ch 4 - chemical bonding and molecular geometry Flashcards
1
Q
NH4
A
ammonium; +1
2
Q
OH
A
hydroxide; -1
3
Q
NO3
A
nitrate; -1
4
Q
NO2
A
nitrite; -1
5
Q
ClO
A
hypochlorite; -1
6
Q
ClO2
A
chlorite; -1
7
Q
ClO3
A
chlorate; -1
8
Q
ClO4
A
perchlorate; -1
9
Q
MnO4
A
permanganate; -1
10
Q
HCO3
A
hydrogen carbonate; -1
11
Q
H2PO4
A
dihydrogen phosphate; -1
12
Q
CO3
A
carbonate; -2
13
Q
SO4
A
sulfate; -2
14
Q
SO3
A
sulfite; -2
15
Q
CrO4
A
chromate; -2
16
Q
Cr2O7
A
dichromate; -2
17
Q
HPO4
A
hydrogen phosphate; -2
18
Q
PO4
A
phosphate; -3
19
Q
binary acid
A
compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound;
releases H+ ions in water
20
Q
electronegativity
A
tendency of an atom to attract electrons in a bond to itself
21
Q
formal charge
A
charge that would result on an atom by taking the number of valence electrons on the neutral atom and subtracting the nonbonding electrons and the number of bonds (1/2 the number of bonding electrons);
VE - LE - Bonds
22
Q
hypervalent molecule
A
molecule containing at least one main group element that has more than eight electrons in its valence shell
23
Q
ionic bond
A
strong electrostatic force of attraction between cations and anions in an ionic compound
24
Q
Lewis structure
A
diagram showing lone pairs and bonding pairs of electrons in a molecule or an ion
25
octet rule
guideline stating that main group atoms will form structures in which eight valence electrons interact with each nucleus, counting bonding electrons as interacting with both atoms connected by the bond
26
oxyacid
compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the covalent compound;
releases H+ ions when dissolved in water
27
pure covalent bond
covalent bonds between atoms of identical electronegativities
28
anion
negatively charged particle
29
cation
positively charged particle
30
naming polyatomic ions
cation, anion, - ate
31
naming monoatomic ions
cation, anion, -ide / metal, nonmetal, -ide
32
naming a cation
-ide
33
naming an anion*
anion cation
34
numeric prefixes
only used for covalent bonds
35
when pairing two nonmetals,
use numeric prefixes and put the least-metallic element last.
36
binary acid
hydro - ic acid
37
oxyacid
ate -> ic acid
ite -> ous acid
38
bond dipole moment
separation of charge in a bond that depends on the difference in electronegativity and the bond distance represented by partial charges or a vector
39
bond distance / length
distance between the nuclei of two bonded atoms
40
covalent bond
formed when electrons are shared between atoms
41
dipole moment
property of a molecule that describes the separation of charge determined by the sum of the individual bond moments based on the molecular structure
42
electron-pair geometry
arrangement around a central atom of all regions of electron density
43
electronegativity
tendency of an atom to attract electrons in a bond to itself
44
formal charge
valence electrons - nonbonding electrons - bonds
45
free radical
molecule that contains an odd number of electrons
46
hypervalent molecule
molecule containing at least one main group element that has more than eight electrons in its valence shell
47
inert pair effect
tendency of heavy atoms to form ions in which their valence s electrons are not lost
48
ionic bond
strong electrostatic force of attraction between cations and anions in an ionic compound
49
lone pair
two valence electrons that are not used to form a covalent bond
50
molecular structure
arrangement of atoms in a molecule or ion;
structure that includes only the placement of the atoms in the molecule
51
octahedral
a shape formed when a central atom has six areas of electron density; four groups form a square and the other two form the apex of pyramids
52
polar covalent bond
covalent bond between atoms of different electronegativities
53
polar molecule / dipole
molecule with an overall dipole movement
54
pure covalent bond
covalent bond between atoms of identical electronegativities
55
single bond
bond in which a single pair of electrons is shared between two atoms;
sigma bond
56
tetrahedral
shape formed when a central atom has four areas of electron density; 109.5º angles between four corners
57
trigonal pyramidal
shape formed when a central atom has three areas of electron density, with A at the apex
58
trigonal planar
shape formed when a central atom has three areas of electron density; a flat triangle
59
the further apart two atoms in the same period are,
the more polar their bond is
60
ion
a molecule with a nonzero net charge due to gaining or losing electrons
61
electron affinity
the energy change for the process of adding an electron to a gaseous atom to form an anion (negative ion);
increases across a period, decreases down a family
62
binary compound
compound containing two different elements
63
binary acid
compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound
64
oxyanion
an anion containing oxygen
65
double / triple bond
covalent bond in which two / three pairs of electrons are shared between atoms;
pi bonds
66
resonance
situation in which more than one Lewis structures can portray the bonding of atoms, and so the average of several is used instead
67
VSEPR
valence-shell electron-pair repulsion theory;
theory used to predict bond angles in a molecule based on positioning regions of high electron density as far apart as possible to minimize electrostatic repulsion;
areas of electron density repel each other
68
electron pair geometry
arrangement around a central atom of all regions of electron density
69
molecular geometry
arrangement of atoms in a molecule or ion;
structure that includes only the placement of the atoms in a molecule
70
covalent radii
radius generally decreases across a period and increases down a group
71
ionization energy
energy required to remove a valence electron;
increases across a period, decreases down a family
