Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > ⭐️Modern Atomic Theory > Flashcards

⭐️Modern Atomic Theory Flashcards

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

Wave-particle duality of nature

A

Electrons and light have properties of both waves (wavelength+frequency) / particles (quanta of energy)

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

Heisenberg’s uncertainty principle

A

It is impossible to know the exact position and momentum of an electron at the same time WE ARE UNCERTAIN WHAT ELECTRONS ARE WHERE IN HEINZ KETCHUP

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

Schrodinger

A

Treated electrons as waves and assigned them quanta numbers (levels, energy levels) ELECTRONS ARE LIKE WAVES, GAVE THEM QUANTA NUMBERS

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

Wave-mechanical view of an atom

A

1) electron cloud model
2) probability of finding an electron in a cloud
3) orbital=region in a space electrons are found PROBABILITY OF CLOUDS IN ORBITALS

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

n

A 
Energy level/size of electron cloud
Quantum number
Given
n=1 to infinity
>>>>>>>>>energy of electron increases
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

l

A

Sublevel, shape of electron cloud

l=0 to (n-1), types s, p, d, and f (SUPER PRETTY DALMATIANS FART)

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

m

A

Orbitals, direction in space
Orbitals hold a max of 2 electrons
m= -l to +l

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

s

A

Spin of electron, +-1/2

+1/2=clockwise spin, counterclockwise=-1/2

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

Pauli’s exclusion principle

A

No 2 electrons for an atom can have the same 4 quantum #’s PAULIEEE STOP EXCLUDING ELECTRONS FROM EACHOTHER

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

How to find the max # of orbitals/level (n to m)?

A

n^2

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

How to find max # of electrons/level (n to s)? (this is the atomic # of the noble gas of that period/level)

A

2n^2

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

Hund’s Rule

A

In a sublevel, each orbital gets an electron before pairing up. (Draw all up arrow first, then down, to show that electrons spin in opposite directions)

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

De Broglie

A

Hypothesized that if Planck (energy in quanta) were correct, then particles can have properties of waves
Used E=mc^2 and E=hV for Tilda=h/(m•v)…you can calculate wavelength of a particle if you know the mass+velocity ELECTRONS ARE LIKE WAVES, MADE AN EQUATION

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

What would each value represent in electron configuration 2s^1

A

2 is the level, s is the sublevel, 1 is the #of electrons on that sublevel

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

What makes a noble gas?

A

Electrons on the outermost energy/quantum level (valence electrons) add up to 8 and therefore have pairs spinning in opposite directions. (Far right of periodic table)

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

The highest energy level holds…

A

Valence electrons because it’s the outermost energy level

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

Louis dot diagram

A

Signifies how many valence electrons are on an element, put dots going (ORDER/PLACEMENT???). Dots next to each other are paired up/spin in opposite directions

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

If the arrows go ..|^v|..|^v|..|^|^| |..how many pairs of electrons are unshared? How many pairs are at least half full?

A

2 unshared pairs of electrons

4 pairs at least half full

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

What if I removed 1 valence electron from 11Na?

A

It would make a cation (positive ion) Na^+ or Na^+1

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

Kernel

A

Electrons that are NOT valance

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

Diagonal rule

A 
1s^2 
2s^2, 2p^6
3s^2, 3p^6, 3d^10
4s^2, 4p^6, 4d^10, 4f^14
5s^2, 5p^6, 5d^10, 5f^14
6s^2, 6p^6, 6d^10
7s^2, 7p^6
22
Q

Sublevel s

A

Max 2 electrons, 1 orbital (box)=one sphere in center axis

23
Q

Sublevel p

A

Max 6 electrons, 3 orbitals (boxes)=2 spheres on x, 2 spheres on y, and 2 spheres on z

24
Q

Sublevel d

A

Max 10 electrons, 5 orbitals (boxes)

25
Q

Sublevel f

A

Max 14 electrons, 7 orbitals (boxes)

26
Q

What would each value represent in electron configuration 2s^1

A

2 is the level, s is the sublevel, 1 is the #of electrons on that sublevel

27
Q

What makes a noble gas?

A

Electrons on the outermost energy/quantum level (valence electrons) add up to 8 and therefore have pairs spinning in opposite directions. (Far right of periodic table)

28
Q

The highest energy level holds…

A

Valence electrons because it’s the outermost energy level

29
Q

Louis dot diagram

A

Signifies how many valence electrons are on an element, put dots going clockwise🔁Dots next to each other are paired up/spin in opposite directions

30
Q

If the arrows go ..|^v|..|^v|..|^|^| |..how many pairs of electrons are unshared? How many pairs are at least half full?

A

2 unshared pairs of electrons

4 pairs at least half full

31
Q

What if I removed 1 valence electron from 11Na?

A

It would make a cation (positive ion) Na^+ or Na^+1

32
Q

Kernel

A

Electrons that are NOT valance

33
Q

Diagonal rule

A 
1s^2 
2s^2, 2p^6
3s^2, 3p^6, 3d^10
4s^2, 4p^6, 4d^10, 4f^14
5s^2, 5p^6, 5d^10, 5f^14
6s^2, 6p^6, 6d^10
7s^2, 7p^6
34
Q

Maximum # of electrons on 1st, 2nd, 3rd, 4th and 5th energy levels

A

2, 8, 18, 32, and 32 electrons

35
Q

How many electrons can be in 1 orbital?

A

2 (1 pair)

36
Q

What names are used for the 3 p orbitals

A

Px Py Pz axes

37
Q

What system of mathematical equations is used to describe the behavior of extremely SMALL particles traveling at velocities near the speed of light?

A

Quantum/wave mechanics. Deals with matter, radiation, waves, subatomic….Equation is T(wavelength)=h/(m•v)

38
Q

Newtonium mechanics

A

Laws of mechanics applicable in the macroscopic world

39
Q

Momentum equation

A

p=m•v mass times velocity

40
Q

Info on De Broglie’s equation

A

T(m)=h(given, m 2/s)/mass(g)•velocity(m/s)

Use cross-multiplication/dig figs

41
Q

Probability of finding an electron in a point in space

A

Ratio between the #of times the electron is in tht certain position and the total #of times it is at all possible positions…^probability, ^likeliness electron will be found @ tht position

42
Q

Shortcut to filling in arrow-pairs of electrons?

A

Only fill it in (using hunds rule) for the last sublevel, that is not full

43
Q

When electrons are switched around to different sublevels then the regular order, what does it mean?

A

The element is in the exited state, ground>excited, electron jumps, absorbs energy. As long as the electrons don’t exceed the max of tht sublevel it’s not incorrect, even if sublevels are missing

44
Q

Silicon in 1s^2 2s^2 2p^7 would be…

A

Incorrect

45
Q

The periods of periodic table represent (horizontal rows)

A

Elements that are similar and have the same energy levels

46
Q

When an electron moves from n=2 to n=4…

A

It gains energy/photons are absorbed, jumps to a higher energy level (source=voltage box or flame)

47
Q

Why can orbitals have nonspherical shapes even though the cloud charge is spherical?

A

May have different shapes on each orbital making up the charge cloud, which together creates a sphere

48
Q

What signifies the SHAPE of electron cloud?

A

Sublevel l

49
Q

Which noble gas is an exception?

A

Helium because it has 2 instead of 8 valence electrons

50
Q

Excited state

A

Switch around electrons to different energy/sublevels, keep the same # of total electrons since it’s still the same element

Chemistry (17 decks)

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