Please help me with my he. Please answer letter a numbers 1-3 completely. Please refer on the text below as well as the picture included. Note: The picture inlcuded is the first page. TYPES OF SOLIDS AND THEIR PROPERTIESSolids 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. PropertiesCrystalline SolidAmorphous solidArrangement of particlesArranged in fixed geometric pattern or lattices.Have random orientation of particlesBehavior when heatedAttractive forces are broken by same amount of energy, thus, becomes liquid at a specific temperature.Softens when gradually heated, they tend to melt over a wide range of temperature. FACTS:More than 90% of naturally occurring and artificially prepared solids are crystalline.The repetition of structural units of substance over long atomic distances is referred to as long-range order.The repeating units of crystalline solids are called lattices.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)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”.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.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.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. Type of SolidForm of Unit ParticleForces Between ParticlePropertiesExampleMolecularAtoms/moleculesLondon Dispersion Dipole-dipole forces Hydrogen Bonds Argon, MethaneCovalent NetworkAtoms in a network of covalent bondsCovalent Bonds Diamond, quartsIonicPositive and negative ionElectrostatic Attraction/Ionic Bonds Typical salts, Sodium Chloride, Potassium Chloride, Calcium NitrateMetallicAtomsMetallic Bonds All metallic elments. Activity: Research and describe the properties for each crystals. Use the following as bases of property comparison.Strength or hardnessMelting pointElectrical conductibilityHeat conductibilityBrittleness PROPERTIES OF LIQUID AND INTERMOLECULAR FORCES1. Surface Tension. It is the measure of elastic force in the surface of a liquid. It is theamount of energy required to stretch or increase the surface of a liquid by a unitarea. Intermolecular forces affect the magnitude of surface tension. Moleculeswithin a liquid are pulled in all direction by intermolecular forces.SURFACE TENSIONNeedleNeedleWaterdegastly2. Capillary Action. It is the tendency of a liquid to rise in narrow tubes or to be drawninto small openings such as those between grains of rock. It is also known ascapillarity which is a result of intermolecular attraction between the liquid and solidmaterials. There are two types of forces involved in capillary action:Cohesion. Intermolecular attraction between like molecules (eg: liquidmolecules).b. Adhesion. Attraction between unlike molecules (eg: water and particles ofthe glass tube in which it passes)a.ConcavemeniscusConvexmeniscusH2OHgAdhesionCohesion3. Viscosity. It is a measure of fluid's resistance to flow. The greater the viscosity, theslower the liquid flows.4. Vapor pressure. It is a measure of the tendency of a material to change into thegaseous or vapour state, and it increases with temperature. The temperature atwhich the vapour pressure at the surface of a liquid becomes equal tothe pressure exerted by the surroundings is called the boiling point of the liquid. Soas the temperature increases, the vapour pressure of water also increases. Whentemperature is high, more molecules have enough energy to escape from the liquid.On the other hand, at lower temperature, fewer molecules have sufficient energy toescape from the liquid.5. Molar Heat of vaporization. It is the energy required to vaporize 1 mol of a liquid ata given temperature. The heat of vaporization may be considered a measure ofstrength of intermolecular forces in a liquid. If intermolecular forces are strong, ittakes a lot of energy to free the molecules from the liquid phase and the heat ofvaporization will be high.

Metallic solids, molecular solids, covalent network solids, and ionic solids are the four types of…

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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 he. Please answer letter a numbers 1-3 completely. Please refer on the text below as well as the picture included. Note: The picture inlcuded is the first page.

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.

Properties	Crystalline Solid	Amorphous solid
Arrangement of particles	Arranged in fixed geometric pattern or lattices.	Have random orientation of particles
Behavior when heated	Attractive forces are broken by same amount of energy, thus, becomes liquid at a specific temperature.	Softens when gradually heated, they tend to melt over a wide range of temperature.

FACTS:

More than 90% of naturally occurring and artificially prepared solids are crystalline.
The repetition of structural units of substance over long atomic distances is referred to as long-range order.
The repeating units of crystalline solids are called lattices.
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)

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”.
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.
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.
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.

Type of Solid	Form of Unit Particle	Forces Between Particle	Properties	Example
Molecular	Atoms/molecules	London Dispersion Dipole-dipole forces Hydrogen Bonds		Argon, Methane
Covalent Network	Atoms in a network of covalent bonds	Covalent Bonds		Diamond, quarts
Ionic	Positive and negative ion	Electrostatic Attraction/Ionic Bonds		Typical salts, Sodium Chloride, Potassium Chloride, Calcium Nitrate
Metallic	Atoms	Metallic Bonds		All metallic elments.

Activity:

Research and describe the properties for each crystals. Use the following as bases of property comparison.
Strength or hardness
Melting point
Electrical conductibility
Heat conductibility
Brittleness

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
Needle
Needle
Water
degastly
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:
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)
a.
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 pressure exerted by the surroundings is called the boiling point of the liquid. So
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
takes a lot of energy to free the molecules from the liquid phase and the heat of
vaporization will be high.

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Activity: Research and describe the properties for each crystals. Use the following as bases of property comparison. Strength or hardness Melting point Electrical conductibility