2.1If you don't have a periodictable, you can refer theelectronegativity values onthe picture shown on the left3.0L Be1.0 1.52.0 25 3.0 3.540No Ma0.9 1.21.5 1.82.1 25side.K Ca se TZn Ga se1.6 1.8V Mn Ee Ce N C0.8 1.0 1.3 1.5 1.6 1.6 15 1.8 1.9 1.8 1.9Rb Sr Y Z N Mo Ie Bu Rh Pd A0.8 1.0 1.2 1.4 1.6 1.8 1.9 22 22 2.2 1.9Ht Ia w Re s Ir e AuAsSeWrite your answers in a paper.Take a picture of your finalwork and attach the picture in1.62.02.4 28inIe1.71.71.81.92.125the provided Google forms.Ba0.7 0.9Eb1.3 1.5 1.7 1.9 22 22 2.2 24 1.9 1.8 1.9Ha1.92.0 22 B. Classification of Bonding based on ElectronegativityComplete the table below based on what is asked.More electronegative | Less electronegativeelement and valueBondingDifference inBond Typebetweenelement and valueelectronegativitySulfur - 2.5Hydrogen - 2.10.4NonpolarSulfur andHydrogencovalent bondSulfur andcesiumChlorine andbromineCalcium andchlorineOxygen andhydrogenNitrogen andhydrogen

Answered: B. Classification of Bonding based on…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter2: Lewis Structures

Section: Chapter Questions

Problem 6CTQ: It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how...

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It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how many valence electrons would such a neutral NH4 molecule have ifit could exist? a. The +1 cation, NH4+ , does exist. How many valence electrons does one NH4+ ion have? b. Draw the Lewis structure for NH4+
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
In each of the following diatomic molecules. which end of the molecule is positive relative to the other end? msp;a.hydrogenfluoride,HFb.chlorinemonofluorideClFc.iodinemonofluorideICl
Two possible Lewis diagrams for sulfine (H2CSO) are (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.
Despite the larger electronegativity difference between the bond atoms, BeCl2(a) has no dipole moment whereas SCl2(g) does possess one. Account for this difference in polarity. The answer should labelling of: Lewis structure, AXE notation, molecular and electron geometry, partial charge, dipole moment, and explanation.
For the following molecules:I. Draw the best Lewis Dot Structures for each of the following molecules. The best structuretakes into consideration resonance structures, calculations of formal charge for each atom,and tries to minimize the overall formal charge for the structure. II. Draw the 3-D VSEPR structures for the following molecules. You may combine these twodrawings (for I and II) into 1 drawing if you wish. III. Label the bond angles. IV. State the electron geometry (basic VSEPR) and molecular shape (derivative VSEPR) foreach molecule. V. State the hybridization around each central atom in the molecule. VI. State whether the overall molecule is polar or nonpolar. VII. For any two of the following molecules, state the strongest intermolecular force betweenmultiple of the same molecule.a. IF2b. H2CO3c. CH3CH2COOHd. N2O4e. PO4^3-f. CH3COCNg. ClO3^-1h. C4H8
Draw the Lewis structures for the following species: (a)CN-; (b) [N3]-; (c) [SCN]- For (b) and (c), there are more than one canonical structure that satisfy the Octet rule, and resonance is likely applied. Which canonical structures do you think would be the major contributor to the overall structure (i.e., resonance hybrid)?
A classmate of yours is convinced that he knows everythingabout electronegativity. (a) In the case of atoms X and Y havingdifferent electronegativities, he says, the diatomic moleculeX¬Y must be polar. Is your classmate correct? (b) Yourclassmate says that the farther the two atoms are apart in abond, the larger the dipole moment will be. Is your classmatecorrect?
Explain below ? The resonance hybrid is more stable than any resonance structurebecause it delocalizes electron density over a larger volume.
Which hybirdization(s) can form sigma bonds?
what bonds are being broken and formed (include sigma and pi bodns as well)
How many π bonds are in the molecule below? (Hint: count only p bonds not s bonds)

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