periodic table assignment 1

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High school chemistry

Course: high school chemistry   >   unit 1, the periodic table.

• Apply: the periodic table
• Determine valence electrons using the periodic table
• Apply: number of valence electrons
• Lewis diagrams for atoms and ions
• Apply: Lewis diagrams of atoms
• Apply: Lewis diagrams of ions

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Video transcript

Browse Course Material

Course info.

• Prof. Donald Sadoway

Departments

• Materials Science and Engineering

As Taught In

• Chemical Engineering

Learning Resource Types

Introduction to solid state chemistry, 2. the periodic table.

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Session Overview

Prerequisites

Before starting this session, you should be familiar with:

• Session 1: Introduction to Solid State Chemistry

Looking Ahead

Prof. Sadoway describes Rutherford’s model of the atom and Bohr’s model of hydrogen ( Session 3 ).

Learning Objectives

After completing this session, you should be able to:

• Explain the structure and layout of the periodic table of elements .
• Understand the structure of chemical formulas .
• Apply the concepts of stoichiometry to balance a chemical equation .
• Understand the relationship between frequency , wavelength and energy for photons.
• Identify the superheavy elements .
• Describe the structure of the atom and the properties of the electron , proton and neutron .
• Define an isotope and understand the naming convention for isotopes.
• Calculate the number of electrons in an ion .
• Define ionization energy .

Lecture Video

• Download video
• Download transcript

Lecture Slides (PDF - 6.0MB)

Periodic Table and Table of Constants

Lecture Summary

This lecture continues the discussion about origins of the periodic table, picking up with Dmitri Mendeleev’s discovery of periodic patterns among different groups of elements. At the high end of the periodic table are the superheavy elements; Prof. Sadoway discusses naming conventions and how these elements are discovered.

Elements are characterized by a range of properties. Starting with the fundamental structure of the atom and characteristics of the electron , proton , and neutron , Prof. Sadoway defines key terms such as:

• atomic mass, proton number, neutron number, and isotopes
• ion, cation, and anion
• mole, Avogadro’s number, Faraday’s constant, elementary charge, and atomic mass unit

The lecture includes a description of Robert Millikan’s oil drop experiment (1909), which measured the value of the elementary charge .

A chemical reaction can be described by an equation based on conservation of mass and Dalton’s law of molar proportions. Using the example of the Kroll process for producing titanium metal, Prof. Sadoway demonstrates how to write a balanced equation , employing stoichiometry to determine how much metal is produced from a given amount of reactants.

The lecture ends with a brief biographical sketch of composer and chemistry professor Alexander Borodin , a contemporary of Mendeleev.

Problems (PDF)

Solutions (PDF)

Textbook Problems

For Further Study

Supplemental readings.

Emsley, J. The Elements . New York, NY: Oxford University Press, 1998. ISBN: 9780198558187.

Weeks, M. E. Discovery of the Elements . Madison, WI: Journal of Chemical Education, 1968.

Seaborg, Glenn T., and E.G. Valens. Elements of the Universe . New York, NY: E.P. Dutton & Co., 1958. ISBN: 9789999238939.

Strathern, P. Mendeleyev’s Dream: The Quest for the Elements . New York, NY: St. Martin’s Press, 2001. ISBN: 9780140284140.

Gordin, M. A Well-Ordered Thing: Dmitrii Mendeleev and the Shadow of the Periodic Table . New York, NY: 2004. ISBN: 9780465027750.

Mendeleyev, Dmitri. The Principles of Chemistry . New York, NY: Longmans Green and Co., 1897.

Dalton, John. A New System of Chemical Philosophy . New York, NY: Philosophical Library, 1964.

Cardwell, D. John Dalton and the Progress of Science . New York, NY: Barnes and Noble, 1968.

Kargon, Robert H. The Rise of Robert Millikan: Portrait of a Life in American Science . New York, NY: Cornell University Press, 1982. ISBN: 9780801414596.

Millikan, Robert A. Electrons, Protons, Photons, Neutrons, Mesotrons, and Cosmic Rays . Chicago, IL: University of Chicago Press, 1947.

