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As you travel down the periodic table, the atomic radius increases due to the fact the energy levels are increasing as well. Since you have more electrons, they fill up more shells and as a result they become more and more distant from the nucleus, causing the  radius to increase. Going left to right, there is are more protons in the nucleus and therefore a greater attraction between the electrons as they are pulled closer to the nucleus. This decreases the radius

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The atomic radius decreases going across the periodic table because because more electrons are added to the atom, which results in a stronger attraction between the electrons and the protons in the nucleus, causing the radius of the atom to decrease.

The atomic radius increases going down the periodic table because the number of energy levels increase, resulting in more distance between the nucleus and outermost electrons, so the radius of the atom increases.

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Going down a group, atomic radius increases because the number of shells for electrons is increasing which makes the radius larger. Radius decreases going left to right on a period because there are are more protons in the nucleus, which create a greater attractive force and pull the electrons to the nucleus and make the atom smaller.

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The atomic radius decreases across a period because elements farther right in a period will have a higher number of protons, and thus have a greater attraction towards the electrons. As a result, the electrons will be pulled in closer.

The atomic radius increases down a group because elements farther down in a group have more occupied energy levels than those above. With more occupied energy levels the electrons will be farther apart from the nucleus and the atomic radius will be larger.

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The atomic radius increases as you go down a group because there are more energy levels being added to the atom. The distance from the outside of the atom to the nucleus increases as you add more energy levels.

The atomic radius decreases as you go across a period because as you go through the period, the number of protons increases This means that the attraction between the nucleus and the electrons will get stronger as you go across the period, pulling in the electrons to the nucleus and making the atomic radius smaller.

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The atomic radius decreases as you go across a period because as number of protons increase, the electrostatic force between the electrons and protons increase. This results in the radius of the atom decreasing because electrons are being drawn into the nucleus with more protons.

The atomic radius increases as you go down a group because there are more energy levels and orbitals as you go down a group. This means the overall radius of the atom gets bigger as you go down a group.

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The atomic radius increases as you travel down a group and to the right across a period because the distance between charged particles increases as energy levels are being added. Since the force of attraction decreases due to the added energy levels, the atomic radius increases.

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As you go from the top to the bottom of a group, the atomic radius would increase, because every time you go down a row, there is a completely new energy level that has instantly increased the size of the atom by an entire shell.

As you go from the left to the right of a period, the atomic radius would decrease, because as more electrons and protons are getting added to an atom (say from Na to Cl), the charges attracting the electrons to the protons increases, almost tightening the figurative "knit ball" that is an atom.

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Electronegativity increases across the periodic table from left to right because the atomic radius decreases. This means that distance between the electrons and protons is lowered, leading to an increased electronegative force between the valence electrons and protons.

Electronegativity decreases from top to bottom of the columns because the atomic radius increases, leading to an increased distance between valence electrons and protons and decreased electronegative force.

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The atomic radius increases as you go down each row (groups) since more energy levels exist. Because of this, the distance between electron (in the outermost energy level) and the nucleus increases.

The atomic radius as you go across the periodic table since the number of protons increases but the number of energy levels stay the same. Because of this, the attraction between electron and nucleus increases, drawing electrons closer to the nucleus and decreasing the distance (and atomic radius)

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The atomic radius increases as you go down a group as the number of electron shells increases, which would cause the size of the atom to be larger.

The atomic radius decreases as you move across a period because the number of protons increases, so the attractive force of the protons pulling in the electrons would increase, causing the overall size of the atom to be smaller.

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The atomic radius increases going down a group as there are more electrons in the atom. As a result, more orbitals are being filled with electrons, causing the atomic radius to increase in size. The atomic radius decreases going across a period to the right as there are more protons and neutrons, creating a stronger attractive force pulling on the electrons. As a result, the radius decreases in size.

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The atomic radius decreases as you go across the peiodic table and as you go down the group becuase the number of energy levels increase due to more electrons and more protons in the nucleus. There will be be a greate arrtraction with them pulling the shell making the size smaller.

