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Atomic Radius: the trends decrease as the periodic table progresses from the left to the right due to an increased number of protons

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Anna Williams - The atomic radius increases from top to bottom and becomes smaller from left to right. This is because the coulombic attraction between the protons and the electrons increases from left to right because of the increase in the core charge. The increases attraction pulls the electrons and the protons closer to each other and decreases the size. However, from top to bottom the size increases because the amount of electrons and protons in the nucleus increases. For example, Bromine has more protons and electrons than Chlorine and since the core charge of both elements is the same, Bromine has a bigger atomic radius. However, even though Chlorine has more protons and electrons than Sodium, Chlorine has a stronger core charge so its atomic radius is smaller.

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increases down a group and decreases across a period. It decreases across a period because there is the same amount of electron shells but there are more protons so it will be pulled in closer because there is more pull on them. It will increase as you go down a group because there are more electron shells and not enough protons in the nucleus to pull them in close.

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Electronegativity increases from bottom to top and from left to right. Electronegativity is the ability of an atom to

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Ionic Radius increases from right to left and from top to bottom.

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Anna Williams - Ionization energy increases from left to right and decreases from top to bottom. This is because the elements towards the right of the periodic table have a stronger core charge than the elements on the left. The coloumbic attraction between the electrons and the protons is stronger. This makes it harder to pull off on electron and increases the energy necessary to remove it. However, it is easier to pull of an electron in the outer shells than the inner shells due to the shielding effect. The electrons closer to the nucleus neutralize the positive charge and lessen the hold of the nucleus on the outer shell electrons.

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It decreases as you go down a column and increases as you go across a row. This is because as you go across a row there are more protons in the nucleus as you go across therefor pulling the electrons in the shells in closer and needing more energy to knock out a pair of electrons.

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Atomic Radius: decreases left to right, due to more protons, Coulombic attraction pulls them in closer to the nucleus, decreasing the radius
Ionization energy: increases left to right, electrons increase as you move across, making it easier for electrons in valence shell to be removed. Electron shielding causes ionization energy to decrease because it "blocks" Coulombic attraction.
Ionic radius: decreases left to right, as more protons are added, the nuclear charge grows, pulling the electrons closer to the nucleus (Coulombs)
Electronegativity: increases left to right, the more protons, the more electron repulsion occurs as you fill orbitals and the stronger the pull of electrons to the nucleus (Coulombs) the greater chance a neighboring electron will be pulled in
Electron affinity: decreases down a group because as more electrons fill shells that affaire are far from the nucleus, shielding increases while Coulombic attraction decreases.

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Anna Williams - The most electronegative element is fluorine and elements become less electronegative as the get farther away from fluorine. In other words, electronegativity increases from left to right and decreases from top to bottom. This is because the core charge of the nucleus is strongest in the halogen family, making coulombic attraction strongest.

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The atomic radius will decrease as you go across a row and increase as you go down a period. The shell model affects this because as you go down the periodic table, there are more electron shells causing the atom to be bigger. the reason that it gets smaller across a row is because there are more protons in the nucleus putting more pull on the electrons making the atom smaller.

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Atomic Radius increases from top to bottom and from right to left of the periodic table. Atomic radius is the distance from the nucleus to the outer shell of electrons. Atomic radius increases as you go down the periodic table because there are more electrons filling more electron shells, so they take up more space. Atomic radius also increases from right to left because the number of electron shells remains constant in a period, but as the number of protons increases, the pull towards the nucleus increases.

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As you move left to right across a row of the table, electronegativity increases because it requires less energy to lose an electron than to gain one. As you move down a column, it decreases becuase atomic number increases and atomic radius increases.

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Ionization energy increases from bottom to top and from left to right of the periodic table. Ionization energy is the amount of energy required to remove an electron from the outer shell of an atom.

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Electronegativity is the likelihood of an atom to attract a pair of electrons from a neighboring atom. As you move down a group in the periodic table, it decreases but as you move across a period it increases. The shell model and shielding affect this because as you go down the periodic table the atoms gradually get bigger which means that there are more electron shells therefore the nucleus will not have as much pull on neighboring atoms.

