General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 4, Problem 4.35SP
Interpretation Introduction
Interpretation:
Given elements has to be arranged according to decreasing electronegativity.
Concept introduction:
Electronegativity:
Electronegativity is described as capable of atom to attract the shared electron towards itself. If the atom has more electronegativity means sharing of electron will be unequal. If the difference in electronegativity is large means an electrons will not be shared. If atoms has same electronegativity means sharing of electron will be equal.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Arrange the following elements in order of increasing electronegativity (from the smallest to largest electronegative value): O, S, Rb, F, Cs, As
Arrange the following elements in order of increasing electronegativity (from the smallest to largest electronegative value):
Si, Rb, F, Cl, Na
Which of the following correctly lists the
elements in order of increasing
electronegativity?
OF, Cs, S, CI
Br, Se, As, Ge
Na, Si, P, F
Be, Ca, Sr, Ba
O Cs, Na, K, Li
Chapter 4 Solutions
General Chemistry: Atoms First
Ch. 4.2 - Prob. 4.1PCh. 4.2 - Prob. 4.2PCh. 4.2 - Prob. 4.3CPCh. 4.4 - Use the electronegativity values in Figure 4.4 to...Ch. 4.4 - Order the following compounds according to the...Ch. 4.4 - An electrostatic potential map of water is shown...Ch. 4.5 - Prob. 4.7PCh. 4.5 - Write formulas for compounds with the following...Ch. 4.5 - Prob. 4.9CPCh. 4.6 - Draw electron-dot structures for the following...
Ch. 4.6 - Draw an electron-dot structure for the hydronium...Ch. 4.7 - Draw electron-dot structures for the following...Ch. 4.7 - There are two molecules with the formula C2H6O....Ch. 4.7 - The following structure is a representation of...Ch. 4.8 - Carbon monoxide, CO, is a deadly gas produced by...Ch. 4.8 - Draw an electron-dot structure for each of the...Ch. 4.8 - Prob. 4.17PCh. 4.9 - Prob. 4.18PCh. 4.9 - Draw as many resonance structures as possible for...Ch. 4.9 - The following structure shows the connections...Ch. 4.10 - Calculate the formal charge on each atom in the...Ch. 4.10 - Calculate the formal charge on each atom in the...Ch. 4.10 - What is a radical, and why are they so reactive?Ch. 4.10 - Prob. 4.24PCh. 4.10 - Draw an electron-dot structure for the ethyl...Ch. 4 - Two electrostatic potential maps are shown, one of...Ch. 4 - Prob. 4.27CPCh. 4 - Prob. 4.28CPCh. 4 - Prob. 4.29CPCh. 4 - Sinapaldehyde, a compound present in the toasted...Ch. 4 - Vitamin C (ascorbic acid) has the following...Ch. 4 - What general trends in electronegativity occur in...Ch. 4 - Prob. 4.33SPCh. 4 - Prob. 4.34SPCh. 4 - Prob. 4.35SPCh. 4 - Prob. 4.36SPCh. 4 - Prob. 4.37SPCh. 4 - Prob. 4.38SPCh. 4 - Show the direction of polarity for each of the...Ch. 4 - Prob. 4.40SPCh. 4 - Prob. 4.41SPCh. 4 - Prob. 4.42SPCh. 4 - Prob. 4.43SPCh. 4 - Prob. 4.44SPCh. 4 - Prob. 4.45SPCh. 4 - Prob. 4.46SPCh. 4 - Prob. 4.47SPCh. 4 - Prob. 4.48SPCh. 4 - Prob. 4.49SPCh. 4 - Prob. 4.50SPCh. 4 - Which of the following substances contains an atom...Ch. 4 - Draw electron-dot structures for the following...Ch. 4 - Prob. 4.53SPCh. 4 - Oxalic acid, H2C2O4, is a mildly poisonous...Ch. 4 - Draw an electron-dot structure for carbon...Ch. 4 - Prob. 4.56SPCh. 4 - Prob. 4.57SPCh. 4 - Prob. 4.58SPCh. 4 - Prob. 4.59SPCh. 4 - Methylphenidate (C14H19NO2), marketed as Ritalin,...Ch. 4 - Pregabalin (C8H17NO2), marketed as Lyrica, is an...Ch. 4 - Draw as many resonance structures as you can that...Ch. 4 - Prob. 4.63SPCh. 4 - Which of the following pairs of structures...Ch. 4 - Which of the following pairs of structures...Ch. 4 - Draw an electron-dot structure for carbon...Ch. 4 - Prob. 4.67SPCh. 4 - Prob. 4.68SPCh. 4 - Prob. 4.69SPCh. 4 - Prob. 4.70SPCh. 4 - Prob. 4.71SPCh. 4 - Prob. 4.72SPCh. 4 - Prob. 4.73SPCh. 4 - Prob. 4.74CHPCh. 