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Physical Science 20 > General Review > Flashcards

General Review Flashcards

1
Q

Difference between Ionic and Molecular compounds?

A

Ionic compounds are formed from a metal and a non-metals.

Molecular compounds are formed from two non-metals.

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2
Q

What is an acid?

A

A hydrogen-containing compound that produces H+ ions when dissolved.

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3
Q

What is an organic compounds?

A

A compound containing carbon (and hydrogen)

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4
Q

How do you get the proper ration of elements in an ionic compound?

A

Cross the charges (and reduce if necessary).

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5
Q

How do you name ionic compounds?

A

Write name of positive ion followed by negative ion but with the ending changed to “ide”.
Example: CuBr2 is Copper Bromide

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6
Q

How do you name a molecular compound?

A

Name of the first element with proper prefix (unless prefix would be mono) followed by the name of the second element with the proper prefix and ide at the end.

Example: CO2 is carbon dioxide.

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7
Q

10 prefixes for molecular compounds.

A

Mon, Di, Tri, Tetra, Penta, Hexa, Hepta, Octa, Nona, Deca.

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8
Q

10 prefixes for organic compounds?

A

meth, eth, prop, but, penta, hexa, hepta, octa, nona, deca.

First 4 are different but 6-10 are same as molecular.

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9
Q

What is a diatomic element?

A

A compound in which 2 elements of the same element share electrons.
Ex: N2, O2, H2, I2, F2, Cl2, Br2.

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10
Q

Two types of acids.

A

Binary Acids: Consist of 2 elements, first one is always Hydrogen. The second is a non-metal.
Naming: hydro prefix, -ic ending. Ex: HCl is hydrochloric acid.

Oxy Acids: Consist of 2 ions (3 or more elements), the first being hydrogen, the second containing oxygen.
Naming: “Ate” becomes “Ic”. “Ite” becomes “Ous”.

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11
Q

Difference between Alkanes and Alkenes.

A

Alkanes follow a C(n)H(2n+2) formula. Ex: C2H6 Ethane. All single bonds.

Alkenes follow a C(n)H(2n) formula. Ex: C2H4 Ethene, Contain a double bond.

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12
Q

Law of Conservation of Mass.

A

Matter cannot be created or destroyed in a chemical reaction, thus the mass of the reactants will equal the mass of the product.

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13
Q

What are the types of Chemical Reactions?

A

Synthesis - 2 or more substances combine to create a new compound: A+B->AB

Decomposition Reaction - One compound breaks down into 2 or more products. AB->A+B

Single Displacement - Atoms of one element take the place of another in a compound and kick the other element out. Metal will always replace metal and a non-metal will always replace a non-metal. A+BC->AC+B

Double Displacement - Two compounds exchange elements (metals) to form two new substances. Usually forms a precipitate (solid). AB+CD->AD+CB

Combustion - Rapid reaction of an organic compound with oxygen. Complete combustion will produce CO2 and H2O.

Neutralization - An ACID and a BASE (if only one, double displacement) react to produce water and a salt (ionic compound). They neutralize each other. HX+YOH->H2O+XY

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14
Q

How do complete and incomplete combustion differ?

A

Complete: Carbon dioxide and water produced. The maximum amount of energy released. Blue flame. No soot or CO.

Incomplete: CO, H, and C are produced. Less energy is released. Orange flame. Soot and CO produced.

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15
Q

Uses of incomplete combustion?

A

Town gas. Some vehicles could use wood gas during a gasoline and diesel shortage.

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16
Q

How many atoms in a mole?

A

6.02x10^23 particles

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17
Q

How many liters of gas in a mole? (at STP)

A

22.4L

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18
Q

Representative particles.

A

Elemet: Atom
Ion: Ions
Ionic Compounds: Formula Units (FU)
Molecular Compound: Molecules

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19
Q

Molar mass?

A

One mole of an element has a weight equal to the atomic mass of the element in grams.

For compounds, use the sum of the atomic masses in the compound.

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20
Q

(#Moles wanted / #Moles given) is used for what?

A

Determining the number of moles in a reaction.

Ex. 2(KClO3) -> 3(O2) + 2(KCl)
How many moles of oxygen are produced when 6 moles of KClO3 decompose?

Want 3(O2)
Given 2(KClO3)
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21
Q

(#Moles wanted / #Moles given) is used for what?

A

Determining the number of moles in a reaction.

Ex. 2(KClO3) -> 3(O2) + 2(KCl)
How many moles of oxygen are produced when 6 moles of KClO3 decompose?

Want 3(O2)
Given 2(KClO3)

(3(O2) / 2(KClO2)) * 6(KClO2)
= (3(O2) / 2)) * 6
= (18(O2) / 2)
= 9(O2)

9 moles of O2 were produced.

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22
Q

How do you determine the limiting reagent?

A

You will be given 2 amounts of reactants.

Convert both givens into moles of wanted. Whichever given produces less moles wanted is the limiting reagent.

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23
Q

Dilute vs Concentrated solutions.

A

Dilute solutions contain a small amount of solute. Concentrated solutions contain a large amount of solute. This is subjective.

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24
Q

Molarity.

A

The number of moles of solute dissolved in 1L of a solution, represented by mol/L or M (M with a line underneath).

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25
Q

What is the difference between heat and temperature?

A

Heat is the thermal energy transferred from one object to another. Measured in joules.

Temperature is the measure of the average kinetic energy of the molecules in a substance. Measures in C, K, F.

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26
Q

10 Parts of Kinetic Molecular Theory

A

All matter consists of atoms.
Atoms may join together to form compounds.
Solids usually maintain both shape and volume.
Liquids usually maintain their volume, but no their shape.
Gases do not maintain shape or volume, they expand to fit their container.
The motion of particles is random.
The particle motion is greatest in gas, less in liquids, least in solids.
Collisions between atoms and molecules transfer energy between them.
Particles in motion possess kinetic energy.
Particles in gases do not exert large forces on one another unless they are colliding.

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27
Q

3 ways that heat moves.

A

Conduction - between neighbouring molecules in a substance. Ex. Heating up one end of a metal rod heats the other.

Convection - transfer of heat when heated liquid or gas particles move from one location to another. Ex. Wall heater heats air which rises to create a circular convection current.

Radiation - Transfer of energy by electromagnetic waves. Heat radiation is the infrared portion of the electromagnetic spectrum. Ex. The sun.

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28
Q

How to convert between C and K?

A

C = K - 273

K = C +273

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29
Q

4 laws of thermodynamics.

A

0th law. 2 systems in thermal equilibrium with a 3rd are in equilibrium with each other.

1st law. Energy cannot be created or destroyed.

2nd law. Heat always moves from hot to cold.

3rd law. Absolute 0 can never be reached.

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30
Q

What is enthalpy?

A

The total internal energy of a system at constant pressure. Given the symbol H.

The total energy of a system cannot be measured, but a change in energy can be. Termed Delta H. When positive, energy is added to the system. When negative, energy is removed from the system.

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31
Q

Difference between endothermic and exothermic?

A

Endothermic - Energy is absorbed (a chemical ice pack). Positive enthalpy. The energy is on the reactant side.

Exothermic - Energy is released (a heat pack). Negative enthalpy. The energy is on the product side.

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32
Q

How to calculate the heats of formation?

A

Delta H = Sum of Delta Hf (products) - Sum of Delta Hf (reactants).

Delta Hf is measured in kJ/mol.

Elements Delta Hf is zero.

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33
Q

Linear expansion.

A

Delta L = aLo*Delta T

Lo: original length.
a: coefficient of linear expansion.
Delta L: Change in length.
Delta T: Change in temperature.

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34
Q

Linear expansion.

A

Delta L = aLo*Delta T

Lo: original length.
a: coefficient of linear expansion.
Delta L: Change in length.
Delta T: Change in temperature.

