This document discusses the molecular structure of atoms. It begins by explaining that all substances are composed of elements, which are the basic substances, and that elements are made up of very small particles called atoms. It then describes the basic structure of an atom, including that atoms have a small, positively charged nucleus surrounded by negatively charged electrons. The number of protons determines the element and equals the number of electrons. Atoms can gain, lose, or share electrons to attain stable electron configurations, forming ions or molecules.
Chemical Structure: Structure of Matter. Atoms – the building blocks of matterulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Chemical Structure: Structure of Matter. Atoms – the building blocks of matterulcerd
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
This slides demonstrate on the formation of positive and negative ions, followed by formation of ionic bonding and covalent bonding. Chemical bonding have various types of bonding. In the presentation, we're sharing only ionic and covalent bonding only.
The compounds which are made up of ions are known as ionic compounds.
In an ionic compound, the positively charged ions and negatively charged ions are held together by the strong electrostatic forces of attraction.
The forces which hold the ions together in an ionic compound are known as ionic bonds and electrovalent bonds.
This slides demonstrate on the formation of positive and negative ions, followed by formation of ionic bonding and covalent bonding. Chemical bonding have various types of bonding. In the presentation, we're sharing only ionic and covalent bonding only.
The compounds which are made up of ions are known as ionic compounds.
In an ionic compound, the positively charged ions and negatively charged ions are held together by the strong electrostatic forces of attraction.
The forces which hold the ions together in an ionic compound are known as ionic bonds and electrovalent bonds.
Contents
The Atom
Materials Used in Electronics
Current in Semiconductors
N-Type and P-Type Semiconductors
The PN Junctions
Diode Operation, Voltage-Current (V-I) Characteristics
Bipolar Junction Transistor (BJT) Structure, Operation, and Characteristics and Parameters
Junction Field Effect Transistors (JFETs) Structure, Characteristics and Parameters and Biasing
Metal Oxide Semiconductor FET (MOSFET) Structure, Characteristics and Parameters and Biasing
The ATOM: Learning Objectives
Describe the structure of an atom
Discuss the Bohr model of an atom
Define electron, proton, neutron, and nucleus
Define atomic number
Discuss electron shells and orbits
Explain energy levels
Define valence electron
Discuss ionization
Define free electron and ion
Discuss the basic concept of the quantum model of the atom
Discuss insulators, conductors, and semiconductors and how they differ
Define the core of an atom
Describe the carbon atom
Name two types each of semiconductors, conductors, and insulators
Explain the band gap
Define valence band and conduction band
Compare a semiconductor atom to a conductor atom
Discuss silicon and germanium atoms
Explain covalent bonds
Define crystal
Describe how current is produced in a semiconductor
Discuss conduction electrons and holes
Explain an electron-hole pair
Discuss recombination
Explain electron and hole current
Describe the properties of n-type and p-type semiconductors
Define doping
Explain how n-type semiconductors are formed
Describe a majority carrier and minority carrier in n-type material
Explain how p-type semiconductors are formed
Describe a majority carrier and minority carrier in p-type material
Describe how a pn junction is formed
Discuss diffusion across a pn junction
Explain the formation of the depletion region
Define barrier potential and discuss its significance
State the values of barrier potential in silicon and germanium
Discuss energy diagrams
Define energy hill
The Fundamentals of Chemistry is an introduction to the Periodic Table, stoichiometry, chemical states, chemical equilibria, acid & base, oxidation & reduction reactions, chemical kinetics, inorganic nomenclature, and chemical bonding.
Slide 1: Title Slide
Extrachromosomal Inheritance
Slide 2: Introduction to Extrachromosomal Inheritance
Definition: Extrachromosomal inheritance refers to the transmission of genetic material that is not found within the nucleus.
Key Components: Involves genes located in mitochondria, chloroplasts, and plasmids.
Slide 3: Mitochondrial Inheritance
Mitochondria: Organelles responsible for energy production.
Mitochondrial DNA (mtDNA): Circular DNA molecule found in mitochondria.
Inheritance Pattern: Maternally inherited, meaning it is passed from mothers to all their offspring.
Diseases: Examples include Leber’s hereditary optic neuropathy (LHON) and mitochondrial myopathy.
Slide 4: Chloroplast Inheritance
Chloroplasts: Organelles responsible for photosynthesis in plants.
Chloroplast DNA (cpDNA): Circular DNA molecule found in chloroplasts.
Inheritance Pattern: Often maternally inherited in most plants, but can vary in some species.
Examples: Variegation in plants, where leaf color patterns are determined by chloroplast DNA.
Slide 5: Plasmid Inheritance
Plasmids: Small, circular DNA molecules found in bacteria and some eukaryotes.
Features: Can carry antibiotic resistance genes and can be transferred between cells through processes like conjugation.
Significance: Important in biotechnology for gene cloning and genetic engineering.
Slide 6: Mechanisms of Extrachromosomal Inheritance
Non-Mendelian Patterns: Do not follow Mendel’s laws of inheritance.
Cytoplasmic Segregation: During cell division, organelles like mitochondria and chloroplasts are randomly distributed to daughter cells.
