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atomic structure Flashcards

(49 cards)

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1
Q

(IB) SPECTRA

A

use of a diffraction grating to break apart visible light

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2
Q

(IB) CONTINUOUS SPECTRUM

A

all the colours of the rainbow, no gaps

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3
Q

(IB) EMISSION SPECTRUM

A

black background, with bands of colour

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4
Q

(IB) ABSORPTION SPECTRUM

A

rainbow with gaps

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5
Q

(IB) order frequency, energy, and wavelength

A

wavelength
frequency
energy

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6
Q

(IB) STATIONARY STATES

A

part of bohr
certain allowable energy levels where the elctron is in a fixed circular orbit around the nucleus

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7
Q

(IB) how does the atom change to another stationary state

A

part of bohr
by ABSORBING or EMITTING a photon that matches the difference in energy between the 2 stationary states

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8
Q

(IB) how are emissions spectra produced

A

part of bohr
by atoms emitting photons when electrons in excited states return to lower energy levels

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9
Q

(IB) hydrogen emission spectrum

A

part of bohr
distances between levels converge
from 400-600 nm, purple, blue, green, red

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10
Q

(IB) transitions to n=2

A

seen in visible light region

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11
Q

(IB) transitions to n=1

A

higher in energy
UV region

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12
Q

(IB) transitions to n=3

A

lower in energy
IR region

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13
Q

(IB) why do elements have its own unique line spectrum

A

electronic signature is unique,
different # of electrons mean different magnitude of energy levels

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14
Q

(IB) pattern of each element with their line spectrum and electronic signature

A

of electrons inc. = # of spectral lines inc.

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15
Q

(IB) what has short wavelength

A

gamma rays
UV

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16
Q

(IB) what has long wavelengths

A

radio
microwave
IR

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17
Q

(IB) what region goes in 400 nm and 700 nm

A

UV = 400 nm
IR = 700 nm

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18
Q

(IB) ELECTROMAGNETIC SPECTRUM

A

alternating electric and magnetic waves travelling at the speed of light

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19
Q

(IB) constant for the speed of light

A

c = 3.00x10^3 mn^-1

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20
Q

(IB) WAVELENGTH

Study These Flashcards
A

lambda
units are meters or SI prefix

21
Q

(IB) FREQUENCY

Study These Flashcards
A

of cycles of the wave (up down up) per sec

(f)
units= HERTZ

22
Q

(IB) speed of light formula

Study These Flashcards
A

c = f(wavelength)

23
Q

(IB) Light as a particle

Study These Flashcards
A

as matter gains energy, it emits EMR of varying wavelengths

24
Q

(IB) MAX PLANCK

Study These Flashcards
A

if matter emits certain quantities of energy, then an atom only has certain quantities of energy to give

25
(IB) planck's formula and constant
E=hf h= 6.63x10^-34
26
(IB) pros of bohr's model
energy levels n=1 through infinity convergence of energy levels 2n^2
27
(IB) cons of bohr's model
orbits treating electrons as particulate
28
(IB) QUANTUM THEORY
matter (electrons) has wavelike properties
29
(IB) DE BROGLIE
3D wave around nucleus, fits energy level
30
(IB) PAULI
orbital 2 electrons in a pair with opposing magnetic spins magnetic attraction oppose electron-electron repulsions
31
(IB) ORBITAL
3D region of space surrounding the nucleus, with 90% of finding 1 or 2 electrons
32
(IB) HEISENBERG
uncertainty principle
33
(IB) UNCERTAINTY PRINCIPLE
can't know the position and momentum of an electron at the same time
34
(IB) SCHRODINGER
wave equations whose solutions gave the probability densities of the location of an electron in an orbital
35
(IB) S orbital
2 electrons max as sublevels inc.=size inc.
36
(IB) P orbital
3 orientations 2 lobes (equivalent in energy) slightly higher in energy than s
37
(IB) D orbital
5 orientations
38
(IB) F orbital
7 orientations
39
(IB) energy sublevel order of orbitals
s
40
(IB) What causes energy levels and sublevels?
effect of nuclear charge shielding effect (screening) penetration
41
(IB) EFFECT OF NUCLEAR CHARGE
as # of protons in nucleus inc.=attraction of electrons to nucleus inc. creates a stabilizing effect
42
(IB) Z ACTUAL
actual nuclear charge
43
(IB) SHIELDING EFFECT (SCREENING)
destabilizing inner electrons repel outer outer electron still has some attraction Z effective < Z actual creates successive E levels
44
(IB) PENETRATION
how close an electron can get to the nucleus
45
(IB) PENETRATION on the S orbital
shape allows for higher penetration
46
(IB) PENETRATION on the P orbital
high electron density away from nucleus less penetration higher energy
47
(IB) AUFBAU PRINCIPLE
add electrons to each sublevel of an atom in its ground state before electrons are added to the next sublevel
48
(IB) HUND'S RULE
spread out electrons into equal energy orbitals before doubling up
49
(IB) ANAMOLIES
Chromium: 6.5 filled orbitals that are ~same energy gives stability Copper: 3d is filled out, 1 unpaired electron in 4s

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