This document outlines the learning outcomes for topics covered in the Leaving Certificate Chemistry curriculum in Ireland. It includes learning outcomes for several topics: the periodic table and atomic structure, atomic structure, radioactivity, electronic structure of atoms, and oxidation and reduction. For each topic, it lists the key concepts students should understand and be able to do, such as describe trends in the periodic table, outline the historical development of atomic theory, and define oxidation and reduction in terms of electron transfer.
Woodward Feiser Rules -Calculation of absorbtion maximum for conjugated dienes and trienes - for unsaturated carbonyl compounds - benzene and its derivatives
Woodward Feiser Rules -Calculation of absorbtion maximum for conjugated dienes and trienes - for unsaturated carbonyl compounds - benzene and its derivatives
Inorganic chemistry Unit-19 Metal Cluster.pdfkoreanhitz70
It's the best notes on the metal cluster of the subject inorganic chemistry. It presents knowledge on borane, diborane, carboranes, their reactions, introduction and classes.
Importance of amines, classification of amines, Preparation of amines, Physical properties, Chemical properties, Basic nature, tests of amines, Carbylamine test, Hinsberg's test, reactions with nitrous acid, electrophilic reactions, -NH2 group protection, Diazonium salts, Uses, Some important conversions, short questions with answers.
Inorganic chemistry Unit-19 Metal Cluster.pdfkoreanhitz70
It's the best notes on the metal cluster of the subject inorganic chemistry. It presents knowledge on borane, diborane, carboranes, their reactions, introduction and classes.
Importance of amines, classification of amines, Preparation of amines, Physical properties, Chemical properties, Basic nature, tests of amines, Carbylamine test, Hinsberg's test, reactions with nitrous acid, electrophilic reactions, -NH2 group protection, Diazonium salts, Uses, Some important conversions, short questions with answers.
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.
ELEMENTARY PARTICLES OF MATTER
Matter is made up of discrete particles, the main ones are:-
1. Atoms 2. Ions 3. Molecules - (AIM)
DEFINITION OF ATOMS
An atom is the smallest particle of an element which can take part in a chemical reaction
THE CONSTITUENTS OF ATOMS
Rutherford in 1911 threw more light on the nature of the atom. He demonstrated that atom is made up of sub-particles which are called:
1. Proton 2. Neutron 3. Electron.
He discovered that the protons and neutrons are concentrated in the nucleus of an atom, while the electrons are revolving round the nucleus.
J.J THOMPSON’S MODEL
J.J Thompson described the atom as being made up of a mixture of positive (Protons) and negative (Electrons) charges.
LORD RUTHERFORD’S MODEL
Lord Rutherford described the atom as being made up of Positive (Protons) and Neutral (Neutrons) charges in its centre (nucleus) while the negative charges (electrons) rotates around its orbit.
He used the planetary bodies rotating around the sun to describe the structure of atoms.
CHARACTERISTICS OF PROTON, ELECTRON AND NEUTRON
DALTON’S ATOMIC THEORY
In 1808, John Dalton proposed the Atomic Theory which can be summarised as follows:
All elements are made up of small, indivisible particles called atoms.
Atoms can neither be created nor destroyed.
Atoms of the same elements are alike in every aspect, and differ from atoms of all other elements.
When atoms combine with other atoms, they do so in simple ratios.
All chemical changes result from the combination or the separation of atoms.
The Atomic Theory was partially supported by experimental evidences deduced from the Law of Conservation of Mass, the Law of Definite Proportions, the Law of Multiple Proportions and so on. It could not explain electrolysis and certain other phenomena. As a result of new discoveries, Dalton’s original Atomic Theory has undergone several modifications but the principal aspects as outlined above are still useful in the study of chemistry.
MODIFICATIONS OF DALTON’S ATOMIC THEORY
All Elements Are Made Up Of Small Indivisible Particles Called Atoms: This statement has been proven wrong by Rutherford’s discovery – the atom is built up of three main types of sub-particles: the proton, the electron, the neutron. It is not an indivisible solid piece.
The Atom Can Neither Be Created Nor Destroyed: This statement still holds good for ordinary chemical reactions and is embodied in the basic Law of Conservation of Mass. During a nuclear reaction, such as the fission of Uranium – 235, the nucleus is broken up into smaller units which form simpler atoms while a tremendous amount of heat energy is released. These changes that occur during nuclear fission destroy the atoms of the element involved.
