Chemistry

Can someone check to see if my answers look ok.

For the following crystals, explain how their melting points are related to the bonding forces and the crystal structure:

a)Copper,Cu
Copper has metallic bonds between atoms. It can occur as isometric cubic and octahedral crystals, but this is rare. The melting point is 1084.62 °C. The metalic bonds are strong, but the crystals are small and the thermal conductivity is high.

b)Water,H2O
Water as a solid has covalent molecular bonds between atoms and hydrogen bonding between molecules. It has hexagonal crystals. The melting point is 0 °C. Hydrogen bonds are weak so not much energy is required.

c)Sodium chloride,NaCl
Sodium chloride has ionic bonding in cubic close packed (ccp) crystals. The melting point is 801 °C. The temperature for melting must break ionic bonds and electrostatic forces.

d)Diamond,C
Diamond is tetrahedrally covalent bonded carbon atoms in a face centered cubic lattice. It has a melting point of 3547 °C. The covalent bonds are very strong.

  1. 👍 0
  2. 👎 0
  3. 👁 69
asked by Nancy

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    • A student crystallized a compound from benzene and observed only a few crystals when the solution cooled to room temperature. To increase the yield of crystals, the students chilled the mixture in an ice-water bath. The

    asked by david on September 20, 2012
  2. Scienece

    A student crystallized a compound from benzene and observed only a few crystals when the solution cooled to room temperature. To increase the yield of crystals, the students chilled the mixture in an ice-water bath. The chilling

    asked by Josaff on September 26, 2015
  3. organic chem!

    when trying to purify aspirin, why would i have to add hot water to the crystals that are formed, and then recool the crystals? what does this do to the crystals?

    asked by chrissy on January 24, 2010
  4. Science

    David has to dissolve salt crystals in the water. What would be the best thing to do to help the crystals dissolve quickly? A)heat the salt crystals B)crush the salt crystals C)cool the water in the tank D)use the largest salt

    asked by Sally on October 25, 2011
  5. Chemistry

    When HCl reacts with Na2CO3, what is created? More specifically, what are the crystals that remain? The questions that I need to answer: 4) What is the shape of the crystals of the product? 5) Have you seen crystals like these

    asked by Ria on March 22, 2009
  6. Organic Chemistry

    In lab, we purified acetanilide through recrystallization. We did not have have time to test the melting point to check the purification, so we put the recovered crystals in a 50ml beaker, covered the top with parafilm with a few

    asked by Rayna on October 27, 2014
  7. Chemistry 11

    When HCl reacts with Na2CO3 and H2O, what is created? More specifically, what are the crystals that remain? The questions that I need to answer: 4) What is the shape of the crystals of the product? 5) Have you seen crystals like

    asked by Ria on March 24, 2009
  8. Chem

    In the previous experiment, you recrystallized salicylic acid. If you were askedto take melting point of your crystals, would it be necessary to dry the salicylicacid crystals thoroughly first? What result would you expect from

    asked by Jason on October 13, 2008
  9. chemistry

    Iodide and diamond crystals both contain covalent bonds and yet the physical properties of their crystals are very different. Their melting points are 387K and 3827K respectively. State this type of structure present in each case

    asked by cylinder on December 14, 2017
  10. lab chemistry

    I did a project for lab chemistry where my aim was to see which substance, from a selection of 4 chlorides, recrystallises from a solution to form the most crystals. The 4 chlorides were KCl, NaCl, MgCl2 and CaCl2. KCl and NaCl

    asked by Anonymous on December 9, 2008

More Similar Questions