Heteroplasmy: Presence of more than one type of organellar genome within a cell, leading to variation in expression.
Slide 7: Examples of Extrachromosomal Inheritance
Four O’clock Plant (Mirabilis jalapa): Shows variegated leaves due to different cpDNA in leaf cells.
Petite Mutants in Yeast: Result from mutations in mitochondrial DNA affecting respiration.
Slide 8: Importance of Extrachromosomal Inheritance
Evolution: Provides insight into the evolution of eukaryotic cells.
Medicine: Understanding mitochondrial inheritance helps in diagnosing and treating mitochondrial diseases.
Agriculture: Chloroplast inheritance can be used in plant breeding and genetic modification.
Slide 9: Recent Research and Advances
Gene Editing: Techniques like CRISPR-Cas9 are being used to edit mitochondrial and chloroplast DNA.
Therapies: Development of mitochondrial replacement therapy (MRT) for preventing mitochondrial diseases.
Slide 10: Conclusion
Summary: Extrachromosomal inheritance involves the transmission of genetic material outside the nucleus and plays a crucial role in genetics, medicine, and biotechnology.
Future Directions: Continued research and technological advancements hold promise for new treatments and applications.
Slide 11: Questions and Discussion
Invite Audience: Open the floor for any questions or further discussion on the topic.
This presentation explores a brief idea about the structural and functional attributes of nucleotides, the structure and function of genetic materials along with the impact of UV rays and pH upon them.
Nutraceutical market, scope and growth: Herbal drug technologyLokesh Patil
As consumer awareness of health and wellness rises, the nutraceutical market—which includes goods like functional meals, drinks, and dietary supplements that provide health advantages beyond basic nutrition—is growing significantly. As healthcare expenses rise, the population ages, and people want natural and preventative health solutions more and more, this industry is increasing quickly. Further driving market expansion are product formulation innovations and the use of cutting-edge technology for customized nutrition. With its worldwide reach, the nutraceutical industry is expected to keep growing and provide significant chances for research and investment in a number of categories, including vitamins, minerals, probiotics, and herbal supplements.
What is greenhouse gasses and how many gasses are there to affect the Earth.moosaasad1975
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Observation of Io’s Resurfacing via Plume Deposition Using Ground-based Adapt...Sérgio Sacani
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on Io’s surface have been monitored from both spacecraft and ground-based telescopes.
Here, we present the highest spatial resolution images of Io ever obtained from a groundbased telescope. These images, acquired by the SHARK-VIS instrument on the Large
Binocular Telescope, show evidence of a major resurfacing event on Io’s trailing hemisphere. When compared to the most recent spacecraft images, the SHARK-VIS images
show that a plume deposit from a powerful eruption at Pillan Patera has covered part
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2. Introduction
Every substance in the universe is composed of certain basic substances; we know such basic
substances as elements.
When we crush two substances into fine particles or powdered form and observe it under
magnifying glass than what is visible now are compounds of very minute particles. This very minute
particle is known as an atom. Atoms are so minute that they are not visible even by a microscope.
Group of similar atoms is called an element whose fundamental component is atom.
Fig: 1. Atom
The circular central portion of the atom is known as Nucleus. It is also known as center of the atom.
There are two types of particles namely Proton and Neutron in the center of an atom, which is
called Nucleus.
Surrounding the nucleus there is one more type of particle known as electron which moves a
definite circular path also called Orbit.
Proton Electrically positively charged Positive charge
Electron Electrically negatively charged Negative charge
Neutron Electrically neutral No charge
2
3. Fig: 2. Our Solar System
Atomic Number
3
Compare Fig: 1. and Fig: 2. and think about following:-
•Is there any resemblance between both the figures?
•What is at the center of both the figures?
•What is rotating around the center in both the figures?
What makes the electron rotate around the nucleus in an atom?
Proton and neutron are relatively very heavy particles whereas electrons are very light in their
comparison.
Due to the attraction of the positively charged proton in the nucleus, the negatively charged electrons
rotate around the nucleus in a circular path.
4. In an atom, the number of proton and electron are equal. Since the positive charges and the
negative charges are equal, an atom is neutral with respect to the electrical charge.
The number of proton or electron present in an atom of an element is called “atomic number”.
Therefore;
The Atomic Number of an Element = The Number of Protons Present in it =
The Number of Electrons in it.
Name of the
Element
Symbol Atomic Number Number of
Protons
Number of
Electrons
HYDROGEN H 1 1 1
HELIUM He 2 2 2
LITHIUM Li 3 3 3
BERYLLIUM Be 4 4
BORON B 5 5
CARBON C 6 6
NITROGEN N 7 7
OXYGEN O 8 8
FLUORINE F 9 9
NEON Ne 10
SODIUM Na 11 11
MAGNESIUM Mg 12 12
ALUMINIUM Al 13 13
SILICON Si 14 14
PHOSPHOROUS P 15 15
SULPHUR S 16 16
CHLORINE Cl 17
ARGON Ar 18
POTASSIUM K 19
CALCIUM Ca 20 20 20
4
5. Electronic Configuration
The distribution of electrons among various molecular orbitals is called the electronic configuration
of the molecule.
