The document discusses oxidation states and redox reactions. It defines oxidation as the loss of electrons or gain of electronegative elements, and reduction as the gain of electrons or loss of electronegative elements. Redox reactions involve the transfer of electrons from the reduced species to the oxidized species. Rules for determining oxidation states are outlined, such as atoms in their elemental state having an oxidation state of 0, and the sum of oxidation states in a neutral molecule or polyatomic ion equaling the overall charge. Examples of oxidation and reduction reactions are provided.
This chapter tell you about the reduction in the Oxidation reaction there he is revolutions their transfer of ions and also about the oxidizing agent in the reducing agent
This chapter tell you about the reduction in the Oxidation reaction there he is revolutions their transfer of ions and also about the oxidizing agent in the reducing agent
Unit 8 - Information and Communication Technology (Paper I).pdfThiyagu K
This slides describes the basic concepts of ICT, basics of Email, Emerging Technology and Digital Initiatives in Education. This presentations aligns with the UGC Paper I syllabus.
Biological screening of herbal drugs: Introduction and Need for
Phyto-Pharmacological Screening, New Strategies for evaluating
Natural Products, In vitro evaluation techniques for Antioxidants, Antimicrobial and Anticancer drugs. In vivo evaluation techniques
for Anti-inflammatory, Antiulcer, Anticancer, Wound healing, Antidiabetic, Hepatoprotective, Cardio protective, Diuretics and
Antifertility, Toxicity studies as per OECD guidelines
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
2024.06.01 Introducing a competency framework for languag learning materials ...Sandy Millin
http://sandymillin.wordpress.com/iateflwebinar2024
Published classroom materials form the basis of syllabuses, drive teacher professional development, and have a potentially huge influence on learners, teachers and education systems. All teachers also create their own materials, whether a few sentences on a blackboard, a highly-structured fully-realised online course, or anything in between. Despite this, the knowledge and skills needed to create effective language learning materials are rarely part of teacher training, and are mostly learnt by trial and error.
Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
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.
Acetabularia Information For Class 9 .docxvaibhavrinwa19
Acetabularia acetabulum is a single-celled green alga that in its vegetative state is morphologically differentiated into a basal rhizoid and an axially elongated stalk, which bears whorls of branching hairs. The single diploid nucleus resides in the rhizoid.
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.
6. For Example :
(i)
(ii)
(iii)
(iv)
C + O2
2Mg+O2
Zn + S
Mg + Cl2
-------------> CO2
-------------> 2MgO
-------------> ZnS
-------------> MgCl2
}Addition of oxygen
}Addition of electronegative element
Lecture- 1
REDOX REACTIONS-CLASSICAL IDEA
OXIDATION:
The addition of oxygen or any other electronegative element or removal of
hydrogen or any other electropositive element.
7. For Example :
(i)
(ii)
(iii)
(iv)
C + O2
2Mg+O2
Zn + S
Mg + Cl2
-------------> CO2
-------------> 2MgO
-------------> ZnS
-------------> MgCl2
}Addition of oxygen
}Addition of electronegative element
Lecture- 1
REDOX REACTIONS-CLASSICAL IDEA
OXIDATION:
The addition of oxygen or any other electronegative element or removal of
hydrogen or any other electropositive element.
8. Lecture- 1
(i) Cl2 + H2
(ii) Br2 + H2S
------------->
------------->
2HCl
2HBr + S
(iii)
(iv)
2FeCl3 + Fe
2HgCl2 + SnCl2
------------->
------------->
2FeCl2
Hg2Cl2 + SnCl4
}Addition of hydrogen
}Addition of electropositive element
Reduction
The addition of hydrogen or any other electropositive element or removal of
oxygen or any other electronegative element.
For example, the reduction reactions are :
9. Lecture- 1
Oxidizing Agent or Oxidant
A substance which gives oxygen or removes hydrogen is called an
oxidizing agent or oxidant.
10. Lecture- 1
A substance which provides hydrogen or removes oxygen is called a
reducing agent or reductant.
