The document contains sample exam questions from various years on topics related to atomic structure, the periodic table, ionization energies, atomic spectra, bonding, and the historical experiments that led to discoveries about atomic structure. It includes multiple choice and open response questions testing definitions, explanations of trends, interpretations of data, and descriptions of experiments. The questions would require a strong understanding of foundational atomic and molecular concepts as well as the ability to apply this knowledge to analyze new situations.
The document summarizes key information about radioactivity, including the discoveries of Becquerel, Marie Curie, and Pierre Curie in the late 19th century. It describes the three main types of radiation (alpha, beta, gamma) and provides examples of common radionuclides that emit each type, such as americium-241, carbon-14, and cobalt-60. Uses of radioisotopes discussed include carbon-14 dating, cobalt-60 for cancer treatment, and food irradiation. The document also covers half-life, nuclear reactions, and distinguishes between chemical and nuclear processes.
The document provides an overview of oxidation and reduction concepts including:
- Oxidation involves loss of electrons while reduction involves gain of electrons.
- Examples of oxidation and reduction reactions are given for sodium-chlorine, magnesium-oxygen, and zinc-copper sulfate.
- Oxidizing and reducing agents are defined as substances that cause oxidation or reduction in other substances.
- The electrochemical series orders metals by their tendency to be oxidized.
- Electrolysis and examples like copper plating and extracting copper from scrap iron using electrolysis are summarized.
The document summarizes the structure of an atom in 3 paragraphs:
1) It describes the three main subatomic particles - electrons, protons, and neutrons - and their relative masses and charges.
2) It outlines the historical discoveries of these particles, including Thomson discovering electrons in 1900, discoveries of positively charged particles (protons) in the late 1800s, and Chadwick discovering neutrons in 1932.
3) It discusses several historical models of the atom, including Thomson's "plum pudding" model, Rutherford's discovery of the nucleus from alpha scattering experiments, and Bohr's improvement adding discrete electron orbits that explained atomic stability.
The document discusses the periodic table of elements and its development over time. It explains how elements are arranged based on their proton number and how this arrangement allows prediction of element properties based on periodic trends. Examples are given of common elements and their uses to illustrate the practical importance of the periodic table.
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPointMr. Walajtys
This document covers naming and writing formulas for ions, ionic compounds, molecular compounds, acids, and bases. It provides objectives and definitions for each section, examples of naming and writing formulas, and explanations of naming conventions and rules including prefixes, charges, and endings for different types of compounds.
The document discusses the development of atomic theory and models of atomic structure based on experiments. Key points include:
1. Early experiments with cathode ray tubes led Thomson to discover the electron and determine its small mass and negative charge.
2. Rutherford's gold foil experiment showed that the mass and positive charge of atoms are concentrated in a very small, dense nucleus.
3. Later experiments discovered the proton in the nucleus and the neutron, establishing the main subatomic particles that make up all elements.
4. Models evolved from Thomson's "plum pudding" model to Rutherford's nuclear model to better explain experimental results and the stability of atoms.
The document discusses the electron configuration of potassium, which has 19 electrons arranged in shells with the inner shell containing 2 electrons, the next shell containing 8 electrons, the next shell containing 8 electrons, and the outer shell containing the remaining 1 electron. It also discusses periodic trends such as elements in the same group having similar properties and how additional electron shells are added as you move down periods of the periodic table.
Properties of coordination compounds part 3Chris Sonntag
This document discusses the stability of coordination compounds. It covers factors that influence stability such as thermodynamic equilibrium, ligand field stabilization energy, the Jahn-Teller effect, and the HSAB principle of acid-base theory. It also discusses the chelate effect where multidentate ligands form more stable complexes than monodentate ligands. Review questions at the end assess understanding of these concepts and how they relate to predicting magnetic properties and orbital contributions to magnetism in coordination complexes.
Chemical Terminology: Lesson 1 elements and reactionsChris Sonntag
This document discusses inorganic chemistry terminology and reactions. It defines common non-English element names like antimony, tin, and lead. It also covers nomenclature for salts, complexes, and organometallic compounds. Several types of inorganic reactions are described, including Lewis acid-base, redox, photochemical, radical, and diradical reactions. Key reactions like Fenton, Wurtz, Ullmann, Stille, and Grignard reactions are also mentioned. Mechanisms are provided for redox and Grignard reactions.
Muhammad Sufyan from Chenab College Jhang presented on ionization energy. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom to form a cation. Across a period, ionization energy increases as atomic number increases because the nuclear charge is stronger, attracting electrons more tightly. Down a group, ionization energy decreases as atomic size increases with more electron shells, holding electrons more loosely. Factors that influence ionization energy include atomic size, nuclear charge, orbital nature, and shielding effects. Ionization energy can indicate metallic character and help predict elemental valency.
The document provides information on several chemistry concepts and experiments. It includes:
1) A chapter on matter that discusses states of matter, kinetic theory, and heating curves.
2) Chapters on chemical formulas, periodic table, chemical bonds, and electrochemistry.
3) An experiment on determining the end point of a neutralization reaction between potassium hydroxide and hydrochloric acid.
This document discusses oxidation and reduction reactions and provides rules for determining oxidation numbers:
1) Oxidation involves loss of electrons and increases oxidation number, while reduction involves gain of electrons and decreases oxidation number.
2) The sum of oxidation numbers in a molecule or ion must equal the overall charge.
3) Transition metals can have variable oxidation numbers depending on their compounds. Their oxidation states are included in names.
