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Chem 1120 > Midterm Deck > Flashcards

Midterm Deck Flashcards

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1
Q

Chemistry

A

the study of the properties and transformations of matter and the interactions btwn matter and E

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2
Q

Measurement

A

using an instrument to quantify property relative to an international standard

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3
Q

SI Units

A

Base:

  • mass (kg)
  • length (m)
  • time (s)
  • amount (mol)

Derived:

  • volume (m^3)
  • density (kg m^-3)
  • E (J kg m^2s^-2)
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4
Q

Trueness

A

an indication of how close a measurement (or mean of repeated measurements) is to the accepted “true” value

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5
Q

Precision

A

an indication of how close together repeated measurements are

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6
Q

Accuracy

A

combination of trueness and precision -> governed by systematic error/bias

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7
Q

Systematic Error

A

error w/ the system measurement -> can be eliminated

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8
Q

Random Error

A

noise; human error -> can’t eliminate

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9
Q

Scientific Notation

A

x.yE^z

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10
Q

Sig. Figs.

A
  • w/in the accuracy of the measurement
  • leading 0’s not significant
    trailing 0’s sig. unless ambiguous
  • exact #’s have unlimited sig.figs.
  • calculations:
    ~ multiplication/division -> sig.figs. limited by the factor w/ the fewest sig.figs.
    ~ addition/subtraction -> limited to the # of decimal places
    ~ avoid rounding until the very end
    ~ BEDMAS
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11
Q

Uncertainty

A
  • limits the # of meaningful digits that should be used to express the measured value
  • only express the #s that align w/ your uncertainty
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12
Q

Structure of the Atom

A

massive nucleus containing protons and neutrons w/ e-s surrounding

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13
Q

Atomic Particles

A

very small particles that are building blocks for atoms -> e-s, protons, and neutrons

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14
Q

Newtonian Mechanics

A
  • macroscopic objects
  • deterministic
  • observer independent from system
  • continuously variable
  • 1643-1727
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15
Q

Quantum Mechanics

A
  • Planck, Heisenberg, Schrodinger, Bohr, Einstein
  • submicroscopic (e-s, photons)
  • probabilistic
  • observer entangled in system
  • quantized -> “blocky”
  • 1900-1920
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16
Q

Wavelength

A

distance btwn 2 crests/troughs

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17
Q

Frequency

A

how many waves past a given spot per second

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18
Q

Velocity

A

the speed of something in a given direction (V = deltaX/deltaT)

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19
Q

Amplitude

A

halfway btwn the troughs and crests of waves

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20
Q

Diffraction

A

wave encounters an obstacle/slit comparable in size to its walv., it bends around it

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21
Q

Refraction

A
  • wavl. dependant

- change in direction of wave propaganation due to a change in its transition medium

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22
Q

Interference

A
  • constructive -> when two waves meet in phase

- destructive -> when two waves meet out of phase

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23
Q

Longitudinal Waves

A
  • oscillations of particles are parallel to the direction of propagation
  • eg. sound
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24
Q

Transverse Waves

A
  • particles oscillate perpendicularly to the direction of wave motion
  • eg. light
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25
Q

Electromagnetic Wave

A
  • coupling of magnetic and electric fields -> waves perpendicular to electric and magnetic fields and each other
  • speed of light = (walv.)(freq)
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26
Q

Electromagnetic Spectrum in Order of Decreasing E (inc walv., dec freq)

A

Gamma rays, x-rays, ultra-violet light,

visible light, infra-red light, microwaves, radio waves, TV waves

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27
Q

Range of Visible Light

A
  • Violet (400nm)
  • Blue (450-500nm)
  • Green (500-550nm)
  • Yellow (600nm)
  • Orange (650nm)
  • Red (750-700nm)
28
Q

Photoelectric Effect

A
  • KEmax = eV0 = 1/2MeV^2

- KEmax is independant of the intensity and proportional to its freq. b/c of lights particle and wave like duality

29
Q

Rutherford’s Experiment

A

determined structure of the atom by blasting particles at a gold sheet -> some passes through, other bounced off -> nucleus!

30
Q

Relationship Between Emission and Absorption Spectra of the Elements

A
  • only emits/absorbs ery specific freq’s b/c of the e- rings in an atom
  • instantaneous transition
  • emission = falling e-s
  • absorption = jumping e-s
31
Q

The Bohr Equation

A
  • N can be 1,2,3,8,….
  • Constant is -ive b/c the nucleus is +ive
  • Giving the absolute Es of state
  • Z = the charge of the nucleus
  • This eqtn only holds for systems in which there is one e- -> Can’t quantify the e- e- repulsion if there is more than 1 e- involved -> Only for hydrogenic atoms/ions
  • Moving towards 0 energies -> free
32
Q

