Answer:
Yes. Example: <u>Sulfur hexafluoride (SF₆) molecule</u>
Explanation:
According to the octet rule, elements tend to form chemical bonds in order to have <u>8 electrons in their valence shell</u> and gain the stable s²p⁶ electronic configuration.
However, this rule is generally followed by main group elements only.
Exception: <u>SF₆ molecule</u>
In this molecule, six fluorine atoms are attached to the central sulfur atom by single covalent bonds.
<u>Each fluorine atom has 8 electrons in their valence shells</u>. Thus, it <u>follows the octet rule.</u>
Whereas, there are <u>12 electrons around the central sulfur atom</u> in the SF₆ molecule. Therefore, <u>sulfur does not follow the octet rule.</u>
<u>Therefore, the SF₆ molecule is known as a </u><u>hypervalent molecule</u><u> or expanded-valence molecule.</u>
CaCO3 <span>→</span> CaO + CO<span>2
</span>H2CO3 →<span> H</span>2O<span> + CO</span>2<span>
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Muddy water is indeed a mixture
Answer:
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Answer:
The correct order of the elements, taking into account their ionic radius from highest to lowest, is:
<em>a) Cl⁻¹ > F⁻¹ > Na⁺¹ > Mg⁺²</em>
<em>b) S⁻² > O⁻² > Li⁺¹ > Be⁺²</em>
<em>c) S⁻² > Cl⁻¹ > K⁺¹ > Na⁺¹</em>
Explanation:
In ions the ionic radius is determined by the amount of electrons an element gains or loses to become an ion. The more negative an ion is, the greater its ionic radius.
As a rule, anions (negative charge) have a larger ionic radius than cations (positive charge), because the loss of electrons means a contraction of the ionic radius, while the gain of electrons means a greater radius.
To determine which ionic radius is greater in anions or cations with the same charge, it must be considered that in the periodic table the ionic radius increases from top to bottom and from right to left.
Learn more:
Ionic radius example brainly.com/question/2279609
