Jan13
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The document contains the schedule and topics for a chemistry class covering Chapter 11 on gases, liquids, and solids. It includes the reading assignment which covers intermolecular forces and properties of liquids, as well as homework assignments on gas laws, phase changes, and properties of solutions that are due on Wednesday and Friday. The class will have a reading quiz and homework quiz over sections 11.1-11.4 on Friday.
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This document provides an overview of chemistry concepts including the definition of chemistry, major branches of chemistry, early theories of matter, and important figures in the development of modern chemistry such as Aristotle, Democritus, Boyle, Priestley, and Dalton. It also discusses the classification of matter as elements, compounds, and mixtures. Key chemistry concepts like physical and chemical properties, physical and chemical changes, energy, heat, and phase changes are introduced.
INTERMOLECULAR FORCES OF ATTRACTION.pptx
Intermolecular forces are the attractive forces between molecules. The main types are London dispersion forces, dipole-dipole forces, and hydrogen bonding. Properties like melting point, boiling point, solubility, and viscosity depend on the strength of intermolecular forces - stronger forces require more energy to overcome and result in higher melting and boiling points, like dissolving like, and slower flow. Hydrogen bonding is the strongest intermolecular force.
Chemical Reactions
The document discusses various topics relating to chemistry including chemical reactions, the periodic table, chemical bonding, and reaction rates. It provides definitions and explanations of key terms and concepts. Examples are given to illustrate different types of chemical reactions like synthesis, decomposition, combustion, and displacement reactions. Factors that affect reaction rates like concentration, temperature, surface area, and catalysts are also summarized.
Chapter 2
The document discusses the fundamental concepts of chemistry including the structure of atoms, types of chemical bonds, and acid-base chemistry. It explains that all matter is composed of atoms that can bond through covalent, ionic, or hydrogen bonds to form molecules and compounds. Special attention is given to the unique properties of water that allow it to act as both an acid and base and maintain homeostasis through buffer systems in living organisms.
Kmt, intermolecular forces, intro energy
The document discusses liquids and solids from the perspective of the kinetic molecular theory. It explains that in liquids, particles are more closely packed than gases due to intermolecular forces, but are still able to flow freely unlike solids where particle motion is limited to vibration. Key differences between liquids and solids include density, compressibility, diffusion rates, and types of molecular structures (crystalline vs amorphous). The document also covers concepts such as surface tension, intermolecular forces including hydrogen bonding and London dispersion forces, and how force strength influences melting and boiling points.
Classifying Matter
This document discusses the properties and states of matter. It defines matter as anything that has mass and takes up space, and explains that matter is made up of atoms. It then describes the three main states of matter - solids, liquids, and gases - and how their properties differ based on factors like the arrangement and movement of particles. The document also briefly introduces plasma and Bose-Einstein condensates as more advanced states of matter. It concludes by contrasting physical and chemical properties and changes in matter.
Heat
This document outlines a lesson plan on heat that covers curriculum expectations, prior knowledge, demonstrations, and assessments. It discusses key concepts like the particle theory of solids, liquids, and gases. Experiments are proposed to show how heat causes expansion and convection currents. Misconceptions about particle size and heat transfer mechanisms are addressed. Societal applications involving heat transfer are also described.
Matter of our surrounding |part 2
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9th cbse
Can Matter change its state?
Effect of change of temperature
Effects of change of pressure
Evaporation
Factors affecting evaporation
How does evaporation cause cooling
Summary
Matter of our surrounding |part 2
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Jan13
- 1. Monday Jan 13 • Roll sheet, please sign • Reading Quiz on 11.3-11.4 • Chapter 11 – 11.1 – 11.2 – 11.3 – 11.4 Gases, Liquids, and Solids Intermolecular Forces Select Properties of Liquids Phase Changes
- 2. Office Hours My office is Parmer 324 • MWF 10:30-11:30 here in Lewis Hall • Or by appointment (e-mail me) • Office hours will be posted on the myDU page each week (if there are changes)
- 3. Pre-Class Reading Assignment Reading for Wednesday Sections 11.5-11.6 There will be a Reading Quiz at the beginning of class.