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Ionic Radius -

The trends go as you go down a row the radius gets bigger and as you go across a row the get smaller until you hit the negative ions where they get bigger but then decrease. This can be explained by Coulomb's law because as you go down the periodic table there are going to be more electrons so they will push each other apart and as you go across the table the there are more protons so it decreases this effect.  Using the shielding effect to explain is essentially the same concept there are more electrons as you go down the table so there are more electrons that can shield the outer electrons from the positive charges creating a larger radius because they are farther away and as you go across the table the there are more protons so it decreases this effect.  Electron repulsion explains the trend because since there are more electrons as you move down there is more repulsion between the electrons and as you go across the table the there are more protons so it decreases this effect.  The shell model can also explain this trend as since there are more electrons as you move down there are more shells needed so the radius increases.

Atomic Radius -

The trend is as you go down it increases and as you go left it increases.  This is because there are more less protons on the left side because it is the start of the row so there is coulomb's law.  There is also more repulsion effect.  There are more shells because there are more electrons.  There is also more shielding effect because there are more electrons.

Electron Affinity - The trend is as you go down a column the electron affinity decreases. This is because it increase the more atoms you add to each orbital.  So since there are more electrons in the outer shell there is less shielding effect.  There is also less coulomb's law because there are more electrons closer to the nucleus.  There is also more repulsion between the electrons

Ionization Energy -

Increases as you go up and across a row.  Coulomb's law is used to calculate the ionization energy because of the repulsion of electrons.  The electrons are repulsed by each other so since there are more electrons they repulse each other.  The electrons in the outer shell are the ones that are lost. The valence electrons in the outer shell are shielded so they are less attracted and therefore are lost easer

Electronegativity -

It increases as you go right and up the table.  It increases because there is more attraction between the nucleus and the electrons so there is more energy required.  It also increases as you go across the table because there are more electrons between the outside electrons and the nucleus making it easier for electrons to be attracted.  The outer shell is where the electrons that are attracted go.  When the electronegativity increases so does the electron repulsion.

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Ionic Radius is similar to atomic radius except instead of increasing from bottom to top, it is the opposite. This is where shielding is mainly in action.

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Electronegativity is the measure of a tendency of an atom to attract a bonding pair of electrons. the most electronegative element is fluorine. From left to right the elements increase in electronegative as well as from bottom to top. This is influenced by electron shielding and electron repulsion.

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is a measure of the size of its atoms or the distance front the center of the nucleus to the outside edge of the electron cloud. The bigger the radii, the further the distance between the two nuclei. From top to bottom, atomic radius increases and from left to right it decreases.

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Electronegativity is the tendency of an atom to attract a bonding pair of electrons. As you move across a period electonegativity increases but as you move down a group, it decreases. Coulomb's law effects this trend because the greater the attraction to the nucleus, the more likely it will attract a bonding pair. Shielding and the shell model relate to this trend because as there are more shells, the weaker the attraction between the electrons and the nucleus becomes making it harder for for them to attract bonding pairs. Electron repulsion effects the trend because as you double up on electrons, the harder it becomes to attract a bonding pair.

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Ionic Radius increases down a group because these elements have more electrons which fill up more electron shells. These electron shells are increasingly further away from the nucleus and, therefore, cause an increase in the Radius of an ion. Additionally, ionic radius decreases across a period because these elements contain more protons which cause an increase in nuclear charge. Due to Coulomb's law, these electrons are more tightly held and closer to the nucleus, therefore decreasing the radius of an ion. However, there is a discrepancy when one moves from cations to anions because cations are losing an electron while

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Electron Affinity will increase across a period and decrease down a row for the same reasons as Electronegativity: the Columbic attraction decreases across a period since the electrons are more likely to leave an atom, the shielding effect and electron repulsion cause an increase across a period because the electrons are easily removed from the nucleus and its positive charge, and the shell model will cause an increase in electron affinity across a period because the electrons in that atom can easily leave the ato or bring others in since there is an increase in the numbr of electrons.