The Atoms Of The Same Elements Are Alike In Every Aspect And Differ From Atoms Of All Other Elements: The discovery of isotopes makes this statement unacceptable. Chlorine, for example has two different atom
This presentation will help anyone studying C1 in science. For further help, tips and advice please don`t hesitate to email me at cpugh5345@yahoo.co.uk
Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
The Roman Empire A Historical Colossus.pdfkaushalkr1407
The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
Ethnobotany and Ethnopharmacology:
Ethnobotany in herbal drug evaluation,
Impact of Ethnobotany in traditional medicine,
New development in herbals,
Bio-prospecting tools for drug discovery,
Role of Ethnopharmacology in drug evaluation,
Reverse Pharmacology.
Instructions for Submissions thorugh G- Classroom.pptxJheel Barad
This presentation provides a briefing on how to upload submissions and documents in Google Classroom. It was prepared as part of an orientation for new Sainik School in-service teacher trainees. As a training officer, my goal is to ensure that you are comfortable and proficient with this essential tool for managing assignments and fostering student engagement.
Students, digital devices and success - Andreas Schleicher - 27 May 2024..pptxEduSkills OECD
Andreas Schleicher presents at the OECD webinar ‘Digital devices in schools: detrimental distraction or secret to success?’ on 27 May 2024. The presentation was based on findings from PISA 2022 results and the webinar helped launch the PISA in Focus ‘Managing screen time: How to protect and equip students against distraction’ https://www.oecd-ilibrary.org/education/managing-screen-time_7c225af4-en and the OECD Education Policy Perspective ‘Students, digital devices and success’ can be found here - https://oe.cd/il/5yV
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
In this webinar you will learn how your organization can access TechSoup's wide variety of product discount and donation programs. From hardware to software, we'll give you a tour of the tools available to help your nonprofit with productivity, collaboration, financial management, donor tracking, security, and more.
Palestine last event orientationfvgnh .pptxRaedMohamed3
An EFL lesson about the current events in Palestine. It is intended to be for intermediate students who wish to increase their listening skills through a short lesson in power point.
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
For more information, visit-www.vavaclasses.com
This is a presentation by Dada Robert in a Your Skill Boost masterclass organised by the Excellence Foundation for South Sudan (EFSS) on Saturday, the 25th and Sunday, the 26th of May 2024.
He discussed the concept of quality improvement, emphasizing its applicability to various aspects of life, including personal, project, and program improvements. He defined quality as doing the right thing at the right time in the right way to achieve the best possible results and discussed the concept of the "gap" between what we know and what we do, and how this gap represents the areas we need to improve. He explained the scientific approach to quality improvement, which involves systematic performance analysis, testing and learning, and implementing change ideas. He also highlighted the importance of client focus and a team approach to quality improvement.
1 periodic table and atomic structure learning outcomes
1. Learning Outcomes Leaving Certificate Chemistry
1 Periodic table and atomic structure
Each topic has a set of boxes which the pupil can tick to show how well
they understanding or how well they know the topic. This is useful for
revision. Bold text indicates Higher Level.
1.1 The periodic table of elements. (3 class periods)
By the end of this section pupils should be able to
Good
Fair
Poor
Good
Fair
Poor
describe the periodic table as a list of elements arranged so as to
demonstrate trends in their physical and chemical properties
define the term element
associate the first 36 elements with their elemental symbols
distinguish between elements and compounds
state the principle resemblances of elements within each main group, in
particular alkali metals, alkaline earth metals, halogens and noble gases
describe the reaction between water and lithium, sodium and potassium
having seen the reaction demonstrated
describe by means of a chemical equation the reaction between water
and lithium, sodium and potassium having seen the reaction
demonstrated
outline the history of the idea of elements, including the contributions of
the Greeks, Boyle, Davy and Moseley
outline the contributions of Mendeleev, Dobereiner, Newlands and
Moseley to the structure of the modern periodic table
compare mendeleev’s periodic table with the modern periodic table
arrange elements in order of relative atromic mass and note differences
with modern periodic table
1.2 Atomic Structure (6 class periods)
By the end of this section pupils should be able
outline the historical development of atomic theory (outline principles only,
mathematical treatment not required):
Dalton: atomic theory;
Crookes: vacuum tubes, cathode rays;
Stoney: naming of the electron;
Thomson: negative charge of the electron; e/m for electrons
(experimental details not required);
Millikan: magnitude of charge of electrons as shown by oil drop
experiment (experimental details not required);
2. Learning Outcomes Leaving Certificate Chemistry
Rutherford: discovery of the nucleus as shown by the particle scattering
experiment; discovery of protons in nuclei of various atoms;
Bohr: model of the atom;
Chadwick: discovery of the neutron.
