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4 years ago

Does potassium nitrate (KN03) incorporate ionic bonding, covalent bonding, or both? Explain.

Chemistry

1 answer:

ladessa [460]4 years ago

4 0

Answer: $KNO_3$ incorporates both ionic bonding and covalent bonding.

Explanation:

A covalent bond is formed when an element shares its valence electron with another element. This bond is formed between two non metals.

An ionic bond is formed when an element completely transfers its valence electron to another element. The element which donates the electron is known as electropositive element and the element which accepts the electrons is known as electronegative element. This bond is formed between a metal and an non-metal.

For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

Here potassium is having an oxidation state of +1 called as $K^{+}$ cation and nitrate $NO_3^{-}$ is an anion with oxidation state of -1. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral $KNO_3$ . $NO_3^-$ is formed by sharing of electrons between two non metals nitrogen and oxygen.

Thus $KNO_3$ incorporates both ionic bonding and covalent bonding.

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At room temperature, the surface tension of water is 72.0 mJ·m–2. What is the energy required to change a spherical drop of wate

Keith_Richards [23]

It is given that the surface area of sphere is 4 π r² and its volume is (4/3 π r³)
With a diameter of 1.2 mm you have a radius of 0.6 mm so the surface area about 4.5 mm² and the volume is about 0.9 mm³
The total surface energy of the original droplet is (4.5 x 10⁻⁶ m x 72) = 3.24 x 10⁻⁴mJ
The five smaller droplets need to have the same volume as the original so:
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Since this smaller volume still have volume (4/3 π r³) so r = 0.35 mm
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3 years ago

Read the chemical equation. Fe2O3 + CO → Fe + CO2 If 3 moles of Fe2O3 react with 1.5 moles of CO, how many moles of each product

vfiekz [6]

Answer:- A) 1 mole of Fe and 1.5 moles of $CO_2$ .

Solution:- The balanced equation is:

$Fe_2O_3+3CO\rightarrow 2Fe+3CO_2$

From balanced equation, there is 1:3 mol ratio between $Fe_2O_3$ and CO, From given data, 3 moles of $Fe_2O_3$ and 1.5 moles of CO are taken for the reaction. CO is the limiting reactant as it's moles are less than the other reactant and which is also clear from the mole ratio. We could do the calculations also to support this. Let's calculate the moles of CO required to react completely with given 3 moles of $Fe_2O_3$ .

$3molFe_2O_3(\frac{3molCO}{1molFe_2O_3})$

= 9 mol CO

So, from calculations, 9 moles of CO are required to react completely with 3 moles of Iron(III)oxide but only 1.5 moles of CO are available. Hence, CO is the limiting reactant and the product moles are calculated from this as:

$1.5molCO(\frac{2molFe}{3molCO})$

= 1 mol Fe

$1.5molCO(\frac{3molCO_2}{3molCO})$

= 1.5 mol $CO_2$

So, the correct choice is A) 1 mole of Fe and 1.5 moles of $CO_2$ .

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4 years ago

Procedure for the experiment.

Elis [28]

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A solid residue of limestone and some gypsum.

Explanation:

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3 years ago