How Many Electrons Does Potassium Have In Its Outside Electron Shell

Quantum Numbers – Physical Chemistry Which of the following sets of quantum numbers ( ) could correspond to a orbital? Possible Answers:

Correct answer:

Explanation : Since we’re looking at the orbital, we know, The range of possible values for is 0 to, Possible values for range to, Therefore, among the answer choices, is the only possible combination of quantum numbers corresponding to an orbital. Which of the following sets of quantum numbers could correspond to a orbital? Possible Answers:

Correct answer:

Explanation : Since we’re looking at the orbital, we know, The range of possible values for is 0 to, Possible values for range to, Therefore, among the answer choices,

is the only possible combination of quantum numbers corresponding to a orbital.

What can be concluded about the quantum numbers for potassium and potassium ion? Possible Answers: All valence electron(s) of potassium ion have a different orbital angular momentum quantum number than valence electron(s) of potassium Valence electron(s) of potassium ion have higher energy Valence electron(s) of potassium has a higher principal quantum number than valence electron(s) of potassium ion Correct answer: Valence electron(s) of potassium has a higher principal quantum number than valence electron(s) of potassium ion Explanation : Potassium has one valence electron.

This means that there is one electron in its outermost shell (4th shell).
Potassium ion, on the other hand, loses an electron and has a complete octet (has eight valence electrons) in its 3rd shell.
Recall that the principal quantum number signifies the shell.
Since the valence electron of potassium is found in the fourth shell,,

Similarly, the valence electrons of potassium ion are found in the third shell and for them. Valence electron of potassium has the higher principal quantum number. Orbital angular momentum number () is the second quantum number and it signifies the type of orbital.

It is always greater than or equal to zero.
There are four main types of orbital: s, p, d, and f,
Each orbital can hold two electrons.
In a given shell, there are one ‘ s ‘ orbital, three ‘ p ‘ orbitals, five ‘ d ‘ orbitals, and seven ‘ f ‘ orbitals.
L’ = 0 for ‘ s ‘ orbitals, ‘l’ = 1 for ‘ p ‘ orbitals, ‘l’ = 2 for ‘ d ‘ orbitals, and ‘l’ = 3 for ‘ f ‘ orbitals.

In potassium, there is only one valence electron; therefore, there is only one electron in the fourth shell and it can fit into the ‘s’ orbital. In potassium ion, there are eight valence electrons; therefore, two electrons can be found in the ‘ s ‘ orbital and the remaining six electrons can be found in the three ‘ p ‘ orbitals.

Consider the following descriptions of quantum numbers:
A: energy level within a subshell
B: shape of orbital
C: spin of electron
D: energy level

Which of the following is the correct pairing of quantum numbers (1st, 2nd, 3rd, and 4th) with the given descriptions? Possible Answers: A: 4th, B: 2nd, C: 3rd, D: 1st A: 3rd, B: 2nd, C: 4th, D: 1st A: 3rd, B: 4th, C: 2nd, D: 1st A: 2nd, B: 3rd, C: 4th, D: 1st Correct answer: A: 3rd, B: 2nd, C: 4th, D: 1st Explanation : There are four quantum numbers.

The first quantum, or principal quantum number, is designated by the letter ‘n’. It signifies the electron shell, or the energy level of the electron. The second quantum number, or orbital angular momentum quantum number, is designated by the letter ‘l’. It signifies the shape (or type) of the orbital.

The third quantum number, or magnetic quantum number, is designated by, This signifies the energy level within a subshell. Each orbital can be located in different orientations in space. For example, each of the three ‘p’ orbitals are oriented differently in space and have different energy levels.

The third quantum number describes this phenomenon.
Finally, the fourth quantum number, or spin quantum number, is designated by and describes the spin of the electron.
An electron can spin clockwise or counterclockwise.
Describes the direction of the spin.
Since an electron can only rotate two ways, can only be two values or,

These four numbers together describe the potential location of an electron inside an atom. Note that no two electrons can have the same set of quantum numbers (meaning at least one of the four numbers will be different). Which of the following is true regarding ethene? (The electrons in answer choices refer to carbon electrons) Possible Answers: The electrons in bond have the same set of quantum numbers The electrons in the bonds and the bond have different principal quantum number The electrons in the bond have the same orbital angular momentum number The electrons in the bonds have the same set of quantum numbers Correct answer: The electrons in the bond have the same orbital angular momentum number Explanation : Ethene, or, has a carbon-carbon single () and double () bond.

Recall that a bond can be found in hybridized orbitals whereas a bond cannot. This means that the carbon atoms in ethene hybridize the single ‘ s ‘ orbital and two of the ‘ p ‘ orbitals, forming a hybridization. The bonds () are found in these three hybridized orbitals. The remaining unhybridized ‘ p ‘ orbital will house the two electrons in the bond.

The orbital angular momentum number is the second quantum number and it signifies the type of orbital. An electron found in a ‘ p ‘ orbital will always have an, Since both electrons in the bond are found in the ‘p’ orbital, the ‘l’ value for both electrons is the same.

Which of the following is/are true regarding the principal quantum number?
I. Principal quantum number signifies the energy level
II. Principal quantum number can never equal zero
III. Principal quantum number can be positive or negative

Possible Answers: Explanation : Quantum numbers are fancy coordinate systems that describe the potential location of an electron within an atom. The first quantum number is called the principal quantum number and it signifies the shell the electron is located in.

Recall that electron shells are discrete orbits in an atom that have discrete energy; therefore, the principal quantum number signifies the energy level of an electron.
The principal quantum number is always an integer and is always greater than zero.
If the electron is found within the first shell, if then the electron is found within the second shell, and so and and so forth.

Also, since it is always greater than zero, the principal quantum number can never be negative. How many subshells are there with n = 4 in an atom? Possible Answers: Correct answer: Explanation : The types of subshells, from smallest to largest, are as follows: s, p, d, and f,

n =4
l =2
m =-3

Explanation : The principle quantum number ( n ) and the angular quantum number ( l ) are acceptable. However, the magnetic quantum number ( m ) is restricted to lie between – l and l, Therefore, for l =2, the only possible numbers for m are -2, -1, 0, 1, 2.

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Contents

0.1 How many electrons does potassium have on its outer shell?
0.2 How many electrons are on the outside shell?

1 Why does potassium have only 8 electrons in 3rd shell?
- - 1.0.1 Why does potassium have only 8 electrons in M shell?
  - 1.0.2 Why is it 2 8 8 1 and not 2 8 9?
2 Why do shells start with K?
- 2.1 Does potassium follow the octet rule?
  - 2.1.1 What is the K shell?
- 2.2 Does the outer shell have 2 electrons?
  - 2.2.1 Does potassium have 4 electron shells?
3 Does a potassium atom one electron in its outer level?
- - 3.0.1 How many electrons do potassium sodium and lithium have in their outer shell?
4 Is the 3rd shell 8 or 18?
- - 4.0.1 Does K+ have 8 valence electrons?
5 Why can the K shell only hold 2 electrons?
- - 5.0.1 Which shell can hold 8 electrons?
- 5.1 Can no outer shell contain more than 8 electrons?
6 What element has 8 electron shells?
- - 6.0.1 Why does the K shell only have 2 electrons?
- 6.1 What elements have 7 electrons in outer shell?
7 How does potassium get a full outer shell?
- - 7.0.1 Which element has 2 electrons in K shell?

How many electrons does potassium have on its outer shell?

Answer (Detailed Solution Below) – Option 1 : One

The Potassium has one electron in its outer shell. Atomic Symbol – K, Atomic Number-19. The full electronic configuration of potassium is 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1, It has 19 electrons and 19 protons with one valence electron in the outer shell. Metals can have a valency of 1,2 or 3 only. It has a very low melting point. It is the second least dense metal after lithium. It reacts violently when coming in contact with water because it is a very reactive metal. Potassium chloride is used to make fertilizers. It was first isolated by English chemist Sir Humphry Davy in 1807.

Get proficient with the General Science concepts with detailed lessons on the topic Chemistry among many others.

How many electrons are on the outside shell?

Subshells and orbitals – The Bohr model is useful to explain the reactivity and chemical bonding of many elements, but it actually doesn’t give a very accurate description of how electrons are distributed in space around the nucleus. Specifically, electrons don’t really circle the nucleus, but rather spend most of their time in sometimes-complex-shaped regions of space around the nucleus, known as electron orbitals,

We can’t actually know where an electron is at any given moment in time, but we can mathematically determine the volume of space in which it is most likely to be found—say, the volume of space in which it will spend 90% of its time.
This high-probability region makes up an orbital, and each orbital can hold up to two electrons.

So, how do these mathematically defined orbitals fit in with the electron shells we saw in the Bohr model? We can break each electron shell down into one or more subshells, which are simply sets of one or more orbitals. Subshells are designated by the letters s, p, d, and f, and each letter indicates a different shape.

For instance, s subshells have a single, spherical orbital, while p subshells contain three dumbbell-shaped orbitals at right angles to each other.
Most of organic chemistry—the chemistry of carbon-containing compounds, which are central to biology—involves interactions between electrons in s and p subshells, so these are the most important subshell types to be familiar with.

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However, atoms with many electrons may place some of their electrons in d and f subshells. Subshells d and f have more complex shapes and contain five and seven orbitals, respectively. The first electron shell, 1n, corresponds to a single 1, s orbital.

The 1, s orbital is the closest orbital to the nucleus, and it fills with electrons first, before any other orbital.
Hydrogen has just one electron, so it has a single spot in the 1, s orbital occupied.
This can be written out in a shorthand form called an electron configuration as 1, s, start superscript, 1, end superscript, where the superscripted 1 refers to the one electron in the 1, s orbital.

Helium has two electrons, so it can completely fill the 1, s orbital with its two electrons. This is written out as 1, s, squared, referring to the two electrons of helium in the 1, s orbital. On the periodic table, hydrogen and helium are the only two elements in the first row, or period, which reflects that they only have electrons in their first shell.

Hydrogen and helium are the only two elements that have electrons exclusively in the 1, s orbital in their neutral, non-charged, state.
The second electron shell, 2n, contains another spherical s orbital plus three dumbbell-shaped p orbitals, each of which can hold two electrons.
After the 1, s orbital is filled, the second electron shell begins to fill, with electrons going first into the 2, s orbital and then into the three p orbitals.

Elements in the second row of the periodic table place their electrons in the 2n shell as well as the 1n shell. For instance, lithium ( start text, L, i, end text ) has three electrons: two fill the 1, s orbital, and the third is placed in the 2, s orbital, giving an electron configuration of 1, s, squared 2, s, start superscript, 1, end superscript,

Neon ( start text, N, e, end text ), on the other hand, has a total of ten electrons: two are in its innermost 1, s orbital and eight fill the second shell—two each in the 2, s and three p orbitals, 1, s, squared 2, s, squared 2, p, start superscript, 6, end superscript, Because its 2n shell is filled, it is energetically stable as a single atom and will rarely form chemical bonds with other atoms.

The third electron shell, 3n, also contains an s orbital and three p orbitals, and the third-row elements of the periodic table place their electrons in these orbitals, much as second-row elements do for the 2n shell. The 3n shell also contains a d orbital, but this orbital is considerably higher in energy than the 3, s and 3, p orbitals and does not begin to fill until the fourth row of the periodic table.

This is why third-row elements, such as argon, can be stable with just eight valence electrons: their s and p subshells are filled, even though the entire 3n shell is not.
While electron shells and orbitals are closely related, orbitals provide a more accurate picture of the electron configuration of an atom.

That’s because orbitals actually specify the shape and position of the regions of space that electrons occupy.

Why does potassium have only 8 electrons in 3rd shell?

Free Child Development and Pedagogy Mock Test 10 Questions 10 Marks 10 Mins The correct answer is K and Ar, Explanation:

Potassium (K):

Potassium is a chemical element with the atomic number 19 and the symbol K. Potassium has an extra shell of electrons, resulting in 8 more electrons in the third shell. This extra shell of electrons protects the outer electron from the nucleus’s attractive force. As a result, less energy is required to remove potassium’s outer electron, making it more reactive.

So, Potassium (K) having 8 electrons in the third shell is very reactive,

Argon:

Argon is a noble or inert gas with the atomic number 18 and the symbol Ar. Argon is inactive (non-reactive) because in the third shell 8 electrons are present. When the elements react, their atoms complete their outer shells by losing, gaining, or sharing electrons. Noble gas (Argon) atoms have complete outer shells and do not lose, gain, or share electrons.

So, Argon (Ar) having 8 electrons in the third shell is very inactive, Thus, K having 8 electrons in the third shell is very reactive while the Ar having 8 electrons in the third shell is very inactive. Last updated on Apr 10, 2023 The CG TET Revised Results were released on January 17, 2023! The CG TET Answer Key (Provisional) for the exam conducted on September 18th, 2022 has been released.

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Why does potassium have only 8 electrons in M shell?

The presence of 8 electrons in the outermost shell makes the atom very stable. Due to this rule the shells M and N which have the capacity to hold more than eight electrons are allowed to hold only 8 electrons.

Why is it 2 8 8 1 and not 2 8 9?

According to octet rule, the outermost shell of an atom can accommodate maximum 8 electrons (except K shell which can accommodate maximum 2 electrons). Hence, the electronic configuration of potassium is 2,8,8,1 and not 2,8,9.

Why do shells start with K?

Why is the first shell called K shell? Join Vedantu’s FREE Mastercalss Answer Verified Hint : We know that the characteristics of an orbital are expressed in terms of Quantum numbers. These quantum numbers help in getting the complete information about all the electrons in an atom.

Complete Step By Step Answer: Note :

Among these Quantum numbers principal quantum number (n) is the most important one it tells about the shell to which the electron belongs. It also explains the main lines of the spectrum on the basis of the electronic jumps between these shells. The various principal energy shells are designated by the letters K, L, M, N, O, Petc.The first shell is known as K shell.A Spectroscopist, Charles G.

Barkla gave the names to the electron shells. He studied the X-rays that were emitted by atoms when they hit the high energy electrons. He concluded that atoms appeared to emit two types of X-rays. These X-rays differ in energy and Charles originally called the higher energy X-ray type A and the lower energy X-rays type B.

He later renamed these two to K and L since he realized that the highest energy X-rays produced in his experiment might not be the highest energy X-rays possible. It later turned out that K has the highest energy possible. Thus, the innermost shell was called the K- shell.

Does potassium follow the octet rule?

Potassium is an exception to the octet rule and can hold up to 12 electrons in its valence electron energy level in a compound.

What is the K shell?

: the innermost shell of electrons surrounding an atomic nucleus and constituting the lowest available energy level for the electrons compare l-shell, m-shell

Does the outer shell have 2 electrons?

Elements of group II have two electrons in their outermost shells. So, Magnesium, Calcium, and Strontium are the 3 elements that have two electrons in their outermost orbit. Was this answer helpful?

Does potassium have 4 electron shells?

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Page ID 49249 On a chemical level, an important clue to the unraveling of the electronic structure of atoms is the existence of noble gases, which are almost completely unable to form chemical compounds. This lack of reactivity suggests that the atoms of these elements have structures which do not permit interaction with the structures of other atoms.

A second clue is the close correspondence between the valence of an element and the extent to which its atomic number differs from that of the nearest noble gas.
Elements which have a valence of 1, for instance, have atomic numbers one more or one less than that of a noble gas.
Thus the atoms of the alkali metals Li, Na, K, Rb, and Cs all contain one electron more than the corresponding noble gases He, Ne, Ar, Kr, and Xe, while atoms of hydrogen H and the halogens F, Cl, Br, and I all contain one electron less.

Similar remarks apply to a valence of 2, The alkaline-earth metal atoms Be, Mg, Ca, Sr, and Ba all contain two electrons more than a noble-gas atom, while the elements O, S, Se, and Te all contain two electrons less. Exactly the same pattern of behavior also extends to elements with a valence of 3 or 4.

As early as 1902, Lewis began to suggest (in his lectures to general chemistry students, no less) that the behavior just described could be explained by assuming that the electrons in atoms were arranged in shells, all electrons in the same shell being approximately the same distance from the nucleus.

The pictures which he eventually developed for helium, chlorine, and potassium atoms are illustrated below. In the helium atom the two electrons occupy only one shell, in the chlorine atom the 17 electrons are arranged in three shells, and in the potassium atom the 19 electrons occupy four shells.

Lewis suggested that each shell can only accommodate so many electrons. Once this number has been reached, the shell must be regarded as filled, and any extra electrons are accommodated in the next shell, somewhat farther from the nucleus. Once a shell is filled, moreover, it is assumed to have a particularly stable structure which prevents the electrons in the shell from any involvement with other atoms.

Thus it is only the electrons in the outermost incompletely filled shell (called valence electrons ) that have any chemical importance. Furthermore, if the outermost shell is filled, then the resulting atom will have little or no tendency to react with other atoms and form compounds with them. Figure \(\PageIndex \) The shell structure of atoms of He, Cl, and K, as suggested by Lewis. Note the valence electrons are in red. Helium has one shell filled by two red dots. Chlorine has 2 red dots on its inner most shell, followed by 8 red dots on the next shell.

The outer most shell has 7 red dots. Potassium has 2 dots on its inner most shell followed by 8 red dots respectively for the next two shells. The outermost shell has 1 red dot. Assuming that the noble gases all contain an outermost filled shell, it is now quite simple to work out how many electrons can be accommodated in each shell.

Since the first noble gas helium has two electrons, we know that only two electrons are needed to fill the first shell. A further eight electrons brings us to the next noble gas neon ( Z = 10). Accordingly we deduce that the second shell can accommodate a maximum of eight electrons.

Does a potassium atom one electron in its outer level?

A neutral atom of potassium has one electron in its outer level. This is not a stable outer energy level. When potassium forms a compound with iodine, potassium loses one electron from its fourth level, and the third level becomes a complete outer level. The potassium atom has become an ion.

How many electrons do potassium sodium and lithium have in their outer shell?

Examples –

All the Group 1 elements – lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr) – have one electron in the outer shell.
The Group 7 elements – fluorine (F), chlorine (Cl), bromine (Br), iodine (I) and astatine (At) – have seven electrons in the outer shell.
Group 0 elements – helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe) and radon (Rn) – have full outer shells. (Group 0 is sometimes called Group 8 ).

Is the 3rd shell 8 or 18?

The third shell holds 18 electrons ; 2 in a 3s orbital; 6 in three 3p orbitals; and 10 in five 3d orbitals. The fourth shell holds 32 electrons; 2 in a 4s orbital; 6 in three 4p orbitals; 10 in five 4d orbitals; and 14 in seven 4f orbitals.

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Does K+ have 8 valence electrons?

Quantum Numbers – Physical Chemistry Which of the following sets of quantum numbers ( ) could correspond to a orbital? Possible Answers:

Correct answer:

Explanation : Since we’re looking at the orbital, we know, The range of possible values for is 0 to, Possible values for range to, Therefore, among the answer choices,

is the only possible combination of quantum numbers corresponding to a orbital.

This means that there is one electron in its outermost shell (4th shell).
Potassium ion, on the other hand, loses an electron and has a complete octet (has eight valence electrons) in its 3rd shell.
Recall that the principal quantum number signifies the shell.
Since the valence electron of potassium is found in the fourth shell,,

It is always greater than or equal to zero.
There are four main types of orbital: s, p, d, and f,
Each orbital can hold two electrons.
In a given shell, there are one ‘ s ‘ orbital, three ‘ p ‘ orbitals, five ‘ d ‘ orbitals, and seven ‘ f ‘ orbitals.
L’ = 0 for ‘ s ‘ orbitals, ‘l’ = 1 for ‘ p ‘ orbitals, ‘l’ = 2 for ‘ d ‘ orbitals, and ‘l’ = 3 for ‘ f ‘ orbitals.

Consider the following descriptions of quantum numbers:
A: energy level within a subshell
B: shape of orbital
C: spin of electron
D: energy level

The first quantum, or principal quantum number, is designated by the letter ‘n’.
It signifies the electron shell, or the energy level of the electron.
The second quantum number, or orbital angular momentum quantum number, is designated by the letter ‘l’.
It signifies the shape (or type) of the orbital.

The third quantum number describes this phenomenon. Finally, the fourth quantum number, or spin quantum number, is designated by and describes the spin of the electron. An electron can spin clockwise or counterclockwise. describes the direction of the spin. Since an electron can only rotate two ways, can only be two values or,

Recall that a bond can be found in hybridized orbitals whereas a bond cannot. This means that the carbon atoms in ethene hybridize the single ‘ s ‘ orbital and two of the ‘ p ‘ orbitals, forming a hybridization. The bonds () are found in these three hybridized orbitals. The remaining unhybridized ‘ p ‘ orbital will house the two electrons in the bond.

Which of the following is/are true regarding the principal quantum number?
I. Principal quantum number signifies the energy level
II. Principal quantum number can never equal zero
III. Principal quantum number can be positive or negative

Recall that electron shells are discrete orbits in an atom that have discrete energy; therefore, the principal quantum number signifies the energy level of an electron.
The principal quantum number is always an integer and is always greater than zero.
If the electron is found within the first shell, if then the electron is found within the second shell, and so and and so forth.

n =4
l =2
m =-3

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Why can the K shell only hold 2 electrons?

Inorganic Chemistry (Atomic Structure) The key factor determining the chemical properties of each element is the configuration of its electrons. Likewise, the energy associated with atoms and molecules is a function of their electrons. Think of the atom; it has a positively charged nucleus with negatively charged electrons orbiting the nucleus.

Just like the opposite poles of a magnet, oppositely charged particles attract each other.
Because of these attractive forces, it requires energy to pull them apart.
In an atom, electrons can be moved further away from the nucleus, but only if energy of some form is applied.
Likewise when electrons move closer to the nucleus energy can be released.

When I was a kid, we wore fluorescent masks at Halloween. We would shine light on them to “charge” the mask and then when the lights were turned off they would glow or fluoresce. At the time I didn’t know how they worked, I just knew they were fun. Now I know that the light, which is electromagnetic radiation, has energy that can be used to push electrons into orbitals further from the nucleus.

When the light is turned off, the electrons “fall” back down into a lower orbital releasing energy, which caused the mask to glow in the dark. As was mentioned above, the electrons of the atom are located in orbitals, From our discussion above we learned that the energy associated with the electrons in an atom is a function of its position or distance from the nucleus.

Therefore, electrons in orbitals close to the nucleus posses less energy than electrons in orbitals that are further away from the nucleus. Another important property of orbitals is that each orbital can hold a maximum of 2 electrons. Based on the amount of energy in each orbital they are arranged into what are referred to as electron shells or energy shells, which contain one or more orbitals.

All of the electrons in a given electron shell have the same amount of energy.
To accommodate the electrons in the largest of the naturally occurring elements, seven electron shells are required.
However, most biologically important molecules are considerably smaller, so we will only be dealing with the first three energy shells as we discuss electron configuration.

The first shell can only accommodate one orbital, thus the maximum number of electrons in the first electron shell is two. The second and third shells each contain four orbitals and can therefore accommodate 8 electrons each. (For those who have or will take more chemistry, I should point out that the third energy shell has more than four orbitals.

However, for reasons beyond the scope of this class we can ignore the other orbitals.) One other important fact is that as electrons are added to electron shells, they occupy the innermost shells first before filling the outer shells.
It’s like parking spaces at Walmart; those closest to the store fill first, and once they are filled shoppers have no choice but to park in spaces further away.

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For example, hydrogen has one electron which is located in the first (innermost) electron shell. Helium has two electrons, both in the first energy shell. All of the space in the first energy shell is now filled. Lithium has 3 electrons, two of them are in the first shell and the third electron is in the second electron shell.

The reason that this is important to know is because the chemical properties of an element are determined by the number of electrons in its outer electron shell,
We define the “outer electron shell” as the last shell that has electrons in it, so for hydrogen, its outer electron shell would be the first shell, and for lithium its outer shell would be the second shell.

Each of these elements has one electron in its outer shell, which means that they will have similar chemical properties. So, let’s try an example. Oxygen has an atomic number of 8, which means it has 8 protons and 8 electrons. How many electrons are there in the outer electron shell of oxygen? The first two electrons will go into the first shell leaving 6 to go into the second shell. image created by BYU-I student Hannah Crowder Fall 2013 The image above represents the electron configuration for carbon. Carbon has an atomic number of 6, hence 6 electrons. The first two electrons fill the first shell (dark blue) and the next 4 are in the second shell (light blue).

Which shell can hold 8 electrons?

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Skills to Develop

To describe how electrons are grouped within atoms.

