Chemistry Periodic Properties Flashcards
The substance of this work is summarized in the ___, which states that the chemical properties of the elements are dependent, in a systematic way, upon their atomic numbers
periodic law
Since [chemicals] share the same valence ___, elements within a group also share similar chemical properties
electron configuration
The Roman numeral ___ each group represents the number of valence electrons
above
The A elements are the ___, which have either s or p sublevels as their outermost orbitals
representative elements
These representative elements are those in Groups IQ through VIIA, all of which have incompletely filled s or p subshells of the ___ principal number
highest
The B elements are the ___, including the transition elements, which have partly filled d sublevels, and the lanthanide and actinide series, which have partly filled f sublevels
nonrepresentative elements
The position of an element on the periodic table can be used to determine the ___ of valence electrons
electron configuration
All elements seek to gain or lose valence electrons so as to achieve the ___, fully-filled formations possessed by the inert or noble gases of Group VIIIA
stable
First, from left to right across a period, ___ are added one at a time and the electrons of the outermost shell experience an increasing degree of nuclear attraction, becoming closer and more tightly bound to the nucleus
protons
When the electrons of the outermost shell experience an increasing degree of nuclear attraction, this net positive charge from the nucleus, as felt by an electron, is called the ___ (Zeff)
effective nuclear charge
Second, from top to bottom down a given column, the outermost electrons become less tightly bound to the nucleus. This is because the number of filled principal energy levels (which shield the outermost electrons from attraction by the nucleus) ___ downward within each group
increases
Taken together, these trends show that Zeff is at a maximum for elements in the top-right of the table and at a minimum for those in the bottom-left and help explain elemental properties such as ___, ionization potential, electron affinity, and electronegativity
atomic radius
The atomic radius of an element is equal to one-half the distance between the centers of two atoms of that element that are just barely ___ each other
touching
In general, the atomic radius decreases across a period from left to right and increases ___ a given group; the atoms with the largest atomic radii will be located at the bottom of groups and toward the left of the table (Group IA)
down
From left to right across a ___, electrons are added one at a time to the outer energy shell
period
Electrons within the same shell do not ___ one another from the attractive pull of protons
shield
Therefore, since the number of protons is also increasing from left to right across a period, the effective nuclear charge (Zeff) ___ as well
increases
The greater the positive charge experienced by the valence electrons (the larger the Zeff), the closer those electrons are pulled toward the ___ and the smaller the atomic radius
nucleus
From top to bottom down a ___, the number of electrons and filled electron shells increase
group
Although the number of ___ electrons within a group remains the same, these valence electrons will be found farther from the nucleus as they are in progressively larger energy shells
valence
As ___ are found in progressively larger energy shells, Zeff will become smaller with distance, so valence electrons in higher energy shells will feel less pull from the nucleus
electrons
Also, with more electrons comes increased ___ from the additional negative (-) charges. Thus, the atomic radii will increase
repulsion
The ___ is the radius of a cation or an anion
ionic radius
In most situations, cations (positive ions) will be smaller than corresponding neutral ___ since possessing fewer electrons leads to less repulsion among the remaining electrons
atoms
The ___ (IE) is the energy required to completely remove an electron from a gaseous atom or ion
ionization energy
Removing an ___ from an atom always requires an input of energy and is endothermic
electron
The first ionization energy is the energy required to remove one valence electron from the parent atom, the second ionization energy is the ___ needed to remove a second valence electron from the univalent ion to form the divalent ion, and so on
energy
However, if the removal of a second ___ from an element would give it a fully-filled or half-filled valence shell, then the second ionization energy would be lower than the first since atoms are more stable when the valence shell is fully or half-filled
electron
___ (EA) is the energy change that occurs when an electron is added to a gaseous atom, an it represents the ease with which the atom can accept an electron
electron affinity
The ___ the Zeff, the greater the electron affinity will be
higher
The more common sign convention for ___ states that a positive electron affinity value represents energy release when an electron is added to an atom; the other states that a negative electron affinity represents a release of energy
electron affinity
Group IIA elements, or alkaline-earth metals, have low ___ affinity values
electron
Alkaline earth metals are relatively stable because their s ___ is filled
subshell
Group VIIA elements, or halogens, have high electron affinities because the addition of an electron to the atom results in completely filled shell, which represents a ___ electron configuration
stable
Achieving the stable octet (halogens) involves a release of energy, and the strong attraction of the ___ for the electron leads to a high change in energy
nucleus
The Group VIIIA elements (noble gases) have electron affinities on the order of ___ because they already possess full shells and cannot readily accept electrons
zero
Electronegativity is a measure of the ___ an atom has for electrons in a chemical bond
attraction
The greater an atom’s ___, the greater its attraction for bonding electrons
electronegativity
___ are related to effective nuclear charge: elements with low Zeff will have low electronegativities because their nuclei do not attract electrons strongly, while elements with high Zeff will have high electronegativities because of the strong pull the nucleus has on electrons
electronegativities
