Physical Science Week 2.1.pptx
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This document provides an overview of molecular polarity. It defines key terms like electronegativity, polar bonds, and non-polar bonds. It explains how the polarity of molecules is determined by two main factors: 1) the polarity of the bonds between atoms as determined by electronegativity differences, and 2) the geometrical shape of the molecule as predicted by VSEPR theory. Examples of polar and non-polar molecules are given to illustrate how molecular polarity relates to bond polarity and molecular geometry.
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Polar and Non-Polar Bonds
Polar and non-polar bonds are covalent bonds. Polar bond is unequal sharing of electrons whereas non-polar bonds are equal sharing of electrons.
COMPOUNDS
A compound is a pure substance composed of two or more elements chemically bonded together, such as sodium chloride or water. Compounds can only be broken down or formed through a chemical reaction that breaks and rearranges bonds between atoms. Some common compounds found in homes include sodium chloride, water, glucose, and other substances containing ionically or covalently bonded elements.
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Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
P2.-Polar-and-Non-Polar-Molecules (1).pptx
This document discusses polar and nonpolar molecules. It defines polarity as separation of electric charge leading to a molecule having a partial positive and negative end. Polar bonds form when electrons are shared unequally between atoms, while nonpolar bonds form when electrons are shared equally. Whether a molecule is polar or nonpolar depends on whether it has any polar bonds and if it has symmetrical charge distribution. Polar molecules are asymmetrical with polar bonds and have higher melting/boiling points, while nonpolar molecules have symmetrical or equal charge distribution. The document provides examples and exercises to classify different types of bonds and molecules.
Electronegativity
The electronegativity of an element is a measure of how strongly it attracts electrons in a covalent bond. Electronegativity increases left to right and top to bottom in a period, and metals have the lowest values while nonmetals have the highest. The difference in electronegativity between two bonded atoms indicates bond type - ionic bonds form when difference is >1.7, covalent bonds form when difference is <1.7, and polar covalent bonds form for differences in between. Electronegativity values can be used to predict and investigate bond types.
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Polarity of Molecules.pptx
This document discusses the polarity of molecules. It defines electronegativity and the VSEPR theory for determining molecular geometry. A molecule's polarity depends on the polarity of its bonds, determined by electronegativity differences, and its geometry. Polar bonds result from unequal sharing of electron pairs between different elements. Molecular geometry is predicted using VSEPR theory to minimize electron pair repulsion. Both factors, bond polarity and geometry, must be considered to classify a molecule as polar or nonpolar. Examples are provided to demonstrate how to determine a molecule's polarity.
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Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
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Electronegativity
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The document provides information about ionic and covalent (molecular) bonding:
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Ionic bonding
Ionic bonds form when a metal transfers an electron to a nonmetal, giving each atom an octet of electrons. For example, sodium loses an electron to form Na+ while chlorine gains that electron to form Cl-. The resulting ions are held together by electrostatic attraction to form an ionic compound, sodium chloride (NaCl). NaCl crystallizes into a repeating pattern where Na+ and Cl- ions alternate in a crystal lattice. Ionic compounds conduct electricity when molten or dissolved due to the movement of ions.
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The document discusses different types of chemical bonds including intramolecular and intermolecular forces. It defines ionic bonds as occurring between metal and non-metal atoms through the transfer of electrons, and covalent bonds as occurring between non-metal atoms through the sharing of electrons. The document also discusses metallic bonding, the octet rule, and provides examples of different ionic compounds.
covalent bond
This document discusses properties and uses of covalent compounds. It states that covalent compounds generally have lower melting and boiling points than ionic compounds. They are also more flexible, flammable, and less soluble in water than ionic compounds. The document notes that many fuels, medicines, clothes, and foods contain covalent bonds. It provides examples such as fuels powering daily life and clothes made from covalent materials. Covalent compounds share electrons between nonmetal atoms rather than transferring electrons.
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.
Atomic combinations
The document discusses chemical bonding and atomic combinations. It explains that atoms form bonds to achieve stable electron configurations, and that there are different bond types including covalent and polar bonds. Valence shell electron pair repulsion theory is used to predict molecular shapes based on electron arrangements around central atoms. Bond properties like length, energy, and strength are also discussed.
Chemical bonding by Saliha Rais
Chemical bonds are the forces that hold atoms together in molecules and crystals. There are two main types of bonds: ionic and covalent. Ionic bonds involve a complete transfer of electrons between atoms, giving one atom a positive charge and the other a negative charge. Covalent bonds involve sharing of electron pairs between atoms. Covalent bonding can involve single, double or triple bonds with one, two or three shared pairs respectively. Ionic compounds are usually solids with high melting points, while covalent compounds have lower melting points due to weaker intermolecular forces.
covalentbonding.pptx
This document discusses the properties and uses of covalent compounds. Some key points:
1) Covalent compounds have lower melting and boiling points than ionic compounds. They are also soft, flexible, and their molecules can easily move around.
