Polarity Fall 2021 Prachi Patel

Draw and upload a picture of the Lewis structure of H₂O (as seen above) with an arrow next to the molecule to show the direction along each of the bonds in which the electron density increases (from low density to high density). Please select file(s) Select file(s) Save Answer

For the Lewis acid-base reaction: Draw the skeletal structure of the product(s) for the Lewis acid-base reaction. Include lone pairs and formal charges (if applicable) on the structures. Click and drag to start drawing a structure. For the Lewis acid-base reaction: + __ Al

Draw and upload as an attachment the Lewis structure for acetic acid (CH3COOH). (Remember no heic files!) Label with partial charges (8* and 8) the relative polarities of the atoms, if any. Use the editor to format your answer

Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical- radical combination reaction is the formation of a new electron-pair bond. Consider the formation of hydrogen peroxide. 2 OH(g) → H,02(g) > Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons. OH(g) H,O,(g) Select Draw Rings More Erase Select Draw Rings More Erase H H Q

Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical- radical combination reaction is the formation of a new electron-pair bond. Consider the formation of hydrogen peroxide. 2 OH(g) → H,0,(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons. OH(g) H,0,(g) Rings Select Draw Rings More Erase Select Draw More Erase H.

Please do question 6 and 7 and please very short answers

Use the notes on the green page to help.  Use CER, Claim-answer to the question, reasoning-why its drawn correctly, evidence- to show why the others are incorrect. Answer completely.

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance chemical symbol, chemical formula or Lewis structure boiling point do HIC-H || (Choose one) A HIC H B H₂ (Choose one) :0: || (Choose one) ✓ HIC H Co (Choose one) S ? C D X

O.002015 mol 4. For the acid in Option do the following: HO,CCH,C H2 CH,CO2H a) Draw a Lewis structure of the acid and mark the acidic hydrogen(s) with an asterisk (*). (Hint: Organic acids, those composed of C. H. and 0, will have the partial structure "HO2C-" or "-CO2H" written in the formula, In these cases, both oxygens are bonded to the carbon and the hydrogen is bonded to one of the oxygen atoms) b) Draw a structure of the conjugate base of the acid you drew in 4a) c) Draw a structure of the conjugate base of the species for which you drew a structure in 4b) d) Which of the structures you've draw above (4a, 4b, or 4c) can act as both an acid and a base? Write appropriate chemical equations to explain your answer. Xavier University of Louisiana 176

Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical- radical combination reaction is the formation of a new electron-pair bond. Consider the chemical equation. N(g)+NO(g) → NNO(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons. N(g) NO(g) Select Draw Rings More Erase Select Draw Rings More Erase N Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Science Books of

Please answer for question four and please very short answers

Here's an electrostatic potential map for hydrochloric acid (HCI). : Draw and upload here as an attachment (remember no heic files!) a Lewis structure that represents a hydrochloric acid molecule (HCI). Label with partial charges (8* and 8) the relative polarities of the atoms, if any. How did you determine whether there are partial charges and how did you determine where to put them?

Draw and upload as an attachment the Lewis structure for hydrobromic acid (HBr). (Remember no heic files!) Label with partial charges (S* and 8-) the relative polarities of the atoms, if any. Use the editor to format your answer

PART 3: Use Lewis dot structures to show the covalent bonding in the following pairs of elements. Once you have determined the structure for the molecule, write its structural formula in the space provided; use a dash to represent a shared pair of electrons, and dots to show unshared electrons. 1) nitrogen triiodide (NI3) Final Answer: Show work here.HINT: nitrogen is in the middle! 2) carbon tetrabromide (CBr4) Show work here.HINT: carbon is in the middle! 3) dihydrogen monoxide (H2O) Show work here.HINT: oxygen is in the middle!

Here's an electrostatic potential map for water (H₂O): Draw and upload here as an attachment (remember no heic files!) a Lewis structure that represents a water molecule (H₂O). Label with partial charges (8* and 8) the relative polarities of the atoms, if any. How did you determine whether there are partial charges and how did you determine where to put them?

help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

Answer the questions in the table below about the shape of the phosgene (COCI₂) molecule. How many electron groups are around the central carbon atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central carbon atom? (You may need to use the scrollbar to see all the choices.) 0 (choose one) X Ś

Draw 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).

Using your general knowledge of periodic trends in electronegativity, predict whether the C=O bond and the C-H bonds in formaldehyde will be strongly polar, weakly polar or nonpolar.  Calculate the electronegativity difference ΔχO-C across the C=O bond and the electronegativity difference ΔχC-H to confirm or correct your predictions. For any strongly polar bond(s) on the molecule, draw the bond dipole moment adjacent to the bond in the VSEPR structure above, using crossed arrow notation to show the direction of the positive and negative bond dipoles.  Predict whether the overall molecule should be polar or nonpolar. ___________________ Explain your reasoning below. If the overall molecule is polar, draw the net dipole next to the molecule, using crossed arrow notation to indicate the direction of the dipole.

Using bond energies and the energy change of the reaction, calculate the bond energy of the CO double bond. Do not round your answer. C3H8 is propane C3H8 + 5O2 → 3CO2 + 4H2O . Bond Energy(kJ/mol) C-H 411 C-C 346 O=O 495 O-H 459 Reaction energy(kJ) -2047