Honors Chemistry: Chapter 4- Problem Set (with some 6)
|
|
- Diane O’Connor’
- 5 years ago
- Views:
Transcription
1 Honors Chemistry: Chapter 4- Problem Set (with some 6) All answers and work on a separate sheet of paper! Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Atoms of one element change into atoms of another element during chemical reactions. 2. Atoms combine in one-to-one ratios to form compounds. 3. Atoms of one element are different from atoms of other elements. 4. According to Dalton s atomic theory, atoms are composed of protons, electrons and neutrons. 5. Atoms of elements are electrically neutral. 6. The mass of an electron is equal to the mass of a neutron. 7. The charge on all protons is the same. 8. The atomic number of an element is the sum of the protons and electrons in an atom of that element. 9. An atom of nitrogen has 7 protons and 7 neutrons. 10. Relative atomic masses are expressed in amu's. 11. The number of neutrons in the nucleus can be calculated by subtracting the atomic number from the mass number. 12. In his periodic table, Mendeleev arranged the element in ascending order of atomic number. 13. The representative elements are the Group A elements. 14. The transition metals and inner transition metals are the Group B elements. 15. The element in Group 4A, period 3 is gallium. Match each description in Column B with the correct term in Column A Column A Column B 1. atom a. the group 7A elements 2. Dalton s atomic theory b. horizontal rows of the periodic table c. Group A elements 3. Democritius d. arrangement of elements according to 4. electrons similarities in their properties e. a portion of the B Group elements 5. protons f. Group 1A elements 6. neutrons g. Group 0 elements or group 8A 7. nucleus h. vertical column on the periodic table 8. atomic number i. represents the number of protons in an atom 9. mass number j. 1/12 of the mass of the carbon 12 atom 10. isotopes k. total number of protons and neutrons in an atom 11. atomic mass unit (amu) l. weighted average mass of the atoms in a 12. atomic mass naturally occurring sample of an element 13. periodic table m. atoms that have the same number of protons but different numbers of neutrons 14. periods n. positively charged subatomic particles 15. group o. subatomic particles with no charge 16. representative elements p. negatively charged subatomic particles 17. alkali metals q. the central positively charged core of the atom 18. transition metals r. teacher in ancient Greece 19. halogens s. theory to explain the reactive behavior of elements 20. noble gases t. smallest particle of an element that retains the properties of that element Solve the following problems:
2 1. Given the relative abundance of the following naturally occurring isotopes of oxygen, calculate the average atomic mass of oxygen: Oxygen % Oxygen % Oxygen % 2. A sample of chlorine contains 2 isotopes Cl-35 mass and Cl-37 mass Calculate the weighted average atomic mass if the relative abundance is 75.8% Cl-35 and 24.2% Cl What is the atomic mass of silicon if 92.21% of its atoms have mass amu, 4.70% have mass amu, and 3.09% have mass amu? 4. Calculate the numbers of each subatomic particle for the isotopes provided: 81 a. Se b. Cs 2 55 c. Zn-32 d. Sn 4+ e. Al 5. Name the following elements and classify them as metal, nonmetal, transition metal or metalloid. a. halogen in period 5 b. Group 3B period 5 c. Alkaline earth metal in period 3 d. Group 3A and period 2 Answers: amu ; amu; amu
3 Honors Chemistry: Chapter 5- Problem Set All answers and work on a separate sheet of paper! Definition Matching: Match the terms in Column A with the Definitions in Column B. Column A Column B 1. quantum a. the most stable arrangement of electrons around 2. excited state the nucleus of an atom 3. atomic orbitals b. 1s 2 2s 2 2p 6 4. quantum mechanical model c. Electrons enter orbitals of lowest energy first 5. photons d. One electron per oribital before double up 6. de Broglie s equation e. An atomic orbital can only hold two electrons 7. visible light f. region of space around the nucleus which has a 8. ground state high probability of containing an electron 9. wavelength g. the amount of energy required to move an electron 10. neon from its present energy level to the next level 11. Hund s rule h. modern description of electron behavior 12. Pauli exclusion principle i. light quanta 13. Aufbau Principle j. predicts that all matter exhibits wavelike motions 14. electron configuration