how many valence electrons? a. 1 b. 2 c. 3 d. 4 Explanation: Use Ref. Table S. 736 kj/mol is the value for Mg. Use the Periodic Table to find Mg. It has 2 valence electrons. 23. An atom of which of the following elements has the greatest ability to attract electrons? a. silicon b. sulfur c. nitrogen d. chlorine Explanation: See Ref. Table S. Electronegativity is a measure of the ability of an atom to attract electrons. The greater the ability to attract, the higher the electronegativity. Chlorine has the highest electronegativity of the choices given. 24. At STP, which substance is the best conductor of electricity? a. nitrogen b. neon c. sulfur d. silver Explanation: The best conductors of electricity are metals. Silver is a metal, the others are nonmetals. 25. Which metal is obtained commercially by the electrolysis of salt? a. Zn
4 b. K c. Fe d. Ag Explanation: See Ref. Table J. Metals, including K, listed near the top of Table J occur as compounds in nature. The pure, uncombined form of these metals results from commercial electrolysis of salt. Notice that these metals (Mg, Na, Ca, Ba, Cs, K, Rb and Li) are either alkali metals or alkaline earth metals, the most reactive metals. You would not expect to find these very active metals uncombined. Au can be found in nuggets and dust. (Remember the California gold rush and the silver mines in Nevada?) but you will not find "nuggets" of alkali or alkaline metals in nature. See also #16, this topic. 26. Which element can be found in nature in the free (uncombined) state? a. Ca b. Ba c. Au d. Al Explanation: Remember the Gold Rush? Gold is found as dust or nuggets uncombined in nature. See Ref. Table J. Metals listed near the bottom are rarely found combined with other elements (Au or gold is found at the bottom of the table). However the metals near the top of Table J occur as compounds in nature. The pure, uncombined form of these metals results from commercial processing. See also #15, this topic. 27. Which formula represents a molecular substance? a. CaO b. CO c. Li2O d. Al2O3 Explanation: Use Ref. Table S to determine the electronegativity difference of each of the choices. The difference between C (2.6) and O (3.4) is 0.9 or in the range of covalent bonding (covalent bonds have electronegativity differences of less than 1.7). The other three compounds have differences in the ionic bond range or over Which sequence of Group 18 elements demonstrates a gradual decrease in the strength of the Van der Waals forces? All the choices are elements in the liquid state. a. Ar, Kr, Ne, Xe b. Kr, Xe, Ar, Ne c. Ne, Ar, Kr, Xe d. Xe, Kr, Ar, Ne Explanation: Van der Waals forces are weak forces of attraction between molecules. These forces decrease as the molecule gets smaller and increase as the molecule increases. Look at the periodic table and notice how in answer 4, the elements are getting smaller. Therefore the Van der Waals forces would also be decreasing. 29. Which substance is an example of a network solid? a. nitrogen dioxide b. sulfur dioxide c. carbon dioxide d. silicon dioxide Explanation: Only silicon dioxide forms a network solid, a network of covalent bonds extending throughout the crystal without forming a molecule. 30. Which combination of atoms can form a polar covalent bond? a. H and H b. H and Br c. N and N d. Na and Br Explanation: See Reference Table S. The electronegativity difference between H (2.1) and Br (3.0) is 0.9. If the difference is less than 1.7 (but not zero, usually more than 0.4), a polar covalent bond is formed. A nonpolar covalent bond is formed when the difference is close to zero (usually up to 0.4). If the difference is more than 1.7, an ionic bond is formed. 31. A strontium atom differs from a strontium ion in that the atom has a greater
5 a. number of electrons b. number of protons c. atomic number d. mass number Explanation: Strontium has 2 valence electrons in its outer shell. It is easier to lose these 2 electrons than it is to gain 6 more electrons. Losing 2 electrons will give the strontium ion a charge of +2. Ions are charged atoms. An neutral atom has no charge because it has the same number of protons and electrons. An ion can have more or less electrons than an atom of the same element does. A strontium atom would have 2 more electrons than a strontium ion. 32. Which bond has the greatest ionic character? a. H---CL b. H---F c. H---O d. H---N Explanation: See Ref. Table S. H has an electronegativity of 2.1 and F has an electronegativity of 4.0. Subtract the two values and the difference is 1.9. Ionic bonds have differences of 1.7 or greater. Find the electronegativity differences for the other choices. H--F has the greatest difference and is the most ionic of the choices. 33. A compound differs from a mixture in that a compound always has a a. homogeneous composition b. maximum of two components c. minimum of three components d. heterogeneous composition Explanation: By definition compounds are homogenous. They cannot be separated by physical means. A mixture (salad for example) is not homogenous. 34. Which substance cannot be decomposed into simpler substances? a. ammonia b. aluminum c. methane d. methanol Explanation: Elements cannot be decomposed into simpler substances because an element by definition is one kind of substance, one kind of atom. The other choices are compounds-- composed of two or more elements. 35. Which statement describes a chemical property? a. Its crystals are a metallic gray. b. It dissolves in alcohol. c. It forms a violet-colored gas. d. It reacts with hydrogen to form a gas. Explanation: While all the answers are true for iodine, only choice 4 describes a chemical property. The other choices are physical properties 36. A student investigated the physical and chemical properties of a sample of unknown gas and then investigated the gas. Which statement represents a conclusion rather than an experimental observation? a. The gas is colorless. b. The gas is carbon dioxide. c. When the gas is bubbled in limewater, the liquid becomes cloudy. d. When placed in the gas, a flaming splint stops burning. Explanation: Color, turning limewater cloudy, and inability to support combustion (cause a flame to go out) are observations. Figuring out what compound has these characteristics involves making a hunch or adding up the evidence (conclusion). Sort of like Judge Judy on TV. She listens to the facts (observations) and then decides who is at fault (conclusion). Another example: there are muddy footprints on a clean floor (observation). Figuring out who made the footprints is a conclusion. Was it the dog? 37. To determine the density of an irregularly shaped object, a student immersed the object in 21.2 milliliters of H2O in a graduated cylinder, causing the level of the H2O to rise to 27.8 milliliters. If the object had a mass of 22.4 grams, what was the density of the object?