How Atoms Work

How the Periodic Table Works

John Dalton

Jöns Berzelius

Amedeo Avogadro

Michael Faraday

Robert Millikan - 1923 Nobel Prize in Physics

Dmitri Mendeleev

Alexander Borodin

Charles-Augustin de Coulomb

William Thomson, Lord Kelvin

Borodin, Alexander P. “Polovtsian Dances.” Prince Igor . Available as Ballet Music from Operas . Performed by New York Philharmonic, conducted by Leonard Bernstein. New York, NY: Sony, 1993.

Lehrer, T. The Remains of Tom Lehrer . Los Angeles, CA: Warner Archives/Rhino, 2000.

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• The first periodic table
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• Significance of atomic numbers
• Elucidation of the periodic law
• Classification of elements into groups
• Periodic trends in properties
• Electronic structure
• Periodicity of properties of the elements
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What is the periodic table?

Where does the periodic table come from, why does the periodic table split.

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• How is the atomic number of an atom defined?

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• UEN Digital Press with Pressbooks - Introductory Chemistry - The Periodic Table
• Chemistry LibreTexts - The Periodic Table
• Ohio State University - Origins - Mendeleev's Periodic Table
• National Center for Biotechnology Information - PubChem - Periodic Table of Elements
• NeoK12 - Educational Videos and Games for School Kids - Periodic Table
• LiveScience - Periodic Table of the Elements
• Khan Academy - The periodic table, electron shells, and orbitals
• Western Oregon University - A brief history of the development of Periodic Table
• Royal Society of Chemistry - Patterns in the Periodic Table
• periodic table - Children's Encyclopedia (Ages 8-11)
• periodic table - Student Encyclopedia (Ages 11 and up)
• Table Of Contents

The periodic table is a tabular array of the chemical elements organized by atomic number , from the element with the lowest atomic number, hydrogen , to the element with the highest atomic number, oganesson . The atomic number of an element is the number of protons in the nucleus of an atom of that element. Hydrogen has 1 proton, and oganesson has 118.

What do periodic table groups have in common?

The groups of the periodic table are displayed as vertical columns numbered from 1 to 18. The elements in a group have very similar chemical properties, which arise from the number of valence electrons present—that is, the number of electrons in the outermost shell of an atom .

The arrangement of the elements in the periodic table comes from the electronic configuration of the elements. Because of the Pauli exclusion principle , no more than two electrons can fill the same orbital. The first row of the periodic table consists of just two elements, hydrogen and helium . As atoms have more electrons, they have more orbits available to fill, and thus the rows contain more elements farther down in the table.

The periodic table has two rows at the bottom that are usually split out from the main body of the table. These rows contain elements in the lanthanoid and actinoid series, usually from 57 to 71 ( lanthanum to lutetium ) and 89 to 103 ( actinium to lawrencium ), respectively. There is no scientific reason for this. It is merely done to make the table more compact.

periodic table , in chemistry , the organized array of all the chemical elements in order of increasing atomic number —i.e., the total number of protons in the atomic nucleus. When the chemical elements are thus arranged, there is a recurring pattern called the “periodic law” in their properties, in which elements in the same column (group) have similar properties. The initial discovery, which was made by Dmitry I. Mendeleev in the mid-19th century, has been of inestimable value in the development of chemistry .

It was not actually recognized until the second decade of the 20th century that the order of elements in the periodic system is that of their atomic numbers, the integers of which are equal to the positive electrical charges of the atomic nuclei expressed in electronic units. In subsequent years great progress was made in explaining the periodic law in terms of the electronic structure of atoms and molecules. This clarification has increased the value of the law, which is used as much today as it was at the beginning of the 20th century, when it expressed the only known relationship among the elements.

History of the periodic law

The early years of the 19th century witnessed a rapid development in analytical chemistry—the art of distinguishing different chemical substances—and the consequent building up of a vast body of knowledge of the chemical and physical properties of both elements and compounds . This rapid expansion of chemical knowledge soon necessitated classification , for on the classification of chemical knowledge are based not only the systematized literature of chemistry but also the laboratory arts by which chemistry is passed on as a living science from one generation of chemists to another. Relationships were discerned more readily among the compounds than among the elements; it thus occurred that the classification of elements lagged many years behind that of compounds. In fact, no general agreement had been reached among chemists as to the classification of elements for nearly half a century after the systems of classification of compounds had become established in general use.