k. the distance between two consecutive wave crests l. the lowest energy level for a given electron m. when the electrons are not in their lowest energy states n. example of electromagnetic radiation Answer the following questions: 1. How many orbitals are in each of the following sublevels? a. 4p b. 3d c. 4f d. 2s 2. Identify the elements described below: a. contains a full third energy level b. contains only 1 electron in the 4p sublevel c. contains only 1 electron in the 5s sublevel d. contains 5 electrons in the 4s and 4p sublevel e. contains 3 electrons in the 4d sublevel 3. For each of the following elements draw orbital diagrams. a. C b.s c. K d.ar 4. For each of the following elements, write electron configurations. a. Fe b. Lead c. Uranium d. Zinc e. Tungsten 5. How does quantum theory explain the photoelectric effect 6. Write an electron configuration for an atom of calcium in the excited state 7. Write electron configurations for each of the following ions: a. O 2- b. Al 3+ c. Cu 2+ d. P 3- Solve the following problems: 1. What is the frequency of radiation whose wavelength is 2.40 x 10-3 m? 2. How much energy is associated with a green wavelength of visible light that has a wavelength of 4.86 nm?
4 3. What is the frequency of a photon having a wavelength 662 nm? 4. The frequency of a green photon is 6.26 x Hz. What is the wavelength? 5. Calculate the frequency of a wave that has a wavelength of 6.0 x 10-3 m. 6. Calculate the frequency of an x-ray having a wavelength of 2.5 x 10 4 nm. 7. Calculate the energy associated with a microwave having a frequency of 7.5 x s Calculate the energy of a photon having a wavelength of 6.6 x 10-3 m. 9. How much energy is associated with a photon in the ultraviolet region of the spectrum with a frequency of 6.6 x s -1? 10. How much energy is associated with a light that measures 3.50 in the spectroscope? This chart summarizes the quantum model of the hydrogen atom. For each energy change in the chart below, calculate quantities needed to complete the chart. Show your work! Use energy transition to determine if the energy is released or absorbed. Transition E (J) v (s -1 ) λ (m) Is energy Released or Absorbed n=6 to n= x n=3 to n= x n=6 to n= x 10-7 n=1 to n= x n=2 to n= x 10-7 How does the energy associated with transitions between higher energy levels compare to those that are between lower energy levels? Answers to PS 5: x Hz x J x Hz x 10-7 m x Hz x Hz x J x J x J x Chart: v λ a x x 10-6 b x x 10-6 c x x 10-7 d x x 10-7 e x x 10-7
5 Honors Chemistry: Problem Set Chapter 6 All answers and work on a separate sheet of paper! Match the terms in Column A with the definitions in Column B 1. ionization energy a. half the distance between the nuclei of two atoms 2. electronegativity b. when the elements are arranged in order of increasing 3. atomic radius atomic number, there is a periodic pattern in their 4. cations physical and chemical properties. 5. periodic law c. positively charged ion d. tendency for the atoms of an element to attract electrons when they are chemically combined with another element 1. period a. an element in which the outermost s and p sublevels are 2. inner transition metal filled 3. representative elements b. a horizontal row on the periodic table 4. transition metal c. an element whose outermost s sublevel and nearby d 5. noble gas contain electrons 6. group d. an element whose outermost s and nearby f sublevel contain electrons. e. a vertical column on the periodic table f. an element whose outermost s or p sublevels are only partially filled Elements Li, Be, B, C Be, Mg, Ca, Sr Sn, As S, F Ga, Ge, As, Se Se, Br, Te, I Ca, Sr, Se, Br W, Pb, Sb, P Ni, Pt, Kr, I Most Metallic Largest Radius Highest Ionization Energy Lowest Electronegativity Highest Electron Affinity Fr, Ba, C, N Explain why Ba has a lower ionization energy then Mg. Why does atomic size decrease proceeding left to right across a period? 1. Consider the following elements: Ca, H, Co, Al, Si, S, Cl a. How many would be conductive? b. How many would likely be liquid or gas? c. How many will likely form colored compounds? d. How many are metalloids? 2. Write the symbol for the element that is described below. a. Period 3 alkali metal. b. Outer electron configuration is 4s 2 4p 4. c. Has 7 valence electrons in the 5s and 5p. d. Metalloid in period 3. e. Smallest noble gas. f. Largest alkali metal. g. Most electronegative period 2 element. h. Most reactive halogen. i. Most reactive alkali metal.
