Biology Summer Work 2015: This packet has been put together by your. successful in Biology.
|
|
|
- Cameron Reeves
- 7 years ago
- Views:
Transcription
1 Biology Summer Work 2015: This packet has been put together by your Biology teachers for you to work on during the summer. It will help you review topics that you have learned in 9 th grade and will help you be successful in Biology. This packet will be due on Thursday, September 3, Please expect to take the test on Wednesday, September 9, Name: 9 th Grade Teacher:
2
3 Chemistry Review Name Lesson 1: Atomic Structure Basic Atomic Structure What are Atoms? (text w/music) Atomic Symbols Notes: (Your Biology teacher expects to see notes for every clip)
4 1. Identify the three types of particles that make up an atom and their charges: Particle Charge of particle 2. The Nucleus contains and 3. The space that surrounds the nucleus and contains electrons is called the 4. What keeps electrons from just shooting off away from the atom? (video #1). 5. A neutral atom has the same number of and. 6. The word atom means. 7. When comparing the mass of these particles, and have a mass of 1 atomic mass unit (AMU) while the mass of is 1/2000 AMU. Therefore, when calculating the mass of an atom, only the mass of the and are considered. ATOMIC NUMBER Elements are identified by the number of p+ they contain. 8. If an atom has 11 p +, it must be. 9. If an atom has p +, it must be N. 10. H has protons, neutrons and electrons. 11. Complete the table below using a periodic table (online or in your agenda pad) Element Element Atomic # # Protons # Neutrons # Electrons Mass # Name Symbol Lithium Li 3 6 C Atoms that exist and combine with other dissimilar atoms are called. 13. Elements are made up of and compounds are made of of molecules. 30 Zinc Atomic # Symbol Name Atomic Mass 3 Li 6.941
5 Chemistry Review Lesson 2: Atoms, Isotopes and Ions Atoms and Isotopes: What are Isotopes? Protons/neutrons/electrons in atoms/ions from mass/atomic number and charge Notes: (Your Biology teacher expects to see notes for every clip)
6 1. An isotope is a different of the same. 2. Isotopes and atoms of an element have the same # of but different numbers of. 3. Ions are atoms with unequal number of and. Neutral Atoms: 1. The # of and # of are equal. 2. A neutral oxygen atom has 8p +. How many e - will it have? 3. How many p + and e - does a neutral Calcium atom have? Stability # of protons never changes for a given element; only e- are lost or gained. 4. When the # of p + no longer equals # of e-, the atom is an: 5. An excess # of e - means the atom has a charge 6. Fewer e - than p + means the atom has a charge 7. Complete the table below using a periodic table (online or in your agenda pad) Element Element Atomic # # Protons # Neutrons # Electrons Mass # Name Symbol Iron Charge +/-/o Hg If you know only the following information can you always determine what the element is? (Yes/No). a) number of protons b) number of neutrons c) number of electrons in a neutral atom 9. The number of protons in one atom of an element determines the atom s, and the number of electrons determines the of an element. 10. The atomic number tells you the number of in one atom of an element. It also tells you the number of in a neutral atom of that element. 11. The atomic number gives the identity of an element as well as its location on the Periodic Table. No two different elements will have the same.