recall that matter is composed of particles, which may be atoms,
molecules or ions
define an atom
appreciate that atoms are minute particles
state the law of conservation of mass
describe, relative mass, relative charge and location of a proton, neutron,
and electron in an atom
define atomic number (Z) mass number(A)
define relative atomic mass (Ar) using the C12 scale
define isotope
describe the composition of isotopes using hydrogen and carbon as
examples
describe how a mass spectrometer can be used to determine relative
atomic mass
describe the principles on which the Mass Spectrometer is based
explain the fundamental processes that occur in a mass
spectrometer
calculate the approximate relative atomic masses from abundance of
isotopes of given mass number
1.3 Radioactivity (2 class periods)
By the end of this section pupils should be able
define radioactivity
describe the nature and penetrating ability of alpha, beta and gamma
radiation
give one example each of the following: an α emitter, a β emitter and a γemitter
explain how radiation is detected having seen a demonstration / video (
principles of a geiger muller tube not required)
define radioisotopes
define and explain half life (non-mathematical treatment)
Good
Fair
Poor
3. Learning Outcomes Leaving Certificate Chemistry
give a historical outline of:
Becquerel’s discovery of radiation from uranium salts
Marie and Pierre Curie’s discovery of polonium and radium
comment on the widespread occurrence of radioactivity
distinguish between a chemical reaction and a nuclear reaction
(simple equations required, confine to α and β emissions)
state three uses of radioactivity, including food irradiation and the use of
60
Co for cancer treatment
explain how 14C is used for age determination (calculations not required)
1.4 Electronic Structure of Atoms (11 class periods)
By the end of this section pupils should be able
define and explain energy levels in atoms
describe the organization of particles in atoms of elements numbers 1-20
classify the first twenty elements in the periodic table on the basis of the
number of outer electrons
list the numbers of electrons in each main energy level in atoms of
elements nos. 1–20
describe and explain the emission spectrum of the hydrogen atom
using the Balmer series in the emission spectrum as an example
describe and explain the absorption spectrum
use flame tests to provide evidence that energy is absorbed or released in
discrete units when electrons move from one energy level to another
explain how flame tests provide evidence that energy is absorbed or
released in discrete units when electrons move from one energy
level to another
relate energy levels in atoms to everyday applications such as sodium
street lights and fireworks
discuss the uses of atomic absorption spectrometry (AAS) as an
analytical technique
illustrate how line spectra provide evidence for energy levels
use a spectroscope or a spectrometer to view emission spectra of
elements
define and explain energy sub-levels
state the Heisenberg uncertainty principle
state the dual wave-particle nature of the electron (mathematical
treatment not required)
Good
Fair
Poor
4. Learning Outcomes Leaving Certificate Chemistry
define and explain atomic orbitals
describe the shapes of s and p orbitals
build up the electronic structure of the first 36 elements
derive the electronic configurations of ions of s- and p block
elements only
describe the arrangement of electrons in individual orbitals of pblock atoms
define and explain atomic radius
explain the general trends in values of atomic radii (covalent radii only)
down a group
across a period (main group elements only)
define and explain first ionisation energy
explain the general trends in first ionisation energy values:
down a group
across a period (main group elements) and
explain the exceptions to the general trends across a period
define and explain second and successive ionisation energies
describe how second and successive ionisation energies provide
evidence for energy levels
recognise the relationship and trends in successive ionisation
energies of an individual element
explain how chemical properties of elements depend on their electronic
structure
explain how atomic radius, screening effect and nuclear charge account
for general trends in properties of elements in groups I and VII
1.5 Oxidation and Reduction (7 class periods)
By the end of this section pupils should be able
define oxidation and reduction in terms of electron transfer
use simple examples , e.g. Na with Cl2, Mg with O2, Zn with Cu2+ to
describe oxidation and reduction in terms of electron transfer
apply knowledge of oxidation and reduction to explain the rusting of iron
define oxidising agent and reducing agent
arrange the electrochemical series of metals in order of their ease of
oxidation (reactions, other than displacement reactions, not required)
Good
Fair
Poor
5. Learning Outcomes Leaving Certificate Chemistry
carry out an experiment to show that halogens act as oxidising
agents(reactions with bromides, iodides, Fe2+ and sulfites; half equations
only required)
carry out an experiment to demonstrate the displacement reactions of
metals (Zn with Cu2+, Mg with Cu2+)
explain what happens at each electrode during the electrolysis of:
copper sulfate solution with copper electrodes
acidified water with inert electrodes
(half equations only required)
describe and account for the observations of what happens at each
electrode during the electrolysis of (teacher demo)
aqueous sodium sulfate (using universal indicator)
aqueous potassium iodide (using phenolphthalein indicator)
with inert electrodes (half equations only required)
describe the extraction of copper by displacements using scrap iron
describe and explain ionic movement as observed during teacher
demonstration
describe the following electrolytic processes: purification of copper,
chrome and nickel plating. Give one everyday application of chrome and
nickel plating e.g. cutlery