Notes: Electrons and Periodic Table (text Ch. 4 & 5)
|
|
- Lisa Alexander
- 5 years ago
- Views:
Transcription
1 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 get missing information from a fellow classmate or the chemistry website: I. The Wave Nature of Light Light travels through space as a wave. Waves have three primary characteristics: Wavelength (λ): the distance between 2 consecutive crests or troughs. Often measured in meters. Frequency (f): the number of wave cycles (successive crests or troughs) that pass a given point per unit of time. Often measured in cycles per second ( s 1 or Hertz). Speed (c): a constant for all forms of light; c = 3.00 x 10 8 m/s The speed of light, wavelength, and frequency are related by this formula: Wavelength and frequency are proportional 1
2 II. The Particle Nature of Light Not all properties of light can be explained by the wave model. Max Planck and Albert Einstein refined our understanding of light to include its particle nature. Light can be described as a stream of particles called photons. The details of the particle nature of light will not be investigated in this class. We will only highlight the relationship between the energy of light and its frequency: h = Planck s constant = x J. s Energy and frequency are proportional. All atoms absorb and emit light when excited by electricity or heat Elements emit light in unique, distinct patterns called Spectra corresponds to the movement of electrons between Spectra are like fingerprints that can be used to an element (Flame Test Lab) III. The Electron Cloud Electrons are found outside the nucleus, in a region of space called the. Electrons are organized in of positive integer value (n = 1, 2, 3,...). Within each energy level are, designated by a letter: s, p, d, or f. 2
3 Each sublevel corresponds to a certain electron cloud shape, called an. Analogy: The electron cloud is like an apartment building. The energy levels are like floors in the apartment building. The sublevels are like apartments on a floor of the building. Just like there are different sizes of sublevels, there are different sizes of apartments: 1 bedroom, 2 bedroom, etc. The orbitals are like rooms within an apartment. The electrons are like people living in the rooms. What do the atomic orbitals look like? Some examples: How are they organized around the nucleus? Here is a picture of the orbitals that make up the first four sublevels. Each orbital can hold a maximum of 2 electrons. An s sublevel contains 1 s orbital. How many total electrons can fit in an s sublevel? A p sublevel contains 3 p orbitals. How many total electrons can fit in a p sublevel? A d sublevel contains 5 d orbitals. How many total electrons can fit in a d sublevel? An f sublevel contains 7 f orbitals. How many total electrons can fit in an f sublevel? 3
4 IV. Electron Configurations and Orbital Diagrams Three rules govern the filling of atomic orbitals: 1. The Aufbau Principle: Electrons enter orbitals of lowest energy first. The Aufbau order lists the orbitals from lowest to highest energy: ( Aufbau is from the German verb aufbauen: to build up) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 14 6d 10 7p 6 First # = energy level, letter = type of sublevel, superscript # = max # of electrons You will learn to use the Periodic Table to determine the Aufbau order. It is not to be memorized. 2. The Pauli Exclusion Principle: An atomic orbital may hold at most 2 electrons, and they must have opposite spins (called paired spins). 3. Hund s Rule: When electrons occupy orbitals of equal energy (such as three p orbitals), one electron enters each orbital until all the orbitals contain one electron with spins parallel. Second electrons then add to each orbital so that their spins are paired with the first electron in the orbital. An electron configuration uses the Aufbau order to show how electrons are distributed within the atomic orbitals. Examples of electron configurations: Element Total # of Electrons Electron Configuration Carbon Fluorine Magnesium Argon Orbital diagrams show with arrow notation how the electrons are arranged in atomic orbitals for a given element. Element Orbital Diagram Carbon Fluorine Magnesium Argon 4
