k2s ionic or covalent

We expect C6(CH3)6 to have the lowest melting point and Ge to have the highest melting point, with RbI somewhere in between. The ions may either be monatomic or polyatomic. Thanks. Marisa Alviar-Agnew (Sacramento City College). Properties and several examples of each type are listed in the following table and are described in the table below. Classify \(\ce{Ge}\), \(\ce{RbI}\), \(\ce{C6(CH3)6}\), and \(\ce{Zn}\) as ionic, molecular, covalent, or metallic solids and arrange them in order of increasing melting points. Ionic crystals are hard and brittle and have high melting points. Answer =  SCN-  (Thiocyanate) is   Polar What is polar and non-polar? Answer =  AsH3  ( Arsine )  is  Polar What is polar and non-polar? As a result, the melting and boiling points of molecular crystals are much lower. Why don't libraries smell like bookstores? Network solids include diamond, quartz, many metalloids, and oxides of transition metals and metalloids. Answer =  CF2Cl2  (Dichlorodifluoromethane)  is  Polar What is polar and non-polar? B Arranging these substances in order of increasing melting points is straightforward, with one exception. A bond can be covalent, ionic or metallic. Molecular crystals are held together by weak intermolecular forces. In all cases, the intermolecular forces holding the particles together are far weaker than either ionic or covalent bonds. 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic, 12.6: Types of Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole, 1.4: The Scientific Method: How Chemists Think, Chapter 2: Measurement and Problem Solving, 2.2: Scientific Notation: Writing Large and Small Numbers, 2.3: Significant Figures: Writing Numbers to Reflect Precision, 2.6: Problem Solving and Unit Conversions, 2.7: Solving Multistep Conversion Problems, 2.10: Numerical Problem-Solving Strategies and the Solution Map, 2.E: Measurement and Problem Solving (Exercises), 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas, 3.4: Classifying Matter According to Its Composition, 3.5: Differences in Matter: Physical and Chemical Properties, 3.6: Changes in Matter: Physical and Chemical Changes, 3.7: Conservation of Mass: There is No New Matter, 3.9: Energy and Chemical and Physical Change, 3.10: Temperature: Random Motion of Molecules and Atoms, 3.12: Energy and Heat Capacity Calculations, 4.4: The Properties of Protons, Neutrons, and Electrons, 4.5: Elements: Defined by Their Numbers of Protons, 4.6: Looking for Patterns: The Periodic Law and the Periodic Table, 4.8: Isotopes: When the Number of Neutrons Varies, 4.9: Atomic Mass: The Average Mass of an Element’s Atoms, 5.2: Compounds Display Constant Composition, 5.3: Chemical Formulas: How to Represent Compounds, 5.4: A Molecular View of Elements and Compounds, 5.5: Writing Formulas for Ionic Compounds, 5.11: Formula Mass: The Mass of a Molecule or Formula Unit, 6.5: Chemical Formulas as Conversion Factors, 6.6: Mass Percent Composition of Compounds, 6.7: Mass Percent Composition from a Chemical Formula, 6.8: Calculating Empirical Formulas for Compounds, 6.9: Calculating Molecular Formulas for Compounds, 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents, 7.4: How to Write Balanced Chemical Equations, 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water, 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid, 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations, 7.8: Acid–Base and Gas Evolution Reactions, Chapter 8: Quantities in Chemical Reactions, 8.1: Climate Change: Too Much Carbon Dioxide, 8.3: Making Molecules: Mole-to-Mole Conversions, 8.4: Making Molecules: Mass-to-Mass Conversions, 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield, 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants, 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction, Chapter 9: Electrons in Atoms and the Periodic Table, 9.1: Blimps, Balloons, and Models of the Atom, 9.5: The Quantum-Mechanical Model: Atoms with Orbitals, 9.6: Quantum-Mechanical Orbitals and Electron Configurations, 9.7: Electron Configurations and the Periodic Table, 9.8: The Explanatory Power of the Quantum-Mechanical Model, 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character, 10.2: Representing Valence Electrons with Dots, 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred, 10.4: Covalent Lewis Structures: Electrons Shared, 10.5: Writing Lewis Structures for Covalent Compounds, 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule, 10.8: Electronegativity and Polarity: Why Oil and Water Don’t Mix, 11.2: Kinetic Molecular Theory: A Model for Gases, 11.3: Pressure: The Result of Constant Molecular Collisions, 11.5: Charles’s Law: Volume and Temperature, 11.6: Gay-Lussac's Law: Temperature and Pressure, 11.7: The Combined Gas Law: Pressure, Volume, and Temperature, 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles, 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen, Chapter 12: Liquids, Solids, and Intermolecular Forces, 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity, 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy, 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz, 13.5: Solution Concentration: Mass Percent, 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter, 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration, 14.1: Sour Patch Kids and International Spy Movies, 14.4: Molecular Definitions of Acids and Bases, 14.6: Acid–Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution, 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity, 14.10: Buffers: Solutions That Resist pH Change, melting points depend strongly on electron configuration, easily deformed under stress; ductile and malleable, Explain the following laws within the Ideal Gas Law. Lacking ions or free electrons, molecular crystals are poor electrical conductors. How long will the footprints on the moon last? Answer Save. I'll tell you the ionic or Molecular bond list below. 3.BrCl. How much does does a 100 dollar roblox gift card get you in robhx? For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. Determine whether each of the following compounds would be best represented by an ionic or a covalent Lewis structure.? Generally, ionic crystals form from a combination of Group 1 or 2 metals and Group 16 or 17 nonmetals or nonmetallic polyatomic ions. Answer Save. Answer =  C2Cl4 (  Tetrachloroethylene )   is nonPolar What is polar and non-polar? 1 decade ago. No. Ano ang Imahinasyong guhit na naghahati sa daigdig sa magkaibang araw? What compounds contains covalent … The actual melting points are C6(CH3)6, 166°C; Zn, 419°C; RbI, 642°C; and Ge, 938°C. Relevance-Forever Celtics fan <33. I'll tell you the ionic or Covalent bond list below. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. How long will the footprints on the moon last? Arrange the solids in order of increasing melting points based on your classification, beginning with molecular solids. Being composed of atoms rather than ions, they do not conduct electricity in any state. Answer =  CLO3-  (Chlorate)  is  Polar What is polar and non-polar? Update: Can you explain why please. Discuss how differences in electronegativity contribute to this description. It is an ionic molecule because potassium is a metal and sulfur is a non-metal. This agrees with our prediction. K2S or potassium sulfide is an ionic compound. Relevance. The ions are atoms that have gained one or more electrons (known as anions, which are negatively charged) and atoms that have lost one or more electrons (known as cations, which are positively charged). A bond cannot be both covalent and ionic. Question: Is H2SO3 an ionic or  Molecular bond  ? Answer =  CLO3-  (Chlorate)  is  Polar What is polar and non-polar? Chemical bond A chemical bond is a lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. K2S or potassium sulfide is an ionic compound. 5 years ago. Then we can enjoy music, television, work on the computer, or whatever other activity we want to undertake. Some molecular crystals, such as ice, have molecules held together by hydrogen bonds. Ionic bonding is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions, and is the primary interaction occurring in ionic compounds. Anonymous. Question =  Is C4H10 polar or  nonpolar   ? What is the rising action of faith love and dr lazaro? Informations sur votre appareil et sur votre connexion Internet, y compris votre adresse IP, Navigation et recherche lors de l’utilisation des sites Web et applications Verizon Media. All Rights Reserved. The intermolecular forces may be dispersion forces in the case of nonpolar crystals, or dipole-dipole forces in the case of polar crystals. These electrons, also referred to as delocalized electrons, do not belong to any one atom, but are capable of moving through the entire crystal.

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