Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
36 Cards in this Set
- Front
- Back
|
the electrostatic attraction between positively charged nuclei and negatively charged electrons permits two atoms to be held together by
|
chemical bond
|
|
|
when atoms share eletrons, the electrical attraction of an atom for the shared electrons is called the atom's
|
electronegativity
|
|
|
NH3 is a ______ molecule
|
polar
|
|
|
a neutral group of atins held together by covalent bonds is a
|
molecule
|
|
|
a bond that is less then 5% ionic is considered
|
nonpolar covalent
|
|
|
compared with molecular bonds, the strength of intermolecular forces us
|
weaker
|
|
|
according to the VESPR theory, the shape of an AB3 molecule is
|
trigonal-planar
|
|
|
as atoms bond with each other, they
|
decrease their potential energy, thus creating more-stable arrangments of matter
|
|
|
the greater the electronegativity difference between two bonded atoms, the greater the percentage of __________ in the bond
|
ionic character
|
|
|
how many electrons must be shown in the lewis structure of the hydroxide ion OH-?
|
8
|
|
|
the forces of attraction between molecules in a molecular compound are
|
weaker than the forces among formula units in ionic bonding
|
|
|
how many extra electrons are in the lewis structyre of the phosphate ion (PO4)3-
|
3
|
|
|
in drawing a lewis structure, the central atom is generally the
|
least electronegative atom
|
|
|
when a polar molecule attracts the electron in a nonpolar molecule,
|
a dipole is induced
|
|
|
in a crystal, the electrons of adjacent ions
|
repel each other
|
|
|
what is placed between a molecule's resonance structures to indicate resonance?
|
double-headed arrow
|
|
|
which best explains the observation that metals are malleable and ionic crystals are brittle?
|
their chemical bonds
|
|
|
ionic compunds are brittle because strong attractive forces
|
hold the layers in relatively fixed positions
|
|
|
Use VESPR theory to predict the shape of the carbon tetraiodide molecule, CI4
|
tetrahedral
|
|
|
compared with ionic compounds, molecular compounds
|
have lower melting points
|
|
|
the strong forces of attraction vetween the positive and negative regions of molecules are called
|
dipole-dipole forces
|
|
|
In metallic bonds, the mobile electrons surrounding the positive ions are called
|
an electron sea
|
|
|
the NH3 structure shows ___covalent bonds
|
3
|
|
|
According to VESPR, the structure of the ammonia molecule, NH3, is
|
trigonal-pyramidal
|
|
|
a chemical bond formed by the attraction between positive ions and surrounding mobile elctrons is a
|
metallic bond
|
|
|
the equal but opposite charher present in the two regions of a polar molecule create a
|
dipole
|
|
|
bond length is the average distance between two bonded atoms ast which potential energy is at a
|
minimum
|
|
|
dipole-dipole forces are considered the most important forces in polar substances because the london dispersion forces present in polar substances are usually much _____ than the dipole-dipole forces
|
weaker
|
|
|
the pair of elements that forms a bond with the least ionic charcter is
a.na and cl b.k and cl c.o and cl d.mg and cl |
o and cl
|
|
|
VSEPR theory is a model for predicting
|
the shape of molecules
|
|
|
after drawing a lewis structure, one should
|
confirm that the total number of valence electrons used equals the number available
|
|
|
in drawing a lewis structure, each nonmetal atom except hydrogen should be surrounded by
|
8 electrons
|
|
|
the energy released when 1 mol of an ionic crystalline compound is formed from gaseous ions is called the
|
lattice energy
|
|
|
nonpolar covalent bonds are not common because
|
one atom usually attracts electrons strongly than the other
|
|
|
lattice energy is a measure of the
|
strength of an ionic bond
|
|
|
the lewis structure for the ammonium ion NH4 has
|
polar covalent bond
|