Although we have discussed the general arrangement of subatomic particles in atoms, we have said little about how electrons occupy the space about the nucleus. Do they move around the nucleus at random, or do they exist in some ordered arrangement? The modern theory of electron behavior is called quantum mechanics. It makes the following statements about electrons in atoms:

Electrons in atoms can have only certain specific energies. We say that the energies of the electrons are quantized.
Electrons are organized according to their energies into sets called shells. Generally the higher the energy of a shell, the farther it is (on average) from the nucleus. Shells do not have specific, fixed distances from the nucleus, but an electron in a higher-energy shell will spend more time farther from the nucleus than does an electron in a lower-energy shell.
Shells are further divided into subsets of electrons called subshells. The first shell has only one subshell, the second shell has two subshells, the third shell has three subshells, and so on. The subshells of each shell are labeled, in order, with the letters s, p, d, and f, Thus, the first shell has only an s subshell, the second shell has an s and a p subshell, the third shell has s, p, and d subshells, and so forth.
Different subshells hold a different maximum number of electrons. Any s subshell can hold up to 2 electrons; p supshell up to 6 electrons; d subshell up to 10; and f subshell up to 14.

It is the arrangement of electrons into shells that has the most effect on chemical properties, so we will focus on mainly on shells here. We use numbers to indicate which shell an electron is in. The first shell, closest to the nucleus and with the lowest-energy electrons, is shell 1.

This first shell has only one subshell (labeled 1s) and can hold a maximum of 2 electrons. This is why there are two elements in the first row of the periodic table (H & He). Because the first shell can only hold a maximum of 2 electrons, the third electron must go into the second shell. Therefore the lithium (Li), which has three total electrons, will have two electrons in the first shell and one electron in the second shell.

Notice that lithium is the first element in the second row of the periodic table. The second shell has two subshells (labeled 2 s and 2 p). The 2 s subshell holds a maximum of 2 electrons, and the 2 p subshell holds a maximum of 6 electrons. This means that the second shell can hold a maximum of eight electrons (2+6=8).

Notice that there are eight elements in the second row of the periodic table.
It is only the electrons in the outer-most shell, called the VALENCE shell, that tend to react (be gained, lost, or shared).
You might imagine that, if two atoms bumped into each other, it would be the outer electrons that would interact first.

The following is a list of total electrons, electrons by shell, and valence electrons for the first 10 elements.

Hydrogen has 1 electron in the first shell (so one valence electron).
Helium has 2 electrons – both in the first shell (so two valence electrons).
Lithium has 3 electrons – 2 in the first shell, and 1 in the second shell (so one valence electron).
Beryllim has 4 electrons – 2 in the first shell, and 2 in the second shell (so two valence electrons).
Boron has 5 electrons – 2 in the first shell, and 3 in the second shell (so three valence electrons).
Carbon has 6 electrons – 2 in the first shell, and 4 in the second shell (so four valence electrons).
Nitrogen has 7 electrons – 2 in the first shell, and 5 in the second shell (so five valence electrons).
Oxygen has 8 electrons – 2 in the first shell, and 6 in the second shell (so six valence electrons).
Fluorine has 9 electrons – 2 in the first shell, and 7 in the second shell (so seven valence electrons).
Neon has 10 electrons – 2 in the first shell, and 8 in the second shell (so eight valence electrons).

Figure 2.6.1 below lists the atomic number for the main group elements. The atomic number defines the number of protons in the nucleus of each atom. For neutral atoms, the number of positive protons will equal the total number of negative electrons (zero net charge). For example, bromine (Br) has 35 protons and 35 total electrons. Periodic tables always list the atomic number. Figure 2.6.1 – Atomic Number for Each of the Main Group Elements The number of valence electrons for each main group element can be determined by the column, or group, it occupies on the periodic table. Table 2.6.2 below summarizes the number of valence electrons for each main group column of elements.

For example, the elements in the first column (sometimes labeled IA), all have one valence electron.
The second column (IIA) has two valence electrons.
We skip the short block of ten elements in the middle because this is where a subshell fills out of order.
The elements in columns IIIA, IVA, VA, VIA, and VIIA, and VIIIA* have three, four, five, six, seven, and eight* valence electrons, respectively.