ReducingAgent
13. Lecture- 1
Na+ + e–
Mg2+ + 2e–
Sn4+ + 2e–
Na
Mg
Sn2+
Fe2+
--------------->
--------------->
--------------->
---------------> Fe3+ + e–
(ii) Loss of electrons resulting in decrease of negative charge.
MnO
[Fe(CN)6]4–
--------------->
--------------->
MnO + e–
[Fe(CN)6]3– + e–
Electronic Concept
Oxidation is a process which involves loss of electrons by an atom or group
of atoms.
For example,
(i) Loss of electrons resulting in increase in positive charge.
14. Lecture- 1
--------------->
--------------->
--------------->
Fe2+
Sn2+
Sb3+
(iii) Gain of electrons resulting in increase of negative charge.
Cl 2e–
S + 2e–
---------------> 2Cl–
---------------> S2–
Electronic Concept
Reduction : A process which involves gain of electrons by an atom or group
of atoms.
(i) Gain of electrons resulting in decrease of positive charge.
Fe3+ + e–
Sn4+ + 2e–
Sb5+ + 2e–
15. Lecture- 1
Lets Understand !!
OXIDATION-REDUCTION REACTIONS AS ELECTRONS TRANSFER
REACTIONS
Oxidation takes place at the cost of reduction and vice versa.
17. Lecture- 1
Lets Understand !!
OXIDATION NUMBER
The charge which an atom of the element has in its ion or appears to have
when present in the combined state with other atoms.
Oxidation numbers are also called oxidation states.
Oxidation number also gives the charge which an atom appears to have
when all other atoms are removed from it as ions.
18. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
1. The oxidation number of an element in the free or elementary state or in
any of its allotropic forms is always zero.
19. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
1. The oxidation number of an element in the free or elementary state or in
any of its allotropic forms is always zero.
20. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
2. The oxidation number of an element in a single (monoatomic) ion is the
same as the charge on the ion.
21. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
2. The oxidation number of an element in a single (monoatomic) ion is the
same as the charge on the ion.
22. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
3. In compounds formed by the combination of non-metallic atoms, the atom
with higher electronegativity is given negative oxidation number.
23. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
4. In all compounds of hydrogen, the oxidation number of hydrogen is +1
except in hydrides of active metals such as LiH, NaH, KH, MgH2, CaH2,
etc., where hydrogen has the oxidation number of –1.
24. Lecture- 1
7.
8. The second exception is found in compounds in which oxygen is bonded to
fluorine.
Rules for the Determination of Oxidation Number of an Atom
5. The oxidation number of oxygen is –2 in most of the compounds.
6. However, there are two exceptions. The first exception is peroxides and
superoxides
25. Lecture- 1
Rules for the Determination of Oxidation Number of an Atom
7. The most electronegative element, fluorine has oxidation number –1. For
other halogens, the oxidation number is generally – 1, but there are
exceptions when these are bonded to a more electronegative halogen atom
or oxygen.
26. Lecture- 1
For a polyatomic ion, the sum of the oxidation numbers of all the atoms is
equal to charge on the ion.
Rules for the Determination of Oxidation Number of an Atom
8. For neutral molecule, the sum of the oxidation numbers of all the atoms is
equal to zero.
27. Lecture- 1
For a polyatomic ion, the sum of the oxidation numbers of all the atoms is
equal to charge on the ion.
Rules for the Determination of Oxidation Number of an Atom
8. For neutral molecule, the sum of the oxidation numbers of all the atoms is
equal to zero.
28. Lecture- 1
Oxidation Number of
Free elements
Fluorine
Simple ions
Oxygen
F2O (+ 2); F2O2 (+ 1)
Hydrogen = + 1;
metal hydrides (–1)
Sum of O.N. of atoms in molecules = 0
Sum of O.N. of atoms in polyatomic ions = (Charge on them).
Watch out !!
= 0
= –1
= Charge on them
= OXIDES (–2);
peroxides (–1);
