POLARITY OF MOLECULES.pptx
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This document provides an overview of molecular polarity. It defines key terms like electronegativity, polar bonds, and molecular polarity. The objectives are to define electronegativity, distinguish between polar and non-polar molecules, and explain how molecular polarity relates to properties like melting points and solubility. Examples of polar molecules like water and non-polar molecules like nitrogen are given. Bond polarity is determined by differences in electronegativity between atoms, while molecular polarity depends on both bond polarity and molecular geometry.
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Lewis and Kossel were the first to successfully explain chemical bonding in terms of electrons. They proposed that atoms bond to achieve stable electron configurations like noble gases. Lewis pictured atoms as a positively charged nucleus surrounded by 8 electrons. Atoms bond by transferring or sharing electrons to achieve stable octets. Lewis symbols were introduced to represent valence electrons. Covalent bonds form when atoms share valence electrons in order to gain full outer shells. Resonance structures represent situations where no single Lewis structure adequately describes the molecule.
Chemical Bonding and Molecular Structure-class XI
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CH 4 CHEMICAL BONDING AND MOLECULAR STRUCTURE 3.pdf
Lewis and Kossel were the first to successfully explain chemical bonding in terms of electrons. They proposed that atoms bond to achieve stable electron configurations like noble gases. Lewis pictured atoms as a positively charged nucleus surrounded by 8 electrons. He proposed that atoms bond by transferring or sharing electrons to achieve stable octets. Lewis symbols were introduced to represent valence electrons. Covalent bonds form when atoms share valence electrons to achieve stable octets. Resonance structures represent situations where no single Lewis structure adequately describes the molecule.
LGIS-Theme 1a.pptx
This document provides an overview of organic chemistry concepts including:
- The origin of organic chemistry as the study of compounds from living organisms.
- The role of carbon in organic compounds and their importance to human biology.
- Principles of atomic structure including electron shells and orbitals.
- Bond formation through sharing or transferring electrons to attain stable configurations.
- Drawing Lewis structures and accounting for formal charges and resonance.
- Molecular geometry from hybrid atomic orbitals and how this relates to bond angles.
- Intermolecular forces between molecules and various effects that influence molecular properties.
Polar Bonds and Polar Molecules.pptx
This document discusses molecular polarity and how to determine if molecules are polar or nonpolar. It defines polar and nonpolar covalent bonds based on differences in electronegativity between atoms. A molecule is polar if it contains polar bonds in an asymmetrical arrangement, whereas a molecule is nonpolar if the polar bonds are symmetrical or if all bonds are nonpolar. Examples of polar molecules include HCl and H2O, while nonpolar examples include CO2 and CF4.
Chemical Bonds 2.ppt
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
Chemical Bonds 1.ppt
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
Organic Chemistry 1.pdf
Organic Chemistry deals with carbon compounds and their structures and reactions. It originally focused on living substances but now includes synthetic compounds. Carbon forms the backbone of organic molecules due to its ability to form chains and complex structures through covalent bonding, including single, double and triple bonds. The hybridization of atomic orbitals, such as sp3 hybridization, allows carbon to form four bonds to other atoms and explains the shapes of organic molecules like methane. Understanding bonding concepts such as ionic and covalent bonds is essential to organic chemistry.
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Chemical bonding can occur via ionic bonds or covalent bonds. Ionic bonds form when electrons are transferred from one atom to another, leaving cation and anion. Covalent bonds form when atoms share electrons via overlapping orbitals. The octet rule states that atoms seek to obtain eight electrons in their valence shell. Hybridization is the mixing of atomic orbitals to form new hybrid orbitals for bonding. Common hybridizations include sp, sp2, and sp3 which determine molecular geometry. Bond properties like order, length, energy are influenced by hybridization.
BONDING.pptx
The atomic mass of an element can vary because the number of neutrons in the nucleus may be variable, even though the number of protons remains the same for a given element. There are four main types of atomic bonding - ionic, covalent, metallic, and van der Waals - which determine key material properties like hardness, melting point, and whether a material is a metal, polymer, or ceramic based on electron configuration and bonding forces between atoms. These bonding types arise from atoms seeking stable electron configurations through gaining, losing, or sharing valence electrons.
