What type of orbital is designated by the quantum numbers n = 3, l = 0 ?

Answers

Answer 1

Answer:

Answer:

The quantum numbers n = 3 and l = 0 correspond to a specific type of orbital within the third principal energy level (n = 3) of an atom.

When l = 0, it corresponds to the s orbital. So, the orbital designated by the quantum numbers n = 3, l = 0 is the 3s orbital. The 3s orbital is spherically symmetrical and has a single orientation within its energy level.

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Bromine, a liquid at room temperature, has a boiling point of 58°C and a melting point of –7.2°C. Bromine can be classified as acompound. impure substance. mixture. pure substance.

Which is a characteristic of mixtures? They are chemically bonded together. They can be classified as pure substances. They have fixed ratios between their components. They can be separated by physical processes.

Answers

the answer is d i just took the quiz

The statement "They can be separated by physical processes" is a characteristic of mixtures (option D)

What are mixtures?

Mixtures are physical combinations of two or more substances. The components of a mixture are not chemically bonded together, and they can be separated by physical processes such as filtration, distillation, and evaporation.

Pure substances, on the other hand, are made up of only one type of atom or molecule. They cannot be separated by physical processes.

Therefore, the correct answer is They can be separated by physical processes (option D)

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Which substance, when dissolved in water, forms a solution that conducts an electric current?(1) C2H5OH (3) C12H22O11
(2) C6H12O6 (4) CH3COOH

Answers

Answer: Option (4) is the correct answer.

Explanation:

Substance which are able to conduct electricity are ionic in nature. This means that only ionic substances can conduct electricity because they dissociate into ions.

Therefore, out of the given options only acetic acid $(CH_(3)COOH)$ is ionic in nature.

$CH_(3)COOH \rightleftharpoons CH_(3)COO^(-) + H^(+)$

Though $CH_(3)COOH$ is a weak acid but it does dissociate into ions and hence, it forms a solution that conducts an electric current.

Consider the solutions, 0.04 m urea [(NH2)2C=O)], 0.04 m AgNO3 and 0.04 m CaCl2. Which has (i) the highest osmotic pressure, (ii) the lowest vapor pressure, (iii) the highest boiling point?

Answers

Answer:

i) Highest osmotic pressure: CaCl2

ii) lower vapor pressure : CaCl2

iii) highest boiling point : CaCl2

Explanation:

The colligative properties depend upon the number of solute particles in a solution.

The following four are the colligative properties:

a) osmotic pressure : more the concentration of the solute, more the osmotic pressure

b) vapor pressure: more the concentration of the solute, lesser the vapor pressure.

c) elevation in boiling point: more the concentration of the solute, more the boiling point.

d) depression in freezing point: more the concentration of the solute, lesser the freezing point.

the number of particle produced by urea = 1

the number of particle produced by AgNO3 = 2

the number of particle produced by CaCl2 = 3

As concentrations are same, CaCl2 will have more number of solute particles and urea will have least

i) Highest osmotic pressure: CaCl2

ii) lower vapor pressure : CaCl2

iii) highest boiling point : CaCl2

Final answer:

The solution with the highest number of particles in solution (CaCl2 in this case), experiences the highest osmotic pressure, lowest vapor pressure and highest boiling point due to the principles of colligative properties.

Explanation:

The question pertains to the colligative properties of solutions, which would be governed by the number of particles in the solution. The solutions are 0.04 m urea [(NH2)2C=O)], 0.04 m AgNO3, and 0.04 m CaCl2. For (i) Highest osmotic pressure, the solution with the highest ion count would yield the highest osmotic pressure. CaCl2 dissociates into three ions (Ca²+, and 2 Cl¯), therefore, it would exhibit the highest osmotic pressure. For (ii) Lowest vapor pressure, this would coincide with the solution with the highest osmotic pressure, again making it CaCl2, due to the greatest decrease in vapor pressure. For (iii) the highest boiling point, this too would be CaCl2 for the reasons stated above. The presence of more particles in a solution interferes more with the evaporation process, requiring more energy (higher temperature) to achieve boiling.

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Which of the following statements is not correct?0.20 mole of O2 = 6.4 g
0.75 mole of H2CO3 = 47 g
3.42 moles CO = 95.8 g
4.1 moles Li2O = 94 g

Answers

Answer:

4.1 moles Li2O = 94 g (incorrect)

4.1 mole of Li2O = 122.6g(correct)

Explanation:

1. Molar mass of O2 = 32

0.2 mole of 32 = 0.2×32 = 6.4g (correct)

2. Molar mass of H2CO3 = 62.03

0.75 mole of 62.03 = 0.75×62.03 = 46.5g (47 is correct)

3. Molar mass of CO = 28

3.42 moles of 30 = 3.42×28 = 95.76 (95.8 is correct)

4. Molar mass of Li2O = 29.9

4.1 mole of Li2O = 4.1×29.9 = 122.59g (94g is incorrect)

Answer:

It's 4.1 moles Li2O = 94 g on Odyssey ware

A solution was prepared by dissolving 0.42 mol hexane into 500g CCl4. What is the change in freezing point of this solution? The Kf for CCl4 is 30.0oC/m. The freezing point of CCl4 is -22.92 °C.