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Ionization energy increases across a period and decreases down a group becuase in a period there will be a bigger force pulling from the protons so it would require a bigger force to overcome this pull. It decreases down a column becase the number of shells increase which makes the pull on those eletrons from the nucleus less.

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The ionization energy increases across a period because elements farther along a period will have a smaller atomic radius.The valence electrons will have a greater attraction keeping them in the atom and will need more ionization energy to be removed.

The ionization energy decreases down a group because elements farther down in a group will have more occupied energy levels and thus a larger atomic radius. A higher atomic radius will mean that the attraction between the nucleus and the valence electrons is not as high, meaning the ionization energy needed to remove the electron is lower.

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IE increases going left to right because there is a stronger attraction between the electrons and the nucleus, making it more difficult to overcome that force and create an ion.
IE decreases going down a group because the valence electrons are further from the nucleus (hence the nucleus has a lower attractive force on them), making it easier to remove the electrons and create an ion.

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The atomic radius decreases across a period because the increasing number of protons cause a higher level of coulombic forces to be present, thus pulling the electrons closer to the nucleus.
The atomic radius increases down a group because the the number of shells in the element increases down a group. As the number of shells increase, so too does the atomic radius.

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Electronegativity decreases from the top of a group to the bottom which increases the atomic radius. Electronegativity increases from the left to the right along with an increase in valence electrons attempting to get a full octet.

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The Ionization Energy increases across the periodic table because the smaller the atomic radius is, the more attracted electrons are to the nucleus. More attraction would require more energy to remove an electron. On the other hand, the ionization energy decreases going down the periodic table because there's less attraction between the electrons and nucleus which requires less energy to remove an electron from the atom.

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The atomic radius decreases as you go across the periodic table because the ratio of protons to electrons increases, meaning that the number of protons is greater than the number of electrons. This increases the attractive force in the atom and pulls the electrons inwards decreasing the radius.

The atomic radius increases as you go down the periodic table because electron orbitals/shells increase as well. This increases the distance from the valence shell to the nucleus which increases the atomic radius.

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The ionization energy increases as you go across a period because there are more protons being added, meaning that the attraction between the electrons and the nucleus gets stronger, and more energy is required to remove the electron.

The ionization energy decreases as you go down a group because as you go down, the atomic radius increases, so the electrons are further away from the nucleus. This means that the attractive force between the nucleus and the electrons won't be as strong, and it will take less energy to remove the electron.

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The ionization energy increaes going across the periodic table because the number of protons and electrons increases, so there will be a greater attractive force between the protons in the nucleus and electrons in the shells, and it will require more energy to overcome this force.

The ionization energy decreaes going down the periodic table because the number of electron shells increaes, meaning there is more distance between the protons in the nucleus and the valence electrons, resulting in a smaller attractive force between them that requires less energy to overcome.

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Ionization energy increases as you travel up a group or to the left across a period as the distance between charged particles decreases due to their being less energy levels. Since the force of attraction increases due to less energy levels being present, the amount of energy needed to remove a valence electron from the atom increases as well.

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Patterns with ionization energy have to do with atomic radius. As you go down the periodic table, the atomic radius increases. This means that the distance between electron and nucleus increases, and attraction between the two is smaller. This means that smaller force would be required to overcome ionization energy, so ionization energy decreases as you go down the periodic table.

As you go across the periodic table, the atomic radius decreases, meaning the attraction between nucleus and electrons increases. This means more energy is required to overcome ionization energy, therefore ionization energy increases.

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Atomic radius decreases across a period because of the fact that there is an increase in the number of protons and electrons in an atom of an element as we move across, and one proton has more power than an electron, so there will be a greater force of attraction between them making the radius smaller

The atomic radius increases as we go down a group because of the fact that there are more electrons, and more orbitals are filled with more electrons, which causes the radius to hence increase.

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Ionization energy decreases going down a group. As the atomic radius increases going down a group, the distance between the nucleus and electrons is larger. As a result, the attractive force pulling on the electrons is weaker. Therefore, the energy needed to eject an electron from the atom decreases as well. Ionization energy increases going across a period as the atomic radius decreases. This means that there is a stronger attractive force pulling on the electrons from the nucleus, causing the energy needed to eject an electron to increase.

