7.2 Valence Electrons and Bonding Patterns
|
|
- Georgia Stephens
- 7 years ago
- Views:
Transcription
1 7.2 Valence Electrons and Bonding Patterns Only valence electrons form bonds When a chemical bond forms some valence electrons are either shared or transferred between atoms. Only the unpaired valence electrons in an atom participate in chemical bonds. for complex reasons, the 5 th, 6 th, and 7 th valence electrons pair up and reduce the number of electrons available for bonding. The diagram below shows the main group elements along with their paired and unpaired valence electrons. Each unpaired valence electron can form ONE covalent bond In a molecular compound, each unpaired valence electron can form one covalent chemical bond. For example, both nitrogen (N) and phosphorous (P) atoms each have three unpaired valence electrons. In molecular compounds, these elements both form three covalent bonds. In a molecular compound, each unpaired valence electron forms one covalent bond Ion charge and valence electrons When forming a positive ion, each valence electron can contribute 1 unit of positive charge to the ion. This occurs when an atom loses its valence electron(s) to another atom, leaving a charge of +1 for every valence electron lost. For example, sodium (Na) and potassium (K) have a single valence electron and form singly charged ions (+1). Magnesium (Mg) and calcium (Ca) have two valence electrons each. These elements form ions with a charge of +2. In positive ions, each valence electron can contribute 1 unit of positive charge A NATURAL APPROACH TO CHEMISTRY 207
2 Section 7.2 Valence Electrons and Bonding Patterns The octet rule eight valence electrons = chemical stability In Chapter 6 you learned that the noble gasses have eight valence electrons (except for He which has two). These elements form no bonds because they are already at the most stable configuration of electrons. From the noble gasses we infer that elements with eight valence electrons are chemically stable. The observed behavior of the rest of the elements confirms that elements form chemical bonds to achieve the magic configuration of 8 valence electrons. This observation is known as the octet rule. The octet rule states that elements transfer or share electrons in chemical bonds to reach a stable configuration of 8 valence electrons. Elements form bonds to reach 8 valence electrons 2 valence electrons are most stable for H, Li, Be, and B The elements hydrogen, lithium, beryllium, and boron have so few electrons that their version of the octet rule is really based on helium as the closest noble gas. Helium fills the first energy level with its 2 electrons. That means either 0 or 2 valence electrons are also a noble gas electron configuration. The octet rule for hydrogen, lithium, beryllium, and boron is more accurately the duet rule or the rule of 2. These elements form chemical bonds to achieve 2 valence electrons. H, Li, Be, and B form bonds to reach 2 valence electrons Shared electrons are counted by both atoms In a covalent bond, a shared electron gets counted as a valence electron by both atoms. For example, molecular hydrogen (H 2 ) shares electrons to get 2 valence electrons - like helium. In water (H 2 O) each of the two hydrogen atoms shares 1 electron with oxygen giving each hydrogen 2 valence electrons and oxygen 8 valence electrons. octet rule - elements transfer or share electrons in chemical bonds to reach a stable configuration of 8 valence electrons. The light elements H, Li, Be, and B have helium as the closest noble gas so the preferred state is 2 valence electrons instead of A NATURAL APPROACH TO CHEMISTRY
3 Valence electrons and ion formation ionic charge and the periodic table There are two ways in which elements satisfy the octet rule: by sharing electrons in a covalent bonds, or by transferring electrons in an ionic bond. When the difference in electronegativity is larger than 2.1, the chemical bond is ionic. Most elements form some ionic compounds. The table below shows the most common charges for ions of the main group elements. Ion patterns You should see several patterns: 1. Elements on the left side tend to form positively charged ions, and elements on the right side form negatively charged ions; 2. Elements in the middle sometimes form positive and sometimes form negative ions and are marked as variable charge; 3. The alkali metals (group 1) form +1 charged ions because they have one valence electron; 4. The alkali earth metals (group 2) form +2 charged ions because they have two valence electrons; 5. Boron-like elements (group 13) form +3 charged ions because they have three valence electrons; 6. Oxygen-like elements (group 16) form -2 charged ions. These elements have 6 valence electrons. Their easiest path to the octet rule is to gain 2 electrons; 7. The halogens (group 17) form -1 charged ions. These elements have 7 valence electrons. Their easiest path to the octet rule is to gain one electron. A NATURAL APPROACH TO CHEMISTRY 209
4 Section 7.2 Valence Electrons and Bonding Patterns Electron configuration of ions Why sodium forms a +1 ion Why oxygen forms a -2 ion Sodium is an alkali metal with one valence electron. Sodium usually loses its one valence electron to become Na + in order to satisfy the octet rule and have an electron configuration like that of a noble gas. Theoretically, sodium could also gain 7 electrons to become Na -7, but losing one is so much more likely that we do not ever observe Na -7 ions in nature. The electron configuration of Na, Na +, and Ne are shown below. Note that Na + has the same electron configuration as neon. Sodium tends to form Na + ions because this is the lowest energy path by which sodium can satisfy the octet rule and reach a noble gas electron configuration. Oxygen atoms have six valence electrons. In order to have an electron configuration like that of a noble gas, oxygen could either gain two electrons to have the same electron configuration as neon, or lose six electrons to have the same electron configuration as helium. Considering that oxygen has high ionization energy, it is not likely to lose six electrons. Also, oxygen has high electronegativity, so it has the ability to grab electrons from other atoms. For oxygen it makes sense that it will gain two electron rather than lose six. Write the electron configuration for a magnesium ion (Mg 2+ ) Asked: electron configuration of Mg 2+ Given: Mg, atomic #12, charge of +2. Relationships: The electron configuration of magnesium is 1s 2, 2s 2, 2p 6, 3s 2 Solve: Answer: Mg must lose 2 electrons to become Mg 2+. Therefore it loses the pair of 3s 2 electrons. The electron configuration of Mg 2+ is 1s 2, 2s 2, 2p 6, which is identical to neon. 210 A NATURAL APPROACH TO CHEMISTRY
