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Vertical rows on the periodic table.

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Horizontal rows on the periodic table.

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The amount of energy required to remove an electron from an isolated atom or molecule.

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Atomic radius is half the distance from nuclei of identical  neighboring atoms in a solid state.

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Electronegativity is when an atom is able to share an electron with another atom in a chemical bond.

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The vertical rows in the periodic table.

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The horizontal rows in the periodic table

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Ionization energy is the amount of energy that a gaseous atom in the ground electronic state must absorb to discharge an electron.

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Atomic radius is the total distance from an atom's nucleus to the outermost orbital of an electron.

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Electronegativty is a measure of a tendency of an atom to attract a bonding pair of electrons

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The vertical rows of the periodic table. Elements in the same row have the same amount of valence electrons.

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The horizontal rows of the periodic table. The elements that are in the same period have the same number of energy levels.

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The energy required to pull an electron from an ion.

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The distance between the center of the nucleus and the outer border of the electron cloud.

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An atom's ability to attract electrons. The higher it is, the easier it is for it to attract them.

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Elements arranged from top to bottom. Elements in the same column share the same number of electrons.

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The horizontal rows in the periodic table. All the elements on the same row have the same amount of energy shells.

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The level of energy needed to change an electron from a gaseous to an ion atom.

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The measure from the nucleus to the outermost electrons.

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An atom's ability to attract electrons.

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Elements arranged in groups (from left to right), have the same number of electrons in the outermost shell, this are called valence electrons.

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Elements arranged in periods share the same number of energy shells.

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It’s the energy required to remove an electron from a gaseous atom or ion.

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The elements that are organized from top to bottom. The elements in the same group share the same electrons in their outer shell.

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This are the rows from left to right in the periodic table, all the elements on the same period have the same energy shells

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Is the energy required to remove an electron from a gaseous atom or ion

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Is a measure of the typical distance from the nucleus to the

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The ability to attract electrons.

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Hoe strong atoms attract electrons to themselves.

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The distance from the nucleus and the furthest part of the cloud of electrons.

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The energy needed to take away an electron from a molecule or an atom. 

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The energy needed to take away an electron from a molecule or an atom.

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Vertical columns that organize elements according to the number of valence electrons they contain.

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Horizontal rows that organize elements according to the number of energy shells they contain.

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Ionization energy refers to the amount of energy needed to remove an electron from an isolated atom or molecule.

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Ionization energy refers to the amount of energy needed to remove an electron from an isolated atom or molecule.

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The distance from the center of the nucleus to the outermost shell containing electrons

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The measurement of an atom's ability to attract electrons to itself when bonding.

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The horizontal rows on the periodic table that have same amount of electron shells.

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Similarly to periods, groups also define a characteristic shared by various collections of atoms. These columns help easily identify how many valence electrons atoms have.

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Periods are sections of the periodic table which help us define similarities between the elements. These are the rows which determine the number of electron shells a collection of atoms will have.

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Ionization Energy can be defined as the energy needed to remove an electron from an atom in gaseous state.

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It is defined as the distance between the nucleus of an atom and the limit or outer shell of an atom’s electron field. These have a simple relation with the amount of protons an atom has. The greater the amount of protons, the lesser the atomic radius since the nucleus will have greater attraction to the electrons, therefore making the radius smaller.

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An atom’s ability to attract and keep in orbit electrons. The greater the electronegativity of an atom in a bond, the more likely it is for there to be an unevenly distributed amount of electrons.

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The measure of the distance between the nucleus to the edge.

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The ability of the atom to attract electrons.

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