Answer: The compound in medicines should be non polar.
It is important for any drug to be able to dissolve itself through the cell membrane which consists of a lipid bi-layer, in order to diffuse in the body and circulate biologically, performing its function.
Non polar compounds are lipid soluble and therefore can dissolve in the lipid layers.
Polar compounds are water soluble and fail to cross the cell membrane.
Therefore scientists need to be sure of using compounds that are non polar in nature so they pass through the cell membrane and enter into the blood circulation of the body and perform its due function.
Explanation:
Explanation:
To delineate the the nature of the bonds that would be formed between the two elements, let us first write the electronic configuration of the two species;
Be = 2, 2
F = 2, 7
Beryllium is a metal with two valence electrons whereas fluorine is a halogen with seven valence electrons.
When Be loses two electrons it becomes isoelectronic with He;
Be → Be²⁺ + 2e⁻
Also, when fluorine gains an electron, it becomes isoelectronic with Ne;
F + e⁻ → F⁻
This loss and gain of electrons between the two elements creates an electrostatic attraction them and they enter into an electrovalent bond.
Hence;
Be²⁺ + 2F⁻ → BeF₂
Answer:
Fluorine
Explanation:
Fluorine has 9 total electrons. The first two are in the 1s level, and the remaining electrons are on the outer level of the atom, with 2 in the s level and 5 in the p level. The electron configuration is 1s2 2s2 2p5.
Answer:
For N₂F₂:
Molar fraction = 0.84
Partial pressure = 1.12 atm
For SF₄:
Molar fraction = 0.16
Partial pressure = 0.208 atm
Explanation:
It seems your question is missing the values required to solve the problem. However, an internet search showed me the following values for your question. If the values in your problem are different, your answer will be different as well, however the solving method will remain the same:
" A 5.00L tank at 0.7°C is filled with 16.5g of dinitrogen difluoride gas and 5.00g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. "
First we calculate the moles of each gas, using their molar mass:
- 16.5 g N₂F₂ ÷ 66 g/mol = 0.25 mol N₂F₂
- 5.00 g SF₄ ÷ 108 g/mol = 0.0463 mol SF₄
Total mol number = 0.25 + 0.0463 = 0.2963 mol
- Mole Fraction N₂F₂ = 0.25/0.2963 = 0.84
- Mole Fraction SF₄ = 0.0463/0.2963 = 0.16
Now we <u>use PV=nRT to calculate the partial pressure of each gas</u>:
P = ?
V = 5.00 L
T = 0.7 °C ⇒ 0.7 + 273.16 = 273.86 K
For N₂F₂:
- P * 5.00 L = 0.25 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 273.86 K
For SF₄:
- P * 5.00 L = 0.0463 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 273.86 K
Answer:
Option A is your answer
Explanation:
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