7 12. The of an element is the total number of protons and neutrons in the of the atom. 13. The of an element is the average mass of an element s naturally occurring atom, or isotopes, taking into account the of each isotope. 14. The mass number is used to calculate the number of and in one atom of an element. In order to calculate the number of neutrons you must subtract the from the. 15. Complete the table below. Element Ion Symbol Name H 1+ S 2- K 1+ # Protons # Electrons Charge Anion/Cation
8 Chemistry Review Lesson #3: Period Table and Lewis Dot Diagrams A Tour of the Periodic Table Notes: (There is a lot in this video; groups periods, gallium, reactivity, halogens etc.) Periodic Table Part II: How to use the table Notes: at least three points not mentioned above Drawing Lewis Dot Diagrams Notes: be specific this will help with the table on page 3
9 Answer the following questions: 1. In the periodic table, the vertical columns are called, while the rows are called. 2. Color the following groups on the periodic table below with the corresponding colors Alkali Metals - yellow Alkaline Earth Metals green Halogens - orange Noble Gases - red 3. The number of electrons in the outer energy shell of a particular atom are called electrons. 4. What are two ways to determine the number of valence electrons a particular atom has? Hint: One is much easier than the other. a) b) 5. The Alkali metals are ( circle one) Highly/ Non reactive, and all have valence electron(s) 6. The Alkaline Earth metals have valence electron(s). 7. The Halogens have valence electrons, thus they are (circle one) Highly/ Non -reactive. 8. The Noble gases have valence electrons, making them (circle one) Highly/ Non -reactive. 9. Circle the non-metals on the periodic table above. 10. Why are these non-metals, known as CHNOPS, so important to Biology? Here s the big connection!!! 11. Label the transition metals using a large bracket on the periodic table above. 12. Draw a zigzag line along the metalloids you should remember this from last year! 13. As we move towards the bottom of the periodic table, the atomic mass. (increases/decreases). 14. As we move across a row, the atomic mass. (increases/decreases) because
10 Bohr Diagrams: The Bohr Diagram is used to show the exact number of electrons for a particular atom of an element. The images below show Bohr Diagrams of Carbon. You Try: In the space provided, draw the Bohr diagram for Chlorine (Cl). a) How many valence electrons does an atom of Chlorine have? b) How did you know this by looking at your Bohr diagram? Electron Configuration and Stability Every atom wants to be stable, and stability for an atom is achieved by having the right number of electrons in its outermost shell. Atoms that already have the ideal number of electrons in their outer shell have no desire for more electrons, and don't want to lose any either. These atoms tend to be un-reactive or inert. Atoms that that do not have the ideal number tend to be reactive, striving to get their hands on more, or get rid of some electrons. The atom will strive to achieve stability by gaining or losing electrons in their outer shell. If this cannot be achieved by shuffling their own electrons around, atoms interact or react with other atoms to take/ give (ionic bonds) or share (covalent bonds) electrons to achieve their goal. Atoms that that do not have the ideal number tend to be reactive, striving to get their hands on more, or get rid of some electrons. The table below lists shells one to five, and shows the maximum number of electrons each shell can hold. Remember, a full shell makes a happy atom. We will only be working with 3 shells this year! Shell Can hold is stable with an outer shell holding
11 Lewis Dot Diagrams: It s really tedious and downright Bohr-ing (get it?) to draw out all of those rings, so we usually show valence electrons using the Lewis Dot Diagram. Watch the tutorial on drawing Lewis Dots and complete the table below. Element Name Symbol Protons Electrons How many shells? E - in the outer shell Lewis Dot Model show electrons in outermost shell Hydrogen H H Helium He 2 Lithium Li Beryllium Be 4 4 Carbon C 6 6 Oxygen O Fluorine F 9 Neon Ne Sodium Na Magnesium Mg Chlorine Cl Argon Ar
12 Chemistry Review Lesson #4: Bonding Bond's in Biological Molecules - Notes: (Your Biology teacher expects to see at least three concepts) Intro to Chemistry: Intro to Bonding 1. What do Bonds do? 2. Ionic Bonds produce. 3. Draw the Lewis dot structure of Sodium using pen and Draw a Lewis dot structure of Chlorine in pencil. 4. Use arrows to indicate what happens to the electrons when they interact and any charges that result. 5. What types of elements form ionic bonds? 6. Another term of covalent bond is 7. In covalent bonding, electrons are 8. Draw the Lewis dot of two hydrogen atoms, one in pen and one in pencil. Circle the shared electrons. 9. Redraw this molecule using a line to represent the covalent bond. 10. What type of molecules form Covalent bonds?
13 Intro to Chemistry: Ionic Bonding 2: When atoms bond ionically, one atom electrons and another atom electrons. 12. If the first atom gives away 2 electrons, the charge of the atom will be. The charge of the atom that received the electrons will be. 13. How to these charged atoms behave toward one another and why? 14. What does the word "salt" mean to a chemist? 15. List some characteristics of Ionic Compounds Intro to Chemistry: Covalent Bonds ½ What attracts two molecules toward each other in covalent bonds? Notes: (numerous definitions including polar and non-polar covalent bonds)
14 Ionic and Molecular Compounds Notes: That's Why Carbon Is a Tramp: Biology # What are organic molecules? 18. The atomic # of C=. 19. How does being small benefit carbon? 20. What does it mean when we say "carbon is kind"? 21. What does the speaker mean when saying "Carbon is a tramp"? 22. What is the octet rule? 23. Carbon it requires electrons to fill its outer orbital. 24. Draw a Lewis dot diagram of 1 carbon using a pen. Surround it with 4 Lewis dot diagrams of hydrogen using pencil. 25. Show how electrons are shared between these atoms. 26. What is the chemical formula for the molecule you just drew? 27. What is the difference between non-polar and polar covalent bonds? 28. Why do oxygen molecules "stick together"? 29. In general, which type of bond is the strongest?
15 Episode 1: Global Warming, It's All About Carbon Notes: Episode 2: Global Warming, It's All About Carbon Notes: 30. Create a Lewis Dot diagram for the compound KCl. Is this ionic or covalent? Label any charges 31. Create a Lewis Dot diagram for MgCl 2. Is this ionic or covalent? Label any charges 32. Create a Lewis Dot diagram for NH 3. Is this ionic or covalent? Circle any shared electrons 33. Create a Lewis Dot diagram for CH 4.Is this ionic or covalent? Circle any shared electrons 34. Create a Lewis Dot diagram for H 2 0. Is this ionic or covalent? Is this polar or non-polar?
Chapter 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
Untitled 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
******* 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
SCPS 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
7.4. 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
List 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
19.1 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
Test Bank - Chapter 4 Multiple Choice
Test Bank - Chapter 4 The questions in the test bank cover the concepts from the lessons in Chapter 4. Select questions from any of the categories that match the content you covered with students. The
Atoms and Molecules. Preparation. Objectives. Standards. Materials. Grade Level: 5-8 Group Size: 20-30 Time: 60 90 Minutes Presenters: 2-4
Atoms and Molecules Preparation Grade Level: 5-8 Group Size: 20-30 Time: 60 90 Minutes Presenters: 2-4 Objectives This lesson will enable students to: Describe how atoms are the building blocks of matter
PROTONS AND ELECTRONS
reflect Imagine that you have a bowl of oranges, bananas, pineapples, berries, pears, and watermelon. How do you identify each piece of fruit? Most likely, you are familiar with the characteristics of
Lewis 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
Unit 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.
Molecular Models in Biology
Molecular Models in Biology Objectives: After this lab a student will be able to: 1) Understand the properties of atoms that give rise to bonds. 2) Understand how and why atoms form ions. 3) Model covalent,
Bonding 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
Chapter 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
ATOMS 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
Periodic 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
Electrons 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
Laboratory 11: Molecular Compounds and Lewis Structures
Introduction Laboratory 11: Molecular Compounds and Lewis Structures Molecular compounds are formed by sharing electrons between non-metal atoms. A useful theory for understanding the formation of molecular
Trends 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
UNIT (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
PERIODIC 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
Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num
. ATOMIC STRUCTURE FUNDAMENTALS LEARNING OBJECTIVES To review the basics concepts of atomic structure that have direct relevance to the fundamental concepts of organic chemistry. This material is essential
Electron Configurations, Isoelectronic Elements, & Ionization Reactions. Chemistry 11
Electron Configurations, Isoelectronic Elements, & Ionization Reactions Chemistry 11 Note: Of the 3 subatomic particles, the electron plays the greatest role in determining the physical and chemical properties
47374_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.
The 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
ANSWER KEY : BUILD AN ATOM PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom )
ANSWER KEY : PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom ) 1. Explore the Build an Atom simulation with your group. As you explore, talk about what
Chapter 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
The Atom and the Periodic Table. Electron Cloud Structure Energy Levels Rows on the Periodic Table Bohr Models Electron Dot Diagrams
The Atom and the Periodic Table Electron Cloud Structure Energy Levels Rows on the Periodic Table Bohr Models Electron Dot Diagrams Review The vertical columns in the periodic table are called groups.
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
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
Chapter 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
Ionic 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
Part I: Principal Energy Levels and Sublevels
Part I: Principal Energy Levels and Sublevels As you already know, all atoms are made of subatomic particles, including protons, neutrons, and electrons. Positive protons and neutral neutrons are found
Trends 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
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance
Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance Lewis Dot notation is a way of describing the outer shell (also called the valence shell) of an
Periodic 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
Atoms, 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
In 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.
Name 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
Chapter 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
PERIODIC TABLE. reflect
reflect Suppose you wanted to organize your locker at school. How could you separate and arrange everything in an organized way? You could place the books, notebooks, and folders on a shelf that is separate
Chapter 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)
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.
Chapter 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
2. 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
Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D
Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D Electrons in Atoms (std.1d) What are Bohr Models? planetary model in which the negatively-charged electrons orbit a small, positively-charged
Chapter 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
19.2 Chemical Formulas
In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula
Unit 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
TRENDS 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
MODERN 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
Chemistry - 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
CHEMISTRY BONDING REVIEW
Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.
