13. Liquids, Solids & Intermolecular Forces

Atomic, Ionic, and Molecular Solids

Ionic Solids, Molecular Solids, Metallic Solids, Network Covalent Solids, & Atomic Solids

Describe the reactions that occur when an Si1OH24 sol 
becomes a gel. What is the formula of the ceramic obtained 
when the gel is dried and sintered?

Which statement correctly describes a difference between 
graphene and graphite? 
(a) Graphene is a molecule but graphite is not. (b) Graphene 
is a single sheet of carbon atoms and graphite contains 
many, and larger, sheets of carbon atoms. (c) Graphene is an 
insulator but graphite is a metal. (d) Graphite is pure carbon 
but graphene is not. (e) The carbons are sp2 hybridized in 
graphene but sp3 hybridized in graphite.

Which solid in each pair has the higher melting point and why? d. NaCl(s) or CaO(s)

Classify each of the following as a component of a silicate ceramic, an oxide ceramic, or a nonoxide ceramic.
a. B4C

Silicon is the fundamental component of integrated circuits. 
Si has the same structure as diamond. (a) Is Si a molecular, 
metallic, ionic, or covalent-network solid?

Which would you expect to be the more ductile element,
(a) Ag or Mo? In each case explain your reasoning.

What kinds of attractive forces exist between particles 
(atoms, molecules, or ions) in (a) molecular crystals?

Introduction of carbon into a metallic lattice generally results 
in a harder, less ductile substance with lower electrical 
and thermal conductivities. Explain why this might be so.

Types of Solids

Indicate whether each statement is true or false: 
(c) Nonmetallic elements are never found in alloys.

For a given substance, the liquid crystalline phase tends to be more viscous than the liquid phase. Why?

Silicon nitride 1Si3N42, a high-temperature ceramic useful 
for making engine components, is a covalent network solid 
in which each Si atom is bonded to four N atoms and each 
N atom is bonded to three Si atoms. Explain why silicon 
nitride is more brittle than a metal like copper.

Which solid in each pair has the higher melting point and why? c. Kr(s) or Xe(s)

Draw an MO energy-level diagram that shows the population 
of the 4s band for potassium metal.

Tungsten has the highest melting point of any metal in the
periodic table: 3422 °C. The distance between W atoms in
tungsten metal is 274 pm. (b) If you put tungsten metal under
high pressure, predict what would happen to the distance
between W atoms.

What is the major electrostatic force found within an ammonia molecule, NH3?

Identify each solid as molecular, ionic, or atomic. b. CO2(s)

Explain why silicon carbide–reinforced alumina is stronger
and tougher than pure alumina.

Which type (or types) of crystalline solid is characterized by each of the following? 
(a) High mobility of electrons throughout the solid;

Doing Solids: Crash Course Chemistry #33

The smectic liquid crystalline phase can be said to be more highly ordered than the nematic phase. In what sense is this true?

The following diagrams represent the electron population of
the composite s–d band for three metals—Ag, Mo, and Y:
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/d1d37f66625549f8-1670859906409.jpg" alt="" />
Which diagram corresponds to which metal? (LO 12.7)
(a) Ag = 3, Mo = 1, Y = 2
(b) Ag = 2, Mo = 1, Y = 3
(c) Ag = 2, Mo = 3, Y = 1
(d) Ag = 1, Mo = 2, Y = 3

Which solid has the highest melting point? Why? C(s, diamond), Kr(s), NaCl(s), H2O(s)

Which type (or types) of crystalline solid is characterized by each of the following? 
(b) softness, relatively low melting point;

Silicon carbide, SiC, is a covalent network solid with a structure
similar to that of diamond. Sketch a small portion of
the SiC structure.

For each of the following alloy compositions, indicate
whether you would expect it to be a substitutional alloy, an
interstitial alloy, or an intermetallic compound:
(b) Fe0.60Ni0.40

Which of the substances Na3PO4, CBr4, rubber, Au, and 
quartz best fits each of the following descriptions? 
(a) Amorphous solid 
(b) Ionic solid 
(c) Molecular solid 
(d) Covalent network solid 
(e) Metallic solid

Which of these statements about alloys and intermetallic compounds 
is false? (a) Bronze is an example of an alloy. (b) “Alloy” 
is just another word for “a chemical compound of fixed 
composition that is made of two or more metals.” (c) Intermetallics 
are compounds of two or more metals that have a definite 
composition and are not considered alloys. (d) If you mix 
two metals together and, at the atomic level, they separate into 
two or more different compositional phases, you have created 
a heterogeneous alloy. (e) Alloys can be formed even if the atoms 
that comprise them are rather different in size.

Atomic, Ionic and Molecular Solids Example 1

As it cools off, olive oil slowly hardens and forms a solid over a range of temperatures. Which best describes it as a solid?&nbsp;

Which type (or types) of crystalline solid is characterized by each of the following? 
(d) network of covalent bonds.

