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A. Research and describe the properties for each crystals. Use the following as bases of property comparison. 1. Strength or hardness 2. Melting point 3. Electrical conductibility

A. Research and describe the properties for each crystals. Use the following as bases of property comparison. 1. Strength or hardness 2. Melting point 3. Electrical conductibility

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help me with my hw. Please answer letter a numbers 1-3 completely. Please base or refer on the pictures included. 

6:33 PROPERTIES OF LIQUID AND INTERMOLECULAR FORCES 1. Surface Tension. It is the measure of elastic force in the surface of a liquid. It is the amount of energy required to stretch or increase the surface of a liquid by a unit area. Intermolecular forces affect the magnitude of surface tension. Molecules within a liquid are pulled in all direction by intermolecular forces. SURFACE TENSION Water on the utace are aacted to one de 2. Capillary Action. It is the tendency of a liquid to rise in narrow tubes or to be drawn into small openings such as those between grains of rock. It is also known as capillarity which is a result of intermolecular attraction between the liquid and solid materials. There are two types of forces involved in capillary action: a. Cohesion. Intermolecular attraction between like molecules (eg: liquid molecules). b. Adhesion. Attraction between unlike molecules (eg: water and particles of the glass tube in which it passes) Concave meniscus Convex meniscus H2O Hg Adhesion Cohesion 3. Viscosity. It is a measure of fluid's resistance to flow. The greater the viscosity, the slower the liquid flows. 4. Vapor pressure. It is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature. The temperature at which the vapour pressure at the surface of a liquid becomes equal to the pressu as the temperature increases, the vapour pressure of water also increases. When temperature is high, more molecules have enough energy to escape from the liquid. On the other hand, at lower temperature, fewer molecules have sufficient energy to escape from the liquid. 5. Molar Heat of vaporization. It is the energy required to vaporize 1 mol of a liquid at a given temperature. The heat of vaporization may be considered a measure of strength of intermolecular forces in a liquid. If intermolecular forces are strong, it exerted the surroundings is called the boiling point of the liquid. So takes a lot of energy to free the molecules from the liquid phase and the heat of vaporization will be high. TYPES OF SOLIDS AND THEIR PROPERTIES Solids can be categorized as crystalline and amorphous. The difference in properties of these two groups of solid arises from the presence or absence of long range order of arrangement of the particles in the solid. Crystalline Solid Properties Arrangement particles Behavior when heated Amorphous solid of Arranged in fixed geometric Have random orientation of pattern or lattices. Attractive forces are broken by Softens when gradually heated, same amount of energy, thus, they tend to melt over a wide becomes liquid at a specific | range of temperature. |particles temperature. FACTS: 1. More than 90% of naturally occurring and artificially prepared solids are crystalline. 2. The repetition of structural units of substance over long atomic distances is referred to as long-range order. 3. The repeating units of crystalline solids are called lattices. 4. X-ray diffraction is a technique used to determine the atomic and molecular structure of a crystal, wherein atoms cause a beams of incident X-rays to diffract into many specific directions. FOUR TYPES OF CRYSTALS (SOLID) 1. Metallic crystals. Made of atoms that readily lose electrons to form positive ions (cations) but no atom in the crystal would readily gain electrons. The metal atoms gives up their electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal. The crystal is held together by electrostatic interactions between
Transcribed Image Text:6:33 PROPERTIES OF LIQUID AND INTERMOLECULAR FORCES 1. Surface Tension. It is the measure of elastic force in the surface of a liquid. It is the amount of energy required to stretch or increase the surface of a liquid by a unit area. Intermolecular forces affect the magnitude of surface tension. Molecules within a liquid are pulled in all direction by intermolecular forces. SURFACE TENSION Water on the utace are aacted to one de 2. Capillary Action. It is the tendency of a liquid to rise in narrow tubes or to be drawn into small openings such as those between grains of rock. It is also known as capillarity which is a result of intermolecular attraction between the liquid and solid materials. There are two types of forces involved in capillary action: a. Cohesion. Intermolecular attraction between like molecules (eg: liquid molecules). b. Adhesion. Attraction between unlike molecules (eg: water and particles of the glass tube in which it passes) Concave meniscus Convex meniscus H2O Hg Adhesion Cohesion 3. Viscosity. It is a measure of fluid's resistance to flow. The greater the viscosity, the slower the liquid flows. 4. Vapor pressure. It is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature. The temperature at which the vapour pressure at the surface of a liquid becomes equal to the pressu as the temperature increases, the vapour pressure of water also increases. When temperature is high, more molecules have enough energy to escape from the liquid. On the other hand, at lower temperature, fewer molecules have sufficient energy to escape from the liquid. 5. Molar Heat of vaporization. It is the energy required to vaporize 1 mol of a liquid at a given temperature. The heat of vaporization may be considered a measure of strength of intermolecular forces in a liquid. If intermolecular forces are strong, it exerted the surroundings is called the boiling point of the liquid. So takes a lot of energy to free the molecules from the liquid phase and the heat of vaporization will be high. TYPES OF SOLIDS AND THEIR PROPERTIES Solids can be categorized as crystalline and amorphous. The difference in properties of these two groups of solid arises from the presence or absence of long range order of arrangement of the particles in the solid. Crystalline Solid Properties Arrangement particles Behavior when heated Amorphous solid of Arranged in fixed geometric Have random orientation of pattern or lattices. Attractive forces are broken by Softens when gradually heated, same amount of energy, thus, they tend to melt over a wide becomes liquid at a specific | range of temperature. |particles temperature. FACTS: 1. More than 90% of naturally occurring and artificially prepared solids are crystalline. 2. The repetition of structural units of substance over long atomic distances is referred to as long-range order. 3. The repeating units of crystalline solids are called lattices. 4. X-ray diffraction is a technique used to determine the atomic and molecular structure of a crystal, wherein atoms cause a beams of incident X-rays to diffract into many specific directions. FOUR TYPES OF CRYSTALS (SOLID) 1. Metallic crystals. Made of atoms that readily lose electrons to form positive ions (cations) but no atom in the crystal would readily gain electrons. The metal atoms gives up their electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal. The crystal is held together by electrostatic interactions between