4) Some anomalies may occur where oxidation numbers are fractional or elements appear to gain/lose no electrons.
Seminar form 4= revision on intro to chemistry, structure of atoms, formulae ...MRSMPC
The document contains questions from a chemistry exam covering topics like rates of reaction, empirical formulas, and chemical equations. Question 1 asks students to identify variables in an experiment investigating the effect of temperature on the rate of reaction between sulfuric acid and magnesium. Question 2 involves drawing a graph of temperature over time and determining the melting point of a substance from the graph. Question 3 covers concepts like nucleon number, electron configuration, and isotopes. Question 4 asks students to determine the empirical formula of magnesium oxide from experimental data.
F.sc. Part 1 Chemistry Chapterwise Test Solved by Malik XufyanMalik Xufyan
1. The document discusses test series and publications for chemistry from class 9 to MSc from Maliks Chemistry and Jhang Institute for Advanced Studies.
2. It provides the chapter list and page numbers for the chemistry test series covering topics such as basic concepts, gases, liquids, atomic structure, chemical bonding, and electrochemistry.
3. Contact information is given for Malik Xufyan and Jhang Institute for Advanced Studies for their chemistry publications and test series.
This document outlines the learning outcomes for the topic of periodic table and atomic structure in Leaving Certificate Chemistry in Ireland. It includes 3 sections - the periodic table and atomic structure, atomic structure, and radioactivity. For each section, it lists the key concepts students should understand, such as describing trends in the periodic table, outlining the historical development of atomic theory, and defining and explaining terms like isotopes, ionization energy, and oxidation and reduction reactions. It provides a detailed overview of the essential knowledge students are expected to retain about fundamental chemical concepts relating to the periodic table, atomic structure, and radioactivity.
This document discusses coordination compounds and their properties. It explains that coordination compounds often have distinct colors and can produce different numbers of ions in solution. Werner proposed a theory to represent the structures of coordination compounds using brackets. Coordination compounds have defined geometries depending on the coordination number of the central metal atom. They can also form various isomers based on ligand arrangement or stereochemistry. Common applications of coordination compounds include water softening, metal purification, and medical chelation therapy.
Environmentatl chemistry water (questions and answers)Martin Brown
This document contains exam questions from 2009-2002 on the topics of water treatment, water quality testing, acid-base chemistry, and sewage treatment. It asks students to define concepts like conjugate acid-base pairs, calculate pH values, identify chemicals used in water treatment and their purposes, and describe the multi-stage processes involved in treating water and sewage.
This document outlines the key learning outcomes for two topics in Leaving Certificate Chemistry: 8.1 Chemical Equilibrium and 8.2 Le Chatelier's Principle. For 8.1, students should be able to explain concepts related to reversible reactions and chemical equilibrium, write equilibrium constant expressions, and perform calculations involving equilibrium constants. For 8.2, students should be able to state Le Chatelier's principle and use it to predict how concentration, pressure, temperature, and catalysts affect equilibrium position, as demonstrated through experiments on example chemical mixtures. Industrial applications are also discussed.
5.2 structure of aliphatic hydrocarbonsMartin Brown
This document discusses the structure and properties of aliphatic hydrocarbons. It defines aliphatic hydrocarbons as hydrocarbons containing only carbon and hydrogen atoms arranged in straight or branched chains or rings, excluding benzene rings. The three main types of aliphatic hydrocarbons are alkanes, alkenes, and alkynes. Alkanes have the general formula CnH2n+2 and include methane, ethane, propane, etc. Alkenes have the formula CnH2n and contain carbon-carbon double bonds. Alkynes have the formula CnH2n-2 and contain carbon-carbon triple bonds. Physical properties like state, solubility,
5.4 exothermic and endothermic reactionsMartin Brown
This document discusses exothermic and endothermic reactions. Exothermic reactions release heat, while endothermic reactions absorb heat. Combustion reactions of hydrocarbons like methane and propane are exothermic, producing carbon dioxide, water vapor, and large amounts of heat. The heat of reaction, ΔH, indicates whether a reaction is exothermic (negative ΔH) or endothermic (positive ΔH). Bond energies represent the energy required to break bonds, while heat of combustion measures the heat released from complete combustion. A bomb calorimeter is used to accurately measure heats of combustion by igniting samples in excess oxygen. Hess's law states that the heat change of a reaction depends only on
The document contains exam questions and answers related to hydrocarbons that can be used as fuels. Some key details include:
- Butane is a major component of LPG, which stands for liquefied petroleum gas.
- Methane is a major component of natural gas. Mercaptans are often added to natural gas to give it an odor to detect leaks. Methane's release contributes to the greenhouse effect and global warming.
- The heat of combustion of butane is calculated to be -2881 kJ/mol based on heats of formation of products and reactants.
Benzene is an aromatic hydrocarbon with a planar hexagonal ring structure. Each carbon atom in the ring forms four bonds - one with a hydrogen atom and three sigma bonds with the other carbon atoms in the ring. The sixth valence electron of each carbon is delocalized and shared among all six carbon atoms, giving benzene unusual stability and properties compared to other unsaturated hydrocarbons. Aromatic compounds contain a benzene ring in their structure and include benzene itself along with methylbenzene and ethylbenzene. These aromatic hydrocarbons are liquids that are insoluble in water but soluble in non-polar solvents.
The document discusses hard water and its causes. Hard water is water that does not easily form soap lathers, due to the presence of calcium and magnesium ions that react with soap. There are two types of hardness: temporary hardness caused by calcium and magnesium bicarbonates that can be removed by boiling, and permanent hardness caused by calcium and magnesium chlorides and sulfates that cannot be removed by boiling. Methods for softening hard water include using ion exchange resins that replace calcium and magnesium ions with sodium ions.
