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Chemistry > ⭐️Modern Atomic Theory > Flashcards

⭐️Modern Atomic Theory Flashcards

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1
Q

Wave-particle duality of nature

A

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

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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

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3
Q

Schrodinger

A

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

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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

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5
Q

n

A 
Energy level/size of electron cloud
Quantum number
Given
n=1 to infinity
>>>>>>>>>energy of electron increases
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6
Q

l

A

Sublevel, shape of electron cloud

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

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7
Q

m

A

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

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8
Q

s

A

Spin of electron, +-1/2

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

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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

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10
Q

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

A

n^2

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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

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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)

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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

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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

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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)

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16
Q

The highest energy level holds…

A

Valence electrons because it’s the outermost energy level

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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

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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

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19
Q

What if I removed 1 valence electron from 11Na?

A

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

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20
Q

Kernel

A

Electrons that are NOT valance

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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)

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