6 a g / ml b. 6.6 g / ml c. 3.0 g / ml d. 3.4 g/ ml Explanation: D = M / V. First find the volume of the object by subtracting 21.2 ml from 27.8 ml or 6.6 ml Step 2: D = M / V or D = 22.4 g / 6.6 ml = 3.4 g / ml See also Table T
B) 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 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 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 informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
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 informationIn the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
More informationName period AP chemistry Unit 2 worksheet Practice problems
Name period AP chemistry Unit 2 worksheet Practice problems 1. What are the SI units for a. Wavelength of light b. frequency of light c. speed of light Meter hertz (s -1 ) m s -1 (m/s) 2. T/F (correct
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 informationWhich substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
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 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 informationFind a pair of elements in the periodic table with atomic numbers less than 20 that are an exception to the original periodic law.
Example Exercise 6.1 Periodic Law Find the two elements in the fifth row of the periodic table that violate the original periodic law proposed by Mendeleev. Mendeleev proposed that elements be arranged
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 informationPeriodic Table. 1. In the modern Periodic Table, the elements are arranged in order of increasing. A. atomic number B. mass number
Name: ate: 1. In the modern, the elements are arranged in order of increasing. atomic number. mass number. oxidation number. valence number 5. s the elements in Group I are considered in order of increasing
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 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 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 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 informationList the 3 main types of subatomic particles and indicate the mass and electrical charge of each.
Basic Chemistry Why do we study chemistry in a biology course? All living organisms are composed of chemicals. To understand life, we must understand the structure, function, and properties of the chemicals
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 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 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 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 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 informationChapter 2 The Chemical Context of Life
Chapter 2 The Chemical Context of Life Multiple-Choice Questions 1) About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living
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 informationChem term # 1 review sheet C. 12 A. 1
hem term # 1 review sheet Name: ate: 1. n isotope of which element has an atomic number of 6 and a mass number of 14?. carbon. magnesium. nitrogen. silicon 6. Which atoms represent different isotopes of
More informationTRENDS IN THE PERIODIC TABLE
Noble gases Period alogens Alkaline earth metals Alkali metals TRENDS IN TE PERIDI TABLE Usual charge +1 + +3-3 - -1 Number of Valence e - s 1 3 4 5 6 7 Electron dot diagram X X X X X X X X X 8 Group 1
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 informationTrends of the Periodic Table Basics
Trends of the Periodic Table Basics 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 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 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 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 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 informationREVIEW QUESTIONS Chapter 8
Chemistry 101 ANSWER KEY REVIEW QUESTIONS Chapter 8 Use only a periodic table to answer the following questions. 1. Write complete electron configuration for each of the following elements: a) Aluminum
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas
More informationCST Practice Test. Multiple Choice Questions
CST Practice Test Young NAME CST Practice Test Multiple Choice Questions 1) At 1 atm and 298 K, which of the K a values listed below represents the strongest acid? 5) Which electron-dot symbol represents
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 informationReview - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008
Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid
More informationChapter 8 Basic Concepts of the Chemical Bonding
Chapter 8 Basic Concepts of the Chemical Bonding 1. There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. (a). 4, 2 (b). 2, 4 (c). 4, 3 (d). 2, 3 Explanation: Read the question
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 informationCandidate Style Answer
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
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 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 information6.5 Periodic Variations in Element Properties
324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends
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 informationQuestions on Chapter 8 Basic Concepts of Chemical Bonding
Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,
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 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 informationChem final review sheet with answers
hem final review sheet with answers Name: ate: 1. Which pair of elements form an ionic bond with each other?. Kl. Il. Pl. Hl 6. Which atom listed has the greatest ability to attract the electrons that
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 informationAPPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
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 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 informationATOMS 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 informationName Class Date. What is ionic bonding? What happens to atoms that gain or lose electrons? What kinds of solids are formed from ionic bonds?
