General Chemistry 2 PDF

GENRAL CHEMISTRY 2 EDGAR A. RIVERA Master Teacher 1   Use the kinetic molecular model to explain properties of liquids and solids (STEM_GC11IMF-IIIa-c-99)  Describe and differentiate the types of intermolecular forces(STEM_GC11IMF-IIIa-c-100)  Describe...

GENRAL CHEMISTRY 2 EDGAR A. RIVERA Master Teacher 1   Use the kinetic molecular model to explain properties of liquids and solids (STEM_GC11IMF-IIIa-c-99)  Describe and differentiate the types of intermolecular forces(STEM_GC11IMF-IIIa-c-100)  Describe the following properties of liquids, and explain the effect of intermolecular forces on these properties: surface tension, viscosity, vapor pressure, boiling point, MELCs and molar heat of vaporization (STEM_GC11IMF-IIIa- c-102)  Explain the properties of water with its molecular structure and intermolecular forces (STEM_GC11IMF- IIIa-c-103)  Describe the difference in structure of crystalline and amorphous solids (STEM_GC11IMF-IIIa-c-104 )   MELC: Use the kinetic molecular model to explain properties of liquids and solids (STEM_GC11IMF-IIIa-c- 99) OBJECTIVES: LESSON 1:  state kinetic molecular model; Bronsted Acid  compare the properties of liquids and solids with those of gases; & Bases  apply the kinetic molecular theory to describe liquids and solids; and  recognize the importance of the properties of solids, liquids and gas.  1. draw the Lewis structures of the following molecules with the correct shape around the central atom; 2. indicate each bond’s polarity by drawing an arrow to represent the bond dipole along each bond; 3. determine the molecule’s polarity and indicate this with an arrow to represent the dipole; 4.circle their choice in each box to mark the molecule as polar or nonpolar Answer This! Answer   Divide the class into three groups. Assign one group to act out the solid, the second as liquid and the third one as gas (students acting as particles (or molecules ) and they will present their behavior and positions relative to each other in the solid, liquid and gaseous state. )  Each group will have 5 minutes (3 minutes to discuss among Roleplay of themselves how to act the assigned state, and 2 minutes to act it.) the three  One member of the group will explain their act.  Allow the other groups to make comments on the group physical acts. states – RUBRIC: solid, liquid, gas.  Molecular Behavior Properties of Gas Liquid Solid Matter Properties of Volume/Shape Solids Gas, Density and Liquids Compressibility Motion of Molecules  a. Compare the distances among molecules in the gas, liquid and solid and rank the phases in increasing distance between particles. b. Describe the characteristic movement of the particles of gas, liquid and solid. Questions c. How are the molecules of gas, liquid and solid arranged? d. Arrange the three phases of matter in order of increasing volume of empty space between its molecules. e. Identify the property of matter that corresponds to the molecular behavior. Possible Answer   Direction: Based on the figure below, write A if the statement refers to solids only, B if the statement refers to liquids only, and C if the statement refers to a gas and D for both solids and liquids only. Provide another sheet of paper for your Activity No. answer. 1: Solid, Liquid, or Gas? 5. Particles 1. 2. 3. 4. They expand arelow The particles They have to fixed indofill close nottheir volumehave expansion containers. contact but no with fixed one sufficient when shape. another energy heated areleading to and to strong overcome also forces their slightly of attraction attractive compressible and vibrate about in a fixed forces. position. A CD B   The Kinetic Molecular Theory (KMT) is a model used to explain the behavior of matter. It is based on a series of postulates.  Some of the postulates of KMT are as follows: What is 1. The matter is made of particles that are constantly in Kinetic motion. This energy in motion is called kinetic energy. Molecular 2. The amount of kinetic energy in a substance is related to its temperature. Theory 3. There is space between particles. The amount of space in (KMT)? between particles is related to the substance's state of matter. 4. Phase changes happen when the temperature of the substance changes sufficiently. 5. There are attractive forces in between particles called intermolecular forces.  Kinetic Molecular Theory and Properties of Liquid Figure 1. Photo of water in a swimming pool; the other is of liquid water on the molecular level. What properties of liquids are evident in these two pictures?  