3 bonding Flashcards
(83 cards)
1
Q
what type of ion does group 1 form?
A
1+
2
Q
what type of ion does group 2 form?
A
2+
3
Q
what type of ion does group 3 form?
A
3+
4
Q
what type of ion does group 5 form?
A
3-
5
Q
what type of ion does group 6 form?
A
2-
6
Q
what type of ion does group 7 form?
A
1-
7
Q
what is an ammonium ion?
A
NH4+
8
Q
what is a hydroxide ion?
A
OH-
9
Q
what is a nitrate ion?
A
NO3-
10
Q
what is a nitrite ion?
A
NO2-
11
Q
what is a hydrogencarbonate ion?
A
HCO3-
12
Q
what is a chlorate (I) ion?
A
ClO-
13
Q
what is a chlorate (V) ion?
A
ClO3-
14
Q
what is a carbonate ion?
A
CO3^2-
15
Q
what is a sulfate ion?
A
SO4^2-
16
Q
what is a sulfite ion?
A
SO3^2-
17
Q
what is a dichromate ion?
A
Cr2O7^2-
18
Q
what is a phosphate ion?
A
PO4^3-
19
Q
what is the shape of a molecule with 2 bonding pairs and 0 lone pairs called?
A
linear
20
Q
what is the shape of a molecule with 3 bonding pairs and 0 lone pairs called?
A
trigonal planar
21
Q
what is the shape of a molecule with 4 bonding pairs and 0 lone pairs called?
A
tetrahedral
22
Q
what is the shape of a molecule with 5 bonding pairs and 0 lone pairs called?
A
trigonal bipyramidal
23
Q
what is the shape of a molecule with 6 bonding pairs and 0 lone pairs called?
A
octahedral
24
Q
what is the shape of a molecule with 2 bonding pairs and 1 lone pair called?
A
v-shaped
25
what is the shape of a molecule with 3 bonding pairs and 1 lone pair called?
pyramidal
26
what is the shape of a molecule with 4 bonding pairs and 1 lone pair called?
seesaw
27
what is the shape of a molecule with 5 bonding pairs and 1 lone pair called?
square pyramidal
28
what is the shape of a molecule with 2 bonding pairs and 2 lone pairs called?
v-shaped
29
what is the shape of a molecule with 3 bonding pairs and 2 lone pairs called?
trigonal planar
30
what is the shape of a molecule with 4 bonding pairs and 2 lone pairs called?
square planar
31
how many bonding pairs and lone pairs does a linear shaped molecule have?
2 bonding pairs
0 lone pairs
32
how many bonding pairs and lone pairs does a trigonal planar shaped molecule have?
3 bonding pairs
0 lone pairs
OR
3 bonding pairs
2 lone pairs
33
how many bonding pairs and lone pairs does a tetrahedral shaped molecule have?
4 bonding pairs
0 lone pairs
34
how many bonding pairs and lone pairs does a trigonal bipyramidal shaped molecule have?
5 bonding pairs
0 lone pairs
35
how many bonding pairs and lone pairs does a octahedral shaped molecule have?
6 bonding pairs
0 lone pairs
36
how many bonding pairs and lone pairs does a V shaped shaped molecule have?
2 bonding pairs
1 lone pair
OR
2 bonding pairs
2 lone pairs
37
how many bonding pairs and lone pairs does a pyramidal shaped molecule have?
3 bonding pairs
1 lone pair
38
how many bonding pairs and lone pairs does a seesaw shaped molecule have?
4 bonding pairs
1 lone pair
39
how many bonding pairs and lone pairs does a square pyramidal shaped molecule have?
5 bonding pairs
1 lone pair
40
how many bonding pairs and lone pairs does a square planar shaped molecule have?
4 bonding pairs
2 lone pairs
41
what is the bond angle of a linear shaped molecule?
180
42
what is the bond angle of a trigonal planar shaped molecule?
120
43
what is the bond angle of a tetrahedralshaped molecule?
