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The force attraction by group 1 metals for their valence electrons?
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∙ 13y ago
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Wiki User
∙ 13y ago
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Why are valence electrons easier to remove from an atom than core electrons?
the force of attraction between then nucleus and the valence electrons is less than that between the nucleus and the core 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
The attraction between a positive metal ion and the electrons surrounding it is an?
Metals can be thought of as a lattice of metal ions surrounded by electrons. Again the force of attraction is electrostatic. These electrons are delocalised and metals get their conductiity from thir movement under an applied electric field. Positive metal ions in chemical compounds are surrounded by negativelly charged anions. The force between the oppositely charged ions is electrostatic.
Why is silver a better conductor than gold?
Gold has more electrons than silver. As such gold will also have more protons. Because of the opposite charges of the protons and electrons there will be a greater force of attraction between the electrons and the nucleus than there is in silver as silver has less protons. The valence electrons in silver are further away from the nucleus than the valence electrons in gold and they are therefore less attracted to the nucleus The valence electrons in silver can be lost more easily than those in gold in order to conduct heat and electricity.
Why metals are flexible?
The formation of metallic bonds causes them to be flexible and strong. Metallic bonds become strong because positive and negative charged electrons have a strong force of attraction. Metallic bonds are flexible because of their malleability.
The force of attraction by group 1 metals for their valence electrons is?
Dr. Hubble!
Why are valence electrons easier to remove from an atom than core electrons?
the force of attraction between then nucleus and the valence electrons is less than that between the nucleus and the core electrons
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.
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.
Why do force of attraction between nucleus and electrons decrease in alkali metal as increase in size?
As alkali metals increase in size, the distance of the outermost electrons from the nucleus increases. The attraction between the electrons and the nucleus is electrostatic, and it is a fundamental property of electrostatic attractions that the attraction decreases with increasing distance between the attracting charges. Another way of describing this is that the attractive force is partially "screened" by the inner electrons between the outermost electrons and the nucleus.
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
Why are metals good conductors of electricity?
Because metals release negative ions which conduct electricity. Because of the force of attraction between valence electron and also because the free electrons can move freely through the lattice carrying a charge.
What is the force of attraction between a positively charged metal ion and the electrons in a metal?
electrostatic force
The attraction between a positive metal ion and the electrons surrounding it is an?
Metals can be thought of as a lattice of metal ions surrounded by electrons. Again the force of attraction is electrostatic. These electrons are delocalised and metals get their conductiity from thir movement under an applied electric field. Positive metal ions in chemical compounds are surrounded by negativelly charged anions. The force between the oppositely charged ions is electrostatic.
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 is the outer shell of an atom?
The outer shell is the valence electrons and they are very loosely bound to the nucleus - less force by the nucleus on the valence electrons, so valence shell's electrons are exchanged first in any reaction.
Why do atoms with a low electronegativity like lithium have a weak attractive force for electrons?
they have few valence electrons and aren't close to having eight valence electrons
