The polarity of a molecule is determined by its molecular structure and the distribution of electrons within that structure. Polarity arises from differences in electronegativity between the atoms in a molecule. Electronegativity is a measure of an atom's ability to attract and hold onto electrons. When two atoms with different electronegativities bond together, the electrons in the bond are not shared equally, leading to an uneven distribution of charge within the molecule.
Polar Molecules: When there is an uneven distribution of charge within a molecule due to differences in electronegativity, the molecule is said to be polar. This results in a separation of charges, with one end of the molecule having a partial positive charge (δ+) and the other end having a partial negative charge (δ-).
Nonpolar Molecules: Nonpolar molecules have an even distribution of charge, meaning there are no significant differences in electronegativity between the atoms. As a result, there is no separation of charges within the molecule.
Electronegativity: The electronegativity of an atom is determined by the periodic table, and elements with higher electronegativities tend to attract electrons more strongly. The electronegativity difference between atoms in a bond is a key factor in determining the molecule's polarity.
Symmetry: In some cases, a molecule may have polar bonds but still be nonpolar overall due to its molecular geometry. If the polar bonds are arranged symmetrically so that the dipole moments cancel each other out, the molecule is nonpolar.
Dipole Moment: The dipole moment of a molecule is a measure of its polarity. It is a vector quantity that points from the positive end (δ+) to the negative end (δ-) of the molecule. A larger dipole moment indicates a more polar molecule.
Examples:
Water (H2O) is a polar molecule because oxygen is more electronegative than hydrogen, creating a significant dipole moment.
Carbon tetrachloride (CCl4) is a nonpolar molecule even though it has polar C-Cl bonds because the tetrahedral arrangement of the chlorine atoms results in cancellation of the dipole moments.
Solubility and Intermolecular Interactions: The polarity of a molecule plays a crucial role in its interactions with other molecules. Polar molecules tend to be soluble in polar solvents, while nonpolar molecules are more soluble in nonpolar solvents. Additionally, polar-polar interactions (dipole-dipole interactions) and nonpolar-nonpolar interactions (Van der Waals forces) are significant in determining the physical properties of substances.
Understanding the polarity of molecules is important in various fields, including chemistry, biology, and materials science, as it helps explain and predict the behavior of substances in chemical reactions and physical processes.
The polarity of a molecule is determined by its molecular structure and the distribution of electrons within that structure. Polarity arises from differences in electronegativity between the atoms in a molecule. Electronegativity is a measure of an atom's ability to attract and hold onto electrons. When two atoms with different electronegativities bond together, the electrons in the bond are not shared equally, leading to an uneven distribution of charge within the molecule.
Polar Molecules: When there is an uneven distribution of charge within a molecule due to differences in electronegativity, the molecule is said to be polar. This results in a separation of charges, with one end of the molecule having a partial positive charge (δ+) and the other end having a partial negative charge (δ-).
Nonpolar Molecules: Nonpolar molecules have an even distribution of charge, meaning there are no significant differences in electronegativity between the atoms. As a result, there is no separation of charges within the molecule.
Electronegativity: The electronegativity of an atom is determined by the periodic table, and elements with higher electronegativities tend to attract electrons more strongly. The electronegativity difference between atoms in a bond is a key factor in determining the molecule's polarity.
Symmetry: In some cases, a molecule may have polar bonds but still be nonpolar overall due to its molecular geometry. If the polar bonds are arranged symmetrically so that the dipole moments cancel each other out, the molecule is nonpolar.
Dipole Moment: The dipole moment of a molecule is a measure of its polarity. It is a vector quantity that points from the positive end (δ+) to the negative end (δ-) of the molecule. A larger dipole moment indicates a more polar molecule.
Examples:
Water (H2O) is a polar molecule because oxygen is more electronegative than hydrogen, creating a significant dipole moment.
