review Flashcards
(113 cards)
1
Q
what are lewis structures and what do they show
A
electron diagrams for individual elements showing valence electrons
2
Q
what are intramolecular forces
A
the forces within a molecule
3
Q
what forces hold a molecule together
A
bonds
4
Q
what types of bonds are there
A
covalent and ionic
5
Q
ionic bonds do not _____
A
share electrons
6
Q
ionic bonding
metals ____ valence electrons
A
loose
7
Q
ionic bonding
non metals _____ valence electrons
A
gain
8
Q
covalent bonds do ______
A
share electrons
9
Q
what are covalent bonds
A
bonds holding molecular compounds together
10
Q
what are covalent bind structures also called
A
lewis structures
11
Q
which element goes in the middle with covalent bond structures
A
the element with the most bonding electrons
12
Q
exception to each element needing 8 valence electrons
A
hydrogen (2)
13
Q
when do double and triple bonds form
A
when each element should have 8 valence electrons and there should be no lone pairs
14
Q
make vespr shapes
A
linear bent trigonal pyramidal trigonal planar tetrahedral
15
Q
where are electronegativities found
A
on the periodic table
16
Q
what does the electro negativity show
A
how badly an element wants electrons
17
Q
the higher the electro negativity the _____ it pulls
A
stronger
18
Q
arrow points towards element with _____ electronegativty
A
higher
19
Q
what do you do with the difference in electro negativity between 2 atoms
A
the diffference determines the bond
20
Q
electronegativity 3.3-1.7 is _____
A
mostly ionic
21
Q
electronegativity 1.7-0.5 is ________
A
polar covalent
22
Q
electronegativity 0.5-0 is ______
A
slightly polar covalent
23
Q
electronegativity 0 is ______
A
non polar covalent
24
Q
another word for non polar covalent is
A
perfect sharing
25
polarity of a linear with middle atom bonded to the same atoms
non polar
26
polarity of a linear with middle atom bonded to different atoms
polar
27
polarity of a trigonal planar with middle atom bonded to the same atoms
non polar
28
polarity of a trigonal planar with middle atom bonded to different atoms
polar
29
polarity of a bent
polar
30
polarity of a tetrahedral with middle atom bonded to the same atoms
non polar
31
polarity of a tetrahedral with middle atom bonded different atoms
polar
32
what do intermolecular forces cause
cause attraction between molecules
33
intermolecular forces are weaker than ______
bonding within a molecule
34
what are intermolecular forces responsible for and why
responsible for boiling points and melting points of compounds
since when you boil/melt a molecule you are only breaking these forces between molecules
35
intermolecular forces occur between ______
molecular compounds
36
dipole dipole three things
occur between polar molecular compounds only
slightly positive end of one molecule is attracted to the slightly negative end of another molecule
permanent attractions
37
london dispersion three things
OCCUR BETWEEN NON POLARS
occur between all molecular compounds
caused by electrons in atoms and molecules constantly being in motion (making it polar)
forces are stronger as the molecule becomes larger or has more electrons
38
hydrogen bonding two things
NOF
hydrogen has such a low electronegativity compared to these three so it has its electrons pulled so far away from it. something else
39
why are metals solid at room temp
metal atoms have very strong forces between them
40
how to melt metals
need to add lots of energy (high temp) to overcome these strong forces
41
what are the big circles on a metallic bond model
metal cations
42
what are the small circles on a metallic bond model
sea of delocalized electrons
43
which has stronger forces of attraction ionic compounds or metallic
metallic
44
how to melt ionic compounds
need to add lots of energy (high temp) to overcome these strong forces
45
what kind of structure do ionic compounds have
crystal structure
46
how do crystal structures form
so that oppositely charged ions are as close together as possible
47
what is a crystal lattice
a 3-D array of alternating positive and negative ions
48
are intermolecular forces within or between
between
49
what are the intramolecular forces
metallic
ionic
covalent
network covalent
50
are intramolecular forces within or between
within
51
scale of forces from lowest to highest
```
london dispersion
dipole dipole
hydrogen bond
covalent
ionic
network covalent
```
52
what is the scale of forces used for
used for ordering compounds based on their boiling points
53
if two molecular compounds only have london dispersion which has the higher boiling point
bigger molecule/ moles le with more electrons
54
what is constant in boyle’s law
temperature
55
Boyle’s law formula
p1 v1=p2 v2
56
what is constant in charles law
pressure
57
charles law formula
V1/T1=V2/T2
58
when do you use combined gas law
when all three variables change
59
combined gas law formula
P1 V1/T1=P2 V2/T2
