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CHEM 101 > exam 1 > Flashcards

exam 1 Flashcards

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1
Q

chemistry is the study of

A

the composition, properties, and interactions of matter

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2
Q

alchemy

A

pseudoscience involved with transforming cheap metals into gold

  • contribution: methods to prepare mineral acids (HCl, HBr, etc.)
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3
Q

Phlogiston Theory & Antoine Lavoisier

A
  • outdated explanation for combustion
  • “phlogiston” spirit present in fire and when it burned, the spirit burned out = explained why fire eventually died out

Antoine Lavoisier: explained true nature of combustion, carefully weighed reactants and products, suggesting that matter is neither created nor destroyed

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4
Q

the scientific method involves 3 steps:

A
  1. making observations (collecting data)
  2. suggesting explanations (hypothesis)
  3. conducting experiments (testing experiments)
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5
Q

theories vs. laws

A

laws: describe or predict facets of the natural world
- a law summarizes WHAT happens

theories: well-tested hypotheses that explain a phenomenon
- theory attempts to explain WHY something happens

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6
Q

3 domains of chemistry

A
  1. macroscopic: things you can sense around you
  2. microscopic: what’s happening when you zoom in (water molecules)
  3. symbolic: use of symbols, formulas, and equations to represent chemical concepts
    - H2O for water
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7
Q

matter definition & 3 states

A

matter: anything that has mass and occupies space

  • solid
  • liquid
  • gas
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8
Q

mass vs. weight

A

mass: amount of matter present in an object

weight: refers to the force that gravity exerts on an object

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9
Q

pure substances

A
  • have a constant composition

elements & compounds

elements: cannot be broken down into simpler substances by any means (iron, silver, gold, etc.)

compounds: can be broken into elements via chemical changes (carbon dioxide, water, etc.)

compounds are pure substances bc only one type of substance in this mixture

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10
Q

mixtures + 2 types of mixtures

A

mixtures: composed of 2 or more types of matter that can be separated by physical changes

  • homogeneous: indistinguishable components (solutions) uniform composition
  • heterogeneous: visibly distinguishable components
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11
Q

atoms vs molecules

A

atoms: smallest particle of an element which have properties of that element

molecules: consist of two or more atoms joined by forces called chemical bonds

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12
Q

physical vs chemical change

A

physical: result in changing the form of a substance, without altering its chemical composition

chemical: change one substance into a new substance with different properties and compositions

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13
Q

intensive vs. extensive properties

A

intensive: DO NOT depend on the amount of matter present
- ex. boiling point, color, temperature, luster, hardness

extensive: dependent on the amount of matter present
- ex. volume, mass, size, weight, length

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14
Q

volume

A

amount of space an object occupies

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15
Q

density

A

ratio of mass of object to volume (d =m/v)

density is intensive property, that does not change w/ matter)

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16
Q

precision vs. accuracy

A

precision: agreement among several measurements (reproducibility)

accuracy: agreement of a measurement with the true value

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17
Q

2 types of errors

random errors & sytematic errors

A

random error: caused by factors which vary from one measurement to another (ex. measuring height with slightly different postures)

systematic error: indicates repeated error in the same direction (ex. instrument calibrated or used incorrectly)

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18
Q

avg mass formula

A

sum of (fractional abundance x isotopic mass)

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19
Q

converting from celcius to kelvin

A

add 273.15 to C

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20
Q

uncertainty

A

estimate of amount by which measruement differs from true value

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21
Q

Dalton’s Atomic Theory

(5 parts)