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Atomic Radius Increases down a group because these elements have greater numbers of electrons which require greater numbers of electron shells. These electron shells are increasingly further away from the nucleus and, therefore increase the atomic Radius. Atomic radius decreases across a period because these elements have increasing numbers of protons which, due to Coulomb's law, causes the electrons to be more tightly and, therefore, closer to the nucleus. This decreases the atomic radius.

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Electronegativity will increase across a period and decrease down a row because the Coulombic attraction will decrease across a period because the electrons are more likely to go out of the atom or attract other electrons to the atom. The shielding effect will decrease across a period, causing an increase in elctronegativity, because the electron is easily repulsed from the nucleus. The electron repulsion will cause the electronegativity to increase across a period because the electrons are more likely to leave the atom or bring othe electrons in because they can easily more away from the positive charge. Finally, the shell model shows that the electroneativity will increase across a period because more electrons in the outermost orbtal increase the likelihood of an electron leaving the orbital and atom or bringing other electrons into the atom

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Ionization energy is the amount of energy it requires for an atom to discharge an electron. Ionization energy increases as you move across a period, and decreases as you move down a group. Coulomb's law effects this trend because as the electrons have a stronger attraction to the nucleus, the more energy it will take to free them. It involves electron shielding and the shell model because as there becomes more shells, the weaker the attraction is between the electron and the nucleus making there less energy needed to break the bond. Lastly, electron repulsion relates to this trend because whenever there is electron repulsion it effects the ionization energy.

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Atomic radius decreases as you move left to right across the table because within a row, the electrons are all added to the same shell, but the increasing number of protons causes a greater nuclear attraction, decreasing atomic radius.

Atomic Radius increases as you move down a column of the table because  the electrons are placed in further shells, and the shielding effect counteracts the increasing nuclear attraction, so the atomic radius increases as more electron shells are occupied and the quantum number increases.

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The atomic radius will increase down acolumn and decrease across a period for the same reasons as the ionic radius: the Coulombic attractions decreases aross the period because the pull between electrons and protons is smaller, the shielding effect is preventing electrons from growing further away from the nucleus, the electron repulsion will increase going down because there are more electrons tobe repulsed from the nucleus and move away from the protons, and the shell model shows that as you add a new orbital, electrons can easily move further away from the nucleus.

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Electron Affinity decreases down a group because those elements have increasing number of electrons, which require a greater number of electron shells. Due to the shielding effect, the valence electrons of these elements are less attracted to the nucleus and the atom is, therefore, less likely to attract another electron. Electron Affinity increases across a period because these elements contain more protons and, therefore have a greater nuclear charge. Due to the principle of Coulomb's law these electrons are more attracted to the nucleus and the nucleus is more likely to attract another electron with this additional strength in charge.

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The ionic radii decrease with positive ions and increases with negative ions. So, among positive ions (cations), the number of protons increases. This decreases the radius because it pulls in the electrons towards the nucleus. (The electrons are negatively charged and protons are positively charged.) With the negative ions (anions), the extra layers of electrons that are added increases the ionic radii.

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The size of the atomic radius generally decreases in size as you go across the periodic table because the number of protons and electrons are increasing. Since a proton has a better shielding effect than an electron, the electrons are pulled towards the nucleus, so there is a smaller atomic radius.

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The electronegativity increases across a periodic table because the decrease in the size of the atoms as you move across the periodic table. The smaller the size of the atom, the easier it is to attract electrons from atoms bonded to it

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Atomic Radius is the radius of an atom. The atomic radius is similar to the ionic radius. As you move across the periodic table the atomic radius decreases and as you move down the group, the ionic radius increases. The coulomb's law effects the atomic radius because the higher the attraction between the electrons and nucleus, the smaller the atomic radius. The shielding effect and the shell model effect the atomic radius because the more electron shells, the larger the atomic radius. Electron repulsion effects the atomic radius because instead of creating a new electron shell, the electrons double up.