Protein_Basics.pptx
The document discusses the properties of amino acids. It explains that amino acids can be hydrophobic, hydrophilic, or amphipathic based on their hydropathy index. Amphipathic amino acids are beneficial because they can tolerate changes in environment between hydrophilic and hydrophobic. The document also discusses the differences between ampholytes and amphoteric molecules, and explains concepts like electronegativity, dipole moments, and dielectric constants in the context of amino acid properties.
Atomic Structure and chemical BONDING.pptx
This document discusses fundamentals of atomic structure and interatomic bonding. It covers topics like atomic models, quantum numbers, electron configurations, and the periodic table. The key types of atomic bonding are also summarized, including ionic, covalent, metallic, hydrogen and van der Waals bonds. Interatomic forces are described as a function of separation distance, including both attractive and repulsive forces.
Chemical bonding
The document provides a reading list for essential and supplementary textbooks on topics related to physical chemistry and inorganic chemistry. The essential reading section lists 4 textbooks, while the supplementary reading section lists 3 additional textbooks. The document concludes by recommending specific textbooks to cover topics related to ionic bonding, types of chemical bonds, and molecular orbital theory.
CHEMICAL BONDING II: Molecular geometry and Hybridization of Atomic orbitals
Chemical Bonding II: Molecular Geometry, Hybridization of Atomic Orbitals. VSEPR NOTATION, POLAR MOLECULES, DIPOLE MOMENT
Chapter 2 chemical_bonding_final
The document discusses theories related to molecular structure and chemical bonding, including:
- Lewis theory which proposes that atoms bond by sharing valence electrons to achieve stable octet configurations.
- Limitations of the octet rule are discussed, including cases where the central atom has an incomplete or expanded octet.
- Sidgwick–Powell theory predicts molecular geometry based on the number of electron pairs around the central atom.
- VSEPR theory builds on this by accounting for differences in repulsion between bond pairs and lone pairs, allowing for more accurate prediction of molecular geometry. Lone pairs occupy more space and influence the shape.
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- 1. LESSON 3 POLARITY OF MOLECULES SENIOR HIGH SCHOOL PHYSICAL SCIENCE
- 2. OOTD: OBJECTIVES OF THE DAY! At the end of this lesson, you should be able to: 1. define electronegativity; 2. find the electronegativity of elements in the periodic table; 3. distinguish between polar and non-polar molecules; 4. relate the properties of molecules to its polarity and its application and importance in our daily life.
- 3. INTRODUCTION Molecule - Is a group of two or more atoms held together by chemical bonds.
- 4. EXAMPLE OF MOLECULES WATER SALT OZONE NITROGEN
- 5. EXAMPLE OF MOLECULES ETHYL ALCOHOL ISOPROPYL ALCOHOL SUGAR COFFEE
- 10. LAW OWN PAY AIR LONE PAIR
- 11. PAW LIAR BANE END POLAR BOND
- 13. NOON FOE LARD BOON AND NON-POLAR BOND
- 14. MOLECULAR
- 15. POLARITY • It refers to the distribution of electric charge around atoms, chemical groups or molecules. • It is a physical property of compounds which relates other physical properties such as melting points, solubility, and intermolecular interactions between the polarity of a molecules.
- 18. Symbolized as X where there is the tendency for an atom of a given chemical element to attract shared electrons when forming chemical bond.
- 22. Non-polar covalent bond - A covalent bond having equal sharing of electrons that distributes the charges evenly and cancels out. - Cannot expect positive and negative charges if shared electrons are equal in number and in charge. - Thus, this result to a symmetrical structure of molecule. Ex. Atmospheric gases- N, O, H Halogens – Fl, Cl, Br
- 24. BOND POLARITY • ELECTRONEGATIVITY (EN) • It is the measure of relative tendency of an atom to attract electrons to itself when chemically combined with another atom. • It is the measure of relative tendency of an atom to attract electrons to itself when chemically combined with another atom.
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- 28. MOLECULAR POLARITY For polyatomic molecules, both the bond polarity and molecular shape determine the overall molecular polarity. Ex. H2O, CCl4, NH3 and CO2
- 29. In terms of molecular geometry, the valence shell electron pair repulsion (VSEPR) theory would help us to determine the spatial arrangement of atoms in a polyatomic molecule.