6 Honors Chemistry: Review Unit 2 All answers and work on a separate sheet of paper! 1. Complete the table for the following elements: Element Name A-Z Format Mass Format # of Protons # of electrons # of Neutrons Atomic # Mass # Mn 12 Br As-76 Actinium How many neutrons are in each atom? a. 23 Na b. 81 Br c. 19 F Element X has two isotopes: X-100 and X-104. If the atomic mass of X is amu, which isotope is more abundant and why? 4. Identify each element as a metal, metalloid, or nonmetal. a. fluorine b. germanium c. zinc d. phosphorus e. lithium f. hydrogen 5. Name two elements that have properties similar to potassium. 6. How many sublevels are in the following principal energy levels? a. n = 1 c. n=3 e. n=5 b. n=2 d. n=4 f. n=6 7. How many orbitals are in the following sublevels? a. 1s b. 5s c. 4d d. 4f e. 7s f. 3p g. 5 th energy level h. 6d 8. Write an orbital diagram for the following elements. a. Magnesium b. Oxygen 9. Write a complete electron configuration for each of the following elements. a. hydrogen: b. vanadium c. seaborgium d. barium ion (Ba 2+ ) e. bromide (Br - ) f. silver g. krypton h. arsenic i. radon j. tungsten k. gold 10. Arrange the following types of electromagnetic radiation in order of increasing energy. a. infared c. visible light e. microwaves b. cosmic rays d. radio waves f. ultraviolet rays
7 11. Subatomic particle Who discovered What was the experiment What observations were made Proton Neutron Electron 12. Describe the 4 aspects of Dalton s model of the atom. 13. Describe Rutherford s atom. How was the deflection of alpha particles explained by his model? Solve: 14. The two most abundant isotopes of carbon are carbon-12 ( mass amu) and carbon 13 (mass amu). Their relative abundances are 98.9% and 1.10% respectively. Calculate the atomic mass of carbon. 15. What is the wavelength of the radiation whose frequency is 5.00 xo Hz? 16. An inexpensive laser that is available to the public emits light that has a wavelength of 670 nm. What are the color and frequency of the radiation? 17. What is the energy of a photon whose frequency is 2.22 x Hz? 18. What is the wavelength of a photon whose energy is 6.00 x J? 19. Suppose that you favorite AM radio station broadcasts at a frequency of 1600 KHz. What is the wavelength in meters of the radiation from the station? 20. Which family of elements is characterized by and s 2 p 3 configuration? 21. Consider the elements: Br, S, V, Rb, Ag, Sb, H, Al a. How many would be lusterous? b. How many are metalloids? c. How many would have colored compounds? d. How many would be solid at room temperature? e. How many would be ductile? 22. Name the elements that are described below: a. one that has 5 outer electrons on the third period b. one with 4s 2 4p 5 electron configuration c. the 4 th period, group 6A element d. outer electron configuration 2s 2 2p 4 e. 4s 2 f. 3d 10 4s Why would you expect sodium and lithium to have similar chemical and physical properties? 24. Explain why Mg is smaller than atoms of sodium and calcium. 25. Arrange the following elements in order of decreasing ionization energy: a. Cs, Li, K b. Cl, Si, P,Ar c. Ca, Ba, Be, Sr 26. Which element in each pair has the higher electronegativity? a. Na, Mg b. Rb, I c. Cl, Br
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals
More informationHonors Unit 6 Atomic Structure
Honors Unit 6 Atomic Structure Miss Adams Honors Chemistry 1 Name: 1 Homework #1: Frequency, Wavelength and the Speed of Light Show all of your work for the problems, including the initial formula, substitution
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 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 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 informationChapter 2: The Structure of the Atom and the Periodic Table
Chapter 2: The Structure of the Atom and the Periodic Table 1. What are the three primary particles found in an atom? A) neutron, positron, and electron B) electron, neutron, and proton C) electron, proton,
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 informationSearching for an Organizing Principle. Searching for an Organizing Principle. How did chemists begin to organize the known elements?