J.W. Döbereiner in 1817 showed that the combining weight, meaning atomic weight , of strontium lies midway between those of calcium and barium , and some years later he showed that other such “ triads ” exist (chlorine, bromine , and iodine [halogens] and lithium , sodium , and potassium [alkali metals]). J.-B.-A. Dumas, L. Gmelin, E. Lenssen, Max von Pettenkofer, and J.P. Cooke expanded Döbereiner’s suggestions between 1827 and 1858 by showing that similar relationships extended further than the triads of elements, fluorine being added to the halogens and magnesium to the alkaline-earth metals, while oxygen , sulfur , selenium , and tellurium were classed as one family and nitrogen , phosphorus , arsenic , antimony , and bismuth as another family of elements.

Attempts were later made to show that the atomic weights of the elements could be expressed by an arithmetic function , and in 1862 A.-E.-B. de Chancourtois proposed a classification of the elements based on the new values of atomic weights given by Stanislao Cannizzaro’s system of 1858. De Chancourtois plotted the atomic weights on the surface of a cylinder with a circumference of 16 units, corresponding to the approximate atomic weight of oxygen. The resulting helical curve brought closely related elements onto corresponding points above or below one another on the cylinder, and he suggested in consequence that “the properties of the elements are the properties of numbers,” a remarkable prediction in the light of modern knowledge.

Classification of the elements

In 1864, J.A.R. Newlands proposed classifying the elements in the order of increasing atomic weights, the elements being assigned ordinal numbers from unity upward and divided into seven groups having properties closely related to the first seven of the elements then known: hydrogen , lithium, beryllium , boron , carbon , nitrogen, and oxygen. This relationship was termed the law of octaves, by analogy with the seven intervals of the musical scale.

Then in 1869, as a result of an extensive correlation of the properties and the atomic weights of the elements, with special attention to valency (that is, the number of single bonds the element can form), Mendeleev proposed the periodic law, by which “the elements arranged according to the magnitude of atomic weights show a periodic change of properties.” Lothar Meyer had independently reached a similar conclusion, published after the appearance of Mendeleev’s paper.

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1-7 The Periodic Table of Elements

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BELL RINGER 1-7c Bell Ringer SE - Periodic Table (Doc) 1-7c Bell Ringer SE - Periodic Table (PDF) 1-7c Bell Ringer TE - Periodic Table (Doc) 1-7c Bell Ringer TE - Periodic Table (PDF) DOODLE NOTES 1-7c Doodle Notes - Periodic Table (Doc) 1-7c Doodle Notes - Periodic Table (PDF) EXIT QUIZ 1-7c Exit Quiz SE - Periodic Table (Doc) 1-7c Exit Quiz SE - Periodic Table (PDF) 1-7c Exit Quiz TE - Periodic Table (Doc) 1-7c Exit Quiz TE - Periodic Table (PDF) HOMEWORK ASSIGNMENT 1-7c Homework SE - Periodic Table (Doc) 1-7c Homework SE - Periodic Table (PDF) 1-7c Homework TE - Periodic Table (Doc) 1-7c Homework TE - Periodic Table (PDF) LESSON PLAN 1-7c Lesson Plan - Periodic Table (Doc) 1-7c Lesson Plan - Periodic Table (PDF)

BELL RINGER 1-7d Bell Ringer SE - Periodic Table (Doc) 1-7d Bell Ringer SE - Periodic Table (PDF) 1-7d Bell Ringer TE - Periodic Table (Doc) 1-7d Bell Ringer TE - Periodic Table (PDF) EXIT QUIZ 1-7d Exit Quiz SE - Periodic Table (Doc) 1-7d Exit Quiz SE - Periodic Table (PDF) 1-7d Exit Quiz TE - Periodic Table (Doc) 1-7d Exit Quiz TE - Periodic Table (PDF) HOMEWORK ASSIGNMENT 1-7d Homework SE - Periodic Table (Doc) 1-7d Homework SE - Periodic Table (PDF) 1-7d Homework TE - Periodic Table (Doc) 1-7d Homework TE - Periodic Table (PDF) LESSON PLAN 1-7d Lesson Plan - Periodic Table (Doc) 1-7c Lesson Plan - Periodic Table (PDF) DOODLE NOTES 1-7d Vocabulary Doodle Notes SE - Periodic Table (Doc) 1-7d Vocabulary Doodle Notes SE - Periodic Table (PDF)

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Electronic Structure and Periodic Properties of Elements

Assignment—atomic structure and the periodic table.

