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3 years ago

The Lewis structure for a chlorate ion, ClO3-, should show single bond(s), double bond(s), and lone pair(s).

Chemistry

2 answers:

Yuliya22 [10]3 years ago

7 0

Answer: A molecule of $ClO_3^-$ has 1 single bond, 2 double bonds and 8 lone pairs.

Explanation:

Lewis-dot structure is defined as the structure which represents the number of valence electrons around the atoms. The electrons are represented as dots.

This structure helps in the determination of bonding electrons and non-bonding electrons.

For the given compound $ClO_3^-$

As we know that chlorine has '7' valence electrons and oxygen has '6' valence electron. The negative charge gets add up in the total number of valence electrons.

Total number of valence electrons in $ClO_3^-$ = 7 + 3(6) + 1 = 26

In $ClO_3^-$ , two electrons of 2 oxygen atoms combine with 2 electrons of chlorine and 1 electron of one oxygen atom combines with 1 electron of chlorine atom.

A lone pair remains on the central atom which is chlorine.

Hence, a molecule of $ClO_3^-$ has 1 single bond, 2 double bonds and 8 lone pairs.

eduard3 years ago

3 0

1 single bond, 2 double bond 2 lone pairs

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For the reaction of C 2H 4( g) with O 2( g), to form CO 2( g) and H 2O( g), what number of grams of CO 2 could be produced from

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Explanation:

Based on the reaction:

C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(g)

1 mole of C₂H₄ reacts with 3 moles of oxygen to produce 2 moles of CO₂

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5.0g * (1mol / 32g) = 0.156moles

For a complete reaction of 0.0713 moles of C2H4 are required:

0.0713 moles C₂H₄ * (3 moles O₂ / 1 mol C₂H₄) = 0.214 moles of O₂

As there are just 0.156 moles, O₂ is limiting reactant.

The moles of CO₂ produced are:

0.156 moles O₂ * (2mol CO₂ / 3mol O₂) = 0.104 moles CO₂

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0.104 moles CO₂ * (44.01g / mol) =

<h3>4.58g of CO₂ could be produced</h3>

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The Lewis structure for a chlorate ion, ClO3-, should show ____ single bond(s), ____ double bond(s), and ____ lone pair(s).

The Lewis structure for a chlorate ion, ClO3-, should show single bond(s), double bond(s), and lone pair(s).