Arrangement of Electrons in Atoms
|
|
|
- Timothy Ross
- 5 years ago
- Views:
Transcription
1 Page III-6b- / Chapter Six Part II Lecture Notes The Structure of Atoms and Periodic Trends Chapter Six Part Arrangement of Electrons in Atoms Electrons in atoms are arranged as SHELLS (n) SUBSHELLS (l) CH Professor Michael Russell ORBITALS (ml) Arrangement of Electrons in Atoms Electron Spin Quantum Number, ms Each orbital can be assigned no more than electrons! This is tied to the existence of a 4th quantum number, the electron spin quantum number, ms. ms arises naturally when relativity (Einstein) combined with quantum mechanics (Paul Dirac) Paul Dirac Magnetism In diamagnetic systems, all electron spins are paired - no net magnetic moment. In paramagnetic systems, unpaired spins present. Magnetic fields randomly arranged unless placed in an external magnetic field. Electron spin can be proven experimentally. Two spin directions are given by ms where ms = +/ and -/. Leads to magnetism in atoms and ions In ferromagnetic substances the orientations of magnetic fields from unpaired electrons are affected by spins from electrons around them. When an external field is applied and then removed, the substance maintains the magnetic moment and becomes a permanent magnet. Page III-6b- / Chapter Six Part II Lecture Notes Magnetism H - a magnetic field
2 Page III-6b- / Chapter Six Part II Lecture Notes Electron Spin Quantum Number Measuring Paramagnetism Paramagnetic: substance is attracted to a magnetic field. Substance has unpaired electrons. Diamagnetic: NOT attracted to a magnetic field; spin paired. Paramagnetic: substance is attracted to a magnetic field. Substance has unpaired electrons. Sample of FeO with strong magnet Sample of FeO Diamagnetic: NOT attracted to a magnetic field Pauli Exclusion Principle No two electrons in the same atom can have the same set of 4 quantum numbers. QUANTUM NUMBERS,,, 4,... l ---> subshell,,,... (n - ) ml ---> orbital -l l ms ---> electron spin +/ and -/ That is, each electron has a unique address which will consist of its own values of n, l, ml and ms. See: Quantum Numbers Handout Wolfgang Pauli Electrons in Atoms When n =, then l = and ml = this shell has a single orbital (s) to which e- can be assigned n =, l =, ml =, ms = + / - this is electron # n =, l =, ml =, ms = -/ - this is electron # When n =, then l = (s), (p) e- three p orbitals 6e- TOTAL = 8e- electron number s orbital n l ml ms / -/ s - / p 4 - -/ p 5 / p 6 -/ p 7 + / p 8 + -/ p s Electrons in Atoms When n =, then l = (s), (p), (d) s orbital ethree p orbitals 6efive d orbitals etotal = 8eEach electron has its own set of four quantum numbers! Wolfgang Pauli Page III-6b- / Chapter Six Part II Lecture Notes electron number n ---> shell n l ml ms / -/ / -/ / -/ / -/ / -/ / -/ / -/ / -/ / -/ s s p p p p p p d d d d d d d d d d
3 electron number Electrons in Atoms n l ml ms 4 / 4s 4 -/ 4s 4 - / 4p / 4p 5 4 / 4p 6 4 -/ 4p / 4p / 4p / 4d 4 - -/ 4d 4 - / 4d 4 - -/ 4d 4 / 4d 4 4 -/ 4d / 4d / 4d / 4d / 4d When n = 4, l = (s), (p), (d), (f) 4s orbital e- three 4p orbitals 6e- five 4d orbitals e- seven 4f orbitals 4e- TOTAL = e- and so on and so on... Page III-6b- / Chapter Six Part II Lecture Notes electron number n l ml ms / 4f 4 - -/ 4f 4 - / 4f 4 - -/ 4f 4 - / 4f / 4f 5 4 / 4f 6 4 -/ 4f / 4f / 4f / 4f 4 + -/ 4f 4 + / 4f 4 + -/ 4f Distribution of Electrons in Shells Assigning Electrons to Atoms Electrons generally assigned to orbitals of successively higher energy. For H atoms, E = - Rhc(/n ). E depends only on n. For many-electron atoms, energy depends on both n and l. Assigning Electrons to Subshells In H atom all subshells of same n have same energy. In many-electron atom: a) subshells increase in energy as value of n + l increases. (The important n + l rule) b) for subshells of same n + l, subshell with lower n is lower in energy. See Electron Configurations Handout Using the n + l rule assumes zero point energy - the lowest energy state possible, or ground state An Aufbau Diagram Electron Filling Order Writing Atomic Electron Configurations Two ways of writing configs. One is called the spectroscopic or "spdf" notation. SPECTROSCOPIC NOTATION for H, atomic number = s no. of electrons Aufbau comes from a German word meaning building up, formulated by Bohr and Pauli in 9s Page III-6b- / Chapter Six Part II Lecture Notes value of n value of l