5 Some elements have large numbers of electrons, making their electron configurations cumbersome to write out in full. The noble gas configuration was developed for use with larger elements, as a shorthand way of writing electron configurations. Use the noble gas (Group 18) in the period above the element to write its noble gas configuration. Examples: Element Full Electron Configuration Noble Gas Configuration Sr Mn Bi V. Valence electrons Valence electrons are the electrons in the outer energy level of an atom. They are like the front lines of an army, because they are the ones involved in chemical reactions. Valence electrons are shared or transferred during reactions. The number of valence electrons is directly responsible for an element s chemical behavior and reactivity. The number of valence electrons can be determined from electron configurations. Count all the electrons in the outer (highest) energy level for that atom: Li Be B C N O F Element Electron Configuration # Valence Electrons Electron Dot Structure Ne The number of valence electrons for the representative element groups (Group A elements or Groups 1-2 and 13-18) follows an easy pattern from 1 8 going across the Periodic Table from left to right. Notice that the elements in a group (also called a family) all have the same number of valence electrons. Example: Group 1 elements (Alkali metals) all have 1 valence electron. Therefore, these elements will behave in similar ways. Try this: Find an element on the periodic table that has chemical reactivity similar to sulfur. 5
6 VI. Ions An ion is a charged particle that forms when an atom loses or gains electrons. Atoms lose or gain electrons in order to bond with other atoms and become more stable (less reactive). Remember: atoms are neutral because the # of protons (+) = the # of electrons (-) When an atom loses electrons, this results in a positively charged ion (cation). When an atom gains electrons, this results in a negatively charged ion (anion). Example: Sodium atoms have 11 p+ and 11 e-. If a sodium atom loses one electron, its charge will be +1 because it then has 11 p+ but only 10 e-. Element Ion formed Lost or gained electrons? How many? Sodium Na + Chlorine Cl Magnesium Mg 2+ Nitrogen N 3 Oxygen O 2 Aluminum Al 3+ A pattern exists with the Representative Elements (Groups 1, 2, 13, 15-17). With your teacher s assistance, assign the following charges on your periodic table to the Groups: Group 1: 1+ (or just +) Group 2: 2+ Group 13: 3+ Group 15 3 Group 16 2 Group 17 1 (or just ) Group 18 elements are the Noble Gases; for our purposes, they do not form ions. For Groups 3-12 and 14, ion charges can vary within the group, and even vary for one metal (ex. sometimes Cu is +1 and sometimes it is +2), so we cannot assign a charge for these groups as we did above. We will go into this in more detail later. You must memorize the charges for these 3 ions: (they are always the same) Ag is 1+ Zn is 2+ Cd is 2+ ***Note that the formulas and charges for polyatomic ions can be found on the back of your Periodic Table, with the exception of the phosphite ion: PO3 3- (memorize this one!) 6
7 VII. Ions and Electron Configuration Electron configurations for ions must be adjusted, based on the number of valence electrons lost or gained to form the ion. Element e- dot structure Lose or gain e-? How many? Ca.. Ca lose 2 O Ion formula w/ charge Ca 2+ Al F K N Now, for each of the above elements, write the electron configuration for the atom, and then adjust the configuration for the ion by losing or gaining the proper number of valence electrons. Element Electron config for ATOM Electron config for ION Ca Ca: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 Ca 2+ : 1s 2 2s 2 2p 6 3s 2 3p 6 (lost 2) O Al F K N Ionic compound form when a metal loses electrons to a nonmetal, and the resulting oppositely charged ions attract. With your teacher s assistance, make electron dot diagrams for the following pairs of elements, showing how electrons transfer to form the compound. 1) calcium and fluorine 2) sodium and nitrogen 3) aluminum and oxygen 7
8 VIII. Periodic Trends Trends in properties of the elements that follow a pattern down a group and across a period in the periodic table. 1. Trends in Atomic Radius Group trend: atomic radius going down a group. As you move down a group, energy levels are added, thus increasing the size of the electron cloud, so the atoms get larger. Periodic trend: atomic radius going left to right across a period. [NOTE: from now on, across a period will refer to the left-to-right direction] The atoms are getting heavier across a period. So why don t they get larger in volume? The reason has to do with increasing nuclear charge. With an increase in the # of protons from left to right, the nucleus gets a more powerful + charge. So it pulls the electron cloud in tighter. 