Chemistry: Fill in the orbital diagrams and write the electron configuration for the following elements.

Step-by-step explanation: Cu(29)= 1s2 2s2 2p63s23p64s13d10 , Actually Cu is an exception of Auf bau...

Fill in the orbital diagrams and write the electron, №15255719, 31.03.2020 11:50

Chemistry

1. explain the relevance of the conductivity lab to the relevance of the subject of chemistry. - 2. using the periodic table, discuss the importance of the unique group and period location of sodium and chlorine. classify each element as either a metal or a non-metal, and use these classifications to explain their likely behavior for losing or gaining electrons, in terms of their ionization energy or electronegativity, forming cations or anions respectively. - 3. using the aeld, illustrate the atomic structure of the sodium and chlorine atoms,

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P Answered by Master

9

I'm your teacher(Mr.Lopez) and I know that you are cheating.

See me after class.

By the way this is one of the answers.

12. Write the electron configuration of the sodium ion (Na+1) and the chloride ion (Cl-1).

[Ne]3s^1

[Ne]3s^2 3p^5

Chemistry

1. explain the relevance of the conductivity lab to the relevance of the subject of chemistry. - 2. using the periodic table, discuss the importance of the unique group and period location of sodium and chlorine. classify each element as either a metal or a non-metal, and use these classifications to explain their likely behavior for losing or gaining electrons, in terms of their ionization energy or electronegativity, forming cations or anions respectively. - 3. using the aeld, illustrate the atomic structure of the sodium and chlorine atoms,

Step-by-step answer

P Answered by Master

9

I'm your teacher(Mr.Lopez) and I know that you are cheating.

See me after class.

By the way this is one of the answers.

12. Write the electron configuration of the sodium ion (Na+1) and the chloride ion (Cl-1).

[Ne]3s^1

[Ne]3s^2 3p^5

Chemistry

The electron configuration can also be represented by writing the symbol for the occupied subshell and adding a superscript to indicate the number of electrons in that subshell. for example, consider a carbon atom having an atomic number of 6. the total number of electrons in a neutral carbon atom is 6. the electron configuration of the carbon atom represented by the orbital diagram is this electron configuration can be written as 1s22s22p2 use the rules for determining electron configurations to write the electron configuration for p . express

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P Answered by PhD

2

the electron configuration for P iin complete form in order of increasing orbital energy is: 1s² 2s² 2p⁶ 3s² 3p³

Explanation:

As stated, writing the symbol for the occupied subshell and adding a superscript to indicate the number of electrons in that subshell is a common way to represent the electron configuration of the atoms.

There are several rules that you have to follow to write such electron configurations. I will explain the needed to write the electron configuration for the atoms of P (phosphorus) in the requested form.

1) First, determine the number of electrons of the atom:

Use the atomic number. Phosphorus has atomic number 15.The atomic number is the number of protons. So, phosphorus has 15 protons.A neutral atom has the same number of electrons than protons. So, phosphorus atoms have 15 electrons.

2) Fill the orbitals in order of incrasing orbital energy

Aufbau rules are very helpful. As per it this is the order of the orbitals:

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ ...

15 electrons ⇒ 1s² 2s² 2p⁶ 3s² 3p³Check the number of electrons: 2 + 2 + 6 + 2 + 3 = 15Hence, that is the electron configuration for P iin complete form in order of increasing orbital energy.

3) Other rules that you must consult to deal with some special issues of the electron configurations are: the exclusion principle of Pauli and the Hund's rule, but they are beyond the interest of this question.

Chemistry

The electron configuration can also be represented by writing the symbol for the occupied subshell and adding a superscript to indicate the number of electrons in that subshell. for example, consider a carbon atom having an atomic number of 6. the total number of electrons in a neutral carbon atom is 6. the electron configuration of the carbon atom represented by the orbital diagram is this electron configuration can be written as 1s22s22p2 use the rules for determining electron configurations to write the electron configuration for p . express

Step-by-step answer

P Answered by PhD

2

the electron configuration for P iin complete form in order of increasing orbital energy is: 1s² 2s² 2p⁶ 3s² 3p³

Explanation:

As stated, writing the symbol for the occupied subshell and adding a superscript to indicate the number of electrons in that subshell is a common way to represent the electron configuration of the atoms.

There are several rules that you have to follow to write such electron configurations. I will explain the needed to write the electron configuration for the atoms of P (phosphorus) in the requested form.

1) First, determine the number of electrons of the atom:

Use the atomic number. Phosphorus has atomic number 15.The atomic number is the number of protons. So, phosphorus has 15 protons.A neutral atom has the same number of electrons than protons. So, phosphorus atoms have 15 electrons.

2) Fill the orbitals in order of incrasing orbital energy

Aufbau rules are very helpful. As per it this is the order of the orbitals:

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ ...

15 electrons ⇒ 1s² 2s² 2p⁶ 3s² 3p³Check the number of electrons: 2 + 2 + 6 + 2 + 3 = 15Hence, that is the electron configuration for P iin complete form in order of increasing orbital energy.

3) Other rules that you must consult to deal with some special issues of the electron configurations are: the exclusion principle of Pauli and the Hund's rule, but they are beyond the interest of this question.

Chemistry

Write the electron configuration, orbital filling diagram, and shorthand notation for gallium

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P Answered by Specialist

1

Electron configuration-
$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4s^{2} 3d^{10} 4p^{1}$

Shorthand notation-
[Ar] $4s^{2} 3 d^{10} 4p^{1}$

And I can't really show it the orbital filling diagram, but it would look exactly like your last problem except the 4p orbital would have one "half" arrow on the first line pointing upwards

Hope this helps!

Chemistry

Write the electron configuration, orbital filling diagram, and shorthand notation for gallium

Step-by-step answer

P Answered by Master

1

Electron configuration-
$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4s^{2} 3d^{10} 4p^{1}$

Shorthand notation-
[Ar] $4s^{2} 3 d^{10} 4p^{1}$

And I can't really show it the orbital filling diagram, but it would look exactly like your last problem except the 4p orbital would have one "half" arrow on the first line pointing upwards

Hope this helps!

Chemistry

PLEASE HELP! Write the full electron configuration for phosphorus, atomic symbol P, then draw an orbital box diagram that accounts for all of the electrons in phosphorus. You don’t need to include the orbital box diagram as part of your answer. Based on your drawing, explain why phosphorus is either paramagnetic or diamagnetic.

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P Answered by PhD

13

1) The full electron configuration for phosphorus is 1s²2s²2p⁶3s²3p

2) Phosphorus is paramagnetic

Explanation:

1) To write the electron configuration, we follow the electron filling order, that is starting from 1s, to 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4f, 5s, 5p, 5d, 6s till the electrons are all accounted for (up to 58)

We note that the s orbitals can each take two electrons while the p orbital can take 6 electrons and the d orbital can take 10 electrons

The electron configuration chart for phosphorus, P, is given as follows;

1s²2s²2p⁶3s²3p.

2) Diamagnetism is the temporary magnetism is the magnetism of a material that exists in the presence of a magnetic field due to a a change in the atomic electron orbital motion

Paramagnetism is a magnetism in which a material is weakly attracted by an applied external magnetic field such that there is induced magnetism in the applied magnetic field direction

Paramagnetic materials have have unpaired electrons that give them permanent magnetic moments in the absence of an applied magnetic field as such unpaired electrons are termed paramagnetic electrons and atoms that have one or more unpaired electrons are paramagnetic

Phosphorus, with the 3 partially filled p orbitals have 3 unpaired electrons in their outermost shell giving them the overall properties of a paramagnetic materials.

Chemistry

PLEASE HELP! Write the full electron configuration for phosphorus, atomic symbol P, then draw an orbital box diagram that accounts for all of the electrons in phosphorus. You don’t need to include the orbital box diagram as part of your answer. Based on your drawing, explain why phosphorus is either paramagnetic or diamagnetic.

Step-by-step answer

P Answered by PhD

13

1) The full electron configuration for phosphorus is 1s²2s²2p⁶3s²3p

2) Phosphorus is paramagnetic

Explanation:

1) To write the electron configuration, we follow the electron filling order, that is starting from 1s, to 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4f, 5s, 5p, 5d, 6s till the electrons are all accounted for (up to 58)

We note that the s orbitals can each take two electrons while the p orbital can take 6 electrons and the d orbital can take 10 electrons

The electron configuration chart for phosphorus, P, is given as follows;

1s²2s²2p⁶3s²3p.

