Bohr model of Silver Atom-How to draw Silver (Ag) Bohr-Rutherford diagram?

Bohr model describes the visual representation of orbiting electrons around the small nucleus. It used different electron shells such as K, L, M, N…so on. These shells hold a specific number of electrons, the electron shell which is closest to the nucleus has less energy and the electron shell which is farthest from the nucleus has more energy.

Bohr’s diagram is very interesting and easy to draw. Here, we will draw the Bohr model of the Silver atom with some simple steps.

Steps to draw the Bohr Model of Silver atom

1. Find the number of protons, electrons, and neutrons in the Silver

Protons are the positively charged particles and neutrons are the uncharged particles, both these are constituents of the atom nuclei. Electrons are the negatively charged particles that orbit the nucleus of an atom

To find the number of protons an atom contains, just look at its atomic number.

If the atomic number of atom is 45, then proton will also be 45, if atomic number is 46, then proton will also be 46.

As the atomic number of Silver is 47 so the number of protons present in it is also 47.

Now, to determine the number of neutrons in an atom, use this formula.

⇒ Number of neutrons in atom = Atomic mass of the atom(rounded to the nearest whole number) – Number of proton in an atom

For example, An atom have 33.988 atomic mass and 16 protons.

Then, to find the number of neutron, round the atomic mass to the near whole number, so, atomic mass 33.988 round to 34.

= (34 – 16 protons) = 18 number of neutrons in the atom

Now, to get the number of neutrons in a Silver atom, look at its atomic mass which is 107.8682, rounded off to the nearest whole number it is 108. The number of protons present in Silver is 47.

∴ Hence, the number of neutrons in Silver atom = (108 – 47) = 61.

It should be noted that “The number of electrons in a neutral atom is equal to the number of protons”.

As the Silver (Ag) atom is neutral thus the number of electrons present in it will be equal to its number of protons i.e., 47, as we discussed earlier.

⇒ The number of electrons in a Silver atom = 47

⇒ The number of protons in the Silver atom = 47

⇒ The number of neutrons in a Silver atom = 61

Let’s read in detail – How to find number of protons, electrons, neutrons?

2. Draw the nucleus of an atom

A nucleus is a dense and small region that contains the number of protons and neutrons of an atom.

In this step, we have to draw a small circle that consists of a number of protons and the number of neutrons of a Silver atom.

3. Draw the First electron shell

“An electron shell may be thought of as an orbit followed by electrons around an atom’s nucleus.”

The first electron shell is also called the K-shell, this is the closest shell to the nucleus of an atom and can hold a maximum of two electrons.

As we identified, the Silver atom has a total of 47 electrons. So we need to put 2 electrons from the 47 available in the first shell, next to each other, as shown below.

Now, that we have successfully drawn the first shell of the Silver atom that can hold 2 electrons, we know that we have used 2 electrons out of the 47 available in the first shell.

∴ (47-2) = 45 electrons.

This shows we are left with 45 electrons that we need to accommodate in the subsequent shells of the Silver atom.

4. Draw the Second electron shell

The second shell also called the L-shell that can hold a maximum of 8 electrons. This shell is drawn after the first electron shell.

In the second electron shell, the electrons are added one at a time, starting from the top position and then going in a clockwise direction.

In second shell, electrons are added one at a time in clockwise direction as a clock position – 12 o’clock, 3 o’clock, 6 o’clock, 9 o’clock positions.

Once you place the electrons one at a time to each of the four sides(Top – Right – Bottom – Left], start pairing or doubling them.

As we have 45 remaining electrons of a Silver atom, out of which the second shell can hold only a maximum of 8 valence electrons.

Thus, we place the next 8 electrons of the Silver atom in the second shell. Start from the top position and put electrons one at a time, moving in a clockwise direction (Top-Right-Bottom-Left), and finally pair them up.

At this step, out of the 47 electrons of the Silver atom, we have placed 2 electrons in the first shell and 8 electrons in the second shell.

∴ [47 – (2+8)] = 37 electrons.

This means we are now left with 37 electrons. So let’s see how we can assign them their appropriate positions in the next shells of the Silver atom.

5. Draw the Third electron shell

The third electron shell also called the M-shell can accommodate up to 18 electrons. For the elements in the first few periods of the Periodic Table, the third shell holds up to 8 electrons only. But actually, in totality, it has the capacity to hold 18 electrons.

⇒ The third subshell exhibits this capacity of holding ‘up to 18’’ electrons for atomic numbers greater than 20 such as 21,22,23,24, 25, 26, and so on.