35
Q

Volumetric Expansion.

A

Delta L = B * Vo * Delta T

Delta L: Change in length.
B: Coefficient of volumetric expansion.
Vo: Volume original.
Delta T: Change in temperature.

36
Q

What is Calorimetry?

A

The study of how much heat (energy) is exchanged in a chemical reaction.

37
Q

What is specific heat capacity?

A

The quantity of heat (Joules) required to raise the temperature of a unit of mass (Kg) by a unit of change in temperature (C).
Ex. Water: 4.2*10^3 Joules / KgC

38
Q

Heat calculations (no state change).

A

Delta Q = m * c * Delta T

Delta Q: Change in the quantity of heat (joules).
m: mass (kg).
c: specific heat capacity.
Delta T: Change in temperature.

Remember that: Q1 - Q2 = 0. (What one mixture loses, another gains).

39
Q

What is latent heat?

A

Quantity of heat energy that is required to change the state of a unit mass of a substance.

Ql = mL
Ql = quantity of heat transferred.
m = mass (kg)
L = latent heat (J/kg)

During state change, there is no temperature change. Ex. As 0C ice is heated, it changes to 0C water before the temperature rises. (during state change, energy needs to be added or removed for the state change before temperature can change).

40
Q

How is water’s behavior anomalous?

A

Unlike other substances, water is most dense at 4C, then becomes less dense as it gets colder. This is why frozen pipes break, or frozen cans explode.

41
Q

Difference between transverse and longitudinal pulses?

A

Transverse: direction of travel in the medium is perpendicular to the motion of the wave.

Longitudinal: A wave whose displacement is in the direction of the motion of the wave.

42
Q

What is a wave? (Definition)

A

A disturbance that moves outward from its point of origin transferring energy through a medium by means of vibration.

43
Q

f=1/T

A

f is in Hertz, T is in seconds.

44
Q

Pendulum Equation.

A

T=2Pi * root(L/g)
T is the period.
L is the length of the pendulum.
g is the acceleration due to gravity.

45
Q

What is the universal wave equation?

A

v=f lambda
v is speed.
f is frequency.
lambda is the wavelength.

46
Q

What happens when a pulse moving along a medium reaches a fixed end?

A

It is reflected but inverted.

47
Q

What happens when a pulse moving along a medium reaches a free end?

A

The wave is reflected. No inversion occurs.

48
Q

What happens when a wave moves from a less dense medium to a more dense medium?

A

A pulse is reflected from the boundary with the same qualities, but a smaller amplitude.
A transmitted wave has the same frequency, lower different wavelength, speed, and amplitude.

49
Q

What happens when a wave moves from a more dense medium to a less dense medium?

A

The reflected wave has the same qualities, but lower amplitude.
The transmitted wave has the same frequency, but higher speed, wavelength, and amplitude.

50
Q

What happens when two crests meet, or two troughs meet?

A

They constructively interfere as they pass each other (greater displacement as they overlap)

51
Q

What happens when a crest and a trough meet?

A

They destructively interfere (less displacement as they overlap) as they pass each other.

52
Q

What is a standing wave?

A 
When two waves with the same wavelength and amplitude overlap each other but are travelling in the opposite direction.
Creates nodal points (points that undergo no motion).
Creates antinodes (points that undergo maximum displacement).
53
Q

2 points sources of waves. How would you increase/decrease the nodal lines?

A

To decrease nodal lines: Move points closer together, and lower frequency.
To increase nodal lines: Move points farther apart, and increase frequency.

54
Q

What happens when a plane wave approaches a wall with a slit?

A

The wave diffracts. The narrower the slit, the more pronounced the diffraction. Higher frequency waves diffract less.

55
Q

Speed of sound equation.

A

v=331.4+(0.6(m/s)/C)T

Where T is temperature in degrees Celsius.

56
Q

Mach number equation.

