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LD Chemistry Test
LD Chemistry - Periodic Table Test
| Question | Answer |
|---|---|
| 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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