2. Trends in Ionic Radius Positive ions are always smaller than the neutral metal atoms from which they were formed. When metal ions form, typically the outer energy level will be emptied, resulting in an overall smaller electron cloud. Also, the excess of protons compared to electrons draws the remaining electrons in closer. Example: Na vs. Na+ Negative ions are always larger than the neutral nonmetal atoms from which they were formed. There is more repulsion in the cloud due to the added electrons, therefore making it spread out, but there are no extra protons to pull it closer. Example: F vs. F - Group trend: Ionic radius (for both cations and anions) generally as you move down a group. This is mainly due to succeeding being filled. Periodic trend: Ionic radius (for both cations and anions) generally as you move across a period from left to right. This is mainly due to increasing. ***NOTE: anions within one period are larger than the cations within one period. This is due to the fact that cations have lost an energy level. 8
9 3. Trends in Ionization Energy (electron-losing) Ionization energy: the measure of the energy required to remove an electron from the outermost energy level of an atom. Group trend: ionization energy going down a group This is due to the shielding effect: an electron in the outer energy level of a large atom is easier to remove because it is well-shielded from the pull of the nucleus by the inner electrons. Diagram of the shielding effect: Periodic trend: ionization energy going across a period This is due to nuclear charge -- across a period, nuclear charge increases, so it becomes more difficult to remove an electron (held tighter). Note that this periodic trend supports the idea that metals have a much greater tendency to lose electrons than nonmetals do. 4. Trends in Electronegativity Electronegativity: the tendency of an atom to attract electrons to itself when it is chemically bonded with another element. Electronegativity is a numerical scale which can be used to predict whether atoms will form ionic or covalent bonds in molecules. In H2O, oxygen is more electronegative than hydrogen, so it pulls the electrons closer, and thus obtains a partially negative charge. Diagram of water molecule: Group trend: electronegativity down a group. Larger atoms have more energy levels, so it is harder for them to attract electrons to the nucleus (shielding effect). Periodic trend: electronegativity across a period. Nonmetallic character increases across a period, and nonmetals attract electrons more than metals do, because of increasing nuclear charge. 9
10 Summary of Periodic Trends: Atomic radius and ionic radius increase down a group, and decrease across a period. Ionization energy and electronegativity decrease down a group, and increase across a period. Write in the patterns that the trends follow on this periodic table: 1 Group 1 2 Periodic Table *Be sure that you can label and describe all of the following on a Periodic Table: (Study your gallery walk and the Periodic Table you colored) Groups and Periods Metals Nonmetals Metalloids Alkali metals Alkaline earth metals Transition metals Lanthanides Actinides Halogens Noble Gases 10
Name Chemistry-PAP Period. Notes: Electrons. Light travels through space as a wave. Waves have three primary characteristics:
Name Chemistry-PAP Period The Wave Nature of Light Notes: Electrons Light travels through space as a wave. Waves have three primary characteristics: Wavelength (λ): the distance between 2 consecutive crests
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 informationSAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca
SAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca 2. Which of the following influenced your answer to number one the most? a. effective nuclear
More informationClassify 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 informationChapter 10: Modern Atomic Theory and the Periodic Table. How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation
Chapter 10: Modern Atomic Theory and the Periodic Table How does atomic structure relate to the periodic table? 10.1 Electromagnetic Radiation Electromagnetic (EM) radiation is a form of energy that exhibits
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 informationUnit 2 - Electrons and Periodic Behavior
Unit 2 - Electrons and Periodic Behavior Models of the Atom I. The Bohr Model of the Atom A. Electron Orbits, or Energy Levels 1. Electrons can circle the nucleus only in allowed paths or orbits 2. The
More informationGetting to know the Periodic Table: Recall: Elements are organized based on atomic number and similar properties
Getting to know the Periodic Table: Recall: Elements are organized based on atomic number and similar properties 1. Find your staircase on the right side of the periodic table. Feel free to make the lines
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 informationWhy is it called a periodic table?
