Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 1A > Week Three > Flashcards

Week Three Flashcards

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

White Light

A

passed through a prim, separates into a continuous spectrum of colours

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

Light Spectrum

A

consists of mainly black background, and a series of line at different wavelengths
- each element produces its own unique line specturm

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

Maxwell’s Theory

A

light consists of electro-magnetic waves. that travel in at 3.0 x 10^8ms^-1

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

Speed of light symbol

A

c

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

h

A

wavelength

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

v

A

frequency

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

frequency formula

A

frequency = speed/wavelength

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

Planck Theory

A

elements emit or absorb light energy in discrete amounts.

- the energy of a quantum (E) is the amount that can be emitted (or absorbed) in the form of radiation

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

Quantum Energy Formula

A

E= Hv where H is planck’s constant

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

Planck’s Constant

A

6.63 x 10^-34Js

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

Bohr’s Theory

A
  • electron occupy discrete orbitals
  • Energy is not radiated continually
  • absorption of fixed quantities of energy occurs
  • emission of fixed quantity of energy occurs
  • electrons have spin
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Addition of heat to electrons

A

atoms absorb the energy and electrons jump to higher energy levels
- after a while, electrons return to a lower level and energy is released as light

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

how energy difference between shells is measured

A

by measuring the wavelength or frequency of light emitted

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

Energy difference formula

A

DE= hV where v is frequency

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

Electron wavelength behaviour

A

behave like standing waves

- occupy discrete electronic energies

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

Quantum Numbers

A

4 numbers

  • principal quantum number (n)
  • angular momentum number (L)
  • magnetic quantum number(ml)
  • spin quantum (ms)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Principal quantum number (n)

A

shells of electrons are number by their principal quantum number
n=1 shell has up to 2 electrons
n= 2shell has up to 8 electrons

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

Shell structure

A

the potential energy increases as the distance of the shell from the nucleus increases
- gaps between the amount of energy needed decrease as you move up the shells as you need less energy to move between shells

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

increasing the number of protons

A

decreases the energy of all shells and moves them closer to nucleus

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

Angular Momentum Quantum Number

A

each shell consists of sub shells

- l has possible values ranging from 0 to n-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Angular Momentum Quantum Number - first shell

A

s orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Angular Momentum Quantum Number - second shell

A

s and p orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Angular Momentum Quantum Number- third shell

A

s, p and d orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Angular Momentum Quantum Number - fourth shell

A

s,p,d and f orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

orbital energy increase

A

increases as the shells go across the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Magnetic Quantum Number (Ml)

A

orientation and orbital direction

- tells how many orbitals there are for the l value

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

l = 0

A

s orbital - one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

l = 1

A

p orbital
- ml = +1,0,-1
3 p orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

l = 2

A

d orbitals

- ml = +2,+1,0,-1,-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

l= 3

A

f orbital

- ml= +3,+2,+1,0,-1,-2,-3

31
Q

Electromagnetic radiation

A

Used to study structures of atoms

32
Q

What has Wavelength properties

A

Light

33
Q

Frequency

A

Variation of wavelength

- number of wave crests passing a point in space in one second

34
Q

Wavelength

A

Variation in space, distance between wave crests

35
Q

Amplitude

A

Max displacement of a wave from midline

36
Q

Increasing amplitude

A

Increases light

37
Q

Speed of light

A

2.998 x 10^8ms-1

38
Q

Speed of light formula

A

Frequency/ wavelength

39
Q

Photoelectric effect

A

Energy (light) absorbed by an organism and passes onto organism

40
Q

Photons

A

Packets/ bundles of light

41
Q

How atoms can form higher energy state

A

Absorb photon of particular energy

42
Q

Absorption spectrum

A

Dark lines on visible

43
Q

Emission spectrum

A

Coloured lines on dark background

44
Q

Wavelength of electron

A

Wavelength = h/mu

45
Q

Atom bound electron - energy

A

Quantised energy

46
Q

Free electrons - energy

A

Any

47
Q

Nodes

A

Area zero electrons density in orbital

Increases as n increases

48
Q

S orbital electron distribution

A

Spherical

49
Q

P orbital - electron distribution

A

Dumbbell

- 2 ends of dumbell different phases

50
Q

D orbital - electron distribution

A

Clover shaped - 4/5

Dz2 - dumbbell with doughnut around

51
Q

Phase

A

Starting point ofwave with respect

52
Q

Orbital energy

A

Determined by atomic number z and principal quantum number n

53
Q

Ionisation energy

A

Energy of orbital

Energy required to remove electron completely from orbital

54
Q

Aufbau principle

A

Orbitals are filled in order of increasing energy

55
Q

Pauli exclusion principle

A

No two electrons in same atom can have the same quantum numbers

56
Q

Hunds rule

A

Electrons occupy sets of degenerate orbitals so to give max number of unpaired spins

57
Q

Paramagnetic

A

Will attract magnetic field

Atoms with unpaired electrons

58
Q

Diagmagnetic

A

Not attracted to magnetic field

59
Q

De broglie equation

A

Links wavelength of particles with speed and mass

P = h/ wavelength

60
Q

Squaring wavelength

A

Gives electron density

61
Q

S electrons

A

Higher attraction to nucleus

Potential energy is lower than other orbitals

62
Q

ISOelectric

A

Same number of electrons, same ground state electron configuration

63
Q

Core electrons

A

Increases as atomic number z increases

Force of attraction between nucleus and electron in inner shell is stronger

64
Q

Valence electrons

A

Occupy orbitals in outer shells

Are used in bonding

65
Q

Greater positive charge

A

Closer the electrons are to the nucleus

Smaller the atom

66
Q

Shielding

A

Electrons closer to the nucleus shield the positive pull from outer electrons
Can be shielded by closer shell or same shell

67
Q

Effective nuclear charge - Zeff

A

Every electron is attracted to nucleus and repelled by other electrons
Charge felt by electron

68
Q

Zeff formula

A

Zeff = Z - 6

Where z is actual nuclear charge and 6 is shield constant more than 0 but less than atomic number

69
Q

Across period - charge

A

Charge increases, size decreases

70
Q

Down group - charge

A

Charge increases

71
Q

Metallic radii

A

Half distance between metallic nuclei

72
Q

Covalent radii

A

Chemically bonded to non metallic nuclei

73
Q

Atomic radii

A

Increases down group

Decreases along rows

74
Q

Ionic radii

A

Radius of charged ion
Radius decreases when atom forms cation
Radius increases when anion is formed

Chemistry 1A (12 decks)

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