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pogonyaev
3 years ago
5

Choose the electron configurations which are possible for an unexcited atom. Example 1 – 1s22s22p4 Example 2 – 1s22s22p63s23p33d

1 Example 3 – 1s22s22p83s1 Example 4 – 1s22s22p63s1
Chemistry
1 answer:
Aleonysh [2.5K]3 years ago
8 0

Answer:

Examples 1, 3 and 4

Explanation:

An unexcited atom is an atom in the ground state i.e the atom has it's valence electrons in it's lowest energy level possible. This actually implies the normal electronic configuration of the atom. Thus, examples 1, 3 and 4 have the actual electronic configuration with there valence electrons in the lowest possible energy level.

Example 1: 1S² 2S² 2P⁴

Example 3: 1S² 2S² 2P⁶ 3S¹ (There seem to be a mistake in the question provided, P energy level can only 6 electrons not 8)

Example 4: 1S² 2S² 2P⁶ 3S¹

NOTE: If you take a look at example 2, it will be deduced that the 3P energy level has only 3 valence electrons and the last valence electron jumped to 3d energy level; making that atom appear to be in it's excited state.

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What is responsible for the larger size of an anion in comparison with the atom from which it is form?
GarryVolchara [31]

Answer:

electron-electron repulsion

Explanation:

When electrons add into valence shell of neutral elements, the element assumes a negative oxidation state. With this, the number of electrons having (-) charges will be larger than the number of protons having positive (+) charges. As a result, the extra electrons repel one another (i.e., like charges repel) and a larger radius is the result.  

In contrast, when cations are formed, electrons are removed from the valence level (oxidation) producing an element having a greater number of protons than electrons. The larger number of protons will function to attract the electron cloud with a greater force that results in a contraction of atomic radius and a smaller spherical volume than the neutral unionized element.    

To visualize, see attached chart that shows atomic and ionic radii before and after ionization of the elements.  

Download pdf
4 0
3 years ago
A 6 l volume of ideal neon gas (monatomic) is at a pressure of 3.2 atmospheres and a temperature of 310 k. the atomic mass of ne
Tatiana [17]

Answer is: the final pressure of the gas is closest to 3,17 atm.

<span><span> p</span>₁ = 3,2 atm.</span><span>
T₁ = 310 K.</span><span>
V₁ = 6 L.</span><span>
p₂ = ?</span><span>
T₂ = 410K.</span><span>
V₂ = 8,0 L.</span><span>
<span>Use combined gas law - the volume of amount of gas is proportional to the ratio of its Kelvin temperature and its pressure.</span><span> 
p</span></span><span>₁V₁/T₁ = p₂V₂/T₂.</span><span>
<span>3,2 atm · 6,0 L ÷ 310 K  = p</span>₂ · 8,0 L ÷ 410 K.</span><span>
0,0619 = 0,0195p</span><span>₂.</span><span>
p</span><span>₂ = 3,17 atm.</span>

3 0
3 years ago
How many moles of oxygen (o) are in a sample of 3.98x10^23 atoms
gregori [183]
1 mol ------- 6,02·10²³ 
X ------------ 3,98·10²³
X = 3,98·10²³/<span>6,02·10²³ 
<u>X= 0,6611</u> moles of oxygen
________________________
:)
</span>
5 0
4 years ago
Why does food have potential energy?
Savatey [412]

Answer:

So that if we feel weak, energy is released through it so we can do work and do stuff like walk or think. It's like stored energy that can do things for the future.

Please give brainliest if it helped.

3 0
3 years ago
Read 2 more answers
How many moles are in 272 grams of hydrogen peroxide (H2O2) ?
Strike441 [17]

Answer:

8 moles

Explanation:

When we are asked to convert from grams of a substance into moles, we have to use the substance's molar mass.

Meaning that for this problem, we'll <em>use the molar mass of hydrogen peroxide</em> (H₂O₂), as follows:

  • 272 g ÷ 34 g/mol = 8 mol

There are 8 moles in 272 grams of hydrogen peroxide.

7 0
3 years ago
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