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The ionization energy of an atom increase as you go across a period because the attraction between the nucleus (protons) and electrons increases as number of protons increase. As electromagnetic forces increase between atoms when going across a period, it takes more and more energy to remove an electron from the atom. This is why ionization energy increases.

The ionization energy decreases when you go down a group because there are more energy levels as you move down a group. This means electrons are farther away from the nucleus hence as you go down, the electromagnetic forces between electrons and the nucleus decrease. This means less energy is required to remove an electron from the atom which is why ionization energy will decrease.

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Ionization energy increases as you move left to right across the table due to the atomic radius. As the valence electrons are closer to the nucleus, they require more energy to be removed since there is a stronger bond. On the other hand IE decreases going down the table since the valence electrons are further from the nucleus and have a weaker attractive force. This makes it far easier to remove the electron from the atom

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Electronegativity increases across a period because elements farther right in a period will have a lower atomic radius. As a result, there will be greater attractive forces holding the electrons to the atom, indicating a greater electronegativity.

Electronegativity decreases down a group because elements farther down in a group will have more occupied energy levels and thus a higher atomic radius. As a result, there will be less attractive forces holding the electrons to the atom, indicating a smaller electronegativity.

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As you go across a period, the ionization energy would increase. This is because as you go across, the number of protons increases so there would be a stronger attractive force between the electrons and the protons. This would cause the amount of energy required to remove one electron to increase.

As you go down a group, the ionization energy would decrease. This is because, as you increase the number of electron shells, the valence electrons are getting further and further away from the nucleus, so the amount of energy required to remove one electron would decrease as you keep adding shells.

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Electronegativity increases across a period because there is a greater (positive) attractive force from the nucleus due to the increased amount of protons; the electrons from other elements are attracted to this force.
Electronegativity decreases going down a group because the nucleus has a smaller attractive force on the electrons due to the increased size of the atom, making other elements' electrons also less attracted to that atom.

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As you go from the top to the bottom of a group, the ionization energy would decrease, because the further away an energy level would get from the nucleus, the weaker its electrostatic pull would be, thereby decreasing the energy needed to push it to the next energy level (or just out of the atom).

As you go from the left to the right of a period, the ionization energy would increase, because as the number of electrons in the outer shell increase, they shield one another from photons through greater electrostatic forces that would make it harder to release them into greater energy levels.

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Ionization energy increases across a period because the atomic radius decreases, thus increasing the force of attraction between the protons and electrons. More energy is required to displace electrons as that force of attraction increases.

Ionization energy decreases down a group because the atomic radius increases down a group. This causes there to be a smaller force of attraction between the protons and electrons, which decreases the energy required to displace an electron.

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The electronegativity increases when you go across becuase the ditance between the electrons and nuclues where the protoms are decreases which means that there is a greater force between the elctrons and nuclues. It dreases as you go down a column because there is a biggere distnace between the elecons and the protons which means that there is a lesser force.

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The electronegativity increases as you go across a period since the atomic radius decreases. This means that the attraction between the electrons and the nucleus is stronger since they are closer together.

The electronegativity decreases as you go down a group because the increased atomic radius means that the electrons are further away from the nucleus and the attraction between the electrons and the nucleus isn't as strong.

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The electronegativity of an atom increases when you move across a period because atomic radius decreases. This means the attraction between electrons and the nucleus of an atom is high hence the electronegativity increases.

The electronegativity of an atom decreases down a column as the atomic radius increases. This means electrons are attracted to the nucleus with less force and therefor require less energy to bond.

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Ionization energy increases across a period because due to the fact that we have more protons available, there will be a greater force of attraction between the protons and the electrons, and we'd need more energy in order to move the electrons to a higher energy level.

Ionization energy decreases down a group because more electron orbitals come into an atom as we move down a group, which spaces out the electrons far away from the protons, hence making the electrostatic energy between them weaker.

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Electronegativity increases going across the periodic table becuase atomic radius decreases while the number of protons in the nucleus increases, meaning there is a stronger attractive force from the nucleus, so  the nucleus can attract electrons more strongly.