⇒ The atomic number of Silver (Ag) is 47. As 47 is visibly greater than 20, this means the M-shell in the Silver Bohr model will be filled to its maximum capacity by accommodating a total of 18 electrons, as shown below.

The electrons are placed in a clockwise manner, as we discussed in step 4. Starting from the top position, put the electrons one at a time while moving in a clockwise direction (Top-Right—Bottom-Left), before pairing up the electrons.

By the time we have reached this step, out of the 47 electrons of the Silver atom, we have placed 2 electrons in the first shell, 8 electrons in the second shell and 18 electrons in the third electron shell which means a total of 2+8+18 = 28 electrons are used so far.

∴ 47 – [ 2+ 8+ 18] = 47 – 28 = 19 electrons.

Now let’s see how these remaining 19 electrons are placed in the subsequent shells of the Silver Bohr model.

6. Draw the Fourth electron shell

The fourth electron shell i.e., N-shell has a maximum capacity of holding 32 electrons in total. It consists of s, p, d, and f subshells.

The s subshell can contain 2 electrons, 6 electrons can be placed in the p-subshell, 10 electrons can be placed in the d-subshell while a total of 14 electrons can be accommodated in the f-subshell of shell number 4. 2+6+10+14 makes a total of 32 electrons.

⇒ But the electrons are placed in these subshells following the Aufbau Principle. Aufbau Principle states that electrons are filled diagonally, as shown below. Therefore, the electrons are filled in the s-subshell of shell number 5 before filling electrons in the d-subshell of shell number 4.

⇒ As there are only 19 electrons available to be accommodated in the 4^th and 5^th electron shells of the Silver (Ag) Bohr model. Thus, after placing 8 electrons in the Fourth shell (2 electrons in 4s and 6 electrons in 4p), 2 electrons can be accommodated in 5s and the remaining 9 electrons consequently go into 4d.

⇒ But the thing to remember is that a partially filled 4d subshell with nine electrons is less stable than a completely filled 4d subshell with ten electrons. So instead of a distribution of two electrons in 5s and nine electrons in 4d, there are ten electrons in 4d and only 1 electron in the 5s subshell of the Silver (Ag) atom.

⇒ In short, the Fourth electron shell of the Silver Bohr model contains a total of 18 electrons while the Fifth electron shell contains a single electron only.

So at this step of drawing the Silver Bohr model, we will place a total of 18 electrons in the Fourth electron shell, as shown below. The clockwise pattern of filling and then pairing electrons is strictly followed at this step as well.

7. Draw the Fifth electron shell

As a final step, the remaining 1 electron is placed at the top of the Fifth electron shell, as shown below.

Now, the 5th shell has only 1 electron.

In this way, we have the final representation of the Bohr model of the Silver (Ag) atom that contains 47 protons and 61 neutrons in the nucleus region while a total of 47 electrons circulate around the nucleus in specific orbits called shells.

The first electron shell of Silver has two electrons, there are eight electrons in the second shell, eighteen electrons in both the third and the fourth electron shells, and one electron in the fifth shell of Silver (Ag).

Also Read:-

• Scandium Bohr model
• Titanium Bohr model
• Vanadium Bohr model
• Oxygen Bohr model
• Boron Bohr model
• Beryllium Bohr model
• Lithium Bohr model
• Helium Bohr model
• Nitrogen Bohr model
• Fluorine Bohr model
• Neon Bohr model
• Carbon Bohr model
• Sodium Bohr model
• Silicon Bohr model
• Magnesium Bohr model
• Sulfur Bohr model
• Chlorine Bohr model
• Phosphorus Bohr model
• Aluminum Bohr model
• Argon Bohr model
• Potassium Bohr model
• Bromine Bohr model
• Calcium Bohr model
• Arsenic Bohr model
• Gold Bohr model
• Krypton Bohr model
• Iodine Bohr model
• Copper Bohr model
• Iron Bohr model
• Uranium Bohr model
• Nickel Bohr model

Also check :- Bohr model for all elements of Periodic table

FAQ

Summary

• The Bohr model of Silver (Ag) is drawn with five electron shells, the first shell contains 2 electrons, the second shell contains 8 electrons, the third and fourth electron shells contain 18 electrons each and the fifth electron shell has 1 electron only.
• The atomic number of Silver is 47. As Silver (Ag) is a neutral atom hence the number of protons and electrons available for its Bohr diagram are equal i.e., 47.
• The number of neutrons for the Bohr diagram of Silver can be found by subtracting the number of protons from the atomic mass (rounded off to the nearest whole number).
• The electron configuration of Silver in terms of the shells is [2,8,18,18,1] while in the standard form it is [Kr] 4d¹⁰ 5s¹.