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xenn [34]
3 years ago
11

Select all the correct images, select the two atomic models that belong to the same element.

Chemistry
1 answer:
Scrat [10]3 years ago
8 0

Check the circled atoms in the attached diagram

Explanation:

The circled options all belongs to the same elements. They are simply isotopes.

Since:

          Red ball = protons

          Yellow ball = neutron

           Blue ball = electron

The protons are positively charged and with the neutrally charged neutrons they both occupy the vicinity of the nucleus of an atom.

Electrons moves round the nucleus in orbits.

Atoms of the same elements have the same number of protons.

The circled options all have two protons.

The atoms only differ in the number of neutrons which signifies that they are merely isotopes.

More descriptively, the atoms are Helium atoms.

learn more:

Isotope brainly.com/question/4551913

#learnwithBrainly

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What can help overcome a positive enthalpy of solution and allow a solid
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Answer: D. An increase in entropy

Explanation:

Entropy is the measure of randomness or disorder of a system. If a system moves from  an disordered arrangement to an ordered arrangement, the entropy is said to increase and vice versa.

For a reaction to be spontaneous, the enthalpy of the solution must decrease and the entropy must increase.

To overcome a positive enthalpy of solution and allow a solid  solute to dissolve in water, an increase in entropy would make the reaction spontaneous as the system would move to a more disordered state.

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Why was Niels Bohr’s atomic model superior to all the earlier models?
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What is the electron configuration for<br> 08<br> 16
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The electron configuration for Oxygen : [He] 2s²2p⁴

<h3>Further explanation</h3>

Writing electron configurations starts from the lowest to the highest sub-shell energy level. There are 4 sub-shells in the shell of an atom, namely s, p, d, and f. The maximum number of electrons for each sub-shell is  

• s: 2 electrons  

• p: 6 electrons  

• d: 10 electrons and  

• f: 14 electrons  

Charging electrons in the sub-shell uses the following sequence:  

<em>1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.  </em>

The element is Oxgen, with symbol O, and :

the atomic number=8=number of electron

the atomic mass=16

The electron configuration based on the number of electrons(for Oxygen=8), so the configuration :

\tt _8^{16}O:1s^22s^22p^4 or we can write with noble gas [He] 2s²2p⁴

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