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LD Chemistry Test

LD Chemistry - Periodic Table Test

What does the Periodic Law State? It is organized by increasing atomic numbers.
The elements are generally categorized in three types: Metals, Non-Metals, and Metalloids
The elements are also given seven classifications according to their position on the Periodic Table: Alkaline, Alkaline earth metals, Transition elements, Halogens, Noble Gases, Nitrogen Group & Oxygen group
The physical properties of a metal are: Luster, Solid at room temperature, ductile, & malleable.
The physical properties of a nonmetal are: Dull, Brittle, Poor conductors, All phases of matter at room temperature
The physical properties of a metalloid are: Ok conductors and Nonmetal/metal properties
The horizontal rows on the table are called: Period
The vertical columns are called: Group or Family
The diatomic elements are: Br, I, N, Cl, H, O, F
The phase of each of these is: L, S, g, g, g, g, g
The ___________ molecules contain one element per molecule. Monatomic
The ______ _______ are considered monatomic molecules, they are competed outer shell. Noble gases
The most active metals are found ______ _______ of the periodic table Lower left
The most active nonmetals are found ______ _______ of the periodic table. Upper right
Groups 1, 2, 13 - 18 have how many valence electrons each? 1 - 8 electrons
Transition elements are found in the ______ of the table and have three properties. Middle
Transition elements have three properties to remember React with 2 outer most principle energy levels, can form more than one type of binary compound, & compounds & icons tend to be colored
How do we know that Xe and Kr are capable of reacting with other elements under special conditions? They have a full outer shell of electrons and can have positive ions unlike the other elements.
The atomic radius ________ as you go across a period and _______ as you go down a group. Decreases, Increases
This occurs across a period because _______ _______ increases. Nuclear charge
This occurs down a group because The number of energy required to remove the most closely bond electrons
The Ionization energy for an atom is defined as The amount of energy required to remove the most loosely bound electrons increases across a period and decreases down a group
The electro-negativity of an atom is defined as The ability to attract electrons and generally increases across a period and decrease down a group
Metals tend to lose electors during a ______ reaction, which produces _____ ions. These ions are ________ in size as compared to the element that they are formed from. Chemical, Positive, Smaller
What is the electron configuration of a K+ ion and an Ar atom? 2-8-8
Nonmetals tend to gain electrons and become negative ions. These ions are _____ in size as compared to the element that they are produced from. There are _____ electrons ______ the size of the atom. Larger, More, Increasing
Elements with an atomic number greater than ____ have no known stable isotopes and are considered radioactive. 83
What properties are given on Table S for selected elements? First Ionization Energy, Electro-negativity, Melting Point, Boiling Point, Density, & Atomic Radius
Created by: desilva13



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