Kinetic Molecular Theory and Properties Figure 2. Pyrite crystals and phosphorus structure trioxide molecular of Solid What properties of solids do you notice?   Direction: Draw the molecular models of solid and liquid, explain or compare their motion, volume, shape, density, compressibility and answer the given questions. Write your answer on a separate sheet of paper. SOLID LIQUID 1. 6. Activity No. 1 Kinetic molecular model Molecular Model and Properties of Motion of molecules 2. 7. Solids and Liquids Volume and shape 3. 8. 4. 9. Density 5. 10. Compressibility Answer the following questions: 1. Why liquids are less dense than solids? 2. Why liquids are much more difficult to compress than gases? 3. Why solids are almost incompressible?  Direction: Complete the paragraph below by supplying the correct term. Write your answer on a separate sheet of paper. strong forces Kinetic energy Solids have (1)_____________________. The (2)___________________ is not attractive forces There are consequences of the sufficient to overcome the (3)__________________. orderly arrangement of molecules in (4)___________.solids The particles are vibration Since not free to move and their movement is limited to (6)____________. (5)_________ fixed they are held in (7)_________________, volume they occupy a (8)_________________ and high density. Also, since they are not free to move, diffusion thus, have (9)_________ Exrcises lightly is slow and can only be compressed very (10)___________. kinetic energy to overcome their attractive Liquid particles have sufficient (11)_______________ forces. Thus, the particles can at short distances and collide with each other. But liquid particles do not move away independent of each other. Liquids, fixed therefore, have(12) ___________ shape volume but do not have fixed (13)___________. liquids is more rapid than those of solids because of the Diffusion of (14)____________ closely packed particles in solids. Since the particles are quite close, very slight but greater than of solids. compressibility is also (15)___________   Direction: Complete the table below by finding two solids and two liquids in your life. For each one, you’ll describe how you think the molecules are moving, and draw or sketch of their movement. Write your answer on a separate sheet of paper. Description of Picture of State of Substance Molecular Molecular Matter Motion Motion Performance Task No. 1: Kinetic Molecular Theory in My Life Rubric Use numbers 1-5 with 1 the lowest and 5 the highest Rating Criteria 5 4 3 2 1 Correct usage of data Accuracy of data Application of concepts TOTAL POINTS (15) END LESSON 1   MELC: Describe and differentiate the types of intermolecular forces(STEM_GC11IMF-IIIa-c-100) OBJECTIVES: Lesson 2: 1. differentiate between intramolecular and Types of intermolecular forces of attraction; Intermolecular 2. describe and explain the different Forces intermolecular forces; and 3. apply the concept of intermolecular forces to some observed phenomenon   Direction: Determine the electronegativity difference between the bonded atoms and classify the chemical bond in the given compounds as polar or nonpolar, based on the bonding range table below. Activity No. 1: Polar or Nonpolar?  Electronegativity Polar or nonpolar Difference covalent bond? H – O (in H2O) (1) (2) 2.1 3.5 Cl – Cl (3) (4) Activity No. 1: 3.0 3.0 (5) (6) Polar or Nonpolar? N – H (in NH3) 2.5 2.1 C – H (in CH4) (7) (8) 2.5 2.1 K – Br (in KBr) (9) (10) 0.82 2.96 1. Which of the given compounds is polar? Nonpolar? 2. What is the difference between polar and nonpolar?  The force between neighboring molecules is called an intermolecular force of attraction. In contrast, the attractive force between the atoms of a molecule or compound is intramolecular forces Intermolecular Forces & Intramolecular Forces  Intermolecular Forces is the force of attraction between molecules IMF IMF IMF IMF INTERMOLECULAR FORCES OF ATTRACTION  Dispersion Forces Types of Dipole-Dipole Forces Intermolecular Forces Ion-Dipole Forces Hydrogen Bond  Non polar molecules Polar molecules central atom has no If it is not a non polar, lone pair of electrons then it is a polar. Surrounding atoms How to are the same. identify polar and non polar molecule? Non polar molecules Polar molecules Polar molecules Non polar molecules  H - FON Polar Molecules Non polar Molecules Dipole-Dipole Force London Dispersion Hydrogen bonded to Force F, O, & N London Dispersion Force