The Periodic Table Why is it called a periodic table? The properties of the elements in the table repeat in a "periodic" way (specific pattern). Periodic law: There is a periodic repetition of chemical
More informationElectronic Structure and Bonding Review
Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern
More informationThe Quantum Mechanical Model
Recall The Quantum Mechanical Model Quantum Numbers Four numbers, called quantum numbers, describe the characteristics of electrons and their orbitals Quantum Numbers Quantum Numbers The Case of Hydrogen
More information6.4 Electronic Structure of Atoms (Electron Configurations)
Chapter 6 Electronic Structure and Periodic Properties of Elements 317 Orbital n l m l degeneracy Radial nodes (no.) 4f 4 3 7 0 4p 4 1 3 2 7f 7 3 7 3 5d 5 2 5 2 Check Your Learning How many orbitals have
More informationFor the Periodic Table above indicate each of the following TRENDS: atomic size and ionic size. Na Na + F F - Ne < < < <
Chapter 6 Organizing the Elements THE PERIODIC TABLE AND PERIODIC LAW Periodic Table Summary Sheet For the Periodic Table above indicate each of the following TRENDS: atomic size and ionic size Na Na +
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 informationLIGHT AND THE QUANTUM MODEL
LIGHT AND THE QUANTUM MODEL WAVES Wavelength ( ) - length of one complete wave Frequency ( ) - # of waves that pass a point during a certain time period hertz (Hz) = 1/s Amplitude (A) - distance from the
More informationCHAPTER NOTES CHAPTER 14. Chemical Periodicity
Goals : To gain an understanding of : 1. Electron configurations 2. Periodicity. CHAPTER NOTES CHAPTER 14 Chemical Periodicity The periodic law states that when the elements are arranged according to increasing
More informationProfessor K. Section 8 Electron Configuration Periodic Table
Professor K Section 8 Electron Configuration Periodic Table Schrödinger Cannot be solved for multielectron atoms We must assume the orbitals are all hydrogen-like Differences In the H atom, all subshells
More informationName Date Class THE PERIODIC TABLE
Name Date Class 6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the
More informationElectron Configuration and Chemical Periodicity
Electron Configuration and Chemical Periodicity The Periodic Table Periodic law (Mendeleev, Meyer, 1870) periodic reoccurrence of similar physical and chemical properties of the elements arranged by increasing
More informationUnit 2 - Electrons and Periodic Behavior
Unit 2 - Electrons and Periodic Behavior I. The Bohr Model of the Atom A. Electron Orbits, or Energy Levels 1. Electrons can circle the nucleus only in allowed paths or orbits 2. The energy of the electron
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 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 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 informationName: Unit 3 Guide-Electrons In Atoms
Name: Unit 3 Guide-Electrons In Atoms Importance of Electrons Draw a complete Bohr model of the atom. Write an element s electron configuration. Know how the symbols used in ECs relate to electron properties
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 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 informationTo review Rutherford s model of the atom To explore the nature of electromagnetic radiation To see how atoms emit light
Objectives To review Rutherford s model of the atom To explore the nature of electromagnetic radiation To see how atoms emit light 1 A. Rutherford s Atom.but there is a problem here!! 2 Using Rutherford
More informationElectronic Structure and the Periodic Table. Unit 6 Honors Chemistry
Electronic Structure and the Periodic Table Unit 6 Honors Chemistry Wave Theory of Light James Clerk Maxwell Electromagnetic waves a form of energy that exhibits wavelike behavior as it travels through
More informationTrends in Atomic Size. Atomic Radius-one half the distance between the nuclei of two atoms of the same element when the atoms are joined
Periodic trends Trends in Atomic Size Atomic Radius-one half the distance between the nuclei of two atoms of the same element when the atoms are joined Trends in Atomic Size Group Trend: Atomic radii of
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 informationElectron Configurations and the Periodic Table
Electron Configurations and the Periodic Table The periodic table can be used as a guide for electron configurations. The period number is the value of n. Groups 1A and 2A have the s-orbital filled. Groups
More informationSection 11: Electron Configuration and Periodic Trends
Section 11: Electron Configuration and Periodic Trends The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 11.01 The Bohr Model of the Atom
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 informationAtomic Structure. Ch 3 Prentice Hall
Atomic Structure Ch 3 Prentice Hall The Nuclear Atom By 1919 Rutherford concluded that the atom has a dense positive center called the nucleus containing what he called protons The electrons surround
More informationHonors Chemistry: Chapter 4- Problem Set (with some 6)
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
More informationModern Atomic Theory and Electron Configurations
Chem 101 Modern Atomic Theory and Electron Configurations Lectures 8 and 9 Types of Electromagnetic Radiation Electromagnetic radiation is given off by atoms when they have been excited by any form of
