GenChem2 (PeriodicTable) Flashcards
Periodic Law states that the chemical properties of the elements are dependent, in a systematic way, upon their
Atomic numbers
How many periods (rows) are there?
7
They represent n=1 to n=7
Groups represent elements that have the same electronic configuration in their _____, and the have similar chemical properties because of it
Valence Shell
The Roman numeral above each group represents the number of
Valence Electrons
A groups have ____ sublevels as their outermost orbitals
B groups have _____ sublevels as their outermost orbitals
s and p
d and f
The B elements include these groups
transition elements
lanthanide series
actinide series
This B element group has partially filled d levels
Transition elements
This B element has partially filled f sublevels
Lanthanide and Actinide Series
As one goes from left to right across a period, the electrons of the outermost shell experience INCREASING/DECREASING amount of nuclear attraction
As one goes from left to right across a period, the electrons of the outermost shell experience INCREASING amount of nuclear attraction
(they become closer and more tightly bound to the nucleus)
As one goes down a column, the outermost electrons become MORE/LESS tightly bound to the nucleus
As one goes down a column, the outermost electrons become LESS tightly bound to the nucleus
The _____ is equal to one-half the distance between the centers of two atoms of that element that are just touching each other
Atomic radius
Atomic radius ______ from right to left and ________ down a given group
Atomic radius decreases from right to left and increases down a given group
The atoms with the largest atomic radius will be located where on the periodic table?
Bottom of group 1
The energy required to completely remove an electron from a gaseous atom or ion.
Ionization Energy (IE) or Ionization Potential
Is removing an electron exothermic or endothermic?
Endothermic, as it requires energy.
The energy required to remove one valence electron from the parent atom
The energy required to remove a second valence electron from the univalent ion to form the divalent ion
Second Ionization energy
Which has a greater ionization energy, second or first ionization energy?
second ionization energy
IEs grow increasingly large
From left to right across the periodic table, ionization energy INCREASES/DECREASES
Why?
From left to right across the periodic table, ionization energy INCREASES
The atomic radius DECREASES
Moving down a group, ionization energy INCREASES/DECREASES
Why?
Moving down a group, ionization energy DECREASES
The atomic radius increases
Defined as the energy change that occurs when an electron is added to a gaseous atom, and represents the ease to with which the atom can accept an electron.
Electron Affinity
Positive electron affinity (in this text) represents energy absorption when an electron is added or energy release?
Energy release
Group IIA elements have HIGH/LOW electron affinityies
Group VIIA elements have HIGH/LOW electron affinities
Group IIA elements have LOW electron affinityies
Group VIIA elements have HIGH electron affinities
A measure of the attraction an atom has for electrons in a chemical bond
Electronegativity
Electronegativities are related to…
Ionization energies
Electrons with low ionization energies have HIGH/LOW electronegativities
Why?
Electrons with low ionization energies have LOW electronegativities
Their nuclei do not strongly attract electrons.
Electrons with high ionization energies have HIGH/LOW electronegativities
Why?
Electrons with high ionization energies have HIGH electronegativities
The nucleus has a strong pull on the electrons
As you move from left to right across the periodic table, electronegativity ______
As you increases the atomic number in a group, electronegativity ______
Increases
Decreases because of increased distance between valence shell and nucleus
The three categories of elements in the periodic table
Nonmetals, Metals, Metalloids
Category of elements that have high densities and high melting points, and are solid at room temperature
Metals
Metalshave the ability to be deformed without breaking, like hammering it into different shapes. This characteristic ability of metals is called
Malleability
The ability of metal to be drawn into a wire
Ductility
Metals have a SMALL/LARGE atomic radius
Metals have a HIGH/LOW IE
Metals have a HIGH/LOW electronegativity
These properties are explained by
Metals have a LARGE atomic radius
Metals have a LOW IE
Metals have a LOW electronegativity
These properties are explained by the few electrons in the valence shell which can be easily removed.
