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3 years ago

Is it true that all atoms strive to have eight electrons in their outermost shell?

2 answers:

7 0

YESS It is true!!. In general, atoms are most stable, least reactive, when their outermost electron shell is full. Most of the elements important in biology need eight electrons in their outermost shell in order to be stable, and this rule of thumb is known as the octet rule.

ladessa [460]3 years ago

4 0

Y⃨E⃨S⃨ In general, atoms are most stable, least reactive, when their outermost electron shell is full. Most of the elements important in biology need eight electrons in their outermost shell in order to be stable, and this rule of thumb is known as the octet rule.

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What does the little ‘3’ in 2NH3 mean?

Svet_ta [14]

Answer:

It determines the number of molecules

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3 years ago

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Nearly every compound of silicon has the element in the ⁺4 oxidation state. In contrast, most compounds of lead have the element

baherus [9]

Boron shows analogous behaviour with silicon. Every compound of Boron have +3 oxidation state, while as we go down the the oxidation state become +1 and +3. For example, gallium, indium, etc.

Similarly, every compound of silicon has the element in the ⁺4 oxidation state. In contrast, most compounds of lead have the element in the ⁺2 state because of inert pair effect.

<h3>What is Inert pair effect? </h3>

The inert-pair effect is defined as the tendency of two electrons in the outermost atomic s-orbital almost remain unshared in the compounds of the post-transition metals.

<h3>How we calculate Oxidation state? </h3>

Each atom in an element either be in its uncombined or free state has oxidation number of zero. Such as each atom in H₂, Cl₂ , P4, ,O₂ , Na, Al, O3, S8, and Mg, all have an oxidation number zero.
The oxidation state of ions that comprise of only one atom is the actual charge on the ion.
The oxidation state of hydrogen is +1, excluding when it is bonded to metals having two elements. For example, CaH2, its oxidation state is –1.
Fluorine and other halogens have an oxidation state equal to –1 when they appear as a form of halide ions in their compounds.

Since the inert pair effect increases as we go down the group and become more predominant, therefore, the stability of +2 oxidation state goes on increasing down the group. Therefore, gallium, indium are mostly found in +1 oxidation state.

Thus, we concluded that Boron shows analogous behaviour with silicon. Every compound of Boron have +3 oxidation state, while as we go down the the oxidation state become +1 and +3. For example, gallium, indium, etc.

learn more about oxidation state:

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4 0

2 years ago

What is the primary buffer in the plasma?

Alecsey [184]

Answer:

Bicarbonate, the conjugate base of carbonic acid.

Explanation:

7 0

3 years ago

Balance the redox reaction Al(s) + MnO4^- (aq) --> MnO2 (s) + Al(OH)4^- (aq) in aqueous basic solution

GREYUIT [131]

Answer:

Al + MnO4- + 2H2O → Al(OH)4- + MnO2

Explanation:

First of all, we out down the skeleton equation;

Al + MnO4- → MnO2 + Al(OH)4-

Secondly, we write the oxidation and reduction equation in basic medium;

Oxidation half equation:Al + 4H2O + 4OH- → Al(OH)4- + 4H2O + 3e-

Reduction half equation:MnO4- + 4H2O + 3e- → MnO2 + 2H2O + 4OH-

Thirdly, we add the two half reactions together to obtain:

Al + MnO4- + 8H2O + 4OH- + 3e- → Al(OH)4- + MnO2 + 6H2O + 3e- + 4OH-

Lastly, cancel out species that occur on both sides of the reaction equation;

Al + MnO4- + 8H2O→ Al(OH)4- + MnO2 + 6H2O

The simplified equation now becomes;

Al + MnO4- + 2H2O → Al(OH)4- + MnO2

4 0

3 years ago

If any 1 studying 11th can u plz send me the chemistry notes for chapter 2 STRUCTURE OF AN ATOM lesson

timofeeve [1]

Answer:

Atom is the smallest particle of matter that can take part in a chemical reaction.

Atom is made of electron, proton and neutrons.

Atom is not capable of independent existence.

Two or more atoms combine together to form molecules.

Electron:

Negatively charged particle discovered on the basis of ‘cathode ray discharge tube’ experiments.

Conclusion from ‘cathode ray discharge tube’ experiment:

Cathode rays start from cathode and move toward anode.

These rays are not visible but their behaviour can be observed with fluorescent or phosphorus sent material.

In the absence of electric or magnetic field these travels in strait lines.

In the presence of electric or magnetic field the behaviour of cathode rays is similar to negatively charged particles which suggest that these rays contain negatively charge particles called electron.

Proton:

Positively charged particle discovered on the basis of anode ray experiment.

Some of the characteristics of anode rays, also called canal rays, are:

These travel in straight line and posses mass many times the mass of an electron.

These are not originated from anode.

These are deflected by electric and magnetic field.

Unlike cathode rays, the positively charged particles depend upon the nature of the gas from which these originate.

Neutron:

Neutral particles discovered by bombarding a thin sheet of beryllium by α- particles.

Conclusion from α- particles scattering experiment:

Most of the α-particles passed through foil undeflected, indicating most of the space in atom is empty.

Some of the α-particles are deflected to certain angles, which means that there is positively mass present in atom.

Only some of the α-particles suffered large deflections, which means that the positively charged mass must be occupying very small space.

Strong deflections or even bouncing back of α-particles from metal foil indicate the direct collision with positively charged mass in atom.

Comparison between the subatomic particles of an atom

subatomic particles comparison

Thomson model of atom:

atom is considered asa uniform positively charged sphere with radius about 10-10 m, in which electrons are is uniformly distributed.

Electrons are embedded in such a manner to give most stable electrostatic arrangement.

Mass of atom is assumed to be uniformly distributed in atom.

Also known as plum pudding raisin pudding orwatermelon model.

Rutherford’s Nuclear Model of Atom:

Based upon α-particles scattering experiment.

Most part of the atom is empty.

Atom possesses a highly dense, positively charged centre, called nucleus of the order 10-13 cm.

Entire mass of the atom is concentrated inside the nucleus.

Electrons revolve around the nucleus in circular orbits.

Electrons and the nucleus are held together by electrostatic forces of attraction.

Drawbacks of Rutherford’s Model:

It doesn’t explain the stability of atom.

It doesn’t say anything about the electronic distribution of electrons around nucleus.

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3 years ago

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