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 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 informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
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 informationATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter is made of atoms. There are a limited number of types of atoms; these are the elements. (EU 1.A) Development of Atomic Theory Atoms are so small
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 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 informationWhy Patterns for Charges of Common Cations and Anions? Electrons in Atoms
Electrons in Atoms From Light to Energy of Electrons in Atom Quantum mechanical description of Atom 1. Principal quantum number: Shell 2. Orientation (shape) of : Subshell 3. Orbitals hold electrons with
More informationChapter 7. Electron Configuration and the Periodic Table
Chapter 7 Electron Configuration and the Periodic Table Topics Development of the periodic table The modern periodic table Effective nuclear charge Periodic trends in properties of elements Electron configuration
More informationPeriodic Table. Metalloids diagonal between metals and nonmetals. Have metallic and non-metallic properties
Chapter 6 Periodic Table Most elements are metals Metals are shiny, malleable, ductile, and good conductors of heat and electricity Most metals are solid at room temperature Non-metals in upper right corner,
More informationElectrons in Atoms. So why does potassium explode in water? Quantum Mechanics Periodic Trends Chemical Bonding
Electrons in Atoms So why does potassium explode in water? Quantum Mechanics Periodic Trends Chemical Bonding 12.1 Development of Atomic Models Dalton s Thompson s Rutherford s Bohr s carbon Quantum Model
More informationMade the FIRST periodic table
Made the FIRST periodic table 1869 Mendeleev organized the periodic table based on the similar properties and relativities of certain elements Later, Henri Moseley organized the elements by increasing
More informationName Class Date ELECTRONS AND THE STRUCTURE OF ATOMS
The Periodic Table ELECTRONS AND THE STRUCTURE OF ATOMS 6.1 Organizing the Elements Essential Understanding Although Dmitri Mendeleev is often credited as the father of the periodic table, the work of
More informationThe orbitals in an atom are arranged in shells and subshells. orbital 3s 3p 3d. Shell: all orbitals with the same value of n.
Shells and Subshells The orbitals in an atom are arranged in shells and subshells. n=3 orbital 3s 3p 3d Shell: all orbitals with the same value of n n=3 3s 3p 3d Subshell: all orbitals with the same value
More information2 Electons Electrons: Quantum Numbers, Energy Levels and Electron Configurations
Electrons: Quantum Numbers, Energy Levels and Electron Configurations For chemical reactions to occur a collision between atoms or molecules must happen. These collisions typically result in an exchange
More informationElectron Configuration and Periodic Trends - Chapter 5 section 3 Guided Notes
Electron Configuration and Periodic Trends - Chapter 5 section 3 Guided Notes There are several important atomic characteristics that show predictable that you should know. Atomic Radius The first and
More informationModern Atomic Theory. (a.k.a. the electron chapter!) Chemistry 1: Chapters 5, 6, and 7 Chemistry 1 Honors: Chapter 11
Modern Atomic Theory (a.k.a. the electron chapter!) 1 Chemistry 1: Chapters 5, 6, and 7 Chemistry 1 Honors: Chapter 11 ELECTROMAGNETIC RADIATION 2 Electromagnetic radiation. 3 4 Electromagnetic Radiation
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 informationAssessment Chapter 5 Pre-Test Chapter: The Periodic Law Use the periodic table below to answer the questions in this Chapter Test.
Assessment Chapter 5 Pre-Test Chapter: The Periodic Law Use the periodic table below to answer the questions in this Chapter Test. In the space provided, write the letter of the term or phrase that best
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 informationPeriodic Table Trends. Atomic Radius Ionic Radius Ionization Energy Electronegativity
Periodic Table Trends Atomic Radius Ionic Radius Ionization Energy Electronegativity 1. Atomic Radius Atomic Radius - distance from nucleus to outermost atom Measured by dividing the distance between 2
More informationHonors Unit 6 Notes - Atomic Structure
Name: Honors Unit 6 Notes - Atomic Structure Objectives: 1. Students will have a general understanding of the wave nature of light and the interrelationship between frequency, wavelength, and speed of
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 informationFocus Learning Targets for Periodic Trends and Bonding (1) Discuss the development of the periodic table by Mendeleev. (2) Locate and state important
Focus Learning Targets for Periodic Trends and Bonding (1) Discuss the development of the periodic table by Mendeleev. (2) Locate and state important properties of main chemical families including the
More informationPeriodic Classification and Properties Page of 6
The Modern Periodic Table In the modern Periodic table the elements are arranged according to electron configuration of the atoms of the elements. The elements are placed in the increasing order of their
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 information= proton (positive charge) = electron (negative charge) = neutron (no charge) A Z. ,, and are notations that represent isotopes of carbon.