4 Writing Atomic Electron Configurations Page III-6b-4 / Chapter Six Part II Lecture Notes Two ways of writing configs. Other is called the orbital box notation. ORBITAL BOX NOTATION for He, atomic number = s s Arrows depict electron spin One electron has n =, l =, m l =, m s = + / Other electron has n =, l =, m l =, m s = - / Atomic Electron Configurations Diagram Electron Configurations and the Periodic Table Lithium Group A Atomic number = s s ---> total electrons paramagnetic s s p p s Beryllium Boron s p Group A Atomic number = 4 s s ---> 4 total electrons diamagnetic s p Group A Atomic number = 5 s s p ---> 5 total electrons paramagnetic s p s p s s Page III-6b-4 / Chapter Six Part II Lecture Notes
5 Page III-6b-5 / Chapter Six Part II Lecture Notes s s s p p Carbon Group 4A Atomic number = 6 s s p ---> 6 total electrons paramagnetic Friedrich Hund Here we see for the first time HUND'S RULE. When placing electrons in a set of orbitals having the same energy, we place them singly as long as possible. s s s p p Nitrogen Group 5A Atomic number = 7 s s p ---> 7 total electrons paramagnetic Oxygen Fluorine s p Group 6A Atomic number = 8 s s p 4 ---> 8 total electrons paramagnetic s p Group 7A Atomic number = 9 s s p 5 ---> 9 total electrons paramagnetic s p s p s s s s s p p Neon Group 8A Atomic number = s s p 6 ---> total electrons diamagnetic Note that we have reached the end of the nd period, and the nd shell is full! Page III-6b-5 / Chapter Six Part II Lecture Notes Electron Configurations of p-block Elements
![All Group A elements have [core]ns configurations.](/docs-images/89/98940750/images/6-2.jpg "Aluminum Group A Atomic number = s s p 6 s p or [Ne] s p All * Group A elements have")
![[core] ns np configurations where n is the period number.](/docs-images/89/98940750/images/6-3.jpg "* some have (n-)d as well s s s p p Phosphorus Group 5A Atomic number = 5 s s p 6 s p or")
![[Ne] s p Relationship of Electron Configuration and Region of the Periodic Table All *](/docs-images/89/98940750/images/6-4.jpg "Group 5A elements have [core ] ns np configurations where n is the period number.")
![have the configuration [core]ns x (n - )d y and so are "d-block" elements.](/docs-images/89/98940750/images/6-6.jpg "K s s p 6 s p 6 4s or [Ar]4s Ca s s p 6 s p 6 4s or [Ar]4s Sc s s p 6 s p 6 4s d or")
![[Ar]4s d Ti s s p 6 s p 6 4s d or [Ar]4s d V s s p 6 s p 6 4s d or [Ar]4s d Cr s s p 6 s](/docs-images/89/98940750/images/6-7.jpg "p 6 4s d 5 or [Ar]4s d 5 Mn s s p 6 s p 6 4s d 5 or [Ar]4s d 5 Note: exceptions!")
6 Page III-6b-6 / Chapter Six Part II Lecture Notes Sodium Group A Atomic number = s s p 6 s or "neon core" + s [Ne] s (uses noble gas notation) And: we have begun a new period! All Group A elements have [core]ns configurations. Aluminum Group A Atomic number = s s p 6 s p or [Ne] s p All * Group A elements have [core] ns np configurations where n is the period number. * some have (n-)d as well s s s p p Phosphorus Group 5A Atomic number = 5 s s p 6 s p or [Ne] s p Relationship of Electron Configuration and Region of the Periodic Table All * Group 5A elements have [core ] ns np configurations where n is the period number. * some have (n-)d also s s s p p Gray = s block Orange = p block Green = d block Violet = f block Transition Metals Fourth Period Electron Configurations All transition metals have the configuration [core]ns x (n - )d y and so are "d-block" elements. K s s p 6 s p 6 4s or [Ar]4s Ca s s p 6 s p 6 4s or [Ar]4s Sc s s p 6 s p 6 4s d or [Ar]4s d Ti s s p 6 s p 6 4s d or [Ar]4s d V s s p 6 s p 6 4s d or [Ar]4s d Cr s s p 6 s p 6 4s d 5 or [Ar]4s d 5 Mn s s p 6 s p 6 4s d 5 or [Ar]4s d 5 Note: exceptions! Chromium Iron Copper Cu s s p 6 s p 6 4s d or [Ar]4s d Page III-6b-6 / Chapter Six Part II Lecture Notes
