chapter 6 review Flashcards
the charge on an ion is
either positive or negative
if a compound forms by ionic bonding, what is true
a positively charged atom or group of atoms attracts a negatively charged atom or group of atoms.
the net charge of the compound is zero.
several ions group together in a tightly packed structure.
properties of ionic compounds
crystal structure, high melting point, hardness, brittleness
the crystal structure of an ionic compound depends on the
sizes of the cations and anions
ratio of cations to anions
the melting points of ionic compounds are higher than the melting points of molecular compounds because
attractive forces between ions are greater than the attractive forces between molecules
a covalent bond is formed when two atoms
share one or more pairs of electrons with one another.
two atoms will likely for a polar covalent bond if the electronegativity difference is
1.0
bonding in molecules or ions that cannot be represented adequately by a single Lewis structure is represented by
resonance structures
as the electronegativity difference between bonded atoms decreases, the bond becomes more
covalent
the boiling point of water is higher than the boiling hydrogen sulfide because water molecules are
more polar and form hydrogen bonds
as atoms bond with each other they
decrease their potential energy, thus creating more stable arrangements of matter
which type of bonding is characterized by overlapping orbitals that allow outer electrons of atoms to move freely throughout the entire lattice
metallic
an ionic bond results from electrical attraction between
cations and anions
a non polar covalent bond is unlikely when two atoms of different elements join because the atoms are likely to differ in
electronegativity
bond length is the distance between two bonded atoms at
their minimum potential energy
to draw a lewis structure, it is necessary to know
which atoms are in the molecule
the number of valence electrons of each atom
the number of atoms in the molecule
for multiple covalent bonds to form in molecules, the molecules must contain carbon, nitrogen, or
oxygen
lattice energy is the indication of the
strength of an ionic bond
a molecule containing two atoms is called a
diatomic molecule
a neutral group of atoms held together by covalent bonds is called a
molecule
a charged group of covalently bonded atoms is called a
polyatomic ion
the simplest collection of atoms from which the formula of an ionic compound can be established is called a
formula unit
the energy required to break a chemical bond and form neutral isolated atoms is
bond energy
a chemical bond that results from the attraction between metal atoms and the surrounding sea of electrons is called
metallic bond
explain the intermolecular force that contributes to the high boiling point of water
strong dipole forces cause a strong attraction between a hydrogen atom of one water molecule and the unshared electron pair of an adjacent molecule
what is meant by sp^3 hybridization
1 s orbital and 3 p orbitals that combine to form 4 hybridized orbitals of equal energy
compare and contrast ionic bonding and covalent bonding
ionic bonding is the electrical attraction between cations and anions
covalent bonding involves the sharing of electron pairs between two atoms
why do most atoms form covalent bonds
nature favors arrangements that lower potential energy
explain why most metals are malleable and ductile but ionic crystals are not
in metals, one plane of atoms can easily slide past one another without breaking bonds
in ionic crystals, shifting causes build up of forces the can make the layers come apart.
explain why some molecules are best represented by resonance structures and to what degree do these structures indicate the actual structure of the molecule
a single lewis structure could not represent some molecules.
a polyatomic ion must have what
a charge and more than two atoms
