Semester 1 Exam Flashcards
1
Q
List metric prefixes pico-giga
A
pico p 10^-12 nano n 10^-9 micro μ 10^-6 milli m 10^-3 centi c 10^-2 kilo k 10^3 mega M 10^6 giga G 10^9
2
Q
Temperature conversions
A
C=((5/9)(F-32)
F=((9/5)C)+32
K=C+273
3
Q
How to make an isotope symbol
A
Mass number up left
Element symbol
Atomic number down left
4
Q
Acid naming w/ polyatomics
A
I -ate something -ic(ky) but I didn’t (b)-ite a (m)-ous
eg carbonate=carbonic acid
nitrate=nitrous acid
5
Q
Acid naming w/ binary acids (ie H+ion)
A
Hydro+ion name+ic
eg HCl=hydrochloric acid
6
Q
What is an alkane
A
A hydrocarbon with all single bonds
7
Q
How to make alkane formulas
A
C(n)H(2n+2) 1 C=Methane 2 C=Ethane 3 C=Propane 4 C=Butane 5+ C=Greek prefixes (eg Pentane
8
Q
How to demonstrate heat added to a chemical equation
A
Put a Δ over the arrow
9
Q
Strong electrolytes
A
Strong acids: HCl HBr HI HNO3 HCLO3 HCLO4 H2SO4
Strong bases: Group 1 hydroxides
Ionic compounds
10
Q
Weak electrolytes
A
weak acids and bases
11
Q
NH3 + H2O–>
A
NH4 + OH-
12
Q
Definition of acid
A
Molecule that can donate a proton
13
Q
Base
A
Molecule that accepts protons and creates hydroxides
14
Q
What is reduction
A
Gain e- reduce oxidation #
15
Q
What is oxidation
A
Lose e- increase oxidation #
16
Q
Oxidation rules
A
Element by itself: 0 Neutral compounds add up to 0 Ions add up to charge of ion Oxygen: 2- Hydrogen 1+
17
Q
Kinetic Energy=
A
1/2(mass x velocity)
18
Q
Joules calorie
A
4.184J
19
Q
1st law of thermodynamics
A
Conservation of energy
20
Q
How is enthalpy notated
A
ΔH
21
Q
How is enthalpy calculated
A
per mole
22
Q
What does the sign of enthalpy indicate
A
Positive:endothermic
Negative:exothermic
23
Q
q=CΔT purpose and parts
A
Heat of system when taking into account calorimeter, C:heat capacity of calorimeter
24
Q
Heat capacity
A
Specific heat w/o mass
Unit J/ºC
25
Enthalpy of formation
E to form a compound, generally negative because formation is exothermic
26
How to calculate ΔH of reaction
(ΔHf of products) - (ΔHf of reactants)
27
If you add heat to ice at 0ºC what happens to temperature
It stays the same;the energy is used to melt the ice
28
How to calculate energy to melt and vaporize
ΔHfusion x mass = energy to melt
| ΔHvaporization x mass=energy to vaporize
29
Formula for speed of light
Wavelength x Frequency
| λ v = c
30
Wavelength of visible light
400-700nm
31
List types of electromagnetic radiation in order of increasing wavelength
gamma, x-rays, UV, visible, infrared, microwaves, radio
32
E of photon =
Planck's constant x frequency
33
Heisenberg's uncertainty principle
You can't simultaneously know the velocity and position of a particle
34
Quantum number
| n
n: principle quantum #
| ~Integers ≥1, usually [1, 4]
35
Quantum number
| l
```
l: angular momentum quantum #
~[0-(n-1)]
~l= 0 letter s
l=1 letter p
l=2 letter d
l=3 letter f
```
36
Quantum number
| ml
ml: magnetic quantum #
~[-L, +L]
Determines position in orbital
37
Quantum number
| ms
ms: spin magnetic quantum #
~(-1/2) or (+1/2)
- = down arrow + = up arrow
38
Shape of s orbital
Sphere
39
Shape of p orbital
dumbbell
40
Shape of d orbital
Clover or dude with hula hoop
41
Exceptions when doing electron configurations
ns2 nd4 → ns1 nd5
| ns2 nd9 → ns1 nd10
42
What is effective nuclear charge
Zeff= positive charge of nucleus after taking into account electron screening
43
How to calculate Zeff
Zeff= Protons (Z) - Core Electrons (S)
44
What is electron affinity
Energy change to add an electron to a gaseous atom
| Almost always negative
45
What is ionization energy
Energy change to remove an electron from a gaseous atom
| Almost always positive
46
What is an isoelectronic series
Group of ions all containing the same number of electrons
Higher atomic #=lower atomic radius
Higher atomic #=higher Zeff
47
Trend for metallic character
Increases left and down PT
48
Metal oxide + water -->
Metal hydroxide (base)
49
Nonmetal oxide + water-->
acid
50
Nonmetal oxide + base-->
salt + water
51
alkali metal + water-->
H2 + base (explosive)
52
What group is alkali metals
1
53
What group is alkaline earth metals
2
54
What do lewis symbols show
Just the one atom and its valence e-
55
When are bonds polar
When one atom is more electronegative than the other
56
Trend of electronegativity
Increases up and right on PT
57
Which way does the dipole moment arrow point
Towards the more electronegative atom in the bond
58
Exceptions to the octet: less than the octet
B=6 e-
Be=4 e-
H= 2 e-
59
Exceptions to the octet: more than the octet
Below 1st two periods