2) Covalent compounds tend to be more flammable and not conduct electricity in water. They also aren't usually very soluble.
3) Many important substances like fuels, medicines, foods, and clothes contain covalent bonds between their elements. Covalent bonding explains the nature of substances.
Lesson 1 Intro to Chemical Bonding
This document discusses covalent bonding and molecular compounds. It defines a chemical bond as a force that holds atoms together, and describes covalent bonding as atoms sharing electrons. As two atoms approach each other to form a bond, their potential energy decreases to a minimum at the bond length. Bond length and bond energy vary between different bonded atoms. The octet rule states atoms want 8 electrons in their valence shell. Practice problems classify bonds and identify valence electrons.
L3-MOLECULAR POLARITY.pptx
1) Molecules and compounds can be classified as polar or non-polar based on differences in electronegativity between bonded atoms.
2) Polar molecules have separated partial charges while non-polar molecules have evenly distributed charges. Ionic compounds are automatically polar while covalent compounds can be polar or non-polar.
3) Polar and non-polar substances exhibit different physical properties due to differences in intermolecular forces, with ionic compounds having highest melting points and polar covalent compounds being more soluble than non-polar.
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Physical Science Week 2.1.pptx
- 1. LESSON 3 POLARITY OF MOLECULES SENIOR HIGH SCHOOL PHYSICAL SC IENC E
- 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.
- 4. EXAMPLE OF MOLECULES W ATER SALT O ZO N E NITROGEN
- 5. EXAMPLE OF MOLECULES ETHYL ALC O H O L ISOPROPYL ALCOHOL SUGAR C OFFEE
- 6. INTRODUCTION • Molecule is a group of two or more atoms held together by chemical bonds.
- 8. H O W TO PLAY? Read the group of unrelated words and solve them into real words/phrases before time runs out.
- 12. GUESS THE GIBBERISH #1 LAW O W N PAYAIR LONE PAIR
- 13. GUESS THE GIBBERISH #2 PAW LIAR BANE END POLAR BOND
- 14. GUESS THE GIBBERISH #3 EEL LEAK TRUE NEED GOT THIEVES BEAT TEA ELECTRO- NEGATIVITY
- 15. GUESS THE GIBBERISH #4 N O O N FOE LARD B O O N A N D NON-POLAR BOND
- 16. GUESS THE GIBBERISH #5 MALL LET CURE LIAR JAW MEETTHREE MOLECULAR GEOMETRY
- 17. LIST OF IMPORTANT TERMS 1. Lone Pair 2. Electronegativity 3. Polar Bond 4. Non-Polar Bond 5. Molecular Geometry
- 18. POLARITY • It refers to the distribution of electric charge around atoms, chemical groups, or molecules.
- 19. 2 FACTORS THAT DETERMINE THE POLARITY OF MOLECULES 1. The polarity of the bonds between atoms can be studied based on electronegativity. 2. The geometrical shape of the molecule which can be predicted via the valence shell electron pair repulsion (VSEPR) theory.
- 20. POLARITY OF MOLECULES • All compounds can be classified based on what type of chemicalbond formedwhentheatoms combined. • The classification of the compoundcan be used to determinewhether amoleculeispolar or non-polar. • The two classificationsofcompounds arecovalent and ionic.
- 21. COVALENT AND IONIC • Covalent Compound is a molecule formed by covalent bonds, in which the atoms share one or more pairs of valence • Ionic Compounds are made up of ions rather than molecules. Instead of sharing electrons in covalent bonds, ionic compound transfer electrons from one atom to another to form bond that relies on electrostatic attraction to keep the atoms
- 22. BOND POLARITY • ELECTRONEGATIVITY (EN) • It is the measure of relative tendency of an atom to attract electrons to itselfwhenchemicallycombinedwithanother atom. • The higher the value of electronegativity, the more it tends to attract electrontoward itself.
- 24. ELECTRONEGATIVITY DIFFERENCE DIFFERENCE IN ELECTRONEGATIVITY TYPE OF COMPOUND (BOND POLARITY) Greater than or equal to 1.7 IONIC O.5 – 1.6 COVALENT POLAR Less than 0.5 NON-POLAR
- 25. EXAMPLE 1. Predict whether the bond type between the following pairs of atoms will be ionic, polar covalent,or nonpolarcovalent. 1. C andCl 2. Mg andO 3. H andCl 4. N andN 5. K andF
- 26. MOLECULAR POLARITY • For polyatomic molecules, both the bond polarity and molecular shape determine the overall molecular polarity. H2O, CCl4,NH3 and CO2
- 27. MOLECULAR POLARITY • In terms of molecular geometry, the valence shell electron pair repulsion (VSEPR) would help us to determine the theory spatial arrangement of atoms in apolyatomic molecule.