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3 years ago

Two non-metals that have less than 10 protons

Chemistry

1 answer:

solong [7]3 years ago

8 0

If you where to randomly pick two nonmetals that have less than 10 protons it would be Hydrogen and carbon.

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Why is an alloy is often more useful than a pure metal

mrs_skeptik [129]

<h2>Answer:</h2>

A pure metal has specific properties. Sometimes we need that metal but with modified properties. So for the modification of properties we make alloys.

<h3>Explanation;</h3>

An alloy is a mixture of two elements, one of which is a metal.
Alloys often have properties that are different to the metals they contain.
This makes them more useful than the pure metals alone.
For example, alloys are often harder than the metal they contain.

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3 years ago

Question 2 (1 point)<br>At the center of the atom is the electron.<br>True<br>False

Stells [14]

Answer:

False the electrons are on the outside of the atoms

Explanation:

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3 years ago

I need help solving a kinetics equation.

Lady bird [3.3K]

Answer:

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3 years ago

Which object is a good conductor of heat and electricity?

Alex

Answer:

Explanation:

Metals are good conductors of heat

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3 years ago

Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select the one letter

maksim [4K]

Answer : The only reaction (C) that shows that the same reactant undergoes both oxidation and reduction.

Explanation :

Disproportionation reaction : It is defined as the reaction in which the same reactant undergoes both oxidation and reduction reaction. It is a redox reaction.

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

(A) The given balanced reaction is,

$H_2SeO_4(aq)+2Cl^-(aq)+2H^+(aq)\rightarrow H_2SeO_3(aq)+Cl_2(g)+H_2O(l)$

This reaction is a redox reaction but not disproportionation reaction because in this reaction there are two reactants in which chlorine shows oxidation and selenium shows reduction.

(B) The given balanced reaction is,

$S_8(s)+8O_2(g)\rightarrow 8SO_2(g)$

This reaction is a redox reaction but not disproportionation reaction because in this reaction there are two reactants in which sulfur shows oxidation and oxygen shows reduction.

(C) The given balanced reaction is,

$3Br_2(aq)+6OH^-(aq)\rightarrow 5Br^-(aq)+BrO_3^-(aq)+3H_2O(l)$

This reaction is a disproportionation reaction because in this reaction only one reactant bromine that shows both oxidation and reduction reaction.

(D) The given balanced reaction is,

$Ca^{2+}(aq)+SO_4^{2-}(aq)\rightarrow CaSO_4(s)$

This reaction is a combination reaction in which the two reactant react to give a single product. There is no changes in the oxidation state of calcium and sulfate.

(E) The given balanced reaction is,

$PtCl_4(s)+2Cl^-(aq)\rightarrow PtCl_6^{2-}(aq)$

This reaction is a combination reaction in which the two reactant react to give a single product. There is no changes in the oxidation state of platinum and chlorine.

Hence, the only reaction (C) that shows that the same reactant undergoes both oxidation and reduction.

6 0

3 years ago