Hydrogen bonding How can we identify Non polar Molecules intermolecular forces? Dipole-Dipole Force Hydrogen bonding London Dispersion London Dispersion Force Force  H - FON Polar Molecules Non polar Molecules Dipole-Dipole Force London Dispersion Hydrogen bonded to Force F, O, & N London Dispersion Force Hydrogen bonding How can we Polar Molecules Non polar Molecules identify Non polar Molecules intermolecular Dipole-Dipole Force forces? London Dispersion Force  H - FON Polar Molecules Non polar Molecules Dipole-Dipole Force London Dispersion Hydrogen bonded to Force F, O, & N London Dispersion Force Hydrogen bonding How can we identify Non polar Molecules intermolecular forces? Dipole-Dipole Force Hydrogen bonding Hydrogen bonding London Dispersion Force  Dispersion forces – these forces of attraction result from temporary dipole moments induced in ordinarily nonpolar molecules. Dispersion Forces (also known as There London forces) will be a time when…..   Induced Dipole Dispersion Forces (also known as London forces) Dispersion forces or London Dispersion Force (Vander Waals Forces) – are attractive forces between temporary dipole and induced dipole or polar molecules Dispersion Forces (also known as London forces) Dipole-Dipole Force Dipole-Dipole Forces Dipole Dipole forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.  An ion-dipole intermolecular force of attraction results from the interaction between an ion and a polar molecule. ION DIPOLE FORCES   Direction: Complete the paragraph by supplying the correct term. Write your answer on a separate sheet of paper. Exercises 1 Hydrogen Bond Hydrogen Bond Hydrogen Bond Hydrogen Bond END LESSON 2   MELC: Describe the following properties of liquids, and explain the effect of intermolecular forces on these properties: surface tension, viscosity, vapor pressure, boiling point, and molar heat of vaporization (STEM_GC11IMF-IIIa-c-102) LESSON 3: OBJECTIVES: Properties of 1. identify the properties of liquids being described in a given Liquids and situation; Intermolecul 2. describe the following properties of liquids: surface tension, viscosity, vapor pressure, boiling point, and molar heat of ar Forces vaporization; 3. explain the effect of intermolecular forces on the properties of liquids; and 4. appreciate the importance of the properties of liquids in human society.  1. Surface tension 2. Viscosity 3. Capillary Action Properties 4. Vapor Pressure and Boiling of a liquid Point 5. Molar Heat of vaporization  Surface tension refers to the force that causes the molecules on the surface of a liquid to be pushed together and form a layer. Surface tension  Cohesion (chemistry), the intermolecular attraction between like-molecules. each molecule at the Surface center is attracted equally to all molecules tension adjacent to it If the intermolecular force of attraction of a liquid is strong, there is the greater force needed to break through the surface, and the greater the surface tension is.   Viscosity is a measure of a fluid’s resistance to flow. Viscosity Which liquid has the highest and lowest viscosity? A or B?  structure of honey syrup Viscosity The greater the number of H-bonds, the stronger the intermolecular force of attraction is, and the higher the viscosity of the liquid Viscosity The larger the molecule, even if it is nonpolar, the stronger the intermolecular forces and the greater the viscosity compared to nonpolar substances made up of small molecules.   Capillary action is the tendency of a liquid to rise in narrow tubes or be drawn into small openings such as those between grains of a rock. Capillary action, also known as capillarity, is Capillary a result of intermolecular attraction between Action the liquid and solid materials.   The boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the atmospheric pressure. Vapor  The vapor pressure of a liquid is the Pressure equilibrium pressure of a vapor above its and Boiling liquid (or solid), or the pressure of the vapor resulting from evaporation of a liquid above a Point sample of the liquid in a closed container.  Liquids that have high vapor pressure have low boiling points. The higher the vapor pressure of a liquid, the lower its boiling point.   The molar heat of vaporization (ΔHvap) is the energy required to vaporize 1 mole of a liquid at a given temperature.  