Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem > atomic structure > Flashcards

atomic structure Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

SPECTRA

A

use of a diffraction grating to break apart visible light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

CONTINUOUS SPECTRUM

A

all the colours of the rainbow, no gaps

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

EMISSION SPECTRUM

A

black background, with bands of colour

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

ABSORPTION SPECTRUM

A

rainbow with gaps

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

order frequency, energy, and wavelength

A

wavelength
frequency
energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

STATIONARY STATES

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

how are emissions spectra produced

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

hydrogen emission spectrum

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

transitions to n=2

A

seen in visible light region

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

transitions to n=1

A

higher in energy
UV region

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

transitions to n=3

A

lower in energy
IR region

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

why do elements have its own unique line spectrum

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

pattern of each element with their line spectrum and electronic signature

A

of electrons inc. = # of spectral lines inc.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what has short wavelength

A

gamma rays
UV

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what has long wavelengths

A

radio
microwave
IR

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what region goes in 400 nm and 700 nm

A

UV = 400 nm
IR = 700 nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

ELECTROMAGNETIC SPECTRUM

A

alternating electric and magnetic waves travelling at the speed of light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

constant for the speed of light

A

c = 3.00x10^3 mn^-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

WAVELENGTH

A

lambda
units are meters or SI prefix

21
Q

FREQUENCY

A

(f)
# of cycles of the wave (up down up) per sec
units= HERTZ

22
Q

speed of light formula

A

c = f(wavelength)

23
Q

Light as a particle

A

as matter gains energy, it emits EMR of varying wavelengths

24
Q

MAX PLANCK

A

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

25
Q

planck’s formula and constant

A

E=hf
h= 6.63x10^-34

26
Q

pros of bohr’s model

A

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

27
Q

cons of bohr’s model

A

orbits
treating electrons as particulate

28
Q

QUANTUM THEORY

A

matter (electrons) has wavelike properties

29
Q

DE BROGLIE

A

3D wave around nucleus, fits energy level

30
Q

PAULI

A

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

31
Q

ORBITAL

A

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

32
Q

HEISENBERG

A

uncertainty principle

33
Q

UNCERTAINTY PRINCIPLE

A

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

34
Q

SCHRODINGER

A

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

35
Q

S orbital

A

2 electrons max
as sublevels inc.=size inc.

36
Q

P orbital

A

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

37
Q

D orbital

A

5 orientations

38
Q

F orbital

A

7 orientations

39
Q

energy sublevel order of orbitals

A

s<p<d<f

40
Q

What causes energy levels and sublevels?

A

effect of nuclear charge
shielding effect (screening)
penetration

41
Q

EFFECT OF NUCLEAR CHARGE

A

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

42
Q

Z ACTUAL

A

actual nuclear charge

43
Q

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

PENETRATION

A

how close an electron can get to the nucleus

45
Q

PENETRATION on the S orbital

A

shape allows for higher penetration

46
Q

PENETRATION on the P orbital

A

high electron density away from nucleus
less penetration
higher energy

47
Q

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

HUND’S RULE

A

spread out electrons into equal energy orbitals before doubling up

49
Q

ANAMOLIES

A

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

Chem (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions