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2 years ago

An ion of iron has an 26 protons, 30 neutrons, and 23 electrons. what are its atomic number, atomic mass, and net charge?

Chemistry

2 answers:

Murrr4er [49]2 years ago

6 0

Answer:

Z=26, A = 56, charge +3.

Explanation:

The atomic number is represented by Z. Is equal to the total number of protons that the atom has. Z=26.

The atomic mass is represented by A. The number results from the total sum of protons and neutrons of an atom. Both particles have a weight of 1 uma, are in the nucleus and give the mass to the atom.

Mass number (A) = atomic number (Z) + number of neutrons (N)

A = 26 + 30

A = 56

The net charge of the atom can be calculated by subtracting the negative charges from the positive ones. The positive charges come from the protons and the negative ones from the electrons.

26-23=3

This iron ion has a positive charge +3.

k0ka [10]2 years ago

6 0

The atomic number of iron ion is $\boxed{26}$ .

The atomic mass of an iron ion is $\boxed{56}$ .

The net charge on an iron ion is $\boxed{ + 3}$ .

Further Explanation:

The smallest particle that is the building block of matter is known as an atom. Most of the space in an atom is empty, and its mass is concentrated inside a small region called the nucleus.

An atom is written as $_{\text{Z}}^{\text{A}}{\text{X}}$ , where A is the mass number, Z is the atomic number and X is the letter symbol of the element.

Protons, electrons, and neutrons are the three subatomic particles that are present in the atom. The Protons and neutrons present in an atom are collectively called nucleons because these are located in the nucleus of the atom. Electrons revolve around the nucleus in definite orbits.

The positively charged subatomic particle is called proton. It is equal to the atomic number (Z) of the element.

Electron is the negatively charged subatomic particle. The number of electrons present in an atom is equal to the number of protons of an atom in a neutral atom.

The subatomic particle with no charge is called neutron. It is situated within the nucleus. The number of neutrons present in the nucleus of an atom is called the neutron number. Atomic mass or mass number is the total number of nucleons within the atomic nucleus. So if the atomic number or the proton number is known, the number of neutrons can be calculated by the difference of mass number (A) and atomic number (Z).

The ion of iron has 26 protons. As the number of protons is same as to the atomic number of the element. So the atomic number (Z) of iron is 26.

The expression to calculate the atomic mass of the element is,

${\text{Atomic mass}}\left({\text{A}}\right)={\text{Number of protons}}+{\text{Number of neutrons}}$ ......(1)

The number of protons in iron ion is 26.

The number of neutrons in iron ion is 30.

Substitute these values in equation (1) to calculate the atomic mass of iron.

$\begin{aligned}{\text{Atomic mass of iron}}&={\text{26}}+{\text{30}}\\&={\mathbf{56}}\\\end{aligned}$

The formula to calculate the net charge on the ion is,

${\text{Net charge}}={\text{Number of protons}}-{\text{Number of electrons}}$ ......(2)

The number of protons in iron ion is 26.

The number of electrons in iron ion is 23.

Substitute these values in equation (2) to calculate the net charge on the iron ion.

$\begin{aligned}{\text{Net charge on iron ion}}&=26 - 23\\&={\mathbf{ + 3}}\\\end{aligned}$

So the atomic number, atomic mass and net charge on iron ion are 26, 56, and +3 respectively.

Learn more:

1. Which particle is equal to the atomic number of an element?: brainly.com/question/1424763

2. Name the subatomic particle with least mass: brainly.com/question/2224691

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Structure of the atom

Keywords: subatomic particle, proton, electron, neutron, mass, positively charged, neutral, negatively charged, atomic number, atomic mass, no charge, building block, matter, atom, nucleus, 26, 56, +3, net charge, ion, iron.

