Answer:
atoms tend to react in order to gain 8 valence electrons
Explanation:
The octet rule describes the tendency of atoms of elements to react in order to have eight electrons in their valence shell. This is because having eight valence electrons confers stability to the atoms of these elements in the compounds they form.
The octet rule only does not apply to the transition elements or the inner transition elements as only the s and p electrons are involved. the electronic configuration in atoms having an octet is s²p⁶.
For example, sodium atom has one valence electron in its valence shell but a complete octet in the inner shell; it will react with chlorine atom which has seven valence electrons to form a stable compound, sodium chloride by donating its one valence electron in order to have an octet. Similarly, the chlorine atom will then have an octet by accepting the one electron from sodium atom.
Answer:
Real gas particles have significant volume
Real gas particles have more complex interactions than ideal gas particles.
Explanation:
An ideal gas is an imaginary concept and a gas behaves almost ideally at certain pressure and temperature conditions.
The gas in real deviates from the ideal behavior as some of the assumptions made for ideal gases are not true in case of real gases.
Real gas particles have significant volume as compared to vessel unlike ideal gases.
There are interactions present in between real gas molecules at high pressure conditions.
Answer:
moon
Explanation:
the moon's gravitational pull generates tidal force which affects earth's tides
Answer:
The type of reaction for the following equation is combustion equation.
Explanation:
Combustion reaction is defined as the chemical reaction in which a hydrocarbon reacts with oxygen gas to produce carbon dioxide gas and water molecule.
The reaction given to us:
When 1 mole of ethane reacts with 7/2 moles of oxygen gas it gives 3 moles of water and 2 moles of carbon dioxide gas.
The type of reaction for the following equation is combustion equation.
