The weakest force of molecular attraction is dispersion.
(Option B)
The dispersion force is also known as London dispersion forces is a weak intermolecular force.
These dispersion forces arise due to temporary fluctuations in electron distribution within molecules, creating temporary dipoles.
These temporary dipoles induce similar dipoles in neighboring molecules, resulting in attractive forces between them.
Dispersion forces are present in all molecules, regardless of their polarity or the presence of other types of bonds or interactions.
However, they tend to be weaker compared to other intermolecular forces, such as dipole-dipole interactions and hydrogen bonds.
Learn more about Dispersion forces here: brainly.com/question/1454795
#SPJ6
b. dispersion
Definition of Dispersion by Mimiwhatsup: a mixture in which fine particles of one kind of substance is scattered throughout another substance.
(B) False
Isopropyl methyl ether is slightly soluble in water because the oxygen atom of ethers with 3 or lesser carbon atoms can form hydrogen bonds with water. Therefore, the given statement is true.
Hydrogen bonding is a special class of attractive intermolecular forces that arise because of the dipole-dipole interaction between hydrogen that is bonded to a highly electronegative atom and another highly electronegative atom that lies in the neighborhood of the hydrogen atom.
For example, in water, hydrogen is covalently bonded to the oxygen atom. Therefore, hydrogen bonding arises because of the dipole-dipole interactions between the hydrogen atom of one water molecule and the oxygen atom of another water molecule.
The solubility of ether in water depends upon the extent of the formation of hydrogen bonds with water. Ether which contains three carbon atoms is soluble in water due to these lower hydrocarbon atoms can form hydrogen bonding with water.
But the solubility of hydrocarbons or ethers decreases as increase the number of carbon atoms. This is because higher ethers or ethers with more carbons have more hydrophobic parts. Therefore they cannot be soluble in water as they cannot form hydrogen bonds with water molecules.
Learn more about hydrogen bonding, here:
#SPJ2
Answer:
True
Hydrogen bond is a partial intermolecular bonding interaction between a lone pair on an electron rich donor atom, particularly the second-row elements nitrogen (N), oxygen (O), or fluorine (F), and the antibonding orbital of a bond between hydrogen (H) and a more
electronegative atom or group. Such an interacting system is generally denoted Dn–H···Ac, where the solid line denotes a polar covalent bond, and the dotted or dashed line indicates the hydrogen bond. The use of three centered dots for the hydrogen bond is specifically recommended by the IUPAC. While hydrogen bonding has both covalence and electrostatic contributions, and the degrees to which they contribute are currently debated, the present evidence strongly implies that the primary contribution is covelant.
Hydrogen bonds can be intermolecular (occurring between separate molecules) or
intramolecular (occurring among parts of the same molecule)
water, air, oil
B
air, water, oil
C
oil, water, air
D
none of the above
b. 50.00 mL
c. 75.00 mL
d. 100.00 mL
e. 25.00 mL
Answer:
We need 75 mL of 0.1 M NaOH ( Option C)
Explanation:
Step 1: Data given
Molarity of NaOH solution = 0.100 M
volume of 0.150 M CH3COOH = 50.00 mL = 0.05 L
Step 2: The balanced equation
CH3COOH + NaOH → CH3COONa + H2O
Step 3: Calculate moles of CH3COOH
Moles CH3COOH = Molarity * volume
Moles CH3COOH = 0.150 M * 0.05 L
Moles CH3COOH = 0.0075 moles
Step 4: Calculate moles of NaOH
For 1 mol of CH3COOH we need 1 mol of NaOH
For 0.0075 mol CH3COOH we need 0.0075 mole of NaOH
Step 5: Calculate volume of NaOH
volume = moles / molarity
volume = 0.0075 moles / 0.100 M
Volume = 0.075 L = 75 mL
We need 75 mL of 0.1 M NaOH
0.0340 g O2
Step 1. Write the balanced chemical equation
4Fe(OH)^(+) + 4OH^(-) + O2 + 2H2O → 4Fe(OH)3
Step 2. Calculate the moles of Fe^(2+)
Moles of Fe^(2+) = 50.0 mL Fe^(2+) × [0.0850 mmol Fe^(2+)/1 mL Fe^(2+)]
= 4.250 mmol Fe^(2+)
Step 3. Calculate the moles of O2
Moles of O2 = 4.250 mmol Fe^(2+) × [1 mmol O2/4 mmol Fe^(2+)]
= 1.062 mmol O2
Step 4. Calculate the mass of O2
Mass of O2 = 1.062 mmol O2 × (32.00 mg O2/1 mmol O2) = 34.0 mg O2
= 0.0340 g O2
0.0342 grams of O2 are consumed to precipitate all of the iron in 50.0 mL of 0.0850 M Fe(II) solution.