4 - Thiofulminic acid, , is a highly reactive...Ch. 4 - Draw two resonance structures for methyl...Ch. 4 - Prob. 4.78CHPCh. 4 - Prob. 4.79CHPCh. 4 - Prob. 4.80CHPCh. 4 - Prob. 4.81CHPCh. 4 - Prob. 4.82CHPCh. 4 - Prob. 4.83CHPCh. 4 - Prob. 4.84CHPCh. 4 - Prob. 4.85CHPCh. 4 - Sulfur reacts with chlorine to give a product that...Ch. 4 - Sulfur reacts with ammonia to give a product A...Ch. 4 - Prob. 4.88MPCh. 4 - Prob. 4.89MP
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
- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardWhich of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions: Br, Ca, Na, N, F, Al, Sn, S, Cd?arrow_forwardH, Na, Rb Rank from highest to lowest electronegativity.arrow_forward
- Which element has the largest electronegativity? Ga, Al,In ?arrow_forward(a) Use a polar arrow to indicate the polarity of each bond: N¬H, F¬N, I¬Cl. (b) Rank the following bonds in order of increasing polarity and decreasing percent ionic character: H¬N, H¬O, H¬C.arrow_forwardAlthough I3- is a known ion, F3- is not. (a) Draw the Lewis structure for I3- (it is linear, not a triangle). (b) One of your classmates says that F3 - does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says F3- does not exist because it would violate the octet rule.Is this classmate possibly correct? (d) Yet another classmatesays F3- does not exist because F is too small to make bonds tomore than one atom. Is this classmate possibly correct?arrow_forward
- Consider the formate ion, HCO2", which is the anion formed when formic acid loses an H* ion. The H and the two O atoms are bonded to the central C atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? Explain briefly (c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2? Explain brieflyarrow_forwardConsider the following compounds: CaCl 2 , CaI 2 , and MgCl 2 . Answer the following questions based on expected periodic trends: (a) Which is expected to have t he shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forwardArrange the following in order of increasing electronegativityS, Se, Cl, Br, Iarrow_forward
- Which of the following elements should have the largest electronegativity? (Atomic numbers in parentheses to help you find elements on the Table) O Se (34) O (53) O Sr (38) O O(8)arrow_forwardWhat possible error(s) exist in the Lewis structure (assume we are trying to represent the best possible Lewis structure for the NO₂S ion knowing N is the central atom in this polyatomic ion)? [:ö==S: N= CO :O: The best structure would have double bond and two lone pairs on each oxygen atom and a single bond with three lone pairs on the sulfur. There are no errors. This is the best possible structure. The Lewis structure above does not minimize formal charges, thus is the not the best possible structure. The nitrogen atom has an expanded octet, and this structure is impossible. The Lewis structure contains the wrong number of electrons, thus this structure is impossible.arrow_forwardWrite the Lewis symbol for atoms of each of the following elements:(a) Al, (b) Br, (c) Ar, (d) Sr.arrow_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 Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY