Hello, an explanation for any/all of these would be really helpful!
1. Where are the formal and partial charges for this structure?
2. If any, where would the hydrogens be?
3. Put a box around all of the atoms that are not sp3 or s hybridized and label their hybridizations.
Homework Answers
Partial charges arises due to the electronegativity difference between the atoms . the more electronegative atom pulls an electron and aquires partial negative charge while less electronegative aquires positive charge.
oxygen is more electronegative than carbon and hydrogen . Also nitrogen is more electronegative than carbon.
There is no electronegative difference between carbon and hydrogen .
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Hello, an explanation for any/all of these would be really
helpful!
1. Where are the formal...
a,b and c please 2. Molecular Structure (a) (5 points) Circle the compound with the highest...
a,b
and c please
2. Molecular Structure (a) (5 points) Circle the compound with the highest boiling point and draw a box around the compound with the lowest boiling point OH Br (b) (5 points) The fictional molecule below has several charged atoms. All lone pair electrons and bonds to hydrogens are explicitly shown. Add circled formal charges to all appropriate atoms. (the double bonded oxygen should have just one lone pair) :ОНн Нн Н н н NH3 н Н...
The formal charge is the "charge" an element would have in a molecule or ion if all of the bondin...
1. The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. We can draw three inequivalent Lewis structures for the tellurite ion , TeO32-. The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure.2. The best...
For Pravastatin , the molecular formula C23H36O7, answer the following a) all sp or sp2 hybridized...
For Pravastatin , the molecular formula C23H36O7, answer the following a) all sp or sp2 hybridized atoms b)all reasonably stable resonance structures showing lone pairs and charges or if it does not have any resonance structures label the polar bonds using partial positive/partial negative signs c) the most acidic hydrogen(s) in the structure and the most basic position(s) d) Identify all possible stereocenters and determine the maximum number of stereoisomers, determine if any alkenes E or Z pictures would also...
1. A. Put the following atoms in order of increasing electronegativity Br N Н B. Using the atoms above, which pair of a...
1. A. Put the following atoms in order of increasing electronegativity Br N Н B. Using the atoms above, which pair of atoms will create the most polar bond? C. Put the bonds below in order from least to greatest bond polarity С-Н N-H Н-Br D. Explain how you arrived at your answers to B and C 2. A. For the following Lewis structures, determine the formal charge on all of the atoms in the structure H H O :...
1.Draw one valid Lewis structure (including all lone pair electrons and any formal charges) for the...
1.Draw one valid Lewis structure (including all lone pair
electrons and any formal charges) for the anion
(CH2CN)−.
Assume the atoms are arranged as shown below.
H
C
C
N
H
2. Follow the curved arrows to
draw a second resonance structure for the following
species.
Make sure to minimize the formal charge on all atoms, and include resonance where appropriate Phosphorus...
Make sure to minimize the formal charge on all atoms, and
include resonance where appropriate
Phosphorus Trifluoride, PF Lewis Structure 3-D Molecular Structure Number of Valence Electrons Steric Number of Central Atom Electron Group Geometry Molecular Geometry Bond Angle(s) Polar? (If yes show dipole on 3-D structure) 08
a) Draw a Lewis structure including all resonance structures and nonzero formal charges for the isolated...
a) Draw a Lewis structure including all resonance structures and nonzero formal charges for the isolated azide anion, N3- b) .Based on the Lewis structure, predict whether the two N-N bond lengths in the azide ion will be the same or different; if different, which one is longer; and whether the bond lengths are shorter or longer than those in N2 c) Draw a Lewis structure including all resonance structures and nonzero formal charges for hydrogen azide, HN3 d) Based...
Write in any formal charges not equal to zero. If there are none, please check the...
Write in any formal charges not equal to zero. If there are none, please check the box below. X x 5 H H :0: | HỮN––c=0 Η Η There are no missing formal charges. Examine the picture in the box below. Select the atomic orbitals in the table below that would blend together to produce the set of hybrid orbitals pictured int hybrid set, select "missing atomic orbitals'. х ? missing atomic orbitals D Convert the Lewis structure below into...