Carbon tetrachloride (CCl4) is a nonpolar molecule even though it has polar C-Cl bonds because the tetrahedral arrangement of the chlorine atoms results in cancellation of the dipole moments.
Solubility and Intermolecular Interactions: The polarity of a molecule plays a crucial role in its interactions with other molecules. Polar molecules tend to be soluble in polar solvents, while nonpolar molecules are more soluble in nonpolar solvents. Additionally, polar-polar interactions (dipole-dipole interactions) and nonpolar-nonpolar interactions (Van der Waals forces) are significant in determining the physical properties of substances.
Understanding the polarity of molecules is important in various fields, including chemistry, biology, and materials science, as it helps explain and predict the behavior of substances in chemical reactions and physical processes.
Polarity Is the separation of an electric charge which leads a molecule to have a p o s i t i v e an d negative end.
- The distribution of electrical charge over the atoms joined by the bond. Charge is evenly distributed in a nonpolar, but unevenly distributed in a polar molecule.
POLAR MOLECULE- Unequal distribution of charges, one is more positive and the other is more negative.
- Dissolves in water.
-Asymmetrical in shape
NONPOLAR MOLECULE- Equal distribution of charges, no dipole (+/-).
- Does not dissolve in water.
- Symmetrical in shape
Can be determined by two factors:
1. electronegativity difference
2. molecular geometry through the VSEPR ( Valence Shell E l e c tron Pair Repulsion) theory
FIRST STEP: Determine the total number of electrons of the given molecule.
SECOND STEP: Draw lines to bond the atoms (one line means two electrons).
THIRD STEP: Check if the OCTET RULE is followed. Eight electrons should should be around the element. Except for hydrogen which only needs two electrons.
FOURTH STEP: Rearrange the electrons of the bonded atom. You may create double or triple bond if necessary.
FIFTH STEP: Generic Check Formula and and compare Molecular to the shape.
SIXTH STEP: answer the following questions:
-Bonded elements are the same?
(If no, it's POLAR)
(If YES, answer the following question: With lone pairs?)
(If without lone pair, it's NONPOLAR);
(If with lone pairs, is it asymmetric or symmetric?--- Asymmetric= Polar; Symmetric= Nonpolar)
Polarity Is the separation of an electric charge which leads a molecule to have a p o s i t i v e an d negative end.
- The distribution of electrical charge over the atoms joined by the bond. Charge is evenly distributed in a nonpolar, but unevenly distributed in a polar molecule.
POLAR MOLECULE- Unequal distribution of charges, one is more positive and the other is more negative.
- Dissolves in water.
-Asymmetrical in shape
NONPOLAR MOLECULE- Equal distribution of charges, no dipole (+/-).
- Does not dissolve in water.
- Symmetrical in shape
Can be determined by two factors:
1. electronegativity difference
2. molecular geometry through the VSEPR ( Valence Shell E l e c tron Pair Repulsion) theory
FIRST STEP: Determine the total number of electrons of the given molecule.
SECOND STEP: Draw lines to bond the atoms (one line means two electrons).
THIRD STEP: Check if the OCTET RULE is followed. Eight electrons should should be around the element. Except for hydrogen which only needs two electrons.
FOURTH STEP: Rearrange the electrons of the bonded atom. You may create double or triple bond if necessary.
FIFTH STEP: Generic Check Formula and and compare Molecular to the shape.
SIXTH STEP: answer the following questions:
-Bonded elements are the same?
(If no, it's POLAR)
(If YES, answer the following question: With lone pairs?)
(If without lone pair, it's NONPOLAR);
(If with lone pairs, is it asymmetric or symmetric?--- Asymmetric= Polar; Symmetric= Nonpolar)
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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.
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
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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.
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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.
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!
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5. LEARNING OBJECTIVES
1.Define electronegativity.
2.Find the electronegativity of elements in the periodic
table.
3.Explain the VSEPR Theory.
4.Draw the Geometry of molecules using VSPER
Theory.