Searching for an Organizing Principle Searching for an Organizing Principle How did chemists begin to organize the known elements? Searching for an Organizing Principle A few elements, including copper,
More informationA1: Atomic Structure Worksheet (Goals 1 3, Chapter 4)
Unit 3 Assignment Packet Name: Period: A1: Atomic Structure Worksheet (Goals 1 3, Chapter 4) 1. Democritus, who lived in Greece during the 4 th century B.C., suggested that is made up of tiny particles
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 informationName Date Class MODELS OF THE ATOM
5.1 MODELS OF THE ATOM Section Review Objectives Identify inadequacies in the Rutherford atomic model Identify the new assumption in the Bohr model of the atom Describe the energies and positions of electrons
More information5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.
1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added
More informationUnit 3 Periodic Table and Quantum HW Packet Name Date. Periodic Table Concepts. 1. In what family are the most active metals located?
Directions: Answer the following questions. Periodic Table Concepts 1. In what family are the most active metals located? 2. In what family are the most active non-metals located? 3. What family on the
More informationModern Atomic Theory
Modern Atomic Theory Review of the Discovery of the Atom 1803 John Dalton discovered that elements are made of atoms. He thought that atoms were solid, like a marble. 1875 Crooks discovered the electron.
More informationName: Electrons in Atoms Chemical Periodicity Chapters 13 and 14
Name: Electrons in Atoms Chemical Periodicity Chapters 13 and 14 1 Chapter 13 Electrons in Atoms We need to further develop our understanding of atomic structure to help us understand how atoms bond to
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 informationChapter 2 Atoms and the Periodic Table
Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.
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 informationName: Class: Date: ID: A
Name: Class: _ Date: _ ID: A EOC review II Matching Match each item with the correct statement below. a. atomic orbital d. ground state b. aufbau principle e. Pauli exclusion principle c. electron configuration
More information3.1 Classification of Matter. Copyright 2009 by Pearson Education, Inc.
Chapter 3 Atoms and Elements 3.1 Classification of Matter Copyright 2009 by Pearson Education, Inc. 1 Matter Matter is the stuff that makes up all things. Copyright 2009 by Pearson Education, Inc. 2 Pure
More informationWhat particles form the nucleus of an atom? CHEMISTRY OLYMPICS 2nd 6 weeks
CHEMISTRY OLYMPICS 2nd 6 weeks Class Battle Between: Bauer, Cannon, Hermsdorf, Lawton, and Muller What particles form the nucleus of an atom? A) protons and neutrons B) electrons only C) neutrons and electrons
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) 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 information1. Draw a wave below and label the following parts: peak, trough, wavelength and amplitude
Wave Nature of Light 1. Draw a wave below and label the following parts: peak, trough, wavelength and amplitude 2. Draw two waves with different frequencies and circle the wave that has a higher frequency.
