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What elements achieve noble gas configuration by losing one electron?
Elements in Group 1 of the periodic table, such as lithium and sodium, achieve noble gas configuration by losing one electron. This leaves them with a stable octet electron configuration, similar to the nearest noble gas in the periodic table.
What happens to the reactivity as you move down group 1 in the periodic table?
Reactivity in group 1 of elements increases as we go down the group (to francium) because in the alkali metals as we go down the group number of atomic shells increases so the elements with most shells will easily release their electrons in the outer most shell.
What happens if an atom X of an element in group 1 if reacts to become X positive?
When an atom X from group 1 of the periodic table reacts to become X positive, it loses one electron from its outermost shell. This loss of an electron results in the formation of a positively charged ion (cation) with a charge of +1. Consequently, the atom achieves a more stable electron configuration, often resembling that of the nearest noble gas. This process typically occurs during reactions with nonmetals, where the atom readily donates its valence electron.
Why do metals on the left hand side of the of the periodic table are said to be highly reducing?
Reducing agent reduces others and oxidised itself.reduction means gain of electrons and oxidation means loss of electrons.as the metals on left hand side of the periodic table have lower ionisation potential so they are easily lose electrons and oxidised and reduces others.so they are highly reducing.
Does iodine gain or loss electron?
Barium loses electrons to obtain a stable octet, like any other metal.
How do you justify the position of hydrogen at the top of various group?
Hydrogen was placed in the first group because has a high tendency to loss an electron.
What is the difference between oxidation number and the number of valence electrons?
The oxidation number is the charge that an atom has when forming a compound, determined by the electron gain or loss. Valence electrons are the electrons in the outermost shell of an atom, which are involved in forming chemical bonds. While the oxidation number can vary based on the compound, the number of valence electrons remains constant for elements in the same group of the periodic table.
How many electrons does sulfur need to lose to become a noble gas element?
Sulfur has six valence electrons and is in group 16 of the periodic table. To achieve a stable noble gas configuration, it needs to lose two electrons, resulting in a positive charge of +2, similar to the electron configuration of neon. This loss allows sulfur to attain a full outer shell, characteristic of noble gases.
How many electrons does a single cesium atom lose?
All right Cesium is an Alkali Metal so it belongs to the first column of the periodic table. Every element in that column has a charge of 1+ as a cation. So to answer your question, a single Cesium atom loses 1 electron when it becomes a cation. The cation looks like this: Cs = 55 Electrons Cs^+ = 54 Electrons As you can see it only loses one :)
How are oxidation numbers predictable using the periodic table?
In very simple terms to achieve the octet atoms either lose valence electrons or gain them. The number of valence electrons for the period 2 elements is relativelly straightforward use the group number and remember to take 10 away from B, C, N, O and F. So as an example boron in group 13 has 3 valence electrons- so gain of +5 or loss of 3. Gaining five seems so excessive so your best guess is +3, which is true in say B2O3As for using the periodic table to predict- not so easy- take gallium - in group 13 has 3 valence electrons- so it could lose 3 to give an octet, which indeed is its most common ON but can also lose 1 electron to form Ga+
Will Li gain or lose when reacting to Cl?
Li loses one electrons. Cl gains the electron.
Why are group one elements largely ionic?
Group 1 elements have one electron in their outermost electron shell, making it easier for them to lose this electron to achieve a full outer shell. This electron loss results in the formation of positively charged ions, which readily form ionic bonds with other elements to achieve a stable electron configuration.