A
  1. matter is comprised of tiny particles called atoms
  2. atoms of a given element are identical
  3. atoms of different elemtns differ from each other
  4. chemical compounds are formed when atoms of different elements combine w/ each other
  5. chemical reactions involve reorganization of the atoms
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22
Q

law of conservation of mass

A

matter cannot be created or destroyed

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23
Q

law of definite proportion

A

compounds always contain the same proportion of elements by mass

water will always contain 2 H atoms and 1 O atom

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24
Q

J.J. Thomson

A
  • discovered the electron
  • studied electrical discharge in cathode ray tubes
  • known for plum pudding model
  • determined the charge to mass ratio of electrons (every electron has neg charge)

think jj sounds so electric

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25
Q

Robert Milikan

A
  • discovered what the charge of an electron was
  • famous oil drop experiment
  • would shoot x rays to the oil drops and the oil drops would basically float

think milk and oil dont mix so milkman brought the charge

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26
Q

plum pudding model

A

electrons and protons just scattered all throughout, no specific central structure

think jiggly w no structure

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27
Q

radioactivity

+ 3 types of radioactive emission

A

in late 1800s, scientists found that some elements produce high-energy radiation

3 types:
gamma rays: high energy “light”
beta particles: high speed electrons
alpha particles: posseses a 2+ charge

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28
Q

Ernest Rutherford

A
  • discovered the nucelus
  • performed experiments to test plum pudding model
  • dense positively charged core
  • threw beam of alpha particles at thin metal foil and some of them would go to the middle and just completely shift course

think ruth is the center of my life

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29
Q

what makes atoms different?

2 things

A
  1. number of electrons
  2. arrangement of electrons
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30
Q

isotopes

A

atoms w/ same number of protons and electrons, but different number of neutrons

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31
Q

fixed volume & fixed shape for solid, liquid, gas

A

solids: fixed volume & shape
liquids: fixed volume, no fixed shape
gases: no fixed volume, no fixed shape

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32
Q

representation of atom w/ atomic number 84 & mass 206

A

206 Po
84

mass number on top, atomic number on bottom

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33
Q

calculating # of electrons, protons, & neutrons from mass # & atomic #

A

atomic # = # of protons & electrons

mass # - # of protons = # of neutrons

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34
Q

formula for atomic mass

A

sum of (fractional abundance x mass of isotope)

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35
Q

electromagnetic radiation

A

fancy word for light

energy that behaves like a wave and travels at the speed of light in a vacuum

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36
Q

speed of light in a vacuum

A

2.998 x 10^8 m/s

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37
Q

the 4 characteristics of waves

A
  1. wavelength
  2. frequency
  3. amplitude
  4. speed
38
Q

characteristics of waves

wavelength

A

the distance between 2 consecutive peaks in a wave

symbol: λ (lambda)

39
Q

characteristics of waves

frequency

A

number of cycles per second that pass through a point in space

symbol: ν

unit: 1/s or Hz (hertz)

40
Q

characteristics of waves

amplitude

A

magnitude of the wave’s displacement

(the size of the peak of that wave)

41
Q

characteristics of waves

speed

A

how fast the wave travels

42
Q

random side note on slides

amplitude of sound wave analogous to __________

A

volume

the louder the sound, the greater the amplitude

43
Q

relationship b/w wavelength and frequency

A

inversely related

  • wavelength halves = frequency doubles

only true for light, sound waves don’t behave the same

44
Q

formula for speed of light, wavelength, and frequency

A

c = λv

c = speed of light
λ = wavelength
v = frequency

45
Q

the electromagnetic spectrum

A
  • red are the lowest energy levels (on the right)
  • higher the frequency, higher the energy
  • increasing energy and frequency going to the left
  • increasing wavelength going to the right

that random chart looking thing where it goes from blue to red

46
Q

interference

A

2 waves come into contact with each other

47
Q

2 types of interference

A
  • constructive: 2 waves that are IN PHASE (same peaks & troughs) add together
    result: higher amplitude
  • destructive: 2 waves that are OUT OF PHASE (perfectly misaligned, their peaks & troughs match up)
    result: balance out and becomes straight line
48
Q

standing waves + nodes

A

waves that remain constrained in a region of space (not moving in space but have oscillations like a guitar string)

