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Nataly_w [17]
3 years ago
15

What are energy sublevels?

Chemistry
2 answers:
MaRussiya [10]3 years ago
5 0
The answer is B: multiple orbitals of specific magnitude within an energy level
sdas [7]3 years ago
3 0

Answer:

Option B

Explanation:

First, we need to know what is an energy level.

An energy level corresponds to the row of the periodic table of element. So, if you see the attached picture, you can see that we have 7 rows where the elements are distributed, so, we have 7 energy levels for all those elements.

Knowing that, the sub levels are the caps where the electrons of the atoms are carried. These sublevels or caps, are called orbitals, these can be of several types

s orbytal: can hold 2 electrons

p orbytal: can hold up to 6 electrons.

d orbytal: can hold up to 10 electrons

f orbytal: can hold up to 14 electrons

g orbytal: can hold up to 18 electrons.

Depending on the row (or energy level) and the atom, we can know how many electrons can carry an element, in which period or row is, and the sub levels. For example, the Chlorine, with an atomic number of 17, can carry up to 7 electrons in it's outer level and it's on the third row (two energy levels). This can be known with it's electronic configuration:

[Cl] = 1s^2 2s^2 2p^6 3s^2 3p^5

The last energy level is 3, so it's the third period, and the electrons of those sub level are 2 and 5, 7 electrons.

Hope this can help better

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An ideal gas is a gas. <br> Perfect<br> Theoretical<br> Real
dusya [7]

Answer:

An ideal gas is a theoretical gas composed of many randomly moving point particles that are not subject to interparticle interactions. The ideal gas concept is useful because it obeys the ideal gas law, a simplified equation of state, and is amenable to analysis under statistical mechanics.

5 0
3 years ago
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When 10.0 grams of sulfur reacts with fluorine gas at a pressure of 2.69 atmosphere in a 5.00 L container at 0.00 degrees Celsiu
Gwar [14]

Answer:

74.1%

Explanation:

Based on the reaction:

S₈ + 16F₂ → 8SF₄

<em>1 mole of sulfur reacts with 16 moles of F₂ to produce 8 moles of SF₄</em>

<em />

To solve this question we must find the moles of each reactant in order to find the moles of SF₄. Thus, we can find the theoretical mass produced. Percent yield is:

Percent yield = Actual yield (25.0g) / Theoretical yield * 100

<em>Moles S₈: 256.52g/mol</em>

10.0g * (1mol / 256.52g) = 0.0390 moles

<em>Moles F₂:</em>

<em>PV = nRT</em>

PV/RT = n

<em>Where P is pressure in atm, V is volume in liters, R is gas constant and T is absolute temperature (0°C = 273.15K)</em>

2.69atm*5.00L / 0.082atmL/molK*273.15K = n

0.600 moles = n

For a complete reaction of 0.600 moles F₂ are required:

0.600mol F₂ * (1mol S₈ / 8 mol F₂) = 0.075 moles S₈

As there are just 0.0390 moles, S₈ is limiting reactant.

The theoretical moles and mass of SF₄ -Molar mass: 108.07g/mol- is:

0.0390 moles S₈ * (8mol SF₄ / 1mol S₈) = 0.312 moles SF₄ * (108.07g) =

33.7g

Percent yield = 25.0g / 33.7g * 100

= 74.1%

6 0
2 years ago
What is the volume, in liters, of 0.500 mol of c3h8 gas at stp? (hint..use avogadro’s principle to solve this)?
wolverine [178]
When we are at STP conditions, we can use this conversion: 1 mol= 22.4 L

0.500 mol C₃H₈ (22.4 L/ 1 mol)= 11.2 L
3 0
3 years ago
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Please Answer ASAP
adelina 88 [10]

The answer to this question would be S2o6 which is C.


3 0
3 years ago
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Timed PLS help
Bezzdna [24]

Answer:

19.5g is the theoretical yield of alum

Explanation:

Based on the balanced reaction, 4 moles of sulfuric acid produce 2 moles of alum. To solve this question we need to find the moles of H2SO4. With these moles we can find the moles of alum and its mass assuming all sulfuric acid reacts producing alum.

<em>Moles Sulfuric Acid:</em>

8.3mL = 0.0083L * (9.9mol/L) = 0.08217 moles sulfuric acid

<em>Moles Alum:</em>

0.08217 moles sulfuric acid * (2mol KAl(SO4)2•12H2O / 4mol H2SO4) =

0.041085 moles KAl(SO4)2•12H2O

<em>Mass Alum -Molar mass: 474.3884 g/mol-</em>

0.041085 moles KAl(SO4)2•12H2O * (474.3884 g/mol) =

<h3>19.5g is the theoretical yield of alum</h3>
3 0
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