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University Chem 1 > Chapter 2 & 3 > Flashcards

Chapter 2 & 3 Flashcards

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1
Q

accuracy

A

refers to how close the measured value is to the actual value

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2
Q

precision

A

refers to how close a series of measurements are to one another

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3
Q

random error

A

error that has an equal probability of being high or low

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4
Q

systematic error

A

error that tends toward being either too high or too low

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5
Q

density

A

the ratio of a substance’s mass to its volume

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6
Q

intensive property

A

independent of the amount of substance

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7
Q

extensive property

A

depends on the amount of substance

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8
Q

energy

A

the capacity to do work

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9
Q

work

A

the action of a force through a distance

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10
Q

kinetic energy

A

energy of motion

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11
Q

potential energy

A

energy associated with position

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12
Q

thermal energy

A

energy associated with the temperature of an object

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13
Q

law of conservation of energy

A

energy cannot be created nor destroyed

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14
Q

calorie

A

the amount of energy required to raise the temperature of 1g of water by 1 degree celsius

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15
Q

exothermic

A

system loses energy, change in energy is negative

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16
Q

endothermic

A

system gains energy, change in energy is positive

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17
Q

mole

A

amount of material containing 6.022 x 10^23 particles

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18
Q

Schrodinger

A

introduced the idea that quantum strangeness could not be transferred to the macroscopic world

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19
Q

quantum-mechanical model

A

a model that explains the strange behavior of electrons

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20
Q

wave-particle duality

A

light behaves as both particles and waves

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21
Q

electromagnetic radiation

A

a type of energy embodied in oscillating perpendicular electric and magnetic fields

22
Q

amplitude

A

vertical height of a crest of a wave

23
Q

wavelength

A

distance between adjacent crests of a wave

24
Q

frequency

A

the number of cycles that pass through a stationary point in a given amount of time

25
Q

wave equation

A

c = 𝝼𝝀

26
Q

electromagnetic spectrum

A

includes all wavelengths of electromagnetic radiation

27
Q

electromagnetic radiation with the shortest wavelength

A

gamma rays

28
Q

The most energetic forms of electromagnetic radiation have what kind of wavelength?

A

short wavelength

29
Q

The most energetic forms of electromagnetic radiation have what kind of frequency?

A

high frequency

30
Q

Electromagnetic Spectrum from low energy to high

A

Radio, Microwave, Infrared, Visible, UV, X-rays, Gamma

31
Q

electromagnetic radiation with the longest wavelength

A

radio

32
Q

interference

A

waves interact with each other in a characteristic way

33
Q

constructive interference

A

waves in phase, add together, greater intensity

34
Q

destructive interference

A

waves out of phase, subtract, cancel out

35
Q

diffraction

A

when a wave encounters an obstacle or a slit that is comparable in size to its wavelength, it bends around it

36
Q

photoelectric effect

A

the observation that metals emit electrons when light shines upon them

37
Q

binding energy

A

the energy with which an electron is bound to the metal

38
Q

threshold frequency

A

no electrons are emitted below this frequency of light

39
Q

Does intensity of the light affect the threshold frequency?

A

no nigga

40
Q

Einstein proposed:

A

light energy must come in packets

41
Q

equation for energy of one photon

A

E = h𝜈 or E = hc/𝝀

42
Q

Increasing the intensity of the light shown on a metal does what?

A

increases the amount of photons, not the energy of each photon

43
Q

Threshold frequency condition

A

h𝜈 = ɸ

44
Q

Equation for the Kinetic Energy of the emitted electron:

A

KE = h𝜈 - ɸ

45
Q

emission spectrum

A

a series of bright lines. it is always the same for a particular element.

46
Q

Johannes Rydberg

A

analyzed atomic spectra and developed an equation that predicts the wavelengths of the hydrogen emission spectrum

47
Q

The Bohr Model

A

developed by Niels Bohr in an attempt to explain the atomic spectra. Electrons orbit nucleus in various energy states.

48
Q

absorbtion spectrum

A

consists of dark lines on a bright background. measure by passing white light through a sample and observing what wavelengths are missing

49
Q

Louis de Broglie

A

proposed the wave nature of the electron

50
Q

de Broglie wavelength equation:

A

𝝀 = h/(mv)

51
Q

The uncertainty principle

A

formulated by Heisenberg. states that it is not possible to know the position and velocity of an electron simultaneously.

52
Q

deterministic

A

the present determines the future

University Chem 1 (8 decks)

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