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Electron affinity increases upwardly on the periodic table and it also increases from left to right. This is because the electrons that are added to the energy levels get nearer to the nucleus. This means that there is a stronger attraction between the nucleus and its electrons.

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Ionization Energy will increase across a period and decrease down a column because the Coulmbic attraction will increase since it will be harder to get an electron out of the orbital. The shielding effect causes an effect by preventing the outermost electrons from realeasing out of the atom, wich means as you go across the period you need more energy to release the atom and less as you go down. The electron repulsion will make ionization energy increase across a period because the electrons are not being repulsed as much and so more energy will be needed to do so.Finally, the shell model will increase the ionization energy across a period because as more electrons are added in the orbitals, it is harder to break them out of orbit.

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Ionic Radius: Cations are smaller the more electrons they lose and anions are bigger the more electrons they gain. For cations, an increase of orbitals makes the radius go down and for anions it is the opposite. This rule also applies to electron shielding because it increases with shell model.

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Ionization energy increased as you go across the periodic table because it takes more of an attractive force for one of the outer electrons based on the nuclear charge, which also means it takes more energy to pull the outer electron away. The screening and shielding effect does not have much effect on increases in ionization energy.

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The atomic radius decreases from left to right because as the atom gains protons the Coloumbic attraction between two of the same atoms increases making its radius smaller. As it goes down the group electron shielding makes the electrons more spread out as it goes down making the atomic radius increase as it goes down

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ionization energy increases from left to right on a period and increases up a group. the greater the force between the nucleus and the incoming electrons, the more energy needed to remove an electron from the outer shell. so based on coulombs law as you increases the number of protons therefore increasing the force, the more ionization energy need which is why the trend increases from left to right of a period. in groups however, the more shells the atom has the greater the distance between the nucleus and the incoming electrons therefore decreasing the force and the energy so ionization energy increases up a column.

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An Ionic Radius is the radius of an ion. As you move across a period, the Ionic radius decreases. However, as you move down the group, the ionic radius increases. The Ionic radius decreases as you move across a period because of Coulomb's law. Since you gain more protons, the attraction becomes stronger making the radius smaller. The shell model and shielding effect the Ionic radius because the more electron shells you have, the bigger the ionic radius. Lastly, electron repulsion effects the size of the ion because instead of creating a new electron shell, the electrons double up.

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electronegativity increases from left to right on a period and increases up a group. the more protons an atom has the greater the tendency to attract electrons because positive charges attract negative charges but 2 negative charges repeal each other based on electron repulsi

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Atomic radius: gets smaller moving up and to the right on the periodic table. A proton has a larger effect than an electron so the electrons are pulled toward the nucleus more the radius is smaller. It is caused by electron shielding, the less orbitals there are the less shielding there is so the larger an atomic radius is.

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The electron negativity decrease as you go down a group because it's going farther away from the nucleus making it a weaker type of attraction because of its distance. While it increases as you go right because it gains electrons making the attraion bigger meaning it is more likely to pick up other electrons.

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atomic radius increases down a group and increases from right to left of a period. this is because as you go across a period more protons are added to that atom bringing the electrons in closer making the radius smaller. this can be determined using the shell model.

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The ionice radius increases as you go left to right because it's gaining protons which adding onto the electron repulsion and pushing the electrons into other orbitials increasing its radius. The same explanation can be used to describe why the ionic radius increases as you go down the group

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Ionization Energy: The further an electron is from the nucleus the easier it can be removed from an atom and that lowers the ionisation energy. The higher the nuclear charge the higher the value. Because the nuclear charge in the elements on the right of the periodic table are greater those have a lower electron repulsion and a higher ionization energy. The shell model, deriving from Coulombs law, explains and predicts this value as well because you can see the relative energies of the electrons and minimal energy required to remove them.

