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3 years ago

What are the covalent bonds that form between atoms of different electronegativities called?

2 answers:

6 0

The covalent bonds that form between atoms of different electronegativities called polar bonds. Just like in water. The cause of polarity in water molecules is because of the high electronegativity difference between oxygen and hydrogen.

Montano1993 [528]3 years ago

5 0

Answer: c. polar bonds

Explanation:

A polar covalent bond is defined as the bond which is formed when there is a difference of electronegativities between the atoms. It is also defined as the bond which is formed due to the unequal sharing of electrons between the atoms.

Ionic bond is formed when there is complete transfer of electron from one atom to another atom.

Non-polar covalent bond is defined as the bond which is formed when there is no difference of electronegativities between the atoms. It is also defined as the bond which is formed due to the equal sharing of electrons between the atoms.

Hence, the correct answer is polar bonds.

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A 280 mL bubble contains 0.283 g of a gas at 0.951 atm and 25.0°C What is the molar mass of this gas?

tekilochka [14]

Answer: 28.3 g/mol

Explanation:

According to the ideal gas equation:'

$PV=nRT$

P= Pressure of the gas = 0.951 atm

V= Volume of the gas = 280 mL = 0.28 L (1L=1000 ml)

T= Temperature of the gas = 25°C=(25+273)K=298 K (0°C = 273 K)

R= Value of gas constant = 0.0821 Latm/K mol

$n=\frac{PV}{RT}=\frac{0.951\times 0.28L}{0.0821 \times 298}=0.010moles$

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

$0.010=\frac{0.283}{\text {Molar mass}}$

${\text {Molar mass}}=28.3g/mol$

Thus the molar mass of the gas is 28.3 g/mol.

7 0

3 years ago

Which of the following does NOT show the law of conservation of mass?

algol [13]

I think the correct answer from the choices listed above is option B. 24 mL of Mg burn in 32 mL O2 to produce 56 mL of MgO does not show the law of conservation of mass. Volumes cannot be added because there are volume effects when you add different substances. So, the reactants is not equal to the product.

4 0

4 years ago

Read 2 more answers

A 5.098 mass % aqueous solution of potassium hydroxide has a density of 1.05 g/mL. Calculate the molality of the solution. Give

GarryVolchara [31]

Answer: The molarity of solution is 0.954 M

Explanation:

We are given:

5.098 mass % solution of potassium hydroxide

This means that 5.098 grams of potassium hydroxide is present in 100 grams of solution

To calculate volume of a substance, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Density of solution = 1.05 g/mL

Mass of solution = 100 g

Putting values in above equation, we get:

$1.05g/mL=\frac{100g}{\text{Volume of solution}}\\\\\text{Volume of solution}=\frac{100g}{1.05g/mL}=95.24mL$

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

Given mass of potassium hydroxide = 5.098 g

Molar mass of potassium hydroxide = 56.1 g/mol

Volume of solution = 95.24 mL

Putting values in above equation, we get:

$\text{Molarity of solution}=\frac{5.098\times 1000}{56.1\times 95.24}\\\\\text{Molarity of solution}=0.954M$

Hence, the molarity of solution is 0.954 M

7 0

4 years ago

If you had 15 moles of Oxygen (O2), how many moles of water (H2O) would you be able to make?

larisa [96]

Answer:

30 moles of water will produced.

Explanation:

Given data:

Number of moles of O₂ react = 15 mol

Number of moles of water formed = ?

Solution:

Chemical equation:

2H₂ + O₂ → 2H₂O

Now we will compare the moles of water with oxygen.

O₂ : H₂O

1 : 2

15 : 2×15 = 30 mol

30 moles of water will produced.

5 0

3 years ago

Which household items would be considered a base? Select all that apply. *

mrs_skeptik [129]

Answer:

Drain Cleaner, soap, bleach

i think thats it, sorry if i got something wrong

6 0

3 years ago