![Page III-6b-7 / Chapter Six Part II Lecture Notes Electron Configuration Anomalies Cr s s p 6 s p 6 4s d 5 or [Ar]4s d 5 Cu](/docs-images/89/98940750/images/7-0.jpg "s s p 6 s p 6 4s d or [Ar]4s d Chromium, copper and other elements do not follow the n + l filling orders Anomalies arise")
![have the configuration [core]ns x (n - )d y (n - )f z and so are "f-block" elements Exceptions exist: Cerium [Xe] 6s 5d 4f](/docs-images/89/98940750/images/7-2.jpg "[Xe] 6s 4f expected Uranium [Rn] 7s 6d 5f [Rn] 7s 5f 4 expected Transition Metals Electron Configurations Filling Order")
![Iron: [Ar] 4s d 6 Zinc: [Ar] 4s d Technetium: [Kr] 5s 4d 5 Niobium: [Kr] 5s 4d Osmium: [Xe] 6s 4f 4 5d 6 Meitnerium: [Rn]](/docs-images/89/98940750/images/7-3.jpg "7s 5f 4 6d 7 notice f orbitals in 6th period & beyond Anion Configurations Cation Configurations To form anions from")
![elements add or more e- using normal n + l rules P [Ne] s p + e- ---> P - [Ne] s p 6 To form cations from elements remove](/docs-images/89/98940750/images/7-6.jpg "or more e- from subshell of highest n [or highest (n + l)].")
7 Page III-6b-7 / Chapter Six Part II Lecture Notes Electron Configuration Anomalies Cr s s p 6 s p 6 4s d 5 or [Ar]4s d 5 Cu s s p 6 s p 6 4s d or [Ar]4s d Chromium, copper and other elements do not follow the n + l filling orders Anomalies arise from stability associated with half-filled and completely filled d-subshells. Know how n + l rule works, and know that anomalies exist on the periodic table Lanthanides and Actinides All these elements have the configuration [core]ns x (n - )d y (n - )f z and so are "f-block" elements Exceptions exist: Cerium [Xe] 6s 5d 4f [Xe] 6s 4f expected Uranium [Rn] 7s 6d 5f [Rn] 7s 5f 4 expected Transition Metals Electron Configurations Filling Order Iron: [Ar] 4s d 6 Zinc: [Ar] 4s d Technetium: [Kr] 5s 4d 5 Niobium: [Kr] 5s 4d Osmium: [Xe] 6s 4f 4 5d 6 Meitnerium: [Rn] 7s 5f 4 6d 7 notice f orbitals in 6th period & beyond Anion Configurations Cation Configurations To form anions from elements add or more e- using normal n + l rules P [Ne] s p + e- ---> P - [Ne] s p 6 To form cations from elements remove or more e- from subshell of highest n [or highest (n + l)]. P [Ne] s p - e- ---> P + [Ne] s s p s p s p s p s p s p s p s p s s s s Page III-6b-7 / Chapter Six Part II Lecture Notes
8 Page III-6b-8 / Chapter Six Part II Lecture Notes Ion Configurations For transition metals, remove ns electrons and then (n - ) electrons. Fe [Ar] 4s d 6 ---> Fe + [Ar] d 6 ---> Fe + [Ar] d 5 Fe Fe + Magnetic Properties Magnetic properties of ions assist us with charges DIAMAGNETIC ions have no unpaired electrons. Ions with unpaired electrons are PARAMAGNETIC. As number of unpaired electrons increases, the degree of paramagnetism also increases 4s d To form cations, always remove electrons of highest n value first! 4s 4s d Fe + d 4s 4s d d Zn + diamagnetic Mn + most paramagnetic, 5 unpaired e - s 4s d Fe + paramagnetic, 4 unpaired e - s Periodic Trends CH Q&D Guide to Periodic Trends: Atomic and ionic size: increase left and down Ionization energy and Electron affinity: increase right and up See Periodic Trends Handout CH Periodic Trends "Cheat Sheet" Larger orbitals. Electrons held less tightly. Electrons held more tightly Effective Nuclear Charge, Z* Z* is the effective nuclear charge experienced by the outermost electrons Inner electrons screen the effect of the nuclear charge from the outermost electrons Explains why E(s) < E(p) Z* increases across a period owing to incomplete shielding by inner electrons. Estimate Z* by --> [ Z - (no. inner electrons) ] Charge felt by s e- in Li: Z* = - = Be Z* = 4 - = B Z* = 5 - = and so on! Effective Nuclear Charge, Z* The s electron PENETRATES the region occupied by the s electron. s electron experiences a higher positive charge than expected. Page III-6b-8 / Chapter Six Part II Lecture Notes