109.5
44
what is the bond angle of a trigonal bipyramidal shaped molecule?
90
120
45
what is the bond angle of a octahedralshaped molecule?
90
46
what is the bond angle of a v shaped shaped molecule?
117.5
OR
104.5
47
what is the bond angle of a pyramidal shaped molecule?
107
48
what is the bond angle of a seesaw shaped molecule?
119
89
49
what is the bond angle of a square pyramidal shaped molecule?
89
50
what is the bond angle of a square planar shaped molecule?
90
51
define metallic bonding
a strong electrostatic attraction of positive metal ions surrounded by a sea of delocalised electrons
52
define ionic bonding
a strong electrostatic attraction between oppositely charged ions
53
define covalent bonding
a shared pair of electrons between 2 atoms
54
define dative covalent/coordinate bonding
a shared electron pair where both electrons come from the same atom
55
what structure do metallic structures have?
giant metallic lattice
56
what structures do ionic structures have?
giant ionic lattice
57
what structure do covalent structures have?
macromolecular
OR
simple molecular
58
what are 3 properties about metallic structures?
good thermal and electrical conductors
very strong
malleable and ductile
59
what does the melting and boiling point depend on in metallic lattices?
strength of metallic bonds
60
how do you find the stronger attraction of metallic bonds?
which has a greater charge
which has more electrons in the sea of delocalised electrons
which is smaller and therefore has more charge density
61
which has a higher BP and MP? a molecule with a strong metallic bond or a molecule with a weak metallic bond?
strong
62
what are 3 properties of ionic structures?
good electrical conductors
brittle
high melting and boiling point
63
why are metallic structures malleable and ductile?
because layers of metal ions can slide past eachother
64
what are 3 examples of things with macromolecular structures?
silicon
silicon oxide
carbon
65
what are 2 examples of macromolecular crystals?
diamond
graphite
66
describe the structure of diamond
macromolecular
each carbon has 4 covalent bonds
tetrahedral
high melting point
doesn't conduct electricity
67
describe the structure of graphite
macromolecular
each carbon has 3 bonds
separate layers held together with van de waals forces
high melting point
conducts electricity
68
what are coordinate bonds represented with?
an arrow that goes from the atom that is donating the 2 electrons
69
define electronegativity
the power of an atom to attract a pair of electrons in a covalent bond
70
what determines electronegativity?
nuclear charge
atomic radius
shielding
71
if an atom has high electronegativity it has...
high nuclear charge
low atomic radius
low amount of shielding
72
what is the most electronegative atom?
fluorine
73
what does non-polar mean?
an even distribution of electrons
74
what does polar mean?
an uneven distribution of electrons
75
what are the 3 types of inter molecular forces?
permanent dipole dipole
van de waals (induced dipole dipole)
hydrogen bonding
76
what is the strongest inter-molecular force?
hydrogen bonding
77
what is the weakest intermolecular force?
van de waals (induced dipole dipole)
78
how do you find out whether a molecule has hydrogen bonding?
if there is a:
H-F
H-N
H-O
79
how do you tell the difference between molecules with permanent dipole dipole forces and van de waals forces?
molecules with permanent dipole dipole forces are polar
molecules with van de waals forces are non polar
80
the stronger an intermolecular force...
the more energy required to break the force
the higher the melting and boiling point
81
how does hydrogen bonding arise?
very large difference in electronegativity between (atoms
creates a dipole on the (bond)
lone pair on ______ atom in one molecule STRONGLY attracts a ∂+H atom on a different molecule
82
how do permanent dipole dipole forces arise?
difference in electronegativity leads to bond polarity
dipoles don’t cancel therefore the molecule has an overall permanent dipole
attraction between ∂+ on one molecule and ∂− on another
83
how do van de waals forces arise?
random movement of electrons in one molecule leads to an
uneven distribution of electron, creating a
temporary dipole in one molecule. this
induces a dipole in a neighboring molecule
dipoles attract