CHAPTER 1 2 Ionic Bonds SECTION Chemical Bonding BEFORE YOU READ After you read this section, you should be able to answer these questions: What is ionic bonding? What happens to atoms that gain or lose
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy. Analyze From the formulas for three
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 informationChemistry Assessment Unit AS 1
Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111]
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 informationCHEMISTRY II FINAL EXAM REVIEW
Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas
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 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 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
More information19.1 Bonding and Molecules
Most of the matter around you and inside of you is in the form of compounds. For example, your body is about 80 percent water. You learned in the last unit that water, H 2 O, is made up of hydrogen and
More informationHonors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
More informationSection 1: Arranging the Elements Pages 106-112
Study Guide Chapter 5 Periodic Table Section 1: Arranging the Elements Pages 106-112 DISCOVERING A PATTERN 1. How did Mendeleev arrange the elements? a. by increasing density b. by increasing melting point
More informationTest Review Periodic Trends and The Mole
Test Review Periodic Trends and The Mole The Mole SHOW ALL WORK ON YOUR OWN PAPER FOR CREDIT!! 1 2 (NH42SO2 %N 24.1 %H 6.9 %S 27.6 %O 41.3 % Al %C 35.3 %H 4.4 %O 47.1 Al(C2H3O23 13.2 3 How many moles are
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 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 informationChapter 8 Atomic Electronic Configurations and Periodicity
Chapter 8 Electron Configurations Page 1 Chapter 8 Atomic Electronic Configurations and Periodicity 8-1. Substances that are weakly attracted to a magnetic field but lose their magnetism when removed from
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More information100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals.
2.21 Ionic Bonding 100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals. Forming ions Metal atoms lose electrons to form +ve ions. Non-metal
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 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c.
More informationEXAMPLE EXERCISE 4.1 Change of Physical State
EXAMPLE EXERCISE 4.1 Change of Physical State State the term that applies to each of the following changes of physical state: (a) Snow changes from a solid to a liquid. (b) Gasoline changes from a liquid
More informationChapter 2: The Chemical Context of Life
Chapter 2: The Chemical Context of Life Name Period This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you
More informationName Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck. atoms- the smallest particle of an element that can be identified with that element
Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck atoms- the smallest particle of an element that can be identified with that element are the building blocks of matter consists of protons and
More informationBonds. Bond Length. Forces that hold groups of atoms together and make them function as a unit. Bond Energy. Chapter 8. Bonding: General Concepts
Bonds hapter 8 Bonding: General oncepts Forces that hold groups of atoms together and make them function as a unit. Bond Energy Bond Length It is the energy required to break a bond. The distance where
More informationStudy Guide For Chapter 7
Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance
More informationIonic and Metallic Bonding
Ionic and Metallic Bonding BNDING AND INTERACTINS 71 Ions For students using the Foundation edition, assign problems 1, 3 5, 7 12, 14, 15, 18 20 Essential Understanding Ions form when atoms gain or lose
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 informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More informationH 2O gas: molecules are very far apart
Non-Covalent Molecular Forces 2/27/06 3/1/06 How does this reaction occur: H 2 O (liquid) H 2 O (gas)? Add energy H 2O gas: molecules are very far apart H 2O liquid: bonding between molecules Use heat
More informationStoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.
Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven
More informationHorizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations.
The Periodic Table Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations. Vertical Rows are called Families or Groups.
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 information5.4 Trends in the Periodic Table
5.4 Trends in the Periodic Table Think about all the things that change over time or in a predictable way. For example, the size of the computer has continually decreased over time. You may become more
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 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 informationW1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
More informationChapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
More informationChem 115 POGIL Worksheet - Week 4 Moles & Stoichiometry
Chem 115 POGIL Worksheet - Week 4 Moles & Stoichiometry Why? Chemists are concerned with mass relationships in chemical reactions, usually run on a macroscopic scale (grams, kilograms, etc.). To deal with
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 informationLewis Dot Structures of Atoms and Ions
Why? The chemical properties of an element are based on the number of electrons in the outer shell of its atoms. We use Lewis dot structures to map these valence electrons in order to identify stable electron
More informationChemical Building Blocks: Chapter 3: Elements and Periodic Table
Name: Class: Date: Chemical Building Blocks: Chapter 3: Elements and Periodic Table Study Guide Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
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 informationChemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
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 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
More information