9 environmental chemistry water learning outcomesMartin Brown
This document outlines the learning outcomes for the environmental chemistry section of the Leaving Certificate Chemistry curriculum in Ireland. It covers four topics: 1) the pH scale, 2) hardness in water, 3) water treatment, and 4) water analysis. The key points covered include defining pH and calculating pH of solutions, identifying causes of water hardness and methods for removal, describing water treatment processes like sedimentation and chlorination, and outlining instrumental methods for water analysis including pH meters, atomic absorption spectroscopy, and colorimetry.
Crude oil is separated into fractions by fractional distillation based on differences in boiling points. The fractions include refinery gas, light gasoline, naphtha, kerosene, gas oil, and residue. These fractions are used to produce fuels like petrol, diesel, and jet fuel. Petrol is a complex mixture of hydrocarbons, mainly alkanes and aromatics. Its octane rating, which indicates its resistance to premature ignition, can be increased through processes like isomerization, dehydrocyclization, and catalytic cracking that produce more branched and cyclic molecules.
This document summarizes water treatment and sewage treatment processes. It describes how surface water is treated through steps like sedimentation, flocculation, filtration, chlorination and fluoridation to remove contaminants. Sewage treatment involves primary, secondary and sometimes tertiary levels to remove solids, break down organic waste biologically, and remove nutrients like nitrates and phosphates. The document also discusses how excess nutrients can cause eutrophication of waterways and pollution from heavy metals and legislation limits their levels.
Water undergoes self-ionization in which a small percentage of water molecules dissociate into hydronium (H3O+) and hydroxide (OH-) ions. The concentration of these ions is extremely small and the equilibrium lies very much in the forward direction. The self-ionization of water can be represented by the equilibrium constant Kw, which is equal to the product of the hydronium and hydroxide ion concentrations. Kw is temperature dependent and decreases with increasing temperature. The pH scale was developed to quantify the concentration of hydronium ions in solution and thus indicate whether a solution is acidic, basic, or neutral. pH is defined as the negative logarithm of the hydronium ion concentration
Hydrocarbons like crude oil, natural gas, and coal are fossil fuels formed from the remains of ancient marine plants and animals. Methane is a hydrocarbon produced naturally in coal mines, slurry pits, waste dumps, and the digestive tracts of animals, but it poses fire, explosion, and suffocation hazards if it accumulates.
The document discusses the chemical alkynes, specifically ethyne (C2H2). It describes the laboratory preparation of ethyne from calcium dicarbide and water, which produces ethyne gas. Ethyne is colorless, insoluble in water but soluble in nonpolar solvents, and burns with a very hot, smoky flame when combusted. It can be used to cut and weld steel in oxy-acetylene torches. The document also discusses the manufacture and uses of hydrogen, including from natural gas reforming and electrolysis of water, and its use in the Haber process and as a fuel. Fuel cells that use hydrogen are also mentioned.
2.6.2 balancing equation_using_oxidation_numbersMartin Brown
The document provides steps for balancing chemical equations using oxidation numbers:
1. Write out reactants and products and assign oxidation numbers.
2. Identify atoms whose oxidation numbers change during oxidation and reduction reactions.
3. Write the electron transfers involved in oxidation and reduction.
4. Balance the overall electron transfers between reactants and products.
5. Insert the balanced electron transfer numbers into the chemical equation.
6. Balance the overall chemical equation by inspection, balancing hydrogen last.
The document discusses valence shell electron pair repulsion (VSEPR) theory, which predicts the shapes of molecules based on electron pair repulsion. It explains that electron pairs are either bonding pairs involved in bonds or lone pairs not involved in bonds. Lone pairs repel other electron pairs more strongly than bonding pairs do. Example molecules like methane, ammonia, water, boron trifluoride, beryllium chloride, carbon dioxide are presented along with their electron arrangements and predicted molecular shapes like tetrahedral, trigonal pyramidal, bent, linear based on the number of electron pairs and lone pairs.
The document outlines the learning outcomes for the chemical bonding section of the Leaving Certificate Chemistry curriculum in Ireland. It is divided into multiple subsections on topics like ionic bonding, covalent bonding, electronegativity, molecular shapes, and oxidation numbers. For each subsection, it lists the key concepts students should understand by the end of the section and provides boxes to check their level of understanding of each topic.
The document discusses the nature of different types of bonds based on electronegativity differences between atoms. A pure covalent H-H bond is non-polar as electrons are shared equally. A polar covalent H-Cl bond results from the chlorine atom attracting the shared electrons more strongly, giving chlorine a partial negative charge and hydrogen a partial positive charge. Whether a molecule with polar bonds is itself polar depends on the molecular geometry. Water is polar due to its bent, non-linear shape whereas carbon dioxide is non-polar due to its linear shape.
The document discusses covalent bonds. It explains that covalent bonds involve the sharing of electron pairs between atoms. Electrons from each atom are shared in pairs to form single, double or triple bonds. Single bonds are formed by one shared pair, double bonds by two shared pairs, and triple bonds by three shared pairs. Covalent bonds preferentially form between elements in groups IV-VII of the periodic table and are an alternative to ionic bonding between atoms.
