Consider the resonance structures of formate. Select the true statemets about the resonance structures. The actual structure of formate is an average of the two resonance forms. Each oxygen atom has a double bond 50% of the time. Each carbon-oxygen bond is somewhere between a single and double bond. The actual structure of formate switches back and forth between the two resonance forms. SA stv MacBook Air

Draw three resonance structures for N3-. This species has its three atoms bonded sequentially in the following fashion: N-N-N. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Now select the statement from the multiple choices which is true about this most important resonance structure.In the most important resonance structure of N3- : a) The leftmost bond (between N and N) is a single bond.b) The rightmost bond (between N and N) is a single bond.c) The formal charge on the leftmost (N) atom is -1.d) The number of nonbonding pairs (lone pairs) of electrons on the leftmost (N) atom is 4.e) The number of nonbonding (lone) pairs of electrons on the rightmost (N) atom is 4.

How many equivalent resonance structures that follow the octet rule can be drawn for O3? One Two Three O Four This molecule has no resonance structures.

Predicting the single-bonded molecular compounds formed by two elements.

Consider the SO 3 molecule. How many valence electrons does the molecule have?   How many lone pairs of electrons are on the central atom?   How many lone pairs of electrons in total are on the substituent atoms?   How many resonance structures can be drawn for the molecule?  If the ion doesn't exhibit resonance, indicate "1" as only one structure can be drawn for the molecule.

* If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice.

Give ∆H(reaction) in kj/mol

Use Lewis theory to determine the chemical formula for the compound formed between Na and I. Use Lewis theory to determine the chemical formula for the compound formed between Na and I. Which one? A-NaI B-Na2I2 C-Na2I D-Na3I E-NaI2

Consider the following ion: BrO3−. a)  Show the full electron configuration for Br.  b)  Draw the most correct Lewis structure for BrO3− and briefly explain why your Lewis structure is correct. c)  If the structure is stabilised by resonance, draw at least one of the possible resonance forms. If it is not stabilised by resonance, briefly explain why.  d)  What is the electronic geometry of BrO3−? What is its molecular shape?  e)  Does BrO3− have a dipole moment? Briefly justify your answer. f)  On average, would you expect IO3− to have longer or shorter bonds than BrO3−? Briefly explain your answer.  g)  Which of the following molecules would you expect to have the lowest vapour pressure? Briefly explain your choice. (IMAGE WITH POSSIBILITIES) h)  What is the molecular formula for Compound C? What is the empirical formula for Compound C?

Write the Lewis structure for the following molecule. State the electronic structure (shape based on electron pairs or bonds) AND the geometric structure (shape based on the atoms only). Include all valence electrons in your structure. State how many electrons are used to form covalent bonds in the molecule. Is the molecule polar? H_2S