H is the symbol for enthalpy, which means heat content at a given standard condition. Molar Heat of vaporization   How will you relate molar heat of vaporization to strength of intermolecular forces If the intermolecular attraction is strong, it takes a lot of energy to free the molecules from the liquid phase Molar Heat and the heat of vaporization will be high. of vaporization Acetone Water END LESSON 3   MELC: Explain the properties of water with its molecular structure and intermolecular forces (STEM_GC11IMF- IIIa-c-103) LESSON 4: OBJECTIVES: WATER: A 1. describe each property of water VERY UNUSUAL 2. explain the properties of water related to its LIQUID molecular and intermolecular forces 3. appreciate the importance of water in our life The Water is a good solvent Unique Water has a high specific heat. Properties The boiling point of water unusually high. of Water Solid water is less dense, and in fact floats on liquid water.   A unique property of water is its ability to dissolve a large variety of chemical substances.  It dissolves salts and other ionic compounds, as well as polar covalent compounds such as a l c o h o l s a n d o r g a n i c substances that are capable of forming hydrogen bonds with water. Water is a  Gases like oxygen and carbon dioxide will dissolve good solvent in water meaning that some animals do not need to breathe air in order to respire but they must still be able to absorb oxygen and excrete carbon dioxide.  Water is sometimes called the universal solvent because it can dissolve so many things.   Specific heat is the amount of heat or energy needed to raise the temperature of one gram of a substance by 1oC.  The specific heat of water is 1 calorie/g-°C (4.18 J/g-°C), one of the highest for many liquids. Water has a high specific heat   Boiling point, temperature at which the pressure exerted by the surroundings upon a liquid is equaled by the pressure exerted by the vapour of the liquid The boiling point of water unusually high  Unlike all other liquids, the molecules in solid water are actually farther apart than they are in liquid water. When solid water forms, the hydrogen bonds result in a very open structure with unoccupied spaces, causing the solid to occupy a larger volume than the liquid. This makes ice less dense than liquid water, causing ice to float on water. Solid water is less dense, and in fact floats on liquid water   The hydrogen bond formation among water molecules causes water to have High high surface tension. Surface  This high surface tension causes water to move from the roots of a tree to the tension top of very tall trees and explains why water moves into the fibers of a tower. This phenomenon is called capillarity.   A large amount of heat is needed to vaporize a High heat given amount of water. This causes a significant drop in temperature during of evaporation. This explains why perspiration vaporization lowers the body temperature END LESSON 4   MELC: Describe the difference in structure of crystalline and amorphous solids (STEM_GC11IMF-IIIa-c-104 ) OBJECTIVES: LESSON 5: 1. compare the properties of crystalline and amorphous solids; Structure of 2. discuss the types of crystals based on the Solids kind or nature of the particles that make them up; and 3. appreciate the importance of solids in our society   Direction: Identify the properties or features common to the given solids and their properties that can distinguish one solid from another. You can look at the rigidity of the solids, behavior on heating, and structural patterns. Write your answer on a separate sheet of paper. Questions: 1. What are the two general types of Activity : solids? What features can be used to distinguish a crystalline solid from an What amorphous solid? 2. What is the distinguishing feature of properties? crystalline solids? How are the structures of crystals determined? 3. What are the four types of crystals? What form of unit particles makes up each type of crystal? What forces bind the unit particles of each type of crystal? What are the properties of each type of crystal?  Crystalline Solids TYPES OF SOLID Amorphous Solids What is the difference between Crystalline & Amorphous solid?   Solids whose particles are arranged in regular geometric patterns are called crystalline solids. Crystalline Unit cells is the definite Solids pattern that repeats itself in the solid crystal. Examples Tetragonal = protactinium of crystal Orthorhombic = phosphorous substances Rhombohedral = mercury for Monoclinic = plutonium specific Triclinic = turquoise patterns   Amorphous solids – are solids with fixed shape and volume but their particles are not arranged in a regular geometric pattern.  