9 Area screened by s electrons Page III-6b-9 / Chapter Six Part II Lecture Notes Effective Nuclear Charge, Z* Electron cloud for s electrons Effective Nuclear Charge Z* is the nuclear charge experienced by the outermost electrons due to screening by inner electrons Atom Z* Experienced by Electrons in Valence Orbitals Li +.8 Be??? (~) B +.58 C +. N +.85 O F +5. Increase in Z* across a period Values calculated using Slater s Rules for determining effective nuclear charge: Orbital Energies Orbital energies drop as Z* increases Atomic Size SIZE Size increases as you go down a group. Because electrons are added further from the nucleus, there is less attraction. Size increases on going right to left across a period. n = n = n = n= 4 n = 5 n = 6 r (pm) Moving down group IA, the atomic radii increase with the principle quantum number Group() radii 5 6 n Moving across the rd period we see the atomic radii of the elements decrease. Atomic radii generally increase going right to left on the periodic table. Page III-6b-9 / Chapter Six Part II Lecture Notes r (pm) rd period radii group number
10 Atomic Radii Page III-6b- / Chapter Six Part II Lecture Notes Trends in Atomic Size Radius (pm) 5 K 5 nd period Li rd period Na st transition series Ne Ar Kr 5 He Atomic Number Li,5 pm e and p Ion Sizes Does + the size go up or down when Li +, 6 pm e and p losing an electron to form a cation? Li,5 pm e and p Ion Sizes Li +, 6 pm e and p CATIONS are SMALLER than the atoms from which they come. The electron/proton attraction has gone UP and so size DECREASES. + Forming a cation. F,64 pm 9e and 9p Ion Sizes Does the size go up or down - when gaining an F - electron, 6 pmto form an anion? e and 9 p F,64 pm 9e and 9p Ion Sizes Forming an anion. ANIONS are LARGER than the atoms from which they come. The electron/proton attraction has gone DOWN and so size INCREASES. Trends in ion sizes are the same as atom sizes. - F -, 6 pm e and 9 p Page III-6b- / Chapter Six Part II Lecture Notes
11 Page III-6b- / Chapter Six Part II Lecture Notes Trends in Ion Sizes Redox Reactions Why do metals lose electrons in their reactions? Why does Mg form Mg + ions and not Mg +? Why do nonmetals take on electrons? Ionization Energy Trends in Ionization Energy Mg (g) + 78 kj ---> Mg + (g) + e- Mg + (g) + 45 kj ---> Mg + (g) + e- Mg + (g) + 77 kj ---> Mg + (g) + e- Mg + has protons and only electrons. Therefore, IE for Mg + > Mg. Energy IE = energy cost required is very high to remove to dip into an electron a shell of lower from an n. atom This is in why the gas ox. no. phase. = Group no. Trends in Ionization Energy IE increases R to L across a period because Z* increases. Metals lose electrons more easily than nonmetals. Metals are good reducing agents. Nonmetals lose electrons with difficulty. Trends in Ionization Energy IE increases up a group because size decreases. Reducing ability generally increases down the periodic table (such as in the reactions of Li, Na, and K) Page III-6b- / Chapter Six Part II Lecture Notes
![N atom N- ion [He] [He] + electron EA = 4 kj EA = kj Trends in Electron Affinity Trends](/docs-images/89/98940750/images/12-4.jpg "in Electron Affinity Affinity for electron increases left to right across a period (EA")
12 Lithium Page III-6b- / Chapter Six Part II Lecture Notes Periodic Trend in the Reactivity of Alkali Metals with Water Electron Affinity A few elements GAIN electrons to form anions. Electron affinity is the energy involved when an atom gains an electron. A(g) + e- ---> A - (g) E.A. = E Sodium Potassium Electron Affinity of Oxygen Electron Affinity of Nitrogen E is EXOthermic because O has an affinity for an e-. O atom [He] O - ion [He] + electron E is zero due to electron-electron repulsion. N atom N- ion [He] [He] + electron EA = 4 kj EA = kj Trends in Electron Affinity Trends in Electron Affinity Affinity for electron increases left to right across a period (EA becomes more negative). Affinity increases as you move up a group (EA becomes more negative). Page III-6b- / Chapter Six Part II Lecture Notes Notice: EA (F) < EA (Cl) unknown mechanism, electron repulsion? atom size?
