0
What else can I help you with?
What is a elements oxidation number?
The oxidation number of an element is a measure of the number of electrons that an atom of that element has gained or lost to achieve a stable electron configuration. It is a value that is assigned to an element in a compound to help track the flow of electrons in chemical reactions. Oxidation numbers can be positive, negative, or zero, depending on whether the element has lost, gained, or shared electrons.
How many electrons are lost or gained in Xe?
Xenon (Xe) typically forms compounds by gaining two electrons to achieve a stable electron configuration.
What is the oxidation number for 1s22s22p63s22p5?
The oxidation number for an atom is determined by the number of electrons it gains or loses to achieve a stable electron configuration. For the configuration 1s22s22p63s22p5, sulfur (S) has an oxidation number of -2, as it has gained two electrons to achieve a full valence shell of 8 electrons.
What is the ion notation for an atom with 6 protons and 2 electrons?
we can write the name of element anthen write 4+ as superscript
What is the number of electrons gained or lost in Fluorine?
Fluorine gains one electron to achieve a stable electron configuration of a full outer shell.
How many electrons are gained in Se?
Selinium is a non metal element. There are 34 electrons in a single atom.
How many electrons are needed to be gained or lost in aluminium to achieve stable electron configuration?
Only three electrons.
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.
What is a elements oxidation number?
The oxidation number of an element is a measure of the number of electrons that an atom of that element has gained or lost to achieve a stable electron configuration. It is a value that is assigned to an element in a compound to help track the flow of electrons in chemical reactions. Oxidation numbers can be positive, negative, or zero, depending on whether the element has lost, gained, or shared electrons.
Will electrons be gained or lost if the atom of oxygen becomes stable?
the atomic no of oxygen is 8 to reach the nearest noble gas electronic configuration it excepts 2 electrons and becomes isoelectronic to Neon.
How many electrons are lost or gained in Xe?
Xenon (Xe) typically forms compounds by gaining two electrons to achieve a stable electron configuration.
What is the oxidation number for 1s22s22p63s22p5?
The oxidation number for an atom is determined by the number of electrons it gains or loses to achieve a stable electron configuration. For the configuration 1s22s22p63s22p5, sulfur (S) has an oxidation number of -2, as it has gained two electrons to achieve a full valence shell of 8 electrons.
What is the ion notation for an atom with 6 protons and 2 electrons?
we can write the name of element anthen write 4+ as superscript
What is the number of electrons gained or lost in Fluorine?
Fluorine gains one electron to achieve a stable electron configuration of a full outer shell.
Silicon how many electrons are gained or lost?
Silicon typically gains 4 electrons to achieve a stable octet configuration. This allows it to form stable covalent bonds with neighboring atoms.
Does AS3- lose or gain electrons?
The ion given is formed when the neutral arsenic atom gains three electrons.
What rule is used to predict the number of electrons that must be lost or gained in order to achieve stability?
For doing so, firstly the electronic configuration of the element is written.Then it is seen how many electrons does the element has in its valence shell.The max. no. of electrons that can be present in the valence shell is 8. So, if the element has less than 4 electrons in the valence shell, then it looses them to form stable ion and if it has more than 4 electrons, it must gain 8-no. of valence electrons to form stable ion. If the element has 4 valence electrons, then it shares them with other atoms to form compounds.
