Chem - Ch. 7 + 8 Quiz Flashcards
electrons in highest occupied energy level
valence electron
shows only the element symbol and the amount of valence electrons
electron dot structure
loses electrons and becomes more positive
cation
gains electrons and becomes negative
anion
atoms share electrons to attain the electron configuration of noble gasses
octet rule
negative ion formed when a halogen atom gains an electron (F- Cl- Br- I-)
halide ion
compound made from cations and anions
ionic compound
transfer of electrons from metals to nonmetals, formation of cations & anions
ionic bond
shows number of atoms of each element in the smallest representative unit of a substance
chemical formula
lowest whole-number ratio of ions in an ionic compound
formula unit
number of ions of opposite charge that surrounds the ion in a crystal
coordination number
forces of attraction between the free-floating valence electrons and the (+) charged metal cations
metallic bond
mixture of two or more elements that contain at least one metal — properties are often superior to those of their component elements
alloy
sharing of electrons between 2 nonmetals
Covalent Bond
neutral group of atoms held together by covalent bonds
Molecule
molecule that contains 2 atoms
Diatomic Molecule
shows how many atoms of each element a substance contains
Molecular Formula
reflects that simplest whole number ratio of atoms in a compound (aka divide the subscripts of the molecular formula by 2 bunch of times possible)
Empirical Formula
1 pair of electrons shared between atoms
Single Bond
2 pairs of electrons shared between atoms
Double Bond
3 pairs of electrons shared between atoms
Triple Bond
when a shared electron comes from a single atom to help the other fill the octet rule
Coordinate Covalent Bond
single pair of electrons that do not share a bond with another atom
Unshared Electron Pair (Lone Pair)
energy needed to break bond between two covalently bonded atoms
Bond Dissociation Energy (kJ/mol)
structures that occur when possible to draw two or more valid electron structures that have the same number of electron pairs for a molecule or ion
Resonance Structure
orbitals that apply to an entire molecule when atomic orbitals overlap
Molecular Orbital
can be occupied by two electrons of a covalent bond
Bonding Orbital
symmetric around axis
Sigma Bond
region above the axis and another below it
Pi Bond
bonded angles represent distance between electrons, unshared pairs take up more space than bonded pairs
VSEPR Theory
equal sharing of electrons
Nonpolar Covalent Bond
unequal sharing of electrons
Polar Covalent Bond
molecule with separate charges (one side negative, one side positive)
Polar Molecule
molecule that has two poles, or regions with opposite charges
Dipole
two weakest intermolecular forces
Van der Waals Forces
attraction of oppositely charged regions of polar molecules
Dipole Interactions
electron motion on one molecule affecting the electron motion on then other (weakest)
Dispersion Forces
attractive forces in which a hydrogen atom covalently bonded to a very electromagnetic atom (N, O, F) is also weakly bonded to an unshared electron pair or another electromagnetic atom
Hydrogen Bonding