Which solid in each pair has the higher melting point and why?
d. H2O(s) or H2S(s)

Both covalent-network solids and ionic solids can have
melting points well in excess of room temperature, and both
can be poor conductors of electricity in their pure form.
However, in other ways their properties are quite different.
(a) Which type of solid is more likely to dissolve in water?

Silicon is the fundamental component of integrated circuits. 
Si has the same structure as diamond. (b) Silicon 
readily reacts to form silicon dioxide, SiO2, which is quite 
hard and is insoluble in water. Is SiO2 most likely a molecular, 
metallic, ionic, or covalent-network solid?

Indicatewhethereachstatementistrueorfalse: (c) Molecules that exhibit a liquid crystalline phase do so at well-defined temperatures and pressures.

Which of the following statements does not follow from the 
fact that the alkali metals have relatively weak metal–metal 
bonding? 
(a) The alkali metals are less dense than other metals. 
(b) The alkali metals are soft enough to be cut with a knife. 
(c) The alkali metals are more reactive than other metals. 
(d) The alkali metals have higher melting points than 
other metals. 
(e) The alkali metals have low ionization energies.

Tungsten is hard and has a very high melting point 
(3422 °C), and gold is soft and has a relatively low melting 
point (1064 °C). Are these facts in better agreement with the 
electron-sea model or the MO model (band theory)? Explain.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/734ae803aad25571-1670875145572.jpg" alt="" />

Why are oxide ceramics more corrosion-resistant than metals?

Classify each of the following as a component of a silicate ceramic, an oxide ceramic, or a nonoxide ceramic.
b. Mg2SiO4

You are given a gray substance that melts at 700 °C; the solid 
is a conductor of electricity and is insoluble in water. Which 
type of solid (molecular, metallic, covalent-network, or 
ionic) might this substance be?

Indicate the type of solid (molecular, metallic, ionic, or
covalent-network) for each compound: (c) Ta2O5 (melting point, 1872°C)

Atomic, Ionic and Molecular Solids Concept 1

The melting point of sodium metal is 97.8 °C, and the melting 
point of sodium chloride is 801 °C. What can you infer 
about the relative strength of metallic and ionic bonding 
from these melting points?

Which element or elements are alloyed with gold to make 
the following types of “colored gold” used in the jewelry 
industry? For each type, also indicate what type of alloy is 
formed: (c) green gold.

Determine if each statement is true or false: (b) Substitutional alloys have “solute” atoms that replace “solvent” atoms in a lattice, but interstitial alloys have “solute” atoms that are in between the “solvent”
atoms in a lattice.

The melting points for the second-series transition elements 
increase from 1522 °C for yttrium to 2623 °C for molybdenum 
and then decrease to 321 °C for cadmium. Account for 
the trend using band theory.

Metallic, Ionic, Covalent-Network, and Molecular Solids Explained with Examples!

Two compounds (labeled I and II) have a liquid crystal state. Predict which compound has a higher temperature associ- ated with the solid to liquid crystal phase change. Explain your reasoning. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/a17962b3399d0620-1670918977662.jpg" alt="" />

State whether each sentence is true or false: 
(b) Metals have high electrical conductivities because they 
are denser than other solids.

Shown here are sketches of two processes. Which of the
processes refers to the ductility of metals and which refers
to malleability of metals?
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/fd88ee306175d3f7-1668536809760.jpg" alt="" />
(b) <img src="" alt="" />

Sodium melts at 98 °C, and magnesium melts at 650 °C. 
Account for the higher melting point of magnesium using 
the electron-sea model.

Compound A is hard, doesn’t conduct electricity, and melts at 1400ºC. Compound A represents which of the following:

Types of Solids - Molecular, Network Covalent, Ionic, and Metallic

What kinds of attractive forces exist between particles 
(atoms, molecules, or ions) in (d) and metallic crystals?

Which type (or types) of crystalline solid is characterized by each of the following? 
(c) high melting point and poor electrical conductivity;

Examine diagrams for the electron population of the composite 
s–d band for three metals in question 6. Which metal 
has the highest melting point? (LO 12.7) 
(a) Metal 1 
(b) Metal 2 
(c) Metal 3<img src="https://lightcat-files.s3.amazonaws.com/problem_images/67ce7061abd12aea-1670861432999.jpg" alt="" />

At three different temperatures,T1,T2,and T3,the molecules in a liquid crystal align in these ways: <img src="https://lightcat-files.s3.amazonaws.com/problem_images/efc2b317662ff194-1674761886381.jpg" alt="" /> (a) At which temperature or temperatures is the substance in a liquid crystalline state? At those temperatures, which type of liquid crystalline phase is depicted? [Section 11.7]

Carbon and oxygen combine to form the molecular compound 
CO2, while silicon and oxygen combine to form a 
covalent network solid with the formula unit SiO2. Explain 
the difference in bonding between the two group 4A elements 
and oxygen.