6:33 J. 4. X-ray diffraction is a technique used to determine the atomic and molecular structure of a crystal, wherein atoms cause a beams of incident X-rays to diffract into many specific directions. FOUR TYPES OF CRYSTALS (SOLID) 1. Metallic crystals. Made of atoms that readily lose electrons to form positive ions (cations) but no atom in the crystal would readily gain electrons. The metal atoms gives up their electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal. The crystal is held together by electrostatic interactions between the cations and delocalized electron. These interactions are called "metallic bonds" and the model is termed as "sea of electrons model". 2. Ionic crystals. Made of ions (cations and anions) which form strong electrostatic interactions that hold the crystal lattice together. The electrostatic attractions are numerous and extend throughout the crystal since each ion is surrounded by several ions of opposite charge, making ionic crystals hard and of high melting points. 3. Molecular crystals. Made up of atoms, such as noble gases, or molecules such as sugar, iodine and naphthalene. The atoms or molecules are held together by a mix hydrogen bonding/dipole-dipole and dispersion forces, and these are the attractive forces that are broken when crystal melts. 4. Covalent network crystals. Made of atoms in which atom is covalently bonded to its nearest neighbors. The atoms can be made of one type of atom or made ofcan be made of different atoms. There are no individual molecules and the entire crystal mat be considered one very large molecule. The valence electrons of the atoms in the crystal are all used to form covalent bonds because there are no delocalized electrons, covalent network solids do not conduct electricity. Covalent bonds are the only type of attractive bond between atoms in network solid. Form of Unit Particle Atoms/molecules London Forces Between Туре of Solid Properties Example Particle Molecular Argon, Methane Dispersion Dipole-dipole forces Hydrogen Bonds a Covalent Bonds Diamond, Covalent Network Atoms in network of quarts covalent bonds Ionic Positive and Electrostatic Туyрісаl salts, Attraction/lonic Bonds negative ion Sodium Chloride, Potassium Chloride, Calcium Nitrate Metallic Atoms Metallic Bonds All metallic elments. Activity: A. Research and describe the properties for each crystals. Use the following as bases of property comparison. 1. Strength or hardness 2. Melting point 3. Electrical conductibility 4. Heat conductibility 5. Brittleness B. Choose one type of solid, and analyse explain in two sentences why it has these properties. Example: Metallic crystals have high melting point because a large amount of energy is needed to melt the crystal since the forces of attraction to be broke are numerous and extend throughout the crystal.
Transcribed Image Text:6:33 J. 4. X-ray diffraction is a technique used to determine the atomic and molecular structure of a crystal, wherein atoms cause a beams of incident X-rays to diffract into many specific directions. FOUR TYPES OF CRYSTALS (SOLID) 1. Metallic crystals. Made of atoms that readily lose electrons to form positive ions (cations) but no atom in the crystal would readily gain electrons. The metal atoms gives up their electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal. The crystal is held together by electrostatic interactions between the cations and delocalized electron. These interactions are called "metallic bonds" and the model is termed as "sea of electrons model". 2. Ionic crystals. Made of ions (cations and anions) which form strong electrostatic interactions that hold the crystal lattice together. The electrostatic attractions are numerous and extend throughout the crystal since each ion is surrounded by several ions of opposite charge, making ionic crystals hard and of high melting points. 3. Molecular crystals. Made up of atoms, such as noble gases, or molecules such as sugar, iodine and naphthalene. The atoms or molecules are held together by a mix hydrogen bonding/dipole-dipole and dispersion forces, and these are the attractive forces that are broken when crystal melts. 4. Covalent network crystals. Made of atoms in which atom is covalently bonded to its nearest neighbors. The atoms can be made of one type of atom or made ofcan be made of different atoms. There are no individual molecules and the entire crystal mat be considered one very large molecule. The valence electrons of the atoms in the crystal are all used to form covalent bonds because there are no delocalized electrons, covalent network solids do not conduct electricity. Covalent bonds are the only type of attractive bond between atoms in network solid. Form of Unit Particle Atoms/molecules London Forces Between Туре of Solid Properties Example Particle Molecular Argon, Methane Dispersion Dipole-dipole forces Hydrogen Bonds a Covalent Bonds Diamond, Covalent Network Atoms in network of quarts covalent bonds Ionic Positive and Electrostatic Туyрісаl salts, Attraction/lonic Bonds negative ion Sodium Chloride, Potassium Chloride, Calcium Nitrate Metallic Atoms Metallic Bonds All metallic elments. Activity: A. Research and describe the properties for each crystals. Use the following as bases of property comparison. 1. Strength or hardness 2. Melting point 3. Electrical conductibility 4. Heat conductibility 5. Brittleness B. Choose one type of solid, and analyse explain in two sentences why it has these properties. Example: Metallic crystals have high melting point because a large amount of energy is needed to melt the crystal since the forces of attraction to be broke are numerous and extend throughout the crystal.
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