Chemistry
3rd Edition
ISBN: 9780073402734
Author: Julia Burdge
Publisher: MCGRAW-HILL HIGHER EDUCATION
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 12.4, Problem 1PPA
Interpretation Introduction
Interpretation:
The reason that the given molecule exhibits liquid crystal properties is to be explained.
Concept introduction:
Liquid crystals act like both conventional liquids and solid crystals.
Liquid crystals have the ability to flow and take the shape of the container like liquids and also havea regulararrangement of particles in the lattice like solids.
Liquid crystals scatter light.
Some substances exhibit liquid crystal behavior when they are melted from solids.
As the temperature increases, the solid liquifies but retains some order in one or two dimensions.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
a(i)
Based on the data presented in Figure , determine the intermolecular distance
between two Cl atom in Cl2 molecule.
240
220
Periodicity of atomic radius for Periods 13 (and start of Period 4)-
200
180
(c) doc b
160
140
120
E 100
80
60
40
20
atomic number and symbol
1
2
5
6
10 11 12 13
14
15 16
17 18 19 20
Не
Li Be
B
F Ne
Na Mg Al Si
C Ar K
Ca
Figure Atomic radius of various elements
The effective nuclear charge is the net positive charge experienced by valence
electrons. How can you relate the trend between the effective nuclear charge with
atomic radius?
a(ii)
Atomic radius (in picometres)
QUESTION 1
a)
b)
c)
Define the covalent bonding of atoms. With the aid of diagrams, show the covalent
bonding of intrinsic silicon atoms to form a crystal lattice structure.
Define the following terminologies:
i)
ii)
iii)
Ionization
Recombination
Electron-Hole-Pair (EHP)
With the aid of diagrams, describe the doping process of silicon (Si) material to
obtain p-type and n-type material.
1.1
Explain what happens when impurities
are introduced into a perfect crystal?
Chapter 12 Solutions
Chemistry
Ch. 12.1 - Practice ProblemATTEMPT Saran Wrap, the original...Ch. 12.1 - Prob. 1PPBCh. 12.1 - Practice ProblemCONCEPTUALIZE Which diagram best...Ch. 12.1 - Prob. 1CPCh. 12.1 - Prob. 2CPCh. 12.2 - Prob. 1PPACh. 12.2 - Practice ProblemBUILD Kodel is a polymer used to...Ch. 12.2 - Prob. 1PPCCh. 12.3 - Prob. 1PPACh. 12.3 - Prob. 1PPB
Ch. 12.3 - Prob. 1PPCCh. 12.3 - Prob. 1CPCh. 12.3 - Prob. 2CPCh. 12.4 - Prob. 1PPACh. 12.4 - Prob. 1PPBCh. 12.4 - Prob. 1PPCCh. 12.5 - Prob. 1PPACh. 12.5 - Prob. 1PPBCh. 12.5 - Prob. 1PPCCh. 12.6 - Prob. 1CPCh. 12.6 - Prob. 2CPCh. 12 - 12.1 Bakelite, the first commercially produced...Ch. 12 - Prob. 2QPCh. 12 - Prob. 3QPCh. 12 - Prob. 4QPCh. 12 - Prob. 5QPCh. 12 - Prob. 6QPCh. 12 - Prob. 7QPCh. 12 - Prob. 8QPCh. 12 - Prob. 9QPCh. 12 - Prob. 10QPCh. 12 - Bakelite. described in Review Question 12.1, is...Ch. 12 - Is a normal liquid isotropic or anisotropic? How...Ch. 12 - Prob. 13QPCh. 12 - 12.14 Would each of these molecules be likely to...Ch. 12 - Prob. 15QPCh. 12 - 12.16 Would an ionic compound form a liquid...Ch. 12 - Prob. 17QPCh. 12 - Prob. 18QPCh. 12 - Prob. 19QPCh. 12 - 12.20 What are some advantages and disadvantages...Ch. 12 - Prob. 21QPCh. 12 - 12.22 How does an measure the peak and valley...Ch. 12 - Name four allotropic forms of carbon.Ch. 12 - Prob. 24QPCh. 12 - Prob. 25QPCh. 12 - Prob. 26QPCh. 12 - 12.27 What type of intermolecular forces holds the...Ch. 12 - Prob. 28QPCh. 12 - Prob. 29QPCh. 12 - Prob. 30QPCh. 12 - Prob. 31QPCh. 12 - Prob. 32QPCh. 12 - Prob. 33QPCh. 12 - Prob. 34QPCh. 12 - Prob. 35QPCh. 12 - Prob. 36QPCh. 12 - What types of bonding (covalent, ionic, network,...Ch. 12 - Draw representations of isotactic, syndiotactic....Ch. 12 - Prob. 39QPCh. 12 - Draw representations of block copolymers and graft...Ch. 12 - Prob. 41APCh. 12 - 12.42 Would the compound shown form a liquid...Ch. 12 - Prob. 43APCh. 12 - Prob. 44APCh. 12 - Fluoride ion is commonly used in drinking water...Ch. 12 - Prob. 1SEPPCh. 12 - Prob. 2SEPPCh. 12 - Prob. 3SEPPCh. 12 - Prob. 4SEPP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 1. Melting point can be defined as the temperature at which the solid and liquid forms of a compound are at equilibrium. Group of answer choices True Falsearrow_forward(e) The group IV elements also exhibit allotropy. (i) What is allotropy? (ii) Give two crystalline forms of each of the following group IV elements: Carbon isi Tinarrow_forward3. The number of Bravais lattices are. (a) 7. (b) 14 (c) 10arrow_forward
- How will you distinguish between the following pairs of terms:(i) Tetrahedral and octahedral voids(ii) Crystal lattice and unit cellarrow_forward(Q2) Consider the two-dimensional hexagonal crystal structure illustrated below. Sketch any valid unit cell directly onto the image. You only need to sketch the two axes that are parallel to the page.arrow_forwardIn which of the following pure compounds would intermolecular hydrogen bonding be expected? (Select all that apply.) он O CH, CH,CH,CH;CH,OH OCHĄCH, CH, O None of the Above Submit Answer Retry Entire Group 9 more group attempts remainingarrow_forward
- Which of the following structures would you expect to have the lowest boiling point?arrow_forwardHydrogen bonds form because oxygen draws electron density away from hydrogen in a water molecule. True Falsearrow_forwardThe table below shows some physical properties of halogenatedliquids.Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole–dipole interactions. (c) The trend in electronegativityis F 7 Cl 7 Br; therefore, the most ionic compound 1CH2F22has the lowest boiling point, and the most covalent compound1CH2Br22 has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.arrow_forward
- onlyroundoffat 2decimalplaces in final answer tyIron has an atomic weight of 55.85 g/mol and a density of 7.86 g/cm3. It crystallizes in a cubic unit cell with an edge length of 0.46 nm. How many atoms are in the cell?arrow_forwardThe table below shows some physical properties of halogenatedliquids. Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole-dipole interactions. (c) The trend in electronegativityis F > Cl > Br; therefore, the most ionic compound (CH2F2)has the lowest boiling point, and the most covalent compound(CH2Br2) has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.arrow_forwardQ1 Solid matter held in place by electrostatic attraction forces between positive ions and a "sea" of freely moving electrons describes what type of bonding? ionic covalent metallic hydrogen Q2 A certain mass of nitrogen gas occupies a volume of 1.55 L at a pressure of 5.65 atm. At what pressure will the volume of this sample be 3.93 L? Assume constant temperature and ideal behavior. (?)atmarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY