What type(s) of intermolecular forces exist between two molecules of 1-pentanol? (BLB Ch. 11)

Answers

Answer 1

Answer:

Answer:

Hydrogen bonding

London dispersion forces

Explanation:

The most pronounced and consequential intermolecular forces at play has to be hydrogen bonding due to the dipole created between the oxygen and hydrogen in the hydroxyl group. And then to a lesser extent there are very weak London dispersion forces that are always going to be there in between any two molecules of any species.

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How much heat is transferred when 7.19 grams of H2 reacts with excess nitrogen, according to the following equation: N2(g) + 3 H2 (g) --> 2 NH3 (g) \DeltaΔH = +46.2 kJ

What is the change in electrons for nitrogen in the following reaction?S + NO3 - -> SO2 + NO

A. Gain 2 electrons
B. Gain 3 electrons
C. Lose 2 electrons
D. Lose 3 electrons

Answers

Nitrogen changes from +5 in $NO_3$ - to +2 in NO. This means nitrogen has gained 3 electrons. Option B

To determine the change in electrons for nitrogen in the given reaction, we need to compare the oxidation state of nitrogen in the reactant ( $NO_3$ -) and the product (NO).

In the reactant, -, nitrogen is in the +5 oxidation state. This is because oxygen has an oxidation state of -2, and there are three oxygen atoms in $NO_3$ -. Therefore, nitrogen must have an oxidation state of +5 to balance the overall charge of $NO_3$ -.

In the product, NO, nitrogen is in the +2 oxidation state. This is because oxygen has an oxidation state of -2, and there is only one oxygen atom in NO. Therefore, nitrogen must have an oxidation state of +2 to balance the overall charge of NO.

By comparing the oxidation states of nitrogen in the reactant and the product, we can determine the change in electrons. The change in oxidation state corresponds to the change in the number of electrons gained or lost by the nitrogen atom.

In this case, nitrogen changes from +5 in $NO_3$ - to +2 in NO. This means nitrogen has gained 3 electrons.

Therefore, the correct answer is B) Gain 3 electrons.

The nitrogen atom undergoes a reduction because it gains electrons, reducing its oxidation state from +5 to +2 in the reaction.

Option B

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Use molecular orbital theory to determine whether f22+ is paramagnetic or diamagnetic.

Answers

We have to know whether F₂²⁺ is paramagnetic or diamagnetic.

F₂²⁺ is paramagnetic.

If number of unpaired electron in any species is equal to zero, the species is diamagnetic and the species contains unpaired electrons, then the species is paramagnetic.

The magnetic property can be explained using molecular orbital theory.

Total number of electron present in F₂²⁺ is equal to 16 (i.e, 9+9-2). From the molecular orbital electronic configuration, number of electrons present in pi orbitals present is equal to 2.

So, F₂²⁺ is paramagnetic.

Answer : $F_2^(2+)$ is paramagnetic.

Explanation :

According to the molecular orbital theory, the general molecular orbital configuration will be,

$(\sigma_(1s)),(\sigma_(1s)^*),(\sigma_(2s)),(\sigma_(2s)^*),[(\pi_(2p_x))=(\pi_(2p_y))],(\sigma_(2p_z)),[(\pi_(2p_x)^*)=(\pi_(2p_y)^*)],(\sigma_(2p_z)^*)$

As there are 9 electrons present in fluorine.

The number of electrons present in $F_2^(2+)$ molecule = 2(9) - 2 = 16

The molecular orbital configuration of $F_2^(2+)$ molecule will be,

$(\sigma_(1s))^2,(\sigma_(1s)^*)^2,(\sigma_(2s))^2,(\sigma_(2s)^*)^2,(\sigma_(2p_z))^2,[(\pi_(2p_x))^2=(\pi_(2p_y))^2],[(\pi_(2p_x)^*)^1=(\pi_(2p_y)^*)^1],(\sigma_(2p_z)^*)^0$

Paramagnetic compounds : They have unpaired electrons.

Diamagnetic compounds : They have no unpaired electrons that means all are paired.

The number of unpaired electron in molecule is, 2. So, this is paramagnetic. That means, more the number of unpaired electrons, more paramagnetic.

Thus, is paramagnetic.

Which of the following Ph levels would indicate the weakest base?15

8

6

2

Answers

Answer:

Explanation:

7 is neutral any anything above it is basic and anything below is acidic which means 8 would be the lowest base

Answer:

The pH of a weak base falls somewhere between 7 and 10.

Explanation:

Like weak acids, weak bases do not undergo complete dissociation; instead, their ionization is a two-way reaction with a definite equilibrium point

Classify each type of matter as an element, a compound, a heterogeneous mixture, or a homogeneous mixture. drag each item to the appropriate bin. sugar air hot tea salt water

Answers

Answer :

Sugar : Compound

Air : Homogeneous mixture

Hot tea : Homogeneous mixture

Salt water : Homogeneous mixture

Explanation :

Element : It is a pure substance which is composed of atoms of similar elements.

Compound : It is a pure substance which is made from atoms of different elements combined together in a fixed ratio by mass.

Heterogeneous mixtures : It is a mixture that has non-uniform composition throughout the solution and the particle size or shapes are also different.

There is a physical boundary between the dispersed phase and dispersion medium.

Homogeneous mixtures : It is a mixture that has uniform composition throughout the solution and the particle size or shapes are not different.

There is no physical boundary between the dispersed phase and dispersion medium.

As per question,

Sugar : It is a compound that is made from atoms of different elements combined together in a fixed ratio by mass.

Air : It is a homogeneous mixture of the gaseous substances of nitrogen, oxygen, and smaller amounts of other substances.

Hot tea : It is a homogeneous mixture because its composition is the same throughout the solution.

Salt water : It is a homogeneous mixture because its composition is the same throughout the solution.

Sugar compound

Air Homogeneous mixture

Hot tea Homogeneous mixture

Salt water Homogeneous mixture

Element:

An element is a simplest type of a pure substance which is composed of only one type of matter. For examples; silver, gold platinum etc.

Pure substance:

A compound is a pure substance which is composed of two or more type of matter in definite proportion. For examples; water which is composed by Hydrogen and oxygen etc.

Mixture:

A mixture is made from two or more type of matter in any proportion. Mixture are generally two types:

1. Homogeneous mixture

This is also known as solution, in which the composition of the substances is uniform.

Lemon-flavored water is an example of homogeneous mixture because in this the composition of the substances is uniform.

2. Heterogeneous mixture

In this form of mixture the composition of substance are not uniform and the component of mixture also visible.

Stuffed mushrooms is an example of Heterogeneous mixture because in this form of mixture the composition of substance are not uniform and the component of mixture also visible.

What is the isoelectric point of proteins?

Answers

Isoelectric point. The isoelectric point (pI, pH(I), IEP), is the pH at which a particular molecule carries no net electrical charge in the statistical mean. The standard nomenclature to represent the isoelectric point is pH(I), although pI is also commonly seen, and is used in this article for brevity.

The isoelectric point (pI, pH(I),IEP), is the pH at which a particular molecule carries no net electrical charge in the statistical mean.

A 3.0 L flask containing helium at 145 mmHg is connected by a closed valve to a 2.0 L flask containing argon at 355 mmHg. When the valve is opened and the gases are allowed to mix equally in the two flasks, what is the total pressure (in mmHg) in the two connected flasks after mixing ?

Answers

Answer:

Assuming that both helium and argon act like ideal gases, the total pressure after mixing would be approximately $229\; \rm mmHg$ .

Explanation:

By the ideal gas equation, $P\cdot V = n \cdot R \cdot T$ , where

$P$ is the pressure of the sample.
$V$ is the volume of the container.

$n$ is the number of moles of gas particles in the sample.
$R$ is the ideal gas constant.
$T$ is the temperature of the sample.

Rewrite to obtain:

$\displaystyle n = (P \cdot V)/(R\cdot T)$ , and
$\displaystyle P = (n \cdot R \cdot T)/(V)$ .

Assume that the two samples have the same temperature, $T$ . Also, assume that mixing the two gases did not affect the temperature.

Apply the equation $\displaystyle n = (P \cdot V)/(R\cdot T)$ to find the number of moles of gas particles in each container:

In the helium container, $V = 3.0\; \rm L$ and $P = \rm 145\; mmHg$ . Hence, $\displaystyle n_1 = (P\cdot V)/(R \cdot T) = \frac{(3.0\; \text{L}) \cdot (145\; \text{mmHg})}{R\cdot T}$ .
In the argon container, $V = 2.0\; \rm L$ and $P = 355\; \rm mmHg$ . Hence, $\displaystyle n_2 = (P\cdot V)/(R \cdot T) = \frac{(2.0\; \text{L}) \cdot (355\; \text{mmHg})}{R\cdot T}$ .

After mixing, $V = 2.0 + 3.0 = 5.0\; \rm L$ . Assuming that temperature $T$ stays the same.

$\displaystyle n_1 + n_2 = \frac{(3.0\; \text{L}) \cdot (145\; \text{mmHg})}{R\cdot T} + \frac{(2.0\; \text{L}) \cdot (355\; \text{mmHg})}{R\cdot T}$ .

Apply the equation $\displaystyle P = (n \cdot R \cdot T)/(V)$ to find the pressure after mixing.

$\begin{aligned}P &= \displaystyle \frac{\displaystyle \displaystyle \left(\frac{(3.0\; \text{L}) \cdot (145\; \text{mmHg})}{R\cdot T} + \frac{(2.0\; \text{L}) \cdot (355\; \text{mmHg})}{R\cdot T}\right) \cdot R \cdot T}{5.0\; \rm L} \n &= (3.0\; \rm L * 145\; \rm mmHg + 2.0\; \rm L * 355\; \rm mmHg)/(5.0\; \rm L) \n &\approx 229\; \rm mmHg\end{aligned}$ .