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Ionic Radius increases down a column and decreases across a period because the Coulombic force of attraction will decrease across a period since there will be a smaller pull between the electrons and protons, and as you go down a column there will be an increase in the columbic attraction. The ionic radius will increase down a column and decrease across a period because the shielding effect is blocking some electrons from the positive charge in the nucelus, so the atom can not grow very large because it does not think that is needs to be repulsed. The electron repulsion causes an effect on the ionic radius because as you move down a column, the electrons have a stronger repulsion with the protons due to larger difference from one element to the next in the same column. The elements in the same period will have a decrease in ionic radius because the electrons are pulled closer to the protons, resulting in a larger radius. Finally, the shell model's effect will cause an increase down a column becuse there are more elctrons which means the electrons are getting further away from the nucleus.

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Ionization energy decreases down a group because as the atomic number of an atom increases, so does the number of electrons it requires to remanin neuturally charged. These electrons fill up an increasing number of shells, causing the valence electrons to be further from the nucleus. Due to the shielding effect, these further away electrons are less attracted to the nucleus and, therefore, require less energy to remove. Additionally, ionization energy increases across a period because with an increasing number of protons comes an increase in nuclear charge which, according to Coulomb's law, causes the electron to become more tightly bound to the nucleus and, therefore, require more energy to be removed.

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based on the shell model, ionic radius increases in anions across period and increases down a group. cations decreases across a period and decreases down a group. the difference in the 2 atoms is that cations have a positive charge so when they gain electrons they get smaller because the positively charged nucleus attracts the negative electrons. anions get larger because the negatively charged nucleus repels the negative electrons coming in therefore making the radius larger.

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Electron affinity ncreases upward for the groups and from left to right across periods of a periodic table because the electrons added to energy levels become closer to the nucleus, thus a stronger attraction between the nucleus and its electrons.

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Electronegativity increase across a period as you go left to right. More specifically the closer you are to flour ine the more electronegative it will be. The reason for this is as you go across the period the element will have the same amount of electron orbitals but greater electron repulsion becaus of the increase of protons. The electronegativity of the element go down as you go down the groups because they are moving farther away from fluorine and even tho they are gaining electorns and more electron repulsion, they are moving into farther out shells making them less electronegative .

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Ionic radii decreases across periods because effective nuclear charge increases. That is, the net positive charge experienced by an electron in the atom increases as a result of the number of protons in the nucleus increasing.

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In any one period, the outer electrons lie in the same valence shell. As atomic number increases, effective nuclear charge increases, so there is an increased attraction of electrons to the nucleus. Therefore across the period, size of atom decreases.

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electron affinity decreases down a group and decreases from right to left across periods. this is because as the number of shells increase the electron affinity decreases because the nucleus and the incoming electrons get farther away. so based on Coulumbs law when the distance increases the force would decrease which would also decrease the electron affinity.

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As you go across the periodic table the ionization energy increases also when you go down a group the ionization energy decreases. Ionization energy increases because the atomic radius decreases it becomes more difficult to take away an electron.

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Electronegativity: As you move across the periodic table from left to right the electronegativity rises, working from the bottom of groups to the top (also making fluorine the most electronegative). The more protons there are in the nucleus the more likely it is to attract the electrons. as well, the new electrons are always being shielded and when they are further to the right, they have more shells and more shielding electrons. The reason it increase as you move up a group is because the lower ones are farther from the nucleus' attraction. The shell model is based on coulombs law which allows the statements above about the elements with more shell models being more electronegative.

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As you go left to right on a period the number of protons in the nucleus increases, and with it the elactronegativity. This causes electronegativity to  increase from left to right

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Electron Affinity is the ability for an atom to accept an electron. Electron Affinity increases as you move across the period, but decreases as you go down a group. This relates to Coulomb's law because as the atom gains more protons it will have a higher nuclear charge that will attract electrons from other atoms. However, because of electron shielding, it causes the nuclear charge to become weaker, which then makes the atom less likely to attract an electron. This is based on the shell model and the more shells you have, the more shielding there will be. Lastly, electron repulsion effects electron affinity because when the electron begin to double up, which increases the shielding effect.

