QuestionWhat is the chemical symbol for the ion with electron configuration $[\mathrm{He}] 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6}$ ?

Studdy Solution

STEP 1

Assumptions1. The electron configuration given is for an ion. . The electron configuration notation follows the standard format, where the superscripts represent the number of electrons in each subshell.
3. The symbol [He] represents the electron configuration of a helium atom, which is1s².

STEP 2

First, we need to understand the electron configuration notation. The notation [He] represents the electron configuration of a helium atom, which is1s². This means that the ion has the same electron configuration as helium, plus the additional electrons indicated in the given configuration.

STEP 3

The given electron configuration is [He]2s²2p⁶. This means that the ion has2 electrons in the2s subshell and6 electrons in the2p subshell, in addition to the2 electrons in the1s subshell represented by [He].

STEP 4

Now, we can add up the number of electrons in each subshell to find the total number of electrons in the ion.
$Total\, electrons =2 (from\, [He]) +2 (from\,2s²) +6 (from\,2p⁶)$

STEP 5

Calculate the total number of electrons.
$Total\, electrons =2 +2 + =10$

STEP 6

The atomic number of an element is equal to the number of electrons in a neutral atom of that element. Therefore, the ion with10 electrons in its neutral state corresponds to the element with the atomic number10.

STEP 7

Looking at the periodic table, the element with the atomic number10 is Neon (Ne).
The chemical symbol for the ion is Ne.

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QuestionWhat is the chemical symbol for the ion with electron configuration $[\mathrm{He}] 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6}$ ?

Studdy Solution

STEP 1

Assumptions1. The electron configuration given is for an ion. . The electron configuration notation follows the standard format, where the superscripts represent the number of electrons in each subshell.
3. The symbol [He] represents the electron configuration of a helium atom, which is1s².

STEP 2

First, we need to understand the electron configuration notation. The notation [He] represents the electron configuration of a helium atom, which is1s². This means that the ion has the same electron configuration as helium, plus the additional electrons indicated in the given configuration.

STEP 3

The given electron configuration is [He]2s²2p⁶. This means that the ion has2 electrons in the2s subshell and6 electrons in the2p subshell, in addition to the2 electrons in the1s subshell represented by [He].

STEP 4

Now, we can add up the number of electrons in each subshell to find the total number of electrons in the ion.
$Total\, electrons =2 (from\, [He]) +2 (from\,2s²) +6 (from\,2p⁶)$

STEP 5

Calculate the total number of electrons.
$Total\, electrons =2 +2 + =10$

STEP 6

The atomic number of an element is equal to the number of electrons in a neutral atom of that element. Therefore, the ion with10 electrons in its neutral state corresponds to the element with the atomic number10.

STEP 7

Looking at the periodic table, the element with the atomic number10 is Neon (Ne).
The chemical symbol for the ion is Ne.

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QuestionWhat is the chemical symbol for the ion with electron configuration [He]2 s22p6[\mathrm{He}] 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6}[He]2 s22p6?

Studdy Solution

STEP 1

Assumptions1. The electron configuration given is for an ion. . The electron configuration notation follows the standard format, where the superscripts represent the number of electrons in each subshell.3. The symbol [He] represents the electron configuration of a helium atom, which is1s².

STEP 2

First, we need to understand the electron configuration notation. The notation [He] represents the electron configuration of a helium atom, which is1s². This means that the ion has the same electron configuration as helium, plus the additional electrons indicated in the given configuration.

STEP 3

The given electron configuration is [He]2s²2p⁶. This means that the ion has2 electrons in the2s subshell and6 electrons in the2p subshell, in addition to the2 electrons in the1s subshell represented by [He].

STEP 4

Now, we can add up the number of electrons in each subshell to find the total number of electrons in the ion.Total electrons=2(from [He])+2(from 2s²)+6(from 2p⁶)Total\, electrons =2 (from\, [He]) +2 (from\,2s²) +6 (from\,2p⁶)Totalelectrons=2(from[He])+2(from2s²)+6(from2p⁶)

STEP 5

Calculate the total number of electrons.Total electrons=2+2+=10Total\, electrons =2 +2 + =10Totalelectrons=2+2+=10

STEP 6

The atomic number of an element is equal to the number of electrons in a neutral atom of that element. Therefore, the ion with10 electrons in its neutral state corresponds to the element with the atomic number10.

STEP 7

Looking at the periodic table, the element with the atomic number10 is Neon (Ne).The chemical symbol for the ion is Ne.

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QuestionWhat is the chemical symbol for the ion with electron configuration $[\mathrm{He}] 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6}$ ?

Assumptions1. The electron configuration given is for an ion. . The electron configuration notation follows the standard format, where the superscripts represent the number of electrons in each subshell.
3. The symbol [He] represents the electron configuration of a helium atom, which is1s².

Now, we can add up the number of electrons in each subshell to find the total number of electrons in the ion.
$Total\, electrons =2 (from\, [He]) +2 (from\,2s²) +6 (from\,2p⁶)$

Calculate the total number of electrons.
$Total\, electrons =2 +2 + =10$

Looking at the periodic table, the element with the atomic number10 is Neon (Ne).
The chemical symbol for the ion is Ne.