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Would you expect it to be harder to remove an electron from Na or O?
It would be easier to remove an electron from Na compared to O. Sodium (Na) has a smaller effective nuclear charge and a larger atomic radius compared to oxygen (O), making its valence electron easier to remove. Oxygen has a higher electronegativity and a stronger pull on its electrons, making it harder to remove an electron from O.
Why is the ionization energy needed to remove the first two electrons from Magnesium atoms relatively low?
The ionization energy needed to remove the first two electrons from Magnesium atoms is relatively low because these electrons are in the outermost energy levels and experience less electron-electron repulsion, making them easier to remove compared to inner electrons. Additionally, Magnesium has a relatively small effective nuclear charge, which further reduces the attraction between the nucleus and the outer electrons, making them easier to remove.
Why do non metallic elements pull electrons so effectivley during a reaction?
Nonmetallic elements take electrons from metals because unstable elements want to have a full valence (outer) electron shell. The metallic elements usually have a less then half full valence shell, it would be easy for them just to get rid of the electrons opposed to having to find more. Nonmetals usually only need one to four electrons so taking them from a metal would be easier then losing all of their electrons.
What would you predict about the ionization energies of these elements?
Ionization energy generally increases across a period from left to right due to increasing nuclear charge, which holds electrons more tightly. Conversely, ionization energy decreases down a group as additional electron shells are added, increasing the distance between the nucleus and the outermost electrons, making them easier to remove. Therefore, elements located further to the right in a period and higher up in a group tend to have higher ionization energies compared to those further left or lower down.
Why is it much easier for group 14 elemnts to become stable by sharing instead of transferring electrons?
Group 14 elements, such as carbon and silicon, have four valence electrons, allowing them to form stable covalent bonds by sharing electrons with other atoms. This sharing leads to the formation of strong covalent bonds, which are energetically favorable for these elements, rather than transferring electrons, which would require them to gain or lose multiple electrons to achieve a stable octet. Additionally, the relatively high ionization energies of group 14 elements make electron transfer less favorable compared to the stability gained through covalent bonding.
Would you expect it to be harder to remove an electron from Na or O?
It would be easier to remove an electron from Na compared to O. Sodium (Na) has a smaller effective nuclear charge and a larger atomic radius compared to oxygen (O), making its valence electron easier to remove. Oxygen has a higher electronegativity and a stronger pull on its electrons, making it harder to remove an electron from O.
Why is the ionization energy needed to remove the first two electrons from Magnesium atoms relatively low?
The ionization energy needed to remove the first two electrons from Magnesium atoms is relatively low because these electrons are in the outermost energy levels and experience less electron-electron repulsion, making them easier to remove compared to inner electrons. Additionally, Magnesium has a relatively small effective nuclear charge, which further reduces the attraction between the nucleus and the outer electrons, making them easier to remove.
Why only 12 elements form ions easier than the rest of the elements in periodic table?
I would imagine that these elements are hydrogen, the alkali metals and the halogens. Hydrogen and the alkali metals only have one outer electron, which is easier to displace than the two outer electrons of the alkaline earth metals, for example. In contrast, the halogens only need one more electron to have a complete outer shell; it is easier to accept one electron than the two electrons needed by the chalcogens - oxygen, sulphur, selenium etc.
Do the elements going horizontally on a periodic table have the same number of electrons?
No two elements would have the same atomic number, so, nor atoms of different elements (in neutral state) would have the same number of electrons.
Why do non metallic elements pull electrons so effectivley during a reaction?
Nonmetallic elements take electrons from metals because unstable elements want to have a full valence (outer) electron shell. The metallic elements usually have a less then half full valence shell, it would be easy for them just to get rid of the electrons opposed to having to find more. Nonmetals usually only need one to four electrons so taking them from a metal would be easier then losing all of their electrons.
Can you find out what the element is by the number of electrons in a neutral atom?
Yes, Elements are identified by the amount of electrons it has. Even isotopes are elements are still recognised by their amount of electrons. For example if you had a question: what element has 2 more electrons that Carbon? Carbon has 6 electrons, so 2 more would be 8. That would mean the element would therefore be Oxygen
Where would you find all of the elements with 2 valence electrons?
The elements of the group 2 are some examples.
Does Mercury has two outer electrons?
Yes mercury has two outer electrons the two elements that the two outer electrons would be Iodine and Magnesium.
What would you predict about the ionization energies of these elements?
Ionization energy generally increases across a period from left to right due to increasing nuclear charge, which holds electrons more tightly. Conversely, ionization energy decreases down a group as additional electron shells are added, increasing the distance between the nucleus and the outermost electrons, making them easier to remove. Therefore, elements located further to the right in a period and higher up in a group tend to have higher ionization energies compared to those further left or lower down.
When elements of group 2 lose their valance electrons what would be their charge?
The charge would be positive because the electrons and protons are of equal number so they cancel each other. So if you take the electrons from the element it leaves it unbalanced with x number of protons.
What are Elements that have less than or more than the normal number of electrons?
These would be ions.
Why is it much easier for group 14 elemnts to become stable by sharing instead of transferring electrons?
Group 14 elements, such as carbon and silicon, have four valence electrons, allowing them to form stable covalent bonds by sharing electrons with other atoms. This sharing leads to the formation of strong covalent bonds, which are energetically favorable for these elements, rather than transferring electrons, which would require them to gain or lose multiple electrons to achieve a stable octet. Additionally, the relatively high ionization energies of group 14 elements make electron transfer less favorable compared to the stability gained through covalent bonding.