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Calculate the molality of 75.0 grams of MgCl2 (molar mass=95.21 g/mol) dissolved in 500.0 g of solvent.

nordsb [41]

Answer: The molality of magnesium chloride is 1.58 m

Explanation:

To calculate the molality of solution, we use the equation:

$\text{Molality}=\frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}$

Where,

$m_{solute}$ = Given mass of solute (magnesium chloride) = 75.0

$M_{solute}$ = Molar mass of solute (magnesium chloride) = 95.21 g/mol

$W_{solvent}$ = Mass of solvent = 500.0 g

Putting values in above equation, we get:

$\text{Molality of }MgCl_2=\frac{75.0\times 1000}{95.21\times 500.0}\\\\\text{Molality of }MgCl_2=1.58m$

Hence, the molality of magnesium chloride is 1.58 m

5 0

3 years ago

Read 2 more answers

A frictionless piston cylinder device is subjected to 1.013 bar external pressure. The piston mass is 200 kg, it has an area of

Bad White [126]

Answer:

a) $T_{2} = 360.955\,K$ , $P_{2} = 138569.171\,Pa\,(1.386\,bar)$ , b) $T_{2} = 347.348\,K$ , $V_{2} = 0.14\,m^{3}$

Explanation:

a) The ideal gas is experimenting an isocoric process and the following relationship is used:

$\frac{T_{1}}{P_{1}} = \frac{T_{2}}{P_{2}}$

Final temperature is cleared from this expression:

$Q = n\cdot \bar c_{v}\cdot (T_{2}-T_{1})$

$T_{2} = T_{1} + \frac{Q}{n\cdot \bar c_{v}}$

The number of moles of the ideal gas is:

$n = \frac{P_{1}\cdot V_{1}}{R_{u}\cdot T_{1}}$

$n = \frac{\left(101,325\,Pa + \frac{(200\,kg)\cdot (9.807\,\frac{m}{s^{2}} )}{0.15\,m^{2}} \right)\cdot (0.12\,m^{3})}{(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} )\cdot (298\,K)}$

$n = 5.541\,mol$

The final temperature is:

$T_{2} = 298\,K +\frac{10,500\,J}{(5.541\,mol)\cdot (30.1\,\frac{J}{mol\cdot K} )}$

$T_{2} = 360.955\,K$

The final pressure is:

$P_{2} = \frac{T_{2}}{T_{1}}\cdot P_{1}$

$P_{2} = \frac{360.955\,K}{298\,K}\cdot \left(101,325\,Pa + \frac{(200\,kg)\cdot (9.807\,\frac{m}{s^{2}} )}{0.15\,m^{2}}\right)$

$P_{2} = 138569.171\,Pa\,(1.386\,bar)$

b) The ideal gas is experimenting an isobaric process and the following relationship is used:

$\frac{T_{1}}{V_{1}} = \frac{T_{2}}{V_{2}}$

Final temperature is cleared from this expression:

$Q = n\cdot \bar c_{p}\cdot (T_{2}-T_{1})$

$T_{2} = T_{1} + \frac{Q}{n\cdot \bar c_{p}}$

$T_{2} = 298\,K +\frac{10,500\,J}{(5.541\,mol)\cdot (38.4\,\frac{J}{mol\cdot K} )}$

$T_{2} = 347.348\,K$

The final volume is:

$V_{2} = \frac{T_{2}}{T_{1}}\cdot V_{1}$

$V_{2} = \frac{347.348\,K}{298\,K}\cdot (0.12\,m^{3})$

$V_{2} = 0.14\,m^{3}$

4 0

3 years ago

How many g of MgCO3(s) are needed to make 1.2 L of 1.5 M MgCl2(aq) solution?

maw [93]

Molar mass of MgCO3 is 84.313 g/mol
You can calculate this from data on the periodic table:
Molar mass Mg = 24.305g/mol
molar mass C = 12.011g/mol
molar mass O = 15.999g/mol mass 3 mol = 47.997g
Total = 84.313g/mol

Mass to be used in 1.2L of 1.5M solution = 84.313g * 1.2L * 1.5mol /L = 151.763g
I have not taken significant figures into account
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2 years ago

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Doss [256]

Explanation:

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