ChemQuest 8 Name: Date: Hour: Information: Structure of the Atom Note the following symbols: (they are not to scale) = proton (positive charge) = electron (negative charge) = neutron (no charge) The following
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 informationChapter 8. Periodic Properties of the Element
Chapter 8 Periodic Properties of the Element Mendeleev (1834 1907) Ordered elements by atomic mass Saw a repeating pattern of properties Periodic law when the elements are arranged in order of increasing
More informationUnit 3. The Atom & Modern Atomic Theory
Unit 3 The Atom & Modern Atomic Theory Theories of the Atom Early Models & Thoughts: Democritus Matter is made up of tiny particles called atoms. Smallest unit that retains the identity of the element
More informationAP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity
AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 10-1 10-10 10-8 4 to 7x10-7 10-4 10-1 10 10 4 gamma
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 informationElectron Arrangement - Part 2
Brad Collins Electron Arrangement - Part 2 Chapter 9 Some images Copyright The McGraw-Hill Companies, Inc. Review Energy Levels Multi-electron 4d 4d 4d 4d 4d n = 4 4s 4p 4p 4p 3d 3d 3d 3d 3d n=3, l = 2
More informationWARM-UP. Draw each of the three models of the atom that we learned about last unit. Who came up with each? What was wrong with each?
WARM-UP Draw each of the three models of the atom that we learned about last unit. Who came up with each? What was wrong with each? 1:59 1:58 1:57 1:56 1:55 1:54 1:53 1:52 1:51 1:50 1:49 1:48 1:47 1:46
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 informationElectrons and Molecular Forces
Electrons and Molecular Forces Chemistry 30 Ms. Hayduk Electron Configuration Atomic Structure Atomic Number Number of protons in the nucleus Defines the element Used to organize the periodic table 1 Bohr
More informationValence Electrons. Periodic Table and Valence Electrons. Group Number and Valence Electrons. Learning Check. Learning Check.
Chapter 5 Lecture Chapter 5 Electronic Structure and Periodic Trends 5.6 Trends in Periodic Properties Learning Goal Use the electron configurations of elements to explain the trends in periodic properties.
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 informationLecture Presentation. Chapter 8. Periodic Properties of the Element. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 8 Periodic Properties of the Element Sherril Soman Grand Valley State University Nerve Transmission Movement of ions across cell membranes is the basis for the transmission
More information7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to
1. Which of the following is the most important factor in determining the properties of an element? a. Atomic mass b. Atomic radius c. Periodic table position d. Electron configuration 2. Similar properties
More informationWhite Light. Chapter 7 Electron Structure of the Atom
Chapter 7 Electron Structure of the Atom Electromagnetic Radiation and Energy The Bohr Model of the Hydrogen Atom The Modern Model of the Atom Periodicity of Electron Configurations Valence Electrons for
More informationLIMITATIONS OF RUTHERFORD S ATOMIC MODEL
ELECTRONS IN ATOMS LIMITATIONS OF RUTHERFORD S ATOMIC MODEL Did not explain the chemical properties of atoms For example, it could not explain why metals or compounds of metals give off characteristic
More informationPeriodic Relationships
Periodic Relationships 1 Tabulation of Elements Mendeleev (1869) Arranged by mass Tabulation by chem.& physical properties Predicted missing elements and properties 2 Modern Periodic Table Argon vs. potassium
More informationTrends in the Periodic Table
Trends in the Periodic Table A trend is a predictable change in a particular direction. Example: There is a trend in the alkali metals to increase in reactivity as you move down a group. Atomic Radius
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 informationGroup Trends: the trend that the atoms follow going down any particular group
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 informationELECTRONS IN ATOMS AND THE PERIODIC TABLE. Light and Energy. Chapter Nine