To solve this problem, we need to first calculate the number of moles of Fe(II) in 50.0 mL of 0.0850 M Fe(II) solution.
Moles of Fe(II) = (0.0850 mol/L) * (50.0 mL) = 0.00425 mol
According to the balanced chemical equation, 4 moles of Fe(II) react with 1 mole of O2. Therefore, the number of moles of O2 required to precipitate all of the iron in 50.0 mL of 0.0850 M Fe(II) solution is:
Moles of O2 = (0.00425 mol Fe(II)) * (1 mol O2 / 4 mol Fe(II)) = 0.00106 mol O2
Now we can convert the moles of O2 to grams using the molar mass of O2 (32.00 g/mol):
Grams of O2 = (0.00106 mol O2) * (32.00 g/mol) = 0.0342 g O2
Therefore, 0.0342 grams of O2 are consumed to precipitate all of the iron in 50.0 mL of 0.0850 M Fe(II) solution.
Learn more about precipitate the iron here:
#SPJ6
Yes, because conservation of mass
Answer:
See explanation below.
Explanation:
Both carbon and silicon are members of group 4A(now group 14) i n the periodic table. Carbon is the first member of the group. CO2 is a gas while SiO2 is a solid. In SiO2, there are single bonds between silicon and oxygen and the geometry around the central atom is tetrahedral while in CO2, there are double carbon-oxygen bonds and the geometry around the central atom is linear. CO2 molecules are discrete and contain only weak vanderwaals forces.
Again, silicon bonds to oxygen via its 3p orbital while carbon bonds to oxygen via a 2p orbital. As a result of this, there will be less overlap between the pi orbitals of silicon and that of oxygen. This is why tetrahedral bonds are formed with oxygen leading to a covalent network solid rather than the formation of a silicon-oxygen pi bond. A covalent network solid is known to be made up of a network of atoms of the same or different elements connected to each other continuously throughout the structure by covalent bonds.
In SiO2, each silicon atom is surrounded by four oxygen atoms. Each corner is shared with another tetrahedron. SiO2 forms an infinite three dimensional structure and melts at a very high temperature.
Carbon and oxygen form a molecular compound CO2 with weaker covalent bonds, while silicon and oxygen form a covalent network solid SiO2 with stronger, three-dimensional covalent bonds.
The difference in bonding between carbon and oxygen compared to silicon and oxygen is due to the different nature of their chemical bonds. In the case of carbon and oxygen, they form a molecular compound CO2, where carbon and oxygen atoms share electrons to form covalent bonds. This is because carbon and oxygen have similar electronegativities, so they can share electrons equally. The covalent bonds in CO2 are relatively weak, allowing the compound to exist as a gas at room temperature and pressure.
On the other hand, silicon and oxygen form a covalent network solid with the formula unit SiO2, known as quartz. In this case, silicon and oxygen atoms are covalently bonded in a three-dimensional network structure, where each silicon atom is bonded to four oxygen atoms and each oxygen atom is bonded to two silicon atoms. This network structure gives SiO2 its high melting point and hardness, making it a solid at room temperature and pressure.
In summary, the difference in bonding between carbon and oxygen compared to silicon and oxygen is that carbon and oxygen form a molecular compound with weaker covalent bonds, while silicon and oxygen form a covalent network solid with stronger, three-dimensional covalent bonds.
#SPJ3