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Ionization energy, the amount of energy needed to remove electrons, increases from left to right on the periodic table. This occurs because the distance between the Nucleus and the electrons increases. The higher the the shielding effect, the greater the ionization energy. There are multiple levels of ionization energy depending on the number of electrons removed .

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Electron Affinity: trends for electron affinity include moving down the group makes the value less and groups 6 and 7 have high values unlike the rest of the periodic table. The way the affinity goes down as you move down group and the exception can be explained because the stronger the incoming electrons attraction to the nucleus is the more energy is released and therefore making a higher electron affinity. Because groups 6 and 7 have negative charges already and because of Coulombs law, the force is greater as well. The shielding electrons make up for the nuclear charge as you move down a group, and when there are more electron shells there are more shielding electrons like in groups 6 and 7.

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Ionization energy increases as you go across a row because the number of protons increases which causes a stronger coulombic attraction between the protons and electrons causing it to be harder to remove the valence electron which means higher ionization energy and the elements on the right side of the periodic table have an almost full valence shell meaning it takes more energy to remove an electron than to gain one. It decreases as you go down a group because of electron shielding.

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Electronegativity increases as you go down a group becuase there is more electron shielding and more distance between the nucleus and the electrons. The electronegativity increases as you go across a row because the charge increases and this attracts a bonding pair of electrons. The more protons the higher the nuclear charge.

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The ionic radius decreases as you go across a period because the nuclear charge grows because of more protons being added to the core so the electrons are being pulled more tightly to the center. The ionic radius increases as you go down a group because of the increase in electrons and electron shielding.

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Atomic radius increases as you go from top to bottom of a group because of electron shielding. The pull of the protons is being blocked by the electrons where is cannot pull with as much force. It decreases as you go across a row because the valence electrons are being added to the same orbital and protons are still increasing so when this happens then it is more tightly held together because of the increasing positive charge.

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The atomic radius decreases as you go across a period because the number of protons and number of valence electrons are both increasing causing an increase in coulombic attraction which pulls the electrons closer to the nucleus which makes the atomic radius smaller. The atomic radius also increases as you go down a column because of electron shielding which allows inner electrons to shield the attractive force of the protons in the nucleus from the outer valence electrons making the atomic radius larger.

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Electron affinity increases as you go across a period because the atomic radius decreases. As you move left to right the atoms are decreasing in size the electron affinity is greater because the distance between the nucleus and valence electrons is less and the coulombic attraction is greater. As you go down a group the electron affinity decreases because the atomic radius is increasing which means the valence electrons are farther away and have a weaker coulombic attraction.

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Electronegativity increases across a period because elements on the right side of the periodic table have a fuller valence shell and they are more willing to accept electrons and form bonds where the elements on the left side will give up their electrons not gain more. It decreases as you go down a group because the atomic number (number of protons) increases and so the distance between the valence electrons and the nucleus increases.

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Ionic radius decreases as you go across a period because when a neutral atom gains or loses an electron its radius either increases or decreases. When an atom gains an electron to become an anion it increases in ionic radius and when an atom loses an electron and becomes a cation it decreases in ionic radius. As you move down a group the number of electron shells increases therefore increasing the ionic radius.

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The ionization energy increases as you go left to right  because of being held tighter to the core due to the higher effective nuclear charge. And it decreases as you go down a group because the atomic  radius increases and the electrons are farther from the nucleus making them easier to remove

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Electron affinity increases as you go left to right on the periodic table because the more protons an atom has in its nucleus, the more likely it is to attract an electron because of its strong positive core. As you go down a group, the distance between the nucleus and electrons grows. And this makes a weaker nucleus-electron attraction.

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Electron affinity increases as you go across a period because protons are added and have large coulombic attraction on electrons causing the electron affinity to be greater. Electron affinity decreases as you go down a group because electrons are added to orbitals that are farther away from the nucleus, shielding and electron repulsion increase, and columbic attractions decrease causing electron affinity to decrease.