To download a copy of the assignment, please click on the link Sample Questions .

As you work these matter and measurement problems, consider and explain:

• What type of question is it?
• How do you know what type of question it is?
• What information are you looking for?
• What information do they give?
• How will you go about solving this?
• Show how to solve the problem.
• Be able to answer for a different reaction, number, set of conditions, etc.

Sample Questions

• Which form of electromagnetic radiation has the longest wavelengths?
• A line in the spectrum of atomic mercury has a wavelength of 254 nm. When mercury emits a photon of light at this wavelength, what is the frequency of the light?
• Consider an atom traveling at 1% of the speed of light. The de Broglie wavelength is found to be 1.46 × 10 –3 pm. Which element is this?
• What is the energy of a photon of blue light that has a wavelength of 453 nm?
• The hydrogen molecules they came from have the formula H 4 .
• We could observe more lines if we had a stronger prism.
• There are four electrons in an excited hydrogen atom.
• Only certain energies are allowed for the electron in a hydrogen atom.

• n = 4 to n = 3
• n = 4 to n = 2
• n = 4 to n = 1
• n = 3 to n = 2
• n = 2 to n = 1
• In the hydrogen spectrum, what is the wavelength of light associated with the n = 3 to n = 1 electron transition?
• Energy is emitted.
• Energy is absorbed.
• The electron loses energy.
• The electron gains energy.
• The electron cannot make this transition.
• It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus.
• It does not adequately predict the line spectrum of hydrogen.
• It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.
• It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen.
• It shows the electrons to exist outside of the nucleus.
• The energy of the light emitted when a hydrogen electron goes from n = 2 to n = 1 is what fraction of its ground-state ionization energy?
• The emission spectrum of hydrogen contains a continuum of colors.
• Diffraction produces both constructive and destructive interference.
• All matter displays both particle and wavelike characteristics.
• Niels Bohr developed a quantum model for the hydrogen atom.
• The lowest possible energy state of a molecule or atom is called its ground state.
• A gamma ray of wavelength 1.00 × 10 –8 cm has enough energy to remove an electron from a hydrogen atom.
• space where electrons are unlikely to be found in an atom
• space which may contain electrons, protons, and/or neutrons
• the space in an atom where an electron is most likely to be found
• small, walled spheres that contain electrons
• a single space within an atom that contains all electrons of that atom
• How many f orbitals have the value n = 3?
• If n = 2, how many orbitals are possible?

• The electrons move along the outer surface of the p -orbital, similar to a “figure 8” type of movement.
• The electrons move within the two lobes of the p -orbital, but never beyond the outside surface of the orbital.
• The electrons are concentrated at the center (node) of the two lobes.
• The electrons are only moving in one lobe at any given time.
• The electron movement cannot be exactly determined.
• How many electrons in an atom can have the quantum numbers n = 3, l = 2?
• How many electrons can be contained in all of the orbitals with n = 4?
• n = 1, l = 1, m l = 0, m s = 1/2
• n = 3, l = 0, m l = 0, m s = -1/2
• n = 2, l = 1, m l = -1, m s = 1/2
• n = 4, l = 3, m l = -2, m s = -1/2
• n = 4, l = 2, m l = 0, m s = 1/2
• What is the electron configuration for the barium atom?
• What is the complete electron configuration of tin?
• The exact location of an electron can be determined if we know its energy.
• An electron in a 2 s orbital can have the same n , l , and ml quantum numbers as an electron in a 3 s orbital.
• Ni has two unpaired electrons in its 3 d orbitals.
• In the buildup of atoms, electrons occupy the 4 f orbitals before the 6 s orbitals.
• Only three quantum numbers are needed to uniquely describe an electron.
• What is the statement that “the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals” known as?
• An element with the electron configuration [Xe] 6 s 2 4 f 14 5 d 7 would belong to which class on the periodic table?
• Ti has __________ in its d orbitals.
• radio waves
• 1.18 × 10 15 s -1
• 4.39 × 10<sup-19 J
• 1.03 × 10 -7 m
• 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 2
• Hund’s rule
• transition elements
• two electrons
• Authored by : Jessica Garber. Provided by : Tidewater Community College. License : CC BY: Attribution