5 Simple ionic formulas Ionic crystals Why calcium chloride has the formula CaCl 2 Ionic substances typically form a crystal, which is a large group of oppositely charged ions arranged in a regular pattern. The calcium chloride (CaCl 2 ) crystal in the diagram is a good example. Calcium chloride is often used to melt ice on roads because it is better for the environment than sodium chloride (also used to melt ice). Ionic crystals are neutral even though they are formed through the attractions of trillions of charged ions. You can have any number of ions in the crystal as long as the positive charges exactly balance the negative charges. To determine the formula of an ionic compound, you need to balance the positive and negative charges. For example, calcium makes a Ca 2+ ion. Chlorine makes a Cl - ion. Each calcium atom loses two electrons and each chloride ion gains only one. This means the compound requires two chloride ions to have the same amount of negative charge as one calcium ion. This makes the ratio of calcium to chlorine 1:2, and the formula is therefore CaCl 2. What is the correct formula for calcium oxide, a compound used in making paper, pottery, and adjusting the ph of soils? Asked: Given: What is the formula for the ionic compound calcium oxide? Calcium oxide is made from calcium and oxygen ions. Calcium forms +2 ions and oxygen forms -2 ions. Relationships: Ca +2 and O -2 must combine in a ratio that will balance out the positive and negative charges. Solve: The charge on one Ca +2 ion will balance out with the charge on one O -2 ion. Therefore the ratio is 1:1 and the formula is CaO. A NATURAL APPROACH TO CHEMISTRY 211
6 Section 7.2 Valence Electrons and Bonding Patterns Covalent bonds Covalent bond formation In covalent bonds, electrons are shared between atoms, not transferred. The number of covalent bonds is equal to the number of unpaired valence electrons. The diagram below shows the number of covalent bonds by the main group elements. Covalent bond patterns Paired and unpaired electrons 1. Only non-metals and hydrogen are commonly found as covalently bonded parts of molecules. 2. Carbon-like elements (group 14) form four covalent bonds. 3. Nitrogen-like elements (group 15) form three covalent bonds. 4. Oxygen-like elements in (group 16) form two covalent bonds. 5. Halogens (group 17) form one covalent bond. 6. The number of covalent bonds is equal to the number of unpaired valence electrons. Going from left to right across the periodic table, notice that nitrogen has three unpaired electrons and one pair. The 8 electrons in s and p orbitals act like 8 strangers filling up four bench seats on a bus. Everyone prefers their own seat so up to four, each person sits solo. The fifth person must pair up with someone. The same is true of electrons. The fifth valence electron pairs up and is no longer available for bonding! For reasons of quantum mechanics, only unpaired electrons form bonds. 212 A NATURAL APPROACH TO CHEMISTRY
7 Atoms form bonds with every unpaired electron Every unpaired electron forms a bond Take a look at the molecule of vitamin C to the right. This molecule is made from several carbon, oxygen, and hydrogen atoms. Take a close look at each carbon atom. You will see that every carbon atom has four covalent bonds to other atoms. The oxygen atoms all from two covalent bonds, and the hydrogen atoms all form one covalent bond. Covalent bonds and noble gases Carbon has four valence electrons and they are all unpaired. Therefore carbon forms four chemical bonds. Oxygen has six valence electrons. Four of these electrons are paired and two are unpaired. Oxygen always forms two covalent bonds because it has two unpaired electrons. Hydrogen has one valence electron, and its closest noble gas is helium with two valence electrons. Hydrogen needs one more electron to be like helium. It gets this by forming one covalent bond with another atom. Unpaired electrons create very reactive atoms or molecules One quick way to tell how many covalent bonds an atom will form is to look at its Lewis dot structure. Atoms will form one covalent bond for each unpaired valence electron. Atoms or molecules that have unpaired electrons are highly reactive and are known as free radicals. These are the kind of molecules which can be responsible for aging and diseases like cancer. Sometimes free radicals are created as part of our own natural metabolism, and sometimes they are caused by outside sources like ultraviolet radiation from the sun. Antioxidants are considered an important part of a person s diet because of their role in preventing free radicals from reacting with and damaging DNA. free radical - a molecule or atom that is highly reactive due to its having one or more unpaired valence electrons. antioxidant - a molecule that reacts easily with free radicals. Some sources of antioxidants include brightly colored fruits and vegetables, vitamin E, and chocolate. A NATURAL APPROACH TO CHEMISTRY 213
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
