Chem/Physics review Flashcards
(74 cards)
1
Q
Snell’s Law
A
2
Q
Bernoulli’s Principle
A
3
Q
Continuity Equation
A
4
Q
Oxidation reaction
A
- Loss of Hydrogen
- Loss of electrons
- Gain of Oxygen
- OIL: Oxidation I Lose
5
Q
Reduction reaction
A
- Gain of hydrogen
- Gain of electrons
- Loss of oxygen
RIG: Reduction I Gain
6
Q
Lewis Acid
A
Accepts electrons to form Covalent bonds
7
Q
Lewis Base
A
Donates electrons to form covalent bonds
8
Q
Bronsted Acid
A
Proton Donor H+
9
Q
Brontsted Base
A
Proton acceptor H+
10
Q
Arrhenius Acid
A
Increases concentration of H+ in aqueous solution
11
Q
Arrhenius Base
A
Increase the concentration of OH- in aqueous solution
12
Q
Alpha Decay
A
Atomic mass is reduced by 4. Atomic number (Protons) is reduced by 2. This type of decay emits an alpha particle (helium nucleus)
13
Q
Beta Decay
A
Beta particle is emitted. Atomic number increases by 1 but the atomic mass stays the same.
14
Q
Gamma Decay
A
This type of radioactive decay results in a gamma particle getting emitted. It does not change the atomic mass or atomic number of the element.
15
Q
Alpha glycosidic bond
A
Both carbons have the same sterochemistry
16
Q
Beta glycosidic bond
A
Two carbons have different sterochemistry
17
Q
Determining Hybridization
A
- Count atoms attached to the central atom
- Count lone pairs
- Add above number up
- S=1, P=X-1
18
Q
Specific Gravity equation
A
19
Q
Specific Heat equation
A
20
Q
Parallel Circuit Equations
A
Capicitance of capacitators in parallel
C=C1 + C2 + C3 + …
21
Q
Series Circuit Equation
A
Capacitators
1/C1 + 1/C2 + 1/C3 + ….
22
Q
Galvanic Cell
A
Concerts chemical energy into electrical energy
23
Q
Electrolytic cell
A
Concerts electrical energy into chemical energy.
24
Q
Faraday
A
Faraday is equal to one mole of electric charge.
25
Pressure equation
Pressure = Force / Area perpendicular to the force
Si Unit for pressure is the pascal.
Density x g x change in height
1 Pa= 1N/m2
26
Energy stored in a capacitor
E=1/2CV2
C=Q/V
27
Mirror equation
1/f = 1/i + 1/o
f= Focal length
i= distance from the image to mirror
o= distance from object to mirror
28
Diverging lens
Always make virtual and reduced image
29
Power of lens
D=1/f
D= power in diopters
f= focal length in meters
30
ICE table
31
Rate limiting step
Look at which step requires the most energy. Bond breaking takes energy. Especially when the original molecule is already stable.
32
Work Equation
Force x (Distance) (Cos Ø) = Work
Work = Change in Kinetic energy (KE) = Kinetic Energy final - Kinetic energy initial
33
Kinetic Energy
1/2mv2
34
Power
Work/time
Joules/seconds
Watts
35
Nucleophile
All molecules and ions with a free pair of electrons or at least one pi bond can act as nucleophiles. Because nucleophiles donate electrons, they are Lewis bases.
nucleophile is a chemical species that forms bonds with electrophiles by donating an electron pair
36
Nucleophilic ability
37
Relative Reactivities of Carboxylic acid derivatives
Acyl halides \> anhydrides \> esters and acids \> amides
38
Boiling point
Boiling point is defined as the temperature at which the vapor pressure of a solution is equal to the atmospheric pressure. Decreasing vapor pressure makes this point more difficult to achieve, resulting in a higher boiling temperature.
Boiling requires Pvap = Patm
The more solute particles present, the lower the vapor pressure and the higher the boiling point.
∆Tb = iKbm
39
- ate
Used for ion that has the largest number of oxygen atoms
40
-ite
Used for ion with a smaller number of oxygen atoms.
41
Kinematic equations
42
Torque Equation
τ = rFsin(Ɵ)
43
Velocity Equation
v = d/t
44
Calculating pH
-log [H+] = pH
[H+] = 10^-pH
45
Poiseuille's law
Poiseuille’s law is used to describe laminar flow of incompressible fluids through a long cylindrical tube. Poiseuille’s law contains five variables: the flow rate (Q), the pressure drop between both ends of the tube (ΔP), the radius of the tube (r), the length of the tube (L), and the viscosity (η). It can be written in two equivalent forms, both of which are given below:
46
Intensity levels in Decibels
47
Capacitance
Capacitance = charge/voltage
or an easier way to remember it
Q=VC
48
Buoyant Force
Buoyant force = density of fluid x volume x gravity
or mass x gravity
Buoyant force on an object immersed in a fluid is equal to the weight of the fluid displaced by the object
49
Photon Energy
E=hf
h= planck's constant, 6.62 x 10^-34
f=frequency
Photon is defined as a particle representing a quantum of light or other electromagnetic radiation. A phone carries energy proportional to the radiation frequency
50
Kcat equation
Kcat = Vmax / [E]
[E] = concentration of the enzyme
Vmax is a rate
51
ATP structure
52
Cooperative binding
Sigmoidal shape graph.