The closest energy level to the nucleus is called the first energy level.
Beyond the first energy level, gradually the second, third and the fourth energy levels come in that
order.
In the first energy level maximum 2, in the second energy level maximum 8, in the third energy level
maximum 18 and in the fourth energy level maximum 32 electrons can be accommodated.
Electrons fill orbitals in a way to minimize the energy of the atom. Therefore, the electrons in an
atom fill the principal energy levels in order of increasing energy (the electrons are getting farther
from the nucleus). The order of levels filled looks like this:
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, and 7p
One way to remember this pattern, probably the easiest, is to refer to the periodic table and
remember where each orbital block falls to logically deduce this pattern. Another way is to make a
table like the one below and use vertical lines to determine which subshells correspond with each
other.
Name of the Element Symbol Atomic Number Electro
Configuration
HYDROGEN H 1 (1)
5
To know how many electrons can be accommodated in any energy level, the formula 2n2
is very
helpful, where ‘n’ stands for the serial number of the energy level.
6. HELIUM He 2 (2)
LITHIUM Li 3 (2, 1)
BERYLLIUM Be 4 (2, 2)
BORON B 5 (2, 3)
CARBON C 6 (2, 4)
NITROGEN N 7 (2, 5)
OXYGEN O 8 (2, 6)
FLUORINE F 9 (2, 7)
NEON Ne 10 (2, 8)
SODIUM Na 11 (2, 8, 1)
MAGNESIUM Mg 12 (2, 8, 2)
ALUMINIUM Al 13 (2, 8, 3)
SILICON Si 14 (2, 8, 4)
PHOSPHOROUS P 15 (2, 8, 5)
SULPHUR S 16 (2, 8, 6)
CHLORINE Cl 17 (2,8, 7)
ARGON Ar 18 (2, 8, 8)
Do atoms have tendency to gain, lose or share electrons? Let us find the answer:
Till the outer most energy level of the atom of any element is not completely filled
with electrons, the atom is active and has the tendency to combine with another atom.
Let us take some example to understand the above mentioned concept.
Example: 1
The atomic number of Sodium (Na) is 11, and therefore electron configuration is (2, 8, 1). Its outer
most energy level has only one electron and thus to complete the energy level, it has tendency to
lose one electron.
6
7. Due to loss of an electron, the nuclear charge does not remain neutral but it becomes positively
charged. Therefore after losing 1 electron Na becomes positive ion and is written as (Na+
).
Example: 2
The atomic number of Chlorine (Cl) is 17; therefore the electron configuration is (2, 8, 7). Its
outermost energy level has seven electrons and to complete the energy level it has a tendency to
gain 1 electron.
Due to the gain of 1 electron, the nuclear charge does not remain neutral, but it becomes negatively
charged. Therefore, after gaining 1 electron Cl becomes negative ion and is written as (Cl
-
).
Oppositely charged ions like negative or positive charge are attracted towards each other, combine
to make a molecule of sodium chloride (salt).
The elements which have 1, 2 or 3 electrons in the outer most energy level easily lose 1, 2 or 3
electrons and make positive ions having the valence +1, +2 or +3.
Eg: - Na+
, Mg2+
, Al3+
, etc.
The elements which have 7, 6 or 5 electrons in the outer most energy level gain easily 1, 2 or3
electrons and make it negative ions having the valence -1, -2 or -3.
Eg: - Cl
-
, O2-
, etc.
Sometimes there are no possibilities of gaining or losing of electrons thus two atoms share the
electrons present in their outer most energy level and combine with each other to complete their
energy level.
Example: 3
7
8. Hydrogen atoms share one electron each and complete the energy level having 2 electrons and
making one molecule of Hydrogen (H2).
Similarly, Oxygen atoms share two electrons each and complete the energy level having 8 electrons
and making one molecule of Oxygen (O2).
Exercise
Q.1. MCQs
i. Which particles are not in the nucleus?
a) Proton
b) Neutron
c) Electron
d) None of the above
ii. Which particles are moving around the nucleus?
8
9. a) Proton
b) Neutron
c) Electron
d) None of the above
iii. Which particles do not possess any charge?
a) Proton
b) Neutron
c) Electron
d) None of the above
iv. How many maximum electrons can be accommodated in the first
energy level?
a) 2
b) 8
c) 18
d) 32
v. How many maximum electrons can be accommodated in the second
energy level?
e) 2
f) 8
g) 18
h) 32
vi. How many maximum electrons can be accommodated in the third
energy level?
i) 2
j) 8
k) 18
9
10. l) 32
vii. How many maximum electrons can be accommodated in the fourth
energy level?
m) 2
n) 8
o) 18
p) 32
viii. The circular central portion of the atom is known
a) Proton
b) Nucleus
c) Center
d) Neutron
Q.2. Give two points of difference for:
i. Molecule & Atom
ii. Atom & Ion
iii. Electron & Proton
Q.3. Explain:
i. Basic unit for an element is atom, whereas the basic unit for compound
is molecule.
ii. Atom is neutral with respect to the electrical charge.
iii. Atoms have tendency to gain, lose or share electron.
iv. Electron rotating around the nucleus.
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