13 Implications of Periodic Trends Useful in predicting reactivities, chemical formulas, etc. Page III-6b- / Chapter Six Part II Lecture Notes End of Chapter 6 Part Metals: low ionization energy, give up electrons easily Nonmetals: high electron affinity, love electrons from metals See also: Chapter Six Part Study Guide Chapter Six Part Concept Guide Page III-6b- / Chapter Six Part II Lecture Notes
Chapter 7 The Structure of Atoms and Periodic Trends
Chapter 7 The Structure of Atoms and Periodic Trends Jeffrey Mack California State University, Sacramento Arrangement of Electrons in Atoms Electrons in atoms are arranged as SHELLS (n) SUBSHELLS (l) ORBITALS
Quantum theory predicts that an atom s electrons are found in: To account that orbitals hold two electrons, we need:
Quantum theory predicts that an atom s electrons are found in: To account that orbitals hold two electrons, we need: Shells (principle quantum number, n) Subshells (angular momentum, l) Orbitals (magnetic
Electron Configuration. The electron configuration of an atom tells us how the electrons are distributed among the various atomic orbitals.
Electron Configuration The electron configuration of an atom tells us how the electrons are distributed among the various atomic orbitals. Spin Quantum Number, m s In the 1920s, it was discovered that
Electron 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
6.4 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
The 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
Atomic Electron Configurations and Periodicity
Atomic Electron Configurations and Periodicity Electron Spin The 4 th quantum number is known as the spin quantum number and is designated by m s. It can have the value of either + ½ or ½ It roughly translates
Ch 8 Electron Configurations and Periodicity (Periodic table)
Ch 8 Electron Configurations and Periodicity (Periodic table) - An e 1 configuration is an atom s particular distribution of e 1 among the available subshells and orbitals. For example, the ground state
Electron 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
CHEMISTRY - CLUTCH CH.8 - PERIODIC PROPERTIES OF THE ELEMENTS
!! www.clutchprep.com CONCEPT: ELECTRON CONFIGURATIONS In this chapter we will focus on how an element s - the distribution of electrons within the orbitals of its atoms relates to its chemical and physical
Professor 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
2011 CHEM 120: CHEMICAL REACTIVITY
2011 CHEM 120: CHEMICAL REACTIVITY INORGANIC CHEMISTRY SECTION Lecturer: Dr. M.D. Bala Textbook by Petrucci, Harwood, Herring and Madura 15 Lectures (4/10-29/10) 3 Tutorials 1 Quiz 1 Take-home test https://chemintra.ukzn.ac.za/
Mendeleev s Periodic Law
Mendeleev s Periodic Law Periodic Law When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically. Mendeleev s Periodic Law allows us to predict what
DEVELOPMENT OF THE PERIODIC TABLE
DEVELOPMENT OF THE PERIODIC TABLE Prior to the 1700s, relatively few element were known, and consisted mostly of metals used for coinage, jewelry and weapons. From early 1700s to mid-1800s, chemists discovered
Periodic 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
[3.3] Energy Level Diagrams and Configurations
![[3.3] Energy Level Diagrams and Configurations](/thumbs/87/96003907.jpg "[3.3] Energy Level Diagrams and Configurations")
[3.3] Energy Level Diagrams and Configurations 1 Energy Level Diagrams Energy level diagrams are used to represent the electron arrangement in an atom 2 Pauli s Exclusion Principle No two electrons have
HL Chemistry Topic 12 Atomic Structure
Define: ionization energy - 1 - Trends in Ionization Energy in the Periodic Table Why do these trends in ionization energy occur? Background information: Understand the concept of effective nuclear charge
Notes: 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
Electron 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
Chapter 3 Classification of Elements and Periodicity in Properties
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
The Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol λ.
