Question | Answer |
Ionic Compound | compound composed of negative and positive ions |
ionic bond | electrostatic attraction that binds oppositely charged ions together |
polyatomic ion | tightly bonded group of atoms that behaves as a unit and has a positive or negative charge |
polar molecule | one side of the molecule is slightly negative and one side is slight positive |
double covalent bond | a bond in which two atoms share two pairs of electrons |
electron dot structure (Lewis dot structure) | notation that depicts valence electrons as dots around the atomic symbol of the element; symbol represents inner electrons and atomic nucleus |
hydrogen bond | attractive forces in which a H covalently bonded to a very electronegative atom is also weakly bonded to an unshared e- pair of another electronegative atom |
resonance structure | 1 of 2 or more equally valid e- dot structures of a molecule or a polyatomic atom |
triple covalent bond | 3 pairs of e- are shared by 2 atoms |
lone pair (unshared pair) | pair of valence e- that isn't shared between atoms |
VESPR | valence shell electron pair repulsion; because e- pairs repel, molecules adjust to their shapes so that valence e- pairs are as far apart as possible |
structural formuala | chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ions |
polar covalent bond | covalent bond between atoms in which e- are shared unequally |
metallic bond | force of attraction that holds metals together |
molecule (molecular compound) | neutral group of atoms joined by covalent bonds |
chemical formula | expression that indicates the number and type of atoms present in the smallest representative unit of a substance |
coordinate covalent bond | one atom contributes both bonding electrons |
non-polar covalent bonds | e- are shared equally by the 2 atoms |
single covalent bond | formed when 2 atoms share a pair of electrons |
molecular formula | chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound |
covalent bond | formed by the sharing of electron between atoms |
formula unit | lowest whole number ratio of ions in an ionic compound |
diatomic molecule | molecule consisting of 2 atoms |
alloy | mixture consisting of 2 or more elements; at least one is a metal |
How do ionic compounds form? | Electrons are transferred from one thing to another, when the ions get closer together, they will stick. |
Describe the structure of an ionic compound. | they are made of anions(usually nonmetals) and cations (metals) and held together by ionic bonds |
List several properties of ionic compounds | solid crystals at room temperature, strong electrostatic forces between ions, and dissolve in water and conduct electricity when dissolved in H2O |
Describe the structure of a metallic substance | held on loosely because of a sea of electrons |
List the 7 diatomic elements. | h2 (Hydrogen), O2(Oxygen) N2(Nitrogen), Cl2 (chlorine), Br2 (Bromine), I2 (Iodine), F2 (Fluorine) |