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3 years ago

How does bonding help achieve chemical stability

Chemistry

2 answers:

lys-0071 [83]3 years ago

5 0

Answer: By fulfilling octet of the outermost valence shell.

Explanation: Chemical bonding is the attraction between the atoms , ions or molecule that helps in the formation of the chemical compound.

The bond between the two species can be formed either by sharing of valence shell electrons or by donating electron of the valence shell of one specie to the other.

When the formation of the bond takes place, it will try to complete the octet of the species that are involved in the bond making. This completion of the octet provide stability to the compound .

almond37 [142]3 years ago

3 0

If the outer shell is filled, the atom is stable. Atoms with unfilled outer shells are unstable, and will usually form chemical bonds with other atoms to achieve stability. Example of an unstable atom with a single electron in its outer-most shell. ... In covalent bonds, atoms share electrons to achieve stability.

Hope this helped!

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It is necessary to have a 40% antifreeze solution in the radiator of a certain car. the radiator now has 70 liters of 20% soluti

Akimi4 [234]

The answer is : 17.5 liters drained and replaced by 17.5 liters of 100% solution.
x = amount drained and replaced
(70-x) = remaining amount of 20% solution
.20(70-x) + 1.00(x) = .40(70)
14 - .2x + 1x = 28
1x - .2x = 28 - 14
.8x = 14
x = 14/.8
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Fittoniya [83]

Answer:

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2 years ago

A 1.52 g sample of KCIO3 is reacted according to the balanced equation below. How many liters of O2 is produced at a pressure of

ipn [44]

Answer:

0.486 L

Explanation:

Step 1: Write the balanced reaction

2 KCIO₃(s) ⇒ 2 KCI (s) + 3 O₂(g)

Step 2: Calculate the moles corresponding to 1.52 g of KCIO₃

The molar mass of KCIO₃ is 122.55 g/mol.

1.52 g × 1 mol/122.55 g = 0.0124 mol

Step 3: Calculate the moles of O₂ produced from 0.0124 moles of KCIO₃

The molar ratio of KCIO₃ to O₂ is 2:3. The moles of O₂ produced are 3/2 × 0.0124 mol = 0.0186 mol

Step 4: Calculate the volume corresponding to 0.0186 moles of O₂

0.0186 moles of O₂ are at 37 °C (310 K) and 0.974 atm. We can calculate the volume of oxygen using the ideal gas equation.

P × V = n × R × T

V = n × R × T/P

V = 0.0186 mol × (0.0821 atm.L/mol.K) × 310 K/0.974 atm = 0.486 L

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lukranit [14]

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Paul [167]

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To know more about monosaccharides and disaccharides:

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