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How many valence electron does Ca lose or gain to attain noble-gas electron configuration?
Calcium loses two electrons to obtain a noble-gas electron configuration.
What type of elements become cations?
Metals typically become cations by losing electrons to attain a stable electron configuration. Transition metals and main group metals are common examples of elements that form cations.
Why the metal is very reactive?
Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
Why are the oxidation numbers of alkali metals always positive?
Alkali metals have a single electron in their outermost shell that is easily lost, resulting in a positive oxidation number. When they lose this electron to form ions, they attain a stable electron configuration, which typically involves having a full valence shell with a noble gas electron configuration.
How does an element in group 2 attain a stable electron configuration?
It loses 2 electrons and becomes a +2 ion.
How many electrons must be gained or lost for calcium to attain a noble-gas electron configuration?
Calcium's electron configuration is [Ar] 4s2. To attain a noble gas configuration, calcium must lose 2 electrons to have the same electron configuration as argon, 4s2 3d10.
How many valence electron does Ca lose or gain to attain noble-gas electron configuration?
Calcium loses two electrons to obtain a noble-gas electron configuration.
How many electrons must be gained or lost for calcium to attain a noble gas electron configuration?
Calcium (Ca) has 20 electrons and its electron configuration is [Ar] 4s². To attain a noble gas electron configuration, calcium needs to lose two electrons to achieve the stable electron configuration of argon ([Ar] 4s² 3d¹⁰).
What type of elements become cations?
Metals typically become cations by losing electrons to attain a stable electron configuration. Transition metals and main group metals are common examples of elements that form cations.
Why the metal is very reactive?
Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
Do non-metals form a stable outer electron configuration by losing electrons and becoming anions?
NO. Nonmetals tend to GAIN electrons to complete their outer shell. By gaining electrons, they become a negatively charged species, which is what an anion is. Metals tend to LOSE electrons to end up with a full outer shell; in losing electrons, they develop a positive charge (become cations).
How do metals form ions to achieve the stable gas configuration?
metals lose electrons to form ions so as to obtain noble gas configuration. for e.g. sodium(Na) has 11 electrons i.e. 1 electron in its valent (last) shell, to attain noble gas configuration sodium loses 1 electron which may be gained by a non-metal to stabilize itself.
Why do atoms of non-metals form anions?
Non metals tend to be at the Right Hand Side of the periodic table. They therefore tend to need to GAIN electrons to get a stable octet-noble gas configuration. Gaining electrons mean they become anions. The reverse is true for metals.
What is the different ways in which atoms try to attain the electronic configuration of noble gasses with an example?
Metals like sodium,potassium get noble gas configuration by losing electrons. Elements like nitrogen,oxygen get noble gas configuration by gaining electrons. Halogens get noble gas configuration by sharing electrons.
Why is it easy for a metal to loose an electron?
Metals useually have few valence electrons and they loose electrons from their outermost shell thus, forming an ion with positive charge (cations). This is because it is easy for metals to loose electron and attain stable or octet configuration similar to rare gases. Hence to attain stability metals lose valence electrons. E.g. sodium (At no. =11 ; electronic configu-1s2, 2s2, 2p6, 3s1) metal has one valence electron and it is easy for it to loose 1e rather to gain 7e to attain stable configuration. Hence it loose 1e forming Na+ cation.
Why are the oxidation numbers of alkali metals always positive?
Alkali metals have a single electron in their outermost shell that is easily lost, resulting in a positive oxidation number. When they lose this electron to form ions, they attain a stable electron configuration, which typically involves having a full valence shell with a noble gas electron configuration.
How does an element in group 2 attain a stable electron configuration?
It loses 2 electrons and becomes a +2 ion.
