Unit 5 Chapter 6: Introduction to Chemical Bonding

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32 Terms
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Diatomic molecules
H, N, O, F, Cl, Br, I
ionic bond
results from the electrical attraction between cations & anions EN difference >1.7
polar-covalent bond
EN difference 0.3-1.69
single bond
one pair of electrons shared
double bond
two pairs of electrons shared
triple bond
three pairs of electrons shared
electrons shared unequally
electrons shared equally
ionic bond rule
metal + nonmetal
covalent bond rule
nonmetal + nonmetal/metalloid
metallic bond rule
metal + metal
non-polar covalent bond
EN difference 0-0.3
shared, transferred
electrons are ______ in covalent bonding and ______ in ionic bonding
bond length
the distance between two bonded atoms at their minimum potential energy
bond energy
the energy required to break a bond between two covalently bonded atoms
bond length and bond energy have a(n) _______ proportion
the smallest part of a covalently bonded substance with the properties of that substance
bonding in molecules or ions in which more than one correct Lewis structure can be drawn is known as ______
valence electrons
electrons involved in the formation of any bond
Chemical formula
a shorthand representation of the composition of a substance using atomic symbols and numerical subscripts which indicates the type of elements and ratio of atoms
melting point of an ionic compound
generally very high compared to covalent substances
metal atoms are strongly bonded by a mutually held sea of electrons
electrons are desocialized and free to move around all atoms of the metal
intramolecular forces
bonds between atoms
intermolecular forces
bonds between molecules
polyatomic ions
covalently bonded atoms with an overall charge
VSEPR; valence shell electron pair repulsion
a theory that states that bonded atoms and unshared electron pairs orient themselves as far apart from each other as possible
element that defies the octect rule, only needing two electrons
metals properties
-shiny -good conductors of electricity -malleable -ductile
positively charged ions
negatively charged ions
identical covalent bonds
makes a nonpolar covalent bond
lone pairs
electrons not involved in a chemical bond