60
How to find formal charge
Draw lewis structure
(total ve-) - (# bonds + # unbonded e-)
nb double bonds count as 2
Atoms w/ higher electronegativity more likely to take a negative charge, oxygen often willing to take 1- charge
61
What is an isomer
Same composition, different structure
62
What is a resonance structure
Same composition and structure, different bonds
63
What does VSEPR stand for
Valence shell electron pair repulsion theory
64
Steps for predicting shape w/ VSEPR
~Draw the lewis structure and count the number of electron domains around the central atom
~Determine the electron domain geometry by arranging the electron domains around the central atom so that the repulsions among them are minimized
~Use the arrangement of the bonded atoms to determine the molecular geometry
65
Hybrid orbitals: 1s + 3p=
4sp3
66
What types of bonds are sigma vs pi
All single bonds are sigma
Double bonds have one sigma one pi
Triple bonds have one sigma two pi
67
Pressure=
force/area
68
Pressure units and conversions
1 atm=101325 Pa
1 atm=101.325 kPa
1 atm=760 torr=760mmHg
69
Different values of R in PV=nRT
R=.0821 for atm
| R=62.4 for torr
70
Gas Laws: Boyle's law
P1V1=P2V2
71
Gas Laws: Charles' law
V1/T1 = V2/T2
72
Gas Laws: Avogadro's law
V1/n1 = V2/n2
73
Gas Laws: Ideal gas law
PV=nRT
74
How to represent direct proportionality
X / Y
75
How to represent inverse proportionality
XY
76
Density=
mass/volume
d=PM / RT
M=molar mass
77
STP
1 atm 0ºC
78
1 mol gas @ STP
22.4L
79
Parts of Kinetic molecular theory
~Gases consist of large numbers of molecules that are in continuous random motion
~The combined volume of all the molecules of the gas is negligible compared to the volume of its container
~IMFs between gas molecules are negligible
~The average kinetic energy of the molecules in a gas does not change w/ time
~Average kinetic energy is proportional to absolute temperature
80
What does it mean that average kinetic energy is proportional to absolute temperature
At any given temperature the molecules of all gases have the same average kinetic energy
81
What is effusion
Rate at which a gas can pass through a pinhole
82
How to calculate rate of effusion
r1/r2 = √M2 / M1
r=rate
M=molar mass
83
What causes gases to be less ideal
Gases are less ideal as mass increases and temperature decreases
84
What condition needs to be in place for hydrogen bonding
Hydrogen must be bonded to N O or F
85
What is capillary action
Capillary action causes water to rise up the walls of a small diameter glass tube
86
How do adhesive and cohesive forces affect capillary action
~Adhesive forces between the liquid and the wall tend to increase the surface area of the liquid
~The cohesive force of surface tension tends to reduce surface area, thereby pulling the liquid up the tube
87
What stops capillary action
The liquid climbs until the force of gravity on the liquid balances the adhesive and cohesive forces
88
What are the triple and critical points
On a phase change diagram:
~The triple point is the point where the lines separating solid, liquid, and gas phase meet
~The critical point is the point after which the substance becomes a supercritical fluid
89
What are the conditions for normal boiling point
1 atm
90
What is the most general rule of solubility
Like dissolves like--ie polar dissolves polar and nonpolar dissolves nonpolar
91
How to supersaturate a solution
Add heat to increase the solubility of the solute
92
How do IMFs affect solubility
Strong IMF=low solubility
93
How does pressure affect gas solubility
High pressure=high gas solubility
94
How does temperature affect liquid and gas solubility
High temp=high liquid solubility
| High temp=low gas solubility
95
Units of concentration: Molarity
mols solute / L solution
96
Units of concentration: molality
mols solute / kg solvent
97
Units of concentration: Mass %
g solute / g solution
98
What do colligative properties depend on
Concentration
99
What happens to the boiling and freezing points of a solvent when a solute is added
Boiling point elevates
| Freezing point depresses
100
Formula for boiling pt elevation and freezing point depression
ΔT = i m k
ΔT: add to boiling, subtract from freezing
i=VanHoff factor, number of pieces substance breaks into when dissolved
m=molality
k=boiling/freezing point constant of solvent
101
On what does a state function depend
The state of the material (ie solid, liquid or gas)
102
What is the effect of long hydrocarbon chains/nonpolar tails
Solubility in water decreases
