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Chem
| Term | Definition |
|---|---|
| Alkali metal | An element in Group 1 of the periodic table. These elements are extremely reactive and will react spontaneously with water creating hydrogen gas and hydroxide ions in solution. |
| Alkaline earth metal | An element in Group 2 of the periodic table. These elements are reactive (but less so than Group 1), creating hydrogen gas and hydroxide ions in solution. |
| Anion | A negatively charged ion. |
| Atomic radius | Half the distance between adjacent nuclei. Size of an atom in Picometers (pm) |
| Brittle | The ability to be crushed into pieces when hammered, a property of nonmetals. |
| Cation | A positively charged ion. |
| Diatomic molecule | A nonmetal atom that forms one or more nonpolar covalent bonds with another atom of the same element to form a molecule consisting of the two atoms when there is no other element to bond with. Elements that do this are Br, I, N, H, Cl, H, O and F. |
| Ductile | The ability to be stretched into a wire, a property of metals. |
| Dull | The lack of ability to reflect light efficiently, a property of nonmetals. |
| Group | Columns down the periodic table that contain elements with the same number of valence electrons and thus similar chemical properties. Aka “families” |
| Electronegativity | The relative ability for an atom to gain an electron. Fluorine has the highest electronegativity 4.0 |
| Electron Affinity | The energy change that occurs with the addition of an electron |
| Effective Nuclear Charge | The overall attraction to the nucleus that a valence electron experiences. This increases as the # of protons increases and the occupied number of energy levels remains the same |
| Halogen | An element in Group 17 of the periodic table. These elements are extremely reactive. |
| Ionization Energy | The energy required to remove an electron from the valence shell.Unit: kJ/mol Kilojoules per mol |
| Ionic Radius | The size of an ion compared to the original atom. Metal atoms lose electrons and form + charged ions that are smaller than the original atom, nonmetal atoms form – charged ions that are larger than the original atom. |
| Luster | The ability to reflect light, a property of metals. |
| Malleable | The ability to be hammered or rolled into thin sheets, a property of metals. |
| Metal | Elements that have low electronegativity and ionization energy and large radius that tend to lose electrons to form chemical bonds. |
| Metallic Character | describes the set of chemical properties that are usually associated with the elements classified as metals in the periodic table ie. losing electrons, conductor, malleable, ductile |
| Metalloid | Elements that exhibit properties of both metals and nonmetals. |
| Orbital | The location in the electron cloud with the highest probability of finding an electron. |
| Monatomic Atom | A molecule composed of just one atom |
| Noble gas | A Group 18 element on the periodic table. These elements are nonreactive, with a full valence shell. |
| Nonmetal | Elements that have high electronegativity and ionization energy and small radius that tend to gain or share electrons to form chemical bonds. |
| Nonreactive | Not capable of readily gaining or losing e’s or undergoing a chemical change/reaction. INERT |
| Oxidation | The loss of valence electrons from an atom or ion, resulting in the increase in oxidation number of an element. |
| Periodic Law | Properties of elements repeat in a predictable way when arranged by atomic number |
| Period | Rows across the periodic table with elements having the same number of occupied principal energy levels. |
| Rare Earths | F Block elements. AKA “Inner Transition metals”. Fill the F orbitals. Many are radioactive. |
| Reactivity | aka “activity” is a measure of how readily a substance undergoes a chemical reaction. |
| Reduction | The gain of valence electrons from an atom or ion, resulting in the decrease in oxidation number of an element. |
| Shielding Effect | a decrease in attraction between electrons and the nucleus due to there being extra electrons repelling the valence electron away. More core electrons lessen the effect of the nucleus on valence electrons because opposites repel. |
| Transition metal | Metals from D Block. Display classic metallic properties. Hard, shiny, ductile, malleable and they make COLORED IONS in solution and colored crystals as a solid. Less reactive than Groups 1 & 2. They also have multiple oxidation numbers (polyvalent) |
| Z Effective aka Zeff | The net attraction a valence electron can “feel” from the nucleus. This accounts for the shielding effect. Zeff = Z -S Z is nuclear charge S is the shielding constant The higher the Zeff, the greater the relative attraction |
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