Explain why the enthalpy of vaporization of vanadium 
(460 kJ/mol) is much larger than that of zinc (114 kJ/mol).

Explain why graphite/epoxy composites are good materials 
for making tennis rackets and golf clubs.

Silicon carbide, SiC, has the three-dimensional structure shown in the figure. 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/07db951d22ed2cbe-1665589682461.jpg" alt="" /> 
(b) Would you expect the bonding in SiC to be predominantly 
ionic, metallic, or covalent?

11.3 Structures of Solids | General Chemistry

Identify each solid as molecular, ionic, or atomic. a. CaCl2(s)

How to Identify Types of Solid (Ionic, Metallic, Molecular, and Network Covalent) Examples & Problem

Steel - alloy; CO2 - molecular; Graphite - network covalent; CaCO3 - ionic; Bronze - alloy

Steel - metallic; CO2 - molecular; Graphite - network covalent; CaCO3 - ionic; Bronze - alloy

Steel - alloy; CO2 - network covalent; Graphite -network covalent; CaCO3 - ionic; Bronze - metallic

Steel - metallic; CO2 - network covalent; Graphite - amorphous; CaCO3 - network covalent; Bronze - alloy

Classify each solid as amorphous, molecular, network covalent, alloy or ionic.&nbsp;a) Steel &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; ______________________b) CO2&nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; ______________________c) Graphite &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; ______________________d) CaCO3&nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; ______________________e) Bronze, an alloy of Cu and Sn &nbsp; &nbsp; &nbsp;______________________

For each of the following groups, which metal would you 
expect to have the highest melting point: (b) rubidium, molybdenum, or indium?

Indicate whether each statement is true or false:
(a) Elastomers are rubbery solids.

The following compound undergoes a phase transition from the solid to the smectic liquid crystal phase at 121 °C. Upon further heating, the compound undergoes another transition to liquid phase at 131 °C. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/65d4dfc6ccae5546-1671380085224.jpg" alt="" />
(b) Which image represents the arrangement of molecules at 135 °C?

At three different temperatures,T1,T2,andT3,the molecules in a liquid crystal align in these ways: <img src="https://lightcat-files.s3.amazonaws.com/problem_images/9bc538235290f31e-1665590139305.jpg" alt="" /> (b) Which is the highest of these three temperatures? [Section 11.7]

Identify each solid as molecular, ionic, or atomic. d. I2(s)

Selected chlorides have the following melting points: NaCl
(801 °C), MgCl2 (714 °C), PCl3 (-94 °C), SCl2 (-121 °C)
(a) For each compound, indicate what type its solid
form is (molecular, metallic, ionic, or covalent-network).

State whether each of the following compounds is likely to have a liquid crystalline phase. Explain your reasoning. (a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/1721f015d7a74cce-1670885945076.jpg" alt="" />

Classify each of the following as a component of a silicate ceramic, an oxide ceramic, or a nonoxide ceramic.
c. MoSi2

Draw an MO energy-level diagram for beryllium metal, and 
show the population of the MOs for the following two cases. 
(a) The 2s and 2p bands are well separated in energy. 
(b) The 2s and 2p bands overlap in energy. 
Which diagram agrees with the fact that beryllium has a 
high electrical conductivity? Explain.

What is a ceramic, and what properties distinguish a ceramic 
from a metal?

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Conquer Chemistry

1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Body Centered Cubic Unit Cell

Body Centered Cubic Unit Cell contains 2 atoms total.

Phase Diagrams

Phase&nbsp;Diagrams show&nbsp;what&nbsp;effect&nbsp;temperature and pressure have&nbsp;on a pure substance in a closed system without any air.

Intermolecular Forces and Physical Properties

Intermolecular forces influence physical properties. &nbsp;We will look at direct and indirect relationships.

Face Centered Cubic Unit Cell

Face Centered Cubic Unit Cell contains 4 atoms in total.

Heating and Cooling Curves

Heating and Cooling Curves represent amount of heat (q) absorbed or released by a substance during phase changes.

Clausius-Clapeyron Equation

The Clausius-Clapeyron Equation establishes a quantitative relationship between vapor pressure and temperature.&nbsp;

Molecular Polarity

Polarity of chemical bonds happen in molecules when there is an unequal sharing of electrons.&nbsp;

Intermolecular Forces

Intramolecular Forces are the bonding forces within a molecule. Intermolecular Forces are the attractive forces between 2 molecules.

Simple Cubic Unit Cell

Simple Cubic Unit Cell is the least complex&nbsp;cubic unit cell and contains only 1 atom.

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Crystalline solids represent structures with well-organized patterns and shapes. Amorphous solids represent structures that lack an organized pattern or shape.&nbsp;</div></div>

Crystalline Solids

Crystalline Solids are composed of unit cells, crystal lattice and lattice point.