*Note that helium (He) only has two valence electrons. Some periodic tables place helium in column IIA, others place it in VIIIA, and some in both locations. Figure 2.6.2 – Number of Valence Electrons for Main Group Elements Example \(\PageIndex \): Electrons of Phosphorus How many total and valence electrons are in a neutral phosphorus atom? SOLUTION A neutral phosphorus atom has 15 total electrons. Two electrons can go into first shell, eight in the second shell, and it has five more in the third shell.

The third shell is the outer valence shell, so it has 5 valence electrons.
The number of electrons in each shell becomes more complicated as more electrons are added because there are more subshells being used and because the shell start to fill out of order.
For elements with larger atomic number than 20 (beyond calcium), we will just focus on how many total and how many valence electrons, not the number in each shell.

We have stated that the outer-shell electrons are called valence. The inner (non-valence) shells and electrons are often called the core. Example \(\PageIndex \): Counting total and Valence Electrons in Xenon How many total, valence, and core electrons are there in a neutral xenon atom? SOLUTION Xenon has 54 total, 8 valence, and 46 core electrons.

Can no outer shell contain more than 8 electrons?

The octet rule states that atoms with 8 electrons in their outer shell are stable. Thus, even if the shell has the capacity to hold more electrons, it does not have more than 8 electrons. If the outermost shell holds up more than 8 electros, the atom becomes unstable.

What element has 8 electron shells?

Electrons In The Shells – Take a look at the picture below. Each of those colored balls is an, In an atom, the electrons spin around the center, also called the, The electrons like to be in separate shells/orbitals, Shell number one can only hold 2 electrons, shell two can hold 8, and for the first eighteen elements shell three can hold a maximum of eight electrons.

As you learn about elements with more than eighteen electrons you will find that shell three can hold more than eight. Once one shell is full, the next electron that is added has to move to the next shell. So. for the element of OXYGEN, you already know that the atomic number tells you the number of electrons.

That means there are 8 electrons in an oxygen atom. Looking at the picture, you can see there are two electrons in shell one and six in shell two.

This is a water molecule. Even though you find complex names on other molecules, everyone calls H 2 O “water”. Water is made up of two hydrogen (H) atoms and one oxygen (O) atom. The formula for water is H 2 O, The hydrogen atoms have filled orbitals with two electrons and the oxygen atom is filled with eight electrons.

Two lithium (Li) atoms can bond with one oxygen (O) atom, making the formula Li 2 O, Oxygen likes to have two additional electrons to make it happy. Each lithium atom provides one. You can see that the Oxygen atom has eight electrons (6 of its own, and one from each lithium), and the two lithium atoms have two electrons each.

Two hydrogen (H) atoms can also bond with two oxygen (O) atoms, making the formula H 2 O 2, That’s just one more oxygen than water, but it is a totally different compound. You can see that each of the Oxygen atoms has eight electrons, and the two Hydrogens have two electrons each. See how the electrons are shared?

Chem4Kids.com: Oxygen: Orbital and Bonding Info

Why does the K shell only have 2 electrons?

The number 2 comes from their only being 2 spin states and each member of the pair must be in a different state than the other. The solutions to the Schroedinger equation entail a number of integers. The first integer is referred as to the shell number or primary quantum number.

What elements have 7 electrons in outer shell?

Examples –

All the Group 1 elements – lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr) – have one electron in the outer shell.
The Group 7 elements – fluorine (F), chlorine (Cl), bromine (Br), iodine (I) and astatine (At) – have seven electrons in the outer shell.
Group 0 elements – helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe) and radon (Rn) – have full outer shells. (Group 0 is sometimes called Group 8 ).

How does potassium get a full outer shell?

Therefore electrons are transferred from potassium to sulphur as metals must lose electrons to gain a full outer shell. Two potassium atoms each lose one electron, as each atom only has one electron to lose in its outer shell. This forms K+ ions, each with a 1+ charge. One sulphur atom can gain 2 electrons.

Which element has 2 electrons in K shell?

Since the electrons in atoms are filled in the lower orbits first and then in higher energy orbits, all the atoms except for hydrogen will have two electrons in its ‘K’ shell as they will have more than two electrons (K shell cannot contain more than two electrons according to 2n2 rule).

Skye Skinner