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3 years ago

What is a possible quantum number set for an electron in the 2s orbital of a beryllium (Be) atom?

Chemistry

1 answer:

Artist 52 [7]3 years ago

7 0

Answer is: 2,0,0,±1/2.

1) n = 1. The principal quantum number (n) is one of four quantum numbers which are assigned to each electron in an atom to describe that electron's state.

2) l = 0. The azimuthal quantum number is a quantum number for an atomic orbital that determines its orbital angular momentum and describes the shape of the orbital.

3) ml = 0. Magnetic quantum number specify orientation of electrons in magnetic field and number of electron states (orbitals) in subshells.

Magnetic quantum number (ml) specifies the orientation in space of an orbital of a given energy and shape . Magnetic quantum number divides the subshell into individual orbitals which hold the electrons, there are 2l+1 orbitals in each subshell.

4) The spin quantum number, ms, is the spin of the electron; ms = +1/2 or -1/2.

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When solid Ni metal is put into an aqueous solution of Pb(NO3)2, solid Pb metal and a solution of Ni(NO3)2 result. Write the net

Sonja [21]

Answer:

$Pb^{2+}(aq)+Ni(s)\rightarrow Ni^{2+}(aq)+Pb(s)$

Explanation:

Hello there!

In this case, according to the given information, it turns out firstly necessary for us to write the complete molecular equation as shown below:

$Pb(NO_3)_2(aq)+Ni(s)\rightarrow Ni(NO_3)_2(aq)+Pb(s)$

Now, we can separate the nitrates in ions as they are aqueous to obtain:

$Pb^{2+}(aq)+2(NO_3)^-(aq)+Ni(s)\rightarrow Ni^{2+}(aq)+2(NO_3)^-(aq)+Pb(s)$

And then, we cancel out the nitrate ions as the spectator ones, for us to obtain the net ionic equation:

$Pb^{2+}(aq)+Ni(s)\rightarrow Ni^{2+}(aq)+Pb(s)$

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6 0

3 years ago

How many grams of iron are needed to react with 3.00 g of sulfur?

Wewaii [24]

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7 0

3 years ago

What did the photoelectric experiment demonstrate?

arlik [135]

Explanation:

When an electromagnetic wave like light hits a material, the electrons gets emitted. The emission of electrons is called photoelectric effect. The emitted electrons are called photoelectrons. In this process the transfer of energy takes place from light to an electron.

Hence, the correct option regarding the photoelectric experiment is (A) " Light can cause electrons to be released from the surface of a metal."

4 0

4 years ago

A chemist prepares a solution of vanadium chloride by measuring out of into a volumetric flask and filling to the mark with dist

user100 [1]

The question is incomplete, the complete question is:

A chemist prepares a solution of vanadium (III) chloride (VCl3) by measuring out 0.40g of VCl3 into a 50.mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Cl− anions in the chemist's solution. Be sure your answer is rounded to the correct number of significant digits.

Answer:

0.153M of anions

Explanation:

First we calculate the concentration of the solution. From m/M= CV

m=given mass, M= molar mass, C =concentration of solution, V= volume of solution

Molar mass of compound= 51 + 3(35.5)= 157.5gmol-1

0.4g/157.5gmol-1= C×50/1000

C= 2.54×10-3/0.05= 0.051M

But 1 mole of VCl3 contains 3 moles of anions

Therefore, 0.051M will contain 3×0.051M of anions= 0.153M of anions

4 0

3 years ago

Read 2 more answers

Sulfur trioxide, SO3 , is produced in enormous quantities each year for use in the synthesis of sulfuric acid.

denis23 [38]

Answer:

3.14 L of oxygen (O₂).

Explanation:

We'll begin by calculating the number of mole in 6.3 g of sulphur (S). This can be obtained as follow:

Molar mass of S = 32 g/mol

Mass of S = 6.3 g

Mole of S =.?

Mole = mass / molar mass

Mole of S = 6.3/32

Mole of S = 0.197 mole

Next, we shall write the overall equation of the reaction between sulphur (S) and oxygen (O₂) to produce sulphur trioxide (SO₃) .

This is illustrated below:

S (s) + O₂ (g) —> SO₂ (g)

SO₂ (g) + O₂ (g) —> 2SO₃ (s)

Overall reaction:

2S (s) + 3O₂ (g) —> 2SO₃ (g)

Next, we shall determine the number of mole of oxygen (O₂) needed to completely convert 6.30 g (i.e 0.197 mole) of sulfur.

This is illustrated below:

From the balanced equation above,

2 moles of sulphur (S) required 3 moles of oxygen (O₂) .

Therefore, 0.197 mole of sulphur (S) will require = (0.197 × 3)/2 = 0.296 mole of oxygen (O₂).

Therefore, 0.296 mole of oxygen (O₂) is needed.

Finally, we shall determine the volume of oxygen (O₂) needed as follow:

Number of mole (n) of oxygen (O₂) = 0.296 mole

Temperature (T) = 340 °С = 340 °С + 273 = 613 K

Pressure (P) = 4.75 atm

Gas constant (R) = 0.0821 atm.L/Kmol

Volume (V) of oxygen (O₂) =.?

PV = nRT

4.75 × V = 0.296 × 0.0821 × 613

Divide both side by 4.75

V = (0.296 × 0.0821 × 613) / 4.75

V = 3.14 L

Therefore, 3.14 L of oxygen (O₂) is needed for the reaction.

5 0

3 years ago