CHAPTER 7 Atomic Structure Chapter 8 Atomic Electron Configurations and Periodicity 1 The Electronic Structures of Atoms Electromagnetic Radiation The wavelength of electromagnetic radiation has the symbol
נושא מס' 8: המבנה האלקטרוני של אטומים. Electronic Structure of Atoms. 1 Prof. Zvi C. Koren
נושא מס' 8: המבנה האלקטרוני של אטומים Electronic Structure of Atoms 1 Prof. Zvi C. Koren 19.07.10 The Electron Spin From further experiments, it was evident that the e had additional magnetic properties
CHEM N-3 November 2014
CHEM1101 2014-N-3 November 2014 Electron affinity is the enthalpy change for the reaction A(g) + e A (g). The graph below shows the trend in electron affinities for a sequence of elements in the third
Chapter 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
Chemistry (www.tiwariacademy.com)
() Question 3.1: What is the basic theme of organisation in the periodic table? Answer 1.1: The basic theme of organisation of elements in the periodic table is to classify the elements in periods and
Electron Configuration and Chemical Periodicity. Chapter Eight. AP Chemistry
Electron Configuration and Chemical Periodicity Chapter Eight AP Chemistry General Review Information about the Periodic Table Organization of the Elements 1869: Dmitri Mendeleev - Published an organizational
Periodic 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
Chapter 5. Periodicity and the Electronic Structure of Atoms
Chapter 5 Periodicity and the Electronic Structure of Atoms Electron Spin experiments by Stern and Gerlach showed a beam of silver atoms is split in two by a magnetic field the experiment reveals that
Chap 7 Part 2Tc.notebook November 02, 2017
Chapter 7 Section 4 11 Quantum mechanics electrons are organized in atoms in very specific ways energy levels represent distances from the nucleus inside energy levels are orbitals that can hold 2 electrons
Electron Configurations
Section 3 Electron Configurations Key Terms electron configuration Pauli exclusion principle noble gas Aufbau principle Hund s rule noble-gas configuration Main Ideas Electrons fill in the lowest-energy
ELECTRON CONFIGURATION AND THE PERIODIC TABLE
ELECTRON CONFIGURATION AND THE PERIODIC TABLE The electrons in an atom fill from the lowest to the highest orbitals. The knowledge of the location of the orbitals on the periodic table can greatly help
Chapter 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
Question 3.2: Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
Lecture 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
Periodicity & Many-Electron Atoms
Chap. 8 ELECTRON CONFIGURAT N & CEMICAL PERIODICITY 8.1-8.2 Periodicity & Many-Electron Atoms Understand the correlation of electron configuration and the periodic character of atomic properties such as
CDO AP Chemistry Unit 5
1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic
Chapter 7. Generally, the electronic structure of atoms correlates w. the prop. of the elements
Chapter 7 Periodic Properties of the Elements I) Development of the P.T. Generally, the electronic structure of atoms correlates w. the prop. of the elements - reflected by the arrangement of the elements
Electronic 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
Chapter 8. Mendeleev. Mendeleev s Predictions. Periodic Properties of the Elements
Chapter 8 Periodic Properties of the Elements Mendeleev Order elements by atomic mass Saw a repeating pattern of properties Periodic Law When the elements are arranged in order of increasing atomic mass,
Electron configuration: shows which orbitals are occupied in an atom, and how many electrons they contain
ch8blank Page 1 Chapter 8: Periodic properties of the elements Electron configuration: shows which orbitals are occupied in an atom, and how many electrons they contain Ground state: lowest energy, most
Electron Configuration & Periodicity Unit 3
Name: Electron Configuration & Periodicity Unit 3 (seven class periods) Unit 3.1: First Ionization Energy & Photoelectron Spectroscopy 1) Coulombs Law a) The force of attraction between two charged objects
CHAPTER 2 MANY-ELECTRON ATOMS AND THE PERIODIC TABLE
CHAPTER MANY-ELECTRON ATOMS AND THE PERIODIC TABLE.1 (a) is incorrect because the magnetic quantum number ml can have only whole number values. (c) is incorrect because the maximum value of the angular
Chapter 8: Periodic Properties of the Elements
C h e m i s t r y 1 A : C h a p t e r 8 P a g e 1 Chapter 8: Periodic Properties of the Elements Homework: Read Chapter 8. Work out sample/practice exercises Check for the MasteringChemistry.com assignment
Unit 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
Creating Energy-Level Diagrams Aufbau (building up) Principle Electrons are added to the lowest energy orbital available.
3.6 Atomic Structure and the Periodic Table Bohr's Theory Was Incorrect Because... Only explained the line spectrum of hydrogen Position and motion of an e cannot be specified (since the e is so small,
Chemistry 11. Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms
Chemistry 11 Unit 8 Atoms and the Periodic Table Part II Electronic Structure of Atoms 2 1. Atomic number and atomic mass In the previous section, we have seen that from 50 to 100 years after Dalton proposed
MANY ELECTRON ATOMS Chapter 15
MANY ELECTRON ATOMS Chapter 15 Electron-Electron Repulsions (15.5-15.9) The hydrogen atom Schrödinger equation is exactly solvable yielding the wavefunctions and orbitals of chemistry. Howev er, the Schrödinger
Notes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
Quiz 2/ A/ How many orbitals are possible for n=3? B/ How many orbital nodes do 2S,3P,4d and 5f orbitals exhibit? 11/11/2016 Dr. Mohammed H.