53
Coordinate covalent bonding
Metal ion center surrounded by various ligand interactions
One atom donates it's electrons to form the covalent bond without the other atom contributing.
54
Covalent bonding
Bond formed when atoms of elements share electrons to form that bond
55
Ionic bond
Formed when ions are bound together. Ions with opposite charges will bind together.
56
Coordination Number
Number of ligands attached to the metal centre of a coordination compound
57
Oxidation Number
Charge of the central atom if we remove all the ligands and electron pairs around it
58
Ionization
Process by which an atom or a molecule acquires a negative or positive charge by gaining or losing electrons
59
Ionization energy
How much energy is required for an ion to have a full octet.
Calcium has two valence electrons, so when it is ionized for the first time, it only has one more valence electron between it and a complete octet. If you think of it like that, it wouldn't take a lot of energy for Ca to give up that last electron to reach noble gas configuration, so it has the smallest second ionization energy.
after Na ionizes once, it's essentially a noble gas and it would take A LOT for it to lose an electron
60
Ksp
The products. Basically whatever the molecule dissociated into.
Example:
Mg(OH)2(s) ⇋ Mg2+(aq) + 2OH–(aq)
Ksp = [Mg2+][OH–]2
61
Formula for Charge
q=ne
q is the number of charge (in coulombs)
N is the number of electrons
E is the elementary charge (1.6 x 10-19)
62
Wavelength Properties
Shorter wavelengths = higher frequency and higher energy
Longer wavelengths = Lower frequency and lower energy
Gamma -\> Xray -\> Ultraviolet -\> Visible -\> Infared -\> Microwave -\> Radio
Visible light range is 400ish nm to 750 nm, changes color about every 50 nm
63
Converging optical device
64
Myopia (near sightedness)
involves an eyeball that is longer than a normal eye (normal eye is about 2cm long). Since the cornea acts as a converging lens, objects at far distances (near ∞) would not produce a TINY, inverted, real image at the retina (located at the end of the eyeball, or focal point). The light rays would intersect at the point in front of the retina and continue to land at different points on the retina producing a blurry image.
This is rectified by using a diverging lens to correct the vision. Since all diverging optical devices produce smaller, upright and virtual images (SUV), this image is produced closer to the eye than the object so the myopic person can see it clearly.
65
Hyperopia (far sightedness)
involves an eyeball that is shorter than 2cm. This means that for close objects the image produced would be behind the retina. Therefore, a converging lens is used to correct this vision.
66
Mirror information
- Concave mirror: focal length POSITIVE.
- Convex mirror: focal length NEGATIVE.
- If image and object are on the OPPOSITE sites (aka mirror is in the middle of the two), image distance (di) is NEGATIVE.
- If image and object are on the SAME site (aka mirror is not in the middle of the two), image distance (di) is POSITIVE.
67
Lens information
- Diverging lens: focal length NEGATIVE;
- Converging lens: focal length POSITIVE;
Image distance:
- If image and object are on the OPPOSITE sites (aka lens is in the middle of the two), image distance (di) is POSITIVE.
- If image and object are on the SAME site (aka lens is not in the middle of the two), image distance (di) is NEGATIVE.
68
Alpha Helix
alpha helix is stable because of the many hydrogen bonds that are formed when the backbone is arranged in this way. Notice that the R groups do not contribute to the hydrogen bonding forming the alpha helix.
69
Beta Sheet
Beta sheets are also formed through hydrogen bond interactions. However, instead of a helix arrangement, different regions on the amino acid string line up in rows.
70
Electric Potential Energy
Energy that is needed to move a charge against an electric field.
U=kQq/r
V= electric potential
k= coulomb's constant
Q=charge 2
q= charge 1
r=distance of separation
71
Electrical Potential
difference in potential energy per unit charge between two locations in an electric field
V=kq/r
V= voltage
k=coulomb's law
q=charge
r=distance of separation
72
Electric field
kq/r2
73
E vs Z configuration
Z is when the high priority groups are on the same side.
E is when the high priority groups are on opposite sides.
74
Frequency into hertz
1/f = Hz
