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3 years ago

If two atoms have the same atomic numbers but different mass numbers, then they can be considered atoms of the same element.

Chemistry

2 answers:

stiks02 [169]3 years ago

8 0

Answer:

True.

Explanation:

If two atoms have the same atomic number, they have the same number of protons in the nucleus.

The number of protons derermines the identity of an atom.

So, two atoms with the same atomic number are the same element.

castortr0y [4]3 years ago

7 0

Same elements can have different nuclei. So, true.

You might be interested in

Which atom loses 2 electrons while forming an ion?

BabaBlast [244]

Answer:

it would be a cation ... i believe

Explanation:

To become a cation, a positively charged ion, an atom would have to lose at least two electrons

7 0

3 years ago

Massive amounts of energy are contained in an atom's: Select one:

melamori03 [73]

Nucleus.
____________

6 0

4 years ago

Which intermolecular force is characteristic of compounds with low molar mass, which are liquids at room temperature and have re

eduard

Answer:

Hydrogen bonds.

Explanation:

The intermolecular forces are the forces that are presented between molecules in a substance. As higher is the force, as closer are the molecules, and more difficult will be to separate them.

Because of that, the solids have stronger forces than the liquids, which have stronger forces than the gases. Also, as strong the force, as higher will be the boiling point.

The ionic bond is the strongest and it's presented at ionic compounds, which are solids at room temperature and have high boiling points.

The covalent bonds are presented in the molecules and are formed when atoms share pairs of electrons. Between these molecules, the forces can be London forces, dipole-dipole forces, or hydrogen bonds.

The London forces are the weaker, they are presented at the nonpolar molecules, so it's easy to boil it. For a compound with low molar mass and London forces, it'll probably be at the gas phase at room temperature.

The dipole-dipole forces are presented at the polar molecules, and it's strong than the London forces. And the hydrogen bonds are a specific type of dipole-dipole forces, which is stronger and is formed between hydrogen and F, O, or N.

Because hydrogen has a low molar mass (1 g/mol), the compounds formed by it intends to have a low molar mass. So, to be liquid at room temperature, low mass, and high boiling point, it's more probable that the compound has hydrogen bonds.

6 0

3 years ago

What mass of phosphorus and of chlorine is needed to produce 87 g of pentachloride if the reaction yield is 60%?

Anna11 [10]

Hey there!

theoretical yield = (87* 100 ) / 60 = 145 g of phosphorous pentachloride

the reaction for this process is :

molar mass P2O5 => 239.2125 g/mol

molar mass P4 => 123.90 g/mol

molar mass Cl2 => 70.9060 g/mol

P4 + 5 Cl2 --------------> 2 P2Cl5

moles of P2O5 :

145 g / 239.2125 => 0.6062 moles of P2O5

Therefore:

moles of P4 = 0.6062 mol / 2 => 0.3031 moles

moles of Cl2 = 5/2 * 0.6062 mol = 1.5154 moles

mass of P4 ( phosphours ) = 0.3031 mol * 123.90 => 37.554 grams

mass of Cl2 ( chlorine ) = 1.5154 mol * 70.9060 => 107.45 grams

Hope That helps!

3 0

3 years ago

When the following oxidation-reduction occurs, what is the balanced reduction half-reaction after the electrons in both half rea

Lostsunrise [7]

Answer : The balanced reduction half-reaction is:

$3Cu^{2+}+6e^-\rightarrow 3Cu$

Explanation :

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.

The given balanced redox reaction is :

$Al(s)+Cu^{2+}(aq)\rightarrow Al^{3+}(aq)+Cu(s)$

The half oxidation-reduction reactions are:

Oxidation reaction : $Al\rightarrow Al^{3+}+3e^-$

Reduction reaction : $Cu^{2+}+2e^-\rightarrow Cu$

In order to balance the electrons, we multiply the oxidation reaction by 2 and reduction reaction by 3 and then added both equation, we get the balanced redox reaction.

Oxidation reaction : $2Al\rightarrow 2Al^{3+}+6e^-$

Reduction reaction : $3Cu^{2+}+6e^-\rightarrow 3Cu$

The balanced redox reaction will be:

$2Al(s)+3Cu^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Cu(s)$

Thus, the balanced reduction half-reaction is:

$3Cu^{2+}+6e^-\rightarrow 3Cu$

6 0

3 years ago