Therefore, electronegativity increases from left to right across ___ and decreases from to top bottom down a group
periods
Metals are shiny solids (except for mercury) at ___ and generally have high melting points and densities
room temperature
Metals have the characteristic ability to ___ without breaking
deformed
The ability of a metal to be hammered into ___ is called malleability, and the ability to be drawn into wires is called ductility
wires
Many of the characteristic properties of ___, such as large atomic radius, low ionization energy, and low electronegativity, are due to the fact that the few electrons in the valence shell of a metal atom can easily be removed
metals
Because the valence electrons can move freely, metals are good conductors of heat and ___
electricity
Groups IA and IIA represent the most ___ metals
reactive
The transition elements, are ___ that have partially filed d orbitals
metals
The nonmetals are located on the upper right side of the periodic table and are separated from the metals by a line cutting diagonally through the region of the ___ table containing elements with partially filled p orbitals
periodic
The ___ and ionization energies of metalloids lie between those of metals and nonmetals; therefore, these elements possess characteristics of both those classes
electronegativities
___ are made up of cations and anions, where a cation is a positive ion and an anion is a negative ion
ionic compounds
An older, but still commonly used, \_\_\_is to add the ending -ous or -ic to the root of the Latin name of the element to represent the ions with lesser or greater charge, respectively. Fe2+ - Ferrous Fe3+ - Ferric Cu+ - Cuprous Cu2+ - Cupric
method
Monatomic \_\_\_ are named by dropping the ending of the elemental name and adding -ide. H- - Hydride F- - Fluoride O2- - Oxide S2- - Sulfide N3- - Nitride P3- - Phosphide
anions
Many polyatomic anions contain oxygen and are ___ called oxyanions
therefore
When an \_\_\_ forms two oxyanions, the name of the one with less oxygen ends in -ite and the one with more oxygen ends in -ate. NO2- - Nitrite NO3- - Nitrate SO32- - Sulfite SO43- Sulfate
element
When the series of \_\_\_ contains four oxyanions, prefixes are also used. Hypo- and per- are used o indicate less oxygen and more oxygen, respectively ClO- - Hypochlorite ClO2 - - Chlorite ClO3 - - Chlorate ClO4 - Perchlorate
oxyanions
Polyatomic ___ often gain one or more H+ ions to form anions of lower charge. The resulting ions are named by adding the word hydrogen or dihydrogen to the front of the anion’s name. An older method uses the prefix bi- to indicate the addition of a single hydrogen ion.
HCO3 - Hydrogen carbonate or bicarbonate
HSO4 - Hydrogen sulfate or bisulfate
H2PO4 - Dihydrogen phosphate
anions
All ___ in a given group tend to form monatomic ions with the same charge
elements
Though other main group ___ follow the trend of each element in a group tending to form monatomic ions with the same charge, the intermediate electronegativity of such elements (which makes them less likely to form ionic compounds) and the transition from metallic to nonmetallic character further complicates the picture
elements
___ can also form the hydride ion (H-), which is far too reactive to exist in water. In this respect, hydrogen resembles the halogens in that it only requires one additional electron to reach the next noble gas configuration
hydrogen
The alkali metals have only one loosely bound electron in their outermost ___, giving them the largest atomic radii of all the elements in their respective periods
shell
___ metallic properties and high reactivity are due to their low ionization energies; they easily lose their valence electron to form univalent cations, allowing them to easily form +1 cations
alkali metals
The alkaline earth metals are the elements of Group IIA and also possess many characteristically ___ properties
metallic
The ___ have two electrons in their outer shell and have smaller atomic radii than the alkali metals
alkaline earth metals
___ have low electronegativities and positive electron affinities
alkaline earths
The family containing carbon, Group IVA, exhibits a wide range of characteristics and includes a ___(C), metalloids (Si and Ge), and metals (Sn and Pb)
nonmetal
Although Group IVA do not share many physical properties, they do all have 2 electrons in their ___ p subshells, leading to a configuration that is distant from that of a noble gas
outermost
The 2 ___ in outermost shell make Group IVA tend not to form ions (which would need to be +4 or -4 to reach noble gas configuration)
electrons
Carbon participates in electron sharing; it usually is most stable with four ___ bonds
covalent
___ also commonly holds a positive charge in organic reactions, making several nitrogen-containing compounds good bases
nitrogen
Halogens chemical properties are more uniform: The ___ of halogens are very high, and they are particularly reactive toward alkali metals and alkaline earths, which “want” to donate electrons to the halogens to form stable ionic crystals
electronegativities
___ are completely nonreactive because they each have a complete valence shell, which is an energetically favored arrangement
noble gases
Because noble gases each have a complete ___, this gives them no tendency to gain or lose electrons, high ionization energies, and no electronegativities - they possess low boiling points and are gases at room temperature
valence shell
Chemically, Groups IB to VIIIB (transition metals) have low ionization ___ and may exist in a variety of positively charged forms or oxidation states
energies
___ are capable of losing various numbers of electrons from the s and d orbitals of their valence shells
transition metals
The ___ of complexes causes the d orbitals to be split into two energy sublevels. This enables many of the complexes to absorb certain frequencies of light - those containing the precise amount of energy required to raise electrons from the lower to the higher d sublevel. The frequencies not absorbed - known as subtraction frequencies - give the complexes their characteristic colors
formation
For transition ___, the dissolved ions can form complex ions either with molecules of water (hydration complexes) or with nonmetals, forming highly colored solutions and compounds (e.g., CuSO4 with 5H2O yielding chalcanthite)
metals
