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3 years ago

How does the average atomic mass of an element differ from the mass of an individual atom of the same element?

1 answer:

6 0

In periodic tables, the relative atomic mass is usually not a whole number, even though the mass of both protons and neutrons is 1. This is due to isotopes, which are atoms of the same element, but they have different amounts of neutrons in their nuclei. So the relative mass of an individual atom is always a whole number, and the relative atomic mass is an average of all of the isotopes of the element.

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ivanzaharov [21]

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3 years ago

Which type of van der walls force is responsible for holding polar molecules together? london dispersion dipole-dipole hydrogen

svet-max [94.6K]

Answer:

dipole-dipole

Explanation:

Polar molecules are formed as result of covalent bonds between atoms.

Dipole-dipole attraction are intermolecular bonds. Both London dispersion forces and dipole-dipole attraction are van der waals forces.

In dipole-dipole attraction, polar molecules (unsymmetrical molecules) line up such that the positive pole of one molecule attracts the negative pole of another. Example of such is found in HCl.

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3 years ago

An area where material from deep within Earth's mantle rises to the crust and melts to form magma is called a

AnnyKZ [126]

Answer:

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3 years ago

What are the isomers of c3h6br2...

maks197457 [2]

C3H6Br2 2 isomers:- bominated allkane

CH3CH2CHBr2 1,1-dibromopropane
<span>CH3CHBrCH2Br 1,2-dibromopropane

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7 0

4 years ago

Identify the oxidizing agent and the reducing agent for the following reaction: Zn(s)+Cu2+(aq)→Zn2+(aq)+Cu(s) Express your answe

Ainat [17]

Answer: oxidizing agent: $Cu^{2+}$ , reducing agent : $Zn$

Explanation: Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

For the given reaction:

$Zn(s)+Cu^{2+}(aq)\rightarrow Zn^{2+}(aq)+Cu(s)$

On reactant side:

Oxidation state of zinc = 0

Oxidation state of copper = +2

On product side:

Oxidation state of zinc = +2

Oxidation state of copper = 0

The oxidation state of copper reduces from +2 to 0, it is getting reduced. The substance which itself gets reduced, oxidizes other and is called as oxidizing agent.Thus $Cu^{2+}$ acts as oxidizing agent.

The oxidation state of zinc increases from 0 to +2. Thus, it is getting oxidized and it undergoes oxidation reaction. The substance which itself gets oxidized, reduces other and is called as reducing agent.Thus $Zn$ acts as reducing agent.

3 0

3 years ago