Schrodinger Wave Equation

A
  • H hat = Hamiltonian operator -> Set of mathematical operations that rep the total E of the e-
  • E = actual E of the e- -> eigenvalue
  • Psi = wave function -> Plot of the wave function squared reps the orbital/probability distribution map of the e-
33
Q

Fish psi^2dT = 1

A

the probability of finding an electron somewhere in

the universe is 1

34
Q

n

A
  • principal quantum #
  • determines the overall size
  • allowed values are 1, 2, 3…
  • orbitals w/ higher n values have less -ive Es
  • as n inc the spacing btwn E levels decs
35
Q

l

A
  • angular momentum #
  • determines shape of orbital
  • allowed values are 0, 1, 2, 3…, (n-1)
  • l=0 -> s, l=1 -> p, l=2 -> d, l=3 -> f
36
Q

Msubl

A
  • magnetic quantum #
  • orientation of orbital
  • integer values including 0, ranging from -l to +l
37
Q

MsubS

A
  • spin quantum # = MsubS +/- 1/2

- cannot have 2 e-s of the same spin -> 2 e-s in each orbital

38
Q

Orbital

A

a 3D volume of space close to the nucleus in which there is an arbitrarily high probability than an e- can be found

39
Q

Shaded vs. Unshaded

A

shaded sides only indicate that in these regions of space psi has opp signs -> not stipulated which are +ive or -ive -> not electrical charges

40
Q

Ordering of Orbitals in Terms of E

A

(from most -ive to least -ive)

1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 5f

41
Q

Shielding

A
  • e- of interest experiences a lower effective nuclear charge b/c it is screened from the nucleus by other e-s whose max radial probability is closer -> interference
  • Zeffective = Z-S -> S = screened charge
  • degree to which an e- blocks the e- of interest from the +ive charge of the nucleus
42
Q

Penetration

A
  • the E of the 2s e- is lower than that of the 2p e- b/c the probability of finding the 2s e- very close to the nucleus is higher than that of finding the 2p e- & therefore the effective nuclear charge experienced by the 2s e- is higher than that experienced by the 2p & the 2s is said to “penetrate” the 1s much better than the 2p does -> lil’ bump
43
Q

Nodes

A
  • surface on which the probability of finding an e- is 0

- # of nodes = n - l - 1

44
Q

Afbau Principle

A

only 2 e-s w/ opp spins are allowed in each orbital, occupy lowest level 1st

45
Q

Pauli Exclusion Principle

A
  • no 2 e-s in an atom can have the same 4 quantum #s

- each orbital can have a max of only 2e-s, with opposing spins

46
Q

Hund’s Rule

A

when filling degenerate orbitals, e-s fill them singly first, w/ parallel spins (then pair up w/ opposing spins)

47
Q

Core e-s

A

e-s in complete principal E levels and d and f sublevels

48
Q

Valence e-s

A
  • e-s that are important to chem bonding
  • for main-group elements, the valence e-s are those in the outermost principal E level
  • for transition elements, count outermost d e-s as valence e-s even though they are not in the outermost principal E level
  • chem properties of an element depend on these e-s
  • held most loosely due to shielding effect of core e-s
49
Q

“Periodic” Table

A

patterns of chemical reactivity

50
Q

Relationships of Elements in the Same Group on The Periodic Table

A
  • same # of valence e-s
  • similar properties
  • row # in periodic table = the highest value of n
  • the # of columns in a block corresponds to the max # of e-s that can occupy the particular sublevel of that block
51
Q

S-block

A
  • alkali metals (1) and alkaline earth metals (2)

- far L

52
Q

P-block

A
  • on the R
  • including rows 13-18
  • non-metals
53
Q

D-block

A
  • in middle
  • transition block
  • metals
54
Q

F-block

A
  • lanthanoids (above) and actinoids
  • uncommonly used
  • inner transition elements
55
Q

Main Group Elements

A

s and p block elements (except H)

56
Q

Group 1

A

alkali metals

57
Q

Group 2

A

alkaline earth metals

58
Q

Group 11

A

coinage metals

59
Q

Group 15

A

pnictogens

60
Q

Group 16

A

chalcogens

61
Q

Group 17

A

halogens

62
Q

Group 18

A

noble gases

63
Q

Properties of Metals

A
  • lustrous
  • solid at room temp (except Hg)
  • conductors
  • high melting point
64
Q

Metals Location

A

everything except H -> staircase line on R begins at boron (B) and extends down to polonium (Po)

65
Q

Non-Metals

A

boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), polonium (Po) and astatine (At) are the elements found along the step like line between metals and non-metals of the periodic table

66
Q

Effective Nuclear Charge (Zeff)

A
  • Zeff = Z – S
  • the charge experienced by the e- of interest (valence), taking shielding into account
  • Zeff is less than nuclear charge due to shielding of valence e-s
  • determines how easy/hard it is to remove the valence e-s

Chem 1120 (2 decks)

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