Metals are BAD/GOOD conductors of electricity and heat?
Why?
Metals are GOOD conductors of electricity and heat
The valence electrons can move freely
Which metals are the most reactive metals?
Groups IA and IIA
This category of elements is brittle in the solid state and show little or no metallic luster.
Nonmetals
Nonmetals have HIGH/LOW IE
Nonmetals have HIGH/LOW electronegativit
Nonmetals are GOOD/POOR conductors of heat and electricity
Nonmetals have HIGH ionization energies
Nonmetals have HIGH electronegativity
Nonmetals are POOR conductors of heat and electricity (usually)
Name the one characteristic of nonmetals that they share, otherwise they have a wide range of chemical behaviors and reactivities
Nonmetals share the ability to gain electrons easily
The category of elements located along the line between the metals and nonmetals on the periodic table
Metalloids
Are metalloid properties universal or diverse?
Their properties vary considerably
Densities, BPs, and MPs
Metalloids have HIGH/LOW/INTERMEDIATE electronegativites and IEs
Intermediate between metals and nonmetals, they possess characteristics of both classes
What does the reactivity of metalloids depend pon?
The element with which they are reacting
B behaves as a nonmetal when reacting with…
B behaves as a metal when reacting with…
Na
F
Name the elements classified as metalloids
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium
The elements of group IA are referred to as
Alkali Metals
How do alkali differ from other metals?
Why?
They have lower densities.
They have one loosely bound electron in the valence shell, meaning they have the largest atomic radii in a period.
Alkali metals have ____ IEs
Alkali metals have ____ electronegativity
Alkali metals have _____ reactivity
Why?
Low IEs
Low electronegativity
High reactivity
They easily lose their valence electron
What group do alkali metals react easily with? Especially…
Nonmetals, especially halogens
The elements of group IIA are the…
Alkaline earth metals
Alkaine earths have a LARGER/SMALLER atomic radius than alkali metals
Smaller.
Can the two valence electrons of alkaline earths be removed to form divalent cations?
Yes.
Alkaline earths have _____ IEs
Alkaline earths have _____ electron affinities
Alkaline earths have LOW IEs
Alkaline earths have LOW electron affinities
Elements in group VIIA are the…
Halogens
Halogens have ____ reactivity
Why?
Halogens have HIGH reactivity
Seven electrons in the valence shell
In terms of physical properties, are the halogens uniform or diverse?
Halogens are highly variable.
F2 and CL2 are gaseous, Br2 is liquid, I2 is solid at room temperature
Are the chemical properties of halogens uniform or diverse?
What group of elements are halogens most reactive with?
Uniform.
High electronegativities, high ionization energies
Alkali Metals and Alkaline Earth metals (group IA and IIA)
The group of elements found in group VIIIA are the…
Noble Gases
The noble gases are REACTIVE/NONREACTIVE
The noble gases have HIGH/LOW IEs
The noble gases have HIGH/LOW electronegativities
Why?
NONREACTIVE
HIGH IEs
NO ELECTRONEGATIVITIES
Noble gases have a full valence shull
Groups IB to VIIIB are the
Transition metals.
The transition metals are very SOFT/HARD
The transition metals have HIGH/LOW melting points
Transition elements have HIGH/LOW IEs
The transition metals are very HARD
The transition metals have HIGH BPs
The transition metals have LOW IEs
Transition metals may exist in a variety of positively charged forms, aka
Why?
Oxidation states
Transition metals are capable of losing various numbers of electrons from the s and d orbitals of the valence shell
Dissolves ions of transition metals can form ____ with other molecules of water or with nonmetals
Does the formation of complex ions increase or decrease the solubility of a compound?
Complex Ions
It enhances the solubility
What gives the complex ions their characteristic colors?
The d orbitals split into two energy sublevels, enabling complexes to absorb certain frequencies of light. Those not absorbed are observed.