  • nodes: spaces along standing waves which are not in motion
49
Q

translation wave

A

waves that are not moving but amplitude keeps changing because of interference

50
Q

the ultraviolet catastrophe

A
  • late 1800s to early 1900s
  • physics at that time couldn’t explain why hot objects didn’t give off infinite amount of UV light
  • led to Planck’s theory that energy can only exist in discrete “packets”
51
Q

max planck’s observations + formula

A

energy is quantized
- energy can be gained or lost only in multiples of hv

ΔE = nav

ΔE = change in energy for a system
n = any integer
h = Planck’s constant (6.626 x 10^-34 Jxs)
v = frequency of electromagnetic radiation

52
Q

the photoelectric effect

A

phenomenon in which electrons are emitted from the surface of a metal when light strikes it

  • explained by Einstein
53
Q

properties of the photoelectric effect

A
  1. no electrons are emitted by metals below a specific threshold frequency, regardless of light intensity!
  2. for light with frequencies greater than v0, # of electrons emitted increases with increasing light intensity
  3. for light with frequencies greater than v0, the kinetic energy of electrons emitted increases with increasing light frequency

basically saying that intensity (brightness) of light determines the number of photoelectrons, while frequency (color) of light determines energy

54
Q

photons + relationship of photons & light

A

stream of “particles” of electromagnetic radiation

  • intensity of light is a measure of the # of photons present in the beam (more intense light = more photons)
  • energy of photons is directly proportional to frequency of light
55
Q

significance of E = mc² + derived equation

A
  • shows that energy and mass are related

E = hc/λ

56
Q

continuous vs. line spectra

A

continuous spectra result when white light passes through a prism (contains all wavelengths of visible light)

line spectra display discrete wavelengths of light (specific bands showing, not the entire spectrum)

57
Q

atomic spectrum for hydrogen

A

when energy is applied to hydrogen gas, hydrogen molecules (H2) absorb energy and some molecules are split into atoms (H)

  • electrons are excited
  • electrons don’t like staying at high states wanna go lower, energy is released when they go lower
58
Q

hydrogen emission spectrum

A

1/λ = -R (1/ (n final)^2 - 1/
(n initial)^2)

R = 1.097 x 10^7 1/m

59
Q

Bohr Model for the H-atom

A
  • electrons in hydrogen atoms orbited the nucleus in certain energy levels
  • extended Planck’s idea that light can only exist in specific intervals to electrons
  • an electrons’ energy level is related to the energy level it occupies (further or closer to nucleus dictates how much energy it has)

electron moves further from nucleus = energy absorbed

electron moves closer to nucleus = energy released

60
Q

bohr model equation

A

E = -2.179 x 10^-18 J (Z^2/n^2)

Z = nuclear charge (+1 for H)
n = any integer

61
Q

drawbacks of the Bohr Model

A
  1. insufficient for explaining atoms other than Hydrogen
  2. in reality, electrons do not move around atomic nuclei in circular orbits

(but Bohr spurred quantum mechanics)

62
Q

maximum # of electrons using the quantum numbers

A

n principal level - 2n^2 is the formula to find # of electrons possible

ex. n = 2, 2(2)^2 = 8

  • if ms is only one number given, half the n value that u found
  • l = 0 is s orbital
  • l = 1 is p orbital
  • l = 2 is f orbital
  • l = 3 is d orbital

if 4 quantum numbers are given, the answer is always 1 b/c 4 quantum numbers can only specify ONE electron

63
Q

de Broglie equation

A

every single moving particle (including electron) has a wavelength associated with it

λ = h/mv

h = planck’s constant
m = mass
v = velocity

if mass is larger, denominator is larger so wavelength is smaller = explains why wavelength of macroscopic objects was not sensed bc the wavelength was too small

64
Q

Davisson-Germer experiment (1927)

A
  • provided strong evidence that electrons behave as waves
  • same exact diffraction pattern as waves
  • finally ended the debate and the physics world acknowledged this
65
Q

the Heisenberg uncertainty principle

A

for any particle, can only know the position & momentum with very limited precision