Electronegativity decreaes going across the periodic table because the atomic radius increases so the attractive force between the nucleus and electrons decreases and other electrons will be less attracted to the atom.

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The ionization energy increases as you go across the periodic table since the ratio of protons to electrons increases which increases the attractive force between them. This means it would require greater force to knock the electrons out of its Coulombic attraction.

The ionization energy decreases as you go down the periodic table because the atomic radius increases as you go down the table. This means there is less of an attractive force between the protons and electrons, meaning there is less energy requires for the electrons to escape the atom.

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The atomic radius decreases from left to right on the periodic table because there are more protons but the same number of electron shells, meaning that the attractive force between the atoms with more protons will be greater.

The atomic radius increases from top to bottom because the number of electron shells increases, making the radius larger.

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Electronegativity increases across the periodic table to the right as the atomic radius decreases. This means that the protons in the nucleus have a stronger attractive force pulling on the electrons. Therefore, the electronegative force between the valence electrons and protons increases. Electronegativity decreases down a group as the radius is increasing. Therefore, the attractive force between the protons in the nucleus and valence electrons is weaker. Electronegativity is therefore also decreasing as it's the force of the protons pulling on the electrons.

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Electronegativity increases across a group since there are more protons- this it turn results in a greater attractive force between the protons and electrons in the atom. However it decreases going down a group since there are fewer protons and an overall larger attractive force. As a result the electronegativity decreases.

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Electronegativity increases up a group and moving to the left across a period because the atomic radius decreases. As a result, the force of attraction holding the electrons to the atom will be greater indicating a higher electronegativity value.

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Electronegativity increases across a period because atomic radius decreases across a period. This will cause electrons to have a greater force attracting them to the nucleus.

Electronegativity decreases down a group because the atomic radius increases down a group. This will cause the attractive force between electrons and the nucleus to decrease.

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Atomic radius decreases from the left to the right of the table since there is an increase in the number of protons. The atomic radius increases from top to bottom of the table since it is taking in more electrons.

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Electronegativity has to do with atomic radius as well. As the atomic radius increases, the distance between protons and electrons increases. As a result, the electronegativity also decreases because of this distance and weaker attraction between proton and electron and electronegative force decreases.

Electronegativity increases as you move across the periodic table since the distance between proton and electron decreases. The attraction is stronger, meaning that the protons and electrons are closer. Electronegativity increases because of this distance and electronegative force decreases

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Ionization energy increases from left to right because the electronegativity increases, which means that more energy is needed to remove the electron.

Ionization energy decreases from top to bottom because the electronegative force decreases between the valence electrons and protons (due to increased distance), which leads to less energy needed to create an ion.

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As you go from the top to the bottom of a group, the electronegativity would increase, because the atomic radius would be increasing, thereby greater distance between valence electrons and protons. This would mean that when bonds are formed, the outer electrons would be further from the nucleus, decreasing the electrostatic force between two atoms.

As you go from the left to the right of a period, electronegativity would increase, because these atoms gain a greater electrostatic charge in tandem with a smaller atomic radius. The combination of these two factors increases the overall electronegativity.

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Electronegativity increases across a period because of the fact that there is a smaller atomic radius, hence we need a greater amount of energy to move the electrons.

It decreases as we go down a group because the radius increases, which causes the distance between the electrons + protons to increase, which causes the electronegativity weaker.

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Electronegativity increases across a period because the distance between protons and electrons decreases, so the force between the nucleus and electrons would be stronger.

Electronegativity decreases across a group because the distance between the protons and electrons increases, so the force between the nucleus and the electrons would be weaker.

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Electronegativity increases across as you go across the periodic table because the ratio of protons to electrons increase in the same energy level which increases the Coulombic attraction in the atom.

Electronegativity decreases as you go down a group because the atomic radius increases as energy levels increase. This increases the distance between the valence electrons from the nucleus.

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Ionization energy increases from left to right of the periodic table since the electrons and nucleus is developing a stronger attraction and therefore, more energy is required to take out an electron.

Ionization energy decreases as you go down a group since the electrons and nucleus is becoming more distant and developing a weaker attraction. Therefore, less energy is needed to take out an electron.