Chemistry Chapter 6 Flashcards
(84 cards)
1
Q
mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
A
chemical bond
2
Q
what are the types of chemical bonds
A
ionic and covalent
3
Q
what does an ionic bond do
A
give and take electrons
4
Q
what does an ionic bond do
A
share electrons
5
Q
formed by the transfer of one or more electrons which result in the formation of positive and negative ions which are then attracted to each other
A
ionic bond
6
Q
results from the simultaneous attraction of 2 nuclei for the same electrons resulting in the sharing of the electrons
A
covalent bonds
7
Q
what is a polar bond?
A
unequal sharing of electron
8
Q
what is nonpolar bond?
A
equal sharing of electrons
9
Q
how do you predict bond type
A
use electronegativity difference of the atoms
10
Q
has the electronegativity difference >1.7
A
ionic
11
Q
has the electronegativity difference between 0.3 and 1.7
A
polar
12
Q
has the electronegativity difference
A
nonpolar
13
Q
ionic of molecular?
all solids
A
ionic
14
Q
ionic of molecular?
high melting point
A
ionic
15
Q
ionic of molecular?
do not conduct unless molten or in solution
A
ionic
16
Q
ionic of molecular?
hard, brittle
A
ionic
17
Q
ionic of molecular?
may exist as gas, liquid or solids
A
molecular
18
Q
ionic of molecular?
low melting point
A
molecular
19
Q
ionic of molecular?
poor heat conductors
A
molecular
20
Q
ionic of molecular?
good electrical insulators
A
molecular
21
Q
ionic of molecular?
soft, waxy
A
molecular
22
Q
composed of positive and negative ions combined so that the net charge of the compound is zero
A
ionic compound
23
Q
simplest ration of ions in an ionic compound
A
formula unit
24
Q
ions combining in an orderly arrangement
A
crystal lattice
25
what does crystal lattice do?
reduce energy
26
group of covalently bonded atoms that carries a change
polyatomic ions
27
phosphate
phosphate: PO4^-2
28
nitrate
nitrate: NO3^-1
29
hydroxide
hydroxide: OH^-1
30
sulfate
sulfate: SO4^-2
31
ammonium
ammonium: NH4^+1
32
consists of an agreement of positive ions that are located at the crystal lattice sites and are immersed in a "sea" of mobile electrons
metallic bond
33
what does the mobility of electrons result in?
| what are these things?
metallic properties
- good conductor of electricity and heat
- malleability
- ductility
- luster
34
what does the strength of metal vary with?
the nuclear charge and the number of valence electrons
35
neutral group of atoms held together by covalent bonds
molecule
36
shows the types and number of atoms combined in a single molecule of a molecular compound
molecular formula
37
what is the formation of a covalent bond?
there is a release of energy when bonds are formed, resulting in a lower energy system and more stable system
38
- the ____ energy given _____ the more stable the compound the _____ the bond
- the _____ energy given off the _____stable the compound the _____ bond
more, more, stronger
| less, less, weaker
39
energy required to break a chemical bond and form neutral isolated atoms
bond energy
40
compounds form that each atom, by gaining, losing or sharing electrons, has an octet of electrons in its outer energy level
the octet rule
41
uses dots to show the valence electrons for an element
dot notation
42
uses symbol of each element in the compound and dot pairs or dashes between atoms to represent shared electrons and dots next to a symbol to represent unshared electrons
lewis structures
43
indicates the kind, #, arrangement, and bonds but not the unshared pairs of the atoms in a molecule
structural formula
44
sharing only one pair of electrons between atoms
compounds with single covalent bonds
45
sharing 2 pairs of electrons between two atoms
double bonds
46
sharing 3 pairs of electrons between 3 atoms
triple bonds
47
(17)
linear
48
(16)
angular
49
(15)
pyramidical
50
(14)
tetrahedral
51
an uneven distribution of electrical charge in a molecule
| -causes a molecule to be polar and result in the strongest inter molecular forces-higher boiling point
dipole
52
a special dipole
dipole force
results because _____ and another highly electronegative atom pulls _____ electron very close to it, leaving an almost bare proton
-accounts for the high boiling point of water, low vapor pressure and low density of ice
hydrogen bond
53
in _____ molecules, weak attractive forces exist between molecules
- results from momentary dipoles as electrons move about the atom
- makes it possible for small ____ molecules to exist as liquids or solid under conditions of lower temperature and high pressure
nonpolar
54
boiling point and bond tyype
nonpolar covalent
55
an atom that gains one or more electrons will have a _____ charge
negative
56
an atom that loses one or more electrons will have a ____ charge
positive
57
an atom that gains or loses one or more electrons is called an ____
ion
58
a positive ion is called a ____ and a negative ion is called an _____
cation
| anion
59
atoms will transfer one or more ____ to another to form the bond
electrons
60
each atom is left with a ____ outer shell
complete
61
an ionic bond forms between a ____ ion with a positive charge and a ____ ion with a negative charge
metal
| nonmetal
62
atoms ___ one or more electrons with each other to form the bond
share
63
each atom is left with a ____ outer shell
complete
64
a covalent bond forms between two _____
nonmetals
65
the charge on an ion is
either positive or negative
66
what is a polyatomic ion
has many ions with a charge
67
the crystal structure of an ionic compound depends on the ___ and ____ of the cations and anion
sizes and ratio
68
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
69
a covalent bond is formed when two atoms
share one or more electrons with each other
| two electrons have to be made
70
how many double bonds are in the lewis structure for hydrogen fluoride HF
none
71
two atoms will likely form a polar covalent bond if the electronegativity difference is
between 0.3 and 1.7
72
in a double covalent bond
two atoms share two pairs of electrons
73
the boiling point of water, H2O is higher than the boiling point of sulfide H2S because water molecules are...
more polar and form hydrogen bonds
74
which type of bonding is characterized by overlapping orbital that allow outer electrons of atoms to move about freely throughout the entire lattice
metallic
75
according to VESPR what is the shape of a molecule of CS2
linear
76
according to VESPR theory, what is the shape of a molecule of NBr3
pyramidal
77
an ionic bond results from electrical attraction between
cations and anions
78
a nonpolar covalent bond is unlikely when two atoms of different elements join because the atoms are likely to differ in
electronegativity
79
if two covalently bonded atoms move closer than a distance of the bond length, the potential energy of the atoms
increase
80
for multiple covalent bonds to form in molecules, the molecules mus contain carbon, nitrogen, or
oxygen
81
the principle that states that atoms tend to form compounds in which each atom has eight electrons in its highest occupied energy level is called the
octet rule
82
lattice energy is an indication of the
strength of an ionic bond
83
explain the intermolecular force that contributes to the high boiling point of water
results because hydrogen and another highly electronegative atom pulls hydrogen electron very close to it, leaving an almost bare proton
84
compare and contast ionic bonding and covalent bonding
ionic bonds are formed from one or more electrons and covalent bonds are bonded by the same electron. Ionic bonds from simultaneous attraction ionic of positive and negative ions, and covalent attraction of 2 nuclei