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 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 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 informationAtomic Theory. H. Cannon, C. Clapper and T. Guillot Klein High School
Atomic Theory Unit 3 Development of the Atomic Theory 1. Where is the mass of the atom concentrated? 2. What is located in the nucleus? 3. What is the negative particle that orbits the nucleus? 4. What
More informationMODERN ATOMIC THEORY AND THE PERIODIC TABLE
C10 04/19/2013 13:34:14 Page 114 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
More informationWhich order of statements represents the historical development of the atomic model? A) C D A B B) C D B A C) D B A C D) D B C A
1. The mass of a proton is approximately equal to the mass of A) an electron B) a neutron C) an alpha particle D) a beta particle 2. What is the number of electrons in an atom that has 20 protons and 17
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 informationName Date Period Unit 3 Review: Electrons and the periodic table
Name Date Period Unit 3 Review: Electrons and the periodic table G Chem; Coleman SHOW YOUR WORK ON ANY AND ALL CALCULATIONS. SIG FIGS MATTER. UNITS MATTER. General Questions: 1. Use the following terms
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 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 informationFull file at
16 Chapter 2: Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element. a.
More informationCh. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE
Ch. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE What Makes Red Light Red? (4.1) Electromagnetic Radiation: energy that travels in waves (light) Waves Amplitude: height
More informationAtomic Structure. What is an atom? The smallest particle of an element that retains properties of that element. Gedanken
Atomic Structure What is an atom? The smallest particle of an element that retains properties of that element. Gedanken 1 Atomic Theory Democritus vs. Dalton 500 BC 1808 AD Pure thought Observation + experiment
More informationName Date Class ORGANIZING THE ELEMENTS
6.1 ORGANIZING THE ELEMENTS Section Review Objectives Explain how elements are organized in a periodic table Compare early and modern periodic tables Identify three broad classes of elements Vocabulary
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 informationUnit 3: The Periodic Table and Atomic Theory
Name: Period: Unit 3: The Periodic Table and Atomic Theory Day Page # Description IC/HW 1 2-3 Periodic Table and Quantum Model Notes IC 1 4-5 Orbital Diagrams Notes IC 1 14 3-A: Orbital Diagrams Worksheet
More informationPeriodic Table. Engr. Yvonne Ligaya F. Musico 1
Periodic Table Engr. Yvonne Ligaya F. Musico 1 TOPIC Definition of Periodic Table Historical Development of the Periodic Table The Periodic Law and Organization of Elements in a Periodic Table Periodic
More informationUnit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct.
Unit Two Test Review Click to get a new slide. Choose your answer, then click to see if you were correct. According to the law of definite proportions, any two samples of water, H2O, A. will be made up
More informationName: Date: ChemT1. 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom?
Name: Date: ChemT1 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom? A. the atom is very small B. the electrons are moving
More informationChapter Test B. Chapter: Arrangement of Electrons in Atoms. possible angular momentum quantum numbers? energy level? a. 4 b. 8 c. 16 d.
Assessment Chapter Test B Chapter: Arrangement of Electrons in Atoms PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question
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 information: the smallest particle that has the properties of an element. In, this Greek philosopher suggested that the universe was made of.
Notes: ATOMS AND THE PERIODIC TABLE Atomic Structure: : the smallest particle that has the properties of an element. From the early concept of the atom to the modern atomic theory, scientists have built
More informationElectrons and Periodic Table (Ch. 4 & 5) OTHS Academic Chemistry
Name Objectives: Per. Electrons and Periodic Table (Ch. 4 & 5) OTHS Academic Chemistry Express the arrangement of electrons in atoms through electron configurations Understand the electromagnetic spectrum
More informationTHE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table!
THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table! Development of the Periodic Table! Main Idea: The periodic table evolved over time as scientists discovered more useful ways
More informationA.P. Chemistry Practice Test - Ch. 7, Atomic Structure and Periodicity
A.P. Chemistry Practice Test - Ch. 7, Atomic Structure and Periodicity 1) Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic radiation is MHz. A) 50 B) 20 C)
More informationCHM 100 CHEMISTRY MAN & ENVIRONMENT Atoms and Elements Sample Test
CHM 100 CHEMISTRY MAN & ENVIRONMENT Atoms and Elements Sample Test Multiple Choice: Identify the choice that best completes the statement or answers the question. 1. Which of these elements has two valence
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 informationAtoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2
Name Date Due Atoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2 Directions: Write your answers to the following questions in the space provided. For problem solving, all of the
More informationCDO CP Chemistry Unit 5
1. Of the three particles; protons, neutrons, and electrons, which one(s) are responsible for most of the mass of an atom? a) the protons only b) the electrons only c) the neutrons only d) the protons
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 information1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on
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 number of oxidation states 2.
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following is not one of the postulates of Dalton's atomic theory? A)
More information8. Which of the following could be an isotope of chlorine? (A) 37 Cl 17 (B) 17 Cl 17 (C) 37 Cl 17 (D) 17 Cl 37.5 (E) 17 Cl 37
Electronic Structure Worksheet 1 Given the following list of atomic and ionic species, find the appropriate match for questions 1-4. (A) Fe 2+ (B) Cl (C) K + (D) Cs (E) Hg + 1. Has the electron configuration:
More informationChemistry Chapter 9 Review. 2. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x s -1.
Chemistry Chapter 9 Review 1. What is the frequency of radiation that has a wavelength of 4.7 x 10-5 cm? 2. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x 10 14 s -1. 3. The
More informationCDO AP Chemistry Unit 5
1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic
More informationExam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table
Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table Name /87 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statements by changing
More informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
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 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 informationPart I Assignment: Electron Configurations and the Periodic Table
Chapter 11 The Periodic Table Part I Assignment: Electron Configurations and the Periodic Table Use your periodic table and your new knowledge of how it works with electron configurations to write complete
More informationChapter 2 Atoms and Elements. 2.4 The Atom
Chapter 2 Atoms and Elements 2.4 The Atom Atoms Dalton s Atomic Theory Are tiny particles of matter. Of an element are similar and different from other elements. Of two or more different elements combine
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 6 The Periodic Table
CHAPTER 6 The Periodic Table 6.1 Organizing the Elements Mendeleev: listed the elements in order of increasing atomic mass and in vertical columns according to their properties. Left blank spaces for undiscovered
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 informationDeveloping the Periodic Table
Developing the Periodic Table Early Element Classification Mendeleev s First Periodic Table Mendeleev s First Periodic Table Mendeleev s Periodic Table Arranged by increasing atomic mass Some elements
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 informationAP Chapter 6 Study Questions
Class: Date: AP Chapter 6 Study Questions True/False Indicate whether the statement is true or false. 1. The wavelength of radio waves can be longer than a football field. 2. Black body radiation is the
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 informationUnits 1, 2 study guide- atomic structure
Name: Units 1, 2 study guide- atomic structure 1) Complete the required information for each subatomic particle (T1.3) symbol name charge location Mass (AMU) p + e - n 0 2) Define the following terms:
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 informationHomework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2
Name Period Homework Packet Unit 2 1. Which of the following is the correct empirical formula for a compound that has 37.5% C, 12.6% H, and 49.9% O? (A) C 2 H 4 O (B) CH 4 O 2 (C) CH 5 O 2 (D) CH 4 O (E)
More informationGroups vs. Periods what s the difference?? Groups: Periods:
Before watching the video: Use page 131 in your book or the internet to label the periodic table according to the following guidelines (NOTE: Your key might not look exactly like the book!!!) a. Color
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 informationRegan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
More information9/13/2011. The Greek Philosophers. Atomic Structure & The Periodic Table. Dalton s Atomic Theory. J. J. Thomson. Thomson s Experiment
Atomic Structure & The Periodic Table The Greek Philosophers Democritus believed that all matter is made up of tiny particles that could not be divided Aristotle -- thought that matter was made of only
More informationThe Periodic Table & Formation of Ions
The Periodic Table & Formation of Ions Development of the Periodic Table Mendeleev: Considered to be the father of the periodic table Arranged elements by increasing atomic mass Placed elements with similar
More informationTeacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol.
