CHEMITSTRAY CHATAY SIXAY
Terms
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- a mutual electrical attraction between the nuclei and valence electrons of different atoms that bind the atoms together
- Chemical Bond
- chemical bonding that results from the electrical attraction between large numbers of cations (main group metals) and anions (nonmetals)
- Ionic Bond
- results from the sharing of electron pairs between two atoms
- Covalent Bond
- The degree to which bonding between atoms of two elements is ionic or covalent can be estimated by
- calculating the difference in electronegativity
- 0-0.3
- NON-POLAR
- 0.3-1.7
- POLAR
- 1.7<
- IONIC
- - covalent bond in which the bonded electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge
- Non-polar covalent Bond
- uneven distribution of charge
- Polar
- covalent bond in which the bonded atoms have an unequal attraction for the shared electrons (0.3-1.7)
- Polar covalent bond
- a neutral group of atoms hat are held together by covalent bonds
- Molecule
- a chemical compound whose simplest units are molecules
- molecular compound
- indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
- Chemical Formula
- shows the types and numbers of atoms combined in a single molecule of a molecular bond
- molecular formula
- a molecule containing only two atoms
- diatomic molecule
- - the distance between two bonded atoms at their minimum potential energy (average distance between two bonded atoms)
- bond length
- the energy required to break a chemical bond and form neutral isolated atoms
- bond energy
- Octet Rule
- chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level
- an electron configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol
- Electron Dot Notation
- pair of electrons that is not involved in bonding and that belongs exclusively to one atom
- lone pair (unshared pair)
- formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons
- Lewis structures
- indicates the kind, number, arrangement and bonds but not the unshared pairs of the atoms in a molecule
- Strucural Formula
- covalent bond produced by the sharing of one pair of electrons between two atoms
- single bond
- a covalent bond produced by the sharing of two pairs of electrons between two atoms
- double bond
- covalent bond produced by the sharing of three pairs of electrons between two atoms
- triple bond
- double and triple bonds
- multiple bonds
- Double bonds are shorter and have _ bond energy
- higher
- triple bonds are stronger and higher than ___
- double bonds
- bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
- Resonance
- composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
- ionic compound
- the simplest collection of atoms from which an ionic compound’s formula can be established
- formula unit
- NATURE FAVORS ARRANGEMENTS IN WHICH POTENTIAL ENERGY IS
- minimized
- the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
- lattice energy
- Molecular compounds melt at low temperature because
- the forces of attraction between molecules is weak
- Ionic are higher __ and __ Ionic compounds are hard but brittle
- melting and boiling points
- charged group of covalently bonded atoms
- polyatomic ion
- the chemical bonding that result form the attraction between metal atoms and the surrounding sea of electrons
- metallic bonding
- the ability of a substance to be pounded into thin sheets
- malleability
- ability of a substance to be drawn into wire
- ductility
- uneven distribution of molecular charge
- molecular polarty
- repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible
- VSEPR theory
- VESPR
- Valence-Shell Electron-Pair Repulsion
-
the forces of attraction between molecules
The higher boiling point, the stronger forces between particles - intermolecular forces
- created by equal but opposite charges that are separated by a short distance
- dipole
- - the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
- hydrogen bonding
- the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
- London dispersion forces