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Unit 4
Chemistry
| Question | Answer |
|---|---|
| How do compounds form? | Compounds form from chemically bound atoms or ions. |
| What is the role of an electron in compounds? | Electrons are transferred or shared to give stable electron configuration of the atoms. |
| How does bonding work for compounds? | Bonding involves only the valence electrons. |
| What are valence electrons? | Are the electrons in the outermost principle energy level. |
| What are metallic bonds? | Metallic bonds hold metals together and are the metal ions plus a "sea" of mobile valence electrons. |
| Where are metallic bonds found? | Found in pure metals (copper, iron) and alloys (steel, bronze, brass). |
| What is an alloy? | Is a mixture of 2 or more elements, one of which is a metal. |
| What are some characteristics of metals? | Good conductors of heat and electricity, malleable and ductile. |
| What are Lewis symbols? | Lewis symbols show the valence electrons as dots around the atomic symbol. |
| For the Lewis symbols how many electrons are in group 1, 2, and 13-18? | Group 1: 1 valence electron Group 2: 2 valence electrons Group 13-18: 3,4,5,6,7,8 valence electrons but group 18 has 2. |
| For the Octet rule, how many valence electrons are there? | 8 |
| Define Cation | Metals loses one or more electrons. |
| Define Anion | Nonmetal gains one or more electrons. |
| What are ionic compounds called? | Salts |
| How to draw ionic compounds? | Draw a line to where the electron moves to. |
| What are the properties of ionic compounds? | High melting points and boiling points, conduct electric current in molten state, brittle. |
| What is a molecular (covalent) compound? | A substance composed of molecules that are formed when two or more nonmetal atoms |
| How many electrons do all elements have? | 8, except for Hydrogen, hydrogen has 2 electrons. |
| What are the characteristics of molecular (covalent) compounds? | Low melting/boiling points, poor electric conductivity, and can be polar and nonpolar. |
| Define Molecular Compounds-Lewis Structures. | The shared electron pairs are shown as --- or **. All electrons are paired, no single electrons. |
| For Molecular Compounds... how many bonds are in the single, double and triple bonds? Which ones are the strongest/weakest? | A single bond has 2 electrons, has the weakest strength but longest length. A double bond has 4 electrons and is the middle for both strength and length. A triple bond has 6 electrons and has the strongest strength and shortest length. |
| Define Linear (VSEPR) | There are 2 atoms bonded to the central atom and are no unshared electrons in the central atom. |
| Define Bent (VSEPR) | There are 2 atoms bonded to the central atom and there are unshared atoms at the central atom. |
| define Trigonal Planar (VSEPR) | There are 3 atoms bonded to the central atom and there isn't unshared electrons on the central atom. |
| Define Trigonal Pyramidal (VSEPR) | There are 3 atoms bonded to the central atom and there are unshared atoms on the central atom. |
| Define Tetrahedral (VSEPR) | There are 4 atoms bonded to the central atom. |
| What is a lewis structure? | A Lewis structure shows the total number of valence electrons in a molecule or ion. |
| What is the Tetrahedral bond angle? | 109.5 degrees |
| What is the Linear bond angle? | 180 degrees. |
| What is the Trigonal Planar bond angle? | 120 degrees. |
| Define Linear (Electron pair geometry) | 2 electron groups on central atom. |
| Define Trigonal Planar (Electron pair geometry) | 3 electron groups on central atom. |
| Define Tetrahedral (Electron pair geometry) | 4 electron groups on central atom. |
| Define electronegativity. | Is the ability of an atom in a molecule to attract shared electrons. |
| Define nonpolar. | Nonmetal + nonmetal. 0 ≤ 0.4 (very small) |
| Define polar. | Nonmetal + nonmetal. >0.4≤1.7 (moderate) |
| Define ionic. | Metal + nonmetal. >1.7 (large) |
| What are the 7 diatomic molecules? | H2, N2, O2, F2, Cl2, Br2, and I2. (BrInClHOF) |
| What are the Non-Polar Bond Cancellation? | Linear, trigonal planar, and tetrahedral. (No unshared pairs of e-) |
| What are the Polar Molecular Polarity? | Bent, trigonal pyramidal. Central atom has unshared pair(s)of e-. |
| Define intermolecular forces. | Are forces between molecules. Bonds occur between atoms inside of a molecule. Weaker than ionic, covalent or metallic bonds. Attraction not actual attachment. |
| List the physics of intermolecular forces from smallest to greatest. | Dispersion forces, dipole, hydrogen. |
| Define Hydrogen bonding. | Is the strongest . Constant and due to the large difference in electronegativity between H and O, N, F. |
| Define Dipole forces. | Are strong and constant. Attractions from the slight difference in electronegativity making part of the molecule slightly + and slightly -. |
| Define London Dispersion. | Are very weak and short lived. Slight attraction comes from electrons not being evenly distributed around a nucleus. |
| Define trends in electronegativity. | Decreases from top to bottom. Increases from left to right. Cesium (Cs) is the least electronegative element. Fluorine (F) is the most electronegative element. |
| Define trends in ionization energy. | Decrease from top to bottom. Increase left to right. |
Created by:
CoraEvelynnBaker
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