________ (IF7) can be written so that sulfur has twelve valence electrons.
New cards
2
Vander Waals
________ Forces: attractions between the molecules that are the two weakest attractions between molecules.
New cards
3
VSEPR
According to the ________ theory, the repulsion between electron pairs causes molecular shapes to adjust so that the valence- electron pairs stay as far apart as possible.
New cards
4
Covalent Bond
________: joins two atoms together that are sharing a pair of electrons.
New cards
5
Nitrogen dioxide
________ (NO2) has an odd number of valence electrons and therefore does not satisfy the octet rule.
New cards
6
temperature
They have low in ________ melting points and boiling points.
New cards
7
Nonpolar
________ and caused by temporary asymmetrical dispersion of electrons around it.
New cards
8
Octet Rule
The ________: electron sharing usually occurs so that the atoms attain the electron configurations of noble gases (each having eight valence electrons)
New cards
9
Polar covalent bond
________: the electrons are shared unequally.
New cards
10
Formula Unit
________: the base of an ionic compound NaCl is an ionic compound so the ________ are Na and Cl.
New cards
11
Atoms
________ form double or triple covalent bonds if they can attain a noble gas structure by sharing two pairs or three pairs of electrons.
New cards
12
Phosphorus pentachloride
________ (PCl5) can be written so that phosphorus has ten valence electrons.
New cards
13
Dipole Dipole interactions
________: when polar molecules are attracted to each other.
New cards
14
Boron Trifluoride
________ (BF3) can be written so that boron only has 6 valence electrons.
New cards
15
Dipole
________: in a polar molecule, one end of the molecule is slightly negative and the other slightly more positive.
New cards
16
Molecule
________: a neutral group of atoms joined together by covalent bonds.
New cards
17
Intermolecular forces
________ (IMF): weaker than either ionic or covalent bonds but are responsible for determining the state of matter a molecular compound is at a given temperature and a molecules melting point and boiling point.
New cards
18
Hybridization
________: several atomic orbitals mix to form the same total number of equivalent hybrid orbitals because their bond lengths are identical and their bond energies are identical.
New cards
19
London Dispersion
________ forces: the weakest of all molecular interactions.
New cards
20
Nonpolar covalent bond
________: when the bonding electrons are shared equally.
New cards
21
Metallic bonds
________: metal + metal, structured by delocalized electrons.
New cards
22
Sulfur hexafluoride
________ (SF6) can be written so that sulfur has twelve valence electrons.
New cards
23
Hydrogen bonds
________: when a hydrogen atom bonds to a very electronegative atom (Nitrogen, Oxygen, or Fluorine)
New cards
24
Network solids
________ (or network crystals: solids in which all of the atoms are covalently bonded to each other.
New cards
25
octet rule
The ________ can not be satisfied in molecules whose total number of valence electrons is an odd number.
New cards
26
ionic bonds
metals + nonmetals
New cards
27
Metallic bonds
metal + metal, structured by delocalized electrons
New cards
28
Covalent (molecular) bonds
nonmetal + nonmetals
New cards
29
Molecule
a neutral group of atoms joined together by covalent bonds
New cards
30
Diatomic Molecule
a molecule consisting of two atoms
New cards
31
Molecular Compound
a compound composed of molecules
New cards
32
Formula Unit
the base of an ionic compound NaCl is an ionic compound so the formula units are Na and Cl
New cards
33
Molecule
base unit of a molecular compound
New cards
34
Molecular Formula
a chemical formula of a molecular compound that shows how many atoms of each element a molecule contains
New cards
35
The Octet Rule
electron sharing usually occurs so that the atoms attain the electron configurations of noble gases (each having eight valence electrons)
New cards
36
Covalent Bond
joins two atoms together that are sharing a pair of electrons
New cards
37
Lone Pair
a pair of valence electrons that is not shared between atoms
New cards
38
Double covalent bond
a bond that involves two shared pairs of electrons
New cards
39
Triple covalent bond
a bond formed by sharing three pairs of electrons
New cards
40
Coordinate Covalent bond
a covalent bond in which one atom contributes both bonding electrons
New cards
41
Bond dissociation energy
The energy required to break the bond between two covalently bonded atoms
New cards
42
Nonpolar covalent bond
when the bonding electrons are shared equally
New cards
43
Polar covalent bond
the electrons are shared unequally
New cards
44
Dipole
in a polar molecule, one end of the molecule is slightly negative and the other slightly more positive
New cards
45
molecular orbitals
orbitals that apply to the entire molecule when two atoms combine and their orbitals overlap
New cards
46
Bonding orbital
a molecular orbital that can be occupied by two electrons of a covalent bond
New cards
47
Sigma bonds
formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis and connects two atomic nuclei
New cards
48
Pi bonds
the second bond area formed in a double bond
New cards
49
hybridization
several atomic orbitals mix to form the same total number of equivalent hybrid orbitals because their bond lengths are identical and their bond energies are identical
New cards
50
inter
between
New cards
51
Intra
within
New cards
52
Intermolecular forces (IMF)
weaker than either ionic or covalent bonds but are responsible for determining the state of matter a molecular compound is at a given temperature and a molecules melting point and boiling point
New cards
53
Vander Waals Forces
attractions between the molecules that are the two weakest attractions between molecules
New cards
54
Dipole/Dipole interactions
when polar molecules are attracted to each other
New cards
55
London Dispersion forces
the weakest of all molecular interactions
New cards
56
Hydrogen bonds
when a hydrogen atom bonds to a very electronegative atom (Nitrogen, Oxygen, or Fluorine)
New cards
57
network solids (or network crystals
solids in which all of the atoms are covalently bonded to each other
Studied by 3 people