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 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 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 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 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 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 informationElements 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
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 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 informationLook 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
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 informationTest 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
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 informationCHEMISTRY 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.
More informationPart 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
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 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 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 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 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 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 informationIonic 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
More informationPROTONS 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
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 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 informationMolecular 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,
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 information19.2 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
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 informationLewis 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
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 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 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 informationAP 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
More informationChapter 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
More informationMolecular Models & Lewis Dot Structures
Molecular Models & Lewis Dot Structures Objectives: 1. Draw Lewis structures for atoms, ions and simple molecules. 2. Use Lewis structures as a guide to construct three-dimensional models of small molecules.
More 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 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 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 informationElectrons 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
More informationANSWER 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
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 informationANSWER 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
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 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 informationType of Chemical Bonds
Type of Chemical Bonds Covalent bond Polar Covalent bond Ionic bond Hydrogen bond Metallic bond Van der Waals bonds. Covalent Bonds Covalent bond: bond in which one or more pairs of electrons are shared
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 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 informationB) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
More 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 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 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 informationLEWIS 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
More informationIONISATION 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
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 informationWorksheet 14 - Lewis structures. 1. Complete the Lewis dot symbols for the oxygen atoms below
Worksheet 14 - Lewis structures Determine the Lewis structure of 2 oxygen gas. 1. omplete the Lewis dot symbols for the oxygen atoms below 2. Determine the number of valence electrons available in the
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 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 informationStudent Exploration: Electron Configuration
Name: Date: Student Exploration: Electron Configuration Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule, electron configuration, Hund s rule, orbital, Pauli exclusion
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 informationTheme 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,
More informationChemical Calculations: Formula Masses, Moles, and Chemical Equations
Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic
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 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
More informationSuccess criteria You should be able to write the correct formula for any ionic compound
Chemical Formulas and Names of Ionic Compounds WHY? Going back to pre-historic times, humans have experimented with chemical processes that helped them to make better tools, pottery and weapons. In the
More informationChapter 8 Concepts of Chemical Bonding
Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three types: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms Ionic Bonding
More informationPeriodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
More informationGetting the most from this book...4 About this book...5
Contents Getting the most from this book...4 About this book....5 Content Guidance Topic 1 Atomic structure and the periodic table...8 Topic 2 Bonding and structure...14 Topic 2A Bonding....14 Topic 2B
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 informationBe (g) Be + (g) + e - O (g) O + (g) + e -
2.13 Ionisation Energies Definition :First ionisation energy The first ionisation energy is the energy required when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge
More informationChapter 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
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 informationElectron 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
More informationQuestion: Do all electrons in the same level have the same energy?