A

M#=Vo/Vw

Where Vo is speed of object
Vw is speed of wave in the medium

57
Q

Equation relating distance speed and time.

A

d=vt

V is speed
T is time
D is distance

58
Q

Compression definition

A

An area of higher than normal air pressure

59
Q

Rarefraction definition

A

An area of lower than normal air pressure

60
Q

Amplitude definition

A

A measure of displacement in a wave

61
Q

Wavelength definition

A

Distance from rarefraction to rarefraction or compression to compression

62
Q

Intensity equation

A

I = P / 4Pi(r^2)

I is intensity
P is power
r is radius (distance from source)

63
Q

Difference between echos and reverberations?

A

Echos are distinctly heard if the time interval between the sound and echo is >0.1s (or farther than 17m)

Reverberations are when the sound takes less time to reflect so it sounds prolonged.

64
Q

Parts of sonar

A

Transducer and hydrophone

65
Q

How does ultrasound work?

A

Ultrasound waves (high frequency) are partially reflected by different sound tissues.

Echos are timed and used to create a computerized image.

66
Q

Why does sound travel farther at night?

A

At night, the ground is cooler compared to the air, causing soundwaves to refract downwards (and if the surface is smooth, they can ‘bounce’ and continue).

At the day, the ground is warmer than the air, causing the sound to refract upwards causing the sound to quickly diminish.

67
Q

Beat frequency equation

A

Fb = #beats/time = | F1 - F2 |

68
Q

Doppler effect is what?

A

The apparent change in frequency of a wave caused by relative motion between the source of the wave and the observer.

69
Q

Doppler Effect Equation

A

Source moving towards you:
Fd = (Vw / Vw - Vs) * Fs

Source moving away from you:
Fd = (Vw / Vw + Vs) * Fs

V, velocity
F, frequency
d, doppler
w, sound wave
s, source
70
Q

What is a loop (sound)?

A

The antinode of two waves that are interfering.

71
Q

Two open ends / two fixed ends overtone equations.

A

L = ( (n+1) / 2 ) * Lambda

L: Length of the vibrating object
Lambda: wavelength
n: overtone (0th overtone is fundamental)

72
Q

One open end overtone equation.

A

L = ( ( 1 + 2n ) / 4 ) * Lambda

L: Length of the vibrating object
n: overtone (0th overtone is fundamental)
Lambda: wavelength

73
Q

How does light show aspects of being both a particle and a wave?

A

It acts like a wave, but the photoelectric effect can only be explained in terms of particles.

74
Q

Light travels in straight lines is known as…

A

Linear propagation

74
Q

Light travels in straight lines is known as…

A

Linear propagation

75
Q

Equation to find energy of a light wave with a specific frequency.

A

E = hf
E: energy in joules
f: frequency
h: Planck’s constant (6.63 * 10^-34Js)

76
Q

Universal wave equation but for light

A

c = f * Lambda
c: speed of light
f: frequency
Lambda: wavelength

77
Q

EM spectrum and uses.

A

Radio waves: communication and entertainment.
Microwaves: microwaves (the appliance) and phone calls.
Infrared waves: Night vision goggles, infrared cameras, TV remotes.
Visible light waves: Vision.
UV waves: Sanitization, bug zappers.
X-Rays: x-rays, security,
Gamma rays: Destroying cancer growths, predicting coronal mass ejections.

78
Q

Absolute index of refraction equation.

A

n = c / v

n: index of refraction
c: speed of light
v: velocity of light in the medium

79
Q

relative index of refraction equation

A

1n2 = n2 / n1

1n2 = sin(i) / sin(r)

80
Q

Snell’s law

A

n1 sin(i) = n2 sin(r)

81
Q

How to find critical angle?

A

Substitute 90 degrees into R.

82
Q

Why are diamonds so sparkly?

A

They have a high index of refraction, meaning that total internal refraction easily occurs. Light bounces around before being scattered.

Physical Science 20 (6 decks)

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