∆x x ∆ p (mv) ≥ h/4π

(don’t need to memorize this equation)

66
Q

the Schrödinger equation

A

used to find the probability of where the electron exists

67
Q

the electromagnetic spectrum (order of the waves smallest to largest)

A

gamma rays -> x-ray -> UV -> visible light -> infrared -> microwaves -> radio waves

68
Q

electron density maps

A

intensity of color depicts probability value near a given point in space

69
Q

quantum numbers

A

n = principal quantum number (orbital’s size, energy, and distance from the nucleus)

l = angular momentum (specifies shape of the orbital) up to n-1 # of subshells increase as l increases

ml = specifies orientation of each orbital in 3D space -l to +l

ms = electron spin always +/- 1/2

70
Q

nodes

A

areas with zero probability of finding an electron

  • total number of nodes in an orbital is equal to n-1
71
Q

the Pauli exclusion principle

A

no 2 electrons in the same atom can have the same set of 4 quantum numbers!

  • orbitals can hold a maximum of 2 electrons

like saying 2 people have the same ID number

72
Q

degeneracy

A

denegerate orbitals are orbitals with the same energy

in hydrogen, orbitals with the same value for n are degenerate

73
Q

orbital energy increasing trend

A
  • as energy level (n) increases, energy of orbital increases
  • as angular momentum (l) increases, energy of orbital increases too
74
Q

electron shielding

A

effect where electron experiences reduction in the effective nuclear charge due to electrons occupying inner energy levels

75
Q

penetrating power

A

ability of an electron to get close to the nucleus

  • the lower in energy level is more penetrating (n takes precedent)

ex. 4s and 5p –> 4s e- is more penetrating

76
Q

the Aufbau principle

A

electrons fill the lowest available energy levels (orbitals) before occupying higher levels

77
Q

Hund’s Rule

A

1) electrons fill degenerate (orbitals that have the same energy) singly before pairing

2) unpaired electrons have the same spin

start with spin facing upwards first

  • that diagram looking thing where you draw the half up and down arrows to show electrons -
78
Q

electron configurations & orbital diagrams

A

electron configurations: represent the arrangement of electrons in orbitals of atoms

orbital diagrams: picture that shows arrangement

79
Q

valence and core electrons

A

valence: outermost electrons (includes all of them with the same n value)

core: all the inner electrons (everything but the valence electrons)

80
Q

condensed electron configurations

A

in brackets, write symbol for noble gas that comes directly before element, then write configuration for all remaining electrons

81
Q

special case for electron configuration

A

Cr’s row and everything in it and Cu’s row and everything in it

bump one electron from s to d

ex. 4s2 5d9 becomes 4s1 5d10

82
Q

elements in the same group have ______________

A

similar properties

83
Q

atomic radius definition

A

half the distance between the nuclei of 2 atoms of an element

84
Q

atomic radii trend & why

A
  • increases down groups b/c more orbitals so greater in size
  • decreases across periods b/c effective nuclear charge increases, decreasing atomic radius, greater “pull” for electrons
85
Q

isoelectronic ions

A

ions with the same number of electrons

86
Q

trends for ionic radii

A
  • increases down groups
  • decreases with effective nuclear charge (for isoelectronic ions)
87
Q

ionization energy + trend

A

amount of energy required to remove an electron from an atom to an ion

trend:
- decreases down groups
- increases across periods (left to right)

88
Q

why is there a deviation in ionization energy trend b/w nitrogen and oxygen?

A

oxygen has 2 electrons in the same orbital which causes repulsions b/c they’re both negatively charged particles

for that reason, more favorable to remove electrons from oxygen than from nitrogen

89
Q

electronegativity + trends

A

ability of an atom to attract electrons

Trend:
- decreases down groups
- increases across periods (left to right)

90
Q

Dmitri Mendeleev

A

credited for originally organizing the period table

managed to:
- correct several values for atomic masses
- predict properties of later discovered elements (would put question marks n stuff)

CHEM 101 (6 decks)

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