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atomic structure Flashcards

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

A

lambda
units are meters or SI prefix

21
Q

(IB) FREQUENCY

A

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

(f)
units= HERTZ

22
Q

(IB) speed of light formula

A

c = f(wavelength)

23
Q

(IB) Light as a particle

A

as matter gains energy, it emits EMR of varying wavelengths

24
Q

(IB) MAX PLANCK

A

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

25
Q

(IB) planck’s formula and constant

A

E=hf
h= 6.63x10^-34

26
Q

(IB) pros of bohr’s model

A

energy levels n=1 through infinity
convergence of energy levels
2n^2

27
Q

(IB) cons of bohr’s model

A

orbits
treating electrons as particulate

28
Q

(IB) QUANTUM THEORY

A

matter (electrons) has wavelike properties

29
Q

(IB) DE BROGLIE

A

3D wave around nucleus, fits energy level

30
Q

(IB) PAULI

A

orbital
2 electrons in a pair with opposing magnetic spins
magnetic attraction oppose electron-electron repulsions

31
Q

(IB) ORBITAL

A

3D region of space surrounding the nucleus, with 90% of finding 1 or 2 electrons

32
Q

(IB) HEISENBERG

A

uncertainty principle

33
Q

(IB) UNCERTAINTY PRINCIPLE

A

can’t know the position and momentum of an electron at the same time

34
Q

(IB) SCHRODINGER

A

wave equations whose solutions gave the probability densities of the location of an electron in an orbital

35
Q

(IB) S orbital

A

2 electrons max
as sublevels inc.=size inc.

36
Q

(IB) P orbital

A

3 orientations
2 lobes (equivalent in energy)
slightly higher in energy than s

37
Q

(IB) D orbital

A

5 orientations

38
Q

(IB) F orbital

A

7 orientations

39
Q

(IB) energy sublevel order of orbitals

40
Q

(IB) What causes energy levels and sublevels?

A

effect of nuclear charge
shielding effect (screening)
penetration

41
Q

(IB) EFFECT OF NUCLEAR CHARGE

A

as # of protons in nucleus inc.=attraction of electrons to nucleus inc.
creates a stabilizing effect

42
Q

(IB) Z ACTUAL

A

actual nuclear charge

43
Q

(IB) SHIELDING EFFECT (SCREENING)

A

destabilizing
inner electrons repel outer
outer electron still has some attraction
Z effective < Z actual
creates successive E levels

44
Q

(IB) PENETRATION

A

how close an electron can get to the nucleus

45
Q

(IB) PENETRATION on the S orbital

A

shape allows for higher penetration

46
Q

(IB) PENETRATION on the P orbital

A

high electron density away from nucleus
less penetration
higher energy

47
Q

(IB) AUFBAU PRINCIPLE

A

add electrons to each sublevel of an atom in its ground state before electrons are added to the next sublevel

48
Q

(IB) HUND’S RULE

A

spread out electrons into equal energy orbitals before doubling up

49
Q

(IB) ANAMOLIES

A

Chromium: 6.5 filled orbitals that are ~same energy gives stability
Copper: 3d is filled out, 1 unpaired electron in 4s

Chem (13 decks)

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