Some examples of amorphous solids are glass, rubber, and some plastics. Amorphous Solids  Criteria Crystalline Solid Amorphous Solid Shape Definite and No definite geometrical form geometrical form Crystalline Solids VS Melting point Well-defined melting point Melt over a wide range of Amorphous temperatures Solids Compressibility Rigid and cannot be Some are soft like compressed graphite Cleavage Perfect cleavage Irregular cleavage when broken into when broken into pieces on plane pieces on plane surfaces surfaces  Nature Geometry Key Features of Crystalline Melting Points and Amorphous Heat of Fusion Solids Isotropism Cleavage Property Rigidity  Crystalline Solids – True Solids Amorphous Solids – Pseudo – Solids or super-cooled liquids Nature   Crystalline Solids – Particles are arranged in a repeating pattern. They have a regular and ordered arrangement resulting in a definite shape. Amorphous Solids – Particles are arranged randomly. They do not have an ordered arrangement resulting in irregular shapes Geometry   Crystalline Solids – They have a sharp melting point Amorphous Solids – They do not have sharp melting points. The solid tends to soften gradually over a temperature range Melting Points   Heat of Fusion: (The change in enthalpy when a substance is heated to change its state from solid to liquid.) Crystalline Solids – They have definite heat of fusion. Amorphous Solids – They do not have definite Heat of heat of fusion Fusion   Crystalline Solids – Anisotropic in nature. i.e., the magnitude of physical properties (such as refractive index, electrical conductivity, thermal conductivity etc) is different along with different directions of the crystal. Amorphous Solids – Isotropic in nature. i.e., the magnitude of the physical properties is the same along with all directions of the solid. Isotropism   Crystalline Solids – When cutting with a sharp edge, the two new halves will have smooth surfaces Amorphous Solids – When cutting with a sharp edge, the two resulting halves will have irregular surfaces Cleavage Property  Crystalline Solids – They are rigid solids and applying mild forces will Rigidity not distort its shape. Amorphous Solids – They are not rigid, so mild effects may change the shape.  Ionic solids Types of Covalent solids crystals Molecular solids Metallic solids  The crystal arrangement in ionic solids maximizes attractions and simultaneously minimizes repulsion making the compound possess a high degree of stability. These solids are hard, they are brittle, have high IONIC melting points, and have poor electrical and thermal conductivity. SOLIDS   This type of solids are made up of atoms and are joined by covalent bonds. Some solids from covalent bonds resulting in the formation of molecules. In some solids, however, molecules are not formed. Rather, a covalent network is formed extending throughout the solid crystal. They are very hard, have very high melting COVALENT points, and often have poor thermal and electrical conductivity. SOLIDS   The particles in molecular solids can either be atoms or molecules held together by intermolecular forces like dispersion forces, dipole-dipole forces, and hydrogen bonds. Solids with dispersion forces are also solids at room temperature.  This is also true for solids that are highly polar. This type of solids are soft, have low to moderately high melting points, MOLECULAR and have poor electrical and thermal conductivity. They are poor conductors of heat and electricity because there are no free moving electrons and no charged particles. SOLIDS   These are joined by metallic bonds.  Metallic bonds are characterized by the presence of mobile electrons around the positive metal ion.  The strength of the force depends METALLIC on the metal and, depending on the nature of the metal, they can be soft SOLIDS to hard, and melting points range from low to high.  These solids are good electrical conductors (because of the mobile electrons), good thermal conductors, and are malleable and ductile.  NaCl TYPES OF SOLID   Importance of solids in my life!  Direction: Give at least five examples of each type of crystalline solid that is found in your home. Give the uses/relevance of each in the table below. Write your answer on a separate sheet of paper. Performance Task No. 2 Rubric   Direction: Answer the assessment by clicking the link below. KINETIC MOLECULAR MODEL, PROPERTIES OF LIQUIDS AND ASSESSMENT INTERMOLECULAR FORCES & CRYSTALLINE AND AMORPHOUS SOLIDS (google.com)