Question: Do all electrons in the same level have the same energy? From the Shells Activity, one important conclusion we reached based on the first ionization energy experimental data is that electrons
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 informationAtoms 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
More informationA pure covalent bond is an equal sharing of shared electron pair(s) in a bond. A polar covalent bond is an unequal sharing.
CHAPTER EIGHT BNDING: GENERAL CNCEPT or Review 1. Electronegativity is the ability of an atom in a molecule to attract electrons to itself. Electronegativity is a bonding term. Electron affinity is the
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 informationNomenclature and the Periodic Table To name compounds and to determine molecular formulae from names a knowledge of the periodic table is helpful.
Nomenclature and the Periodic Table To name compounds and to determine molecular formulae from names a knowledge of the periodic table is helpful. Atomic Number = number of protons Mass Number = number
More informationCopyrighted by Gabriel Tang B.Ed., B.Sc.
Chapter 8: The Periodic Table 8.1: Development of the Periodic Table Johann Dobereiner: - first to discover a pattern of a group of elements like Cl, Br, and I (called triads). John Newland: - suggested
More information(b) Formation of calcium chloride:
Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. An ionic compound combines a metal and a non-metal joined together by an ionic bond. 2. An electrostatic force holds
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 informationSummer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
More informationATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE
ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE Chapter 3 Vocabulary Words (27 words) Nucleus Atomic number Proton Mass number Neutron Isotopes Electron Atomic mass unit (amu) Energy level Average
More informationChemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
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 informationExam 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
More informationCHEMICAL NAMES AND FORMULAS
6 CEMICAL NAMES AND FORMULAS SECTION 6.1 INTRODUCTION TO CEMICAL BONDING (pages 133 137) This section explains how to distinguish between ionic and molecular compounds. It also defines cation and anion
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More information1.2 CLASSICAL THEORIES OF CHEMICAL BONDING
1. CLASSICAL TEORIES OF CEMICAL BONDING simply memorizing them. We ll consider some of the organic chemistry that is industrially important. Finally, we ll examine some of the beautiful applications of
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 informationAP CHEMISTRY 2007 SCORING GUIDELINES (Form B)
AP CHEMISTRY 2007 SCORING GUIDELINES (Form B) First Ionization Energy Question 6 Second Ionization Energy Third Ionization Energy (kj mol 1 ) (kj mol 1 ) (kj mol 1 ) Element 1 1,251 2,300 3,820 Element
More informationDirections: 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
More informationQuestion 4.2: Write Lewis dot symbols for atoms of the following elements: Mg, Na, B, O, N, Br.
Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents (atoms, ions etc.) together in a chemical species. Various theories
More informationChapter 4, Lesson 5: Energy Levels, Electrons, and Ionic Bonding
Chapter 4, Lesson 5: Energy Levels, Electrons, and Ionic Bonding Key Concepts The attractions between the protons and electrons of atoms can cause an electron to move completely from one atom to the other.
More informationChemistry 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
More informationChapter 3, Elements, Atoms, Ions, and the Periodic Table
1. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements? Ans. Mendeleev and Meyer 2. Who stated that the
More informationWe will not be doing these type of calculations however, if interested then can read on your own
Chemical Bond Lattice Energies and Types of Ions Na (s) + 1/2Cl 2 (g) NaCl (s) ΔH= -411 kj/mol Energetically favored: lower energy Like a car rolling down a hill We will not be doing these type of calculations
More informationSection 11.3 Atomic Orbitals Objectives
Objectives 1. To learn about the shapes of the s, p and d orbitals 2. To review the energy levels and orbitals of the wave mechanical model of the atom 3. To learn about electron spin A. Electron Location
More information