Teacher Workbooks Science and Nature Series Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. 1 Copyright 23 Teachnology Publishing Company A Division of Teachnology,
More informationElements are the building blocks of matter. Chapter 2
Elements are the building blocks of matter. Chapter 2 S In this chapter we will be covering S ELEMENTS!!! S The Periodic Table and Chemical Properties!!! S The Periodic Table and Atomic Theory! What is
More informationNote Taking Guide: Episode 401. arranged elements by. predicted of missing. discovered that each has a unique. arranged elements by
Note Taking Guide: Episode 401 Dmitri Mendeleev: arranged elements by. predicted of missing. Henry Moseley: discovered that each has a unique. arranged elements by. now all elements fit into place based
More informationHSVD Ms. Chang Page 1
Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which
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 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 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 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 informationHonors Chemistry - 1st Semester Final Practice Exam
Honors Chemistry - 1st Semester Final Practice Exam Mr. Matthew Totaro MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement about the
More informationChapter 4 The Structure of the Atom
Chapter 4 The Structure of the Atom Read pg. 86-97 4.1 Early Theories of Matter The Philosophers Democritus Artistotle - Artistotle s influence so great and the science so primitive (lacking!) his denial
More informationChemistry: Hood River Valley High School Unit 3 Note Packet and Goals. Description A1. Marble Lab. Nailon Isotope Lab A2.
Chemistry: Hood River Valley High School Unit 3 Note Packet and Goals Name: Period: Unit 3 Atomic Structure and Periodic Table Unit Goals- As you work through this unit, you should be able to: 1. describe
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 informationHonors Chemistry Unit 4 ( )
Honors Chemistry Unit 4 (2017-2018) Families (research and present) Metals/nonmetals Trends o Atomic radius o Electronegativity o Ionization energy o Metallic and nonmetallic character Review Ions Oxidation
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 informationE J The electron s energy difference between the second and third levels is J. = J
The wavelength of light emitted is 654 nm. = c f c 3.00 10 8 m/s f c 3.00 108 m 1s 6.54 10 7 m f 4.59 4.59 10 14 z 1 s 10 14 The frequency of the light emitted is 4.59 10 14 z. E hf h 6.63 10 34 J/z E
More informationAccelerated Chemistry Study Guide The Periodic Table, Chapter 5
Accelerated Chemistry Study Guide The Periodic Table, Chapter 5 Terms, definitions, and people Dobereiner Newlands Mendeleev Moseley Periodic table Periodic Law group family period Page 1 of 38 alkali
More informationWarm-up For sulfur: 1. How many valence electrons does it have? 2. What ion does this typically form? 3. Write the electron configuration for the ion.
Warm-up For sulfur: 1. How many valence electrons does it have? 2. What ion does this typically form? 3. Write the electron configuration for the ion. Nucleus Contains 99.9% of the mass of an atom Found
More informationThe Periodic Law Notes (Chapter 5)
The Periodic Law Notes (Chapter 5) I. History of the Periodic Table About 70 elements were known by 1850 (no noble gases) but there didn t appear to be a good way of arranging or relating them to study.
More informationAtoms with More than One Electron
Activity 6 Atoms with More than One Electron GOALS In this activity you will: View the spectra of various materials. Graphically analyze patterns in the amounts of energy required to remove electrons from
More information5) Which statement correctly describes the relationship of wavelength and frequency in a wave?
Exam 2 Name: Multiple Choice (2 pts each) 1) Which of the following bonds is the most polar? a) C O b) N O c) O O d) Si O 2) The maximum electron capacity of an f sublevel is a) 7 c) 14 b) 6 d) 10 3) Which
More information