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Bonding and Compound
This is a review over chapter five in the Physical Science 6th edition textbook
| Question/Term | Answer/definition | |
|---|---|---|
| Define Chemical Bond | An electrostatic attraction that forms between atoms when they share or transfer valence electrons. | |
| What happens when chemical bonds are broken? | When chemical bonds in molecules are broken, and new compounds are formed, some of that stored energy may become available to do work. | |
| What makes it possible for the small number of naturally occurring elements to combine and form the great variety of compounds that exist in the world around us? | Chemical bonding | |
| Why do atoms form chemical bonds? | Most atoms and chemically unstable when they are not bonded to other atoms, and so they are usually found combined with other elements. | |
| What elements exist mostly in the form of molecules that are made of two atoms of the same element bonded together? | Oxygen | nitrogen |
| Define Octet rule | The principle that states that atoms generally are most stable when they have eight electrons in their valence energy level. | |
| What are the two ways by which atoms achieve greater stability? | Atoms can share electrons | An atom can acquire electrons from other atoms or its surroundings. |
| What elements are colorless, odorless, and extremely reactive, and oftentimes combine with other elements | Hydrogen | Oxygen |
| What two properties of all substances involved does chemical bonding change? | Physical | Chemical |
| Define Covalent Bond | A chemical bond formed as the result of two atoms sharing electrons. | |
| Define ionic bond | A chemical bond formed when atoms transfer valence electrons. | |
| What do ionic substances form? | Crystals | |
| A crystal of a particular ionic solid: | always forms with the same ratio of cations to anions | |
| Define Formula Unit | The smallest ratio of the ions within the compounds; What is represented by the chemical formula for an ionic substance. | |
| Define Metallic Bond | The attraction between metal atoms and their sea of shared electrons. | |
| Define diatomic molecules | Molecules made of two atoms | |
| Define Single covalent bond | a chemical bond in which two atoms share two electrons to form one bond. | |
| Define Lewis structure | A system for modeling the covalent bonds between atoms in a molecule and any unbonded electrons in the molecule. | |
| What elements make up the Hydrogen seven? | Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine. | |
| Define Polarity | The name used for unequal distribution of electric charge. | |
| Define polar covalent bond | A covalent bond in which the electron density is unevenly shared between the two bonded atoms, due to a difference in electronegativity or due to inductive effects. | |
| Define nonpolar bond | a type of chemical bond that is formed when electrons are shared equally between two atoms. | |
| Define polar molecule | a molecule in which one end of the molecule is slightly positive, while the other end is slightly negative. | |
| Define chemical formula | A shorthand way of identifying a chemical compound consisting of the element symbols and subscripts that represent the number of atoms of each element. | |
| Define binary compounds | A compound made of only two elements | |
| Define polyatomic ions | A group of covalently bonded atoms that together have gained or lost electrons. | |
| Ammonium symbol | NH₄⁺ | |
| Acetate symbol | C₂H₃O₂⁻ | |
| Bicarbonate symbol | HCO₃⁻ | |
| carbonate symbol | CO₃²⁻ | |
| sulfate symbol | SO₄²⁻ | |
| hydroxide symbol | OH⁻ | |
| Nitrate symbol | NO₃⁻ | |
| phosphate symbol | PO₄³⁻ | |
| sulfite symbol | SO₃²⁻ | |
| define oxidation state | A positive or negative number showing the electric charge on an element when it forms a compound. | |
| When naming binary compounds, how is determining which element is named first in an ionic compound different than doing so for a covalent compound? | In ionic compounds, the element with the positive charge is written first. In covalent compounds, however, the element with the lower group number is written first. | |
| How is the naming of the second element in a binary ionic compound similar to that for a covalent compound? How is it different? | It is similar because for each naming of binary compounds you must drop the last two letters of the element and add the suffix "ide." It is different because prefixes are added to the elements found in chemical formulas. | |
| What is the first rule of naming binary covalent compounds? | The element with the lower group number is written first | |
| What is the second rule of naming binary covalent compounds? | If both elements are in the same group, then the element with the higher period number is written first. | |
| What is the third rule of naming binary covalent compounds? | The second element to be named is modified using the "ide" suffix. | |
| What is the fourth rule of naming binary covalent compounds? | A system of greek prefixes is used to indicate the number of atoms of each element in the compound. |
Created by:
hihello2007
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