Quiz 2/ A/ How many orbitals are possible for n=3? B/ How many orbital nodes do 2S,3P,4d and 5f orbitals exhibit? 11/11/2016 Dr. Mohammed H. Said 1 lecture 2 Effective nuclear charge The effective nuclear
CHEMISTRY - BROWN 13E CH.7 - PERIODIC PROPERTIES OF THE ELEMENTS
!! www.clutchprep.com CONCEPT: EFFECTIVE NUCLEAR CHARGE & SLATER S RULES When looking at any particular electron within an atom it experiences two major forces. A(n) force from the nucleus and a(n) force
Made 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
Chapter 8. Electron Configuration and Chemical Periodicity 10/17/ Development of the Periodic Table
Chapter 8 Electron Configuration and Chemical Periodicity 8-1 Electron Configuration and Chemical Periodicity 8.1 Development of the Periodic Table 8.2 Characteristics of Many-Electron Atoms 8.3 The Quantum-Mechanical
ATOMIC 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
Orbital Diagrams & Electron Configurations for Atoms and Ions
Orbital Diagrams & Electron Configurations for Atoms and Ions Section 3.5 The Periodic Table is like a MAP that describes the arrangement of electrons within their orbitals. Orbital diagrams represent
ATOMIC 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
Part 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
ATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY
ATOMIC THEORY, PERIODICITY, and NUCLEAR CHEMISTRY Note: For all questions referring to solutions, assume that the solvent is water unless otherwise stated. 1. The nuclide is radioactive and decays by the
-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
170 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
LIGHT 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
Section 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
I. The Periodic Law and the Periodic Table. Electronic Configuration and Periodicity. Announcements Newland Law of Octaves
Announcements EM radiation --Exam 3 Oct 3...Includes chapters 7/8/9/10 The excluded items include: 1. Classical distinction between energy and matter (p. 217) 2. Numerical problems involving the Rydberg
CHAPTER 6. Chemical Periodicity
CHAPTER 6 Chemical Periodicity 1 Chapter Goals 1. More About the Periodic Table Periodic Properties of the Elements 2. Atomic Radii 3. Ionization Energy (IE) 4. Electron Affinity (EA) 5. Ionic Radii 6.
Periodic Properties (Booklet Solution)
Periodic Properties (Booklet Solution) Foundation Builders (Objective). (B) Law of triads states that in the set of three elements arranged in increasing order of atomic weight, having similar properties,
Chapter 2 Atoms and the Periodic Table
Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals
Chapter 6 Part 3; Many-electron atoms
Chapter 6 Part 3; Many-electron atoms Read: BLB 6.7 6.9 HW: BLB 6:59,63,64,67,71b-d,74,75,90,97; Packet 6:10 14 Know: s & atoms with many electrons Spin quantum number m s o Pauli exclusion principle o
Electronic configurations, Auf-bau principle, Pauli principle, Hunds rule 1. Which of the following statements in relation to the hydrogen atom is correct? 1) 3s and 3p orbitals are of lower energy than
Chapter 3 Classification of Elements and Periodicity in Properties
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
ELECTRON CONFIGURATION OF ATOMS
ELECTRON CONFIGURATION OF ATOMS 1 Electron Configuration? is the distribution of electrons within the orbitals of its atoms, in relation with chemical and physical properties Objectives: to show how the
Objectives: Learn how to show Electron configuration using:
4 WAYS to SHOW the Electron Configuration(Electron arrangement) Objectives: Learn how to show Electron configuration using: 1. Using Aufbau Energy Diagrams 2. Orbital Diagrams 3. Long hand Electron configuration
CHEMISTRY. CHM201 Class #16 CHEMISTRY. Chapter 7 Continued. Chapter 7 Outline for Class #16
CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies CHM201 Class #16 Chemistry, 5 th Edition Copyright 2017, W. W. Norton & Company CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies Chapter
ORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom.
160 ORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom. 4p 3d 4s 3p 3s 2p 2s 1s Each blank represents an ORBITAL, and can hold two electrons. The 4s subshell
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
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
Homework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2
Name Period Homework Packet Unit 2 1. Which of the following is the correct empirical formula for a compound that has 37.5% C, 12.6% H, and 49.9% O? (A) C 2 H 4 O (B) CH 4 O 2 (C) CH 5 O 2 (D) CH 4 O (E)
Topic 2 : Atomic Structure
Topic 2 : Atomic Structure AJC/P2/Q1a 1. The first ionisation energy of aluminium will be lower than that of sulphur, as S has a higher nuclear charge than Al, but the shielding effect is similar for both
Use the Venn Diagram to compare and contrast the Bohr Model of the atom with the Quantum Mechanical Model of atom
Use the Venn Diagram to compare and contrast the Bohr Model of the atom with the Quantum Mechanical Model of atom Bohr Model Quantum Model Energy level Atomic orbital Quantum Atomic number Quantum mechanical
Modern 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
Unit 8 Building Atoms with Quantum Leaps
Oh boy... Sam Beckett (from Quantum Leap) Unit 8 Building Atoms with Quantum Leaps Physicists Put Atom in Two Places at Once This was the headline in the science section of the New York Times on May 28,
AS VII Periodic Trends
chem101/3, wi2010 po 07 1 AS VII Periodic Trends chem101/3, wi2010 po 07 2 recall: Shielding Z = nuclear charge = # of protons (p + s) Shielding & Repulsion; Z eff Trends: size ionization energy, IE electron
Quantum Theory & Electronic Structure of Atoms. It s Unreal!! Check your intuition at the door.
