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Zinaida [17]
3 years ago
5

Which answer helps to explain why carbon atoms tend to make 4 covalent bonds? which answer helps to explain why carbon atoms ten

d to make 4 covalent bonds? the valence shell needs 8 electrons. the first electron shell has 4 orbitals. the carbon nucleus has 4 protons. all of the above. none of the above; carbon makes 3 covalent bonds?
Chemistry
2 answers:
Kay [80]3 years ago
8 0

Carbon-12 has the following electron configuration: 1s2-2s2-2p2. As seen in the configuration, the right answer is: the first electron shell has 4 orbitals.


Genrish500 [490]3 years ago
3 0

Carbon atoms tend to make 4 covalent bonds because the valence shell needs 8 electrons. For atoms to be stable, they must have filled outermost energy shells called valence shells. This is called the octet rule. Only noble gases (Group 8) elements have naturally filled valence shells which makes them stable elements. All other atoms tend to lose, gain, or share electrons to get the same electron configuration as these noble gases. Metals easily lose their electrons to non-metals which are readily accepting electrons. The bond that results from this transfer of electrons is called an ionic bond. Non-metals tend to share their electrons with other non-metals forming covalent bonds.

FURTHER EXPLANATION

<em>The first electron shell has 4 orbitals. </em>

<u>FALSE</u> The distribution of the electrons in the carbon atom is shown in the following electron configuration:  

 1s^2 \ 2s^2 \ 2p^2

The coefficients of the letters indicate the electron shell and the superscript tells the how many electrons occupy the orbitals. For carbon there are only two electron shells with electrons: electron shell 1 which has the s orbital and electron shell 2 with the s and three p orbitals.  

Therefore, <u>carbon only has one orbital in the first electron shell. </u>

<u> </u>

<em>The carbon nucleus has 4 protons. </em>

<u>FALSE</u> The number of protons in an atom gives it its unique identity. The proton count is given by the atomic number. The atomic number of C is 6. Therefore, <u>it has 6 protons in its nucleus. The atom with 4 protons is Beryllium (Be). </u>

<em>All of the above</em>

<u>FALSE </u> Two statements above are not true.

<em>Carbon makes 3 covalent bonds </em>

<u>FALSE</u> <u>Carbon forms 4 covalent bonds</u> because it can share 4 unpaired electrons with other atoms. It may form single, double. Or triple covalent bonds with other C atoms.

LEARN MORE  

• Ionization Energy brainly.com/question/2153804

• Atomic Number brainly.com/question/1446926

• Ionic Compound brainly.com/question/7007192

Keywords: octet rule, valence electrons, electron configuration

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Mandarinka [93]

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Name the type of organic compound from each description of the functional group: (b) group that is not polar and has a double bo
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1 year ago
Rank the following solutions in order of increasing acidity (least acidic to most acidic): I: [H3O+] = 1x10−5 II: [OH−] = 1x10−1
kozerog [31]

Answer: option C) II < III < I

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Explanation:

First, obtain the pH value of I and II, then compare both with III.

For I

Recall that pH = -log (H+)

So pH3O = -log (H3O+)

= - log (1x10−5)

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For II

pOH = - log(OH-)

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For III

pH = 6

Since, pH range from 1 to 14, with values below 7 to be acidic, 7 to be neutral, above 7 to be alkaline: then, 9 < 6 < 4

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6 0
3 years ago
Calculate the molarity 20ml of 3.5 m kci in to a final volume of 100 ml​
satela [25.4K]

Answer:

Molarity =  0.7 M

Explanation:

Given data:

Volume of KCl = 20 mL ( 0.02 L)

Molarity = 3.5 M

Final volume = 100 mL (0.1 L)

Molarity in 100 mL = ?

Solution:

Molarity = number of moles of solute / volume in litter.

First of all we will determine the number of moles of KCl available.

Number of moles = molarity × volume in litter

Number of moles = 3.5 M × 0.02 L

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Molarity in 100 mL.

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Molarity =  0.07 mol /0.1 L

Molarity =  0.7 M

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Phantasy [73]
The balanced chemical reaction is written as:

<span>3NO2 + H2O = 2HNO3 + NO

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538 L NO2 ( 1 mol / 22.4L ) ( 1 mol NO / 3 mol NO2 ) ( 22.4 L / 1 mol ) = 179.33 L NO is produced</span>
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