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Why do atoms with a low electronegativity like lithium have a weak attractive force for electrons?
Atoms with low electronegativity like lithium have a weak attractive force for electrons because they have less ability to attract and hold onto electrons due to their smaller nuclear charge. This results in a weaker pull on electrons towards the nucleus compared to atoms with higher electronegativity.
Why is it harder to remove an inner shell electron than a valence electron from an atom?
Electrons are attracted to the positive charge on the nucleus. The further an electron is found from the nucleus of an atom, the lower the force of attraction between it and the nucleus. Therefore an electron far away from the nucleus (like a valence electron) will have less of an attraction to the nucleus than one close to it. A lower attraction to the nucleus translates into the fact that less energy would then be required to remove the electron from the vicinity of that nucleus.
Why does aluminum have a higher melting point than Sodium?
Metallic bonding is between metal ions in a sea of delocalised electrons. In Aluminum, there are more delocalised electrons and the ions have a higher charge than Sodium. There is a greater force of attraction between the electrons of aluminum because the protons that are pulling on a 3+ ion are stronger than a 1+ ion. Since it requires more force to overcome these forces of attraction, Aluminum has the higher melting point. - Troy Moss
Why can metals like copper malleable and ductile?
Metals are both ductile and malleable because of their electrons. The electrons move about the entire structure fo the metal, when the metal is pulled or smashed it doesnt crack because there are no similarly charged ions facing each other for repulsion. Picture this ionic representation of Sodium Cholride NaCl (Table Salt)Pretend theres circles around the signes +-+-+-+-+- -+-+-+-+-+ When this is hit down the positive charges will line up causing the structure to have the same charges facing each other which make it split. A metal has electrons flowing like a sea. Picture a structure of atoms with electrons zipping all over the place. When the metal is smashed or pulled the charges wont line up causing no repulsion. the another answer is:- High degrees of ductility occur due to metallic bonds, which are found predominantly in metals and leads to the common perception that metals are ductile in general. In metallic bonds valence shell electrons are delocalized and shared between many atoms. The delocalized electrons allow metal atoms to slide past one another without being subjected to strong repulsive forces that would cause other materials to shatter.
Why are you attracted to the earth?
Attraction to the Earth is caused by the force of gravity.
The force attraction by group 1 metals for their valence electrons?
Group 1 metals, also known as alkali metals, have a strong force of attraction for their valence electrons due to their low ionization energy and large atomic radius. This makes it easy for them to lose their valence electrons and form positively charged ions in order to achieve a stable electron configuration.
Why does valence electron give up outermost energy easily?
The force of attraction between the atom's nucleus and its valence electrons are the least. Hence valence electrons are lost easily.
Why are valence electrons easier to remove from an atom than core electrons?
Valence electrons are further away from the nucleus and experience less attraction to the positively charged protons in the nucleus compared to core electrons. This makes valence electrons easier to remove from an atom. Core electrons are located closer to the nucleus and are more strongly attracted to the nucleus, requiring more energy to remove them from the atom.
What is it called when electrons in the inner energy levels block the attraction between the nucleus and the valence electrons?
It is called shielding or screening effect. Inner electrons shield the valence electrons from the positive charge of the nucleus, reducing the attractive force between them.
What are formed by a loss or gain of valence electrons during a chemical combination of elements?
Cations are formed by the loss of electrons, anions are formed by the gain of electrons. The force of attraction between cations and anions results in ionic bond.
How can you use the word stable to explain why the alkali metals tend to lose valence electrons?
The alkali metals tend to lose valence electrons because they have one electron in their outermost energy level, which makes them unstable. By losing this electron and achieving a full outer shell, they become more stable like the noble gases. This stability is the driving force behind their tendency to lose valence electrons.
What is electron shielding?
•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. •It is also referred to as the screening effect or atomic shielding. •Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. Also, it has trends in the Periodic Table
What is the force of attraction between a positively charged metal ion and the electrons in a metal?
electrostatic force
A force that can attract and repel certain metals?
The force you are referring to is magnetism. Certain metals, such as iron, nickel, and cobalt, are attracted to magnets, while others, like aluminum and copper, are not. This attraction or repulsion is due to the arrangement of electrons within the material.
Why do atoms with a weak electronegativity like lithium have a weak attractive force for electrons?
they have few valence electrons and aren't close to having eight valence electrons
What force pulls electrons and proton together?
The force that pulls electrons and protons together is electromagnetic force. This force is responsible for the attraction between opposite charges (electrons are negatively charged and protons are positively charged), which keeps the electrons orbiting the nucleus of an atom.
Why do halogens attract electrons the most?
Halogens attract electrons the most because they have a high electronegativity - a measure of an atom's ability to attract and hold onto electrons. This is due to their close-to-full valence shells and small atomic radii, which create a strong force of attraction for additional electrons.