5.Distinguish between polar and non-polar molecules.
6.
7.
8.
9.
10. Rule #2.When filling the sides of the
element symbol each side gets one dot
before doubling up. Exceptions are
Hydrogen & Helium.
Rule #1.No side can have more than two
dots because each orbital can only hold
two electrons.
11.
12. ANSWER THIS!
MATCH THE
FOLLOWING ATOMS TO
THEIR
CORRESPONDING
LEWIS DOT
STRUCTURE. USE
YOUR PERIODIC TABLE
OF ELEMENTS FOR
YOU TO BE GUIDED.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23. TWO FACTORS THAT COULD DETERMINE
THE POLARITY OF MOLECULES
• The polarity of the
bonds between
atoms which can
be studied based
on
electronegativity
• The geometrical
shape of the
molecule which
can be predicted
via Valence Shell
Electron Pair
Repulsion Theory
24.
25. Bond Polarity
Exists when two
bonded atoms
unequally share
electrons,
resulting in a
negative and a
positive end.
26. Electronegativity
The measure of the relative
tendency of an atom to attract
electrons to itself when
chemically combined with
another atom. The more
electronegativity the more it
tends to attract electron towards
itself.
27. Types of Polar Bonds
• Polar Covalent
• Occurs when electron pairs are unequally shared. The difference in
electronegativity between atoms is significant
28. examples of Polar Covalent Bonds
a.HCL
* EN of H = 2.1 EN of Cl = 3.0 ∆EN = 0.9
b. HF
* EN of H = 2.1 EN of F = 4.0 ∆EN = 1.9
29. Electronegativity and Bond Character
Electronegativity Difference Bond Character
> 2.1 Ionic
0.5 – 2.0 Polar covalent
0 – 0.4 Nonpolar covalent
30. Types of Polar Bonds
• Non - Polar Covalent
• Occurs when
electron pairs are
shared equally or the
difference in
electronegativity
between atoms is
less than 0.5.
31. examples of Non -Polar Covalent Bonds
a.H2 EN of H = 2.1 ∆EN = 0.0 , not a dipole
b.Cl2 EN of Cl = 3.0 ∆EN = 0.0, not a dipole
c.F2 EN of F = 4.0 ∆EN = 0.0, not a dipole
32. Electronegativity and Bond Character
Electronegativity Difference Bond Character
> 2.1 Ionic
0.5 – 2.0 Polar covalent
0 – 0.4 Nonpolar covalent
BEFORE WE WILL START WITH OUR CLASS ALWAYS REMEMBER AND BE GUIDED WITH OUR CLASS RULES
RR
RR
RR
RR
WE WILL FORM A GROUP WITH 5 MEMBERS. EACH MEMBER OF THE GROUP SHOULD CONTRIBUTE AN IDEA. THIS ACTIVITY SHOULD BE DONE IN 2 MINUTES. SO WORK IN GROUP SINCE YOU ARE IN A TEAM. THE WINNER OF THIS ACTIVITY WILL BE GIVEN
RR
TO UNDERSTAND MORE BETTER ABOUT THE POLARITY OF MOLECULES, LET’S HAVE AN …
THIS EXPERIMENT IS A 5 MINUTE EXPERIMENT. ALL YOU HAVE TO DO TO MIX THE LIQUID IN A TEST TUBE AND STIR IT USING A STIRRING ROD.
VINEGAR & WATER, WATER & GASOLINE, GASOLINE & VINEGAR WATER & FOOD COLOR, VINEGAR & FOOD COLOR, GASOLINE & FOOD COLOR
AND THEN TRY TO OBSERVE THE MIXTURES. YOU ONLY HAVA 3 MINUTES TO DO THIS AND EXPERIMENT AND AFTER THIS YOU ARE GOING TO THE QUESTIONS
There’s o negative answer here. Therefore you make the larger number as your minuend and the lesser as subtrahend and then get the difference.
