States of matter 1 matter and types converted
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The document discusses the three states of matter - solids, liquids, and gases. It describes their characteristics at a microscopic level. Solids have a fixed shape and volume, with particles tightly packed in a repeating pattern that can only vibrate in place. Liquids have a fixed volume but changing shape as particles can move past each other while being attracted. Gases have volumes and shapes that change as particles are always pushing outward and spreading to fill their containers. The document also discusses intermolecular forces such as dispersion forces, dipole-dipole forces, induced dipole forces, and hydrogen bonding that influence the behavior of matter in different states.
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States of matter 1 matter and types converted
- 1. STATES OF MATTER Matter and Types PART-I Nabeela Moosakutty Lecturer Dept. of Pharmaceutics KTN College of Pharmacy
- 2. States of Matter • Different forms of matter: • Solid • Liquid • Gas • State depends on 2 things: • Particle (atoms/molecules) arrangement • Particle motion
- 3. Solid Matter • • • Fixed volume Fixed shape Particles packed together tightly – usually in a repeating pattern Examples: wood, glass, salt, plastic
- 4. Solid Matter • • Particles vibrate in place • remember – matter is always in motion! Want to separate the particles in a solid? BREAK it!
- 5. Liquid Matter • • • • • Fixed volume, changing shape Particles can move from place to place Particles attracted to each other, but more easily separate Take the shape of the container its put in Examples: milk, oil, honey, water
- 6. Gas Matter • • • Volume changes, shape changes Examples: air, oxygen, water vapor Particles always push outward on container • Spread to fill container if there is more space • Or pack closer together when there is less space = PRESSURE from the pushing!
- 8. • THREE STATES OF MATTER Some Characteristics of Gases, L iquids and Sol ids and the M icroscopic E xplanation for the B ehavior Gas Liquids Solids assumes the shape and volume of its container particles can move past one another assumes the shape of the part of the containerwhich it occupies particles can move/slide past one another retains a fixed volume and shape rigid - particles locked into place compressible lots of free space between particles not easily compressible little free space between particles not easily compressible little free space between particles flows easily particles can move past one another flows easily particles can move/slide past one another does not flow easily rigid - particles cannot move/slide past one another
- 9. • TYPES OF I NTERMOLECULAR FORCES Dispersion forces or London forces Itis theweakestintermolecularforce It is a temporary at ractiveforcethat results whentheelectronsin two adjacent atoms occupy positions that make theatoms form temporarydipoles This forceis sometimescal edan induceddipole- induceddipole at raction Theseatractiveforces that cause nonpolar substances to condenseto liquids and tofreezeinto solids when thetemperatureis loweredsuf iciently
- 10. DIPOLE- DIPOLEFORCES Dipole-dipole forces are at ractiveforces betweenthepositive end of onepolar molecule and the negative end of another polar molecule. Dipole- dipole forces havestrengthsthatrange from5 kJ to20 kJ per mole.They aremuchweaker than ionic or covalent bonds and have a significant ef ect only whenthe moleculesinvolvedareclose together(touching oralmost touching).
- 11. INDUCED-DIPOLEFORCES Ion–induceddipoleforces An ion-induceddipole at ractionis a weak at ractionthatresults whentheapproach of an ion induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of electrons in thenonpolar species. • Dipole–InducedDipoleForces A dipole-induced dipole at raction is a weak at raction that results when a polar moleculeinducesa dipole inan atomorina nonpolar molecule by disturbing the arrangement of electrons in thenonpolar species.
- 12. • HYDROGENBOND The hydrogen bond is a special dipole-dipole interaction betweenthe hydrogenatomina polar N-H, O-H orF- H bondand an electronegative O, N or F atom. A – H ----B A and B or are O, N A – H ----A and F
- 13. Pressure: Gases andTemperature Particles speed up (more energy) = Volume increases! • Decreased temperature • (remove heat) Particles slow down (less energy) = Volume decreases! Increased temperature (add heat)