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What is the size order for these scientific particles Proton Neutron Atom Electron Nucleus?
IIRC Atoms (contains Protons/Neutrons and electrons) Nucleus contains Protons and Nuetrons Proton atomic size 1 Nuetron atomic size 1 electron atomic size 1/1836 i.e the proton is 1836 bigger than the electron
What is the effect of an additional electron have on atomic size?
According to me the atomic size of an atom increases or decreses with the change in the number of shells. As atomic size is defined as the distance between the nucleus and valence shell of an atom. So, the addition of an electron does not effect the atomic size. As we can see in the periodic table that while moving along a group the number of electrons increases along with increase in no. of shells, while the atomic size tends to be increase with addition of shells and neglecting the addition of electrons. Same is the case while moving along a period. Atomic size decreases while the attraction between increased nuleus charge increases . Thus the size of the atom decreases.
Is the electron the largest of the three main atomic particles?
The electron is the smallest of the three main atomic particles by a long way. The proton and neutron are of a similar size, with the neutron having (very) slightly more mass. The mass of an electron is around 1/1840 of a proton or electron.
Why is it when an atomic number increases in a group the size of the atoms increase?
As the atomic number increases within a group, additional electron shells are added to the atom, leading to a greater distance between the outermost electrons and the nucleus. This increase in distance results in a larger atomic radius. Additionally, while the effective nuclear charge increases, the shielding effect from inner-shell electrons mitigates this attraction, allowing outer electrons to be held less tightly and thus increasing atomic size.
What is the size of a proton in scientific notation?
A proton is 2x10^-14m, or 0.00000000000002m
When you go down a column on the periodic table how does the atomic size go?
As you go down a column on the periodic table, the atomic size increases. This is because each subsequent element in the column has an additional energy level of electrons, leading to increased distance between the nucleus and the outermost electrons, resulting in larger atomic size.
Why the atomic size of argon is more than chlorine?
The atomic size of an element is primarily determined by the number of electron shells and the effective nuclear charge experienced by the outermost electrons. In the case of argon and chlorine, argon has an additional electron shell compared to chlorine, resulting in a larger atomic size. This additional electron shell in argon leads to greater electron-electron repulsions that push the outer electrons farther away from the nucleus, increasing the atomic size.
What effect on atomic size is more significant an increase in nuclear charge across a period or an increase in occupied energy levels within a group?
An increase in nuclear charge across a period has a more significant effect on atomic size than an increase in occupied energy levels within a group. As the nuclear charge increases, the attraction between the positively charged nucleus and the negatively charged electrons strengthens, pulling the electrons closer and resulting in a decrease in atomic size. In contrast, while the addition of energy levels down a group increases atomic size due to greater electron shielding and distance from the nucleus, the effect of increased nuclear charge across a period is dominant in reducing atomic size.
What property increases going down a group in periodic table?
Atomic size increases going down a group in the periodic table. This is because additional energy levels are being filled with electrons, leading to an increase in distance between the nucleus and the outermost electron shell.
How does a nucleus hold together?
The atomic nucleus is held together by the strong atomic force. This force is attractive, regardless of the charge of the constituent particles.Not asked, but answered for completeness sake, the electromagnetic force competes with the strong atomic force, causing a repulsive effect between protons that is a function of the size of the nucleus. Nuclei greater than 82=lead are unstable due to this competition. Also, the weak atomic force enters in, causing instability as a function of proton/neutron ratio and other factors.
How much more massive is a proton compared to a electron?
By sheer size, I would assume MUCH larger. But through weight, the proton is much heavier compared to an electron. On any element, the atomic number is the weight of the nuetrons and protons. The weight of electrons is so small and insignificant, it is usual not looked on at the highschool level. And has no effect on the molar mass.
Why do the atomic size decreases in periods rather than to be increased due to proton repulsion that leads to nucleus to expansion?
As we move across the period, there is an increase in the atomic number i.e., there is an increase in the number of protons inside the nucleus. This means, there is more nuclear force. This nuclear force pulls the electron orbits as close as it can. thus, the radius of the atom decreases. Hence the atomic size decreases.