Quantum Theory & Electronic Structure of Atoms It s Unreal!! Check your intuition at the door. 1 Quantum Theory of the Atom Description of the atom and subatomic particles. We will focus on the electronic
Advanced Theories of Atomic Structure: Atomic Orbitals
Advanced Theories of Atomic Structure: Atomic Orbitals What are the more advanced theories of atomic structure? Richard Feynman, 1918 1988. Winner of the 1965 Nobel Prize in Physics. The modern scientific
Chapter 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
The structure of the atom
The structure of the atom 1.Rutherford s model of the atom 2. Quantum-mechanics model of the atom The wave nature of microparticles motion The electron cloud The quantum numbers 1. Rutherford s model of
Where are the s, p, d, f orbitals located on the periodic table? Identify them on the diagram below.
Chapter 4 Arrangement of Electrons in Atoms Section 3: Electron Configuration Objectives: Be able to define: Aufbau Principle, Pauli Exclusion Principle, Hund s rule. Be able to list the number of electrons
Test 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
UNIT #3: Electrons in Atoms/Periodic Table and Trends
Name: Period: UNIT #3: Electrons in Atoms/Periodic Table and Trends 1. ELECTRON CONFIGURATION Electrons fill the space surrounding an atom s nucleus in a very specific order following the rules listed
PowerPoint to accompany. Chapter 6. Periodic Properties of the Elements
PowerPoint to accompany Chapter 6 Periodic Properties of the Elements Development of the Periodic Table Elements in the same group generally have similar chemical properties. Properties are not identical,
The 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
CHEM 103 Spectroscopy and the Quantum Mechanical Model
CHEM 103 Spectroscopy and the Quantum Mechanical Model Lecture Notes April 6, 2006 Prof. Sevian Agenda Emission spectroscopy How the quantum mechanical model explains it Where quantum mechanics breaks
Chemistry 121: Atomic and Molecular Chemistry Topic 3: Atomic Structure and Periodicity
Text Chapter 2, 8 & 9 3.1 Nature of light, elementary spectroscopy. 3.2 The quantum theory and the Bohr atom. 3.3 Quantum mechanics; the orbital concept. 3.4 Electron configurations of atoms 3.5 The periodic
Chapter 4. Periodic Trends of the Elements. Chemistry: Atoms First Second Edition Julia Burdge & Jason Overby
Chemistry: Atoms First Second Edition Julia Burdge & Jason Overby Chapter 4 Periodic Trends of the Elements M. Stacey Thomson Pasco-Hernando State College Copyright (c) The McGraw-Hill Companies, Inc.
Atoms and Periodic Properties
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 01 (Chp 6,7): Atoms and Periodic Properties John D. Bookstaver St. Charles Community College
Electron configurations follow the order of sublevels on the periodic table.
Electron configurations follow the order of sublevels on the periodic table. 1 The periodic table consists of sublevel blocks arranged in order of increasing energy. Groups 1A(1)-2A(2) = s level Groups
Summation of Periodic Trends
Summation of Periodic Trends Factors Affecting Atomic Orbital Energies The Effect of Nuclear Charge (Z effective ) Higher nuclear charge lowers orbital energy (stabilizes the system) by increasing nucleus-electron
Metals and Nonmetals
The Periodic Table and Atomic Properties The periodic table originally came from the observation that when the elements are arranged by atomic mass, properties recur periodically. (Mendeleev) Now we understand
Metals and Nonmetals. Metals and Nonmetals. The Periodic Table and Atomic Properties
The Periodic Table and Atomic Properties The periodic table originally came from the observation that when the elements are arranged by atomic mass, properties recur periodically. (Mendeleev) Now we understand
Additional Problem 1.13
Task 1 Due: 11:59pm on Friday, April 27, 2018 You will receive no credit for items you complete after the assignment is due. Grading Policy Additional Problem 1.13 Classify each of the following as a pure
Unit 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
Organizing 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
Summation of Periodic Trends Factors Affecting Atomic Orbital Energies
Summation of Periodic Trends Factors Affecting Atomic Orbital Energies The Effect of Nuclear Charge (Z effective ) Higher nuclear charge lowers orbital energy (stabilizes the system) by increasing nucleus-electron