This document provides an overview of bonding basics, including ionic and covalent bonds. Ionic bonds form when a metal transfers electrons to a nonmetal, resulting in oppositely charged ions that attract. Covalent bonds form when atoms share electrons to achieve a full outer shell. Examples show Lewis diagrams and representing the transfer or sharing of electrons to form ionic compounds like KI or covalent molecules like H2O.
This lesson talks about another gas law, the Charles' Law. This is a simplify lesson for intended for the level of my students understanding. Hope it helps you too!
This lesson talks about another gas law, the Charles' Law. This is a simplify lesson for intended for the level of my students understanding. Hope it helps you too!
There are several misconceptions about the valence shell of the atom. The key questions that arise in the minds of the learners are:
Is valence shell really the outermost shell?
2. Are there only seven shells in an atom?
3. When shells are supposed to be made up of subshells, why can we not represent the subshells in the valence shell structure of the atom?
4. When electrons are said to occur in orbitals, why can we not indicate the orbitals in the valence shell structure?
4. How can we represent the origins for valance band and conduction band in the atomic structure?
5. What are some good metaphors for the core of the atom and the rest of the atom?
Here is a lesson created by Chemistry teachers to address these misconceptions.
Bonding and structure - ionic compounds, covalent compounds and metals. Relationship between intermolecular forces and physical properties. Allotropes.
We will be going over information for Exam 2. Talking a lot about naming of compounds and learning electron domain geometries with molecular geometries.
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.
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
Model Attribute Check Company Auto PropertyCeline George
In Odoo, the multi-company feature allows you to manage multiple companies within a single Odoo database instance. Each company can have its own configurations while still sharing common resources such as products, customers, and suppliers.
A Strategic Approach: GenAI in EducationPeter Windle
Artificial Intelligence (AI) technologies such as Generative AI, Image Generators and Large Language Models have had a dramatic impact on teaching, learning and assessment over the past 18 months. The most immediate threat AI posed was to Academic Integrity with Higher Education Institutes (HEIs) focusing their efforts on combating the use of GenAI in assessment. Guidelines were developed for staff and students, policies put in place too. Innovative educators have forged paths in the use of Generative AI for teaching, learning and assessments leading to pockets of transformation springing up across HEIs, often with little or no top-down guidance, support or direction.
This Gasta posits a strategic approach to integrating AI into HEIs to prepare staff, students and the curriculum for an evolving world and workplace. We will highlight the advantages of working with these technologies beyond the realm of teaching, learning and assessment by considering prompt engineering skills, industry impact, curriculum changes, and the need for staff upskilling. In contrast, not engaging strategically with Generative AI poses risks, including falling behind peers, missed opportunities and failing to ensure our graduates remain employable. The rapid evolution of AI technologies necessitates a proactive and strategic approach if we are to remain relevant.
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.
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.
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
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.
2. Before you can figure out how atoms form
molecules and compounds, you need some
information. You need to be able to figure out all
this from the periodic table.
Total # of # of Valence # of Electrons Oxidation
Element Atomic Symbol
Electrons1 Electrons2 gained or lost3 Number4
Iodine I 53 17 gain 1 -1
Lithium Li 3 1 lose 1 +1
Calcium Ca 20 2 lose 2 +2
Sulfur S 16 6 gain 2 -2
Boron B 5 3 lose 3 +3
Silicon Si 14 4 gain/lose 4 + 4 or - 4
Phosphorus P 15 5 gain 3 -3
1. Total number of electrons equals the atomic number.
2. The number of valence electrons is the same as the column number on the periodic table
3. Less that 4 valence electrons, electrons are lost. More than 4 valence electrons, electrons are gained. Atoms with 4 (carbon, silicon) can gain or lose.
4. Atoms lose electrons to become positive ions. Atoms gain electrons to become negative ions.
3. Ionic Bonds
• Form when one atom loses electrons and
one atom gains electrons.
• Always form between a metal and a
nonmetal. (never between two nonmetals)
• The oxidation numbers must add up to
zero.
4. Example 1.
Potassium + Iodine
First, write the Lewis Diagram for each element.
K I
5. Example 1.
Potassium + Iodine
Next, draw an arrow showing the transfer of electrons
from one atom to the other.
K I
6. Example 1.
Potassium + Iodine
Now, show the charges on the newly formed ions.
Potassium lost an electron to become +1, and Iodine gained
an electron to become -1.
K+ I -
7. Example 1.
Potassium + Iodine
Finally, combine the 2 ions to form the final compound.
K+ + I- KI
8. Example 2.
Magnesium + Oxygen
First, write the Lewis Diagram for each element.
Mg O
9. Example 2.
Magnesium + Oxygen
Next, draw an arrow showing the transfer of electrons
from one atom to the other.
Mg O
10. Example 2.
Magnesium + Oxygen
Now, show the charges on the newly formed ions.
Magnesium lost 2 electrons to become +2, and Oxygen
gained 2 electrons to become -2.
Mg2+ O2-
11. Example 2.
Magnesium + Oxygen
Finally, combine the 2 ions to form the final compound.
Mg2+ +O2- MgO
12. Example 3.
Lithium + Nitrogen
First, write the Lewis Diagram for each element.
Li N
13. Example 3.
Lithium + Nitrogen
Next, draw an arrow showing the transfer of electrons
from one atom to the other. Notice that 1 Lithium does
not provide enough electrons, so add more.
Li N
14. Example 3.
Lithium + Nitrogen
A second Lithium atom provides another electron, still
leaving Nitrogen 1 short. So, add another.
Li N
15. Example 3.
Lithium + Nitrogen
Nitrogen now has eight valence electrons. It took 3 Lithium
atoms to provide enough electrons to fill Nitrogen’s
valence energy level.
Li N
16. Example 3.
Lithium + Nitrogen
Now, show the charges on the newly formed ions. Lithium
lost 1 electron to become +1, and Nitrogen gained 3
electrons to become -3.
Li + N3-
17. Example 3.
Lithium + Nitrogen
Finally, combine the newly formed ions to make the
compound.
Li ++ Li ++ Li ++ N3- Li3N
18. Covalent Bonds
• Form when one atom shares electrons with
another atom.
• Always form between between two
nonmetals.
• The oxidation numbers must add up to
zero.
19. Example 1.
Fluorine + Fluorine
First, write the Lewis Diagram for each element.
F F
20. Example 1.
Fluorine + Fluorine
Next, draw circles showing the electrons that are shared.
F F
21. Example 1.
Fluorine + Fluorine
Finally, draw a line showing the bond between the atoms
and then write the formula.
F F F2
22. Example 2.
3 Hydrogen + Phosphorus
First, write the Lewis Diagram for each element.
H
H P
H
23. Example 2.
3 Hydrogen + Phosphorus
Next, draw circles showing the electrons that are shared.
H
HP
H
24. Example 2.
3 Hydrogen + Phosphorus
Finally, draw lines showing the bond between the atoms
and then write the formula.
H
HP H3P
H
25. Example 3.
2 Hydrogen + Sulfur
First, write the Lewis Diagram for each element.
H
H S
26. Example 3.
2 Hydrogen + Sulfur
Next, draw circles showing the electrons that are shared.
H
HS
27. Example 3.
2 Hydrogen + Sulfur
Finally, draw lines showing the bond between the atoms
and then write the formula.
H
HS H2S