Chemical Bonds & Chemical Aaccounting
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| Na+ ions and Cl- have opposite charges and attract each other. What is the resulting reaction? | an ionic bond
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| Ionic compounds are held together by ionic bonds and exist in a? | crystal
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| In reacting chemically, atoms tend to gain or lose or share electrons so as to have eight valence electrons. This is known as the | Octet rule
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| ?lose electrons to take on the electron structure of the previous noble gas. In doing so, they form positive ions (cations). | Metals
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| ?tend to gain electrons to take on the electron structure of the next noble gas. In doing so, they form negative ions (anions). | Nonmetals
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| The charge of a cation from the representative elements is the same as the family number. | Cation charge
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| The charge of an anion from the representative elements is equal to the family number – 8. | Anions
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| Many nonmetallic elements react by ? rather than by gaining or losing electrons. | Sharing electrons
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| When two atoms share a pair of electrons, a ? is formed. | covalent bond
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| Atoms can share one, two, or three pairs of electrons, forming ?, ?, and ? bonds. | single, double, triple
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| ?compounds are named by using a prefix to denote the number of atoms. | Binary Covalent
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| ? is a measure of an atom’s attraction for the electrons in a bond. | Electronegativity
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| When two atoms with differing electro-negativity form a bond, the bonding electrons are drawn closer to the atom with the higher electro-negativity. Such a bond exhibits a separation of charge and is called a | Polar Covalent bond
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| ? are groups of covalently bonded atoms with a charge. | Polyatomic Ions
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| An atom or molecule with an unpaired electron is known as a ? | Free radical
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| The theory predicts the shape of molecules and polyatomic ions based on repulsions of electron pairs on central atoms. | Valence Shell Electron Pair Repulsion (VSEPR)
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| ? dissolve in water through ion-dipole interactions. | Ionic Substances
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| ? represent the sentences in the language of chemistry. They are the means of communicating a chemical change using the symbols and formulas to represent the elements and compounds involved in a chemical reaction. | Chemical Equations
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| ? are the species present before the reaction. | Reactants
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| ?are the species present after the reaction: | Products
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| ?are numbers used to balance a chemical equation. | Coefficients
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| : When all measurements are made at the same temperature and pressure, the volumes of gaseous reactants and products are in a small whole-number ratio. | Law of Combined Volumes
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| : When measured at the same temperature and pressure, volumes of all gases contain the same number of molecules. | Avogadro’s hypothesis
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| is defined as the number of atoms in a 12-g sample of carbon-12 and is: 6.02 x 1023 | Avogadro's number
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| A ? is defined as the amount of a substance that contains 6.02 x 1023 particles. | mole (mol)
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| ? is the average mass of a formula unit relative to that of a carbon-12 atom | Formula Mass
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| It is simply the sum of the ? for all atoms in a formula. | atomic masses
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| If the formula represents a molecule, often the term ? is used. | Molecular mass (molar mass)
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| ?:One mole of any gas occupies a volume of 22.4 L at standard temperature and pressure (STP). | Molar Volume of a gas
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| ?is defined as 1 atmosphere (atm) of pressure and a temperature of 0 oC. | STP
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| ?involves the quantitative relationship between reactants and products in a balanced chemical equation. | Stoichiometry
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| The ? of a balanced chemical equation represent ?. | Coefficients. moles
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| The amount of solute in a given amount of solvent is defined as? | Solution Concentration
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| A ? contains relative small amounts of solute in a given amount of solvent. | dilute solution
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| A ? contains relatively large amounts of solute in a given amount of solvent. | Concentrated Solution
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| ? is defined as the moles of solute per liter of solution. | Molarity (M)
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Created by:
Taylor Boyleston
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