Periodic Properties Flashcards
Periodic Law
states that the chemical properties of the elements are dependent, in a systematic way, upon their atomic numbers
Periods
the rows on the periodic table
Groups
- The columns on the periodic table
- represent elements that have the same electronic configuration in their valence shell and share similar chemical properties
Representative elements
- have either s o p sublevels as their outermost orbitals
- Groups IA through VIIA, all of which have incompletely filled s or p subshells of the highest principal number
Nonrepresenatative elements
-include transition elements, which have partially filled d sublevels
Atomic Radius
equal to one-half the distance between the centers of two atoms of that element that are just barely touching each other
Ionic Radius
the radius of a cation or an anion
Ionization Energy (IE)
the energy required to completely remove an electron from a gaseous atom or ion
First ionization energy
the energy required to remove on valence electron from the parent atom
Second Ionization Energy
the energy needed to remove a second valence electron from the univalent ion to form the divalent ion
Electron Affinity (EA)
the energy change that occurs when an electron is added to a gaseous atom, and it represents the ease with which the atom can accept an electorn
Alkaline Earth Metals
have low electron affinity values, these elements are relatively stable because their s subshell is filled
Halogens
have high electron affinities because the addition of an electron to the aotm results in a completely filled shell, which represents a stable electron configuration
Electronegativity
a measure of the attraction an atom has for electrons in a chemial bond.
Pauling electronegativity scale
the values range from 0.7 (the most electropositive) for the most electropositive elements to 4.0 (the most electronegative)
Metals
- found on the left side of the periodic table
- shiny solids at room temperature and generally have high melting points and densities
- have the ability to be deformed without breaking
- have large atomic radius, low ionization energy, and low electronegativity
- few electrons in the valence shell of a metal atom can easily be removed
- good conductors of heat and electricity
Malleability
the ability of a metal to be hammered into shapes
Ductility
the ability of metals to be drawn into wires
Nonmetals
- generally brittle in the solid state and show little or no metallic luster
- have high ionization energies and electronegativities and are usually poor conductors of heat and electricity
- has the ability to gain electrons easily
- located on the upper right side of the periodic table and are separated from the metals by a line cuttting diagonally through the region of the periodic table containing elements with partially filled p orbitals
Metalloids
- found along the line between the metals and nonmetals in the periodic table and their properties vary considerably
- densities, boiling points, and melting points fluctuate widely
- the electronegativies and ionization energies of metalloids lie between those of metals and nonmetals
- the reactivity is dependent upon the element with which they are reacting
Ions
-ionic compounds are made up of cations and anions, where a cation is a positive ion and an anion is a negative ion
Hydrogen
- has a large single s valence electron and forms the H+ ion
- it can also form the hydride ion H-
- resembles the halogens in that it only requires on additional electron to reach the next noble gas configuration
Alkali Metals
- the elements of Group IA
- possess most of the physical properties common to metals, yet their densities are lower than those of other metals
- have only one loosely bound electron in their outermost shell, giving them the largest atomic radii of all elements in their respective periods
- they can lose their valence electron to form univalent cations, allowing them to easily form +1cations
Alkali Earth Metals
-the elements of Group IIA
-dependent on the ease with which they lose
electrons
-have two electrons in their outer shell and have smaller atomic radii than the alkali metals, which can be removed to form divalent cations
-commonly form +2cations
Carbon Group
- the family containing carbon, group IVA
- have two electrons in their outermost p subshells
- tends not to form ions, but participates in electron sharing (four covalent bonds)
Pnictogens
- nitrogen and the elements below it in group VA
- forms covalent bonds but most commonly forms three per atom
- commonly holds a positive charge in organic reactions (a good base)
Chalcogens
- group VIA
- elements requiring two additional valence electrons to complete their outermost shells
- tend to be fairly electronegative and to form -2 anions, but can also participate in covalent bonds
Noble Gases
- also called inert gases, found in Group VIIIA
- completely nonreactive b/c they have complete valence shells
- no tendency to gain or lose electrons, high ionization energies, and no electronegativities
- posses low boiling points and are gases at room temp
