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3 years ago

Correct electron configuration for Boron

Chemistry

1 answer:

Alinara [238K]3 years ago

8 0

<span>[He] 2s2 2p1 is your answer</span>

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identify the law that explains the following observation nitrogen dioxide can be formed by reacting 14 G of nitrogen with 32 gra

Mrrafil [7]

Answer:

The law of definite proportions. I had the same question for chemistry and this is what they said was right so I got 100%.

Explanation:

8 0

3 years ago

What is the osmotic pressure of a solution made from 22.3 g of methanol (MM = 32.04 g/mol) that was added to water to make 321 m

xxMikexx [17]

Answer: The osmotic pressure of a solution is 53.05 atm

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

Or,

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

where,

$\pi$ = osmotic pressure of the solution = ?

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (methanol) = 22.3 g

Volume of solution = 321 mL

R = Gas constant = $0.0821\text{ L.atm }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$\pi=1\times \frac{22.3\times 1000}{32.04\times 321}\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 298K$

$\pi=53.05atm$

Hence, the osmotic pressure of a solution is 53.05 atm

7 0

3 years ago

Which compound is bonded covalently? A.KF B.MgS C.BeO D.SO2

Masja [62]

Answer:

SO2 is bonded covalently

Explanation:

Atoms that share electrons in a chemical bond have covalent bonds.

6 0

3 years ago

What is the empirical formula for a compound if a sample contains 1. 0 g of S and 1. 5 g of O? SO SO3 S2O2 S2O3.

Tcecarenko [31]

The empirical formula of the given compound is $\bold{SO_3}$ .

The correct option is B.

<h3>What is an empirical formula?</h3>

The empirical formula of a chemical compound is the simplest whole-number ratio of atoms contained in the substance.

Given,

1.0 g of S

1.5 g of O

To calculate the empirical formula, we will divide the masses of the elements by their atomic weight.

For sulfur

$\bold{\dfrac{1.0}{32} =0.03125\; mol}$

For oxygen

$\bold{\dfrac{1.5}{16} =0.09375\; mol}$

Now, divide the greater value of mole came by the smaller value

$\bold{\dfrac{0.09375\; mol}{0.03125\;mol} = 3}$

Thus, the empirical formula for the given compound is 1 for S and 3 for O

$\bold{SO_3}$

Learn more about empirical formula, here:

brainly.com/question/11588623

7 0

3 years ago

A neutral atom becomes a negatively charged ion by __________ electrons

Inessa [10]

A neutral atom becomes a negatively charged ion by accepting electrons.
For example:
F + e⁻ → F⁻
S + 2e⁻ →S²⁻

8 0

4 years ago