60
when do you use ideal gas law
when given mass or number of moles
61
what to do if given info about pressure and temperature and it’s in a sealed container
use combined gas law
V1=V2
62
what are electrolytes and examples
compounds that conduct electricity in water because they break apart into ions
ionic compounds
acids
63
are molecular compounds electrolytes and why or why not
non electrolytes because they do not break down into ions
64
what is solubility
the ability to dissolve
65
when is the solution saturated
when the solution is holding as much solute as possible and adding anymore solute will not be able to dissolve
66
what does a saturated solution usually have
a small amount of undissolved solute at the bottom that is in constant equilibrium with the solute that is dissolved in the solution (they switch places with each other all the time)
67
steps for preparing a standard solution
weigh out solute
dissolve in half amount of water in a beaker
pour into final volume volumetric flask
fill flask to mark and invert to mix
68
when can you use dilution
when you have a solution that has too high of a concentration
69
dilution formula
V1 C1= V2 C2
70
properties of acids 9 things
```
sour taste
electrolytes
neutralizes bases
turns litmus red
turns bromothymol blue yellow
turns phenolphthalein colourless
reacts with metals to produce H2
ph less than 7
```
71
properties of bases 8 things
```
bitter taste
electrolytes
neutralizes acids
turns litmus blue
turns bromothymol blue blue
turns phenolphthalein pink
ph greater than 7
```
72
properties of neutral substances 3 things
electrolytes and non electrolytes
do not affect indicators the same way
ph of 7
73
arrhenius definition of an acid
has H+ at the beginning of the compound
74
modified arrhenius definition of an acid
reacts with water to form hydronium ions
75
arrhenius definition of a base
has hydroxide ions at the end of an ionic compound
76
modified arrhenius definition of a base
reacts with water to form hydroxide ions
77
weak acids and bases dont ______
don’t 100% break down to form hydronium and hydroxide ions
78
strong acids
```
HCl
HBr
HI
HClO4
H2SO4
HNO3
```
79
strong bases
group 1 and 2 cations with OH
80
what are monoprotic acids
only have 1 H+ ion to give away
81
monoprotic bases
can only accept 1 H+ ionor has 1 OH- ion (ions with only 1- charge)
82
polyprotic acids
Have more than 1 H+ to give away
83
polyprotic bases
can accept more than 1 H+ ion (ions that have more than 1- charge)
84
ph scale interpretation
0 is strong acid
14 is strong base
85
poh scale interpretation
0 is strong base
14 is strong acid
86
ph formula
-log[hydronium ion conc.]
87
poh formula
-log[hydroxide ion conc.]
88
hydroxide ion conc. formula
[OH]=10^-poh
89
hydronium ion conc. formula
[H3O]=10^-ph
90
percent yield formula
% yield=actual/predicted (100)
91
percent error formula
actual-predicted/ predicted (100)
92
where is endpoint labelled
on the curve at ph 7
93
where is equivalent point labelled
on the x axis where it lines up with ph 7
94
titration curve for acid titrated with base
up to down
95
titration curve for base titrated with acid
down to up
96
ppm formula
mass of solute (mg)/mass of solution (kg)
97
percentage by volume formula
volume of solute (ml)/ volume of solution (ml) (100)
98
percentage weight by volume formula
mass of solute (g)/volume of solution (ml) (100)
99
percentage weight by weight formula
mass of solute (g)/mass of solution (g) (100)
100
calculate mass when give litres and percent concentration
divide concentration by 100 mo to get it out of percent
convert L amount to ml and multiply by that number
101
law of combining volumes
use molar ratio
102
decreasing the volume of a gas ______ it’s _______
decreases
space between molecules
103
if the temp of a gas is increased the _____ of the molecule is _______
kinetic energy
increased
104
gases that are _____ will dissolve in water
polar
105
a gas that is ______ can be collected by displacement of water
non polar
106
increasing kinetic energy of molecules _______ the number of collisions with the walls of the container and ____ the pressure
increases
increases
107
decreasing the number of collisions with the walls of a container ______ the free on the walls of the container
decreases
108
if the gas container is a steel canister the ____ will increase if the number of collisions with the wall increases
pressure
109
if the container is a rubber balloon and the kinetic energy of the particles inside decreases, the space between the molecules will _____
decrease
110
if a sample glass is heated in a closed flask, the ___ increases
number of collisions
111
the mass of a gas in an open 10 L container at 20 degrees is _____ than the mass of a gas in an open 10 L container at 49 degrees
greater
112
____ and ____ are always polar
bent and trigonal
| pyramidal
113
intermolecular forces weakest to strongest
LD
DD
HB