- 4. Teams – sit class with your teams in class, you may have a different study group outside of 1 Anayeli, Emily Green, Frank, Fernando 2 Yumna, Nicole, Chrisitian, Max 3 Chandler, Alyssa Hernandez, Joseph, Brenda 4 Oliver, Arley, Valerie, Monica 5 Adrian, Jeannette, Miriam, Tezira 6 Catherine Conte, Saman, Evelina, Catherine Trempe 7 Yazmin, Kaitlyn, Jency, Veronica 8 Clayton, Alexandra, Sweta, Camila 9 Alyssa Domico, Matt Kozlowski, Ignacio, Nikita 10 Jacob, Katy, Marissa, Ryan
- 5. Chapter 11 Homework Turn in today – 9, 15, 17, 19, 21, 23, 25, 27 Due Wednesday in class – 33, 35, 39, 45 Due Friday in class – 7, 49, 51, 53, 55, 57, 59, 61, 73 Quiz on section 11.1-11.4 homework problems on Friday Jan. 17 in class.
- 6. Polar Covalent Bonds From chapter 8 • When two atoms share electrons unequally, a bond dipole results. • The dipole moment, , produced by two equal but opposite charges separated by a distance, r, is calculated: = Qr • It is measured in debyes (D).
- 8. Difference in Electronegativity tells you about the polarity of the bond F2 HF LiF Electroneg ativity difference 4.0-4.0=0 4.0-2.1=1.9 4.0-1.0=3.0 Type of bond Non polar covalent Polar covalent Ionic 1. If the electronegativity difference (usually called ΔEN) is < 0.5, then the bond is nonpolar covalent. 2. If the ΔEN is 0.5 - 1.6, the bond is considered polar covalent 3. If the ΔEN is > 2.0, then the bond is ionic. From chapter 8
- 9. Intermolecular Forces Affect Many Physical Properties – example boiling pt The strength of the attractions between particles can greatly affect the properties of a substance or solution. Why does acetic acid boil at a higher temperature?
- 11. Any questions on 11.1-11.2? Sample Exercise 11.2 List the substances BaCl2 H2, CO, HF, Ne in order of increasing boiling point 1. Are ions present? 2. Is the molecule polar? 3. O,N,F bond with H and lone pair of electrons? 4. Molecular weight?
- 12. Main topics of 11.3-11.4 1. Viscosity 2. Surface tension 3. Enthalpy of phase changes • Phase change diagram 4. Heating Curve 5. Critical Temperature and Pressure
- 13. Viscosity • Resistance of a liquid to flow is called viscosity. • It is related to the ease with which molecules can move past each other. • Viscosity increases with stronger intermolecular forces and decreases with higher temperature.
- 14. Surface Tension results from the net inward force experienced by the molecules on the surface of a liquid.
- 15. Exothermic/Endothermic energy • Ice melting is endothermic • Energy must be put into the system(ice) from surroundings to make ice go from solid to liquid phase • Energy is need to push molecules farther apart • Heat of Fusion, DH fus DH is positive
- 16. Phase Changes DH = H final - H initial Endothermic – takes Energy to push molecules farther apart (arrow up red) DH vap DH sub DH fus DH vap DH sub DH is positive Exothermic – energy is released (arrow down blue) DH fus DH freezing DH condensation DH deposition DH is negative
- 17. Energy Changes Associated with Changes of State DH sub = DH fus + DH vap It takes more heat to vaporize substances than to melt them.
- 18. Specific heat is the amount of heat energy necessary to increase the temperature of a given mass of a particular substance by some amount Specific heat = heat transferred mass temperature change Cs = q m DT For liquid water 4.184 J/g-K
- 19. Heating Curves DH vap DH fus • The heat added to the system at the melting and boiling points goes into pulling the molecules farther apart from each other. • The temperature of the substance does not rise during a phase change. • BC DH fus • DE DH vap
- 20. DH vap Specific heat of water DH fus Specific heat of ice Specific heat of g
- 21. Cooling Curves Exothermic process DT is negative Heat added
- 22. gas Cooling Curves Exothermic process DT is negative F liquid Gas->liquid H solid Liquidsolid G Heat added http://grade9sciencepedagogics.pbworks.com/f/1321228118/Cooling%20Curve%20elearning.png
- 23. Sample Ex 11.3 Part A 1.00 mole of ice at 25C to steam at 125 constant pressure 1 atm Part B DH • 100g water cooled to ice at -30.0 oC Specific heat • H2O(s) 2.03J/gK • H2O(l) 4.184J/gK • H2O(g) 1.84J/gK DH fus 6.01kJ/mol DH vap 40.67kJ/mol
- 24. Chapter 11 Homework Due Wednesday in class – 33, 35, 39, 45 Due Friday in class – 7, 49, 51, 53, 55, 57, 59, 61, 73 Quiz on HW from 11.1-11.4 homework problems on Friday Jan. 17 in class.