Compounds and Molecules - AP Chemistry
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In a solution, a weak electrolyte exists predominately as which of the following?
In a solution, a weak electrolyte exists predominately as which of the following?
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An electrolyte is a substance that when dissolved in a solution breaks up into ions. More specifically, an electrolyte breaks up into cations (positively charged ions) and anions (negatively charged ions). While strong electrolytes break up 100% into anions and cations, weak electrolytes break apart significantly less. Less than 10% of a weak electrolyte ionizes at all in solution. That means the 90%–99% of the weak electrolyte's molecules do not ionize. This is because the intermolecular forces that form between the solution and the weak electrolyte's molecules are not stronger than the intramolecular forces holding the molecule together. While solutions containing weak electrolytes contain both ions formed from the weak electrolyte ions and molecules of the weak electrolyte, they contain mostly molecules of the weak electrolyte.
An electrolyte is a substance that when dissolved in a solution breaks up into ions. More specifically, an electrolyte breaks up into cations (positively charged ions) and anions (negatively charged ions). While strong electrolytes break up 100% into anions and cations, weak electrolytes break apart significantly less. Less than 10% of a weak electrolyte ionizes at all in solution. That means the 90%–99% of the weak electrolyte's molecules do not ionize. This is because the intermolecular forces that form between the solution and the weak electrolyte's molecules are not stronger than the intramolecular forces holding the molecule together. While solutions containing weak electrolytes contain both ions formed from the weak electrolyte ions and molecules of the weak electrolyte, they contain mostly molecules of the weak electrolyte.
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What is the hybridization on the sulfur molecule in the following molecule?
H2S
What is the hybridization on the sulfur molecule in the following molecule?
H2S
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the sulfur has 2 atoms bonded (the H) and 2 pairs of electrons, which is a total of 4 electron domains. The hybridization of the sulfur therefore is sp3
the sulfur has 2 atoms bonded (the H) and 2 pairs of electrons, which is a total of 4 electron domains. The hybridization of the sulfur therefore is sp3
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What is the bond angle in the following structure?
COH2
What is the bond angle in the following structure?
COH2
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CO2H is trigonal planar, so the bond angles will be 120 only.
CO2H is trigonal planar, so the bond angles will be 120 only.
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What is the bond angle in the following structure?
COH2
What is the bond angle in the following structure?
COH2
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CO2H is trigonal planar, so the bond angles will be 120 only.
CO2H is trigonal planar, so the bond angles will be 120 only.
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Which of the following compounds has the greatest amount of sigma bonds?
Which of the following compounds has the greatest amount of sigma bonds?
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Butane has 13 sigma bonds. Ethane has 7 sigma bonds. Benzene has 12 sigma bonds. Lithium Hydroxide has 2 sigma bonds and water has 2 sigma bonds.
Butane has 13 sigma bonds. Ethane has 7 sigma bonds. Benzene has 12 sigma bonds. Lithium Hydroxide has 2 sigma bonds and water has 2 sigma bonds.
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What is the hybridization on the sulfur molecule in the following molecule?
H2S
What is the hybridization on the sulfur molecule in the following molecule?
H2S
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the sulfur has 2 atoms bonded (the H) and 2 pairs of electrons, which is a total of 4 electron domains. The hybridization of the sulfur therefore is sp3
the sulfur has 2 atoms bonded (the H) and 2 pairs of electrons, which is a total of 4 electron domains. The hybridization of the sulfur therefore is sp3
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What is the molecular shape of the following molecule?
SF6
What is the molecular shape of the following molecule?
SF6
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when a central atom of a molecule has 6 electron domains coming off of it (none of which are lone pairs of electrons), it is considered octahedral
when a central atom of a molecule has 6 electron domains coming off of it (none of which are lone pairs of electrons), it is considered octahedral
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Based upon the above image, what type of packing is this?
Based upon the above image, what type of packing is this?
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The figure above represents ABABA packing which is hexagonal close packing.
The figure above represents ABABA packing which is hexagonal close packing.
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Put the following in order from greatest to least intermolecular forces:
I. H2O
II. LiOH
III. CO2
Put the following in order from greatest to least intermolecular forces:
I. H2O
II. LiOH
III. CO2
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LiOH displays ion-dipole IMF, H2O displays hydrogen bonding, and CO2 displays dipole-dipole. Ion-dipole is greater than hydrogen bonding as an IMf, and hydrogen bonding is greater than dipole-dipole.
LiOH displays ion-dipole IMF, H2O displays hydrogen bonding, and CO2 displays dipole-dipole. Ion-dipole is greater than hydrogen bonding as an IMf, and hydrogen bonding is greater than dipole-dipole.
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How many yellow spheres and green spheres are there per unit cell shown?
How many yellow spheres and green spheres are there per unit cell shown?
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For a unit cell, the corners count as 1/8 of a sphere and atoms completely within the unit cell count as 1. This gives us 1 yellow and 1 green sphere in the unit cell shown above.
For a unit cell, the corners count as 1/8 of a sphere and atoms completely within the unit cell count as 1. This gives us 1 yellow and 1 green sphere in the unit cell shown above.
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Based upon the above image, what type of packing is this?
Based upon the above image, what type of packing is this?
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The figure above represents ABCABC packing which is cubic close packing.
The figure above represents ABCABC packing which is cubic close packing.
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Which of the following compounds contains the most π bonds?
Which of the following compounds contains the most π bonds?
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π bonds occur when there is greater than a single bond (double or triple bond). The only compound listed with double bonds or greater is CO2, meaning it is the one that contains the most π bonds.