The octet rule states that atoms are most stable when their outer electron shells contain 8 electrons. Atoms attain this stable electron configuration by gaining, losing, or sharing electrons with other atoms so that their outer shells match the noble gas configuration. The rule applies mainly to nonmetals like carbon, nitrogen, oxygen, and halogens, and also some metals such as sodium and magnesium.
The document contains sample exam questions from various years on topics related to atomic structure and the periodic table. It includes multiple choice and open response questions testing definitions, concepts, and explanations of trends. The questions cover topics such as ionization energies, atomic spectra, isotopes, atomic structure, bonding and shapes of molecules, and the historical experiments that led to discoveries about atomic models.
This document contains a model question paper for class 10 physical science with 40 total marks. It is divided into 4 sections:
1) Section I contains 4 mark questions with detailed answers required (16 marks total). Example questions include chemical reactions of calcium oxide and hydrochloric acid, and the use of detergents.
2) Section II contains short answer questions worth 4 marks total.
3) Section III contains very short answer questions worth 6 marks total.
4) Section IV contains multiple choice questions worth 6 marks total. The final section provides a blueprint of the question distribution.
The document is an answer key for an inorganic chemistry and organic chemistry exam containing multiple choice and descriptive questions.
Some of the questions addressed in the summary include drawing orbital diagrams, electronic configurations of atoms, types of chemical bonds, and properties of ionic compounds.
The descriptive questions require explanations about anomalous electronic configurations, molecular geometry, decomposition of carbonates, quantum numbers, and dual nature of matter.
CBSE10th Science Sample Question Paper 2019Miso Study
Misostudy offers you free CBSE10th Science Sample Question Paper 2019, These papers having most important questions that are specially designed for CBSE class 10 aspirants on the basis of latest exam pattern. Every question is solved by our expert faculty in this field.
This document summarizes key points from a YouTube chemistry lecture on periodic properties. It discusses trends in properties like metallic character, atomic size, ionization energy and electron affinity across periods and down groups in the periodic table. Multiple choice questions are included about these trends, such as increasing ionization energy and decreasing atomic size from left to right in a period. Elements in period 3 and their electronic configurations are discussed. The number of elements in each period is stated. The document emphasizes that the periodic properties of elements are determined by their atomic number.
This document contains review questions and problems about atomic structure and the periodic table. It defines key terms like atoms, elements, isotopes, atomic number and mass number. It also describes the experimental evidence that led scientists like Thomson, Rutherford, and Chadwick to discover the internal structure of atoms, including a tiny, dense nucleus. Questions calculate quantities like the number of atoms needed to span a distance or the number of neutrons in different isotopes.
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Attacking the TEKS: Focus on Atomic Theory presented by Jane Smith, ACT2 2010
This session will expose you to the new TEKS and College Readiness Standards. Ideas for sequencing and planning the unit will be shared along with tips for appropriate demos, labs, and assessments. The intended audience is for teachers with 3 or less years of experience or anyone who wants to delve deeper into the new standards.
NCERT solutions for class 10 science chapter 5 (Periodic Classification of El...DebarajBag
Answer: The first ten elements in modern periodic table are hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and ...for more reading click here,https://bidyashramodia.blogspot.com/2022/06/ncert-solutions-for-class-10-science_24.html
Properties of coordination compounds part 1 (2018)Chris Sonntag
1. The document discusses properties of coordination compounds including electronic spectra, hydration energies, lattice energies, and ionic radii as determined by crystal field theory.
2. Crystal field theory can be used to determine the splitting of d-orbital energies under the influence of ligands in an octahedral or tetrahedral field and explain observations from electronic spectra.
3. Hydration energies and lattice energies of metal ions can also be explained using crystal field theory calculations and comparisons to experimental data.
4. Crystal field theory further explains trends in ionic radii and the structures of spinel compounds containing mixed metal oxides.
This document contains a question bank with multiple choice and short answer questions about chemical bonding. Some key topics covered include ionic and covalent bonding, oxidation-reduction reactions, electronegativity, and the structures of ions and molecules. Students are asked to define terms, identify examples, describe electron configurations and bonding patterns, and explain differences in properties between ionic and covalent compounds. Diagrams illustrate atomic structures and bonding arrangements. The question bank is intended to test students' understanding of fundamental concepts in chemical bonding.
This document provides details about the chapter structure of the atom in a 10th standard chemistry textbook. It lists 100 multiple choice questions from the chapter, ranging from 1 to 4 marks. It covers topics like atomic theory, subatomic particles, cathode rays, atomic models (Thomson, Rutherford, Bohr), quantum numbers, electron configuration and orbitals. The chapter aims to teach students about the internal structure of atoms through experiments and quantum mechanical models.
This chemistry jeopardy game document contains questions and answers about various topics in chemistry including the parts of an atom, elements vs compounds vs mixtures, atomic models including Thomson's plum pudding model and Rutherford's nuclear model, electron configurations, quantum mechanics, isotopes, and more. The document is formatted as a game with questions worth different point values and includes diagrams to illustrate concepts.
The document contains summaries of several diagrams showing different scientific processes and experiments. It provides answers to questions about the diagrams, identifying variables, materials, observations, and conclusions. The key information summarized is that the document contains expert summaries and explanations of multiple scientific diagrams and experiments.
Ch 31 Nuclear Physics and RadioactivityScott Thomas
This document provides an overview of key concepts in nuclear physics and radioactivity covered in Chapter 31, including:
1) Nuclear reactions such as conservation of mass number and charge in nuclear reactions. Mass-energy equivalence and how it relates to energy released in nuclear processes.
2) Properties of the nucleus including isotopes, mass number, and atomic number. The strong nuclear force that binds nucleons together.
