Periodic Trends
The ability of an atom to attract electrons within a chemical bond; it increases as you move up and to the right on the periodic table.
What is electronegativity?
Due to certain periodic trends moving in opposite directions and counteracting each other, this is the idea that elements diagonally adjacent to each other often have similar properties.
What is the diagonal effect?
This group contains elements, primarily metals, with three valence electrons; they often behave as Lewis acids and tend to form X2O3 compounds with oxygen and XY3 compounds with halogens.
What is Group 13?
This group, which contains metals, metalloids, and nonmetals, exhibits a wide range of properties due to its six valence electrons, including metallic, covalent, and ionic bonding; elements tend to form anions with a -2 charge to obtain a full outer shell; oxidation states of +6, -2, or +4 (inert-pair effect); oxygen is a notable member of this group.
What is Group 16?
This is the only halogen that is liquid at room temperature; the rest are solids or gases.
What is Bromine?
The size of an atom, measured from the middle of the nucleus to the outer electrons; it increases as you move down and to the left on the periodic table.
What is atomic radius?
The tendency of heavier elements in groups 13-17 to exhibit lower oxidation states, as in give up electrons less easily, due to the larger positive mass of the nucleus holding electrons more tightly (the shielding effect is weaker in these elements due to placement of orbitals).
What is the inert-pair effect?
Also known as the halogens, this group contains highly reactive nonmetal elements with seven valence electrons; they have relatively high electronegativities due to their tendency to pull electrons toward themselves to obtain a full outer shell; they are strong oxidizing agents (meaning they are reduced easily), and often serve as the anions in ionic salts or acids.
What is Group 17?
This group contains highly stable, nonreactive gases with full sets of valence electrons; they do not react easily because they have full outer shells, so they are stable and do not want to lose or gain any electrons; they exhibit fluorescence when conducting electricity.
What is Group 18?
Most elements in Group 16 exhibit this, or the tendency to exist in different forms or structures in the same physical state.
What is allotropy?
The energy required to remove the outermost electron from an atom; it increases as you move up and to the right on the periodic table.
What is ionization energy?
This element is diagonally adjacent to lithium, causing them to share characteristics such as similar electronegativities and solubilities.
What is magnesium?
Also known as alkali metals, this group contains highly reactive, soft metals with one valence electrons; they form cations in ionic compounds by giving up their electron to obtain a full outer shell; they react violently with water to form strong bases with hydroxide ions.
What is Group 1?
This group contains a range of elements, including metals, metalloids, and nonmetals, that have four valence electrons; these electrons give the elements a variety of properties, able to gain or lose electrons in ionic bonds and able to share electrons in many different configurations in covalent bonds; elements usually have oxidation states of +4 or +2 (due to the inert-pair effect).
What is Group 14?
This is the only Group 15 element that is a gas at room temperature.
What is Nitrogen?
This element is in the same group as chlorine but has a higher electronegativity.
What is fluorine
Although you would expect lead to have an oxidation state of +4 due to its position in group 14, it more commonly exists in this other even state due to the inert-pair effect.
What is +2?
This group, which contains metals, metalloids, and nonmetals, exhibits a wide range of properties due to its five valence electrons, including ionic, covalent, and metallic bonding; elements can give up five electrons or gain three electrons to fill their outer shell, resulting in oxidation states of +5, -3, or +3 (due to the inert-pair effect).
What is Group 15?
Also known as alkaline earth metals, this group contains fairly reactive elements with two valence electrons; the elements easily give up two electrons to form cations with a +2 charge; primarily shiny, soft, ductile metals; form strong bases with hydroxide when reacting with water.
What is Group 2?
Certain elements within various groups exhibit this bonding property, signified by BrINClHOF.
What are diatomic elements?
This group 1 element has a greater ionization energy than potassium and a larger atomic radius than lithium.
What is sodium?
Bonus! This is the scientist that first created the periodic table.
Who is Dmitri Mendeleev?
These two groups often react with each other to form strong electrolytes with cations and anions of +/-1 charges.
What are Groups 1 and 17?
The reactivity and pairing of elements depends not only on their number of valence electrons, but also on the placement of electrons within these regions.
What are orbitals?
Bonus! Acids with hydrogen bonded to a single element are called binary acids. This is what acids are called when they contain hydrogen bonded to a polyatomic ion.
What are ternary acids?