Periodic properties Flashcards
States that the chemical properties of the elements are dependent upon their atomic numbers
periodic law
Elements that have either s or p sublevels as their outer most orbitals that are incompletely filled
representative elements
Transition elements, lanthanide and actinide series; partly filled d sublevels
nonrepresentative elements
The net positive charge from the nucleus as felt by an electron
effective nuclear charge
From right to left, protons are added one at a time and electrons of the outermost shell experience an increasing degree of __ __, becoming ___ and more __ __ to the nucleus. From top to bottom down, the outermost electrons become ____ tightly bound to the nucleus because the number of ___ __ ___ levels, which ___ the outermost electrons from attraction by the nucleus.
nuclear attraction, closer, tightly bound, less, filled principle energy, shield
In general, atomic radius -___ left to right across a period. The __ does not directly affect the size of the atom.
decreases, nucleus
The radius of a cation or anion
ionic radius
___ are smaller than neutral atoms because ___ electrons leads to less repulsion among the remaining electrons. ____ are larger than neutral atoms because having a greater number of electrons causes ____ repulsion, resulting in a ___ distance between electrons and a larger radius
cations, less, anions, more, greater
Energy required to remove one valence electron from the parent atom
first ionization energy
the energy required to remove a second valence electron from the univalent ion to form a divalent ion
second ionization energy
___ ionizations grow increasingly larger. Ionization energy increases as ______ increases
successive, Zeff
The energy change that occurs when an electron is added to a gaseous atom; represents the ease with which the atom can accept an electron
Electron affinity
The higher the ___, the greater the electron affinity will be. A ____ electron affinity value represents energy ___ when an electron is added to an atom. __ ___ ___ have low electron affinity values, while ___ have high electron affinities. ___ ___ have electron affinities on the order of zero
Zeff, positive, release, alkaline earth metals, halogens, noble gasses
measure of attraction an atom has for electrons in a chemical bond
electronegativity
Metals are shiny ___ at room temperature and have high __ ___ and ___. They are ____, and ____. They have generally a large _ ___, a low __ ___, and low _____, because there are few electrons in the valence shells and can easily be removed. This also makes them good ___ of heat and electricity.
solids, melting points, densities, malleable, ductile, atomic radius, ionization energy, electronegativity, conductors
Nonmetals are generally ___ in the solid state. They have ____ ___ ____ and ____ and are generally poor conductors. Most metals __ ___ easily.
brittle, high ionization energy, electronegativity, accept electrons
The metalloids or ____ have variable properties such as __ ___, and ___. The ___ and ___ energies of these lie between those of metal and nonmetals. The ____ depends on the element they are reacting with
semimetals, melting points, densities, electronegativities, ionization, reactivity
The ending ___ is added to to ions of elements with lesser charge, and ___ is added to ions of greater charge
ous, ic
Monoatomic anions are named by dropping the ending of the elemental name and adding ___
ide
Many polyatomic anions contain oxygen and therefore are called ____. When al element forms two of these, the name of the one with less oxygen ends in ___ and the one with more oxygen ends in ____
oxyanions, ite, ate
When the series of oxyanions contains 4, prefixes are also used. ___ is used to indicate less oxygen and ___ is used to indicate more oxygen
hypo, per
Polyatomic anions often gain one or more ___ ions to form anions of lower charge. The resulting ions are named by adding the word ___ or ___ to the front of the anion’s name. ____ can also be used.
hydrogen, hydrogen, dihydrogen, bi
The alkali metals have lower ___ than other metals, and only one loosely bound electron in their ___ shell, giving them the largest __ __ in their periods. They have high ____ due to their low __ ___, and easily lose valence electron to form ____ ___. They have low ___ and react readily with ___.
densities, outermost, atomic radii, reactivity, ionization energy, univalent cations, electronegativity, nonmetals
Alkali earth metals have ___ electrons in their outer shell and ___ atomic radii than alkali metals. However these electrons are not held tightly, and thus can be removed to form __ ___. They have low ___ and positive __ ___.
2, bigger, divalent cations, electronegativities, electron affinities
The carbon group contains ___ electrons in their outermost __ ___. Carbon tends to not form ___, but rather participates in __ __, with 4 __ __
2, p subshells, ions, electron sharing, covalent bonds
Pnictogens including __ and the elements below it, forms __ ___ _____. Nitrogen also commonly holds a ___ charge in __ __ making several nitrogen-containing compounds good ____
nitrogen, 3 covalent bonds, positive, organic reactions, bases
The chalcogens, which contains ___, is characterized by elements requiring ____ additional valence electrons to complete their outer shells. Therefore they are ____ and form ___ anions but can also participate in covalent bonds, preferring to have two __ __ __ and two ____ pairs
oxygen, 2, electronegative, 2-, shared electron pairs, nonbonded
Halogens are highly ____ nonmetals that form ___ ___. They are very _____, and particularly reactive toward __ ___, which want to ___ electrons to the halogens to form stable ionic ____. ___ has the highest electronegativity of all the elements
reactive, -1 anions, electronegative, alkali metals, donate, crystals, fluorine
The noble gases, also called the -_ ___ are completely ____ because they each have a full valence shell. They have high __ __, and no ____. They also have low __ __ and are gases at room temperature,
inert gasses, nonreactive, ionization energies, electronegativities, boiling points
Transition metals are very ___ and high __ and ___ points. The d electrons are held only loosely by the nucleus and are relatively ____, contributing to the ___ and high __ ___. They have low __ __ and also may exist in a variety of ___ states because transition elements are capable of losing various number of electrons from the __ and __ orbitals of their valence shells.
hard, melting, boiling, mobile, malleability, electrical conductivity, ionization energies, oxidation, s, d
Because transition metals can be in many different oxidation states, they can form __ __ either with molecules of water (___ ___) or with ___, forming highly ___ solutions and compounds. This complexation may also enhance the relatively __ ___ of certain compounds.
complex ions, hydration complexes, nonmetals, coloured, low solubility
The formation of complexes by transition metals causes the ___ ___ to be split into two energy ___. This enables many of the complexes to absorb certain ___ of ___ - those containing the precise amount of energy to raise electrons from the lower to the higher __ __. The frequencies not absorbed, known as the __ __, give the complexes their characteristic colours
d orbitals, sublevels, frequencies, light, d sublevel, subtraction frequencies
