Ch. 6 Flashcards
Periodic Law
Law stating that elements are arranged by increasing atomic number and there is a periodic repetition of their properties
Atomic Number
The number of protons in an atom
Group
A vertical column of elements in the periodic table arranged in order of increasing atomic number; aka family
Period
A horizontal row of elements in the modern periodic table
Representative Elements
Elements from groups 1, 2, and 13-18 in the modern periodic table possessing a wide range of chemical and physical properties
Transition Elements
Elements in groups 3-12 of the modern periodic table and are further divided into transition metals and inner transition metals
Metal
An element that is solid at room temperature, a good conductor of heat and electricity, and generally is shiny; most are ductile and malleable
Alkali Metal
Group 1 elements, except Hydrogen; reactive and usually exist as compounds with other elements
Alkaline Earth Metals
Group 2 elements; highly reactive
Transition Metal
An element in groups 3-12 that, with some exceptions, is characterized by a filled outermost s orbital of energy level n, and filled or partially filled d orbitals of energy level n-1
Inner Transition Metal
A type of group B element that is characterized by a filled outermost orbital and filled or partially filled 4f and 5f orbitals
Lanthanide Series
The f-block elements from period 6 that follow the element lanthanum
Actinide Series
The f-block elements from period 7 that follow the element actinium
Nonmetal
Elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity
Halogen
A highly reactive group 17 element
Noble Gas
An extremely unreactive group 18 element
Metalloid
An element that has physical and chemical properties of both metals and nonmetals
Valence Electrons
The electrons in an atom’s outermost orbitals; determine the chemical properties of an element
Principal Energy Level
The major energy levels of an atom
Ion
An atom or bonded group of atoms that has a positive negative or charge
Ionization Energy
The energy required to remove an electron from a gaseous atom
Octet Rule
Atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons
Electronegativity
The relative ability of an element’s atoms to attract electrons in a chemical bond
