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Grade 12 Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

what was the first atomic model and who proposed it?

A

solid sphere model, by Dalton

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2
Q

What was the second atomic model and who proposed it?

A

plum pudding model by JJ Thomson

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3
Q

what was the third atomic model and who proposed it?

A

the nuclear model by Rutherford

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4
Q

what was the fourth atomic model and who proposed it?

A

planetary model by Bohr

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5
Q

what was the fifth atomic model and who proposed it

A

the quantum model by Schrodinger

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6
Q

quantum mechanics

A

the study of motion at the atomic level where classical lawss of motions do not apply because the particles behave like waves

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7
Q

what did de Broglie think?

A

orginated the idea than an electron has both wave and particle properties

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8
Q

what demo did Schrodinger and de Broglie perform?

A

standing wave demo

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9
Q

What did Schrodinger and de Broglie find with the electron from hydrogen?

A

the model showed the electron as a circular stading wave ith wavelenths of whole number multiples

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10
Q

how did other orbits affect the standing wave?

A

would cause it to cancel out or collapse

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11
Q

orbital

A

a region around the nucleus where there is a high probability of finding an electron

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12
Q

what did the Schrodinger wave equation lead to?

A

can be used to calculate electron energy levels, which gives a definable amount of energy to an electron allowing it to be localized to a given orbital

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13
Q

Heisenbergs uncertainty principle

A

the idea that it is impossible to know the exact position and speed of an electron and the same given time

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14
Q

electrons are so small that any attempt to measure its location or speed will affect its location and/or speed

A
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15
Q

what are the two main points of the quantum mechanical model?

A
  • electrons can be in different orbitals by absorbing or emitting quanta of energy
  • the location of electron is given by a probability distribution
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16
Q

electron configuration

A

shows the specific placement of electrons within an energy level

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17
Q

sublevel of an energy level called:

A

orbital

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18
Q

how many electrons can orbital hold?

A

a maximum of 2

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19
Q

what are the 4 types of orbitals??

A

s, p, d, f,
(sharp, principal, diffuse, and fundamental)

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20
Q

how many s orbitals?

A

single

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21
Q

how many p orbitals?

A

groups of 3

22
Q

how many d orbitals?

A

groups of 5

23
Q

how many f orbitals?

A

groups of 7

24
Q

where are s orbitals found?

A

on every energy level

25
Q

where are p orbitals found?

A

at energy level 2 and above

26
Q

where are d orbitals found?

A

energy levels 3 and above

27
Q

where are d orbitals found?

A

in energy levels 3 and above

28
Q

where are f orbitals found?

A

levels 4 and above

29
Q

in what order are electrons placed in energy levels?

A

from lowest enegy (closest to eh nucleus) to highest energy

30
Q

Pauli Exclusion principle

A

when 2 electrons are placed in the same orbital, these electrons will spin in different directions (one arrow points up and another points down)

31
Q

Aufbau pinciple

A

lowest energy orbitals are filled first

32
Q

Hund’s rule

A

when there are multiple orbitals of equal energy, each orbitals gets a single elerctron before pairing up electrons

33
Q

describe longhand configuration

A

writing the lowest energy level and orbital type and put the number of electrons as a superscript for the orabital then conitnue until all electrons have been accounted for

34
Q

describe shorthand or noble gas configuration

A

use the closest noble gas with fewer electrons, place that symbol is square brackets and resume the configuration and continue until all electrons have been accounted for

35
Q

what are the 2 stable electron configurations

A

a filled set or orbitals or a half filled set of orbitals

36
Q

Which elements are exceptions to the rule?

A

Cr, Mo, Cu, Ag, Au

37
Q

how does Cr differ from normalcy?

A

[Ar]4s13d5 NOT [Ar]4s23d4

since it is more stable and takes less energy for the 4s and 3d orbitals to be half filled

38
Q

describe the electron configuration of negative ions

A

negative ions will gain enough electrons to fill the orbitals of their highest energy level. Non-metals make anions so they would be P orbitals that are the highest energy shells

39
Q
A
40
Q

describe the electron configuration of positive ions

A

will lose electrons from the highest avaible energy shell before it loses from the next shell down

41
Q

quantum numbers

A

set of 4 numbers that describe an electron’s location

42
Q

whats the first number?

A

principal quantum number (n), the energy level the electron is in

43
Q

what is the second quantum number

A

secondary quantum number (l), describes sublevel (orbital type)

s= 0
p = 1
d = 2
f = 3

aka angular momentum quantum number

44
Q

what is the third quantum number?

A

magnetic quantum number (m)

descibes which orbital the sublevel electron is in

45
Q

what is the fourth quantum number?

A

spin quantum number

describes whether electron is spinning clockwise (+1/2) or counterclockwise (-1/2)

46
Q

Who discovered the electron?

A

J.J Thomson Joseph john

47
Q

How was the electron discovered?

A

With the cathode ray experiment. Electric current run through a glass tube a stream of negatively charged particles was emittey

48
Q

Who discovered the nucleus?

A

Rutherford

49
Q

How was the nucleus discovered?

A

With the gold foil experiment

50
Q

Who discovered the neutron?

A

James Chadwick

Grade 12 Chemistry (9 decks)

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