2) Diamagnetism is the temporary magnetism is the magnetism of a material that exists in the presence of a magnetic field due to a a change in the atomic electron orbital motion

Paramagnetism is a magnetism in which a material is weakly attracted by an applied external magnetic field such that there is induced magnetism in the applied magnetic field direction

Paramagnetic materials have have unpaired electrons that give them permanent magnetic moments in the absence of an applied magnetic field as such unpaired electrons are termed paramagnetic electrons and atoms that have one or more unpaired electrons are paramagnetic

Phosphorus, with the 3 partially filled p orbitals have 3 unpaired electrons in their outermost shell giving them the overall properties of a paramagnetic materials.

Chemistry

HELP PLZZZ Write the full electron configuration for phosphorus, atomic symbol P, then draw an orbital box diagram that accounts for all of the electrons in phosphorus. You don’t need to include the orbital box diagram as part of your answer. Based on your drawing, explain why phosphorus is either paramagnetic or diamagnetic.

Step-by-step answer

P Answered by PhD

5

The correct configuration is - 1s^2s^22p^63s^23p^3

Explanation:

Diamagnetism is an extremely week type of attraction that is incited by an adjustment in the orbital movement of electrons because of an applied attractive field. This attraction is nonpermanent and continues due to the presence of an external field.

The magnetic properties of a substance can be controlled by analyzing its electron configuration. If it has unpaired electrons in its outer orbital, at that point the substance is paramagnetic, and in the event that all electrons are found paired, the substance is then diamagnetic.

The electron configuration of the phosphorus is -

1s^2s^22p^63s^23p^3 . As it is clear that the outer shell of P has 3 unpaired electron it is paramagnetic.

StudenGPT

Write the full electron configuration, short-hand electron configuration and orbital diagram for the following elements nitrogen chlorine nickel vanadium tungsten

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P Answered by Studen AI

1

Sure! I'd be happy to help you with the electron configurations, shorthand electron configurations, and orbital diagrams for the elements you've mentioned. Let's start by breaking down each element one by one:

1. Nitrogen (N):
The atomic number of nitrogen is 7, which means it has 7 electrons.
- Full Electron Configuration: 1s² 2s² 2p³
- Shorthand Electron Configuration: [He] 2s² 2p³
- Orbital Diagram:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑

2. Chlorine (Cl):
The atomic number of chlorine is 17, so it has 17 electrons.
- Full Electron Configuration: 1s² 2s² 2p⁶ 3s² 3p⁵
- Shorthand Electron Configuration: [Ne] 3s² 3p⁵
- Orbital Diagram:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
3s: ↑↓
3p: ↑ ↑ ↑ ↑ ↑

3. Nickel (Ni):
Nickel has an atomic number of 28, indicating it has 28 electrons.
- Full Electron Configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸
- Shorthand Electron Configuration: [Ar] 4s² 3d⁸
- Orbital Diagram:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
3s: ↑↓
3p: ↑ ↑ ↑
3d: ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑

4. Vanadium (V):
Vanadium has an atomic number of 23, which means it has 23 electrons.
- Full Electron Configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d³
- Shorthand Electron Configuration: [Ar] 4s² 3d³
- Orbital Diagram:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
3s: ↑↓
3p: ↑ ↑ ↑
3d: ↑ ↑ ↑
4s: ↑↓

5. Tungsten (W):
Tungsten has an atomic number of 74, meaning it has 74 electrons.
- Full Electron Configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d⁴
- Shorthand Electron Configuration: [Xe] 6s² 4f¹⁴ 5d⁴
- Orbital Diagram:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
3s: ↑↓
3p: ↑ ↑ ↑
3d: ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑
4s: ↑↓
4p: ↑ ↑ ↑
4d: ↑ ↑ ↑ ↑
4f: ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑ ↑
5s: ↑↓
5p: ↑ ↑ ↑
5d: ↑ ↑ ↑ ↑
6s: ↑↓

I hope this explanation and breakdown of the electron configurations, shorthand configurations, and orbital diagrams for nitrogen, chlorine, nickel, vanadium, and tungsten helps you understand them better! Let me know if you need any additional information.

Fill in the orbital diagrams and write the electron configuration for the following elements.

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