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aleksandr82 [10.1K]
2 years ago
7

How does an ion differ from an atom?

Chemistry
2 answers:
Alex73 [517]2 years ago
5 0
An atom is the smallest particle of an element that retains the chemical properties of the element. Atoms are electrically neutral, with a positively charged nucleus that binds one or more electrons in motion around it. An ion-An atom or molecule that has acquired a charge by either gaining or losing electrons. An atom or molecule with missing electrons has a net positive charge and is called a cation*; one with extra electrons has a net negative charge and is called an anion*.
Studentka2010 [4]2 years ago
3 0
An atom is what you would see on the periodic table e.g. hydrogen and nitrogen are atoms. Atoms have no overall charge and the charge of the electrons is equal to the charge of the protons. (but they are opposite charges- so protons have a +1 charge and electrons have a -1 charge).

An ion is when one or more electrons are either added or removed from an atom to form a charged particle. The atoms are then strongly attracted to each other.

So take, for example, sodium and chlorine atoms. When the atoms react the sodium ion gives up its outer electron and becomes a Na+ ion. This means it has a charge of +1 (due to it losing an electron, the forces are no longer balanced as there is one more proton than electrons). The chlorine gains the electron that sodium lost and becomes a Cl- ion. This meant it has a charge of -1 (due to it gaining an electron there is one more electron than protons, causing to forces to become unbalanced). Both ions then have full outer shells and are attracted to each other due to being oppositely charged.

To sum it up, an atom is what you see on the periodic table and they always have no charge and an ion is when an atom loses or gains at least one electron causing it to have a positive or negative charge.
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For a certain chemical reaction, the standard Gibbs free energy of reaction at 30.0 °C is 110. kJ. Calculate the equlilibriunm c
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Answer:

Explanation:

The equation that relates standard Gibbs free energy, ΔG, with equilibrium constant, K, is:

ΔG = -RT ln K

<em>Where R is gas constant, 8.314J/molK, and T is absolute temperatue (30.0°C + 273.15 = 303.15K).</em>

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Replacing (110kJ = 110000J):

110000J/mol = -8.314J/molK*303.15K ln K

-43.644 = lnK

1.11x10⁻¹⁹ = K

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How many moles of silver can be produced from silver nitrate from 1 mole of zinc?
jasenka [17]

Answer:

Answer: 6.5 moles of silver metal is formed in the given chemical reaction. The moles of excess reagent left are 0.55 moles.

Explanation:

To calculate the moles of silver formed and the moles of excess reagent left after the reaction, we need to balance the equation first and need to find the limiting and excess reagent.

The balanced chemical equation is:

Zn + 2AgNO3 ---> Zn (NO3)2 +2Ag

By Stoichiometry:

2 moles of Silver nitrate reacts with 1 mole of Zinc metal

So, 6.5 moles of silver nitrate will react with = 1/2 x 6.5 = 3.25 moles of zinc metal

The required amount of zinc metal is less than the given amount of zinc metal,  hence, it is considered as an excess reagent.

Therefore, silver nitrate is the limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of silver nitrate produces 2 moles of silver metal

So, 6.5 moles of silver nitrate will produce = 2/2 x 6.5 = 6.5moles of silver metal.

Number of moles of excess reagent left after the completion of reaction = (3.8 - 3.25)moles = 0.55 moles

Hence, 6.5 moles of silver metal is formed in the given chemical reaction. The moles of excess reagent left are 0.55 moles.

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