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How many electrons must be gained or lost for selenium to achieve a noble gas electron configuration?
Selenium should gain two electrons and lose six electrons to achieve a noble gas electron configuration.
How many electrons does a nitrogen atom need to gain in order to attrain a noble-gas?
A nitrogen atom needs to gain three electrons to achieve a stable electron configuration similar to a noble gas. This would result in the nitrogen atom having a full outer electron shell, like that of a noble gas.
What is the charge of nitrogen to achieve noble gas configuration?
To achieve a noble gas configuration, nitrogen needs to gain three electrons to have a completely filled outer shell like neon. This would give it a charge of -3 since each gained electron carries a negative charge.
How could iodine atoms react to achieve a noble gas configuration?
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
Have two valence electrons and get to a stable electron configuration by using two electrons?
You can achieve a stable electron configuration by using two electrons by forming a covalent bond with another atom that also has two valence electrons. In this way, each atom can share its valence electrons to achieve a full outer shell and achieve stability.
How many electrons does nitrogen gain in order to achieve a noble gad electron configuration?
nitrogen has 5 valence electrons. It should gain 3 electrons to achieve a noble gas configuration.
How many electrons does nitrogen gain in order to achieve in order a noble gas electron configuration?
Nitrogen has to gain three electrons
How many electrons does nitrogen have to gain in order to achieve noble gas electron configuration?
Nitrogen needs to gain 3 electrons to achieve noble gas electron configuration, similar to the nearest noble gas, which is neon. By gaining 3 electrons, nitrogen would have a full outer shell of 8 electrons, making it more stable.
How many electrons can nitrogen lose or gain?
Nitrogen can gain 3 electrons to achieve a full outer shell with 8 electrons, or lose 5 electrons to achieve a stable electron configuration similar to the noble gas neon.
What type of bond is nitrogen and fluorine?
Nitrogen and fluorine form a covalent bond. The two atoms share electrons to achieve a stable electron configuration.
What type of bond is nitrogen trifluoride?
Nitrogen trifluoride is a covalent bond. It is formed by sharing electrons between nitrogen and fluorine atoms to achieve a stable electron configuration.
Are nitrogen and carbon ionic or covalent?
Nitrogen and carbon form covalent bonds. They typically share electrons to achieve a stable electron configuration rather than transferring electrons to form ionic bonds.
Why happens when two nitrogen atoms share electrons?
When two nitrogen atoms share electrons, a covalent bond is formed. Each nitrogen atom contributes one electron to the shared pair, creating a stable bond by completing their outer electron shells. This sharing of electrons allows both atoms to achieve a more stable electron configuration.
How many electrons must be gained or lost for selenium to achieve a noble gas electron configuration?
Selenium should gain two electrons and lose six electrons to achieve a noble gas electron configuration.
How many electrons does a nitrogen atom need to gain in order to attrain a noble-gas?
A nitrogen atom needs to gain three electrons to achieve a stable electron configuration similar to a noble gas. This would result in the nitrogen atom having a full outer electron shell, like that of a noble gas.
What electron configuration do atoms acheieve by sharing electrons form covalent bonds?
They achieve the electron configuration of a noble gas.
How many electrons does a nitrogen atom need to gain in order to attain noble-gas electrons configuration?
A nitrogen atom needs to gain 3 electrons in order to attain a noble-gas electron configuration, similar to that of neon. This would allow the nitrogen atom to fill its outermost energy level and achieve greater stability.
