Which of the three atoms diagrammed in Model 4 has the strongest attraction for its outermost electrons? Chlorine. As you move from the smallest atom to the largest atom, does the distance between the outermost electron(s) and the nucleus change significantly.
Which atom K or Na would have a stronger force of attraction between their outermost electron’s and the protons in the nucleus?
S<Na<K S has the smallest radius because the proton number is larger than Na causing attraction to be stronger and so the elections are closer to the nucleus. Although K has more protons than S, the atomic radius is larger because of the extra level of electrons.
Does barium or calcium have a stronger attractive force?
Barium has more electrons shells than calcium, so the nuclear shielding is stronger, and the outmost electrons are further away from the nucleus. This results in a weaker attractive force between the electron and the nucleus, so a smaller energy is required to remove it.
What do the arrows represent in the alkali metals?
The Alkali Metals (Group 1)
The arrows represent the force of attraction between each atom’s single valence electron and its protons!
What is the relationship between attractive force between the electrons and protons and the energy required to remove an electron?
The more protons in the nucleus, the stronger the attraction of the nucleus to electrons. This stronger attraction makes it more difficult to remove electrons. Within a group, the ionization energy decreases as the size of the atom gets larger.
Which element within Period 2 generates the greatest force of attraction?
Explanation: Fluorine has an electronegativity of 4.0 which is the highest of all elements in entire periodic table as well as the second period. Fluorine has 9 positive protons creating an attraction for electrons the most besides Neon with 10. in the second period.
Which element Li or F has a greater attraction for electrons?
3. Explain, in terms of nuclear charge, why Fluorine has a great electronegativity AND ionization energy than Lithium? Fluorine has more protons resulting in a greater nuclear charge, causing a greater attraction for electrons.
Which of the following atoms has the highest coulombic attraction?
Magnesium ion has a higher coulombic attraction compared to the coulombic attraction of Sodium. This is why Magnesium ion is more reactive than Sodium Ion. (Sodium has a +1 charge and Magnesium has a +2 charge.
Does chlorine or sodium have a stronger attractive force?
The protons of the two atoms attract the electrons of the other atom. The thicker arrow shows that chlorine has a stronger attraction for electrons than sodium has. During the interactions between the atoms, the electron in sodium’s outer energy level is transferred to the outer energy level of the chlorine atom.
Why is barium bigger than calcium?
The elements calcium and barium are both in the same Group 2 with calcium being higher, so for the neutral atoms, Ca would have a smaller radius, its outer electrons being in the n = 4 level as compared with the n = 6 level for the Ba atom.
Which of the following elements has the greatest electron affinity?
Chlorine has the highest electron affinity among the elements.
Which metal is likely the most reactive?
The most reactive metal on the periodic table is francium. Francium, however, is a laboratory-produced element and only minute quantities have been made, so for all practical purposes, the most reactive metal is cesium.
What is coulombic attraction?
Coulombicattractionisafancynamefortheattractionthatoccursbetweenoppositelychargedparticles. In chemistry, we talk about the attraction between protons (+) in the nucleus to the electrons (-) surrounding the nucleus.
Which factors determine the amount of attractive force between protons and electrons?
In an atom, the most important factors that influence the force, as calculated by Coulomb’s equation, are the nuclear charge and the distance from the nucleus to the electron of interest. The closer an electron is to a nucleus, the stronger the attractive force (i.e. the more negative F becomes).
Which best describes the relationship between distance and attractive force?
Describe the mathematical relationship between the distance and the attractive force between protons and electrons? As distance increases, attraction decreases. … The greater the number of protons, the greater the pull on the electrons, which means greater force.
What is the relationship between distance and attractive forces when it comes to the protons in the nucleus and the electrons on the outside?
Describe the mathematical relationship between distance and the attractive force between protons and electrons. It is inversely proportional.