3) Radioactive decay processes including alpha, beta, gamma decay and particle emissions. Applications of radioactivity such as smoke detectors and radiation therapy.
4) Additional topics covered are nuclear structure, binding energy, the mass defect, radioactive dating, and the neutrino. Learning objectives provide details on understanding these
The document provides a lesson plan on chemistry topics including:
1. Diagnostic questions, answering techniques, and the particulate nature of matter will be covered.
2. Answering techniques include short answers, active sentences, keywords, and relating topics like acids/bases.
3. The particulate nature of matter is explained using kinetic particle theory including the properties of solids, liquids, and gases. Particle movement and intermolecular forces are related to physical properties.
The document provides a summary of key concepts in solid state and solutions:
1) It defines terms like coordination number, doping, paramagnetic substances, voids in crystal lattices, piezoelectricity, packing efficiency, and F-centers.
2) It discusses properties of unit cells including the number of lattice points in a bcc unit cell and formulas for compounds based on unit cell arrangements.
3) It covers concepts in solutions like molarity, Henry's law, ideal and non-ideal solutions, colligative properties, isotonic solutions, and Van't Hoff factor.
This document provides an overview of basic chemistry concepts including:
- The law of multiple proportions and how it is illustrated by nitrogen and hydrogen oxides.
- Definitions of a mole and how it is used to calculate the number of hydrogen atoms in 1 mole of methane.
- How stoichiometry is used to calculate the amount of water formed from the combustion of a given amount of methane.
- The concept of a limiting reagent and how to calculate the mass of a product given specific amounts of reactants.
- A summary of the key observations and conclusions from Rutherford's gold foil experiment that led to the nuclear model of the atom.
The document contains a chemistry unit on the solid state with questions ranging from one to three marks. It includes questions about crystal lattices, crystal defects, stoichiometric and non-stoichiometric defects, crystal structures, and properties of solids such as ionic bonding and conductivity. Numerical problems calculate properties like density from information about the unit cell structure and composition.
The document discusses the structure of atoms and the discovery of subatomic particles. It explains that:
1) Early experiments showed atoms were divisible and contained electrons and protons.
2) Rutherford's gold foil experiment showed atoms had a small, dense nucleus containing most of the mass.
3) Models were developed to explain the atom's structure, including Thomson's "plum pudding" model and Rutherford's nuclear model.
4) Later, the Bohr model incorporated allowed electron orbits, and neutrons were discovered in atomic nuclei.
This document appears to be a collection of poems submitted for a national poetry competition. It includes 21 poems written by students on various topics. The document provides brief biographies of the students who wrote the poems and acknowledges the work of the teachers and organizers in making the competition a success. It celebrates the talents and efforts of the young writers who participated.
This document appears to be a collection of poems submitted for a national poetry competition. It includes 21 poems written by students on various topics. The document provides brief biographies of the students who wrote the poems and acknowledges the work of the teachers and organizers in making the competition a success. It celebrates the talent and effort shown by the young writers.
Evaluating websites using hoax sites activity 2Martin Brown
Students are divided into groups and each group is assigned a hoax website to evaluate for trustworthiness using a website evaluation worksheet. The hoax websites assigned include sites about explorers, dihydrogen monoxide, tree octopuses, aluminum foil hats, jackalopes, dehydrated water, and a dog island. The goal is to teach students how to evaluate websites for accuracy and reliability.
The campus map shows 6 labeled locations - A, B, C, D, E, F, and G. It includes the gym, chapel, residences, and dining room. The map provides a layout of the buildings and facilities at St Patrick's College.
This document provides instructions for evaluating a website by having students visit a specified website and answering 10 questions about the URL, domain extension, author, contact details, purpose, creation/update dates, internal links, information sources, contradicting information from other sources, advertising, and reasons to trust/not trust the information on the site.
This document provides guidelines for setting up a school library or reading corner, including recommendations for location, shelving, furniture, equipment, signage, managing the library collection, and cataloguing systems. The ideal location is at the heart of the school, is highly visible and accessible, and is well-lit with power and internet. Shelving options include wall-mounted and freestanding units of various types. Furniture should be durable and allow for both formal and informal seating. Collections should be tailored to student interests and abilities. Small libraries can use simple tracking systems while larger ones may implement software-based cataloguing of fiction and non-fiction sections.
Jcsp library project Reading promotion - 10 great opening linesMartin Brown
This document contains 10 opening lines from famous young adult books. The lines provide snippets of intrigue from stories about unexpected visitors in the night, dogs that learn to talk, a boy who disappeared on his birthday, life as a hobbit, violence and death, the afterlife, and soldiers kicking down a door in the night.
Jcsp library project Reading promotion - 10 great halloween reads - posterMartin Brown
The document lists 10 book titles for a Halloween Reads project celebrating its 10th anniversary. The books include titles such as Zom-B, The Restless Dead, The Evil Eye, The Walking Dead, Breathe, Changeling, Trick or Treat, The Night Bus, The Undead, and Thing (the play). The list provides book titles, authors, and publishers for a junior certificate school literacy demonstration library project.
The document discusses the JCSP Library Project, which aims to establish libraries in schools serving students at risk of early school leaving. It established demonstration libraries in 30 schools across Ireland staffed by librarians. The libraries aim to improve literacy, develop a reading culture, and enhance student learning experiences. The document provides guidance on setting up an effective school library, including locating it centrally, curating an appropriate collection, promoting reading, and developing furniture and spaces to support independent and collaborative work.
