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Chemistry Chapter 6

Terms in this set (76)

is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
chemical bond
chemical bonding that results from the electrical attraction between large numbers of cations and anions
ionic bonding
results from teh sharing ot electron pairs between two atoms
covalent bonding
a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a blanced dirstribution of electrical charge
nonpolar covalent bond
meaning that they have an uneven distribution of charge.
polar covalent bond
a neutral group of atoms that are held together by covalent bonds
molecule
chemical compund whose simplest units are molecules
molecular compound
indicates the relative numbers of atoms of each kind in a chemical compund by using atomic symbols and numerical subscripts
chemical formula
shows the types and numbers of atoms combined in a single molecule of a molecular compund
molecular formula
a molecule containing only two atoms
diatomic molecule
the distance between two bonded atoms at their minimum potential energy that is teh average distance between two bonded atoms
bond length
the engergy required to break a chemical bond and form neutral isolated atoms
bond energy
chemical compounds tend to form so that each atom, by gaining,losing, or sharing electrons, has an _______ of electrons in its highest occupied energy level
octet rule
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 elements symbol
electron dot notation
a pair of electrons that is not involved in bonding and that belongs exclusively to one atom
unshared pair or lone pair
formulars in which atomic symbols represent nuclei and innver shell electrons, dot pairs or dashes between two atomic symbols represent electron pair in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electroms.
lewis structures
indicates the kind, number, arrangement, and bond but not the unshared pairs of the atoms in a molecule
structural formula
a covalent bond produced by the sharing of one pair of electrons between two atoms
single bond
a covalent bond produced by the sharing of three pairs of electrons between two atoms.
triple bond
a covalent bond produced by the sharing of two pairs of electrons between two atoms
double bond
double and triple bonds
multiple bonds
refers to bonding in molecules or ions that connot be correctly represented by a single lewins 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 compunds formulac can be established
formula unit
the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
lattice energy
the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
metallic bonding
the ablitily of a substance to be hammered or beaten into thin sheets.
malleability
the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire
ductility
states that repulsion between the sets of valence level elctrons surrounding an atom causes these sets to be oriented as far apart as possible.
VSEPR theory
which is the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies.
hybridization
are orbitals of equal energy produced by the combination of two or more orbitals on the same atom
hybrid orbitals
the forces of attraction between molecules
intermolecular forces
created by equal but opposite charges that are separated by a short distance
dipole
the forces of attraction between polar molecules
dipole dipole forces
the intermoelcular attractions resulting from the constant motion of electrons and teh creation of instaneous dipoles
London dispersion forces
What determines bond length?
average distance between two bonded atoms
in general, how are bond energies and bond lengths related?
shorter bond length stronger bond
Describe the general location of the electrons in a covalent bond
between the two nuclei
When drawing Lewis structures, which atom is usually the central atoms?
least electronegative atom(except for hydrogen)
In general, what is the relationship between lattice energy and the strength of ionic bonding?
closer the ions are, the stronger their bond is
Cite three physical properties of ionic compounds.
very strong, brittle, higher mp and bp
how can the strength of metallic bonding be measured?
network of metal atoms
Role of unshared electron in prediction molecular geometries
take up space to contract
role of double bonds in prediction molecular geometries
its the same as single bonds
What determines the number of hybrid orbitals produced by an atom?
number of orbitals that have combined
In general, how do intermolecular forces compare in strength with those in ionic and metallic bonding?
generally weaker than bonds that join ionic and metallic
what determines the polarity of a molecule?
polarity and the orientation of each bond
What is the everyday importance of this type of intermolecular force?
it puts oxygen in water
What accounts for hydrogen bondings extraordinary strength?
The large electronegativity difference between heydrogen atoms and F, O, or N atoms
t or f Chemical bonding givers two or more atoms a stable e configuration and lower energy, making these atoms stable.
T
frequency of sound wave cause trash to shrink
Ultrasonic Toxic Waste Destroyer
the octet rule applies to full _____ and _____ orbitals
s and p
to form a monatomic anion, such as F, drop the suffix of the elemental name and add the new suffiz _____ to the root of elemental name. Ex. Hydrogen -1
Ide Hydrixde
Explain how ions minimize their energy in an ionic crystal
minimize repulsive forces between like forces and mazimize forces between unlike charges
what does the - sign in front of the numbers of lattice energies mean
it symbolized that energy is released when crystal form
unit for lattice energy
KJ/mol
T or F The electric attraction between + and - ions in an ionic crystal is strong.
T
T or F The covalent bonds of the atoms within a molecule are strong
F
T or F The attraction of one covalent molecule for a neighboring molecule, attractions BETWEEN covalen molecules, is weak
T
Explain why ionic compounds have high MP and BP while covalent molecules have low MP and BP
IC has high because the atttractive forces are strong
CM has low because it has weak attractive forces BETWEEN
What suffixes do polyatomic ions end in?
ate or ite
Metals lose electrons from ___ and ___ orbitals to from + ions
p and d
why are metals shiny
deexcitation energy that are given off
what is the periodicty of group1 and group 2
across a period heat of vaborization increases due to force of attraction
down a period heat of vaborization decreases due to force of attraction
T or F the various geometries available to molecules help them minimize repulsion between electron pairs
T
T or F Bond angles have no effect on moleculoar geometry
F
What determines the shape of a molecule
(1) Number of nonbonding pair
(2) Total number of atoms
Lone pair part in shape
cause the molecule bonding pairs to contract and take up space where a bonding atom could be
how does the VSEPR theory treat polyatomic ions
same as covalently bonded molecules
Which member of Family 14 is best at hybridizing
carbon
what does hybridization only apply to
covalent
hybrid carbon
Sp3d
T or FIntermolecular forces are weaker than the forces of attraction in ionic or metallic bonds
T
how does dipole dipole forces affect the BP of a molecule
stronger attractive forces higher boiling poin greater BP
In some molecules such as _____ and ______ bond dipoles can cancel each other making the molecular polarity ____. Such molecules are said to be _____.
carbon dioxide, carbon tetrachloride, zero, nonpolar
how does a polar covalent molecule induce a dipole in a nonpolar covalent molecule
by temporarily attraction its electrons
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