Concept explainers
(a)
Interpretation:
Whether element 2 has higher electronegative value than that of element 4 should be indicated.
Concept Introduction:
Close relationship between ionic and covalent bonding models becomes apparent if the bond polarity and electronegativity is considered. Electronegativity is the measure of relative attractive for the shared pair of electrons in a bond. Higher the electronegative value for an atom, the more it attracts the shared pair of electrons towards itself.
In Periodic table, when moving from left to right in a period, the electronegativity value increases. While moving from top to bottom within group, the electronegativity value decreases. Nonmetals have higher electronegativity values than metals. Metals gives electrons and nonmetals accepts electrons.
(b)
Interpretation:
Whether element 5 has higher electronegative value than that of element 6 should be indicated.
Concept Introduction:
Close relationship between ionic and covalent bonding models becomes apparent if the bond polarity and electronegativity is considered. Electronegativity is the measure of relative attractive for the shared pair of electrons in a bond. Higher the electronegative value for an atom, the more it attracts the shared pair of electrons towards itself.
In Periodic table, when moving from left to right in a period, the electronegativity value increases. While moving from top to bottom within group, the electronegativity value decreases. Nonmetals have higher electronegativity values than metals. Metals gives electrons and nonmetals accepts electrons.
(c)
Interpretation:
Whether element 7 has higher electronegative value than that of element 8 should be indicated.
Concept Introduction:
Close relationship between ionic and covalent bonding models becomes apparent if the bond polarity and electronegativity is considered. Electronegativity is the measure of relative attractive for the shared pair of electrons in a bond. Higher the electronegative value for an atom, the more it attracts the shared pair of electrons towards itself.
In Periodic table, when moving from left to right in a period, the electronegativity value increases. While moving from top to bottom within group, the electronegativity value decreases. Nonmetals have higher electronegativity values than metals. Metals gives electrons and nonmetals accepts electrons.
(d)
Interpretation:
Whether element 3 has higher electronegative value than that of element 1 should be indicated.
Concept Introduction:
Close relationship between ionic and covalent bonding models becomes apparent if the bond polarity and electronegativity is considered. Electronegativity is the measure of relative attractive for the shared pair of electrons in a bond. Higher the electronegative value for an atom, the more it attracts the shared pair of electrons towards itself.
In Periodic table, when moving from left to right in a period, the electronegativity value increases. While moving from top to bottom within group, the electronegativity value decreases. Nonmetals have higher electronegativity values than metals. Metals gives electrons and nonmetals accepts electrons.
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
General, Organic, and Biological Chemistry
- Which statements are true about electronegativity? (a) Electronegativity increases from left to right in a period of the Periodic Table. (b) Electronegativity increases from top to bottom in a column of the Periodic Table. (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity. (d) The higher the atomic number of an element, the greater its electronegativity.arrow_forward5. Considering the trend associated with electronegativities, which element is the most electronegative? A. Br B. C C. F D. Narrow_forwardDraw the Lewis structure of BH4- and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has: lone pairs = single bonds = double bonds = triple bonds = atoms with a positive formal charge = atoms with a negative formal charge = Is this structure stabilised by resonance? (Enter either yes or no below - no other words).arrow_forward
- Write a Lewis structure for each of the following polyatomic ions. Show all bonding valenceelectron pairs as lines and all nonbonding valence electron pairs as dots. For those ions thatexhibit resonance, draw the various possible resonance forms.a. phosphate ion, PO4 3-b. chlorate ion, ClO3-arrow_forwardASK YOUR TEACHER Choose the selection which gives the correct number of and bonds present in one molecule or ion of phosphate ion, PO43-. Make the central atom in your Lewis structure follow the octet rule if possible. a) There are 0 bonds and 4 bonds in one molecule or ion of this substance. b) There are 3 bonds and 1 bonds in one molecule or ion of this substance. c) There are 4 bonds and 1 bonds in one molecule or ion of this substance. d) There are 4 bonds and 4 bonds in one molecule or ion of this substance. e) There are 4 bonds and 0 bonds in one molecule or ion of this substance.arrow_forwardWhich group has the highest electronegativity in the following series? NH2 F OHarrow_forward
- Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forwardHow many unpaired dots are there in the electric configuration of a sulfur atom, S? Group of answer choices 2 6 8 4 Use electronegativities to predict which bond can be classified as ionic: Group of answer choices A, F-O B, O-O C, Si-O D, Na-O Predict which bond can be classified as polar covalent: Group of answer choices A, S-O B, S-Al C, S-C Predict which bond can be classified as nonpolar covalent: Group of answer choices A, C-O B, C-Si C, C-S D, C-Ca D, S-Searrow_forwardWhat determines which atoms are the central atoms? How do you adjust the number of electrons to form a cation? What about an anion? What causes some molecules with the same number of electron domains to have different shapes? Would they cause the real bond angle to be larger or smaller? Why? Which of the following elements should you expect to form an incomplete octet: H, He, Be, B, C, O? Why? Which of the following elements are good candidates to form an expanded octet: N, F, Ne, P, S, Cl, Ar? Why? What things must you consider when determining if a molecule is polar or non-polar?arrow_forward
- Rank the following element by electronegativity 1 = most of electronegative a 4 b 3 c 1 d 2arrow_forwardThe n-propyl cation can be formed from a molecule such as When the C–Cl bond is broken so that both electrons leave with Cl, the fragments formed are The carbon atom that had been attached to Cl is now sharing ____ electron pairs. In each shared pair the carbon atom owns ____ electron. The number of electrons that belong to carbon is ____. The formal charge on the carbon atom is ____. The correct Lewis structure for the n-propyl cation isarrow_forward• define electronegativity and state how electronegativity varies with position in the periodic table.arrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemical Principles in the LaboratoryChemistryISBN:9781305264434Author:Emil Slowinski, Wayne C. Wolsey, Robert RossiPublisher:Brooks Cole