The document is a notification from the State Examinations Commission to post-primary school authorities regarding the Irish oral examination for the 2014 Leaving Certificate. It states that enclosed is the set of 20 picture sequences that will be used for the Irish oral exam at Higher and Ordinary level. It specifies that these pictures will not be used for the Foundation level oral exam.
Beyond the Advance Presentation for By the Book 9John Rodzvilla
In June 2020, L.L. McKinney, a Black author of young adult novels, began the #publishingpaidme hashtag to create a discussion on how the publishing industry treats Black authors: “what they’re paid. What the marketing is. How the books are treated. How one Black book not reaching its parameters casts a shadow on all Black books and all Black authors, and that’s not the same for our white counterparts.” (Grady 2020) McKinney’s call resulted in an online discussion across 65,000 tweets between authors of all races and the creation of a Google spreadsheet that collected information on over 2,000 titles.
While the conversation was originally meant to discuss the ethical value of book publishing, it became an economic assessment by authors of how publishers treated authors of color and women authors without a full analysis of the data collected. This paper would present the data collected from relevant tweets and the Google database to show not only the range of advances among participating authors split out by their race, gender, sexual orientation and the genre of their work, but also the publishers’ treatment of their titles in terms of deal announcements and pre-pub attention in industry publications. The paper is based on a multi-year project of cleaning and evaluating the collected data to assess what it reveals about the habits and strategies of American publishers in acquiring and promoting titles from a diverse group of authors across the literary, non-fiction, children’s, mystery, romance, and SFF genres.
How to Store Data on the Odoo 17 WebsiteCeline George
Here we are going to discuss how to store data in Odoo 17 Website.
It includes defining a model with few fields in it. Add demo data into the model using data directory. Also using a controller, pass the values into the template while rendering it and display the values in the website.
(T.L.E.) Agriculture: Essentials of GardeningMJDuyan
(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏.𝟎)-𝐅𝐢𝐧𝐚𝐥𝐬
Lesson Outcome:
-Students will understand the basics of gardening, including the importance of soil, water, and sunlight for plant growth. They will learn to identify and use essential gardening tools, plant seeds, and seedlings properly, and manage common garden pests using eco-friendly methods.
Integrated Marketing Communications (IMC)- Concept, Features, Elements, Role of advertising in IMC
Advertising: Concept, Features, Evolution of Advertising, Active Participants, Benefits of advertising to Business firms and consumers.
Classification of advertising: Geographic, Media, Target audience and Functions.
Delegation Inheritance in Odoo 17 and Its Use CasesCeline George
There are 3 types of inheritance in odoo Classical, Extension, and Delegation. Delegation inheritance is used to sink other models to our custom model. And there is no change in the views. This slide will discuss delegation inheritance and its use cases in odoo 17.
Understanding and Interpreting Teachers’ TPACK for Teaching Multimodalities i...Neny Isharyanti
Presented as a plenary session in iTELL 2024 in Salatiga on 4 July 2024.
The plenary focuses on understanding and intepreting relevant TPACK competence for teachers to be adept in teaching multimodality in the digital age. It juxtaposes the results of research on multimodality with its contextual implementation in the teaching of English subject in the Indonesian Emancipated Curriculum.
How to Add Colour Kanban Records in Odoo 17 NotebookCeline George
In Odoo 17, you can enhance the visual appearance of your Kanban view by adding color-coded records using the Notebook feature. This allows you to categorize and distinguish between different types of records based on specific criteria. By adding colors, you can quickly identify and prioritize tasks or items, improving organization and efficiency within your workflow.
How to Install Theme in the Odoo 17 ERPCeline George
With Odoo, we can select from a wide selection of attractive themes. Many excellent ones are free to use, while some require payment. Putting an Odoo theme in the Odoo module directory on our server, downloading the theme, and then installing it is a simple process.
The Jewish Trinity : Sabbath,Shekinah and Sanctuary 4.pdfJackieSparrow3
we may assume that God created the cosmos to be his great temple, in which he rested after his creative work. Nevertheless, his special revelatory presence did not fill the entire earth yet, since it was his intention that his human vice-regent, whom he installed in the garden sanctuary, would extend worldwide the boundaries of that sanctuary and of God’s presence. Adam, of course, disobeyed this mandate, so that humanity no longer enjoyed God’s presence in the little localized garden. Consequently, the entire earth became infected with sin and idolatry in a way it had not been previously before the fall, while yet in its still imperfect newly created state. Therefore, the various expressions about God being unable to inhabit earthly structures are best understood, at least in part, by realizing that the old order and sanctuary have been tainted with sin and must be cleansed and recreated before God’s Shekinah presence, formerly limited to heaven and the holy of holies, can dwell universally throughout creation
The Jewish Trinity : Sabbath,Shekinah and Sanctuary 4.pdf
Sections 1 an 2 exam questions
1. Sections 1 & 2
Atomic Structure – Periodic Table
2002
Question 5
(a) Define first ionisation energy.
(8)
(b) Account fully for the trends in first ionisation energies of elements across the second period of the
periodic table (i.e. Li to Ne).
(15)
(c) Account for the trend in first ionisation energies of the elements going down Group II of the
periodic table, i.e. the alkaline-earth metals.
(6)
The approximate values for the first eight ionisation energies of magnesium are given in the following
table.
(d) Explain why there is an increase in these ionisation energy values.
(9)
(e) Account for the dramatic increase in ionisation energy going from the second to the third
ionisation. Between which two ionisations would you expect the next dramatic increase to occur if the
data for further ionisation energies of magnesium were examined? Give a reason for your answer.(12)
2002
Question10. (b)
(i) What is the colour of the light associated with the line emission spectrum of sodium?
(4)
(ii) Explain how line emission spectra occur.
12)
(iii) What evidence do line emission spectra provide for the existence of energy levels in atoms? (6)
(iv) Why is it possible for line emission spectra to be used to distinguish between different elements?
(3)
2002 Question 11. (b)
What are alpha-particles (α-particles)?
(7)
Describe the experiment carried out by Rutherford and his co-workers that led to the discovery of the
nucleus. Explain how Rutherford interpreted the results of this experiment to conclude that the atom
has a nucleus.
(18)
2003
Question 5.
(a) Define (i) energy level
(ii) atomic orbital.
(8)
(iii) Write the electronic configuration (s, p, etc.) of nitrogen.
(iv) Describe how the electrons are arranged in the orbitals of the highest occupied sublevel of a nitrogen atom in its ground state.
(6)
(b) Define electronegativity.
(6)
(i) Describe using dot and cross diagrams the bonding in the water molecule.
(9)
(ii) What is the shape of the water molecule? Which of the following angles, 104°, 107°, 109°, 120°
or 180° would you expect to be closest to the bond angle in the water molecule? Explain your answer.
(12)
(c) The diagram on the right shows a thin stream of water flowing from a burette. What would you
observe if a charged rod was brought close to the thin stream of water? Explain your answer.
(9)
2. 2003 Question 10.(c)
A student was given samples of the following salts:
sodium sulfate (Na2SO4)
sodium sulfite (Na2SO3)
potassium sulfate (K2SO4)
(i) What test could be carried out to distinguish between the sodium salts and the potassium salt? (4)
What observation would you make in this test?
(6)
(ii) Describe the test which could be carried out to distinguish between the sulfate salts and the sulfite
salt.
(15)
2003 Question 11. (b)
The diagram shows a sketch of the trend in the first ionisation energies
for the elements 3 to 10 in the periodic table.
(i) Account for the general increase in ionisation energies across these
elements.
(7)
(ii) Explain why the ionisation energies of element number 4 and 7 are
exceptionally high relative to the general trend.
(12)
(iii) How does the definition of second ionisation energy differ from that
of first ionisation energy?
(6)
2004 Question 5
(a) Write the electron configuration (s, p, etc.) of the nitrogen atom.
(5)
Show, using dot and cross diagrams, the bond formation in a nitrogen molecule.
Describe the bonding in the nitrogen molecule in terms of sigma (σ) and pi (π) bonding.
(9)
What type of intermolecular forces would you expect to find in nitrogen gas? Explain your answer.(6)
(b) Define first ionisation energy.
(9)
There is a general increase in first ionisation energy across a period of
the periodic table. State the two principal reasons for this trend. (6)
The table shows the first and second ionisation energies of nitrogen,
oxygen, neon and sodium. Account for the decrease in first ionisation
energy between nitrogen and oxygen.
Explain why the second ionisation energy of sodium is significantly
(about nine times) higher than the first while the increase in the
second ionisation energy of neon compared to its first is relatively
small (less than twice the first).
(15)
2004
Question 10. (b)
Describe how Bohr used line emission spectra to explain the existence of energy levels in atoms. (13)
(i) Why does each element have a unique line emission spectrum?
(6)
(ii) The fact that each element has a unique line spectrum forms the basis for an instrumental
technique which can be used to detect heavy metals and to measure their concentrations in a soil or a
water sample. Name the instrumental technique.
(3)
(iii) Bohr’s atomic theory was later modified. Give one reason why this theory was updated.
(3)
2004 Question 11. (a)
Define radioactivity.
(i) State two properties of beta (β) particles.
(ii) Write an equation for the nuclear reaction involved in the beta decay of 14C (carbon-14).
(iii) Explain how the carbon-14 isotope allows certain archaeological discoveries to be dated.
6)
(6)
(6)
(7)
3. 2005 Question 10
(b) The minimum energy required to completely remove the most loosely bound electron from a mole
of gaseous atoms in their ground state defines an important property of every element.
(i) Identify the energy quantity defined above. State the unit used to measure this quantity.
(7)
(ii) Using X to represent an element, express the definition above in the form of a balanced chemical
equation.
(6)
(iii) Would it take more or less energy to remove the most loosely bound electron from an atom if that
electron were not in its ground state? Explain.
(6)
(iv) An element has a low first ionisation energy value and a low electronegativity value. What does
this information tell you about how reactive the element is likely to be, and what is likely to happen to
the atoms of the element when they react?
(6)
2005
Question 5.
(a) What are isotopes?
(5)
Name the scientist pictured on the right who is credited with the discovery in 1896
that uranium salts emit radiation.
(3)
Give an example of a radioactive isotope and state one common use made of this
isotope. (9)
(b) Define atomic radius (covalent radius).
(6)
Describe and account for the trend in atomic radii (covalent radii) of the elements
(i) across the second period, (ii) down any group, of the periodic table.
(15)
(c) Define covalent bond. (6) Distinguish between a sigma () and a pi () covalent
bond.
(6)
2006
Question 5.
5. (a) (i) Describe how you would carry out a flame test on a sample of potassium chloride.
(8)
(ii) Why do different elements have unique atomic spectra?
(6)
(iii) What instrumental technique is based on the fact that each element has unique atomic spectra? (3)
Bohr’s model of the atom explained the existence of energy levels on the basis of atomic spectra.