ELECTRONS IN ATOMS AND THE PERIODIC TABLE Chapter Nine Light and Energy! Electromagnetic radiation (EM) is an especially important form of energy for scientific study.! Many types of radiant energy are
More informationModern Atomic Theory CHAPTER OUTLINE
Chapter 3B Modern Atomic Theory 1 CHAPTER OUTLINE Waves Electromagnetic Radiation Dual Nature of Light Bohr Model of Atom Quantum Mechanical Model of Atom Electron Configuration Electron Configuration
More informationPeriodic Trends. Elemental Properties and Patterns
Periodic Trends Elemental Properties and Patterns The Periodic Law Dimitri Mendeleev was the first scientist to publish an organized periodic table of the known elements. He was perpetually in trouble
More information6.3 Periodic Trends > Chapter 6 The Periodic Table. 6.3 Periodic Trends. 6.1 Organizing the Elements. 6.2 Classifying the Elements
1 63 Periodic Trends > Chapter 6 The Periodic Table 61 Organizing the Elements 62 Classifying the Elements 63 Periodic Trends 2 63 Periodic Trends > CHEMISTRY & YOU How are trends in the weather similar
More informationTrends in Atomic Size. What are the trends among the elements for atomic size? The distances between atoms in a molecule are extremely small.
63 Periodic Trends > 63 Periodic Trends > CHEMISTRY & YOU Chapter 6 The Periodic Table 61 Organizing the Elements 62 Classifying the Elements 63 Periodic Trends How are trends in the weather similar to
More informationChapter 8. Periodic Properties of the Elements
Chapter 8 Periodic Properties of the Elements Mendeleev (1834 1907) Ordered elements by atomic mass. Saw a repeating pattern of properties. Periodic Law When the elements are arranged in order of increasing
More informationElectronic Structure of Atoms and the Periodic table. Electron Spin Quantum # m s
Electronic Structure of Atoms and the Periodic table Chapter 6 & 7, Part 3 October 26 th, 2004 Homework session Wednesday 3:00 5:00 Electron Spin Quantum # m s Each electron is assigned a spinning motion
More informationPeriodic Trends. Elemental Properties and Patterns
Periodic Trends Elemental Properties and Patterns The Periodic Law Dimitri Mendeleev was the first scientist to publish an organized periodic table of the known elements. Henry Moseley Discovered the proton
More informationChapter 7. Characteristics of Atoms. 7.1 Electromagnetic Radiation. Chapter 7 1. The Quantum Mechanical Atom. Atoms: How do we study atoms?
Chapter 7 The Quantum Mechanical Atom 1 Characteristics of Atoms Atoms: possess mass contain positive nuclei contain electrons occupy volume have various properties attract one another combine to form
More informationWorksheet 5 - Chemical Bonding
Worksheet 5 - Chemical Bonding The concept of electron configurations allowed chemists to explain why chemical molecules are formed from the elements. In 1916 the American chemist Gilbert Lewis proposed
More informationPeriodic Relationships
Periodic Relationships 1 Tabulation of Elements Mendeleev (1869) Arranged by mass Tabulation by chem.& physical properties Predicted missing elements and properties 2 Modern Periodic Table Argon vs. potassium
More informationChapter 5 The Periodic Law
z Chapter 5 The Periodic Law z Section 5-1 History of the Periodic Table Mendeleev noticed that when the elements were arranged in order of increasing atomic mass, certain similarities in their chemical
More informationChapter 9: Electrons and the Periodic Table
C h e m i s t r y 1 2 C h 9 : E l e c t r o n s a n d P e r i o d i c T a b l e P a g e 1 Chapter 9: Electrons and the Periodic Table Work on MasteringChemistry assignments What we have learned: Dalton
More informationThe Arrangement of Atoms in the Periodic Table
1 The Arrangement of Atoms in the Periodic Table [Material is from The Free High School Science Texts: Textbooks for High School Students Studying the Sciences Chemistry Grades 10 12. www.fhsst.org unless
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 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 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 information