3. 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
Molecular 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.
Elements, 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,
Find 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
Bohr s Model of the Atom
Bohr Models Bohr s Model of the Atom Focuses on electrons and their arrangement. Bohr stated that electrons move with constant speed in fixed orbits around the nucleus, like planets around a sun. Bohr
5.4 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
Chemical 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.
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
ANSWER KEY. Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take!
ANSWER KEY Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take! From American Chemical Society Middle School Chemistry Unit: Chapter 4 Content Statements: Distinguish the difference
Horizontal 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.
6.5 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
Look at a periodic table to answer the following questions:
Look at a periodic table to answer the following questions: 1. What is the name of group 1? 2. What is the name of group 2? 3. What is the name of group 17? 4. What is the name of group 18? 5. What is
IONISATION ENERGY CONTENTS
IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation
EXPERIMENT 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
Section 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
Which 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
2 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
9/13/2013. 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
Chemistry: 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
Bonding & Molecular Shape Ron Robertson
Bonding & Molecular Shape Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\00bondingtrans.doc The Nature of Bonding Types 1. Ionic 2. Covalent 3. Metallic 4. Coordinate covalent Driving
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 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
Name 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
Chem 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
Theme 3: Bonding and Molecular Structure. (Chapter 8)
Theme 3: Bonding and Molecular Structure. (Chapter 8) End of Chapter questions: 5, 7, 9, 12, 15, 18, 23, 27, 28, 32, 33, 39, 43, 46, 67, 77 Chemical reaction valence electrons of atoms rearranged (lost,
Ions & Their Charges Worksheet
Ions & Their Charges Worksheet Name Date Teacher Diagram of charges based on groups on the periodic table including transition metals and noble gases: IA IIA Transition IIIA IVA VA VIA VIIA VIIIA metals
Chapter 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.
Exam 2 Chemistry 65 Summer 2015. Score:
Name: Exam 2 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of
Ionic and Covalent Bonds
Ionic and Covalent Bonds Ionic Bonds Transfer of Electrons When metals bond with nonmetals, electrons are from the metal to the nonmetal The becomes a cation and the becomes an anion. The between the cation
5. Structure, Geometry, and Polarity of Molecules
5. Structure, Geometry, and Polarity of Molecules What you will accomplish in this experiment This experiment will give you an opportunity to draw Lewis structures of covalent compounds, then use those
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
The 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
LEWIS DIAGRAMS. by DR. STEPHEN THOMPSON MR. JOE STALEY
by DR. STEPHEN THOMPSON MR. JOE STALEY The contents of this module were developed under grant award # P116B-001338 from the Fund for the Improvement of Postsecondary Education (FIPSE), United States Department
Chemistry 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
P. Table & E Configuration Practice TEST
P. Table & E Configuration Practice TEST Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A line spectrum is produced when an electron moves from one energy
Chapter 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,
Chapter 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
neutrons 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
Unit 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
Directions: T. Trimpe 2005 http://sciencespot.net/
Candy Compounds Teacher Information I use this activity after we have discussed ionic and covalent bonds to give my students a chance to practice bonding. I walk around the classroom as students work on
Chapter 7. Electron Structure of the Atom. Chapter 7 Topics
Chapter 7 Electron Structure of the Atom Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Chapter 7 Topics 1. Electromagnetic radiation 2. The Bohr model of
Noble Gases. Outline Nobel Gas Elements Radon and Health Chemistry Homework
Radon and Other Noble Gases The elements in the last column of the periodic table are all very stable, mono-atomic gases. Until 1962, they were called inert gases because they did not react with other
Copyrighted 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
Atomic 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
Chemistry Diagnostic Questions
Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to
Atoms 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,
Science 20. Unit A: Chemical Change. Assignment Booklet A1
Science 20 Unit A: Chemical Change Assignment Booklet A FOR TEACHER S USE ONLY Summary Teacher s Comments Chapter Assignment Total Possible Marks 79 Your Mark Science 20 Unit A: Chemical Change Assignment
CHAPTER 6 Chemical Bonding
CHAPTER 6 Chemical Bonding SECTION 1 Introduction to Chemical Bonding OBJECTIVES 1. Define Chemical bond. 2. Explain why most atoms form chemical bonds. 3. Describe ionic and covalent bonding.. 4. Explain