Bohr’s theory was later modified to incorporate the idea of orbitals in recognition of the wave nature
of the electron and Heisenberg’s uncertainty principle.
(iv) Define atomic orbital.
(6)
(v) What does Heisenberg’s uncertainty principle say about an electron in an atom?
(6)
(b) (i) Define electronegativity.
(6)
(ii) Explain why there is a general increase in electronegativity values across the periods in the
periodic table of the elements.
(6)
(iii) Explain, in terms of the structures of the atoms, the trend in reactivity down Group I (the alkali
metal group) of the periodic table.
(9)
2006
Question10 (a).
(i) What are isotopes?
(4)
(ii) Define relative atomic mass, Ar.
(6)
(iii) What is the principle on which the mass spectrometer is based?
(9)
(iv) Calculate the relative atomic mass of a sample of lithium, given that a mass spectrometer shows
that it consists of 7.4 % of 6Li and 92.6 % of 7Li.
(6)
4. 2007
Question 5.
(a) Define energy level.
(5)
Write the electron configuration (s, p) for the sulfur atom in its ground state, showing the arrangement
in atomic orbitals of the highest energy electrons.
(6)
State how many (i) energy levels, (ii) orbitals, are occupied in a sulfur atom in its ground state.
(6)
(b) Use electronegativity values (Mathematical Tables p 46) to predict the type of bond expected
between hydrogen and sulfur. Write the chemical formula for hydrogen sulfide. Use clear dot and
cross diagrams to show the bonding in hydrogen sulfide.
(15)
Would you expect the hydrogen sulfide molecule to be linear or non-linear in shape? Justify your
answer.
(6)
(c) Hydrogen sulfide has a boiling point of 212.3 K and water has a boiling point of 373 K. Account
for the difference in the boiling points of these substances.
(6)
Would you expect hydrogen sulfide to be soluble in water? Explain your answer.
(6)
2007 Question 11. (a)
In 1910 Rutherford (pictured right) and his co-workers carried out an experiment in
which thin sheets of gold foil were bombarded with alpha particles. The observations
made during the experiment led to the discovery of the atomic nucleus.
(i) Describe the model of atomic structure which existed immediately prior to this
experiment.
(7)
(ii) In this experiment it was observed that most of the alpha particles went straight
through the gold foil. Two other observations were made. State these other observations
and explain how each helped Rutherford deduce that the atom has a nucleus.
(12)
In November 2006 former Soviet agent, Alexander Litvinenko, died in London.
The cause of his death was identified as radiation poisoning by polonium-210.
(iii) Polonium-210 decays emitting an alpha particle.
Copy and complete the equation for the alpha-decay of polonium-210, filling in the values of x
(atomic number), y (mass number) and Z (elemental symbol).
(6)
2008 Question 5
(a) Define electronegativity
(5)
(b) State and explain the trend in electronegativity values down the first group in the periodic
table of the elements.
(9)
(c) Use electronegativity values to predict the types of bonding (i) in water, (ii) in methane,
(iii) in magnesium chloride.
(9)
(d) Use dot and cross diagrams to show the formation of bonds in magnesium chloride. (6)
(e) Explain the term intermolecular forces.
(6)
(f) Use your knowledge of intermolecular forces to explain why methane has a very low
boiling point (b.p. = –164 ºC).
The relative molecular mass of methane is only slightly lower than that of water but the boiling
point of water is much higher (b.p. = 100 ºC). Suggest a reason for this.
(6)
(g) The diagram shows a thin stream of liquid flowing from a burette.
A stream of water is deflected towards a positively charged rod whereas a stream of
cyclohexane is undeflected. Account for these observations.
Explain what would happen in the case of the stream of water if the positively charged rod were
replaced by a negatively charged rod.
(9)
5. 2008 Question 10
(a)
(i) Define energy level.
(4)
(ii) Distinguish between ground state and excited state for the electron
in a hydrogen atom.
(6)
The diagram shows how Bohr related the lines in the hydrogen emission
spectrum to the existence of atomic energy levels.
(iii) Name the series of lines in the visible part of the line emission
spectrum of hydrogen.
(3)
(iv) Explain how the expression E2 – E1 = hf links the occurrence of the
visible lines in the hydrogen spectrum to energy levels in a hydrogen atom.
(12)
2009
Question 5
5. (a) Define first ionisation energy of an element.
(8)
(b) Use the values on page 45 of the Mathematics Tables to plot a graph on graph paper of first
ionisation energy versus atomic number for the elements with atomic numbers from 10 to 20
inclusive.
(12)
(c) Account fully for
(i) the general increase in ionisation energy values across the third period of the Periodic Table,
(ii) the peaks which occur in your graph at elements 12 and 15,
(iii) the sharp decrease in ionisation energy value between elements 18 and 19.
(18)
(d) Write the s, p electron configuration for the potassium atom.
Hence state how many (i) energy sub-levels, (ii) individual orbitals, are occupied by electrons in a
potassium atom.
Explain why there are electrons in the fourth main energy level of potassium although the third main
energy level is incomplete.
(12)
2009
Question 11. (c)
In 1922, Francis Aston, pictured right, was awarded the Nobel Prize in chemistry for detecting
the existence of isotopes using the first mass spectrometer.
(i) What are isotopes?
(7)
(ii) What is the principle of the mass spectrometer?
(9)
(iii) Calculate, to two decimal places, the relative atomic mass of a sample of neon shown
by mass spectrometer to be composed of 90.50% of neon–20 and 9.50% of neon–22. (9)