π bonds occur when there is greater than a single bond (double or triple bond). The only compound listed with double bonds or greater is CO2, meaning it is the one that contains the most π bonds.
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Zinc Sulfide can be described as a cubic close packed arrangement of Zn with sulfur occupying one-half of the tetrahedral holes. Based upon that description and the figure above, what is the formula for zinc sulfide?
Zinc Sulfide can be described as a cubic close packed arrangement of Zn with sulfur occupying one-half of the tetrahedral holes. Based upon that description and the figure above, what is the formula for zinc sulfide?
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The figure above has 8 Zn atoms on the corners (counting as 1/8) and 6 Zn atoms on the faces (counting as ½). This gives 4 Zn atoms in the unit cell. The Sulfur atoms are completely within the unit cell and count as 1 each for a total of 4 S atoms. This gives the formula Zn4S4 which reduces down to ZnS.
The figure above has 8 Zn atoms on the corners (counting as 1/8) and 6 Zn atoms on the faces (counting as ½). This gives 4 Zn atoms in the unit cell. The Sulfur atoms are completely within the unit cell and count as 1 each for a total of 4 S atoms. This gives the formula Zn4S4 which reduces down to ZnS.
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What are the names of the alloy types shown in the figure above:
What are the names of the alloy types shown in the figure above:
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An interstitial alloy has a smaller atom inserted into the unit cell, a substitutional alloy has another atom substitute for the main element, and a pure metal is only composed of a single atom type.
An interstitial alloy has a smaller atom inserted into the unit cell, a substitutional alloy has another atom substitute for the main element, and a pure metal is only composed of a single atom type.
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What is the strongest intermolecular force in the following compound?
CH3CH2CH2CH2OH
What is the strongest intermolecular force in the following compound?
CH3CH2CH2CH2OH
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This is butanol. It is an alcohol; OH is the prime example of hydrogen bonding, which is the strongest intermolecular force.
This is butanol. It is an alcohol; OH is the prime example of hydrogen bonding, which is the strongest intermolecular force.
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Which of the following has the highest boiling point?
Which of the following has the highest boiling point?
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Ionic bonds are the strongest type of bonds, followed by covalent bonds, hydrogen bonds, and lastly, van Der waals forces.
Ionic bonds are the strongest type of bonds, followed by covalent bonds, hydrogen bonds, and lastly, van Der waals forces.
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Which of the following intermolecular forces is the strongest?
Which of the following intermolecular forces is the strongest?
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Ion-dipole forces are the strongest of the intermolecular forces.
Hydrogen bonding is a specific term for a particularly strong dipole-dipole interaction between a hydrogen atom and a very electronegative atom (oxygen, fluorine, or nitrogen). However, hydrogen bonds are still not as strong as ion-dipole interactions.
In order from strongest to weakest, the intermolecular forces given in the answer choices are: ion-dipole, hydrogen bonding, dipole-dipole, and Van der Waals forces.
Ionic bonding is stronger than any of the given intermolecular forces, but is itself NOT an intermolecular force. Ionic bonds are a permanent chemical connection between two atoms, whereas intermolecular forces as a more transient and temporary attraction between independent molecules.
Ion-dipole forces are the strongest of the intermolecular forces.
Hydrogen bonding is a specific term for a particularly strong dipole-dipole interaction between a hydrogen atom and a very electronegative atom (oxygen, fluorine, or nitrogen). However, hydrogen bonds are still not as strong as ion-dipole interactions.
In order from strongest to weakest, the intermolecular forces given in the answer choices are: ion-dipole, hydrogen bonding, dipole-dipole, and Van der Waals forces.
Ionic bonding is stronger than any of the given intermolecular forces, but is itself NOT an intermolecular force. Ionic bonds are a permanent chemical connection between two atoms, whereas intermolecular forces as a more transient and temporary attraction between independent molecules.
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Which of the following is the strongest intermolecular force?
Which of the following is the strongest intermolecular force?
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Ionic and covalent bonds are not intermolecular forces;
Ion-dipole>hydrogen bonds>dipole-dipole>van Der Waals forces
Ionic and covalent bonds are not intermolecular forces;
Ion-dipole>hydrogen bonds>dipole-dipole>van Der Waals forces
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Which of the following compounds experiences the greatest intermolecular forces
Which of the following compounds experiences the greatest intermolecular forces
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IMF strength is in the order of ion-ion>h-bond>dipole-dipole>van der waals. Of the listed compounds there aren't any that display ion-ion IMF, and only ammonia has h-bonding, making it the one with the strongest forces.
IMF strength is in the order of ion-ion>h-bond>dipole-dipole>van der waals. Of the listed compounds there aren't any that display ion-ion IMF, and only ammonia has h-bonding, making it the one with the strongest forces.
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Order the following compounds from lowest boiling point to highest:
He2 (helium gas)
Isobutyl alcohol
Acetone
Water
Order the following compounds from lowest boiling point to highest:
He2 (helium gas)
Isobutyl alcohol
Acetone
Water
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Helium gas will have the lowest boiling point since it is a noble gas and the only intermolecular forces present are dispersion forces, which are the weakest. Acetone has a dipole, so dipole-dipole forces will be present. Water has a dipole and can also hydrogen bond, as can isobutyl alcohol. However, isobutyl alcohol is heavier than water, and will thus have the highest boiling point.
Helium gas will have the lowest boiling point since it is a noble gas and the only intermolecular forces present are dispersion forces, which are the weakest. Acetone has a dipole, so dipole-dipole forces will be present. Water has a dipole and can also hydrogen bond, as can isobutyl alcohol. However, isobutyl alcohol is heavier than water, and will thus have the highest boiling point.
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