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CL4 Definition
Bonding
| Term | Definition |
|---|---|
| Electronegativity | the ability of an atom in an element to attract electrons in an compound |
| Valence electrons | the electrons in the highest occupies level of an elements atoms |
| Electron dot structures | Diagrams that show valence electrons in the atoms of an element as dots. |
| Ions | an atom or molecule with a net charge due to the loss or gain of one or more electrons |
| molecule | a neutral group of atoms joined together by covalent bonds |
| The octet rule | states that in forming compounds, atoms tend to achieve the electron configuration of a noble gas |
| Halide ion | a halogen atom bearing a negative charge |
| Ionic compound | a compound composed of cations and anions. Electrically neutral. |
| Ionic bond | The electrostatic forces that hold ions together in ionic compounds |
| Chemical formula | Shows the number of atoms in each element in the smallest representative unit of a substance. |
| formula unit | the lowest whole-number ratio of ions in an ionic compound |
| The coordination number of an ion | the number of ions of opposite charges that surround the ion in a crystal. |
| Metallic bond | the forces of attraction between the free-floating valence electrons and the positively charged (cations) metal ions. |
| Alloys | mixtures of two or more elements, at least one in which is a metal. |
| covalent bonds | atoms that are held together by sharing electrons are joined by this |
| diatomic molecule | a molecule that contains two atoms |
| molecular compound | a compound composed of molecules |
| molecular formula | the chemical formula of a molecular compound |
| single covalent formed | two atoms held together by sharing one pair of electrons are joined by this |
| structural formula | represents the covalent bonds as dashes and shows the arrangement of covalently bonded atoms. |
| unshared pair | A pair of valence electrons that is not shared between atoms |
| double covalent bond | a bond that involves two shared pairs of electrons |
| triple covalent bond | a bond formed by sharing three pairs of electrons |
| coordinate covalent bond | a covalent bond in which one atom contributes boht bonding electrons |
| polyatomic ion | a tightly bound group of atoms that has a positive or negative charge and behaves as a unit |
| bond dissociation energy | the energy required to break the bond between two covalently bonded atoms |
| nonpolar covalent bond | when the atoms in the bond pull equally, the bonding electrons are shared equally and each bond formed is this |
| polar covalent bond | a covalent bond between atoms in which the electrons are shared equally |
| polar molecule | one end of the molecule is slightly negative and the other end is slightly positive |
| dipole | a molecule that has two poles is called a dipolar molecule or this |
| van der Waales forces | the two weakest attractions between two molecules are collectively called this named after the dutch chemist. |
| dipole interaction | this occurs when polar molecules are attracted to one another |
| dispersion force | the weakest of all molecular interactions are caused by electrons |
| hydrogen bonds | are attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom |
| network solid | solids in which all of the atoms are covalently bonded to each other. |
Created by:
TJ365
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