Aplogies. Hello If you could Answer all that would be Super helpful! thanks! Question 26 (1...
Aplogies. Hello If you could Answer all that would be Super
helpful! thanks!
Question 26 (1 point) If the volume of a sample of Ne is doubled by a temperature change at constant pressure, what must have happened to the temperature (in K)? O It stayed the same lt tripled It went down to 1/3 It went down to 1/2 It doubled Question 27 (1 point) Which technique listed below separates a mixture of liquids on the basis of their...
Any explanation on how to figure out the last two problems would be very helpful! 05...
Any explanation on how to figure out the last two problems would
be very helpful!
05 Question (3 points) Use the standard molar entropies to calculate AS rxn for the following reactions: 4th attempt Part 1 (1 point) Ag+ (aq) + C1 (aq) —AgCl(s) -33 J/K Part 2 (1 point) CH, CH,CH2(g) +502(g) →→ 3C02(g) + 4H2O(1) J/K Part 2 (1 point) CH, CH CH2(g) +502(g) J/K + 3C02(g) + 4H20(1) Part 3 (1 point) NH3(g) +HCI(g) —NH4Cl(s) J/K
a,b
and c please
2. Molecular Structure (a) (5 points) Circle the compound with the highest boiling point and draw a box around the compound with the lowest boiling point OH Br (b) (5 points) The fictional molecule below has several charged atoms. All lone pair electrons and bonds to hydrogens are explicitly shown. Add circled formal charges to all appropriate atoms. (the double bonded oxygen should have just one lone pair) :ОНн Нн Н н н NH3 н Н...
1. A. Put the following atoms in order of increasing electronegativity Br N Н B. Using the atoms above, which pair of atoms will create the most polar bond? C. Put the bonds below in order from least to greatest bond polarity С-Н N-H Н-Br D. Explain how you arrived at your answers to B and C 2. A. For the following Lewis structures, determine the formal charge on all of the atoms in the structure H H O :...
1.Draw one valid Lewis structure (including all lone pair
electrons and any formal charges) for the anion
(CH2CN)−.
Assume the atoms are arranged as shown below.
H
C
C
N
H
2. Follow the curved arrows to
draw a second resonance structure for the following
species.
Make sure to minimize the formal charge on all atoms, and
include resonance where appropriate
Phosphorus Trifluoride, PF Lewis Structure 3-D Molecular Structure Number of Valence Electrons Steric Number of Central Atom Electron Group Geometry Molecular Geometry Bond Angle(s) Polar? (If yes show dipole on 3-D structure) 08
Write in any formal charges not equal to zero. If there are none, please check the box below. X x 5 H H :0: | HỮN––c=0 Η Η There are no missing formal charges. Examine the picture in the box below. Select the atomic orbitals in the table below that would blend together to produce the set of hybrid orbitals pictured int hybrid set, select "missing atomic orbitals'. х ? missing atomic orbitals D Convert the Lewis structure below into...
Aplogies. Hello If you could Answer all that would be Super
helpful! thanks!
Question 26 (1 point) If the volume of a sample of Ne is doubled by a temperature change at constant pressure, what must have happened to the temperature (in K)? O It stayed the same lt tripled It went down to 1/3 It went down to 1/2 It doubled Question 27 (1 point) Which technique listed below separates a mixture of liquids on the basis of their...
Any explanation on how to figure out the last two problems would
be very helpful!
05 Question (3 points) Use the standard molar entropies to calculate AS rxn for the following reactions: 4th attempt Part 1 (1 point) Ag+ (aq) + C1 (aq) —AgCl(s) -33 J/K Part 2 (1 point) CH, CH,CH2(g) +502(g) →→ 3C02(g) + 4H2O(1) J/K Part 2 (1 point) CH, CH CH2(g) +502(g) J/K + 3C02(g) + 4H20(1) Part 3 (1 point) NH3(g) +HCI(g) —NH4Cl(s) J/K
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