FINAL EXAM- Periodicity

A horizontal row of elements in the periodic table.

a set of elements with common properties or of compounds related in composition or structure. SAME AS PERIOD- horizontal row of elements on the periodic table

having the same numbers of electrons or the same electronic structure. Ex. F and O-1

the quality or character of being periodic; the tendency to recur at intervals. The periodic law states that the physical and chemical properties of the elements recur in a systematic and predictable way when the elements are arranged in order of increasing atomic number.

The energy required to remove AN electron from a neutral atom (not ion) of an element in the gaseous state

The energy change that occurs when an electron is acquired by a neutral atom (most atoms release energy when they acquire electrons).

measure of the ability of an atom in a compound to attract electrons from another atom in a compound.

One half of the distance between the center of identical atoms that are not bonded together.

• Column 1 or 1A (except H) • Shiny, soft, low density, never found in elemental state in nature, one valence electron • Loses one VE to form an ion with a +1 charge • Reacts easily with oxygen • Produces hydrogen and a solution in exothermic reaction with water (produces heat, basic substance left behind- bases can be just as harful as acids) • Will float (low density) • Need the ion in your diet

• Column 2 or 2A • Similar to alkali metals- just not as • 2 valence electrons, loses these two valence electrons to form an ion with a +2 charge • Not as vigorously react • Not as shiny, soft, etc • A little harder, more dense, etc

• Column 7 or 17 • All nonmetals • 7 Valence electrons • Gains one electron to form ions with a -1 charge • Diatomic

• Column 8 or 18 • Chemically inactive, rarely form compounds • Has 8 Valence electrons (except He which has only 2 electrons total) • Stable

• Starting in column 3 and all the way over- everything beneath the staircase excluding La, Ac, and Al • Form ions with varying charges • Good conductors of electricity • Have a high luster • Less reactive than alkali and alkaline-earth metals- some so unreactive that they exist in in nature as free, single elements. • D-block element s

• The two rows of elements at the bottom + La and Ac • F block • Same as transitional with varying charges • Lanthanides and Actinides

• Elements that border above the periodic table plus Ge and Sb (B, Si, Ge, As, Sb, Te, and At) • Has some characterists of metals • Some characteristics of nonmetals • Solids at room temperature • Less malleable than metals • Not as brittle as nonmetsl • Semiconductors of electricity

• First two columns, minus H, plus Al • Always loses the same amount of electrons when they lose ions • Form ions that always have the same charge

• Elements to the right of metalloids, plus H • Opposite of metals • Not malleable • Not ductile • Doesn’t conduct hear and electricity • Many valence electrons

• 2 different series* • Make up the inner-transitional metals* • Two rows of elements at the bottom • Lanthanides is the top one • Actinides is the bottom one • F block elements • Actually wedged between groups 3 and 4 • Shiny metals • Similar in reactivity to Group 2 alkaline-earth metals

• S includes the alkali and alkaline earth metals • P includes the nonmetals • D includes the transition metals • F includes the inner transition or rare earth metals

• Corresponds to the column number • Only works for columns 1, 2, and 13-18 but we still refer to 13-18 3-8 • • column number for 1-3 • • for number of columns away from the nobel gases for 5-7 • column 4 can be + or – • column 8 has no charge • Ex. Be is +2, N is -3, and Si is + or – 4

• Number of valence electrons=family/group/column • Row number (horizontal)= number of energy levels • Only works for S and P block • D block- number of energy levels= row #(n)-1 • F block- number of energy levels= row #(n)-2 • Ex. H has one, Al has 3, Hg has 5, and Th has 5

columbic attraction (attraction of negatively charged electrons to the positively charged nucleus) and the size of the radius. Smaller radius= larger columbic attraction since there is a smaller distance between the nucleus and electrons (think of magnets)=easier to gain electrons. Larger radius=lower columbic attraction since there is a bigger distance between nucleus and electrons.

• The energy required to remove AN electron from a neutral atom of an element in a gaseous state. • Ionization energy increases as the atomic radius decreases (Larger radius=easier to remove electrons) • Increases from left to right on the periodic table

• The energy change that occurs when an electron is acquired by a neutral atom. • The more nonmetallic, the higher the electron affinity • Increases right and up on the periodic table